Download H First Semester final review questions

First semester Chemistry review sheet 2014-2015:
Complete your assigned questions on a separate piece of paper.
Question 1. Chapter 6 in your textbook
1. Write formulas for the ionic compounds formed between the following ions.
a. sodium and iodine
e. barium and fluorine
b. calcium and sulfur
f. silver and oxygen
c. zinc and chloride
g. iron(II) and hydroxide
d. aluminum and sulfate
h. mercury(I) and chromate
2. Give the name of each of the following ionic compounds.
a. KCl
e. Li2O
b. CaBr2
f. MgCl2
c. Co(NO3)2
g. FePO4
d. Hg2SO4
h. (NH4)2SO3
3. What determines the order in which the elements in a compound are written?
4. Name the following binary molecular compounds.
a. CO2
d. SeF6
b. CCl4
e. As2O5
c. PCl5
5. Write formulas for each of the following molecular compounds.
a. carbon tetrabromide
c. tetraphosphorus decoxide
b. silicon dioxide
d. diarsenic trisulfide
6. Name each of the following acids.
a. HF
d. H2SO4
b. HClO
e. H3PO4
c. HNO2
7. Give the molecular formula for each of the following acids.
a. sulfurous acid
e. perchloric acid
b. chloric acid
f. carbonic acid
c. hydrochloric acid
g. acetic acid
d. nitric acid
Question 2: Chapter 5 in your book
8. Calculate the average atomic mass for an element with the following isotopes:
234X
0.0054%
235X
0.7204%
238X
99.2742%
Identify the element.
9. Calculate the percent abundance of each isotope if the average atom mass for
63Cu and 65Cu is 63.546 amu.
Question 3: Chapter 5 in your book
10. Given the isotopes 63Cu and 65Cu. Which of the following value(s) differ in
isotopes?
a. number of protons
b. number of electrons
c. number of neutrons
d. mass number
e. atomic number
f. atomic mass
Question 4:
Do #1
Question 5: Chapter 5 in your textbook
11. Complete the following table.
number of
protons
number of
neutrons
number of
electrons
17
18
18
atomic
number
mass
number
29
65
28Si
15O-2
31
Question 6: Chapter 5 in your book
12. What are the columns called?
13. What are the rows called?
14. Use the following list of elements to answer the questions.
Na
Cr
O
Kr
Al
Te
Mg
Br
U
Ca
a. Name the alkali metal(s) listed above.
b. Name the alkaline earth metal(s) listed above.
c. Name the halogen(s) listed above.
d. Name the noble gas(es) listed above.
e. Name the main group element(s) listed above.
f. Name the transition metal(s) listed above.
g. Name the inner transition metal(s) listed above.
h. Name the nonmetal(s) listed above.
i. Name the metal(s) listed above.
j. Name the semimetal(s) or metalloid(s) listed above.
15. What two classes of elements combine to form ionic compounds?
16. What two classes of elements combine to form molecular compounds?
17. Give the symbol for the following elements.
a. noble gas in period 4
b. group 3A and period 5
c. period 6 and group 12
d. period 2 halogen
Zn
Question 7: Chapter 2 in your book
18. State the law of conservation of mass.
19. How many grams of H2SO4 will form in the following reaction if you start with
80.0 g of SO3 and 18.0 g of H2O?
SO3 + H2O  H2SO4
20. How many grams of oxygen are required to react with 32 grams of methane to
produce 88 grams of carbon dioxide and 72 grams of water.
Question #8: do #6
Question #9: do #6
Question #10: do #1
Question #11: Chapter 6 in your book
21. List the seven diatomic molecules.
22. Name a diatomic ion.
Question #12: Chapters 3 and 7 in your book
23. Determine the gram molar mass of the following.
a. methane
d. ammonium oxalate
b. ammonia
e. dinitrogen pentoxide
c. iron(III) oxide
f. sodium sulfate
Question #13: Chapter 7 in your book
24. Determine the percentage composition of each of the following compounds.
a. NaCl
b. AgNO3
c. Mg(OH)2
25. Determine the percentage by mass of water in the hydrate CuSO45H2O.
Question #14: Chapter 7 in your book
26. Determine the number of moles of compound in each of the following samples.
a. 4.50 g H2O
c. 471.6 g Ba(OH)2
b. 4.5 x 1015 molecules of F2
d. 3.45 L of N2 at STP
27. Determine the number of representative particles in the following.
a. 13.5 moles of CH4
c. 27 g of Cu
-3
b. 1.34x10 L of SO2 at STP
d. 25.27 moles of FeO
28. Determine the number of liters in the following gas samples at STP.
a. 56.7 g PCl3
c. 3.91 x 1024 molecules of CO2
b. 34.6 moles of ammonia
d. 2.62 x 102 g of CO
29. What is STP?
Question #15: Chapter 7 in your book
30. Determine the empirical formula of a compound containing 63.50% silver,
8.25% nitrogen, and 28.25% oxygen.
31. Determine the empirical formula of a compound found to contain 52.11 %
carbon, 13.14% hydrogen, and 34.75% oxygen.
32. What is the molecular formula of the molecular formula of the molecule that has
an empirical formula of CH2O and a molar mass of 120.12 g/mol?
33. A compound with a formula mass of 42.08 g/mol is found to be 85.64% carbon
and 14.36% hydrogen by mass. Find its molecular mass.
Question 16: Chapter 13 in your book
34. Determine the frequency of light whose wavelength is 4.257 x 10-7 cm.
35. Determine the energy in joules of a photon whose frequency is 3.55 x 1017 Hz.
36. Cobalt-60 emits gamma radiation with a wavelength of 1.00x10-3 nm, calculate
the energy of a photon of this radiation.
37. Given the electron shifts n=4 n=2
n=3 n=2
n=3 n=1
a. Which shift generates the greatest energy?
b. Which shift generates the largest wavelength?
c. Which shift generates the greatest frequency?
38. For each of the following values of n, indicate the types of sublevels possible.
a. n=1
b. n=2
c. n=3
d. n=4
39. How many orbitals are possible for each sublevel?
a. s sublevel
b. p sublevel
c. d sublevel
d. f sublevel
40. How many electrons could be contained in the following main energy levels?
a. first energy level
b. second energy level
c. third energy level
d. fourth energy level
41. How does a 2s sublevel differ from a 1s sublevel?
Question #17: do #16
Question #18: do #16
Question #19: do #16.
Question #20: Chapter 13 in your book
42. Define each of the following rules used to write electron configurations.
a. Aufbau rule
c. Pauli exclusion principle
b. Hund’s rule
43. Write the complete electron configuration for
a. Ar
b. Br
c. Al
44. Write the noble gas electron configuration for
a. Zn
b. Cr
c. Ba
45. Draw the box diagram electron configuration for
a. Cu
b. N
c. Si
46. How many valence electrons in the following.
a. Br
d. Al
b. Ba
e. N
c. Si
f. Li
Question #21: Chapter 14 in your book
47. Of Cs, Hg, Au which element has the smallest atomic radius? Explain.
48. Arrange the following decreasing electronegativity: C, O, Li, Na, Rb, and F.
49. Arrange the following in decreasing first ionization energies: Li, O, C, K
50. Which element is the most electronegative amoung C, N, O, Br, and S?
51. Write the equation for the second ionization of Mg. Explain why it is a lower
value than the second ionization energy of Na.
52. Rank the following in increasing size: P-3, Cl-, Ne, Ca+2, Sr+2
Question 22: do #20
Question 23: do #21
Question 24: do #17
Question 25: do #9
Question 26: do #17
Question 27: Chapter 15 and 16 in your book
53. Use electron-dot notation to illustrate the number of valence electrons present
in one atom of each of the following atoms.
a. Li
d. C
b. Ca
e. S
c. Cl
f. Al
54. Use electron dot structures to demonstrate the formation of ionic compounds
involving the following elements:
a. Na and S
b. Ca and O
c. Al and S
55. Complete the table:
formula
Lewis dot
N2
CO3-2
SO2
BF3
BrO3
C2H2
CO2
hybridization
bond angle and
shape
number of
sigma and
pi bonds
pi
NA
formal
charge on
central
atom
NA
NA
Question #28: do #27
Question #29: do #27
Question #30: Chapter 16 in your book
56. Use the following bond enthapies to determine the energy in the molecules.
C—H 414 kJ/mol
C==O 730 kJ/mol
C—Cl 331 kJ/mol
a. CH3Cl
b. CO2
Question #31: do #30
Question #32: do #21
Question #33: do #27
Question #34: do #27
Question #35: Chapter 16 in your book
57.
HCl Cl2
SO2 F2
H2O
a. What intermolecular force is present in each of the above molecules?
b. Which of the above is predicted to have the highest boiling point?
c. Which of the above is predicted to have the lowest melting point?
d. Which of above is predicted to have the highest vapor pressure?
Question #36: do #27
Question #37: do #35
Question #38: do #35
Question 39: Chapter 2 in your book
58. Identify the following as a chemical change or a physical change.
a. A piece of wood is sawed in half.
b. Milk turns sour.
c. Melted butter solidifies in the refrigerator.
59. Complete the following and give an example of each.
matter
substance
????
????
????
????
heterogeneous mixture
60. Tell whether the following is a chemical property of a physical property.
a. Its mass is 125.3g.
b. It is shiny solid at room temperature.
c. It is easily etched by nitric acid.
d. It melts when heated to 679°C.
e. It burns in air.
f. It is a good heat conductor.
Question 40: Chapter 3/4 in your book.
61. What is the volume in cubic meters, of a rectangular solid that is 0.25 m long,
6.1 m wide and 4.0 m high?
62. Find the density of a material, given that a 5.03 g sample occupies 3.24 mL.
63. What is the mass of a sample of material that has a volume of 55.1cm3 and a
density of 6.72 g/cm3?
64. How many grams are in 882 mg?
65. Express the 1.00 g/mL in g/dm3.
ANSWERS
Question 1. Chapter 6 in your textbook
1.
a. NaI
e. BaF2
b. CaS
f. Ag2O
c. ZnCl2
g. Fe(OH)2
d. Al2(SO4)3
h. Hg2CrO4
2.
a. potassium chloride
e. lithium oxide
b. calcium bromide
f. magnesium chloride
c. cobalt(II) nitrate
g. iron(III) phosphate
d. mercury (I) sulfate
h. ammonium sulfite
3. metal first then nonmetal or cation then anion or least electronegative to most
electronegative
4.
a. carbon dioxide
d. selenium hexafluoride
b. carbon tetrachloride
e. diarsenic pentoxide
c. phosphorus pentachloride
5.
a. CBr4
c. P4O10
b. SiO2
d. Ar2S3
6.
a. hydrofluoric acid
d. sulfuric acid
b. hypochlorous acid
e. phosphoric acid
c. nitrous acid
7.
a. H2SO3
e. HClO4
b. HClO3
f. H2CO3
c. HCl
g. HC2H3O2 or CH3COOH
d. HNO3
Question 2: Chapter 5 in your book
8. 238.029 amu, Uranium
9. 69.15% 63Cu and 30.85% 65Cu
Question 3: Chapter 5 in your book
10. c and d
Question 5: Chapter 5 in your textbook
11. Complete the following table.
28Si
35Cl
15O-2
65Cu+2
number of
protons
14
17
8
29
number of
neutrons
14
18
7
34
number of
electrons
14
18
10
27
atomic
number
14
17
8
29
mass
number
28
35
15
65
Question 6: Chapter 5 in your book
12. groups or familes
13. periods
14a. sodium
b. magnesium and calcium
c. bromine
d. krypton
e. sodium, oxygen, krypton, aluminum, tellurium, magnesium, bromine, calcium
f. chromium and zinc
g. uranium
h. oxygen, krypton and bromine
i. sodium, chromium, aluminum, magnesium, uranium, calcium and zinc
j. tellurium
15. metals and nonmetals
16. nonmetal
17. a. Kr
b. Sb
c. Hg
d. F
Question 7: Chapter 2 in your book
18. Matter/mass is not created or destroyed.
19. 98.0 g
20. 128 g
Question 11: Chapter 6 in your book
21. H2, N2, O2, F2, Cl2, Br2, I2
22. Hg2+2, mercury (I)
Question #12: Chapter 3 and 7 in your book
23. a. 16 g/mol
d. 124 g/mol
b. 17g/mol
e. 108 g/mol
c. 158.6 g/mol
f. 142 g/mol
Question #13: Chapter 7 in your book
24. a. 39.34% Na, 60.66% Cl
b. 63.50% Ag, 8.25% N, 28.26% O
c. 41.68% Mg, 54.86% O, 3.46% H
25. 36.07%
Question #14: Chapter 7 in your book
26. a. 0.250 mol
c. 2.752 mol
b. 7.5x10-9 mol
d. 0.154 L
24
27. a. 8.13x10 molecules
c. 2.6x1023 atoms
b. 360x1019 molecules
d. 1.52x1025 formula units
28. a. 9.24 L
c. 145 L
b. 775 L
d. 2.10x102 L
29. Standard temperature (0°C or 273 K) and pressure (1 atm or 101.3 kPa)
Question #15: Chapter 7 in your book
30. AgNO3
31. C2H6O
32. C4H8O4
33. C3H6
Question 16: Chapter 13 in your book
34. 7.05x1016 Hz
35. 2.35x10-16 J
36. 1.99x10-13 J
37.
a. n=3 n=1
b. n=3 n=2
c. n=3 n=1
Question 17: Chapter 13 in your book
38. a. s sublevel
b. s and p sublevel
c. s, p and d sublevel
d. s, p, d and f sublevel
39. a. 1
b. 3
c. 5
d. 7
40. a. 2
b. 8
c. 18
d. 32
41. A 2s sublevel has a greater diameter than a 1s sublevel.
Question 20: Chapter 13 in your book
42. see book
43. a. 1s22s22p63s23p6
b. 1s22s22p63s23p64s23d104p5
44. a. [Ar]3s23p64s23d10
b. [Ar]3s23p64s13d5
45.
c. 1s22s22p63s23p1
c. [Xe]6s2
46. a. 7
b. 2
c. 4
d. 3
e. 5
f. 1
Question 21: Chapter 14 in your book
47. Ag
48. F>O>C>Li>Na>Rb
49. O>C>Li>K
50. O
51. Mg+  Mg+2 + e- The second ionization energy of Mg is removing a valence
electron while the second ionization of Na is removing a core (nonvalence) electron
and thus requires more energy.
52. Ne< Ca+2< Cl- < P-3< Sr+2
Question 27: Chapter 15 an 16 in your book
53.
54.
55.
formula
Lewis dot
hybridization
bond angle and
shape
linear
180
number of
sigma and
pi bonds
pi
1 sigma
2 pi
formal
charge on
central
atom
NA
N2
NA
CO3-2
sp2
trigonal planar
120
3 sigma
1 pi
0
SO2
sp2
bent
<120
2 sigma
1 pi
1
BF3
sp2
trigonal planar
120
3 sigma
0 pi
0
BrO3-1
sp3
pyramidal
< 109.5
3 sigma
0 pi
2
C2H2
sp
linear
180
3 sigma
2 pi
NA
CO2
sp
linear
180
2 sigma
2 pi
0
Question 30: Chapter 16 in your book
56. a. 1573 kJ
b. 1460 kJ
Question 35: Chapter 16 in your book
57. HCl is dipole, Cl2 is dispersion, SO2 is dipole, F2 is dispersion,
H2O is hydrogen bonding
Question 39: Chapter 2 in your book
58.
a. physical change
b. chemical change
c. physical change
59. Complete the following and give an example of each.
matter
substance
element
60.
compound
mixture
homogeneous mixture
heterogeneous mixture
Elements are from the periodic table of elements.
Compounds are CO2, HCl, NaHCO3, something with a formula.
Homogeneous mixtures are salt water or brass.
Heterogeneous mixtures are sand or alphabet soup.
a. physical property
b. physical property
c. chemical property
d. physical property
e. chemical property
f. physical property
Question 40: Chapter 3/4 in your book.
61. 75mL
62. 1.55 g/mL
63. 3.70x102 g
64. 8.82x10-1 g
65. 1x103 g/dm3