This document defines molecular compounds and provides examples. It discusses that molecular compounds are composed of non-metal elements that are chemically bonded through covalent bonds where atoms share electron pairs. Examples of common molecular compounds are given such as gases, hydrocarbons, alcohols, carbohydrates, and biological molecules. Methods for drawing and naming molecular compounds such as Lewis dot diagrams and structural formulas are also outlined.
460 BC - Greek philosopher proposes the existence of the atom
He pounded materials until he made them into smaller and smaller parts
He called them atoma which is Greek for “indivisible”.
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He pounded materials until he made them into smaller and smaller parts
He called them atoma which is Greek for “indivisible”.
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5. Examples of Molecular Compounds
Hydrocarbons: methane (CH4), propane (C3H8),
butane (C4H10), octane (C8H18)
Propane gas explosion aftermath in Flor
(July 30, 2013) http://blogs.ft.com/photo-
diary/tag/propane-tanks/
Firefighters walk among thousands of
exploded propane cylinders that litter
the storage yard of a propane plant
after massive explosions overnight in
the plant’s yard, in Tavares, Florida.
Dozens of explosions rocked the
propane tank servicing plant
northwest of Orlando, late on
Monday, injuring seven workers, at
least three critically, and prompting
the evacuation of nearby homes,
authorities said.
8. Examples of Molecular Compounds
Most biological molecules:
enzymes, proteins, fats,
DNA
9. Examples of Molecular Compounds
Most things that you eat: chocolate, caffeine,
Tylenol
10. Properties of Molecular Compounds
soft
low melting point
solutions do not
conduct electricity
11. Molecular Compound
A molecular compound
(or molecule) is a
combination of two or
more atoms held
together by covalent
bonds
12. Covalent Bonds
occurs between the
atoms of non-metals
two atoms share a
pair of electrons
each bond represents
a single pair of shared
electrons
13. Covalent Bonds
Electrons are shared so that the
valence shell for each atom can be full.
For example: water
Hydrogen has 1 valence electron, need 1
more to be full (first shell)
Oxygen has 6 valence electron, need 2
more to be full
Each hydrogen atom shares one pair of
electrons with an oxygen atom
Each hydrogen atom now has 2 electrons
The oxygen now has 8 electrons in its
valence shell
15. Molecular Elements
When two or more
atoms of the same
element combine
A diatomic molecule is
a molecule that
naturally exists as two
of the same atoms
17. Molecular Compounds
When atoms of two or
more different non-metals
combine
Binary compounds consists
of only 2 types of non-
metals
18. Naming Binary Molecular Compounds
For compounds that do
not contain hydrogen:
Name the first element
Name the second
element and change
the ending to “-ide”
add prefixes to indicate
the number of each
atom
19. Naming Binary Molecular Compounds
The prefix “mono” is
not used when there is
only one atom of the
first element
When “mono” is being
added to oxygen, the
last “o” is dropped
Example: “monoxide”
not “monooxide”
20. Naming Binary Molecular Compounds
Example 1: N2O
Name the first element:
nitrogen
Name the second element
using “-ide”: oxide
Add prefixes:
dinitrogen monoxide
21. Naming Binary Molecular Compounds
Example 2: PBr3
Name the first
element: phosphorous
Name the second
element using “-ide”:
bromide
Add prefixes:
phosphorous
tribromide
22. Naming Molecular Compounds
Hydrogen is unique in
many ways, and this is
reflected in the naming
systems
Many compounds
containing hydrogen
have been given simpler
names
For example, dihydrogen
monoxide (H2O) is
simply called “water”
26. Lewis Dot Diagram
Recall: only valence electrons are shown
only UNPAIRED electrons can be shared
Arrangements of electrons around the element
name must take on the same orientation as if there
was an imaginary orbital ring around the atoms
WRONG WAY RIGHT WAY
H ..
H or H H : H or H
: ..
H H
27. Lewis Dot Diagram
Recall: only valence electrons are shown
only UNPAIRED electrons can be shared
Arrangements of electrons around the element
name must take on the same orientation as if there
was an imaginary orbital ring around the atoms
Practice: Draw the Lewis Dot Diagram for CH4
28. Lone Pairs
Pairs of electrons that are NOT shared
Exists as part of ONE atom
Practice:
Draw the Lewis Dot diagram for H2O and NH3
Which atom in each molecule has lone pairs?
29. Lewis Dot Diagram
Sometimes atoms share more than one
unpaired electron
When this happens you get a double or triple
bond
Example: Draw the Lewis Dot diagram for
CO2
31. Drawing Molecular Compounds
Lewis diagrams can be quite time consuming
and is difficult to read and thus most
textbooks use alternate forms of
representation:
Structural diagrams
Line diagrams
32. Structural Diagram
Each pair of shared electrons (2 electrons) is
replaced with a single line segment
connecting the two atoms
Each single line represents a bond
If two atoms share 4 electrons (2 pairs), then
you would use 2 line segments (like an equal
sign) representing double bonds
Lone pairs of electrons are NOT shown
