Test 1

Front 1

Electronegativity

Back 1

Relative attractive power of an atom for electrons in a bond. F, O, Cl, Br, N, I, C, H, Na

Front 2

Organic Chemistry

Back 2

The attractive forces between hydrocarbons. When O/Cl/Br/N/I (the negative elements) covalently bond with C & H (the positive elements)

Front 3

Electronegativity Difference

Back 3

Anything greater than 1.5 is Ionic and anything less than 1.2 is covalent

Front 4

Octet Rule

Back 4

An atom becomes low energy (stable) when it has access to 8 valence electrons. (Only 2 for H) Only the atoms in period 3 or higher. An exceed the octet rule since they have D orbital available. Ex) C, N, O can have a max of 8 electrons = 4 bonds.

Front 5

Lewis Structure

Back 5

Drawing the bonding arrangements:

1) add up the valence electrons

Ex) SOCl2 = (6+6+(7*2)) = 26 electrons

2) Decide on bonding arrangement by having the least electronegative atom in the middle, then have the more electronegative atoms obey the octet rule by adding lone pairs

3) If there are any electrons remaining add as lone pairs to least electronegative atom

4) Check least electronegative atom for octet rule

Front 6

Formal Charge

Back 6

The electron charge on an atom in a molecule relative to its ground state as element

(group number) - [( number of bonds) + (number lone electrons)]

Molecules all add up to a charge of zero

Front 7

Resonance

Back 7

1) lone pairs can become double bonds

2) Double bonds can become different double bonds or lone pairs

3) The octet rule must be obeyed

4) Overall charge stays the same

Front 8

Condensed Structure

Back 8

Written without showing all the individual bonds. Central atom is shown together with the atoms that are bonded to it. The atoms bonded to a central atom are listed after the central atom (carbon). If there are two or more identical groups parentheses and a subscript are used. Double and triple bonds are drawn out.

1) C = C are shown

2) C = O are not shown

Front 9

Skeletal structure