Name: ______________________
1) ____ Which formula represents a nonpolar molecule?
a)
b)
c)
d)
2)
____ The compound XCl is classified as ionic if X represents the element
a)
b)
c)
d)
3)
chlorine
fluorine
hydrogen
nitrogen
____ What is the empirical formula for a compound with the molecular formula C6H12Cl2O2?
a)
b)
c)
d)
6)
ionic, only
metallic, only
both covalent and ionic
both covalent and metallic
____ Which element is composed of molecules that each contain a multiple covalent bond?
a)
b)
c)
d)
5)
H
I
Rb
Br
____ The chemical bonding in sodium phosphate, Na3PO4, is classified as
a)
b)
c)
d)
4)
CH4
HCl
H2O
NH3
CHClO
CH2ClO
C3H6ClO
C6H12Cl2O2
____ Which two particle diagrams represent mixtures of
diatomic elements?
a) A and B
b) A and C
c) B and C
d) B and D
7)
____ Which statement describes oxygen gas, O2(g), and ozone gas, O3(g)?
a)
b)
c)
d)
8)
____ Which type of substance can conduct electricity in the liquid phase but not in the solid phase?
a)
b)
c)
d)
9)
They have different molecular structures, only.
They have different properties, only.
They have different molecular structures and different properties.
They have the same molecular structure and the same properties.
ionic compound
molecular compound
metallic element
nonmetallic element
____ Why is a molecule of CO2 nonpolar even though the bonds between the carbon atom and the oxygen atoms are polar?
a)
b)
c)
d)
The shape of the CO2 molecule is symmetrical.
The shape of the CO2 molecule is asymmetrical.
The CO2 molecule has a deficiency of electrons.
The CO2 molecule has an excess of electrons.
Regents Review _ Bonding
1-3
Created: February 2010
Name: ______________________
10) ____ Which formula represents a molecular compound?
a)
b)
c)
d)
11)
____ The relatively high boiling point of water is due to water having
a)
b)
c)
d)
12)
HI
KI
KCl
LiCl
hydrogen bonding
metallic bonding
nonpolar covalent bonding
strong ionic bonding
____ A compound has the empirical formula CH2O and a gram-formula mass of 60. grams per mole. What is the
molecular formula of this compound?
13)
____ Which formula represents strontium phosphate?
a)
b)
c)
d)
SrPO4
Sr3PO8
Sr2(PO4)3
Sr3(PO4)
14)
____ Which Lewis electron-dot diagram represents calcium oxide?
15)
____ Which formula represents a nonpolar molecule?
a)
b)
c)
d)
16)
____ Which element has an atom with the greatest tendency to attract electrons in a chemical bond?
a)
b)
c)
d)
17)
one pair of electrons
one pair of protons
three pairs of electrons
three pairs of protons
____ An ionic compound is formed when there is a reaction between the elements
a)
b)
c)
d)
19)
carbon
chlorine
silicon
sulfur
____ The nitrogen atoms in a molecule of N2 share a total of
a)
b)
c)
d)
18)
HCl
H2O
NH3
CH4
strontium and chlorine
hydrogen and chlorine
nitrogen and oxygen
sulfur and oxygen
____ Which compound has both ionic and covalent bonding?
a)
b)
c)
d)
CaCO3
CH2Cl2
CH3OH
C6H12O6
Regents Review _ Bonding
2-3
Created: February 2010
Name: ______________________
20) ____ The liquids hexane and water are placed in a test tube. The test tube is stoppered, shaken, and placed in a test tube rack.
The liquids separate into two distinct layers because hexane and water have different
a) formula masses
b) molecular polarities
c) pH values
d) specific heats
21) ____ Hydrogen bonding is a type of
a) strong covalent bond
b) weak ionic bond
c) strong intermolecular force
d) weak intermolecular force
22) ____ Which formula represents copper(I) oxide?
a) CuO
b) CuO2
c) Cu2O
d) Cu2O2
23) ____ Which element, represented by X, reacts with fluorine to produce the compound XF2?
a) aluminum
b) argon
c) magnesium
d) sodium
Base your answers to questions 24 through 26 on the information below.
At STP, iodine, I2, is a crystal, and fluorine, F2, is a gas. Iodine is soluble in ethanol, forming a tincture of iodine. A typical
tincture of iodine is 2% iodine by mass.
24) Compare the strength of the intermolecular forces in a sample of I2 at STP to the strength of the intermolecular forces
in a sample of F2 at STP.
25) In the space provided, draw a Lewis electron-dot diagram for a molecule of I2.
25)
26) Determine the total mass of I2 in 25 grams of this typical tincture of iodine.
26)
Base your answers to questions 27 through 29 on the information below.
Carbon has three naturally occurring isotopes, C-12, C-13, and C-14. Diamond and graphite are familiar forms of solid
carbon. Diamond is one of the hardest substances known, while graphite is a very soft substance. Diamond has a rigid
network of bonded atoms. Graphite has atoms bonded in thin layers that are held together by weak forces. Recent
experiments have produced new forms of solid carbon called fullerenes. One fullerene, C60, is a spherical, cagelike
molecule of carbon.
27) Determine both the total number of protons and the total number of neutrons in an atom of the naturally occurring
carbon isotope with the largest mass number.
Neutrons: _______________
Protons _______________
28) Identify the type of bonding in a fullerene molecule. ______________________
29) State, in terms of the arrangement of atoms, the difference in hardness between diamond and graphite.
Regents Review _ Bonding
3-3
Created: February 2010