general inorganic chemistry

Question 1

What is the concentration of calcium ions in 350 mL of an aqueous solution containing 7.50 g CaCl2?
a. 0.0676 M c. 0.248 M
b. 0.193 M d. 0.535 M

Answer 1

b. 0.193

Question 2

What is the value of the quantum number l for a 5d orbital?
a. 1
b. 2
c. 3
d. 4

Answer 2

b. 2

Question 3

What is the orbital angular momentum quantum number, l, of the electron that is
most easily removed when ground-state aluminum is ionized?
a. 3
b. 2
c. 1
d. 0

Answer 3

c.1

Question 4

Which compound has the highest normal boiling point?
a. CH3CH2COOH b. CH3COOH
c. CH3CH2 CH2OH d. HCOOCH2CH3

Answer 4

a. CH3CH2COOH

Question 5

Which of the following has the largest radius?
a. Ca+2 b. K+
c. Ar d. Cl- e.S-2

Answer 5

e. S^-2

Question 6

Which of the following is not an intensive property?
a. Density
b. temperature
c. Color
d. Volume

Answer 6

d. Volume

Question 7

Which atom has the greatest first ionization energy?
a. Cl b. Na
c. B d. P

Answer 7

a. Cl

Question 8

What are the percentages by mass of each element in CaCl2?
a.33.3% Ca and 66.7% Cl
b.53.1% Ca and 46.9% Cl
c. 36.1% Ca and 63.9% Cl
d. 69.3% Ca and 30.7% Cl

Answer 8

c. 36.1% Ca and 63.9% Cl

Question 9

How many protons (p), neutrons (n) and electrons (e) are there, respectively, in
an atom of the chlorine-39 isotope? Atomic number of Cl=17
a.17 p, 17 n, 22 e
b. 22 p, 17 n, 17 e
c. 17 p, 39 n, 17 e
d.17 p, 22 n, 17 e

Answer 9

d.17 p, 22 n, 17 e

Question 10

0.1 M aqueous solutions of each of the following, which solution has the lowest
pH?
a. Na2CO3
b. Na3PO4
c. Na2S
d. NaCl

Answer 10

d. NaCl

Question 11

Which of the following is classified as a conjugate acid-base pair?
a. HCl / NaOH
b. H3O+ / H2O
c. O2 / H2O
d. H+/Cl- e. NaCl/ OH-

Answer 11

b. H3O+ / H2O

Question 12

Which of the following is always true of a spontaneous process?
a. The process is exothermic
b. The entropy of the system increases
c. The internal energy of the system decreases
d. The total entropy of the system plus the surrounding increases

Answer 12

d. The total entropy of the system plus the surrounding increases

Question 13

0.100 M solution of a weak monoprotic acid HX is 3.5% ionized. What is the pH
of a 0.500 M solution of HX?
a. 0.30
b. 1.76
c. 2.10
d. 2.46

Answer 13

c. 2.10

Question 14

Which of the following is the most likely as a lewis acid?
a. NH3
b. F-
c. H2O
d. Zn2+

Answer 14

d. Zn2+

Question 15

What is the oxidation state of nitrogen in magnesium nitride?
a. -3
b. -2
c. +3
d. +5

Answer 15

a. -3

Question 16

A system expands in volume from 2.0L to 24.5L at constant temperature. Calculate the work (w), in kJ, if the expansion occurs against a constant pressure of 5.00 atm.
a. -11.4 kJ
b. 11.4 kJ
c. -4.14 kJ
d.-1.14 kJ

Answer 16

a. -11.4 kJ

Question 17

Which of the following diatomic molecule has the longest bond length?
a.N2
b. Cl2
c. O2
d. I2

Answer 17

d. I2

Question 18

How many π electrons are present in a molecule of C6H6?
a. 6
b. 4
c. 5
d. 7

Answer 18

a. 6

Question 19

For the following molecule, what is the hybridization for each carbon?

a. sp c. sp4
b. sp2 d. sp3

Question 20

Consider the molecular substances I2, H2O, and C8H18. Which of them is/aresoluble in CCl4?
a. only I2
b. only H2O
c. only C8H18
d. I2 and C8H18
e. H2O and C8H1

Answer 20

d. I2 and C8H18

Question 21

Which change will increase the number of moles of PCl5(g) present at equilibrium?
PCl3(g) + Cl2(g) → PCl5(g) + heat

a. The volume of the reaction is tripled
c. Some of the Cl2(g) is removed
b. The reaction vessel is cooled
d. Krypton gas is added to the reaction vessel

Answer 21

b. The reaction vessel is cooled

Question 22

A gaseous compound is composed of 85.7% C and 14.3%H. Its density is 2.28 g/L at 300K and 1.00 atm pressure. Determine the molecular formula of the compound.
C=12.01, H=1.01

a. C2H4
b. C3H6
c. C4H8
d. C5H10

Answer 22

c. C4H8

Question 23

An aqueous solution labeled 35.0% HCLO4 (𝑤/𝑤 ) had a density of
1.251𝑔/𝑐𝑚3. What is the molarity of the solution? H=1.01, Cl=35.45, O=15.99

a. 4.36 M
b. 3.46 M
c. 6.43 M
d. 2.46 M

Answer 23

a. 4.36 M

Question 24

4. A current of 15.0 A is passed through a solution of CrCl2 for 45 min. How many gram of Cr is deposited on the cathode? Cr=52.00, Cl=35.45
   a. 9.10 g Cr
   b. 11.9 g Cr
   c. 10.9 g Cr
   d. 8.9 g Cr

Answer 24

c. 10.9 g Cr

Question 25

A 1.500 g sample of a compound containing only C,H, and O was burned completely. The only combustion products were 1.738 g CO2 and 0.711 g H2O. What is the empirical formula of the compound? C=12.01, H=1.01, O=15.99 a. C2H4O3 b. C2H3O2 c. C3H4O2 d. C3H4O3

Answer 25

a. C2H4O3

Question 26

certain public water supply contained 0.10 ppb (parts per billion) of chloroform, CHCl3. How many molecules of CHCl3 would be contained in a 0.050 mL drop of this water? C=12.01, H=1.01, O=15.99 a. 5.2 x10-10 molecules b. 3.5 x1010 molecules c. 2.5 x10-10 molecules d. 2.5 x1010 molecules

Answer 26

c. 2.5 x10-10 molecules

Question 27

According to EPA guidelines the permissible level for lead in drinking water is 15 parts per billion (ppb). What is the maximum allowable mass of lead that could be present in 1.00 L of H2O? a. 0.015 ng b. 0.015mg c. 0.015µg d. 0.015g

Answer 27

b. 0.015mg

Question 28

According to the Tyndall effect, a beam of light becomes visible when passed through all of the following except a/an a. aerosol b. emulsion c. colloid d. solution

Answer 28

b. emulsion

Question 29

Which physical property decreases with an increase in intermolecular forces? a. boiling point b. vapor pressure c. enthalpy of vaporization d.viscosity

Answer 29

b. vapor pressure

Question 30

The rate constant of a first-order reaction is 3.68 x10-2s-1 at 150 oC, and the activation energy is 71 kJ/mol. What is the value of the rate constant at 170 oC? a. 9.2 x10-2s-1 b. 3.7 x10-2s-1 c. 2.49 s-1 d. 4.0 x10-2s-1

Answer 30

a. 9.2 x10-2s-1