WorksheetsChemical Bonding-2
Total questions: 25
Worksheet time: 24mins
Name
Class
Date
1.
A covalent bond consists of
a)
a shared electron
b)
two attractive ions
c)
shared electron pair
d)
octet of electrons
2.
Atoms with a strong attraction for electrons they share with another atom exhibit
a)
zero electronegativity
b)
low electronegativity
c)
high electronegativity
d)
negative electronegativity
3.
A bond in which there is unequal sharing of electrons is
a)
ionic
b)
polar covalent
c)
nonpolar covalent
d)
metallic
4.
If two covalently bonded atoms are identical, the bond is identified as
a)
nonpolar covalent
b)
ionic
c)
polar covalent
d)
coordinate covalent
5.
A chemical bond resulting from electrostatic attraction between positive and negative ions is a(n)
a)
nonpolar covalent
b)
ionic
c)
polar covalent
d)
coordinate covalent
6.
VSEPR is based on the assumption that
a)
positive ions repel each other
b)
positive ions attract negative ions
c)
sp2 hybridization occurs
d)
electrons in molecules repel each other
7.
Bond length is equivalent to the distance between nuclei at
a)
minimum potential energy
b)
zero potential energy
c)
maximum potential energy
d)
depends on the molecule
8.
In which of the following are electrons shared unequally?
a)
H2
b)
S8
c)
HCl
d)
Cl2
9.
The correct electron dot structure for an atom, X, which has the electron configuration 1s22s22p5 would have a symbol with ____ electrons around it.
a)
8 dots
b)
5 dots
c)
7 dots
d)
9 dots
10.
VSEPR accounts for the fact that
a)
all valence electrons must be involved in bonding
b)
the C-H bonds in CH4 all have bond angles of 109.5°
c)
the carbon atom has 4 bonding electrons
d)
no two bond angles in a molecule have the same measure
11.
Multiple bonding occurs with all of the following atoms except
a)
C
b)
F
c)
N
d)
O
12.
Metallic bonds occur when
a)
nonmetals bond with nonmetals
b)
metals bond with metals
c)
metals bond with nonmetals
d)
depends on the molecule
13.
Refer to the Potential Energy graph in your notes. At which point are there no significant forces between atoms?
a)
1
b)
2
c)
3
d)
4
14.
Refer to the Potential Energy graph in your notes. At which point are the repulsive forces stronger than the attractive forces?
a)
1
b)
2
c)
3
d)
4
15.
Refer to the Potential Energy graph in your notes. At which point are the atoms forming a chemical bond?
a)
1
b)
2
c)
3
d)
4
16.
The ability of an atom to pull electrons towards itself in a compound is...
a)
electron affinity
b)
electronegativity
c)
polarizability
d)
ionization energy
17.
When drawing Lewis structures, all elements follow the _____ rule (except H and He) in order to be the most stable.
a)
Octave Rule
b)
Duet Rule
c)
Triad Rule
d)
Octet Rule
18.
The electronegativity difference will be between ____ in a polar covalent bond.
a)
0.0-0.4
b)
1.7-3.9
c)
0.5-1.6
d)
4.0-10.0
19.
What is the bond angle in H2O?
a)
180°
b)
120°
c)
109.5°
d)
105°
20.
What is the bond angle in NH3?
a)
180°
b)
120°
c)
107°
d)
105°
21.
What is the bond angle in CH4?
a)
180°
b)
120°
c)
109.5°
d)
105°
22.
What is the VSEPR shape for BH3?
a)
Linear
b)
Trigonal Planar
c)
Trigonal Pyramidal
d)
Trigonal Bipyramidal
23.
What is the VSEPR shape for CO2?
a)
Linear
b)
Trigonal planar
c)
Bent
d)
Trigonal pyramidal
24.
What is the hybridization around the carbon atom in a molecule of CO2?
a)
sp1
b)
sp2
c)
sp3
d)
sp4
25.
What is the hybridization around the Boron in BH3?
a)
sp1
b)
sp2
c)
sp3
d)
sp4
100 %
