Unit
Theme
Day
1
Date
2/20
Unit 4: Bonding
Chm.1.2: Understand the bonding that occurs in simple compounds in terms of bond type, strength, and properties.
Chm.1.2.1: Compare (qualitatively) the relative strengths of ionic, covalent, and metallic bonds.
Chm.1.2.2: Infer the type of bond and chemical formula formed between atoms.
Chm.1.2.3: Compare inter- and intra- particle forces.
Chm.1.2.5: Compare the properties of ionic, covalent, metallic, and network compounds
Standard(s)
Student Friendly Topic
Example/Rigor
Chm.1.2.1
Which statement describes the
 Identify the type of bond
compound formed between
 Describe metallic bonds: “metal ions
between two atoms
sodium and oxygen?
plus ‘sea’ of mobile electrons”

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a. It is NaO2, which is ionic.
b. It is NaO2, which is covalent.
c. It is Na2O, which is ionic.
d. It is Na2O, which is covalent.
Chm.1.2.2
Determine that a bond is
predominately ionic by the location of
the atoms on the Periodic Table
(metals combined with nonmetals) or
when EN > 1.7.
 Determine that a bond is
predominately covalent by the
location of the atoms on the Periodic
Table (nonmetals combined with
nonmetals) or when EN < 1.7.
Chm.1.2.2
 Predict chemical formulas of
compounds using Lewis structures.
Chm.1.2.5
 Apply Valence Shell Electron Pair
Repulsion Theory (VSEPR) for these
electron pair geometries and
molecular geometries, and bond
angles - Electron pair - Molecular
(bond angle); Linear framework –
linear; Trigonal planar framework–
trigonal planar, bent; Tetrahedral
framework– tetrahedral, trigonal
pyramidal, bent; Bond angles (include
distorting effect of lone pair electrons
– no specific angles, conceptually only)

Draw ionic Lewis and covalent
Lewis structures
Draw the Lewis structure of MgCl2.

Predict the shape of a molecule
based on VSEPR theory
The shape of CO2 is best described
as ___________.
4
5
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Chm.1.2.3
 Explain why intermolecular forces are
weaker than ionic, covalent or metallic
bonds
 Explain why hydrogen bonds are
stronger than dipole-dipole forces
which are stronger than dispersion
forces
 Apply the relationship between bond
energy and length of single, double,
and triple bonds (conceptual, no
numbers).
 Describe intermolecular forces for
molecular compounds.
 H-bond as attraction between
molecules when H is bonded to O, N,
or F. Dipole-dipole attractions
between polar molecules.
 London dispersion forces (electrons of
one molecule attracted to nucleus of
another molecule) – i.e. liquefied inert
gases.
 Relative strengths
(H>dipole>London/van der Waals).
Chm.1.2.5
 Explain how ionic bonding in
compounds determines their
characteristics: high MP, high BP,
brittle, and high electrical conductivity
either in molten state or in aqueous
solution.
 Explain how covalent bonding in
compounds determines their
characteristics: low MP, low BP, poor
electrical conductivity, polar nature,
etc.
 Explain how metallic bonding
determines the characteristics of
metals: high MP, high BP, high


Define intermolecular forces.
Identify the intermolecular forces
between 2 molecules
At STP, fluorine is a gas and iodine
is a solid. Why?
a. Fluorine has lower average
kinetic energy than iodine.
b. Fluorine has higher average
kinetic energy than iodine.
c. Fluorine has weaker
intermolecular forces of
attraction than iodine.
d. Fluorine has stronger
intermolecular forces of attraction
than iodine.

Predict the properties of a
substance.
An unknown substance is tested in
the laboratory. The physical test
results are listed below.
 Nonconductor of
electricity
 Insoluble in water
 Soluble in oil
 Low melting point

Based on these results, what is the
unknown substance?
a. ionic and polar.
b. ionic and nonpolar.
c. covalent and polar.
d. covalent and nonpolar.


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7
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3/2
conductivity, malleability, ductility,
and luster.
Describe bond polarity. Polar/nonpolar
molecules (relate to symmetry) ; relate
polarity to solubility—“like dissolves
like”
Describe macromolecules and network
solids: water (ice), graphite/diamond,
polymers (PVC, nylon), proteins (hair,
DNA) intermolecular structure as a
class of molecules with unique
properties.
Cumulative Activity / Unit Wrap-Up / Lab
Unit Test