Download 1 - Academics

REVIEW PROBLEMS FOR FINAL: PAGE 1
1. Manganese has the oxidation number of +5 in
(A)
[MnF6]3–
(C)
[MnO4]2–
(B)
Mn2O7
(D)
[Mn(CN)6]–
Fe(s) + Cu2+(aq) Cu(s) + Fe2+(aq)
2.
Which statement is true for the reaction?
(A)
Cu2+ is oxidized.
(B)
Cu2+ gains in oxidation state.
(C)
Cu2+ is reduced.
(D)
Fe(s) is reduced.
3. In the chemical reaction,
Zn(s) + CuSO4(aq)  ZnSO4(aq) + Cu(s),
(A)
metallic zinc is the reducing agent.
(B)
metallic zinc in reduced.
(C)
copper ion is oxidized.
(D)
sulfate ion is the oxidizing agent.
4. Which is the strongest oxidizing agent?
Standard Reduction Potentials E0
Na+ + e– 
-2.71 V
 Na
Cd2+ + 2e– 
-0.40 V
 Cd
2H+ + 2e– 
0.00 V
 H2
Ag+ + e– 
+0.80 V
 Ag
(A)
Na+
(B)
H2
(C)
Cd0
(D)
Ag+
REVIEW PROBLEMS FOR FINAL: PAGE 2
5. In this reaction
3Mg + 2HNO3(dilute) + 6H+  3Mg2+ + 2NO + 4H2O
the magnesium acts as a reducing agent. How many electrons does each
magnesium atom lose?
(A)
1
(E)
6
(B)
2
(C)
3
(D)
4
6. Balance the equation for this reaction carried out in a basic solution:
H2O + CrO42– + HSnO2–  HSnO3– + CrO2– + OH–
The coefficient of HSnO2– will be
(A)
l
(B)
2
(C)
3
(D)
5
7. With which combination will there be no appreciable reaction?
Standard Reduction Potentials E0
2+
–
Zn 
0.761 V
 Zn + 2e
2+
–
Fe 
0.441 V
 Fe + 2e
2+ + 2e–
Ni 
0.250 V
 Ni
2+
–
Pb 
0.126 V
 Pb + 2e
+4
–
Sn2+ 
–0.14 V
 Sn + 2e
2+
–
Cu 
–0.344 V
 Cu + 2e
–
–
2I 
–0.535 V
 I2 + 2e
+
–
Ag 
–0.799 V
 Ag + e
2+
–
Hg22+ 
–0.910 V
 2Hg + 2e
–
+
–
NO + 2H2O 
 NO3 + 4H +3e –0.96 V
–
–
2Cl 
–1.3583 V
 Cl2 + 2e
(A)
zinc + cupric sulfate solution
(B)
copper + nickel sulfate solution
(C)
stannous chloride + mercuric chloride solutions
(D)
lead + silver nitrate solution
(E)
iron + iodine
REVIEW PROBLEMS FOR FINAL: PAGE 3
INORGANIC NOMENCLATURE:
1. Name, by IUPAC rules, the following compounds:
a. PF5 __Phosphorus__pentafluoride_______________________________
b. CaS
_Calcium sulfide________________
c. (NH4)2S
__Ammonium sulfide____________
d.
FeCl2 _____Iron (II) chloride___or ferrous chloride
e.
NO2
__Nitrogen dioxide_______________
5 pts: ____
2. Give formulae for the following compounds:
a. Water: ____H2O_____________________________
b. Sulfur trioxide: ____SO3____________________
c. Iron (III) sulfide: ____Fe2S3___________________
d. Cobalt (II) fluoride: ___CoF2__________________
e. Disilicon hexanitride: ____Si2N6________________
5 pts: ____
REVIEW PROBLEMS FOR FINAL: PAGE 4
MULTIPLE CHOICE PORTION (Each question is weighted at 5 points):
3. A carbon dioxide molecule is ambling along at the (non-relativistic) velocity
of 0.05000 times the speed of light. The kinetic energy of the carbon
dioxide molecule is:
WATCH THE UNITS!
Mass of 1 Carbon atom: 2.66 x 10-23 g
Mass of 1 Oxygen atom: 1.995 x 10-23 g
a. 5.225 x 10-9
b.
g m /sec
8.209 x 10-12 kg m2 /sec2
c. 5.225 x 10-12 kg m2 / sec2
d. 8.209 x 10-12 g m2 / sec2
Carbon dioxide = CO2; Mass = 2.66 x 10-23 g + 2(1.995 x 10-23 g) = 6.65 x 10-23 g
KE = ½ mv2 = ½[(6.65x10-23g)[.05 x 2.99 x 108m/sec]2 = 8.209 x 10-9g m2/sec2
units don’t match responses:
8.209 x 10-9g m2/sec2( 1kg/1000g)  kgm2/sec2
4. An -particle is a helium nucleus, 4He2. The charge on an -particle is:
a. -6
b. -4
c. -2
d. 0
e. +2 f. + 4
g. +6
REVIEW PROBLEMS FOR FINAL: PAGE 5
5. The force of electrostatic attraction between a single sodium ion and a
single chloride ion, separated by a distance of 0.60 nm, is:
WATCH THE UNITS!
-19
A chloride ion has a charge of - 1.602 x 10 coulombs.
A sodium ion has a charge of + 1.602 x 10-19 coulombs.
a. 6.4 x 10-28 N
b. 2.5 x 10+10 N
c. 6.4 x 10-10 N
d.
2.4 x 10-9 N
e.
About enough force to push Dr O’s pickup to Nebraska Notch.
F = (1/4πεo)(q1 q2)/r2
= (1/4 x 3.141 x 8.85 x 10-12 C2/N m2)[( 1.602 x 10-19 coulombs)( 1.602 x 10-19
coulombs)]
[0.6 nM(1 M/10-9 M)]2 Gotta convert nM to M to get the units right.
6. Which is true about the following three isotopes:
3216
, 3416, and
3516
a. They are all the element sulfur;
b. Because they are isotopes, they are all radioactive;
c. They are the elements Germanium (Ge) , Selenium (Se) and Krypton (Kr),
respectively.
d. They all contain 16 protons;
e. They all contain 16 neutrons;
f. a and d are correct;
7. Which pair has the same total number of electrons:
a. O2- and F- ;
b. Ba2+ and Rn;
c. Fe2+ and Fe3+
REVIEW PROBLEMS FOR FINAL: PAGE 6
d. I- and Cl-
REVIEW PROBLEMS FOR FINAL: PAGE 7
BONUS:
Consider these three isotopes of bromine:
unstable, that is, radioactive, because:
79Br35
, 81Br35 ,
82Br35.
82Br35
is
a) Its n/p ratio is too high;
b) Its p/n ratio is too high;
c) Its e-/p ratio is too low.
d) It has a lousy price/earnings ratio.
8. The correct Lewis structure for the fluoride ion is:
a)
b)
c)
d)
e)
I can’t draw this in Word. However, look for the F with 4 pairs of dots and a –
charge.
9. The mass in grams of one atom of gold is 3.27 x 10-22 g The volume of one
gold atom is 1.69 x 10-23 cm3. What is the density of one gold atom?
a) 5.91 x 10+22 cm3
b) 0.0518 cm3 g-1
c) 19.3 g cm-3
d) 5.53 x 10-45 g cm3
e) Incalculably small
d = mass/volume = 3.27 x 10-22 g / 1.69 x 10-23 cm3
REVIEW PROBLEMS FOR FINAL: PAGE 8
10. The size of an atom is mostly determined by:
a) the volume of space occupied by e- ;
b) the volume of space occupied by protons ;
c) the volume of space occupied by neutrons ;
d) the volume of space occupied by protons & neutrons.
11. A covalent bond is best described as:
a) The complete transfer of a pair of e- between two atoms;
b) The complete transfer of a single e- between two atoms;
c) The sharing of a single e- between two atoms;
d) When an electron falls into the nucleus of another atom.
e) The sharing of a pair of e- between two atoms;
12. An ionic bond is best described as:
a) The complete transfer of a pair of e- between two atoms;
b) The complete transfer of one or more e- between two atoms;
c) The sharing of a single e- between two atoms;
d) When an electron falls into the nucleus of another atom.
e) The sharing of a pair of e- between two atoms;
13. The correct Lewis structure for nitogen gas is:
a)
b)
c)
d)
e)
Once again, I can’t do this in Word, but look for a triple bond, and a lone pair
of e- on each N.
REVIEW PROBLEMS FOR FINAL: PAGE 9
14. Which of the following is a BrØnsted acid:
a) NaOH
b) :NH3
c) HCl
d) :S:2-
e) C2H3O2-
BONUS:
In the reaction H2O + H2O  H3O+ + :OH1
2
1a
2a
Which water molecule is acting as a BrØnsted Base?
1
15. Which of the following is a Lewis acid but not a BrØnsted acid?
a)
b)
c)
d)
16. Identify the Lewis base:
a)
b)
c)
d)
17. Consider:
HCl + NaOH 
The products of this reaction will be:
a) HNa and ClOH
reaction
b) H2O and NaCl
c) H2Cl and NaO d) no
REVIEW PROBLEMS FOR FINAL: PAGE 10
18. The best definition for and explanation of electronegativity is:
a) Electronegativity is the measure of the tendency of a combined atom to
attract a shared pair of electrons to itself; elements in the upper right hand
side of the periodic table tend to be more electronegative because they have
fewer inner core electrons shielding shared valence electrons from the nucleus.
b) Electronegativity is the measure of the tendency of a combined atom to attract
a shared pair of electrons to itself; elements in the lower left hand side of the
periodic table tend to be more electronegative because they have many electrons
attracting shared electrons.
c) Electronegativity is the measure of the tendency of a combined atom to repel a
shared pair of electrons; elements in the lower left hand side of the periodic
table tend to be more electronegative because they have many electrons repeling
shared electrons.
d) Electronegativity is the measure of the tendency of a combined atom to repel a
shared pair of electrons; elements in the upper right hand side of the periodic
table tend to be more electronegative because they have many inner core
electrons shielding shared valence electrons from the nucleus.
19. Atoms in Group VIII of the periodic table:
a) Tend to be highly reactive;
b) Are all Lewis acids;
c) Are all BrØnsted bases;
d) Have filled valence shells;
e) Are called Noble gases because they are all purple coloured.
REVIEW PROBLEMS FOR FINAL: PAGE 11
INORGANIC NOMENCLATURE:
1. Name, by IUPAC rules, the following compounds:
f. NH4F __Ammonium fluoride_________________________________
g. Ba3(PO4)2
h.
H2SO4
_____Barium phosphate___________________________
_____Sulfuric acid_________________________
i. CrCO3 _____Chromium (II) carbonate____________________________
j.
S2O5 ______disulfur pentoxide___________________________
pts: ____
5
6. Give formulae for the following compounds:
f. Hydronium ion: _______H3O+__________________________
g. Manganese(IV)oxide: ____MnO2____________________
h.
Cobalt (III) sulfite: __Co2(SO3)3 _____________________
i. Lithium sulfide: ____Li2S_________________
j. Magnesium chlorate: ___Mg(ClO3)2_________________
5 pts: ____
REVIEW PROBLEMS FOR FINAL: PAGE 12
SHORT ANSWER PORTION:
7. a. Write the balanced NET IONIC equation for the reaction between
hydrochloric acid and sodium hydroxide (All reactants are soluble. All sodium
salts are soluble):
HCl + NaOH  NaCl + H2O
H+ + Cl- + Na+ + OH-  H2O + Na+ + ClH+ + OH-  H2O
b. Write the balanced NET IONIC equation for the reaction between
potassium bromide and silver nitrate. (All reactants are soluble. All potassium
salts are soluble. All silver salts except silver nitrate are insoluble).
KBr + AgNO3  ANO3 + AgBr
K+ + Br- + Ag+ + NO3-  K+ + NO3- + AgBr
Br- + Ag+  AgBr
c. Write the balanced NET IONIC equation for the reaction between
Sodium phosphate and barium chloride. (All reactants are soluble. All
sodium salts are soluble. All phosphate salts except sodium phosphate are
insoluble).
2Na3PO4 + 3BaCl2  Ba3(PO4)2 + 6NaCl
6Na+ + 2PO43- + 3Ba2+ + 6Cl-  Ba3(PO4)2 + 6Na+ + 6Cl2PO43- + 3Ba2+  Ba3(PO4)2
d. Write the balanced equation for the reaction between magnesium metal and
copper (II) ion, producing magnesium ion and copper metal.
Mg + Cu2+  Mg2+ + Cu
REVIEW PROBLEMS FOR FINAL: PAGE 13
e. Complete the reaction:
Uv light
Br2
2Br
Uv light
2Br ·
Br2
MULTIPLE CHOICE PORTION (Each question is weighted at 5 points):
4. In the ion H2P2O72–, the oxidation number for P is
(A) 2
(B) 4
(C) 5
(D) 6
(E) -2
5. In the chemical reaction,
Zn(s) + CuSO4(aq)  ZnSO4(aq) + Cu(s),
(A)
metallic zinc is the reducing agent.
(B)
metallic zinc is reduced.
(C)
copper ion is oxidized.
(D) sulfate ion is the oxidizing agent.
6. In this reaction
3Mg + 2HNO3(dilute) + 6H+  3Mg2+ + 2NO + 4H2O
the magnesium acts as a reducing agent. How many electrons does each
magnesium atom lose?
(A)
1
(B)
2
(C)
3
(D)
4
(E)6
BONUS: What happens when you throw sodium metal into water?
2Na + 2H2O  2NaOH + H2 + heat!
REVIEW PROBLEMS FOR FINAL: PAGE 14
7. What statement best characterises a free radical (in chemistry)?
a. Free radicals are inert compounds, with a full octet of paired electrons;
b. Free radicals are highly reactive compounds, with a full octet of paired
electrons;
c. Free radicals are inert compounds, with at least one unpaired valence
electron;
d. Free radicals are highly reactive compounds, with at least one unpaired
valence electron;
e. Emma Goldman was a free radical.
8. You have a 100 kg bar of pure gold. How many gold atoms in the bar?
(A) 3 x 1023
(B) 3 x 1026
(C) 19696700 (D) 1 x 1031
(E) one or two
9. What is the empirical formula for the substance with this analysis:
Na
B
O
Elemental Analysis
54.0%
8.50%
37.5%
Atomic Molar Masses
B
Na
O
10.8 g·mol–1
23.0 g·mol–1
16.0 g·mol–1
(A)
Na3BO3
(C)
Na2B2O3
(B)
Na4BO4
(D)
NaB2O2
WATCH UNITS!
REVIEW PROBLEMS FOR FINAL: PAGE 15
10. How many moles of Fe are needed to produce
10.0 mol of H2?
4H2O(g) + 3Fe(s)  Fe3O4(s) + 4H2(g)
(A)
7.50 mol
(C)
15.0 mol
(B)
13.3 mol
(D)
30.0 mol
11. Suppose you set fire to some benzene (C6H6):
2 C6H6(l) + 15O2(g)  12CO2(g) + 6H2O(l)
If you burn 10.0 grams of benzene in 10.0 grams of oxygen, which is the limiting
reagent?
MW benzene = 78 g/mol
MW O2
= 32 g/mol
MW CO2
= 44 g/mol
MW H2O
= 18 g/mol
(A) Benzene
Water
(B) Oxygen
(C) Carbon dioxide
(D)
BONUS: There are 250 x 106 folk living in the United States. How many moles
is this?
4.15 x 10-16 moles
REVIEW PROBLEMS FOR FINAL: PAGE 16
12. What mass of iron(III) sulfide is produced from the reaction of 11.6 g of
iron(III) nitrate with excess sodium sulfide?
2Fe(NO3)3(aq) + 3Na2S(aq)  Fe2S3(s) + 6NaNO3(aq)
Molar Masses
208 g·mol–1
Fe(NO3)3 242 g·mol–1
Fe2S3
(A)
4.99 g (B)
6.75 g (C)
9.97 g (D)
11.6 g
13. You react 0.2042 g of KHP with exactly 22.22 mL of NaOH:
KHP + NaOH  KP- + H2O + Na+
MW KHP = 204.2 g/mol
MW NaOH = 40 g/mol
MW KP- = 203.2 g/mol
MW H2O = 18 g/mol
MW Na+ = 23 g/mol
How many moles of KHP reacted?
(A) 1.000
(B) 0.2042
(C) 0.1000
(D) 41.70
(E) 0.001000
REVIEW PROBLEMS FOR FINAL: PAGE 17
14. In problem 13, you reacted 0.2042 g of KHP with exactly 22.22 mL of NaOH:
KHP + NaOH  KP- + H2O + Na+
MW KHP = 204.2 g/mol
MW NaOH = 40 g/mol
MW KP- = 203.2 g/mol
MW H2O = 18 g/mol
MW Na+ = 23 g/mol
The molar concentration of NaOH is:
(A) 0.04500 M (B) 0.5555 M
(C) 0.00004500 M
(D) 0.009200 M
15. This is a graph of what happens to the volume of a gas sample under
varying conditions of temperature:
What is the volume of gas when the temperature is –400 oC?
(A) -400 oC
(B) -10 L
(C) very close to 0 L; in fact, temperatures below –273.15 oC have no physical
meaning.
(D) cannot be determined…the graph doesn’t go that far.
16. A correct statement of Boyle’s Law (which describes the pressure-volume
behaviour of gases) is:
REVIEW PROBLEMS FOR FINAL: PAGE 18
(A) P = kV
(B) 1/P = k/V
(C) P = 1/T
(D) PV = 1/T
(E) P = k/V
REVIEW PROBLEMS FOR FINAL: PAGE 19
17. Your lungs contain approximately 3.00 L of air at 37oC and 1.000 atm
pressure.
If, God forbid, you should go down on the Titanic, holding your breath, what is
the volume of air in your lungs at 200 atm pressure and –5oC?
(A) 13 mL
(B) 3.00 L
(C) 694 L
(D) -2 mL
18. In a sample of a nearly ideal gas, this graph could represent a plot of
(A)
V vs. T at a given constant P.
(B)
P vs. T at a given constant V.
(C)
P vs. V at a given constant T.
(D)
PV vs. P at a given constant T.
REVIEW PROBLEMS FOR FINAL: PAGE 20
19. If 1 L of a gas at 30 °C and 0.9474 atm pressure has a mass of
2.00 g, the mass of a mole of the gas is
(A)
22.4 g.
(B)
44.8 g.
(C)
somewhere between 22.4 and 44.8 g.
(D) 53.6 g.
BONUS: What is the number of molecules in 1.00 mL of an ideal gas at STP?
(A)
2.69  1022
(C)
2.69  1019
(B)
6.02  1020
(D)
22.4  1019
20. What is the volume of 2.00 mol of helium gas at 27 °C and 3.00 atm?
(A)
6.1 x 10–2 L
(B)
1.48 L
(C)
16.4 L
(D) 44.8 L
REVIEW PROBLEMS FOR FINAL: PAGE 21
INORGANIC NOMENCLATURE:
1. Name, by IUPAC rules, the following compounds:
k.
HNO3 __Nitric acid________________________
l. H2SO4
m.
NH4F
n. CaCO3
o.
___Sulfuric acid__________________
___Ammonium fluoride_________
_____Calcium carbonate__________
Fe3(PO4)2
__Iron (II) phosphate_________
5 pts: ____
8. Give formulae for the following compounds:
k.
Carbon dioxide: _CO2___________________________
l. Sodium hypochlorite: ___NaOCl___________
m.
Hydrochloric acid: ___HCl_______________
n. Sodium hydroxide: __NaOH_______________
o.
Manganese (II) oxide: ___MnO__________
5 pts: ____
REVIEW PROBLEMS FOR FINAL: PAGE 22
SHORT ANSWER PORTION:
9. a. Write the balanced NET IONIC equation for the reaction between
calcium carbonate and hydrochloric acid (Calcium carbonate is not soluble.
All chloride salts are soluble.):
CaCO3 + 2HCl - CaCl2 + H2CO3  H2O + CO2
CaCO3 + 2H+ + 2Cl- - Ca2+ + 2Cl- + H2O + CO2
CaCO3 + 2H+ - Ca2+ + H2O + CO2
f. Write the balanced NET IONIC equation for the reaction between magnesium
sulfate
and silver nitrate. (All reactants are soluble. All nitrates are soluble. All silver
salts except silver nitrate are insoluble).
MgSO4 + 2AgNO3  Mg(NO3)2 + Ag2SO4
Mg2+ + SO42- + 2 Ag+ + 2NO3-  Mg2+ + 2NO3- + Ag2SO4
SO42- + 2 Ag+  Ag2SO4
g. Write the balanced NET IONIC equation for the reaction between
barium hydroxide and nitric acid. (All reactants are soluble. All nitrate salts
are soluble).
Ba(OH)2 + 2HNO3  2H2O + Ba(NO3)2
Ba2+ + 2OH- + 2H+ + 2NO3-  2H2O + Ba2+ + 2NO3OH- + H+  H2O
h. Write the the balanced equation for the reaction between Aluminum metal
and hydrochloric acid, producing aluminum chloride and hydrogen gas:
2Al + 6HCl  2AlCl3 + 3H2
i. Complete the reaction:
Br  + H
______HBr_____________
REVIEW PROBLEMS FOR FINAL: PAGE 23
MULTIPLE CHOICE PORTION (Each question is weighted at 5 points):
10. Elecromagnetic radiation recently detected in outer space emitted from a
supernova had a frequency of 8.99 x 1020 Hertz. Its corresponding
wavelength is:
a) 1.11 x 10-21 sec
b) 3.34 x 10-13 m
c) 2.997 x 1012 sec/m
d) 2.697 x 1029 m sec
Bonus: This radiation is (circle one): gamma rays; x-rays, green light, radio
waves.
11. The energy of 1.000 Einstein of light of wavelength 455 nm is:
[1 Einstein = 6.023 x 1023 photons]
a) 2.62 x 105 joules
b) 4.35 x 10-19 joules
c) 3.02 x 10-31 joules
d) 455 joules
7. At what velocity would an electron have to travel to “go like a blue streak”,
that is, have a wavelength of 450 nm?
a) 1.616 x 103 m/sec
b) 1.616 x 10-6 m/sec
c) 6.19 x 10-4 m/sec
d) 3 x 1010 m/sec
REVIEW PROBLEMS FOR FINAL: PAGE 24
8. The Heisenberg Uncertainty Principle states that:
mvx  h/4
In essence, what this means is:
a) No particle can travel faster than Planck’s Constant;
b) The velocity and the position of an electron can be measured to greater than
h/4 significant figures;
c) Electrons exhibit wave-particle duality but nothing else does;
d) The momentum and the position of a particle cannot be simultaneously
measured to unlimited accuracy.
9. An argon atom is isoelectronic with (has the same number of electrons as):
(A)
Cl
(B)
Ca
(C)
Ti4+ (D)
N3–
10. An atom has a valence shell electron configuration of ns1. To which group of
elements in the periodic table does it belong?
(A)
transition metals
(C)
alkaline earth metals (group II)
(B)
the Lanthanides
(D)
alkali metals (Group I)
REVIEW PROBLEMS FOR FINAL: PAGE 25
11. The ground state electron distribution for the Sn2+ ion is
(A)
[Kr]4d105s15p1.
(B)
[Kr]4d105s25p4
(C) [Kr]4d105s25p2.
(D)
[Kr]4d105p2.
12. Which of the following is a d orbital?
The double dumbell one and the dumbell-donut one
13. The number of unpaired electrons in the ground state of Tc0 is
(A)
one
(B)
three (C)
five
(D)
seven
14. The ground–state electronic configuration of the manganese (Mn) atom is
(A)
1s22s22p63s23p64s2 4d5
(B)
1s22s22p63s23p63d7
(C)
1s22s22p63s23p64s24p5
REVIEW PROBLEMS FOR FINAL: PAGE 26
(D)1s22s22p63s23p63d54s2
BONUS: Write the electronic configuration of silver.
[Kr]5s1 4d10
15. The maximum number of electrons that can occupy an orbital labeled dxy is
(A)
l
(B)
2
(C)
3
(D)
4
16. Cadmium normally forms the ion Cd2+, whereas silver gives the Ag+ ion.
What is an explanation of these facts?
(A)
Silver has two 5s electrons, one of which is more difficult to remove
than the other.
(B)
The 4d subshell in silver is completed to give a more stable
structure, leaving only one electron in the 5s subshell.
(C)
Cadmium loses two 4d electrons to form the Cd2+ ion.
(D)
None of these is correct.
(E) All of these are correct.
Ag0 is [Kr]5s1 4d10  Ag+ [Kr]5s0 4d10
Cd0 is [Kr]5s2 4d10  Cd2+ [Kr]5s0 4d10
17. The energy of the hydrogen atom in the ground state
(n = l) is 21.79  10–19 J. A particle strikes a hydrogen atom and excites the
electron to its 5th energy level (n = 5) corresponding to an energy of 0.87  10–19
J. If the electron returns to the ground state in one step, what is the energy of the
photon emitted?
(A)
4.18  10–19 J
(C)
20.92  10–19 J
REVIEW PROBLEMS FOR FINAL: PAGE 27
5.48  10–19 J
(B)
18. F is
a
than Li because
a
22.66  10–19 J
b
&
b
(A)
larger
nuclear charge
(B)
(D)
c:
c
p electrons are lousy at shielding
smaller
p electrons are lousy at shielding.
nuclear charge
F has greater effective
F has greater effective
(C)
smaller
nuclear charge
p electrons are good at shielding.
Li has greater effective
(D)
larger
nuclear charge
There are more
Li has greater effective
p electrons
19. Rank the following in order of electron affinity:
Zn
O,
Mo
(A) Mo > Zn> O
(B)
Mo > O > Zn
(C)
O > Zn > Mo
(D) Zn > O > Mo
(E)
Zn > Mo > O
REVIEW PROBLEMS FOR FINAL: PAGE 28
20: Electronegativity is:
(A) The measure of the tendency of an isolated gaseous atom to attract electrons
to itself.
(B) The measure of the tendency of an isolated gaseous atom to repel electrons.
(C) The measure of the tendency of a combined atom to repel a shared pair of
electrons.
(D) The measure of the tendency of a combined atom to attract a shared pair of
electrons to itself.
21. Which of the following represents electron affinity?
(A) X + energy  X+ + e(B) X + e- 
X- + energy
(C) X + e- + energy  X+
(D) energy + e-  X
22. On the periodic table, indicate wih an arrow the trend in ionization energy:
REVIEW PROBLEMS FOR FINAL: PAGE 29
23. If an electron has quantum numbers n = 3, l = 2, which of the following is
true?
(A) the electron is located at a fixed location in space, 3 units away from the
nucleus.
(B) the electron is most likely to be found in a double-dumbbell shaped
region of space centered about the nucleus, but not always.
(C)
the electron is most likely to be found in a spherical region of space
centered about the nucleus, but not always.
(D) the electron is most likely to be found in a single-dumb-bell region of space
centered about the nucleus, but not always.
BONUS: Which is farther away from the nucleus, a 4s electron or a 2p electron?
4s
REVIEW PROBLEMS FOR FINAL: PAGE 30
INORGANIC NOMENCLATURE:
1. Name, by IUPAC rules, the following compounds:
p.
Ca(ClO4)2 _________Calcium perchlorate_______
q. NaBrO3
r. Fe(IO2)2
s. CuOCl
t.
HIO4
___Sodium bromate_______________
_____Iron (II) iodite_(ferrous iodite)
_______Copper(I) hypochlorite (cuprous hypochlorite)
_________Periodic acid___________
10 pts: ____
12. Give formulae for the following compounds:
p.
Lithium fluoride ___________LiF___________________
q. Sodium sulfide ________Na2S____________
r. Hydrochloric acid: _______HCl_____________
s. Sulfurous acid: ______H2SO3__________
t. Manganese (IV) sulfite_______Mn(SO3)2___
10 pts: ____
REVIEW PROBLEMS FOR FINAL: PAGE 31
SHORT ANSWER PORTION:
13. a. Write the balanced NET IONIC equation for the reaction between
calcium carbonate and hydrochloric acid (Calcium carbonate is not soluble.
All chloride salts are soluble.):
CaCO3 + 2HCl  CaCl2 + H2CO3  H2O + CO2
CaCO3 + 2H+ + 2 Cl-  Ca2+ + 2 Cl- + H2O + CO2
CaCO3 + 2H+  Ca2+ + H2O + CO2
j. Write the balanced NET IONIC equation for the reaction between nitric acid
and silver carbonate. (Silver carbonate is not soluble. All nitrates are soluble.
All silver salts except silver nitrate are insoluble).
Ag2CO3 + 2HNO3  2 AgNO3 + H2CO3  H2O + CO2
Ag2CO3 + 2H+ + 2 NO3-  2Ag+ + 2 NO3- + H2O + CO2
Ag2CO3 + 2H+ +  2Ag+ + H2O + CO2
k. Write the balanced NET IONIC equation for the reaction between
Ammonium phosphate and barium hydroxide. (All reactants are soluble. All
metal phosphate salts are insoluble.).
2(NH4)3PO4 + 3Ba(OH)2  6 NH3 + 6H2O + Ba3(PO4)2
6NH4+ + 2PO43- + 3Ba2+ + 6OH-  6 NH3 + 6H2O + Ba3(PO4)2
l. Draw the correct Lewis structure(s) for H2O
See p R 7.9
e. Draw the correct Lewis structure for CO3=
Can’t do it on Word
20 pts: ______
REVIEW PROBLEMS FOR FINAL: PAGE 32
14. Consider the following graph:
See graph on p 220 in text. The correct selection is the distance at which the
graph dips to its lowest point (c in text)
At what distance will you expect to have a stable H2 molecule?
(A) Distance (a)
(B) Distance (b)
(C) Distance (c)
(D) Distance (d)
(E) Distance (e)
15. Molecular orbitals may be considered
(A) to arise from the mind of Erwin Schrodinger.
(B) to be a linear combination of atomic orbitals.
(C) to be identical to atomic orbitals.
(D) to result from the overlap of two or more protons.
(E) to be areas of space about the nuclei of atoms where valence electrons are
least likely to be found.
REVIEW PROBLEMS FOR FINAL: PAGE 33
16. According to molecular orbital theory, diatomic helium (He2)
(A) Has a  bond and a  bond.
(B) Is sp3 hybridized.
(C) Has a pair of electrons in a 1s bonding orbital, and a pair of electrons in
a 1s* anti bonding orbital.
(D) Is paramagnetic.
(E) Cannot form a stable bond.
(F) Both A and D are correct.
(G) Both C and E are correct.
17. According to molecular orbital theory, diatomic oxygen (O2)
(A) Is a free radical.
(B)
Is paramagnetic
(C)
Has a bond order of 2.
(D) has a a  bond.
(E) All of the above are correct.
(F)
All of the above are incorrect.
REVIEW PROBLEMS FOR FINAL: PAGE 34
BONUS: The best Lewis dot structure for the cyanide ion (CN-) is:
(A)
C
N
(B)
C
N
(C) C
N
(D) C
N
Can’t do this in Word.
18. According to VSEPR Theory, the molecule KrF4 (Cetral atom underlined) is:
(A) sp hybridized, with 180 bond angles
(B) sp2 hybridized, with 120 bond angles
(C) sp3 hybridized, with 109 bond angles
(D) sp3d hybridized, with 90 & 120 bond angles
(E) sp3d2 hybridized, with 90 bond angles
BONUS: NAME KrF4
Krypton tetrafluoride
19. The shape of a water molecule, according to VSEPR theory, is:
(A)
linear.
(C) bent at 90
(B) determined by lone pairs of electrons on O (D) bent at 120


REVIEW PROBLEMS FOR FINAL: PAGE 35
20. Consider the molecule nitrogen (N2):
N2 has
a  bonds
lone pair(s) of e.
 bonds, and each N is
b
(A)
a
1
b
2
(B)
2
1
(C)
3
(D)
1
c
hybridized with
c
sp
d
1
sp2
3
2
sp2
1
sp3
12. Which of these molecules has polar BONDS? (Select all that apply)
(i) CO
(ii)
CF4
(iii) H2O
(iv) F2 (v) CO2
(A) iv only
(B) all of them
(C) i, ii, iii, & v
(D) none of them
13. Which of these molecules is polar?
(i) CO (ii)
CF4 (iii) H2O
(iv) F2 (v) CO2
(A) iv only
(B) all of them
(C) i, ii, iii, & v
(D) none of them
(E) i & iii
d
0
2
REVIEW PROBLEMS FOR FINAL: PAGE 36
14.
A peptide (amide) bond may be represented as:
CAN’t show this in WOrd
(A) only structure I is correct.
(B) only structure 2 is correct.
(C) the molecule flips rapidly back & forth between structure I & structure II.
(D) The  electrons are being shared between the N-C-O atoms. They are
“delocalized”.
BONUS: Consider Nutrasweet®:
Can’t show this in Word
The functional groups labeled “a” and “b” in this dipeptide are:
(A) amine and carboxylic acid
(B) alcohol and aldehyde
REVIEW PROBLEMS FOR FINAL: PAGE 37
1. You take 1.00 mL of 0.200 M NaCl and dilute it to 100.0 mL. You then pipet
out 2.00 mL of the diluted NaCl, and drain it into a clean bucket. Calculate how
many grams of NaCl you have in the bucket. (MW NaCl = 58.44 g/mol)
(A) 2.3 x 10-4 g
(B) 1.7 x 10-2 g
(C) 0.23 g
(D) 58.53 g
2. Suppose you have a pair of electrons 0.10 nM apart. Calculate that distance in
meters.
(A) 1 x 10-10 M
(B) 1 x 10-9 M
(C) 1 Å
(D) 1 x 108 M
3. Suppose you have a pair of electrons 0.10 nM apart. Calculate the force of
electrostatic attraction beteen them in Newtons (1 Newton = 1 kg m/sec2)
(A) 5.53 x 10-51 N
(B) 1.11. x 10-12 N
(C) 2.31 x 10-8 N
(D) 8.99 x 1031 N
REVIEW PROBLEMS FOR FINAL: PAGE 38
27
4. The number of neutrons in the nucleus of an atom of 13Al is
(A)
(B)
(C)
(D)
(E)
9
13
14
27
40
5. When alpha particles (4He2 nuclei) were shot at a gold foil target, most of the
particles were undeflected. This indicated to Rutherford that
(A)
the gold foil was continuous matter.
(B)
the mass of the gold atoms was spread out thinly.
(C)
the atoms of gold were mostly empty space.
(D)
the alpha particles had great penetrating power.
(E)
the alpha particles had charges opposite to those on the nuclei.
6. Which of the following is TRUE?
(A)
(B)
(C)
(D)
(E)
Na+ is an isotope of Na;
All isotopes are radioactive;
Ta180 and Ta181 are isotopes;
Isotopes differ in the number of protons each has;
Two isotopes of an element have VERY different chemistry.
7. The mass of a single atom of Tantalum (Ta) is:
(A) 73 x 10-23 g;
(B) 3.0043 x 10-22 g;
(C) 180.9479 g;
(D) 3.33 x 1021 g;
(E) Impossible to calculate, due to the Heisenberg Uncertainty Principle.
REVIEW PROBLEMS FOR FINAL: PAGE 39
8. The HALOGEN elements have how many valence electrons?
(A) 1
(B) 2
(G) 7
(H) 8
(C) 3
(D) 4
(E) 5
(F) 6
BONUS: There are 72 students taking the CH 103 Hour Exam. This is how
many moles?
(A) 1.2 x 10-22 moles
(B) 1 mole
(C) 72 moles
(D) 103 moles
(E) 6.023 x 1023 moles
9. A compound with the formula CaH2 is called:
(A)
cadmium hydride.
(B) hydrogen carbide.
10. Consider vitamin B12:
g/mole.
(C)
(D) calcium hydrate.
C63H88N14O14PCo, MW = 1355.42
The % by mass Cobalt in Vitamin B12 is:
(A) 0.074 %
(B) 0.55 %
(C) 4.34 %
(D) 23.0%
calcium hydride.
REVIEW PROBLEMS FOR FINAL: PAGE 40
REVIEW PROBLEMS FOR FINAL: PAGE 41
11. Phenolphthalein, the endpoint indicator of many acid/base titrations, has
the following % composition:
C: 66.30%
H: 3.34%
Na: 12.70%
O 17.67%
The simplest formula for Phenolphthalein is:
(A) C7H3Na13O18
(B) C10H6Na1O2
(C) C20H1Na4O5
(D) C66.33H3.34Na12.7O17.76
12. Consider the reaction:
AgNO3
MW:
169.89 g/mole
+ NaI

149.92 g/mole
AgI
234.80 g/mole
+ NaNO3
85.01 g/mole
If you start with 424.73 g of silver nitrate and 374.8 g of sodium iodide, how
many grams of silver iodide will you produce?
(A) 2.5 g
(B) 93.92 g
(C) 587.0 g
(D) 799.53 g
BONUS: This is α-boswellic acid, the key ingredient
in Frankincense. What is the shape around the
carbon that the arrow is pointing to? (Hint, there are
4 things around that carbon)
Tetrahedral
REVIEW PROBLEMS FOR FINAL: PAGE 42
13. Balance the equation
?N2H4 + ?N2O4  ?N2 + ?H2O
How many moles of N2 will be produced for every one mole of N2O4 that
reacts?
2N2H4 + N2O4  3N2 + 4H2O
(A) one
(B) two
(C) three
(D) four
14. Consider the reaction (which you have considered in lab!):
3BaCl2
MW:
+
2 Na3PO4 
208.27 g/mole
163.94 g/mole
Ba3(PO4)2↓
601.2 g/mole
+
6NaCl
58.45g/mole
If you start off with 100.0 g of barium chloride & 100.0 g of sodium phosphate,
which is the LIMITING REAGENT?
(A) barium chloride
(B) sodium phosphate
(C) barium phosphate
(D) sodium chloride
15. Look back at the data in Question 14. What is the THEORETICAL YIELD of
barium phosphate?
(A) 96.22 g
(B) 100.0 g
REVIEW PROBLEMS FOR FINAL: PAGE 43
(C) 200.0g
(D)288.7 g
(E) 366.7 g
(F) 601.2 g
REVIEW PROBLEMS FOR FINAL: PAGE 44
16. Which of these is a Lewis base?
(A) HCl
(B) NH4+
(C) H3O+
(D)
H2O
17. When two water molecules react with each other, they produce:
(A) OH- & H3O+
& OH+
(B) O & H2
(C) H3O+ & H3O+
(D)
18. Which of these is a Brønsted acid?
(A) Cl-
(B) :NH3
(C) OH-
(D)
H2O
19. Which CANNOT be described as a Brønsted-Lowry acid/base reaction?
(A) HCl + NaOH  NaCl + H2O
(B) HCN + H2O  H3O+ + CN(C) BF3 + :NH3  F3B-NH3
(D) H+ + NH3  NH4+
H-
REVIEW PROBLEMS FOR FINAL: PAGE 45
20. Consider the reaction:
N2 + 3H2  2NH3
Which of the following is true?
(A)
(B)
(C)
(D)
N2 is oxidized; H2 is the oxidizing agent;
H2 is oxidized; N2 is the oxidizing agent;
The oxidation state of N in NH3 is 0.
The oxidation state of H in H2 is +1.
21. When solutions of NaBr and Cl2 are mixed, the solution turns orange due to
formation of Br2. Which statement best describes this process?
(A) Sodium ions are reducing Bromide ions to bromine molecules;
(B) Sodium ions are oxidizing Bromide ions to bromine molecules;
(C) Chlorine molecules are oxidizing Bromide ions to bromine molecules;
(D) Chloride ions are oxidizing Bromide ions to bromine molecules;
2Br- + Cl2  Br2 + 2Cl22. You have a 250 mL sealed can full of CO2 in your backpack while you do
back-country telemarking from Underhill, through the Needle’s Eye, to Trapp’s
Cabin. The temperature is a brisk –40.0 o F (Which is also –40.0 o C!). and the
CO2 is at 760.0 Torr. You come back to your room at the Trapp Family Lodge
and set your pack and can of CO2 on the radiator, which is going at full blast.
The temperature of the CO2 goes up to 100o C. The volume of the can doesn’t
change. What is the pressure in the can of CO2?
(A) -1900 Torr
(B) 475 Torr
(C) 1220 Torr
(D) 6202 Torr
REVIEW PROBLEMS FOR FINAL: PAGE 46
23. According to the Kinetic Theory of Gases:
(A) An ideal gas is considered to be composed of particles with no volume and
no attractive or repulsive forces;
(B) All gas particles are assumed to behave like little billiard balls which are
IMMOBILE;
(C) At 0 K all gas molecules are moving rapidly;
(D) The pressure exerted by a gas particle depends only on its mass, not its
velocity;
24. Consider the reaction:
N2(g) + 3F2(g)  2NF3 (g)
If you mixed 1 L of N2 and 4 L of F2 together at STP, and blew them up, how
many Liters of NF3 at STP would you get?
(A) 1 L
(B) 2 L
(C) 3 L
(D) 5 L
25. Radar with a frequency of 500 MHz is used by crime scene investigators to
detect anomalies approximately 3 ft ( 1 meter) below the soil surface, such as
buried bodies. What is the wavelength of this radiation? ( 1 MHz = 106 Hz)
(A) 0.06 M
(B) 0.6 M
(C) 1.67 M
(D) 6 x 105 M
REVIEW PROBLEMS FOR FINAL: PAGE 47
REVIEW PROBLEMS FOR FINAL: PAGE 48
26. The work function of metallic Cesium is 3.43 x 10-19 joules. What minimum
wavelength of light would be necessary to pop electrons off the surface of the Cesium?
(A) 1.72 x 106 M
(B) 7.57 x 10-61 M
(C) 1.55 x 1023 M
(D) 5.79 x 10-7 M
BONUS: Given what you know about the periodic properties of the
elements, would you predict that the work function for Fluorine would be
HIGHER or LOWER than that for cesium? (Circle 1)
HIGHER
LOWER
27. An atom has a valence shell electronic configuration of 6s2 4f10. To
which group of elements does it belong?
(A) The Chalcogens (Group VI)
(B) The Alkaline Earth metals
(C) The Actinides
(D) The Lanthanides
(E) The Transition Metals
28.
The electronic configuration for gold is:
(A) [Xe] 6s2 4f14 5d9
(B) [Xe] 6s2 5d9
(C) [Xe] 6s1 4f14 5d10
(D) [Xe] 6s2 4f14 5d10
REVIEW PROBLEMS FOR FINAL: PAGE 49
31. Rank the following in order of size (largest first, smallest last)
Sulfur, Molybdenum, Radium
Little
Big
(A) S < Mo < Ra
(B) S < Ra < Mo
(C) Mo < S < Ra
(D) Mo < Ra < S
(E) Ra < Mo < S
(F) Ra < S < Mo
32.Define “Electronegativity”:
The measure of the tendency of a combined atom to attract a shared
pair of electrons to itself.