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?