WorksheetsChemical Bonding Test
Total questions: 31
Worksheet time: 16mins
Name
Class
Date
1.
How many valence electrons are in an atom of phosphorus?
a)
2
b)
3
c)
4
d)
5
2.
How many valence electrons are in an atom of magnesium?
a)
b.
b)
3
c)
d.
d)
5
3.
How many valence electrons does a helium atom have?
a)
2
b)
3
c)
4
d)
5
4.
How many valence electrons are in a silicon atom?
a)
2
b)
4
c)
6
d)
8
5.
What is the name given to the electrons in the highest occupied energy level of an atom?
a)
orbital electrons
b)
valence electrons
c)
anions
d)
cations
6.
How does calcium obey the octet rule when reacting to form compounds?
a)
It gains electrons.
b)
It gives up electrons.
c)
It does not change its number of electrons.
d)
Calcium does not obey the octet rule.
7.
Which of the following elements forms an ion with a 1– charge?
a)
fluorine
b)
hydrogen
c)
potassium
d)
sodium
8.
How many electrons does nitrogen gain in order to achieve a noble-gas electron configuration?
a)
1
b)
2
c)
3
d)
4
9.
Which of the following occurs in an ionic bond?
a)
Oppositely charged ions attract.
b)
Two atoms share two electrons.
c)
Two atoms share more than two electrons.
d)
Like-charged ions attract.
10.
Which of the following is true about an ionic compound?
a)
The chemical formula shows the atoms in a molecule.
b)
The formula unit gives the number of each type of ions in a crystal.
c)
It is composed of anions and cations and yet it is electrically neutral.
d)
The chemical formula shows the ions in a molecule.
11.
How many valence electrons are transferred from the nitrogen atom to potassium in the formation of the compound potassium nitride?
a)
0
b)
1
c)
2
d)
3
12.
How many valence electrons are transferred from the calcium atom to iodine in the formation of the compound calcium iodide?
a)
0
b)
1
c)
2
d)
3
13.
Which of the following pairs of elements is most likely to form an ionic compound?
a)
magnesium and fluorine
b)
nitrogen and sulfur
c)
oxygen and chlorine
d)
sodium and aluminum
14.
Most ionic compounds
a)
are crystalline solids at room temperature.
b)
have low melting points.
c)
conduct an electric current in the solid state.
d)
are composed of nonmetallic elements.
15.
What is the basis of a metallic bond?
a)
the attraction of metal ions to mobile electrons
b)
the attraction between neutral metal atoms
c)
the neutralization of protons by electrons
d)
the attraction of oppositely charged ions
16.
What information does a molecular formula provide?
a)
the number and kind of atoms that are bonded by the transfer of electrons
b)
the simplest whole-number ratio of atoms that are bonded by the transfer of electrons
c)
information about a molecule's structure
d)
the number and kind of atoms present in a molecule
17.
What is shown by the structural formula of a molecule or polyatomic ion?
a)
the arrangement of bonded atoms
b)
the number of ionic bonds
c)
the number of metallic bonds
d)
the shapes of molecular orbitals
18.
Why do atoms share electrons in covalent bonds?
a)
to become ions and attract each other
b)
to attain a noble-gas electron configuration
c)
to become more polar
d)
to increase their atomic numbers
19.
Which elements can form diatomic molecules joined by a single covalent bond?
a)
hydrogen only
b)
halogens only
c)
halogens and members of the oxygen group only
d)
hydrogen and the halogens only
20.
What is the representative unit in a molecular compound?
a)
a molecule
b)
an ion
c)
a formula unit
d)
shared electrons
21.
Once formed, how are coordinate covalent bonds different from other covalent bonds?
a)
They are stronger.
b)
They are more ionic in character.
c)
They are weaker.
d)
There is no difference.
22.
Which of the following bonds is the least reactive?
a)
C—C
b)
H—H
c)
O—H
d)
H—Cl
23.
According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as possible?
a)
pairs of valence electrons
b)
inner shell electrons
c)
mobile electrons
d)
the electrons closest to the nuclei
24.
What causes water molecules to have a bent shape, according to VSEPR theory?
a)
repulsive forces between unshared pairs of electrons
b)
interaction between the fixed orbitals of the unshared pairs of oxygen
c)
ionic attraction and repulsion
d)
the unusual location of the free electrons
25.
Which of the following theories provides information concerning both molecular shape and molecular bonding?
a)
molecular orbital theory
b)
VSEPR theory
c)
orbital hybridization theory
d)
Bohr atomic theory
26.
Experimental evidence suggests that the H—C—H bond angles in ethene, C H , are ____.
a)
90
b)
109.5
c)
120
d)
180
27.
What is thought to cause the dispersion forces?
a)
attraction between ions
b)
motion of electrons
c)
sharing of electron pairs
d)
differences in electronegativity
28.
Which of the forces of molecular attraction is the weakest?
a)
dipole interaction
b)
dispersion
c)
hydrogen bond
d)
single covalent bond
29.
What causes dipole interactions?
a)
sharing of electron pairs
b)
attraction between polar molecules
c)
bonding of a covalently bonded hydrogen to an unshared electron pair
d)
attraction between ions
30.
What are the weakest attractions between molecules?
a)
ionic forces
b)
Van der Waals forces
c)
covalent forces
d)
hydrogen forces
31.
What causes hydrogen bonding?
a)
attraction between ions
b)
motion of electrons
c)
sharing of electron pairs
d)
bonding of a covalently bonded hydrogen atom with an unshared electron pair
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