Electronegativity
This or That
Formal Charge
Draw the Structure!
Vocab
100
Define electronegativity
Ability to attract a bonding electron (aka. how tightly an atom holds on to it)
100
Hydrogen's valence shell is filled with how many electrons: 8 or 2?
2
100
What is the formula for calculating formal charge?
FC = valence electrons - bonds - lone pair electrons
100
CCl4
100
Ionic compounds contain a _______ and non-metal, where electrons are __________ between atoms.
metal
transferred
200
Is silicon or carbon more electronegative?
Carbon
200
Which pair, does NOT include an element that is often an exception to the octet rule: P & B, or O & F
O & F
200
When comparing potential Lewis structures, the more stable structure has atoms with FCs closest to _______ .
Zero
200
O2
200
A species with an ODD # of Electrons.
Radical
300
A significant difference in electronegativity between to elements in a bond causes this (also depicted below).
Dipole moment
300
When counting valence electrons for ClF4+ the positive charge means what; you've lost or gained an electron?
lost (subtract 1)
300
Calculate the highlighted atom's formal charge. 
0
300
SF6
300
For ionic compounds, what increases with decreasing size of ions?
Lattice Energy
400
What is the least electronegative element? The most electronegative?
Francium
Fluorine
400
Which ionic compound will have a higher lattice energy: NaF or CaO?
CaO (greater charge)
400
Formal charge of highlighted atom 
+1
400
CO32-
400
Being large enough to have access to the same energy level d orbital allows an element to have this
Expanded Octet
500
What makes a bond polar covalent. (Rather than pure covalent)
Difference electronegativity of atoms in a molecule.
500
Which bond is stronger; ionic or covalent?
Ionic
500
Formal charge of highlighted atom 
-1
500
ClF4-
500
These are different, but equally viable, due to movement of lone pair electrons and/or double bond electrons.
Resonance Structures