Download 60. Write the electron configuration for Zn

Spring Semester Final Exam Study Guide
Honors Chemistry
Name ________________________
Period ________________________
Naming and Formula Writing
AlCl3
1. Write the name or formula for each of the following:
HClO2
Mercury (II) bromide
Cu2S
(NH4)2SO4
Phosphorous acid
NaCN
I4O10
Nitric acid
HI
H3N
Sodium nitrite
PCl3
NiN
Magnesium hydroxide
CrBr3
H3PO4
Carbon trisulfide
Chemical Equations
2. State the law of conservation of matter.
2H2 + O2 → 2H2O
3. Using the chemical equation above:
a. Underline the subscripts
b. Box the coefficients
c. Identify the diatomic molecules
4. Balance the following equations and identify the type of reaction (synthesis,
decomposition, single replacement, double replacement, combustion)
a. ___N2 + ___H2  ___NH3
b. ___KClO3  ___KCl + ___O2
c. ___NaCl + ___F2  ___NaF + ___Cl2
d. ___AgNO3 + ___MgCl2 ___AgCl + ___Mg(NO3)2
e. Aluminum bromide reacts with potassium sulfate to yield potassium
bromide and aluminum sulfate.
1
Spring Semester Final Exam Study Guide
f. Sodium and water form sodium hydroxide and hydrogen
g. Silver oxide decomposes to silver and oxygen.
h. Potassium and magnesium bromide yields potassium bromide and
magnesium
5. Identify the following symbols:
a. (aq)
b. (s)
c. (l)
d. (g)
e. H
f. 
g. M
6. What type of reaction (endothermic, exothermic) has more energy in the
products than reactants? What is the sign for H?
7. What type of reaction has more energy in the reactants than products? What
is the sign for H?
8. How many kJ of heat would you expect to be transferred when 6.44g of sulfur
react with excess oxygen gas to produce sulfur trioxide? H = -791.4kJ
The Mole
9. How many atoms are in a mole of Ca?
2
Spring Semester Final Exam Study Guide
10. How many O atoms are on 3.0 x 1015 molecules of CO2?
11. How many atoms are in 2.6 moles of Al?
12. Convert 6689 moles of NaCl to molecules of NaCl.
13. Convert 3.2 x 1028 molecules of hydrofluoric acid to moles.
14. How many moles are in 60,000,000,000 atoms of Zn?
15. Calculate the molar mass of each of the following compounds:
a. NaOH
b. MgCl2
c. Barium phosphate
16. How many grams of sulfur are in 5.23 moles of sulfur?
17. Convert 192 moles of HCl to g of HCl
18. Convert 510.2 g of aluminum hydroxide to moles.
19. How many moles are in 62 g of CO2 ?
3
Spring Semester Final Exam Study Guide
Stoichiometry
20. Aluminum reacts with oxygen to form aluminum oxide.
a. How many moles of aluminum are needed to form 2.3moles of
aluminum oxide?
b. How many moles of oxygen are required to react completely with 8.4
moles of aluminum?
21. Calcium chloride reacts with potassium sulfide to produce potassium chloride
and calcium sulfide. How many grams of potassium chloride are produced when
50.0 grams of calcium chloride react with xs potassium sulfide?
22. Potassium chlorate decomposes into potassium chloride and oxygen gas.
What volume of oxygen gas will be produced is 25.0 grams of potassium chlorate
decompose at STP.
23. Predict the products and write a balanced equation for the following: Silver
nitrate reacts with barium chloride to produce ___________ and ____________?
Balanced equation: ________________________________________________
24. Using the equation above if 5.0 g of silver nitrate react with 4.0 g of barium
chloride how much silver chloride will be produced? What is the limiting
reactant? How many grams of excess reagent remains?
4
Spring Semester Final Exam Study Guide
Empirical Formulas / % yield
25. A compound is composed of 7.20g of C, 1.20g of hydrogen and 9.60g of
oxygen. The molar mass of the compound is 180g/mole. Determine the
empirical and the molecular formula of the compound.
26. Define:
a. Actual yield
b. Theoretical yield
c. % yield
27. In the reaction between excess K(s) and 4.28 g of O2(g), potassium oxide is
formed . What mass would you expect to form (theoretical yield)? If 17.36 g of
K2O is actually produced, what is the percent yield?
Gases (again)
28. Name four variables that affect gas behavior and identify the relationship.
a. V T
b. P T
c. P V
d. P n
29. Write the equation for the ideal gas law. When is the ideal gas law used?
What units do the variables need to be in to use the Ideal Gas Law?
30. A gas has a pressure of 50.0mmHg at 540K. What will be the pressure at
56C, assuming volume does not change
5
Spring Semester Final Exam Study Guide
31. An underground cavern contains 98 moles of methane gas at a pressure of
15atm and a temperature of 22C. How many liters of methane does this natural
gas deposit contain?
32. What volume does 16.0 g of O2 occupy at STP?
33. When calcium carbonate is heated strongly, carbon dioxide gas is evolved.
CaCO3(s) –––> CaO(s) + CO2 (g)
If 4.74 g of calcium carbonate is heated, what volume of CO2 (g) would be
produced when collected at STP?
Atomic Structure/Periodic Trends
34. What are the five postulates of Dalton’s atomic theory?
35. Atomic number is the same as the number of ________________
36. An atom is defined as the smallest part of an element that
a. Has protons, neutrons and electrons
b. Has protons and neutrons
c. Retains the chemical identity of that element
d. Can form an ion
6
Spring Semester Final Exam Study Guide
37. The atomic number and mass of chlorine are:
a. 17, 35
b. 33, 75
c. 16, 32
d. 29, 64
38. The neutrons of an atom are found _________________________
39. List the three subatomic particles. Name their location. Identify their
charges.
40. An element loses three electrons to form and ion that has a total of 18
electrons. What is the positive charge in the nucleus? What is the element?
41. Which subatomic particle has the smallest mass?
42. An ion is formed when an atom ___________________________________
43. The number of protons always equals the number of ______________ in a
neutral atom.
44. The mass number of an element tells you the # of ______________ and
____________.
45. Who is credited with discovering…
The nucleus _______________
The electron ________________
The Planetary Model of the Atom__________________
46. Isotopes have the same number of ______________ but different numbers of
____________ and different ___________numbers.
47. Vertical columns on the periodic table are called ___________________.
48. Horizontal rows on the periodic table are called ____________________.
49.Which of the following is true about groups of elements:
a. Elements in a group have similar chemical properties
b. Elements in a group have approximately the same atomic mass
c. Elements in a group have the same number of total electrons
d. Elements in a group have the same number of valence electrons
e. Both a and d
7
Spring Semester Final Exam Study Guide
50. KNOW ALL PERIODIC TRENDS for atomic radius and ionization energy
51. As you go across a period from left to right ionization energy:
a. Increases
b. Decreases
c. Doesn’t change
WHY?
52. Define:
Atomic radius
Ionization energy
53. Why does atomic radius decrease as you go across a period?
54.Which groups of elements are the most reactive __________________?
55. Which group of elements is the lease reactive___________________?
56. Which group (family) do the following elements belong to?
Li ________
C ____________
Be _________
N ____________
V __________
O ____________
La _________
F _____________
B __________
Ne ___________
57. What ions will the following elements form?
Li
Be
Al
Ne
N
58. Classify the following as metals, semimetals, or non-metals.
As
Si
Na
B
Ne
Ar
Cl
H
8
Spring Semester Final Exam Study Guide
ELECTRONS:
59. Draw the orbital diagram for Phosphorus.
60. Write the electron configuration for Zn
61. 1s22s22p63s1 is the electron configuration of _________________.
62. What rule states that electrons enter the lowest energy orbitals until all
electrons are accounted for? __________________
63. How many orbitals are there in the:
s group
p group
d group
f group
64. How many electrons can each of the sublevels above hold?
VSPER Shapes and Polarity
65. Compare and contrast ionic and covalent bonds in terms of:
a. Shape
b. Melting and Boiling Point
c. Conductivity
66. What happens to electrons in ionic bonds?________________
67. What happens to electrons in covalent bonds? ________________
68. What type of bond do the following Lewis Dot Structures Represent?
Na  S  Na
O=C=O
9
Spring Semester Final Exam Study Guide
69. Draw Lewis Dot Structures to show what happens to electrons when the
following elements form ionic compounds (Hint: Write the formula first)
Ca + Br
Na + F
Mg + O
Ba + S
70. Draw Lewis Dot Structures to show what happens to electrons in the
following covalent bonds:
F2
N2
H2O
CO2
71. Draw, name the VSPER shapes and identify as polar or nonpolar the
following compounds:
H2O
NH3
10
Spring Semester Final Exam Study Guide
CHCl3
CO2
Equilibrium
72. Describe a system at equilibrium in terms of the rates of reaction.
73. How is Keq is determined?
74. Determine Keq of the following equation: 2H2 (g) + O2 (g)  2H2O (l)
Use the equation below to answer questions 86-88
2NBr3 (g)  N2 (g) + 3Br2 (g)
[NBr3 (g)] = 2.07 x 10-3 M
[N2 (g)] = 4.11 x 10-2 M
[Br2 (g)] = 1.06 x 10-3 M
75. Set up the equilibrium expression.
11
Spring Semester Final Exam Study Guide
76. Find the value of Keq at the conditions shown by the molarities above.
77.
What compound or element(s) does the reaction favor?
Solutions and Acids / Bases
78. In a solution the substance being dissolved is called the _______________
and the substance it is dissolved in is called the ________________.
79. To what volume should 25mL of 15M nitric acid be diluted to prepare a 3.0M
solution?
80. What is the molarity of a solution in which 10.0g of AgNO3 is dissolved in
500mL of solution?
81. What is the pH range of acids? Bases?
82. A solution with more hydroxide ions than hydrogen ions is called a
_________________.
83. Litmus paper turns what color in the presence of an acid? Base?
84. Which of the following pH’s if for the weakest acid? pH 3 , pH 1, pH 6
85. What is the [H+] of a solution with a pH of 4?
12
Spring Semester Final Exam Study Guide
86. What differentiates a weak base from a strong base? What differentiates a
weak acid from a strong acid?
87. What signals the end of most lab titrations?
88.
What volume of 0.175 M HCl is needed to exactly neutralize 25.0 mL of
0.150 M KOH solution?
a. Neutralization Reaction:
b. Solution:
13