Transcript Chapter 8

Chapter 8 Review
“Covalent Bonding”
Chapter 8 Review
 What
is the correct electron
configuration arrangement of the
four valence electrons of the carbon
atom in a methane molecule (CH4):
a) 2s22p2, or b) 2s12p3?
 Which noble gas has the same
electron configuration as the oxygen
in a water molecule?
Chapter 8 Review
 When
placed between oppositely
charged metal plates, the region of
a water molecule attracted to the
negative plate is the ____.
 When one atom contributes both
bonding electrons in a single
covalent bond, the bond is called
a(n) ____.
Chapter 8 Review
The shape of the methane molecule
(CH4) is called ____. What are the bond
angles?
 How is a pair of molecular orbitals
formed?
 Which elements can form diatomic
molecules joined by a single covalent
bond?
 What is a typical characteristic of an
ionic compound? Covalent?

Chapter 8 Review
 Experimental
evidence suggests
that the H-C-H bond angles in
ethene, C2H4, are ____
120 degrees.
 A bond that is not symmetrical along
the axis between two atomic nuclei
is a(n) ____ bond.
 Once formed, how are coordinate
covalent bonds different from other
covalent bonds?
Substances that show relatively
strong attractions to an external
magnetic field are said to be
____________?
 Oxygen is an example of a substance
that is ____________?

Chapter 8 Review
What causes hydrogen bonding?
 How many electrons can occupy a
single molecular orbital?
 According to the VSEPR theory,
molecules adjust their shapes to keep
____ as far apart as possible.
 Which of the following atoms acquires
the most negative charge in a covalent
bond with hydrogen: a) carbon, or
b) oxygen?

Chapter 8 Review
How do atoms achieve noble-gas
electron configurations in single covalent
bonds?
 What is required in order to melt a
network solid?
 Molecular orbital theory is based upon
what model of the atom?
 Where are the electrons most probably
located in a molecular bonding orbital?

Chapter 8 Review
A
molecule with a single covalent
bond is: a) CO2, or b) Cl2?
 A bond formed between a silicon
atom and an oxygen atom is likely to
be a(n) ____ bond.
 Which of the following diatomic
molecules is joined (seemingly) by a
double covalent bond: a) O2, or
b) N2?
Chapter 8 Review
 What
causes water molecules to
have a bent shape, according to the
VSEPR theory?
 Which of these elements does not
exist as a diatomic molecule: a) Ne,
or b) F?
 Which of the following elements can
form diatomic molecules held
together by triple covalent bonds:
a) fluorine, or b) nitrogen?
Chapter 8 Review
 Which
of the following covalent
bonds is the most polar:
a) H-F, or b) H-N?
 What is shown by the structural
formula of a molecule or a
polyatomic ion?
 What is thought to cause the
disperson forces?
Chapter 8 Review
 What are the weakest attractions
between molecules called?
 Which type of solid has the
highest melting point: a) ionic
solids, or b) network solids?
 Why do atoms share electrons in
covalent bonds?
Chapter 8 Review
 How
many valid electron dot
formulas – having the same number
of electron pairs for a molecule or
ion – can be written when a
resonance structure occurs?
Chapter 8 Review
 Which
of the forces of molecular
attraction is the weakest:
a) hydrogen bonding, or
b) dispersion forces?
 In which of the following compounds
is the octet expanded to include 12
electrons: a) PCl5, or b) SF6?
 Why is hydrogen bonding only
possible with hydrogen?
Chapter 8 Review
 What
causes dipole interactions?
 How many electrons does carbon
need to gain in order to obtain a
noble-gas electron configuration?
 How many covalent bonds are in a
covalently bonded molecule
containing 1 phosphorus atom and 3
chlorine atoms?
Chapter 8 Review
 How
many electrons does a
nitrogen atom need to gain in order
to attain a noble-gas electron
configuration?
 What is the bond angle in a water
molecule?
 How many unshared pairs of
electrons are in a molecule of
hydrogen iodide?
Chapter 8 Review
How many electrons are shared in a
single covalent bond?
 What is the total number of covalent
bonds normally associated with a single
carbon atom in a compound?
 How many valence electrons does an
iodine atom have?
 How many unshared pairs of electrons
does the nitrogen atom in ammonia
possess?

Chapter 8 Review
 How
many electrons are shared in a
double covalent bond?
 Know the shape/bond angles of the
following: CO2, H2O, CCl4, NH3,
SO3, PF5, SF6