ORGO I Chaper 1

ionic bond

the bond that forms when an electron is transferred between a metal (cation) and a non metal (anion)

covalent bond

the bond that forms when an electron is shared between 2 nonmetals anions)

polar covalent bond

a covalent bond that forms when an electron is unequally shared between two nonmetals

nonpolar covalent bond

a covalent bond that forms when an electron is equally shared between two nonmetals

5 types of molecular geometries

1. linear

2. trigonal planar

3. tetrahedral

4. trigonal bipyramidal

5. octahedral

linear molecular geometry

2 electron groups

180° angles

trigonal planar molecular geometry

3 electron groups

120° angles

tetrahedral molecular geometry

4 electron groups

109.5° angles

trigonal pyramidal molecular geometry

3 bonding pairs

1 lone pair

trigonal bipyramidal molecular geometry

5 electron groups

120° & 90° angles

octahedral geometry

6 electron groups

90° angles

5 types of hybrid orbitals

1. sp

2. sp²

3. sp³

4. sp³d

5. sp³d²

sp HO geometry & angles

linear geometry

180° angles

sp² HO geometry & angles

trig planar geometry

120° angles

sp³ HO geometry & angles

tetrahedral

109.5° angles

sp³d HO geometry & angles

trig bipyramidal

120° & 90° angles

sp³d² HO geometry & angles

octahedral

90° angles

formula for the # of hybrid orbitals

# of sigma bonds + # of lone pairs

formal charge formula

the # of valence electrons = [ # of non-bonding electrons - ½ (# of bonding electrons) ]

3 formal charge rules

1. the sum of all formal charges in a neutral molecule must be 0

2. the sum of all formal charges in an ion must equal the charge of the ion

3. a negative formal charge will reside on the most electronegative atom

sigma bonds

bonds that form when hybrid (s&p) or unhybridized (p&d) orbitals overlap

pi bonds

bonds that form only when unhybridized p orbitals overlap side to side