Wednesday and Thursday, Fitness Testing
All Classes
Thursday, October 29, 2009
Wednesday, October 28, 2009
In-Class Assignment 1
Read Chapter 8, define all the terms on page 231 and complete practice problems 1-9 on pages 206-209.
Bellringer 9
Calcium carbonate, when heated, form calcium oxide and carbon dioxide gas.
Answer: CaCO3(s) → CaO(s) + CO2(g)
Sulfuric acid, when heated, decomposes to water and sulfur trioxide.
Answer: H2SO4 → H2O(l) + SO3(g)
2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)
Answer: sodium combined with water yields sodium hydroxide and hydrogen gas.
Answer: CaCO3(s) → CaO(s) + CO2(g)
Sulfuric acid, when heated, decomposes to water and sulfur trioxide.
Answer: H2SO4 → H2O(l) + SO3(g)
2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)
Answer: sodium combined with water yields sodium hydroxide and hydrogen gas.
Monday, October 26, 2009
Bellringer 8
Which of the following statements is NOT true about chemical reactions?
a. The atoms rearrange
b. Loss of mass
c. Change in energy
d. New product is formed
a. The atoms rearrange
b. Loss of mass
c. Change in energy
d. New product is formed
Sunday, October 25, 2009
SPOOTAKSCULAR Review
Periodicity
Physical and Chemical Changes
Compounds, Mixtures and Substances
Scientific Method (Synthesis of Hypothesis and Conclusion)
Naming Compounds
Quantitative/Qualitative Data
(Taken from weak SE's from District 9 wk CBA)
Physical and Chemical Changes
Compounds, Mixtures and Substances
Scientific Method (Synthesis of Hypothesis and Conclusion)
Naming Compounds
Quantitative/Qualitative Data
(Taken from weak SE's from District 9 wk CBA)
More Balancing Equations
1
H2 + O2 => H2O
2
H3PO4 + KOH => K3PO4 + H2O
3
K + B2O3 => K2O + B
4
HCl + NaOH => NaCl + H2O
5
Na + NaNO3 => Na2O + N2
6
C + S8 => CS2
7
Na + O2 => Na2O2
8
N2 + O2 => N2O5
9
H3PO4 + Mg(OH)2 => Mg3(PO4)2 + H2O
10
NaOH + H2CO3 => Na2CO3 + H2O
11
KOH + HBr => KBr + H2O
12
H2 + O2 => H2O2
13
Na + O2 => Na2O
14
Al(OH)3 + H2CO3 => Al2(CO3)3 + H2O
15
Al + S8 => Al2S3
16
Cs + N2 => Cs3N
17
Mg + Cl2 => MgCl2
18
Rb + RbNO3 => Rb2O + N2
19
C6H6 + O2 => CO2 + H2O
20
N2 + H2 => NH3
21
C10H22 + O2 => CO2 + H2O
22
Al(OH)3 + HBr => AlBr3 + H2O
23
CH3CH2CH2CH3 + O2 => CO2 + H2O
24
C + O2 => CO2
25
C3H8 + O2 => CO2 + H2O
26
Li + AlCl3 => LiCl + Al
27
C2H6 + O2 => CO2 + H2O
28
NH4OH + H3PO4 => (NH4)3PO4 + H2O
29
Rb + P => Rb3P
30
CH4 + O2 => CO2 + H2O
31
Al(OH)3 + H2SO4 => Al2(SO4)3 + H2O
32
Na + Cl2 => NaCl
33
Rb + S8 => Rb2S
34
H3PO4 + Ca(OH)2 => Ca3(PO4)2 + H2O
35
NH3 + HCl => NH4Cl
36
Li + H2O => LiOH + H2
37
Ca3(PO4)2 + SiO2 + C => CaSiO3 + CO + P
38
NH3 + O2 => N2 + H2O
39
FeS2 + O2 => Fe2O3 + SO2
40
C + SO2 => CS2 + CO
H2 + O2 => H2O
2
H3PO4 + KOH => K3PO4 + H2O
3
K + B2O3 => K2O + B
4
HCl + NaOH => NaCl + H2O
5
Na + NaNO3 => Na2O + N2
6
C + S8 => CS2
7
Na + O2 => Na2O2
8
N2 + O2 => N2O5
9
H3PO4 + Mg(OH)2 => Mg3(PO4)2 + H2O
10
NaOH + H2CO3 => Na2CO3 + H2O
11
KOH + HBr => KBr + H2O
12
H2 + O2 => H2O2
13
Na + O2 => Na2O
14
Al(OH)3 + H2CO3 => Al2(CO3)3 + H2O
15
Al + S8 => Al2S3
16
Cs + N2 => Cs3N
17
Mg + Cl2 => MgCl2
18
Rb + RbNO3 => Rb2O + N2
19
C6H6 + O2 => CO2 + H2O
20
N2 + H2 => NH3
21
C10H22 + O2 => CO2 + H2O
22
Al(OH)3 + HBr => AlBr3 + H2O
23
CH3CH2CH2CH3 + O2 => CO2 + H2O
24
C + O2 => CO2
25
C3H8 + O2 => CO2 + H2O
26
Li + AlCl3 => LiCl + Al
27
C2H6 + O2 => CO2 + H2O
28
NH4OH + H3PO4 => (NH4)3PO4 + H2O
29
Rb + P => Rb3P
30
CH4 + O2 => CO2 + H2O
31
Al(OH)3 + H2SO4 => Al2(SO4)3 + H2O
32
Na + Cl2 => NaCl
33
Rb + S8 => Rb2S
34
H3PO4 + Ca(OH)2 => Ca3(PO4)2 + H2O
35
NH3 + HCl => NH4Cl
36
Li + H2O => LiOH + H2
37
Ca3(PO4)2 + SiO2 + C => CaSiO3 + CO + P
38
NH3 + O2 => N2 + H2O
39
FeS2 + O2 => Fe2O3 + SO2
40
C + SO2 => CS2 + CO
Balancing Chemical Equations Worksheet
Balancing Chemical Equations Worksheet
1. _____ H2 + _____ O2 _____ H2O
2. _____ N2 +_____ H2 _____ NH3
3. _____ S8 + _____ O2 _____ SO3
4. _____ N2 + _____ O2 _____ N2O
5. _____ HgO _____ Hg + _____ O2
6. _____ CO2 + _____ H2O _____ C6H12O6 + _____ O2
7. _____ Zn + _____ HCl _____ ZnCl2 + _____ H2
8. _____ SiCl4 + _____ H2O _____ H4SiO4 + _____ HCl
9. _____ Na + _____ H2O _____ NaOH + _____ H2
10. _____ H3PO4 _____ H4P2O7 + _____ H2O
11. _____ C10H16 + _____ Cl2 _____ C + _____ HCl
12. _____ CO2 + _____ NH3 _____ OC(NH2)2 + _____ H2O
13. _____ Si2H3 + _____ O2 _____ SiO2 + _____ H2O3
14. _____ Al(OH)3 + _____ H2SO4 _____ Al2(SO4)3 + _____ H2O
15. _____ Fe + _____ O2 _____ Fe2O3
16. _____ Fe2(SO4)3 + _____ KOH _____ K2SO4 + _____ Fe(OH)3
17. _____ C7H6O2 + _____ O2 _____ CO2 + _____ H2O
18. _____ H2SO4 + _____ HI _____ H2S + _____ I2 + _____ H2O
19. _____ FeS2 + _____ O2 _____ Fe2O3 + _____ SO2
20. _____ Al + _____ FeO _____ Al2O3 + _____ Fe
21. _____ Fe2O3 + _____ H2 _____ Fe + _____ H2O
22. _____ Na2CO3 + _____ HCl _____ NaCl + _____ H2O + _____ CO2
23. _____ K + _____ Br2 _____ KBr
24. _____ C7H16 + _____ O2 _____ CO2 + _____ H2O
25. _____ P4 + _____ O2 _____ P2O5
1. _____ H2 + _____ O2 _____ H2O
2. _____ N2 +_____ H2 _____ NH3
3. _____ S8 + _____ O2 _____ SO3
4. _____ N2 + _____ O2 _____ N2O
5. _____ HgO _____ Hg + _____ O2
6. _____ CO2 + _____ H2O _____ C6H12O6 + _____ O2
7. _____ Zn + _____ HCl _____ ZnCl2 + _____ H2
8. _____ SiCl4 + _____ H2O _____ H4SiO4 + _____ HCl
9. _____ Na + _____ H2O _____ NaOH + _____ H2
10. _____ H3PO4 _____ H4P2O7 + _____ H2O
11. _____ C10H16 + _____ Cl2 _____ C + _____ HCl
12. _____ CO2 + _____ NH3 _____ OC(NH2)2 + _____ H2O
13. _____ Si2H3 + _____ O2 _____ SiO2 + _____ H2O3
14. _____ Al(OH)3 + _____ H2SO4 _____ Al2(SO4)3 + _____ H2O
15. _____ Fe + _____ O2 _____ Fe2O3
16. _____ Fe2(SO4)3 + _____ KOH _____ K2SO4 + _____ Fe(OH)3
17. _____ C7H6O2 + _____ O2 _____ CO2 + _____ H2O
18. _____ H2SO4 + _____ HI _____ H2S + _____ I2 + _____ H2O
19. _____ FeS2 + _____ O2 _____ Fe2O3 + _____ SO2
20. _____ Al + _____ FeO _____ Al2O3 + _____ Fe
21. _____ Fe2O3 + _____ H2 _____ Fe + _____ H2O
22. _____ Na2CO3 + _____ HCl _____ NaCl + _____ H2O + _____ CO2
23. _____ K + _____ Br2 _____ KBr
24. _____ C7H16 + _____ O2 _____ CO2 + _____ H2O
25. _____ P4 + _____ O2 _____ P2O5
How To Balance A Chemical Equation
http://richardbowles.tripod.com/chemistry/balance.htm
This link will give you the essentials of balancing a chemical equation.
This link will give you the essentials of balancing a chemical equation.
Equation Problems
Skill Developing Problems
What is/are the product(s) containing carbon when methane, CH4, is burned in the air?
Hint . . .CO2
Generalization:Combustion of C containing compounds converts all C to CO2.
Use the common sense method to find the molecular formula for hydrogen sulfide, whose molecular weight is 34.1. (Atomic weight, H, 1.008; S, 32.066) Hint . . .H2S
Generalization:Sulfur and oxygen are group 6 elements, and they form H2O and H2S.
When 30.0 g of Al (atomic weight 27.0) is heated in oxygen (atomic mass 16.0), an aluminum oxide, Al2O3, is formed. How much oxide should be obtained. Hint . . .56.7 g A Variation:How much (in g) oxygen is required?
When KClO3 is heated, it decomposes to give solid KCl and oxygen gas. If 0.500 mol O2 is collected, how many grams of KCl should be obtained? (Atomic wt: K, 39.098; Cl, 35.453) Hint . . .24.9 g Method suggestion:
For the reaction:
2 KClO3 = 2 KCl + 3 O2 the formulation suggestion is: 2 mole KCl 74.6 g KCl
0.50 mol O2 ------------ ------------ = ??.? g KCl
3 mol O2 1 mol KCl
A solution containing pure BaCl2 is treated with excess amounts of H2SO4, and the precipitate BaSO4 is collected and dried. If 13.2 g of BaSO4 are collected, how many moles of Cl- ions are left in the solution?Atomic wt: H, 1.008; O, 16.00; S, 32.06; Cl, 35.45; Ba, 137.33. Hint . . .0.113 mol
Variations:How much (in g) BaCl2 is present in the solution?How much silver nitrate is required to precipitate all the chloride ions?
The reaction is:
BaCl2 + H2SO4 = BaSO4 + 2 H+ + 2 Cl-. 0.0566 mole of Ba correspond to 0.113 mol of Cl- in BaCl2. Method Suggestion 1 mol BaSO4 2 mol Cl-
13.2 g ----------- ----------- = 0.113 mol
233.39 g 1 mol BaSO4
A power plant burns coal, and this process is equivalent to burning 999 kg of sulfur a day. How many kg of SO2 is emitted per day if the power plant does not have pollution control devices to recover the sulfur? Atomic wt: C, 12.00; O, 16.00; S, 32.06. Hint . . .1998 kg
Further consideration:The molecular weight of SO2 is about twice the atomic weight of S. Thus the weight of SO2 is twice that of S. Variations: How much (in mole and L) SO2 is generated per day?If all SO2 is converted to H2SO4, how much (in mol and kg) sulfuric acid is produced? (3055 kg)
How many moles of water will be formed when one mole of propane C3H8 is burned in an excess amount of air? Hint . . .4 molesC3H8 + 5 O2 = 3 CO2 + 4 H2O Skill:Work out a balanced reaction equation.
Variations:How many grams of water will be produced?How many moles of CO2 will be produced?
A mixture containing Na2SO4, but no other sulfate, is analyzed by precipitation with BaCl2. A 2.37 g mixture sample gave a 2.57 g BaSO4 precipitate.
What is the percentage of Na2SO4 in the mixture? Hint . . .66.0 %
Skill:The problem illustrates a strategy for chemical analysis.
When 2.33 g of CaCl2 and Ca(NO3)2 mixture gives 2.22 g of AgCl when Ag(NO3) is used as a reagent to precipitate the chloride Cl- ions. What is the percentage of CaCl2 in the mixture?
Atomic wt: N, 14.0; O, 16.0; Cl, 35.5; Ca, 40.1; Ag, 107.9. Hint . . .36.9 %
Skill:This problem also illustrates a strategy for chemical analysis.
© CChieh@UWaterloo.ca
What is/are the product(s) containing carbon when methane, CH4, is burned in the air?
Hint . . .CO2
Generalization:Combustion of C containing compounds converts all C to CO2.
Use the common sense method to find the molecular formula for hydrogen sulfide, whose molecular weight is 34.1. (Atomic weight, H, 1.008; S, 32.066) Hint . . .H2S
Generalization:Sulfur and oxygen are group 6 elements, and they form H2O and H2S.
When 30.0 g of Al (atomic weight 27.0) is heated in oxygen (atomic mass 16.0), an aluminum oxide, Al2O3, is formed. How much oxide should be obtained. Hint . . .56.7 g A Variation:How much (in g) oxygen is required?
When KClO3 is heated, it decomposes to give solid KCl and oxygen gas. If 0.500 mol O2 is collected, how many grams of KCl should be obtained? (Atomic wt: K, 39.098; Cl, 35.453) Hint . . .24.9 g Method suggestion:
For the reaction:
2 KClO3 = 2 KCl + 3 O2 the formulation suggestion is: 2 mole KCl 74.6 g KCl
0.50 mol O2 ------------ ------------ = ??.? g KCl
3 mol O2 1 mol KCl
A solution containing pure BaCl2 is treated with excess amounts of H2SO4, and the precipitate BaSO4 is collected and dried. If 13.2 g of BaSO4 are collected, how many moles of Cl- ions are left in the solution?Atomic wt: H, 1.008; O, 16.00; S, 32.06; Cl, 35.45; Ba, 137.33. Hint . . .0.113 mol
Variations:How much (in g) BaCl2 is present in the solution?How much silver nitrate is required to precipitate all the chloride ions?
The reaction is:
BaCl2 + H2SO4 = BaSO4 + 2 H+ + 2 Cl-. 0.0566 mole of Ba correspond to 0.113 mol of Cl- in BaCl2. Method Suggestion 1 mol BaSO4 2 mol Cl-
13.2 g ----------- ----------- = 0.113 mol
233.39 g 1 mol BaSO4
A power plant burns coal, and this process is equivalent to burning 999 kg of sulfur a day. How many kg of SO2 is emitted per day if the power plant does not have pollution control devices to recover the sulfur? Atomic wt: C, 12.00; O, 16.00; S, 32.06. Hint . . .1998 kg
Further consideration:The molecular weight of SO2 is about twice the atomic weight of S. Thus the weight of SO2 is twice that of S. Variations: How much (in mole and L) SO2 is generated per day?If all SO2 is converted to H2SO4, how much (in mol and kg) sulfuric acid is produced? (3055 kg)
How many moles of water will be formed when one mole of propane C3H8 is burned in an excess amount of air? Hint . . .4 molesC3H8 + 5 O2 = 3 CO2 + 4 H2O Skill:Work out a balanced reaction equation.
Variations:How many grams of water will be produced?How many moles of CO2 will be produced?
A mixture containing Na2SO4, but no other sulfate, is analyzed by precipitation with BaCl2. A 2.37 g mixture sample gave a 2.57 g BaSO4 precipitate.
What is the percentage of Na2SO4 in the mixture? Hint . . .66.0 %
Skill:The problem illustrates a strategy for chemical analysis.
When 2.33 g of CaCl2 and Ca(NO3)2 mixture gives 2.22 g of AgCl when Ag(NO3) is used as a reagent to precipitate the chloride Cl- ions. What is the percentage of CaCl2 in the mixture?
Atomic wt: N, 14.0; O, 16.0; Cl, 35.5; Ca, 40.1; Ag, 107.9. Hint . . .36.9 %
Skill:This problem also illustrates a strategy for chemical analysis.
© CChieh@UWaterloo.ca
Lecture: Reactions and Equations
Reaction Equations
Key terms
Energy, exothermic reaction, endothermic reactionPhysical reactions, chemical reactions, phase transitionsReactants, productsReaction stoichiometry
Skills to develop
To distinguish chemical changes from physical changes.
To write chemical equations to describe a chemical reaction.
To balance chemical equations.
To calculate the quantities of reactants required or the quantities produced in a chemical reaction.
Chemical Reaction Equations
Changes in a material or system are called reactions, and they are divided into chemical and physical reactions.
Energy is the driving force of all changes, both physical and chemical reactions. Energy is always involved in these reactions. If a system is more stable by losing some energy, a reaction takes place, releasing energy. Such a reaction is said to be exothermic. Supplying energy to a system also causes a reaction. Energy absorbing reactions are called endothermic reactions. Sometimes, the amount of energy involved in a reaction may be so small that the change in energy is not readily noticeable.
An equation can be used to describe a physical reaction, which involves a change of states. For example, melting, sublimation, evaporation, and condensation can be represented as follow.
In these equations, (s) stands for solid, (l) for liquid (l), and (g) for gas,
H2O(s) ® H2O(l) . . . melting
H2O(s) ® H2O(g) . . . sublimation
C2H5OH(l) ® C2H5OH(g) . . . evaporation
NH3(g) ® NH3(l) . . . condensationIn these changes, no chemical bonds are broken or formed, and the molecular identities of the substances have not changed.
Is the phase transition between graphite and diamond is a chemical or physical reaction?
C(graphite) ® C(diamond).
The crystal structures of diamond and graphite are very different, and bonding between the carbon atoms are also different in the two solid states. Because chemical bonds are broken and new bonds are formed, the phase transition of diamond and graphite is a chemical reaction.
Chemicals or substances change converting to one or more other substances, and these changes are called chemical reactions. At the molecular level, atoms or groups of atoms rearrange resulting in breaking and forming some chemical bonds in a chemical reaction. The substances undergoing changes are called reactants, whereas substances newly formed are called products. Physical appearances of products are often different from reactants. Chemical reactions are often accompanied by the appearance of gas, fire, precipitate, color, light, sound, or odor.
These phenomena are related to energy and properties of the reactants and products. For example, the oxidation of propane releases heat and light, and a rapid reaction is an explosion,
C3H8 + 5 O2 ® 3 CO2 + 4 H2O A balanced equation also shows a macroscopic quantitative relationship. This balanced reaction equation shows that five moles of oxygen reacts with one mole of propane generating three moles of carbon dioxide and four moles of water, a total of 7 moles of products in the combustion reaction.
At the molecular level, this equation shows that for each propane molecule, 5 oxygen molecules are required. The three carbon atoms are converted to three molecules of carbon dioxide, whereas the 8 hydrogen atoms in propane are oxidized to 4 water molecules. The numbers of H, C, and O atoms are the same on both sides of the equation.
We study properties of substances so that we know how to make use of them. Tendencies of a substance to react, either by itself or with others, are important chemical properties. Via properties, we understand chemical reactions, which are best studied by experimentation and observation. After you have performed many experiments, you may generalize certain rules and facts. Knowing these rules and facts enable you to solve problems that you have not yet encountered.
The most important aspect of a chemical reaction is to know what are the reactants and what are the products. For this, the best description of a reaction is to write an equation for the reaction. A chemical reaction equation gives the reactants and products, and a balanced chemical reaction equation shows the mole relationships of reactants and products. Often, the amount of energy involved in the reaction is given. Dealing with the quantitative aspect of chemical reactions is called reaction stoichiometry.
For example, when clamshells, CaCO3, are heated, a gas CO2 will be released, leaving a white powder (solid CaO) behind. This reaction is represented by the reaction as depicted in the picture, and the equation of the reaction is written as:
CaCO3 ® CaO + CO2The equation indicates that one mole of CaCO3 gives one mole each of CaO and CO2. Amounts of substances represented by chemical formulas have been introduced on the two previous pages, and these concepts should help to figure out the stoichiometry of reactions when a reaction equation is given.
Example 1
When 10.0 g pure calcium carbonate is heated and converted to solid calcium oxide CaO, how much calcium oxide should be obtained? If the only 5.0 grams CaO is obtained, what is the actual yield? Hint:Under ideal condition, amounts of substance in the reaction equation is as indicated below:
CaCO3 ® CaO + CO2100.0 . . . . . 56 . . . 44 g/mol (formula weights) 1 mol CaCO3 1 mol CaO 56 g CaO
10.0 g CaCO3 ------------ ----------- --------- = 5.6 g CaO
100 g CaCO3 1 mol CaCO3 1 mol CaO
DiscussionAn inefficient conversion is given here, but the method shows the details of consideration. If the amount of CaO obtained is not 5.6 g, one can conclude that the sample may not be pure.
Example 2
When 10.0 g pure calcium carbonate is heated and converted to solid calcium oxide CaO, how much CO2 at standard condition is released? Hint:
CaCO3 ® CaO + CO2 1 mol CO2 22.4 L CO2
10.0 g CaCO3 ----------- ----------- = 2.24 L CO2
100 g CaCO3 1 mol CO2
Discussion
We have taken a short cut in this formulation compared to Example 1. Example 1 and 2 illustrate the evaluation of quantities in g and in L.
Writing Equations for Chemical Reactions
Chemical reaction equations truly represent changes of materials. For many reactions, we may only be able to write equations for the overall reactions. For example, common sense tells us that when sugar is fully oxidized, carbon dioxide and water are the final products. The oxidation reaction is the same as the combustion reaction. Thus we write
C12H22O11 + 12 O2 ® 12 CO2 + 11 H2O This illustrates the methods used for writing balanced reaction equations:
Determine the reactants and productsIn this case, the products are CO2 and H2O, determined by common sense. We know that.
Apply the fundamental principle of conservation of atomsNumbers of atoms of each kind must be the same before and after the reactions.
Balance one type of atoms at a timeBR> We may use H or C to begin. Since there are 12 C atoms on the left, the coefficient is 12 for CO2. Similarly, 22 H atoms produce 11 H2O molecules.
Balance the oxygen atoms on both sides. There are a total of 35 O atoms on the right hand, and the coefficient for O2 should be 11.
Example 3
The compound N2O5 is unstable at room temperature. It decomposes yielding a brown gas NO2 and oxygen. Write a balanced chemical reaction equation for its decomposition. Hint:The first step is to write an unbalanced equation indicating only the reactant and products:
N2O5 ® NO2 + O2 A N2O5 molecule decomposes into two NO2 molecule, and half of O2.
N2O5 ® 2 NO2 + 1/2O2 In order to give whole number stoichiometric coefficients to the equation, we multiply all the stoichiometric coefficients by 2.
2 N2O5 ® 4 NO2 + O2 DiscussionThis example illustrate the steps used in writing a balance equation for a chemical reaction. This balanced equation does not tell us how a N2O5 molecule decompose, it only illustrate the overall reaction.
Example 4
When solutions of CaCl2 and AgNO3 are mixed, a white precipitate is formed. The same precipitate is also observed when NaCl solution is mixed with AgCH3CO2 solution. Write a balanced equation for this the reaction between CaCl2 and AgNO3. Hint:The common ions between NaCl and CaCl2 are Cl- ions, and Ag+ ions are common between the two silver containing compounds. The question illustrates a scientific deduction used in the determination of products. The product is AgCl, and the balanced reaction is
CaCl2 + 2 AgNO3 ® 2 AgCl + Ca(NO3)2 DiscussionIn reality, solutions of salts contain ions. In this case, the solutions contain Ca2+, Cl-, Ag+, and NO3- ions. The Cl- and Ag+ ions form an insoluble solid, and a precipitate is formed,
Cl- + Ag+ ® AgCl(s) Ca2+ and NO3- are by-stander ions.
Chemical Reactions
One of the most important topics in chemistry is chemical reaction. In this page, we only concentrate on the stoichiometry conveyed by reaction equations.
Other topics related to chemical reactions are:
Excess and Limiting Reagents or reactants left over or used upFeatures of chemical reactions or classification of reactionsChemical kinetics or reaction ratesReaction mechanism or how actually reaction proceedThe first two topics are included in this group, but the later topics will be discussed in another course (CHEM123).
Balancing Redox Reactions Balancing oxidation and reduction reaction equations is a little more complicated than what we discussed here. You have to have the skills to assign oxidation states, explain oxidation and reduction in terms of oxidation-state change, and write half reaction euqations. Then you will be able to balance redox reactions. All these are given in the next module on Chemical Reactions.
http://www.science.uwaterloo.ca/~cchieh/cact/c120/reaction.html
Key terms
Energy, exothermic reaction, endothermic reactionPhysical reactions, chemical reactions, phase transitionsReactants, productsReaction stoichiometry
Skills to develop
To distinguish chemical changes from physical changes.
To write chemical equations to describe a chemical reaction.
To balance chemical equations.
To calculate the quantities of reactants required or the quantities produced in a chemical reaction.
Chemical Reaction Equations
Changes in a material or system are called reactions, and they are divided into chemical and physical reactions.
Energy is the driving force of all changes, both physical and chemical reactions. Energy is always involved in these reactions. If a system is more stable by losing some energy, a reaction takes place, releasing energy. Such a reaction is said to be exothermic. Supplying energy to a system also causes a reaction. Energy absorbing reactions are called endothermic reactions. Sometimes, the amount of energy involved in a reaction may be so small that the change in energy is not readily noticeable.
An equation can be used to describe a physical reaction, which involves a change of states. For example, melting, sublimation, evaporation, and condensation can be represented as follow.
In these equations, (s) stands for solid, (l) for liquid (l), and (g) for gas,
H2O(s) ® H2O(l) . . . melting
H2O(s) ® H2O(g) . . . sublimation
C2H5OH(l) ® C2H5OH(g) . . . evaporation
NH3(g) ® NH3(l) . . . condensationIn these changes, no chemical bonds are broken or formed, and the molecular identities of the substances have not changed.
Is the phase transition between graphite and diamond is a chemical or physical reaction?
C(graphite) ® C(diamond).
The crystal structures of diamond and graphite are very different, and bonding between the carbon atoms are also different in the two solid states. Because chemical bonds are broken and new bonds are formed, the phase transition of diamond and graphite is a chemical reaction.
Chemicals or substances change converting to one or more other substances, and these changes are called chemical reactions. At the molecular level, atoms or groups of atoms rearrange resulting in breaking and forming some chemical bonds in a chemical reaction. The substances undergoing changes are called reactants, whereas substances newly formed are called products. Physical appearances of products are often different from reactants. Chemical reactions are often accompanied by the appearance of gas, fire, precipitate, color, light, sound, or odor.
These phenomena are related to energy and properties of the reactants and products. For example, the oxidation of propane releases heat and light, and a rapid reaction is an explosion,
C3H8 + 5 O2 ® 3 CO2 + 4 H2O A balanced equation also shows a macroscopic quantitative relationship. This balanced reaction equation shows that five moles of oxygen reacts with one mole of propane generating three moles of carbon dioxide and four moles of water, a total of 7 moles of products in the combustion reaction.
At the molecular level, this equation shows that for each propane molecule, 5 oxygen molecules are required. The three carbon atoms are converted to three molecules of carbon dioxide, whereas the 8 hydrogen atoms in propane are oxidized to 4 water molecules. The numbers of H, C, and O atoms are the same on both sides of the equation.
We study properties of substances so that we know how to make use of them. Tendencies of a substance to react, either by itself or with others, are important chemical properties. Via properties, we understand chemical reactions, which are best studied by experimentation and observation. After you have performed many experiments, you may generalize certain rules and facts. Knowing these rules and facts enable you to solve problems that you have not yet encountered.
The most important aspect of a chemical reaction is to know what are the reactants and what are the products. For this, the best description of a reaction is to write an equation for the reaction. A chemical reaction equation gives the reactants and products, and a balanced chemical reaction equation shows the mole relationships of reactants and products. Often, the amount of energy involved in the reaction is given. Dealing with the quantitative aspect of chemical reactions is called reaction stoichiometry.
For example, when clamshells, CaCO3, are heated, a gas CO2 will be released, leaving a white powder (solid CaO) behind. This reaction is represented by the reaction as depicted in the picture, and the equation of the reaction is written as:
CaCO3 ® CaO + CO2The equation indicates that one mole of CaCO3 gives one mole each of CaO and CO2. Amounts of substances represented by chemical formulas have been introduced on the two previous pages, and these concepts should help to figure out the stoichiometry of reactions when a reaction equation is given.
Example 1
When 10.0 g pure calcium carbonate is heated and converted to solid calcium oxide CaO, how much calcium oxide should be obtained? If the only 5.0 grams CaO is obtained, what is the actual yield? Hint:Under ideal condition, amounts of substance in the reaction equation is as indicated below:
CaCO3 ® CaO + CO2100.0 . . . . . 56 . . . 44 g/mol (formula weights) 1 mol CaCO3 1 mol CaO 56 g CaO
10.0 g CaCO3 ------------ ----------- --------- = 5.6 g CaO
100 g CaCO3 1 mol CaCO3 1 mol CaO
DiscussionAn inefficient conversion is given here, but the method shows the details of consideration. If the amount of CaO obtained is not 5.6 g, one can conclude that the sample may not be pure.
Example 2
When 10.0 g pure calcium carbonate is heated and converted to solid calcium oxide CaO, how much CO2 at standard condition is released? Hint:
CaCO3 ® CaO + CO2 1 mol CO2 22.4 L CO2
10.0 g CaCO3 ----------- ----------- = 2.24 L CO2
100 g CaCO3 1 mol CO2
Discussion
We have taken a short cut in this formulation compared to Example 1. Example 1 and 2 illustrate the evaluation of quantities in g and in L.
Writing Equations for Chemical Reactions
Chemical reaction equations truly represent changes of materials. For many reactions, we may only be able to write equations for the overall reactions. For example, common sense tells us that when sugar is fully oxidized, carbon dioxide and water are the final products. The oxidation reaction is the same as the combustion reaction. Thus we write
C12H22O11 + 12 O2 ® 12 CO2 + 11 H2O This illustrates the methods used for writing balanced reaction equations:
Determine the reactants and productsIn this case, the products are CO2 and H2O, determined by common sense. We know that.
Apply the fundamental principle of conservation of atomsNumbers of atoms of each kind must be the same before and after the reactions.
Balance one type of atoms at a timeBR> We may use H or C to begin. Since there are 12 C atoms on the left, the coefficient is 12 for CO2. Similarly, 22 H atoms produce 11 H2O molecules.
Balance the oxygen atoms on both sides. There are a total of 35 O atoms on the right hand, and the coefficient for O2 should be 11.
Example 3
The compound N2O5 is unstable at room temperature. It decomposes yielding a brown gas NO2 and oxygen. Write a balanced chemical reaction equation for its decomposition. Hint:The first step is to write an unbalanced equation indicating only the reactant and products:
N2O5 ® NO2 + O2 A N2O5 molecule decomposes into two NO2 molecule, and half of O2.
N2O5 ® 2 NO2 + 1/2O2 In order to give whole number stoichiometric coefficients to the equation, we multiply all the stoichiometric coefficients by 2.
2 N2O5 ® 4 NO2 + O2 DiscussionThis example illustrate the steps used in writing a balance equation for a chemical reaction. This balanced equation does not tell us how a N2O5 molecule decompose, it only illustrate the overall reaction.
Example 4
When solutions of CaCl2 and AgNO3 are mixed, a white precipitate is formed. The same precipitate is also observed when NaCl solution is mixed with AgCH3CO2 solution. Write a balanced equation for this the reaction between CaCl2 and AgNO3. Hint:The common ions between NaCl and CaCl2 are Cl- ions, and Ag+ ions are common between the two silver containing compounds. The question illustrates a scientific deduction used in the determination of products. The product is AgCl, and the balanced reaction is
CaCl2 + 2 AgNO3 ® 2 AgCl + Ca(NO3)2 DiscussionIn reality, solutions of salts contain ions. In this case, the solutions contain Ca2+, Cl-, Ag+, and NO3- ions. The Cl- and Ag+ ions form an insoluble solid, and a precipitate is formed,
Cl- + Ag+ ® AgCl(s) Ca2+ and NO3- are by-stander ions.
Chemical Reactions
One of the most important topics in chemistry is chemical reaction. In this page, we only concentrate on the stoichiometry conveyed by reaction equations.
Other topics related to chemical reactions are:
Excess and Limiting Reagents or reactants left over or used upFeatures of chemical reactions or classification of reactionsChemical kinetics or reaction ratesReaction mechanism or how actually reaction proceedThe first two topics are included in this group, but the later topics will be discussed in another course (CHEM123).
Balancing Redox Reactions Balancing oxidation and reduction reaction equations is a little more complicated than what we discussed here. You have to have the skills to assign oxidation states, explain oxidation and reduction in terms of oxidation-state change, and write half reaction euqations. Then you will be able to balance redox reactions. All these are given in the next module on Chemical Reactions.
http://www.science.uwaterloo.ca/~cchieh/cact/c120/reaction.html
Chapter 8 Vocabulary
activity series of metals
complete ionic equation
balanced equation
decomposition reaction
catalyst
double-replacement reaction
chemical equation
net ionic equation
coefficient
single-replacement reaction
combination reaction
skeleton equation
combustion equation
spectator ion
complete ionic equation
balanced equation
decomposition reaction
catalyst
double-replacement reaction
chemical equation
net ionic equation
coefficient
single-replacement reaction
combination reaction
skeleton equation
combustion equation
spectator ion
Tuesday, October 20, 2009
Monday, October 19, 2009
Naming Compounds Practice Worksheets
http://misterguch.brinkster.net/ioniccovalentworksheets.html
Ionic Compound Names and Formulas
For the list on the left, name the compound. For the list on the right, give the chemical formula that corresponds to the name
Name Formula
1) NaF 13) potassium fluoride
2) K2CO3 14) ammonium sulfate
3) MgCl2 15) magnesium iodide
4) Be(OH)2 16) copper (II) sulfite
5) SrS 17) aluminum phosphate
6) Cu2S 18) lead (II) nitrite
7) ZnI2 19) cobalt (II) selenide
8) Ca3(PO4)2 20) silver cyanide
9) NH4I 21) copper (II) bicarbonate
10) Mn(NO3)3 22) iron (II) oxide
11) FePO4 23) lithium cyanide
12) CoCO3 24) lead (IV) sulfite
Naming Covalent Compounds Worksheet
Write the formulas for the following covalent compounds:
1) antimony tribromide __________________________________
2) hexaboron silicide __________________________________
3) chlorine dioxide __________________________________
4) hydrogen iodide __________________________________
5) iodine pentafluoride __________________________________
6) dinitrogen trioxide __________________________________
7) ammonia __________________________________
8) phosphorus triiodide __________________________________
Write the names for the following covalent compounds:
9) P4S5¬ __________________________________
10) O2 __________________________________
11) SeF6 __________________________________
12) Si2Br¬6 __________________________________
13) SCl4 __________________________________
14) CH4 __________________________________
15) B2Si __________________________________
16) NF3 __________________________________
Ionic Compound Names and Formulas
For the list on the left, name the compound. For the list on the right, give the chemical formula that corresponds to the name
Name Formula
1) NaF 13) potassium fluoride
2) K2CO3 14) ammonium sulfate
3) MgCl2 15) magnesium iodide
4) Be(OH)2 16) copper (II) sulfite
5) SrS 17) aluminum phosphate
6) Cu2S 18) lead (II) nitrite
7) ZnI2 19) cobalt (II) selenide
8) Ca3(PO4)2 20) silver cyanide
9) NH4I 21) copper (II) bicarbonate
10) Mn(NO3)3 22) iron (II) oxide
11) FePO4 23) lithium cyanide
12) CoCO3 24) lead (IV) sulfite
Naming Covalent Compounds Worksheet
Write the formulas for the following covalent compounds:
1) antimony tribromide __________________________________
2) hexaboron silicide __________________________________
3) chlorine dioxide __________________________________
4) hydrogen iodide __________________________________
5) iodine pentafluoride __________________________________
6) dinitrogen trioxide __________________________________
7) ammonia __________________________________
8) phosphorus triiodide __________________________________
Write the names for the following covalent compounds:
9) P4S5¬ __________________________________
10) O2 __________________________________
11) SeF6 __________________________________
12) Si2Br¬6 __________________________________
13) SCl4 __________________________________
14) CH4 __________________________________
15) B2Si __________________________________
16) NF3 __________________________________
Bellringer 6
Complete the following table:
Element # Electrons # Valence Electrons Oxidation # (Charge)
Na
S
He
Ar
Si
Element # Electrons # Valence Electrons Oxidation # (Charge)
Na
S
He
Ar
Si
Thursday, October 15, 2009
Bellringer 5
Valence electrons are the electrons that
a. orbit the outside shell.
b. are stable.
c. do not have a charge.
d. have no energy.
a. orbit the outside shell.
b. are stable.
c. do not have a charge.
d. have no energy.
Monday, October 12, 2009
Lab 2: Naming Chemical Compounds
Table top exercise to match name of chemical compound to its formula.
Naming Chemical Compounds
This link will provide with you a series of videos on naming chemical compounds:
http://www.onlinemathlearning.com/chemical-names.html
http://www.onlinemathlearning.com/chemical-names.html
Lecture, Chapter 6
Compounds
A compound is a group of atoms with a specific number and type of atoms arranged in a specific way. Exactly the same elements in exactly the same proportions are in every bit of the compound.
Example: Water is a compound composed of one oxygen atom and two hydrogen atoms. Each hydrogen atom is attached to an oxygen atom by a chemical bond. H2O is the formula for the compound, water.
If any other elements are attached, it is not water. For example, H2S is hydrogen sulfide. Hydrogen sulfide does not have the same types of atoms as water, so it is a different compound.
If a different number of atoms of hydrogen or oxygen are attached, it is not water. H2O2 is the formula for hydrogen peroxide. It might have the right elements in it to be water, but it does not have them in the right proportion. A molecule is a single formula of a compound joined by covalent bonds.
The Law of Constant Proportions states that a given compound always contains the same proportion by weight of the same elements.
Electron Configuration and Valence Electrons
In a stable atom, the number of electrons is equal to the number of protons.
Electrons in atoms are present in discrete orbits or "shells" around the nucleus of the atom.
There is a ranking or heirarchy of the shells, with the shells further from the nucleus having a higher energy.
The innermost electron shell holds only two electrons.
The outermost shell contains the valence electrons. The maximum number of electrons that can occupy the outer shell is eight. When there are eight electrons in the outer shell, it is said to have an octet of electrons.
The valence of an atom is the likely charge it will take on as an ion.
A valence is the amount of positive or negative charge on an ion of an element.
Example: Hydrogen only has one electron. It can lose an electron to become H+, a hydrogen ion, or it can gain an electron to become H-, a hydride ion.
The Octet Rule
The octet rule states that atoms are most stable when they have a full shell of 8 electrons in the outside electron shell.
Octet = 8
An atom with eight electrons in the outer shell is more stable than an atom which as fewer electrons in the outer shell.
The exception to this is Helium (atomic number 2) which only has two electrons in its outer shell. It has a full shell, so it is a stable inert element.
Valence electrons are the only electrons involved in chemical bonds.
Atoms will form chemical bonds with other atoms by either sharing electrons, or by transferring electrons in order to complete their octet and get 8 electrons in the outer shell.
Ions
In a stable atom, the number of electrons is equal to the number of protons.
An atom which has a different number of electrons than it does protons is called an ion.
Ions are charged particles. Types of ions:
Cation - A positively charged ion.A cation is an atom or group of atoms with a net positive charge, caused by the loss of one or more electrons. Examples: Na+, NH4+, Mg+2
Anion - a negatively charged ion.An anion is an atom or group of atoms with a net negative charge, caused by the gain of one or more electrons.Examples: F-, S2-, NO3-
Polyatomic ion - a group of atoms which function as a group and which has a net positive or negative charge (cation or anion).Examples: NH4+ or NO3-
The Periodic Chart can show how the octet rule works. All of the Group I elements have one electron in the outside shell and they all have a valence of plus one. Group I elements will lose that one electron in the outside shell, to become a single positive ion with a full electron shell of eight electrons (an octet) in the s and p subshells under it.
Bonding
A bond is an attachment among atoms. Atoms may be held together for any of several reasons, but all bonds have to do with the electrons (particularly the outside electrons) of atoms.
There are several types of bonds:
Ionic bonds occur due to a full electrical charge difference attraction.
Covalent bonds occur due to sharing electrons.
There are bonds that come about from partial charges or the position or shape of electrons about an atom.
Ionic Bonds
The attraction between a positive ion and a negative ion is an ionic bond.
Some atoms (such as metals) tend to lose electrons to make the outside ring of electrons more stable. When an atom loses electrons it becomes a positive ion (or cation) because the number of protons exceeds the number of electrons.
Other atoms tend to gain electrons to complete the outside electron ring. The non-metal ions tend to gain electrons to fill out the outer shell. When the number of electrons exceeds the number of protons, the ion is negative. (Non-metal ions and most of the polyatomic ions have a negative charge.)
Ionic compounds - composed of cations and anions which are ionically bonded to each other due to attractions of opposite charges
1. Cations and anions combine in a ratio that produces a neutral compound; smallest whole number ratio is used for formula of an ionic compound.
e.g., Na+ + Cl- --> NaCl (one of each is needed to balance the charges: +1 and -1)
Mg+2 + Cl- ---> MgCl2(two Cl's are needed to balance the charges since Cl is -1 and Mg is +2 charge)
2. Cation is listed first, then anion in the formula
http://facstaff.gpc.edu/~pgore/PhysicalScience/Naming-chemical-compounds.html
A compound is a group of atoms with a specific number and type of atoms arranged in a specific way. Exactly the same elements in exactly the same proportions are in every bit of the compound.
Example: Water is a compound composed of one oxygen atom and two hydrogen atoms. Each hydrogen atom is attached to an oxygen atom by a chemical bond. H2O is the formula for the compound, water.
If any other elements are attached, it is not water. For example, H2S is hydrogen sulfide. Hydrogen sulfide does not have the same types of atoms as water, so it is a different compound.
If a different number of atoms of hydrogen or oxygen are attached, it is not water. H2O2 is the formula for hydrogen peroxide. It might have the right elements in it to be water, but it does not have them in the right proportion. A molecule is a single formula of a compound joined by covalent bonds.
The Law of Constant Proportions states that a given compound always contains the same proportion by weight of the same elements.
Electron Configuration and Valence Electrons
In a stable atom, the number of electrons is equal to the number of protons.
Electrons in atoms are present in discrete orbits or "shells" around the nucleus of the atom.
There is a ranking or heirarchy of the shells, with the shells further from the nucleus having a higher energy.
The innermost electron shell holds only two electrons.
The outermost shell contains the valence electrons. The maximum number of electrons that can occupy the outer shell is eight. When there are eight electrons in the outer shell, it is said to have an octet of electrons.
The valence of an atom is the likely charge it will take on as an ion.
A valence is the amount of positive or negative charge on an ion of an element.
Example: Hydrogen only has one electron. It can lose an electron to become H+, a hydrogen ion, or it can gain an electron to become H-, a hydride ion.
The Octet Rule
The octet rule states that atoms are most stable when they have a full shell of 8 electrons in the outside electron shell.
Octet = 8
An atom with eight electrons in the outer shell is more stable than an atom which as fewer electrons in the outer shell.
The exception to this is Helium (atomic number 2) which only has two electrons in its outer shell. It has a full shell, so it is a stable inert element.
Valence electrons are the only electrons involved in chemical bonds.
Atoms will form chemical bonds with other atoms by either sharing electrons, or by transferring electrons in order to complete their octet and get 8 electrons in the outer shell.
Ions
In a stable atom, the number of electrons is equal to the number of protons.
An atom which has a different number of electrons than it does protons is called an ion.
Ions are charged particles. Types of ions:
Cation - A positively charged ion.A cation is an atom or group of atoms with a net positive charge, caused by the loss of one or more electrons. Examples: Na+, NH4+, Mg+2
Anion - a negatively charged ion.An anion is an atom or group of atoms with a net negative charge, caused by the gain of one or more electrons.Examples: F-, S2-, NO3-
Polyatomic ion - a group of atoms which function as a group and which has a net positive or negative charge (cation or anion).Examples: NH4+ or NO3-
The Periodic Chart can show how the octet rule works. All of the Group I elements have one electron in the outside shell and they all have a valence of plus one. Group I elements will lose that one electron in the outside shell, to become a single positive ion with a full electron shell of eight electrons (an octet) in the s and p subshells under it.
Bonding
A bond is an attachment among atoms. Atoms may be held together for any of several reasons, but all bonds have to do with the electrons (particularly the outside electrons) of atoms.
There are several types of bonds:
Ionic bonds occur due to a full electrical charge difference attraction.
Covalent bonds occur due to sharing electrons.
There are bonds that come about from partial charges or the position or shape of electrons about an atom.
Ionic Bonds
The attraction between a positive ion and a negative ion is an ionic bond.
Some atoms (such as metals) tend to lose electrons to make the outside ring of electrons more stable. When an atom loses electrons it becomes a positive ion (or cation) because the number of protons exceeds the number of electrons.
Other atoms tend to gain electrons to complete the outside electron ring. The non-metal ions tend to gain electrons to fill out the outer shell. When the number of electrons exceeds the number of protons, the ion is negative. (Non-metal ions and most of the polyatomic ions have a negative charge.)
Ionic compounds - composed of cations and anions which are ionically bonded to each other due to attractions of opposite charges
1. Cations and anions combine in a ratio that produces a neutral compound; smallest whole number ratio is used for formula of an ionic compound.
e.g., Na+ + Cl- --> NaCl (one of each is needed to balance the charges: +1 and -1)
Mg+2 + Cl- ---> MgCl2(two Cl's are needed to balance the charges since Cl is -1 and Mg is +2 charge)
2. Cation is listed first, then anion in the formula
http://facstaff.gpc.edu/~pgore/PhysicalScience/Naming-chemical-compounds.html
Bellringer 3
Hydrogen can readily donate its electron to form a ________ .
a. anion
b. cation
c. lion
d. bionic atom
a. anion
b. cation
c. lion
d. bionic atom
Friday, October 9, 2009
Six Weeks Exam RETAKE
You have the opportunity to retake the six weeks exam Tuesday/Wednesday in class.
STUDY this weekend!
Bellringers
Notes
Vocabulary
STUDY this weekend!
Bellringers
Notes
Vocabulary
Monday Madness Bus Routes
Monday Madness Bus Routes
To South Hills High School
5:20 PM WORTH HEIGHTS ELEM 184
5:24 PM RICHARD WILSON ELEM 165
5:28 PM HUBBARD ELEM 137
5:34 PM GREENBRIAR ELEM 134
5:38 PM SEMINARY HILLS PARK 226
5:46 PM ALICE CONTRERAS ELEMENTARY 220
5:52 PM SOUTH HILLS ELEM 167
5:57 PM WESTCREEK ELEM 178
6:00 PM SOUTH HILLS HIGH
From South Hills High School
8:00 PM SOUTH HILLS HIGH
8:05 PM WESTCREEK ELEM 178
8:12 PM SOUTH HILLS ELEM 167
8:17 PM ALICE CONTRERAS ELEMENTARY 220
8:24 PM RICHARD WILSON ELEM 165
8:27 PM WORTH HEIGHTS ELEM 184
8:32 PM HUBBARD ELEM 137
8:37 PM SEMINARY HILLS PARK 226
8:40 PM GREENBRIAR ELEM 134
To South Hills High School
5:20 PM WORTH HEIGHTS ELEM 184
5:24 PM RICHARD WILSON ELEM 165
5:28 PM HUBBARD ELEM 137
5:34 PM GREENBRIAR ELEM 134
5:38 PM SEMINARY HILLS PARK 226
5:46 PM ALICE CONTRERAS ELEMENTARY 220
5:52 PM SOUTH HILLS ELEM 167
5:57 PM WESTCREEK ELEM 178
6:00 PM SOUTH HILLS HIGH
From South Hills High School
8:00 PM SOUTH HILLS HIGH
8:05 PM WESTCREEK ELEM 178
8:12 PM SOUTH HILLS ELEM 167
8:17 PM ALICE CONTRERAS ELEMENTARY 220
8:24 PM RICHARD WILSON ELEM 165
8:27 PM WORTH HEIGHTS ELEM 184
8:32 PM HUBBARD ELEM 137
8:37 PM SEMINARY HILLS PARK 226
8:40 PM GREENBRIAR ELEM 134
Monday Madness
If you are wanting some extra help in any content area, come to South Hills Scorpion’s Monday Madness. Bussing and snacks is provided.
2009 - 2010 Schedule
Dates
October 19, 2009
October 26, 2009
November 2, 2009
November 16, 2009
November 30, 2009
December 7, 2009
December 14, 2009
January 11, 2010
2009 - 2010 Schedule
Dates
October 19, 2009
October 26, 2009
November 2, 2009
November 16, 2009
November 30, 2009
December 7, 2009
December 14, 2009
January 11, 2010
Student Goal Setting/Conference
Name: ____________________________________ Grade:________________________
Subject:___________________________________ Date:_________________________
TAKS Objective
2007-08 TAKS
2008-2009 TAKS
Student Goal
Assessment 1
Assessment 2
Correct/
Tested
Correct/
Tested
Correct/
Tested
Correct/
Tested
Correct/
Tested
1. Understand the nature of science
2. Understand organization of living systems
3. Understand the interdependence of organisms and the environment
4. Understand the properties and structures of matter
5. Understand motion, forces, and energy
Total
Reuired for Passing
Scale Score
Required for Passing
2100
2100
2100
Required for Commended
2400
2400
2400
Te objective(s) I struggled in was/were: _________________________________________________________________________________________
_________________________________________________________________________________________
Assessment
Objective Covered
SE Covered
1.
2.
3.
4.
5.
Planned interventions to promote success:
_____________________________________________________________
_____________________________________________________________
_____________________________________________________________
My Grades/Attendance/Missing Assignments:
GOAL
1ST
2ND
3RD
4th
5th
6th
My Reflection/ Goals:
____________________________________________________________________________________________________________________________________________________________________
____________________________________________________________________________________________________________________________________________________________________
____________________________________________________________________________________________________________________________________________________________________
I am committed to success… No excuses!
Teacher Name_________________________________________ Date:_________________________
Student Signature______________________________________ Date:_________________________
Parent Signature_______________________________________ Date:_________________________
Subject:___________________________________ Date:_________________________
TAKS Objective
2007-08 TAKS
2008-2009 TAKS
Student Goal
Assessment 1
Assessment 2
Correct/
Tested
Correct/
Tested
Correct/
Tested
Correct/
Tested
Correct/
Tested
1. Understand the nature of science
2. Understand organization of living systems
3. Understand the interdependence of organisms and the environment
4. Understand the properties and structures of matter
5. Understand motion, forces, and energy
Total
Reuired for Passing
Scale Score
Required for Passing
2100
2100
2100
Required for Commended
2400
2400
2400
Te objective(s) I struggled in was/were: _________________________________________________________________________________________
_________________________________________________________________________________________
Assessment
Objective Covered
SE Covered
1.
2.
3.
4.
5.
Planned interventions to promote success:
_____________________________________________________________
_____________________________________________________________
_____________________________________________________________
My Grades/Attendance/Missing Assignments:
GOAL
1ST
2ND
3RD
4th
5th
6th
My Reflection/ Goals:
____________________________________________________________________________________________________________________________________________________________________
____________________________________________________________________________________________________________________________________________________________________
____________________________________________________________________________________________________________________________________________________________________
I am committed to success… No excuses!
Teacher Name_________________________________________ Date:_________________________
Student Signature______________________________________ Date:_________________________
Parent Signature_______________________________________ Date:_________________________
To Make Your Own Videos Via Animoto
Thanks for signing-up to use Animoto in the classroom!
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Your Classroom Code is:A4E10909lab
To learn how to set you & your students up with All-Access via yourClassroom Code, go to:http://animoto.com/education/getting_started
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Bellringer 2
Bass populations in North Texas lakes have been on a slow decline. Water samples from the area lake near a nuclear plant indicate a pH of 4 where a year prior it was at an optimum of pH 7. What information can you deduct from this information?
a. Bass are swimming elsewhere.
b. Bass are jumping out of the water.
c. The water is contaminated.
d. Overfishing.
a. Bass are swimming elsewhere.
b. Bass are jumping out of the water.
c. The water is contaminated.
d. Overfishing.
Wednesday, October 7, 2009
Bellringer 1
Sucrose reacted with sulfuric acid to produce the following:
25 grams of carbon
12 grams of sulfur
9 grams of hydrogen
7 grams of oxygen
Calculate the percent produced of each product.
25 grams of carbon
12 grams of sulfur
9 grams of hydrogen
7 grams of oxygen
Calculate the percent produced of each product.
Tuesday, October 6, 2009
Second Six Weeks Begins!
The second six weeks begins this week. Let's start out the some goals:
1. How am going to improve this six weeks?
2. What do I want to focus on?
1. How am going to improve this six weeks?
2. What do I want to focus on?
Monday, October 5, 2009
Chapter 6 Vocabulary
Make sure you take the time to define the following words:
anion
ion
molecular formula
binary compound
ionic compound
molecule
cation
law of definite proportions
monatomic ion
chemical formula
law of multiple proportions
polyatomic ion
formula unit
molecular compound
ternary compound
anion
ion
molecular formula
binary compound
ionic compound
molecule
cation
law of definite proportions
monatomic ion
chemical formula
law of multiple proportions
polyatomic ion
formula unit
molecular compound
ternary compound
Class Survey
Link to the following survey and complete it, earn a free homework pass.
http://www.surveymonkey.com/s.aspx?sm=rDN3C9W1qV17ulEIyZgEEA_3d_3d
http://www.surveymonkey.com/s.aspx?sm=rDN3C9W1qV17ulEIyZgEEA_3d_3d
Thursday, October 1, 2009
Lab 1: pH
The pH scale ranges from 0 to 14. It measures the acidity or basicity of a solution.
A pH of 7 means it is a neutral solution. Pure water has a pH of 7.
A pH of less than 7 means the solution is acidic. A pH of more than 7 means the solution is basic.
The less pH, the more acidic the solution is. The more pH, the more basic the solution is.
pH stands for the power of H, or the amount of H+ ions acids or bases take or contribute in solution. pH equals the negative log of the concentration of H+.pH = -log[H+]When the concentration of H+ ions in a solution is 10-14, the pH is 14. In pure water, the average concentration of H+ ions is 10-7.
You will be performing a pH test on different solutions. You will determine the pH of the solutions with test strips and compare them to pH color chart. You will identify the similarities and differences of the different solutions.
For a chart of the pH scale, go to
http://staff.jccc.net/PDECELL/chemistry/phscale.html
http://www.johnkyrk.com/pH.html
A pH of 7 means it is a neutral solution. Pure water has a pH of 7.
A pH of less than 7 means the solution is acidic. A pH of more than 7 means the solution is basic.
The less pH, the more acidic the solution is. The more pH, the more basic the solution is.
pH stands for the power of H, or the amount of H+ ions acids or bases take or contribute in solution. pH equals the negative log of the concentration of H+.pH = -log[H+]When the concentration of H+ ions in a solution is 10-14, the pH is 14. In pure water, the average concentration of H+ ions is 10-7.
You will be performing a pH test on different solutions. You will determine the pH of the solutions with test strips and compare them to pH color chart. You will identify the similarities and differences of the different solutions.
For a chart of the pH scale, go to
http://staff.jccc.net/PDECELL/chemistry/phscale.html
http://www.johnkyrk.com/pH.html
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