Name: 
 

Enriched Chemistry Chapter 6 Test



Multiple Choice
Identify the choice that best completes the statement or answers the question.
 

 1. 

Bonding in molecules or ions that cannot be correctly represented by a single Lewis structure is
a.
polyatomic.
c.
single bonding.
b.
resonance.
d.
double bonding.
 

 2. 

A polar molecule contains
a.
ions.
b.
a region of positive charge and a region of negative charge.
c.
only London forces.
d.
no bonds.
 

 3. 

The electrostatic attraction between positively charged nuclei and negatively charged electrons permits two atoms to be held together by a(n)
a.
chemical bond.
c.
neutron.
b.
London force.
d.
ion.
 

 4. 

Atoms naturally move
a.
toward high potential energy.
c.
toward less stability.
b.
toward low potential energy.
d.
away from each other.
 

 5. 

If two covalently bonded atoms are identical, the bond is
a.
nonpolar covalent.
c.
dipole covalent.
b.
polar covalent.
d.
coordinate covalent.
 

 6. 

Most chemical bonds are
a.
purely ionic.
c.
partly ionic and partly covalent.
b.
purely covalent.
d.
metallic.
 

 7. 

Nonpolar covalent bonds are not common because
a.
one atom usually attracts electrons more strongly than the other.
b.
ions always form when atoms join.
c.
the electrons usually remain equally distant from both atoms.
d.
dipoles are rare in nature.
 

 8. 

The pair of elements that forms a bond with the least ionic character is
a.
Na and Cl.
c.
O and Cl.
b.
K and Cl.
d.
Mg and Cl.
 

 9. 

In the three molecules, O2, HCl, and F2, what atom would have a partial negative charge?
a.
oxygen
c.
chlorine
b.
hydrogen
d.
fluorine
 

 10. 

Which of the following shows the types and numbers of atoms joined in a single molecule of a molecular compound?
a.
molecular formula
c.
covalent bond
b.
potential energy diagram
d.
ionic bond
 

 11. 

In drawing a Lewis structure, the central atom is generally the
a.
atom with the greatest mass.
b.
atom with the highest atomic number.
c.
atom with the fewest electrons.
d.
least electronegative atom.
 

 12. 

After drawing a Lewis structure, one should
a.
determine the number of each type of atom in the molecule.
b.
add unshared pairs of electrons around nonmetal atoms.
c.
confirm that the total number of valence electrons used equals the number available.
d.
determine the electronegativity of each atom.
 

 13. 

The substance whose Lewis structure shows three covalent bonds is
a.
H2O.
c.
NH3.
b.
CH2Cl2.
d.
CCl4.
 

 14. 

The chemical formula for an ionic compound represents the
a.
number of atoms in each molecule.
b.
number of ions in each molecule.
c.
ratio of the combined ions present in a sample.
d.
total number of ions in the crystal lattice.
 

 15. 

The chemical formula for water, a covalent compound, is H2O. This formula is an example of a(n)
a.
formula unit.
c.
ionic formula.
b.
Lewis structure.
d.
molecular formula.
 

 16. 

In an ionic compound, the orderly arrangement of ions in a crystal is the state of
a.
maximum potential energy.
c.
average potential energy.
b.
minimum potential energy.
d.
zero potential energy.
 

 17. 

Ionic compounds are brittle because the strong attractive forces
a.
allow the layers to shift easily.
b.
cause the compound to vaporize easily.
c.
keep the surface dull.
d.
hold the layers in relatively fixed positions.
 

 18. 

The Lewis structure for the ammonium ion, NH4, has
a.
nonpolar covalent bond.
c.
polar covalent bond.
b.
ionic bond.
d.
metallic bond.
 

 19. 

How many extra electrons are in the Lewis structure of the phosphate ion, PO43–?
a.
0
c.
3
b.
2
d.
4
 

 20. 

The shiny appearance of a metal is most closely related to the metal's
a.
highly mobile valence electrons.
c.
brittle crystalline structure.
b.
covalent bonds.
d.
positive ions.
 

 21. 

As light strikes the surface of a metal, the electrons in the electron sea
a.
allow the light to pass through.
b.
become attached to particular positive ions.
c.
fall to lower energy levels.
d.
absorb and re-emit the light.
 

 22. 

Metals are malleable because the metallic bonding
a.
holds the layers of ions in rigid positions.
b.
maximizes the repulsive forces within the metal.
c.
allows one plane of ions to slide past another.
d.
is easily broken.
 

 23. 

According to VSEPR theory, an AB2 molecule is
a.
trigonal-planar.
c.
linear.
b.
tetrahedral.
d.
octahedral.
 



 
Check Your Work     Start Over