Covalent Bonding
Practice Test
1.
What is the formula for the binary compound of potassium and chlorine?
Binary Molecular Compound
Binary Acid
Contains only two different elements
Contains hydrogen and one other element
Second element uses name + -ide
Uses hydro + root of second element + -ic and acid
a.
KCl
2
b.
K
2
ClO
3
c.
KHCl
d.
KCl
2.
A binary compound is a ___________.
a.
compound made of three types of atoms
b.
compound made of one type of atom
c.
compound made of two types of atoms
d.
compound made of polyatomic ions
3.
Which of these is the electron configuration of an atom most likely to lose an electron?
a.
[He]2s
2
2p
5
b.
1s
2
2s
2
2p
6
3s
2
3p
6
4s
1
c.
1s
2
2s
2
2p
6
d.
1s
2
2s
2
2p
6
3s
2
3p
5
4.
Which of the following atoms will be an exception to the octet rule in a molecule?
a.
C
b.
N
c.
B
d.
O
5.
_____________ is the force that holds two atoms together.
a.
A chemical bond
b.
Nuclear force
c.
Glue
d.
Fission
6.
Sulfate (SO
4
2-
) is a ____________.
a.
monatomic anion
b.
polyatomic cation
c.
monatomic cation
d.
polyatomic anion
7.
If tungsten were not available for use in a lightbulb filament, which of the elements in the table would be the best choice for a substitute?
Melting Points and Boiling Points of Some Metals
Element
Melting point (°C)
Boiling point (°C)
Lithium
180
1347
Tin
232
2623
Aluminum
660
2467
Barium
727
1850
Silver
961
2155
Copper
1083
2570
a.
aluminum
b.
copper
c.
lithium
d.
barium
8.
An ionic compound that will conduct an electric current when it forms an aqueous solution is a(n) _________.
a.
crystal lattice
b.
nonelectrolyte
c.
electrolyte
d.
molecular compound
9.
When two or more atoms join together by sharing their outermost electrons, ________.
a.
an ionic compound is formed
b.
a molecular compound is formed
c.
a mixture is formed
d.
a solution is formed
10.
Atoms with large ionization energy values are __________.
a.
lacking valence electrons
b.
more likely to form positive ions
c.
most likely to lose their outer electrons
d.
less likely to form positive ions
11.
Name the pair that contains an incorrect formula.
a.
magnesium hydroxide Mg(OH)
2
b.
iron(II) sulfite FeSO
3
c.
silver carbonate AgCO
3
d.
aluminum phosphate AlPO
4
12.
Which of the following have the same number of electrons? Cl
–
, O
2–
, F, Ca
2+
, Fe
3+
a.
O
2–
and F
b.
Ca
2+
and Cl
–
c.
Ca
2+
and Fe
3+
d.
F and Cl
–
13.
Which of the following is a correct description of a metallic property?
a.
Metals are malleable.
b.
Metals gain electrons to form anions.
c.
Metals have a dull appearance.
d.
Metals are brittle.
14.
How many sigma and how many pi bonds are present in the ethene molecule (C
2
H
4
)?
a.
4 sigma and 2 pi
b.
5 sigma and 2 pi
c.
4 sigma and 1 pi
d.
5 sigma and 1 pi
15.
Large differences in electronegativity result in __________ bonding between atoms.
a.
covalent
b.
no
c.
ionic
d.
polar
16.
Many simple molecules contain two lone pairs around the central atom. Which type of electron—to—electron repulsions are smallest in these molecules?
a.
lone pair to lone pair
b.
bonding pair to lone pair
c.
All repulsions are equal.
d.
bonding pair to bonding pair
17.
How are ionic bonds formed?
a.
loss of electrons by atoms
b.
gain of electrons by atoms
c.
electrostatic forces between ions
d.
sharing of electrons between atoms
18.
Which element has the highest electronegativity?
a.
Ne
b.
N
c.
F
d.
O
19.
When a hydrogen atom is part of a molecular structure, it is always a ________ atom.
a.
ionic
b.
central
c.
1
–
d.
terminal
20.
What hybridization is present in an octahedral molecular geometry?
a.
sp
2
b.
sp
3d
c.
sp
3
d.
sp
3
d
2
