Chapter 7 & 8.1 - 8.4 Chemical Bonding and Molecular shape

What tells you how many valence electrons you have?

The number column on the periodic table

Ex. Oxygen has 6 valence electrons

What does the ns and np represent?

The valence electrons shells

Lewis Dots

Dots around the symbol to represent the valence electrons in the free atoms

Where does the first two dots go?

The orbital electrons

Maximum of 2 electrons in the p-sub shell

How many dots go in the p orbital?

One dot in each of the first three

Where do the remaining dots go?

In the remaining p electron

Maximum of 6 electrons in p sub shell {Px, Py, Pz}

Why do atoms bond?

It results in a more stable electron configuration

(More stable = lower potential energy)

How do atoms bond together?

By ether transferring or sharing electrons

What happen to the atoms after they bond?

Results in all atoms obtaining an outer shell with eight electrons

Octet rule

Main group atoms gains, lose, or share electrons until they are surrounded by 8 valence electrons

Octet Rule exceptions

H, Li, Be, B attain electron configuration

Li

Loses its one valence electrons

H

Shares or gains one electrons or lose one to form H+

Be

Loses three electrons to become Be2+

(Commonly shares its two electrons in covalent bonds resulting in four valence electrons)

B

Loses three electrons to become B3+

(Commonly shares its three electrons in covalent bonds, resulting in six valence electrons )

Expanding octets for elements in period 3 or below

Uses empty valence d orbitals