JKKENNON
Chemistry I Chapter 6 Outline
CHEMICAL BONDING
In nature, most atoms are joined to other atoms by chemical bonds.
For graded assessments, you will need to be familiar with the following terms: chemical bond,
ionic bonding, covalent bonding, non-polar covalent bonding, polar, polar-covalent bonding, molecule,
molecular compound, chemical formula, molecular formula, bond energy, electron-dot notation, Lewis
structures, structural formula, single bond, multiple bonds, resonance, ionic compound, formula unit,
lattice energy, polyatomic ion, metallic bonding, malleability, ductility, enthalpy of vaporization,
VSEPR theory, hybridization, hybrid orbitals, dipole, hydrogen bonding, and London dispersion
forces.
I.
INTRODUCTION TO CHEMICAL BONDING
A. Atoms seldom exist as ______________________ in nature. This is because independent
atoms are at relatively high __________________ but we know that nature favors
__________ energy states meaning they are less stable when existing ____________ and
more stable existing in ________________. What part of the atom is redistributed during a
chemical bond? ________________ Main group metals tend to __________ electrons and
form _____________ while non-metals tend to _________ electrons and form
___________. Chemical bonding that involves a charge difference between two atoms is
called _______________ and bonding that involves the sharing of electrons is
called__________________. Briefly explain how electrons are involved in both of these
types of chemical
bonds._________________________________________________________. Bonding is
rarely purely covalent or purely ionic. The degree to which bonding between atoms of two
elements is ionic or covalent can be estimated by calculating differences in
______________________. If there is a higher difference in electronegativity between the
atoms of two elements in a chemical bond, that bond is said to be ______________. If
there is a moderate difference between the atoms of two elements in a chemical bond, that
bond is said to be _________________. If there is little or no difference between the
atoms of two elements in a chemical bond, that bond is said to be
______________________, If a molecule or compound is polar, what does this mean?
__________________________________________________. How do you calculate
electronegativity differences? ___________________________________________. How
do you determine whether the bond is ionic, polar-covalent or non-polar
covalent?_________________________________________________________
(STANDARD CLE-3221.3.1)
II.
COVALENT BONDING AND MOLECULAR COMPOUNDS
A. What is a diatomic molecule?____________________________________. Most atoms
__________ potential energies when they are bonded to other atoms as opposed to
existing __________________. Review Figure 6 on page 179 and describe the attractive
and repulsive forces that exist not only in the illustrated example but also in and between
all atoms.
__________________________________________________________________
What determines the relative strength of attraction and repulsion between two or more
charged particles? __________________________________________________________________________
JKKENNON
B. What term is used to describe the average distance between two bonded atoms?
_________________________ When covalent bonds are formed, _______________ is released. Why
is this? ________________________________________________________ What term is used to describe the
energy required to break a chemical bond and form neutral isolated atoms? ______________________
Refer to Table 1 on page 182 and describe the relationship or the proportionality between
bond length and bond energy. ___________________________________________________ Do all atoms “obey”
the octet rule? If not, give an example of a compound that is formed in nature that “violates”
the octet rule. Refer to Figure 10 on page 184 and then cross-reference a periodic table. What
trend do you notice occurs as one moves across a period (left to right)? __________________________
What is an electron-dot notation?
____________________________________________________________________________________________________________
What is a Lewis structure?
_____________________________________________________________________________________________________________
How many electrons are involved in a single covalent bond?__________ How many electrons are
involved in a double covalent bond? ___________ In a triple covalent bond? _______________ Which of
the three types of multiple bonds have greatest bond energies? ________________ What term is
used to describe a bond where molecular bonding cannot be correctly represented by a single
Lewis structure?_________________________________________
(STANDARD CLE-3221.3.1)
III.
IONIC BONDING AND IONIC COMPOUNDS
A. Most ionic compounds exist as ______________________________. A crystal is a 3-D network of
_______________ and _____________ ions mutually attracted to each other. Unlike molecular
compounds, ionic compounds do not exist as independent
_______________________________ that can
be isolated and examined. A
______________________ of an ionic compound shows the ratio of the ions present in a sample of any
size. What type of ratio exists in a unit of sodium chloride? Of calcium
fluoride?______________________________________________________In ionic crystals, ions minimize their
potential energies by combining in an ________________________________________ known as
____________________. What is lattice energy?
_________________________________________________________________________________________________________
Refer to Table 3 on page 193 and identify which compound contains the most negative (or the
greatest) lattice energy of the compounds listed. _________________________ What are polyatomic
ions? ________________________________________________________________________________________________ and
give two examples of polyatomic ions listed in your text. __________________________________
(STANDARD 93221.3.2)
IV.
METALLIC BONDING
A. Why are metals excellent conductors of electricity? ___________________________________________ What
is electricity? _____________________________________ In metals, overlapping orbitals provide several
‘spaces’ for orbiting valence electrons around a metallic compound. This type of electron
behavior is known as the _______________________________________. Why do metals reflect and absorb
light the way they do, in other words, why are they generally
lustrous?_______________________________________________________________________________ Metals are both
ductile and malleable because ___________________________________________________________. Metallic
bond strength varies with the _______________________________ of the metal atoms and the
________________________________ in the metal’s ________________________________. These two factors are
reflected by a metal’s ______________________________________________. Explain, briefly, why enthalpy
JKKENNON
of vaporization can be used to measure the strength of a metallic bond.
_____________________________________________________________________________________________________________
____________. Of the elements listed on Table 4, page 196, which element do you expect requires
the most energy to vaporize a sample of substance? ______________________
(STANDARD CLE-3221.3.1)
V.
MOLECULAR GEOMETRY
A. Molecular properties not only depend on bonding atoms but also
on_______________________________. Molecular polarity influences the forces that act
________________________________ in liquids and solids. What are the two theories that have been
developed to successfully determine the shapes of molecules? _________________________ &
______________________.
B. What does the acronym VSEPR stand for?
_________________________________________________________________________________________. The VSEPR
theory states that repulsion between the sets of ______________________________ surrounding an
atom causes these sets to be oriented ______________________________ possible. Refer to your
textbook on page 197 and show the Lewis dot structure formed between the atoms of
Beryllium Fluoride, BeF2.
What is the geometry of this molecule? ________________________________________ Now lets consider
Boron trifluoride, BF3. Show the Lewis dot structure of this molecule. Then tell what geometry
this molecule represents.
Now consider the molecule methane, CH4. Draw the Lewis dot structure for this molecule and
then indicate this molecule’s geometry.
What do the bond angles measure in a linear molecule?______________ In a trigonal planar
molecule?_______________ In a tetrahedral molecule?__________________ A molecule of ammonia has
one set of __________________ and the bond angles in this type of molecule measures
_________________. A molecule of water has ____________ sets of unshared electron pairs and the
bond angles in this type of molecule measures ______________. These two molecules are not
perfect tetrahedral molecules, therefore they do not perfectly each measure _____________. The
reason for this is because unshared electron pairs repel electrons _______________________ than do
bonding electron pairs. Give an example of an octahedral molecule ______________________________.
C. The other theory used to describe molecular geometry is _______________________. It is used to
describe the orbitals of an atom once arranged in a ___________________________. During
hybridization, commonly, the ______ and the ______ orbitals overlap to form an
________________________ orbital. What are hybrid orbitals?
__________________________________________________________________________________________________________.
Review Table 6 on page 203 and memorize the types of hybridization that correspond to
each type of geometry listed.
D. As liquid is heated, the ___________________________ of its particles increases. At boiling point,
energy is ____________________ to _____________________ forces of attraction between the
liquid’s
particles. Once the substance enters the gas phase, the particles have
________________________________________. Therefore,
__________________________ is a good measure of
the force of attraction between the
JKKENNON
particles in a liquid. The higher the ______________________ the
stronger the attractive
forces are between the molecules. What are forces of attraction
between
molecules called? ______________________________ Are all intermolecular forces the same
for all molecules? _____________ Why or why not?
__________________________________________________________________________________________________________
Referring to Table 7 on page 204, what types of substances have the highest boiling points?
_________________________ and the lowest? ________________________________________
E. The strongest intermolecular forces exist between ______________________________. What creates a
dipole? _____________________________________________________________ Sketch how dipoles are written
when studying a molecules polarity to determine chemical behavior in a system.
Of the four molecules, which 2 are polar and which 2 are nonpolar? Water, H2O; ammonia,
NH3; carbon tetrachloride, CCl4; and carbon dioxide, CO2. Sketch below the dipole moments of
each molecule listed and indicate why each are polar or nonpolar. What periodic trend that
was studied during chapter 5 determines the polarity of a molecule? _________________________
Hydrogen bonding generally occurs between what four molecules?
__________________________________________________________________________________________________________ Besides the
obvious, electronegativity, why does hydrogen bonding occur? What is going on with the
molecular geometry in a molecule that is capable of hydrogen bonding?
What are London dispersion forces?
_________________________________________________________________________________________________________________________
Below, use Figure 29 on page 207 to sketch a diagram of what occurs during a set of
molecules undergoing the effects of London dispersion forces.
London forces are the only intermolecular forces that act on __________________and on
_________________________________. London forces increase with increasing
______________________________________.
(STANDARD CLE-3221.3.1)