LBS 171 REVIEW QUESTIONS
MOLAR MASS
1.) What is the molar mass of a.) Na b.) H
2 c.) NH
4 d.) C
3
H
6
Cl
2
MOLARITY
2.) What is the molarity of a.) 3.62 mol NaCl in a 400.0 mL solution b.) 0.36 g Na
3
PO
4
●12H
2
O in a 200.0 mL solution c.) HCl if 130.0 mL water is added to 20.0 mL of a 0.5 M HCl solution
STOICHIOMETRY
3.) What mass of Al(OH)
3
is needed to create 6.0 mol of AlCl
3
in:
Al(OH)
3
+ 3HCl

AlCl
3
+ 3H
2
O
4.) How many g CO
2
produced from combustion of 27.4 g of C
6
H
8
in the unbalanced
equation: C
6
H
8
+ O
2

CO
2
+ H
2
O
If 87.6 g CO
2
is actually produced in an experiment, what is the percent yield of CO
2
?
5.) How many moles of AlCl
3
are needed to completely react with the NaOH in 120.0 mL
of a 4.2 M NaOH solution in the unbalanced equation:
AlCl
3
+ NaOH(aq)

Al(OH)
3
+ NaCl
LIMITNG REACTANT
6.) What mass of CrCl
3
is produced from 32.6 g Cr and 56.0 g Cl
3 in:
2Cr(s) + 3Cl
2
(g)

2CrCl
3
(s)
What mass of excess reactant is left after the reaction completes?
7.) What mass of CaSO
4
is produced if 13.4 g CaCO
3
, 15.0 L O
2
gas, and 10.0 L SO
2
gas
are added in a closed system in the unbalanced equation:
SO
2
(g) + CaCO
3
(s) + O
2
(g)

CaSO
4
(s) + CO
2
(g)
What volume of O
2
gas remains, if any, after the reaction completes?
D(O
2 gas) = 1.429 g/L, D(SO
2 gas) = 2.551 g/L
RYDBERG
8.) Using the Rydberg equation, find the λ of light emitted when an e
-
falls from n=5 to
n=2 in an H atom

ELECTROMAGNETIC RADIATION
9.) Calculate the frequency of green light with a wavelength of 540 nm. How much energy, in kJ, does 1.0 mol of photons of this light have?
10.) Rank the following types of electromagnetic radiation in order of increasing frequency: Gamma rays, Infrared rays, UV rays, Radio waves
11.) What is the wavelength of EM radiation with an Energy of 3296.1 kJ/mol?
BOHR
12.) What is the energy, in kJ/mol, of an electron in the n = 4 orbit of an H atom?
13.) Compute the minimum frequency of light required to remove an electron from the
n = 3 orbit of an H atom
14.) What are the wavelength and frequency of light emitted when an electron drops from
n = 3 to n =2 ?
QUANTUM NUMBERS
15.) a.) When n = 3, what are the possible values of l
?
b.) When l
= 3, what are the possible values of m l ?
c.) For a 6d orbital, what are the possible values of n, l
, and m l
?
16.) a.) How many subshells occur in the electron shell with n = 3?
b.) How many orbitals occur possible in the electron shell with n = 4?
c.) How many orbitals can be defined by l
= 3?
d.) What is the maximum number of electrons in an atom that can be defined with l
= 1 ?
e.) How many nodal surfaces occur in a d subshell?
17.) Which of the following sets of quantum numbers for an electron in an atom are
Impossible? a.) n = 1, l
= 1, m l
= -1 b.) n = 4, l
= 0, m l = -2 c.) n = 3, l
= 2, m l = 2, m s
= 0

ELECTRON CONFIGURATION
18.) Write the electron configuration for the following: a.) N b.) Co c.) Sr
19.) Write the noble gas shorthand for the following: a.) Fe b.) Cr c.) Gd
20.) Draw an energy level diagram for Al. Is it paramagnetic or diamagnetic?
PERIODIC TRENDS
21.) Arrange the following sets of elements in order of increasing size: a.) K, Po, Ba, Ga b.) Zr, Cr, Cr
2+
, V
22.) Arrange the following sets of elements in order of increasing ionization energy: a.) Be, K, B, N, O b.) Na, Ca 2+ , Ca, Na +
LEWIS DOT STRUCTURES
23.) Draw the Lewis structures for the following compounds: a.) N
2 b.) CO
2 c.) XeF
4 d.) H
2
SO
4
24.) Draw the Lewis structure and all of the resonance structures and calculate the bond
order for the following
compounds: a.) NO
2 b.) PO
4
NAMING COMPOUNDS
25.) Name the following ionic compounds: a.) NaCl b.) CaCO
3 c.) Au(OH)
3

26.) Name the following molecular compounds: a.) S
2
Cl
2 b.) HF
27.) Name the following acids: a.) HClO
3 b.) H
2
CO
3 c.) HCl
28.) Name for the following compounds: a.) HIO
4 b.) Sn(CN)
2 c.) SrSO
3
29.) Give the formula for the following compounds: a.) ammonium chloride b.) hydrophosphorous acid c.) dihydrogen monoxide
MOLECULAR STRUCTURE
30.) Draw the molecular structure and give approximate bond angles for the following
compounds: a.) CH
4 b.) PCl
5 c.) SF
6
31.) Draw and name the molecular structure of the following compounds: a.) H
2
O b.) SF
4 c.) XeF
4
POLARITY
32.) Determine if the following molecules are polar: a.) CO
2
X (C) = 2.5, X (O) = 3.5 b.) CHCl
3
X (C) = 2.5, X (Cl) = 3.5, X (H) = 2.1 c.) CH
4
HYBRIDIZATION
33.) Draw the orbital overlaps responsible for chemical bonding in the following
Molecules: a.) CH
4 b.) C
2
H
4

ORGANIC CHEMISTRY
34.) Draw the organic products of the following reactions
+ Br
2
UV Ligh t a.)
H b.) c.) d.) e.)
+
+ HBr
+ H
2
Pt cat.
H
H
C Cl
AlCl
3
cat.
H
OH + K
2
Cr
2
O
7
(aq)
H + LiAlH
4
H
2
O f.)
O
O
NaOH g.)

h.)
O O
NH
2
NH
2
+
OH OH
HEAT TRANSFER
35.) Calculate the heat absorbed, in kJ, when a 50.0 g block of ice at -2 °C is converted to
steam at 109°C c s
(ice) = 2.09 J/g*°C, c s
(water) = 4.184 J/g*°C, c s
(steam) = 2.01 J/g*°C
ΔH fus
(H
2
O) = 6.01 kJ/mol,
ΔH vap
(H
2
O) = 40.7 kJ/mol,
36.) A 130.0 g bar of iron at 370.0 °C is immersed in 500.0 g of water at 20.0 °C. Find the
final temperature for the iron and the water. c s
(iron) = 0.444 J/g*°C c s
(water) = 4.184 J/g*°C
CHANGE IN ENTHALPY
37.) Find ΔH reaction
ΔH f
° for the combustion of ethanol.
°(ethanol) = -277.7 kJ/mol
ΔH f
°(H
2
0) = -241.8 kJ/mol
ΔH f
°(CO
2
) = -393.51 kJ/mol
38.) 0.140 mol NaOH and 0.030 mol HCl are reacted in 100.0 g water:
NaOH(aq) + HCl(aq)

H
2
O + NaCl(aq)
The water heats from 23.0°C to 26.7°C during the reaction.
Find ΔH reaction
for HCl c s
(H
2
O) = 4.184 J/g*°C