Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
10 Cards in this Set
- Front
- Back
properties of ionic compounds
|
solids at room temperature
very high melting and boiling point crystal at solid state dissociate in water, form positive and negative ions metal + nonmetal transfer electrons |
|
electrolytes
|
contain ions, conduct electricity.
|
|
properties of covalent compounds
|
solids, liquids, gases
low melting and boiling point that varies with polarity. high polarity means high mp/bp, low polarity means low mp/bp crystalline or amorphous structure don't dissociate and don't conduct electricity 2 nonmetals together share electrons |
|
bond strength
|
double and triple bonds are more stable than single bonds.
|
|
bond energy
|
the amount of energy required to break a bond
|
|
bond length
|
the distance separating the nuclei of 2 adjacent atoms. single>double>triple
|
|
resonance
|
2 or more Lewis structures that contribute to real structure
|
|
Valence Shell Electron Pair Repulsion
|
all electrons around the central atom arrange themselves so that they are as far away as possible to limit electronic repulsion. Used to predict the shape of molecules.
|
|
types of bond orientations
|
linear, 180
trigonometric planar, 120 tetrahedral, 109.5 (primary structure of a full octet) trigonal pyramidal, 107 (full octet with a lone pair) bent/angular structure 104.5 (full octet with 2 lone pairs) |
|
rules of VSEPR
|
1. electrons get as far away as possible
2. unbound electrons take up more space |