Chapter Two Practice Quiz
Use the following to answer questions 1-2.
Refer to the following covalent molecule of methane to answer the question(s) below.
1. The total number of valence electrons in methane is
A) 2.
B) 4.
C) 8.
D) 16.
E) 40.
2. The arrow is pointing to
A) a triple bond.
B) a double bond.
C) a single bond.
D) an electron.
E) a valence shell.
3. A normal blood oxygen (O2 ) level is 8.0 mmol/l. What is the normal mass of oxygen per
liter of blood?
A) 2.50 × 10– 4 g
B) 0.256 g
C) 4.00 g
D) 256 g
E) 2.56 × 105 g
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4. Calculate the molecular mass of aspirin, C9 H8 O4 .
A) 29 g/mole
B) 126 g/mole
C) 180. g/mole
D) 126 amu
E) 180. amu
5. Lewis electron dot structures represent ________.
A) the number of unpaired electrons in an atom.
B) the total number of electrons in the atom.
C) the number of protons in the atom.
D) the number of valence electrons.
E) the number of nonbonding electrons.
6. A polyatomic ion ...
A) has many atoms, one of which has gained or lost electrons.
B) is a molecule that has gained or lost electrons.
C) has many atoms, one of which has gained or lost protons.
D) is a molecule that has gained or lost protons.
E) has many charges.
7. Carbon tetrafluoride is a refrigerant and potent greenhouse gas. Which of the following is
the molecular formula for this compound?
A) CF
B) C(IV)F
C) CF(IV)
D) CF4
E) CF4
8. Which of the following is the formula for an ionic compound called manganese(II) chloride?
A) Mg(II)Cl
B) Mn(II)Cl
C) Mg2 Cl
D) M n2 Cl
E) MnCl2
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Use the following to answer questions 9-13.
Refer to the following illustration of an ion to answer the question(s) below.
9. How many electrons are in the valence shell of this ion?
A) 2
B) 8
C) 10
D) 12
E) 22
10. The charge on this ion is _______ making the ion a _______.
A) –10; anion
B) –2; anion
C) –2; cation
D) + 2; anion
E) + 2; cation
11. To make this ion, the atom that it came from had to _______.
A) become a different atom
B) gain electrons
C) become a nonmetal
D) lose electrons
E) become a metal
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12. This figure represents an ion of _______.
A) helium
B) oxygen
C) neon
D) magnesium
E) titanium
13. Which statement best describes why this ion formed from the atom?
A) The ion formed so that it would have a similar electron arrangement as the nearest noble
gas.
B) The ion formed so that it would minimize the mass of the atom.
C) The ion formed because another ion needed the electrons more than the atom above.
D) The ion formed because another ion needed the electrons less than the atom above.
E) There is no particular reason that this ion formed.
14. Which of the following values is Avogadro's number?
A) 6
B) 6.02
C) 6.02 × 102 3
D) 6.02 × 102 6
E) 6.02 × 10123
15. Below are two ions (not drawn to scale). What will they do when in close proximity to one
another?
A)
B)
C)
D)
E)
They will attract one another, forming an ionic compound.
They will attract one another, forming a covalent bond.
The sodium ion will transfer a proton to chloride.
The chloride ion will transfer an electron to sodium.
They will do nothing.
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16. Which of the following elements forms a cation?
A) carbon
B) phosphorous
C) krypton
D) nickel
E) iodine
17. Which of the following is not a valid ionic formula?
A) NaF
B) MgO
C) KCl2
D) CaF2
E) Na2 O
18. How many moles of the antibiotic tetracycline (C2 2H2 4N2 O8 ) are in a 50-mg dose?
A) 8880 moles
B) 22.2 moles
C) 8.88 moles
D) 0.113 moles
E) 1.13 × 10– 4 moles
19. “Laughing gas” has the formula N2 O. Which of the following is the best name for this
compound?
A) nitrogen oxygen
B) nitrogen oxide
C) nitrogen dioxide
D) dinitrogen monoxide
E) nitrogen(II) oxide
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Use the following to answer question 20.
Refer to the following ion of oxygen to answer the question(s) below.
20. Oxygen is a _______ and therefore _______ when it forms an ion.
A) metal; loses electrons
B) metal; gains electrons
C) nonmetal; loses electrons
D) nonmetal; gains electrons
E) metalloid; loses electrons
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Answer Key - Chapter 2 Practice
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
C
C
B
E
D
B
E
E
B
E
D
D
A
C
A
D
C
E
D
D
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