1) There are __________ paired and
__________ unpaired electrons in the Lewis symbol for a phosphorus atom.
A) 4, 2
B) 2, 4
C) 2, 3
D) 4, 3
E) 0, 3
2) In the Lewis symbol for a fluorine
atom, there are __________ paired and __________ unpaired electrons.
A) 4, 2
B) 4,1
C) 2, 5
D) 6, 1
E) 0, 5
3) The halogens, alkali metals, and
alkaline earth metals have __________ valence electrons, respectively.
A) 7, 4, and 6
B) 1, 5, and 7
C) 8, 2, and 3
D) 7, 1, and 2
E) 2, 7, and 4
4) The only noble gas without eight
valence electrons is __________.
A) Ar
B) Ne
C) He
D) Kr
E) All noble gases have eight valence
electrons.
5) Which of the following would have to
lose two electrons in order to achieve a noble gas electron configuration?
O
Sr Na Se Br
A) O, Se
B) Sr
C) Na
D) Br
E) Sr, O, Se
6) Elements from opposite sides of the
periodic table tend to form __________.
A) covalent compounds
B) ionic compounds
C) compounds that are gaseous at room
temperature
D) homonuclear diatomic compounds
E) covalent compounds that are gaseous
at room temperature
7) How many single covalent bonds must
a silicon atom form to have a complete octet in its valence shell?
A) 3
B) 4
C) 1
D) 2
E) 0
8) What is the maximum number of double
bonds that a hydrogen atom can form?
A) 0
B) 1
C) 2
D) 3
E) 4
9) The ability of an atom in a molecule
to attract electrons is best quantified by the __________.
A) paramagnetism
B) diamagnetism
C) electronegativity
D) electron change-to-mass ratio
E) first ionization potential
10) Electronegativity __________ from
left to right within a period and __________ from top to bottom within a group.
A) decreases, increases
B) increases, increases
C) increases, decreases
D) stays the same, increases
E) increases, stays the same
11) The type of compound that is most
likely to contain a covalent bond is __________.
A) one that is composed of a metal from
the far left of the periodic table and a nonmetal from the far right of the
periodic table
B) a solid metal
C) one that is composed of only
nonmetals
D) held together by the electrostatic
forces between oppositely charged ions
E) There is no general rule to predict
covalency in bonds.
12) Of the atoms below, __________ is
the most electronegative.
A) Br
B) O
C) Cl
D) N
E) F
13) Of the atoms below, __________ is
the least electronegative.
A) Rb
B) F
C) Si
D) Cl
E) Ca
14) Which of the following names is/are
correct for the compound TiO2?
A) titanium dioxide and titanium (IV)
oxide
B) titanium (IV) dioxide
C) titanium oxide
D) titanium oxide and titanium (IV)
dioxide
E) titanium (II) oxide
15) The Lewis structure of N2H2 shows __________.
A) a nitrogen-nitrogen triple bond
B) a nitrogen-nitrogen single bond
C) each nitrogen has one nonbonding
electron pair
D) each nitrogen has two nonbonding
electron pairs
E) each hydrogen has one nonbonding
electron pair
Answers: cddcb bbacc ceaac
