Unit 2 (no shapes or bond angles included)

Molecular and Ionic Compound Structure and Properties

Electrons in Metallic Bonds are…

delocalized

Metals are..

• conductive

• malleable

• ductile

Nonpolar Covalent Bond

electrons are shared equally

Polar Covalent Bond

electrons are shared unequally

Ionic Bond

transfer of electrons

Electronegativity

ability of element to attract electrons to itself in a bond

Bond Polarity

if there is a difference in electronegativity values between 2 atoms the bond will be polar

Electronegativity Difference for Nonpolar Covalent Bonds

0-0.4

Electronegativity Difference for Polar Covalent Bonds

0.4-2

Electronegativity Difference for Ionic Bonds

2-4

single bonds

longest and weakest bond

triple bond

shortest and strongest bond

Shape of Ionic Compounds

crystel lattice

Ionic Compounds

both the charge and the size of the ions determine how strong the energy of interaction will be

Ionic Compound Strongest Attraction Clues

1. highest charge

2. smallest radius

Substitutional Alloy

similar size elements

Interstitial Alloy

different size elements

Covalent Compounds

discrete molecules that take on predictable shapes

Octet Rule exception: H and He

2 electrons

Octet Rule exception: Be

4 electrons

Octet Rule exception: B

6 electrons

Octet Rule exception: 3rd row and below

can have more than 8 electrons

Hydrocarbon Alkane formula

C_nH_2n+2

Hydrocarbon Alkene formula

C_nH_2n

Hydrocarbon Alkyne formula

C_nH_2n-2

Hydrocarbon Alkane Bond

single

Hydrocarbon Alkene Bond

double

Hydrocarbon Alkyne Bond

triple

Formal Charges

when you can draw more than 1 Lewis structure for a molecule, there is usually one that is the favored structure

Formal Charge Formula

valence electrons - (lone electrons + bonds attached)

Hybridization

orbitals in an atom come together to make hybrids

Hybridization 2 charge clouds

sp

Hybridization 3 charge clouds

sp²

Hybridization 4 charge clouds

sp³