Name
1) Given the balanced equation representing
a reaction:
Which statement describes the changes
in energy and bonding for the reactant?
1) Energy is absorbed as bonds in H 2O
are formed.
2) Energy is absorbed as bonds in H 2
O are broken.
3) Energy is released as bonds in H2O
are formed.
4) Energy is released as bonds in H2O
are broken.
2) The elements Li and F combine to form
an ionic compound. The electron
configurations in this compound are the
same as the electron configurations of
atoms in Group
1) 1
2) 14
3) 17
4) 18
3) What is the most likely
electronegativity value for a metallic
element?
1) 1.3 2) 2.7 3) 3.4 4) 4.0
4) Based on electronegativity values, which
type of elements tends to have the
greatest attraction for electrons in a
bond?
1) metals
2) metalloids
3) nonmetals
4) noble gases
Bonding Review
5) Which bond is least polar?
1) As–Cl
2) Bi–Cl
3) P–Cl
4) N–Cl
6) Which compound has the least ionic
character?
1) KCl
2) CaCl2
3) AlCl 3
4) CCl 4
7) Which formulas represent one ionic
compound and one covalent compound?
1)
2)
3)
4)
8) A sample of a substance has these
characteristics:
• melting point of 984 K
• hard, brittle solid at room
temperature
• poor conductor of heat and electricity
as a solid
• good conductor of electricity as a
liquid on in an aqueous solution
This sample is classified as
1) a metallic element
2) a radioactive element
3) a molecular compound
4) an ionic compound
9) A molecular compound is formed when a
chemical reaction occurs between atoms
of
1) chlorine and sodium
2) chlorine and yttrium
3) oxygen and hydrogen
4) oxygen and magnesium
10) Which type of substance is soft, has a
low melting point, and is a poor
conductor of heat and electricity?
14) What is the chemical formula for
iron(III) oxide?
1) FeO
2) Fe 2 O 3
3) Fe 3O
4) Fe 3O2
15) Which is the formula for the compound
that forms when magnesium bonds with
phosphorus?
1) Mg2P
2) MgP2
3) Mg2P 3
4) Mg 3 P 2
16) What is the chemical name for H 2S?
1) network solid
2) molecular solid
1) dihydrogen sulfide
3) metallic solid
2) dihydrogen monosulfide
4) ionic solid
3) monohydrogen disulfide
11) Conductivity in a metal results from the
metal atoms having
1) high electronegativity
4) hydrogen sulfide
17) What is the name of the polyatomic ion
in the compound Na2O2?
2) high ionization energy
1) hydroxide
2) oxalate
3) highly mobile protons in the nucleus
3) oxide
4) peroxide
4) highly mobile electrons in the
valence shell
12) Which substance contains metallic
bonds?
18) A compound is made up of iron and
oxygen, only. The ratio of iron ions to
oxide ions is 2:3 in this compound. The
IUPAC name for this compound is
1) Hg( )
2) H 2O( )
1) triiron dioxide
3) NaCl(s)
4) C6H 12O6(s)
2) iron(II) oxide
13) Which formula represents strontium
phosphate?
1) SrPO4
2) Sr3PO 8
3) Sr2(PO4)3
4) Sr 3 (PO 4 ) 2
Bonding Review
3) iron(III) oxide
4) iron trioxide
19) Which formula represents a binary
compound?
1) Ne
2) Br2
3) C 3 H 8
4) H 2SO4
20) Draw a correct Lewis electron-dot structure for each of the following.
a An atom of hydrogen
b An atom of nitrogen
c A molecule of ammonia (NH 3)
Base your answers to questions 21 through 23 on the information below and on your
knowledge of chemistry.
The Lewis electron-dot diagrams for three substances are shown below.
21) Identify the noble gas that has atoms with the same electron configuration as
the positive ion represented in diagram 1, when both the atoms and the ion are in
the ground state.
22) Draw a Lewis electron-dot diagram for a molecule of
Bonding Review
.
23) Describe, in terms of valence electrons, how the chemical bonds form in the
substance represented in diagram 1.
24) Explain, in terms of element classification, why
is an ionic compound.
25) Base your answer to the following question on the information below.
In the space in your answer booklet, draw a Lewis electron-dot diagram for CF 4.
Bonding Review
26) Base your answer to the following
question on your knowledge of chemical
bonding and on the Lewis electron-dot
diagrams of H 2S, CO2, and F2 below.
Explain, in terms of electronegativity, why a
C–O bond in CO2 is more polar than the F–F
bond in F2.
27) Draw an electron-dot diagram for each of the following substances:
a calcium oxide (an ionic compound)
b hydrogen bromide
c carbon dioxide
Bonding Review
28) Base your answer to the following question on An unknown solid was tested and
showed the properties listed below:
Properties
high melting point
soluble in water
conductor of electricity when dissolved in water
non-conductor of electricity as a solid
hard surface
a State the type of bonding you would expect of this substance.
b Explain why this substance conducts electricity when dissolved in water.
c Explain why it is hard.
Bonding Review
Answer Key
Bonding Review
1)
2
2)
4
3)
1
4)
3
5)
4
6)
4
7)
3
8)
4
9)
3
10)
2
11)
4
12)
1
13)
4
14)
2
15)
4
16)
2
17)
4
18)
3
19)
3
20)
21)
argon and Ar
22)
27)
23)
—Valence electrons
are lost by
potassium and
gained by bromine.
—The ions form as
a result of a transfer
of electrons between
the atoms.
24)
—A metal reacts
with a nonmetal to
produce an ionic
compound.
—Potassium is a
metal and oxygen is
a nonmetal.
25)
26)
Responses include,
but are not limited
to: The
electronegativity
difference in a
carbon-oxygen bond
is greater than the
electronegativity
difference in a
fluorine-fluorine
bond The EN
difference for C and
O is 0.9 and the EN
difference for F and
F is 0.
28)
a) Ionic b) When
ionic substances
dissolve in water the
substance breaks
down into ions.
Ions, being charged
particles, can cause
a current to flow. c)
Ionic substances
attract each other
strongly because of
their opposite charge