Transcript Chapter 16
Chapter 16 – Review
“Covalent Bonding”
Milbank High School
Chapter 16 - Review
How
many electrons are shared in a
single covalent bond?
How many valence electrons does
an atom of any halogen have?
How many electrons are shared in a
double covalent bond?
How many electrons does a nitrogen
atom need to gain to attain a noblegas electron configuration?
Chapter 16 - Review
How
many unshared pairs of
electrons does the nitrogen atom in
ammonia (NH3) possess?
How many electrons does carbon
need to gain to obtain a noble-gas
electron configuration?
What is the total number of covalent
bonds normally associated with a
single carbon atom in a compound?
Chapter 16 - Review
How
many unshared pairs of
electrons are there in a molecule of
hydrogen iodide?
How many covalent bonds are there
in a covalently bonded molecule
containing 1 phosphorus atom and 3
chlorine atoms?
What is the name given to the
energy required to break a single
bond?
Chapter 16 - Review
How
do atoms achieve noble-gas
electron configurations in single
covalent bonds?
Why do atoms share electrons in
covalent bonds?
What is shown by the structural
formula of a molecule or polyatomic
ion?
Chapter 16 - Review
What
is the name given to the pairs
of valence electrons that do not
participate in bonding in diatomic
oxygen molecules?
Which elements can form diatomic
molecules joined by a single
covalent bond?
Which of these elements does not
exist as a diatomic molecule: I, Ne,
H, F
Chapter 16 - Review
What
elements can form diatomic
molecules held together by triple
covalent bonds?
What elements can form diatomic
molecules held together by double
covalent bonds?
A covalent bond in which each atom
contributes two electrons is a ___.
Chapter 16 - Review
A diatomic
molecule with a triple
covalent bond is _____.
A molecule with a single covalent
bond is: CO2 or Cl2?
Which noble gas has the same
electron configuration as the oxygen
in a water molecule?
Chapter 16 - Review
What
diatomic molecule is joined by
a double covalent bond?
When one atom contributes both
bonding electrons in a single
covalent bond, the bond is called
a(n) _______.
Once formed, how are coordinate
covalent bonds different from
normally formed covalent bonds?
Chapter 16 - Review
What
is true concerning the resonant
molecule dinitrogen tetraoxide (or
any resonant structure for that
matter!)?
When do exceptions to the octet rule
occur?
Substances in which all of the
electrons are paired are said to be
______.
Chapter 16 - Review
How
many unpaired electrons are
present in each molecule of a paramagnetic substance?
Which of the following types of
magnetism is the strongest:
paramagnetic; diamagnetic; or
ferromagnetic?
Which of the following fails to follow
the octet rule: fluorine or oxygen?
Chapter 16 - Review
In
which of the following compounds
is the octet expanded to include 12
electrons: SO3 or SCl6?
What is one way in which
compounds that do not follow the
octet rule can achieve stability?
Which of the following pairs of
elements can be joined by a covalent
bond: Mg and C; or N and C?
Chapter 16 - Review
What
type of covalent bond is most
stable between small atoms: polar or
nonpolar?
According to VSEPR theory,
molecules adjust their shapes to
keep what items as far apart as
possible?
Chapter 16 - Review
What
causes water molecules to
have a bent shape, according to
VSEPR theory?
What is the measure of the
tetrahedral bond angle?
What is the bond angle in a water
molecule?
What is thought to cause the
dispersion forces?
Chapter 16 - Review
Which
of the forces of molecular
attraction is the weakest?
What causes hydrogen-bonding?
Why is hydrogen-bonding only
possible with hydrogen?