AKA: Covalent Compounds
Notes #13
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Many compounds DO NOT form by their
charges or transferring electrons.
Covalent/ Molecular Compounds:
◦ Joined by a covalent bond
◦ The SHARING of electrons
◦ Between two or more non-metals
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Molecule: any compound joined together by
only covalent bonds. Example: H2O molecule.
Diatomic Molecule: a molecule consisting of
TWO atoms. (Ex: N2, O2, F2, Cl2, Br2, I2)
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A compound composed of molecules is called
a molecular compound.
Molecular compounds have covalent bonds.
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Molecular compounds tend to have relatively
lower melting and boiling points than ionic
compounds.
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Ethane, a component of natural gas, is also a
molecular compound.
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A molecular formula shows how many atoms of each element a
molecule contains.
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In covalent bonds, electron sharing usually
occurs so that atoms attain the electron
configurations of noble gases.
Covalent Bonds: Electron sharing between neutral atoms to
form covalent bonds.
Examples: Let’s use electron dot diagrams to
show the electron sharing between H2, F2,
H2O, NH3
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A prefix in the name of a binary molecular compound tells
how many atoms of an element are present in each
molecule of the compound.
 1. Name the elements in the order listed in
the formula.
 2. Use prefixes to indicate the number of
each kind of atom.
 3. Omit the prefix mono- when the formula
contains only one atom of the first element
in the name.
 4. The suffix of the name of the second
element is -ide.
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1.
2.
3.
4.
Practice: Write the names of the following
molecular compounds.
Cl2O7
N2H4
BCl3
N2O3
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1.
2.
3.
4.
Practice: Write the formulas for the following
molecular compounds.
Carbon tetrabromide
Diphosporous trioxide
Iodine heptafluoride
Phosphorous pentachloride
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Compare and Contrast Ionic and Covalent
Compounds.
Organize your information into a table, chart
or diagram.
As a class, we will discuss your diagrams and
create a public record for you to study with.
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Complete on your own piece of paper.
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Write question AND answer
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Turn in for a grade