Chemistry Spring Semester Final Study Guide
REVIEW FROM MS. HAUGE
1. Give an example of a non polar bond
2. Describe how a polar covalent bond’s electrons are shared or taken
3. Naming compounds
a. CuO
b. B5H9
c. N2O5
d. SO3
4. Unique properties of water and what type of bonds they have.
5. What is the oxidation number of phosphorus in H3PO4?
6. Location of valence electrons
7. What is the correct structure for HCN?
8. What is a neutral group of atoms held together by covalent bonds?
9. What is it called when a chemical bond forms when atoms share electrons?
a. ionic
b. orbital
c. energy
d. covalent
10. What is the Mass of 2.5 moles of carbon?
a. 12.0g b. 18.0g c. 24.0g d. 30.0g
11. What is the total number of moles of copper are there in 180.0g of copper?
a. 2.833 moles
b. .3530 moles
c. 11,440 moles
d. 18.0 moles
12. What is the shape of a molecule with a central atom with three identical bonded atoms and no lone pairs?
13. What is the correct formula for dinitrogen?
14. How many moles of F are there in 1 mole of CF4
a. 4 b. 3 c. 2 d. 1
15. What is the molar mass of Ca(OH)2
a. 57.1g b. 74.1g c. 97.2g d. 58.1g
16. What is the VSEPR Theory? What does it help predict?
17. How many atoms are in a molecule of C12H22O11?
18. Draw and label the different shapes that molecules can exhibit: bent, trigonal planar, tetrahedral, and pyramidal.
19. Identify the shape of this molecule.
20. Using the electronegativity table, determine the type of bond in:
a. NaCl
b. H2
c. SO:
21. How many atoms are there in 3.00 moles of uranium?
a. 714. b. 1.81 X 1024 c. 238. d. 2.01 X 1023
22. How many atoms are there in a molecule of C12H22O11 ?
a. 6.022 X 1023 b. 22 c. 45 d. 56
23. What is the mass of 1.000 moles of MgCl2 ?
a. 223.2 grams b. 95.3 grams c. 44.64 grams d. 0.02240 grams
24. What is the percentage of chlorine in NaCl?
25. When an equation is used to calculate the amount of product that will form during a reaction, then the value obtained is called the______.
26. When two substances react to form products, the reactant which is used up is called the____.
27. The number of particles in a mole is called what?
28. In a chemical equation, what do the coefficients tell us?
29. If this is the correct Lewis dot structure of SeO2, what is its molecular shape?
30. Compared to the bonds between the atoms inside the molecules, forces between molecules are:
a. Weaker
b. Stronger
c. about the same
d. stronger or weaker depending on the compounds
31. A formula that shows the simplest whole-number ratio of the atoms of a compound is a ______formula.
32. What are the different possible signs that signify that a chemical reaction took place?
33. In words, 2CO + O2 à 2CO2 is:
a. Carbon monoxide decomposes into oxygen and carbon dioxide
b. Carbon monoxide reacts with oxygen to produce carbon dioxide
c. Carbon dioxide decomposes into oxygen and carbon monoxide
d. Carbon dioxide reacts with oxygen to produce carbon monoxide
34. What number should products and reactants always have equal amounts of when writing a chemical equation?
35. What is the mass of 1 mole of zinc?
36. Which type of stoichiometric calculation problems does not require the use of the molar mass?
a. Mass-mass problems
b. Mass-particle problems
c. Mole-mass problems
d. Mole-mole problems
37. What is the empirical formula of the compound whose molecular formula is P4O10?
38. Which type of reaction is this?
2H2O + O2 à 2H2O2
39. Which type of reaction is this?
2NaBr + CaF2 à 2NaF + CaBr2
40. Which equation is balanced?
a. 3Al(OH)3 +2H2SO4 à Al2(SO4)3 + 6H2O
b. 2Al(OH)3 +3H2SO4 à 2Al2(SO4)3 + 4H2O
c. 3Al(OH)3 +3H2SO4 à Al2(SO4)3 + 2H2O
d. 2Al(OH)3 +3H2SO4 à Al2(SO4)3 + 6H2O
41. Which type of reaction is this? 2 H2O2 à 2H2O + O2
42. Know and give an example of the following different types of reactions:
a. Decomposition
b. Double replacement
c. Single displacement
d. synthesis
43. Which is the correct mole ratio of AlBr3 to KBr in the chemical reaction (hint balance the equation)
AlBr3 + Kà KBr + Al
a. 1:1
b. 3:4
c. 1:3
d. 1:2
44. Avogadro’s number relates
a. Mass-moles
b. Mass- molecules
c. Moles-molecules
d. Mass-mass
45. What is the percent by mass of oxygen in MgO?
a. 20% b. 40% c. 60% d. 80%
46. A compound is 86% carbon and 14% hydrogen by mass. What is the empirical formula for this compound?
a. CH b. CH2 c. CH3 d. CH4
47. In this reaction: A + B à C + D, if there is not enough A to react with all of B, then B is called a ______reactant.
Refer to the following reaction equation.
2Al + 3FeO à 3Fe + Al2O3
48. How many moles of Al are needed to completely react with 1.2 mole of FeO?
49. How many grams of Fe are produced by reacting 3.4g of Al?
50. In a chemical equation, the symbol (aq) means
Consider the following reaction equation
2 KClO3(s)-->2KCl (s)+3O2(g)
51. How many grams of O2 are produced by decomposing 154.0g KCLO3?
52. How many grams of KCLO3 are needed to produce 56 g of KCl?
SOLUTIONS (CH. 12)
53. An increase in the temperature of a solution usually does what to the solubility of a gas?
54. What is a solute? What is a solvent?
55. What is the molarity of a solution that contains 17g of NH3 in 0.50L of solution?
56. What is an electrolyte?
57. What is the difference between molarity and molality?
58. Define: saturated, unsaturated, supersaturated
59. In water, a substance that ionizes completely in solution is what a ______electrolyte
60. How many moles of NaF are needed to make 2.00 liters of a 0.250M solution?
a. 0.500 b. 1.00 c. 1.50 d. 2.00
ACIDS AND BASES (CH. 14)
61. What is the name of HBr?
62. What is the name of HNO2 ?
63. What is the name of H2SO4?
64. The pH of a solution is 10. What is [H3O] ?
65. The pH of a solution is 10. Then it is . . .
a. acidic b. basic c. neutral
66. What is the conjugate base of HSO4- ?
67. The concentration of a solution of HCl is 10-3 M. The pH is:
a. -3 b. 3 c. 11 d. -11
68. According to the Bronsted-Lowry definition, what is a base? What is an acid?
69. Identify the Bronsted- Lowry acid in the following reaction
H2O + CO32- à HCO3- + OH-
70. What is a neutralization reaction? What are its products?
71. The function of a buffer is to…
72. What are real-life examples of why buffers are needed (on your ppt)?
73. A substance that ionizes completely in water and produces H3O+ is a
a. Weak acid
b. Strong acid
c. Weak base
d. Strong base
74. The neutralization reaction between Al(OH)3 and HNO3 produces what two products?
75. What is a salt?
GAS LAWS
76. What is a gas?
77. Describe kinetic theory.
78. State and define the 4 properties of gas.
79. State and define the following laws: Boyle’s law, Charles’ law, Avogadro’s law, Gay-Lussac’s law.