Question: Determine the number of protons, neutrons and electrons in
the following:
X
A) p+= 36 n = 29 e-= 36
B) p+= 29 n = 29 e-= 36
C) p+= 36 n = 36 e-= 29
D) p+= 29 n = 36 e-= 29
E) p+= 29 n = 36 e-= 36
Answer:View Answer
Question: How many liters of hydrogen gas can be generated by reacting
9.25 grams of barium hydride with water at 20C and 755 mm Hg
pressure according to the chemical equation shown below?
BaH2(s) + 2 H2O(l) Ba(OH)2(aq) + 2 H2(g)
A) 0.219 L
B) 0.799 L
C) 1.60 L
D) 3.21 L
Answer:View Answer
Question: How many of the following species are paramagnetic?
Sc3 Cl Ba2 Se
A) 0
B) 2
C) 1
D) 4
E) 3
Answer:View Answer
Question: Match the following.
A) electrons in the outermost shell
B) 1
C) electrons in completed shells
D) 2
E) number of unpaired electrons in Zn2+
1-Question: valence electrons
1-Question: core electrons
1-Question: number of unpaired electrons in Na
1-Question: 0
1-Question: number of unpaired electrons in Ti2+
Answer:View Answer
Question: Which of the following statements is TRUE?
A) A nucleotide is composed of a sugar, a base and a phosphate
group.
B) A codon is a sequence of 3 bases that codes for a single amino
acid.
C) A gene is a portion of DNA that codes for a single protein
D) A chromosome is a structure within a cell nucleus that houses
DNA.
E) All of the above are true.
Answer:View Answer
Question: Match the following.
A) [Cr(NHQuestion:3(CO)3]3+
B) [Ni(CN)2(OH)2]2-
C) [Zn(NHQuestion:2Cl2]Br2 and [Zn(NHQuestion:2Br2]Cl2
D) [Cu(SCN)4]3- and [Cu(NCS)4]3-
E) [Cr(en)3]3+
1-Question: linkage
1-Question: coordination
1-Question: cis-trans
1-Question: mer-fac
1-Question: optical
Answer:View Answer
Question: What is n for the following equation in relating Kcto Kp?
2 Rb(s) + 2 H2O(l) 2 RbOH(aq) + H2(g)
A) 3
B) -1
C) -2
D) 2
E) 1
Answer:View Answer
Question: Consider the following reaction and its equilibrium constant:
I2(g) 2I(g) Kp= 0.209
A reaction mixture contains 0.89atm I2and1.601.60 atm I. Which of
the following statements is TRUE concerning this system?
A) The reaction will shift in the direction of reactants.
B) The reaction quotient will increase.
C) The reaction will shift in the direction of products.
D) The equilibrium constant will decrease.
E) The system is at equilibrium.
Answer:View Answer
Question: Write a nuclear equation for the alpha decay of 
U.
A) 
U
n
+ 
U
B) 
U
e
+ 
Np
C) 
U
He
+ 
Th
D) 
U
e
+ 
Pa
E) 
U
e
+ 
Pa
Answer:View Answer
Question: Determine the product(s) of the reduction of the following
compound:
A)
B)
C)
D)
E)
Answer:View Answer
Question: In an acid-base neutralization reaction 38.74 mL of 0.500 M
potassium hydroxide reacts with 50.00 mL of sulfuric acid
solution. What is the concentration of the H2SO4solution?
A) 0.194 M
B) 0.387 M
C) 0.775 M
D) 1.29 M
Answer:View Answer
Question: What element is being oxidized in the following redox
reaction?
C3H8O2(aq) + KMnO4(aq) C3H2O4K2(aq) + MnO2(aq)
A) C
B) H
C) O
D) K
E) Mn
Answer:View Answer
Question: In the best Lewis structure for NO +, what is the formal
charge on the N atom?
A) -1
B) 0
C) +1
D) +2
Answer:View Answer
Question: Determine the electron geometry (eg) and molecular geometry
(mg) of CO32.
A) eg=tetrahedral, mg=tetrahedral
B) eg=tetrahedral, mg=trigonal pyramidal
C) eg=trigonal planar, mg=bent
D) eg=trigonal planar, mg=trigonal planar
E) eg=tetrahedral, mg=trigonal planar
Answer:View Answer
Question: Which rate law is bimolecular?
A) rate = k[A][B]3
B) rate = k [A][B]
C) rate = k [A]3
D) rate = k [A][B][C][D]
E) rate = k [A]2[B]2
Answer:View Answer
Question: Identify the oxidation state of H in H2(g).
Mg(s) + 2HI(aq) MgI2(aq) + H2(g)
A) +1
B) +2
C) 0
D) -1
E) -2
Answer:View Answer
Question: Using the following equation for the combustion of octane,
calculate the amount of grams of carbon dioxide formed from 100.0
g of octane. The molar mass of octane is 114.33 g/mole. The molar
mass of carbon dioxide is 44.0095 g/mole.
2 C8H18+ 25 O2 16 CO2+ 18 H2O Hrxn = -11018 kJ
A) 800.1 g
B) 307.9 g
C) 260.1 g
D) 792.3 g
Answer:View Answer
Question: How many valence electrons do the halogens possess?
A) 5
B) 6
C) 2
D) 1
E) 7
Answer:View Answer
Question: Calculate DSrxnfor the following reaction. The S for each
species is shown below the reaction.
P4(g) + 10 Cl2(g) 4 PCl5(g)
S(J/molK) 280.0 223.1 364.6
A) -138.5 J/K
B) -1052.6 J/K
C) +171.3 J/K
D) -583.6 J/K
E) +2334.6 J/K
Answer:View Answer
Question: Give the organic product for the following reaction.
CH3CH2CH2NH2+ HCl
A) ClCH2CH2CH2NH2
B) CH3CHClCH2NH2
C) CH3CH2CHClNH2
D) CH3CH2CH2NHCl
E) CH3CH2CH2NH3+ Cl-
Answer:View Answer
Question: Calculate the hydronium ion concentration in an aqueous
solution with a pH of 4.33 at 25C.
A) 2.1 10-10M
B) 9.7 10-10 M
C) 4.7 10-5M
D) 3.8 10-5M
E) 6.3 10-6M
Answer:View Answer
Question: The isomerization reaction, CH3NC CH3CN, is first order and
the rate constant is equal to 0.46 s-1at 600 K. What is the
concentration of CH3NC after 0.20 minutes if the initial
concentration is 0.30 M?
A) 1.2 10-3M
B) 2.7 10-3M
C) 1.2 10-1M
D) 2.7 10-1M
Answer:View Answer
Question: Calculate the pH of a buffer that is 0.020 M HF and 0.040 M
NaF. The Kafor HF is 3.5 10-4.
A) 2.06
B) 4.86
C) 3.16
D) 3.36
E) 3.76
Answer:View Answer
Question: Identify the compound with the lowest standard free energy of
formation.
A) NaCl(s)
B) O2(g)
C) NO(g)
D) O3(g)
E) It is hard to determine.
Answer:View Answer
Question: Write the formula for the compound formed between potassium
and sulfur.
A) KS
B) KS2
C) K2S
D) K2SO3
E) K3S2
Answer:View Answer
Question: What is the O-B-O bond angle in BO33-?
A) less than 109.5
B) 109.5
C) 120
D) greater than 120
Answer:View Answer
Question: In which set do all elements tend to form cations in binary
ionic compounds?
A) K, Ga, O
B) Sr, Ni, Hg
C) N, P, Bi
D) O, Br, I
Answer:View Answer
Question: Type I diabetes develops when the pancreas does not make
enough ________.
A) cholesterol
B) sucrose
C) blood
D) insulin
E) iron
Answer:View Answer
Question: How much energy is required to vaporize 48.7 g of
dichloromethane (CH2ClQuestion: at its boiling point, if its Hvapis 31.6
kJ/mol?
A) 31.2 kJ
B) 6.49 kJ
C) 55.1 kJ
D) 15.4 kJ
E) 18.1 kJ
Answer:View Answer
Question: A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF.
Calculate the pH of the solution after the addition of 0.100
moles of solid NaOH. Assume no volume change upon the addition of
base. The Kafor HF is 3.5 10-4.
A) 3.22
B) 3.82
C) 3.69
D) 3.09
E) 4.46
Answer:View Answer
Question: Name the following compound.
A) trans-2-butane
B) cis-2-butene
C) cis-2-pentene
D) trans-3-pentene
E) 2-pentene
Answer:View Answer
Question: Calculate the solubility (in g/L) of calcium fluoride in
water at 25C if the Kspfor Ca F2 is
1.5 10-10.
A) 9.6 10-4g/L
B) 2.6 10-2g/L
C) 3.3 10-2g/L
D) 4.1 10-2g/L
Answer:View Answer
Question: Give the set of four quantum numbers that could represent the
last electron added (using the Aufbau principle) to the Ne atom.
A) n = 2, l = 1, ml= 1, ms= + 
B) n = 3, l = 0, ml= 1, ms= + 
C) n = 3, l = 2, ml=1, ms= + 
D) n = 2, l = 1, ml= 1, ms= – 
E) n = 3, l =2, ml= 1, ms= – 
Answer:View Answer
Question: What is n for the following equation in relating Kcto Kp?
4 NH3(g) + 3 O2(g) 2 N2(g) + 6 H2O(g)
A) 3
B) -1
C) -2
D) 2
E) 1
Answer:View Answer
Question: How many valence shell electrons does an atom of indium have?
A) 1
B) 4
C) 3
D) 49
E) 2
Answer:View Answer
Question: A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH.
Determine the pH of the solution after the addition of 300.0 mL
of KOH. The Kaof HF is 3.5 10-4.
A) 12.40
B) 9.33
C) 5.06
D) 8.94
E) 12.00
Answer:View Answer
Question: The average distance between nitrogen and oxygen atoms is 115
pm in a compound called nitric oxide. What is this distance in
millimeters?
A) 1.15 10-8 mm
B) 1.15 10-7 mm
C) 1.15 1013 mm
D) 1.15 1017mm
Answer:View Answer
Question: What is the volume of 5.60 g of O2at 7.78 atm and 415K?
A) 1.53 L
B) 565 L
C) 24.5 L
D) 25.0 L
E) 0.766 L
Answer:View Answer
Question: Determine the longest wavelength of light required to remove
an electron from a sample of potassium metal, if the binding
energy for an electron in K is 1.76 103kJ/mol.
A) 147 nm
B) 68.0 nm
C) 113 nm
D) 885 nm
E) 387 nm
Answer:View Answer
Question: A FeCl3solution is 0.175 M. How many mL of a 0.175 M FeCl3
solution are needed to make 450. mL of a solution that is 0.300 M
in Cl-ion?
A) 0.771 mL
B) 257 mL
C) 771 mL
D) It is not possible to make a more concentrated solution from a
less concentrated solution.
Answer:View Answer
Question: Explain the common ion effect with respect to molar
solubility.
Answer:View Answer
Question: Describe the difference between a pure covalent bond and a
polar covalent bond.
Answer:View Answer
Question: How does a dosimeter measure exposure to radioactivity?
Answer:View Answer
Question: Calculate the osmotic pressure, in torr, of a solution
containing 3.00 mg of a sugar (342 g/mole) in 15.0 mL of water at
25C.
Answer:View Answer
Question: Explain why oil and water do not mix.
Answer:View Answer
Question: Why is an equilibrium constant unitless?
Answer:View Answer
Question: Sketch one of the 3p orbitals below. How are they different
from the 2p orbitals?
Answer:View Answer
Question: Why are the chemical properties of nitrogen and phosphorus so
different when they are in the same family?
Answer:View Answer