Water
Fructose
Carbon Dioxide
Ammonia

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To get eight valence electrons
To become more stable
In ionic bonds, metals lose electrons and non-metals gain electrons.
What happens when both elements need electrons?

Molecules and Molecular Compounds
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Compounds that are NOT held together by an electrical attraction, but instead by a sharing of electrons.
Atoms held together by sharing electrons and filling the outer energy levels are joined by a covalent bond.
NONMETALS ONLY!! - No metals

Molecules and Molecular Compounds
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A molecule is a neutral group of atoms joined together covalent bonds. A compound composed of molecules is called a molecular compound .
The chemical formula for a molecule is called the molecular formula .
A chemical formula tells you how many atoms of each element one molecule of a compound contains.

Learning Check
Indicate whether a bond between the following would be 1) Ionic 2) covalent
A. sodium and oxygen
B. nitrogen and oxygen
C. phosphorus and chlorine
D. calcium and sulfur
E. chlorine and bromine

Atom
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Noble gases are monatomic.
They exist as single atoms and do not combine with any other elements.
Ex: He, Ne, Ar, Kr, Xe, Rn

7 Diatomic Molecules
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Some elements will covalently bond to themselves to form a molecule composed of TWO atoms.
Some elements occur as “diatomic” molecules in nature because they are more stable than individual atoms
The 7 diatomic elements are all gases :
H
2
, O
2
, N
2
, Cl
2
, Br
2
, I
2
, F
2

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Distance between two bonding nuclei at the position of maximum attracting is bond length
Bond length is determined by the size of the atoms and how many electron pairs are shared
Bond energy is the energy required to break a chemical bond and form neutral isolated atoms.

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Remember that all compounds want to attain the electron configuration of noble gases .
Hydrogen only needs 2 , the rest need 8 .
Regarding covalent bonds, electrons are shared between the atoms so that they attain the electron configuration of noble gases.

1)
A small group of molecules has an odd number of valence electrons and cannot form an octet around each atom
-Ex: NO
2
O
N O
2)
Fewer than eight electrons: BORON is stable with 6!
H - B - H
-
Ex: BH
3
H

3)
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Some central atoms have more than eight valence electrons
Referred to as an “ expanded ” octet
Explained by d-orbitals
PCl
5
(10 e ) SF
6
(12 e )

Drawing Valence Electrons
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“Electron-dot notation”: Electrons are represented as dots located around the symbol of the element. You must put one electron on each side before you double up.
X

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Chlorine
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Neon
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Magnesium
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Sulfur
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Silicon

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Page 209 #10-12, 15, 19

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To draw Lewis structures for covalent bonds, use the
NASB method:
N (Needed): Find the number of electrons needed to form full octets for all elements. For most nonmetals, they need 8. Hydrogen needs only 2.
A (Available): Find the number of electrons available by adding up all of the valence electrons for all elements involved.
S (Shared): Subtract the two numbers. S= N-A
B (Bond): A bond is formed with 2 electrons, so divide by 2 to find how many bonds to draw between the elements.
Draw the molecule. Put first atom in the center.
H’s are always outside. Draw in the bonds, then fill in the rest of the electrons.
Check to ensure all atoms have a full octet.

Draw the Lewis-dot-structure for the following molecules
1. HF
2. CCl
2
H
2

Draw the Lewis-dot-structure for the following molecules
1. H
2
O
2. CO
2

Each bond involves the sharing of _____ _________ of electrons.
Single Bonds= __ e ’s
Double Bonds= __ e ’s
Triple Bonds=__ e ’s

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Occurs when more than one valid
Lewis Structure can be written for a molecule or ion
Differ only in the position of electron pairs, never the atoms positions
Actual molecule behaves as if it has one structure
Example: O
3

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6.2 page 209 #16-18, 21, 23