1. Do the following arithmetic operations:
(a) 14.57 mm – 11.6 mm
(b) 23.7 cm x 5.8 cm
2. Do the following metric conversions:
(a) 347 mg to g
(b) 175 cL to kL
3. Give the reading on each instrument:
4. Answer the following questions for these three species:
18
O
18
O-
18
O2-
(a) determine the number of protons, neutrons, and electrons
(b) write the electron configuration notation
(c) write the electron dot notation
(d) give the number of unpaired electrons
5. Answer the following questions for these three atoms:
31
P
112
Cd
120
Sn
(a) determine the number of protons, neutrons, and electrons
(b) write the electron configuration notation
(c) write the electron dot notation
(d) give the number of unpaired electrons
(e) arrange the atoms from smallest atomic radii to largest atomic radii
(f) arrange the atoms from lowest ionization energy to highest ionization energy
(g) arrange the atoms from lowest electronegativity to highest electronegativity
6. Answer the following questions concerning a 12.5 g sample of iron:
(a) determine the number of moles of iron
(b) determine the number of atoms of iron
7. Answer the following questions for these three bonds:
C-C
C-F
C-I
(a) identify each bond as either nonpolar covalent, polar covalent, or ionic
(b) identify the bond that is the most polar
8. Answer the following questions for these six molecules or ions:
SiCl4
AsH3
O2
CO
NO2 -
SiS2
(a) draw the Lewis structure
(b) determine the shape of the molecule
(c) determine the polarity of the bonds in the molecule or ion
(d) determine the polarity of the molecule or ion
9. Give the names of the following compounds:
(a) Mg3 N2
(b) Na2 SO4
(c) FeCl3
(d) SnCr 2 O7
(e) SF2
(f) N2 O
(g) HBr
(h) H2 CO3
10. Give the formulas of the following compounds:
(a) aluminum oxide
(b) ammonium sulfide
(c) nickel (II) hydroxide
(d) silver phosphate
(e) carbon tetrachloride
(f) diphosphorus trioxide
(g) nitric acid
(h) hydrofluoric acid
11. Answer the following questions concerning a 17.2 g sample of diboron trioxide:
(a) determine the number of moles of diboron trioxide
(b) determine the number of molecules of diboron trioxide
(c) determine the number of moles of boron
(d) determine the number of atoms of boron
(e) determine the number of moles of atomic oxygen
(f) determine the number of atoms of oxygen
12. Determine the percent composition by mass of each element in potassium permanganate.
13. A compound has the following composition by mass: 50.0% sodium, 15.2% silicon, and 34.8%
oxygen. Determine the empirical formula of the compound.
14. A compound having a molar mass between 110 and 130 grams has the following composition by
mass: 93.70% carbon and 6.30% hydrogen.
(a) determine the empirical formula of the compound
(b) determine the molecular formula of the compound
15. Complete and balance the following reactions in molecular form:
(a) aluminum metal and chlorine gas react
(b) lead (II) oxide is decomposed
(c) methanol (CH3 OH) is burned in air
(d) zinc metal is added to a soliution of silver nitrate
(e) magnesium metal is added to a solution of acetic acid
(f) lithium metal is added to water
(g) fluorine gas is bubbled through a solution of sodium chloride
(h) methane is burned in air
16. For the following reactions write (1) the molecular equation with phases, (2) the ionic equation with
phases, and (3) the net ionic equation with phases
(a) solutions of calcium bromide and potassium sulfate are mixed
(b) solutions of phosphoric acid and sodium hydroxide are mixed
17. Magnesium nitride decomposes when heated to magnesium metal and nitrogen gas.
(a) balance the equation
(b) identify the element oxidized and the element reduced
(c) calculate the number of moles of magnesium metal and the number of moles of nitrogen gas that
are produced from the decomposition of 0.250 moles of magesium nitride
18. Determine the pressure of dry hydrogen gas at 25ºC in each of the following. Atmospheric pressure
is 753 mm Hg and water vapor pressure at 25ºC is 24 mm Hg.
19. Neptunium (IV) oxide reacts with hydrofluoric acid and hydrogen gas to produce neptunium (III)
fluoride and water.
(a) balance the equation
(b) calculate the mass of neptunium (III) fluoride produced when 0.645 grams of neptunium (IV)
oxide reacts with 25.0 mL of 0.500 M hydrofluoric acid and 125 mL of hydrogen gas at a
temperature of 23°C and a pressure of 152 torr
(c) identify the limiting reactant
(d) if the actual yield of neptunium (III) fluoride was 0.531 grams, claculate the percent yield
20. Determine the volume the hydrogen gas from problem 19b would occupy at STP.
21 Identify the acid and the base in the following reaction:
(a) CH3 NH2 + H2 O ?
CH3 NH3 + + OH-
(b) C6 H5 OH + H2 O ?
C6 H5 O- + H3 O+
22. Give the conjugate acid of the following bases:
(a) NH3
(b) HCO3
-
23 Give the conjugate base of the following acids:
(a) HClO4
(b) HCO3
-
24. Find the [H3 O+], [OH-], and pH of the following solutions:
(a) 0.125 M hydrochloric acid
(b) 0.125 M sodium hydroxide
25. Identify the two components from below that if combined in equal amounts would form a buffer
HCl
HNO2
NaOH
NaCl
KNO2
ANSWERS
1. (a) 3.0 mm
(b) 140 cm2
2. (a) 0.347 g
(b) 0.00175 kL
3. (a) 13.80 mL
(b) 22.5°C
4. (a) 8 p, 10 n, 8 e
2
2
(b) 1s 2s 2p
4
..
(c) . O :
.
(d) 2
(c) 11.60 cm
8 p, 10 n, 9 e
2
2
1s 2s 2p
5
.. : O:
.
1
8 p, 10 n, 10 e
1s 2 2s 2 2p6
. . 2: O:
..
0
5. (a) 15 p, 16 n, 15 e
2
48 p, 64 n, 48 e
3
2
50 p, 70 n, 50 e
(b) [Ne]3s 3p
.
(c) . P :
.
[Kr]5s 4d
Cd :
[Kr]5s 2 4d10 5p2
.
. Sn :
(d) 3
0
2
(e) P < Sn < Cd
10
(f) Cd < Sn < P
(g) Cd < Sn < P
(b) 1.35 x 1023 atoms Fe
6. (a) 0.224 mol Fe
7. (a) C-C nonpolar covalent
C-F polar covalent
C-I polar covalent
(b) C-F
8. (a)
(b) tetrahedral
trigonal
pyramidal
linear
linear
bent (120º)
linear
linear
(c) polar
polar
nonpolar
polar
polar
polar
(d) nonpolar
polar
nonpolar
polar
polar
nonpolar
9. (a) magnesium nitride
(e) sulfur difluoride
(b) sodium sulfate
(c) iron (III) chloride
(d) tin (II) dichromate
(f) dinitrogen monoxide (g) hydrobromic acid
(h) carbonic acid
(b) (NH4 )2 S
(c) Ni(OH) 2
(d) Ag3 PO4
(f) P2 O3
(g) HNO3
(h) HF
11. (a) 0.247 mol B2 O3
(b) 1.49 x 1023 molec.
(c) 0.494 mol B
(d) 2.98 x 1023 atoms
(e) 0.741 mol O
(f) 4.46 x 1023 atoms
10. (a) Al2 O3
(e) CCl4
12. 24.75% K, 34.76% Mn, 40.49% O
13. Na4 SiO4
14. (a) C5 H4
(b) C10 H8
15. (a) 2Al + 3Cl2 → 2AlCl3
(b) 2PbO → 2Pb + O2
(c) 2CH3 OH + 3O2 → 2CO2 + 4H2 O
(d) Zn + 2AgNO3 → Zn(NO3 )2 + 2Ag
(e) Mg + 2HC 2 H3 O2 → Mg(C2 H3 O2 )2 + H2
(f) 2Li + 2H2 O → 2LiOH + H2
(g) F2 + 2NaCl → 2NaF + Cl2
16. (a) CaBr 2 (aq) + K2 SO4 (aq) ?
-
2+
CaSO4 (s) + 2KBr(aq)
+
Ca (aq) + 2Br (aq) + 2K (aq) + SO4 2-(aq) ?
-
CaSO4 (s) + 2K+(aq) + 2Br (aq)
Ca2+(aq) + SO4 2-(aq) → CaSO4 (s)
(b) H3 PO4 (aq) + 3NaOH(aq) → 3H2 O(l) + Na3 PO4 (aq)
-
H3 PO4 (aq) + 3Na+(aq) + 3OH (aq) ? 3H2 O(l) + 3Na+(aq) + PO4 3-(aq)
H3 PO4 (aq) + 3OH-(aq) → 3H2 O(l) + PO4 3-(aq)
17. (a) Mg3N2 → 3Mg + N2
(b) N oxidized, Mg reduced
(c) 0.750 mol Mg, 0.250 mol N2
18. (a) 157 mm Hg
(b) 910. mm Hg
(c) 729 mm Hg
19. (a) 2NpO2 + 6HF + H2 → 2NpF3 + 4H2 O
(b) 0.605 g NpF3
(c) H2
(d) 87.6%
20. 23.0 mL
21. (a) acid: H2 O, base: CH3 NH2 (b)
22. (a) NH4 +
23. (a) ClO4
-
24. (a) 0.903
25. HNO2 and KNO2
(b) H2 CO3
(b) CO3 2(b) 13.097
acid: C6 H5 OH, base: H2 O
(d) 719 mm Hg