Bonding test Study Guide

Cations

• Formed by losing all valence electrons

• Positively charged

• Alkali metals(Group 1A), Alkaline earth metals (Group 2A), Group 3A

Anions

• Formed by gaining 1 or more valence electrons

• negatively charged

• Group 5A, Group 6A, Halogens ( Group 7A)

Polyatomics

Ammonium: NH4 1+

Acetate: C2H3O2 1-

Hydroxide: OH 1-

Cyanide: CN 1-

Nitrate: NO3 1-

Bicarbonate: HCO3 1-

Carbonate: CO3 2-

Sulfate:SO4 2-

Chromate: CrO4 2-

Phosphate:PO4 3-

Naming Polyatomics

Ate - Base

Ite - Minus 1 oxygen

Per- plus 1 oxygen

Hypo ite - Minus 2 oxygen

Naming Ionic

• First name metal, then non-metal

• Transition metals use Roman numerals as well as Tin and Lead

• Non-transition metals with known charges are just the element name, as well as silver, zinc, and cadmium

• For non-metals, just add ide to the end unless polyatomic

( to figure out subscripts, write the charges and then cross them)

Naming Covalent

• use charge to determine charges.

• The first non metal does not use mono

• second non metal uses all prefixes and adds ide to the end

Prefixes

mono

di

tri

tetra

penta

hexta

hepta

octa

nona

deca

Properties of ionic compouds

• ions are strongly bonded

• structure is rigid

• high meting points because of strong forces between ions

• brittle

Ionic conductivity

• conductivity requires charges that move

Solid (S): will not conduct

liquid (L): will conduct

dissolved in water(Aq): will conduct

Gas(s): Will not conduct

Metalic Bonding

• two metals

• Electrons are held loosely and free to move through a solid (Sea of electrons). Electrons are mobile

• The attraction between cations and the sea of delocalized electrons

Solid (S): will conduct

liquird (L): will conduct

dissolved in water(Aq): will not conduct

Gas(s): Will not conduct

Metalic Properties

• Malleable

• Ductile - drawn into wires

• Good conductors of heat

• Good conductors of electricity

Sigma and Pi in Covalent Bonds

Single - 1 sigma

Double - 1 sigma, 1 pi

Tripple - 1 sigma, 2 pi

As the number of bonds grows, the bond grows shorter and stronger, the presence of pi brings the atom closer.

Ionic Bond

• The transfer of valence electrons from cations to anions or metals to nonmetals

Covalent Bond

• Sharing of a pair of valence electrons between anions or two non metals

• cannot conduct electricity

Molecular structure

• The central atom will be the least electronegative and the atom that there is the least amount of

• Hydrogen will not be a central atom it is typically halogens

Diagramming molecular compounds

• Count up valence electrons for each atom

• Draw bonds and subtract 2 electrons for each bond

• add additional electrons

• If the octet/ duet rule is not met, try double bonds.

Boron will be happy with 6 and Hydrogen will be happy with 2

Formal charge

To make sure that the bonds are correct

Valence electrons - (the dots and lines added together) = 0

Bonding domains

Number of elements around the center

Non bonding domains

number of electron lone paires

Lone pairs + elements

Number of electron domains

Linear

Bonding domains : 2

nonbonding domains: 0

Number of electron domains: 2

Bond angle: 180

Trigonal Planar

Bonding domains : 3

nonbonding domains: 0

Number of electron domains: 3

Bond angle: 120

Bent ( single lone)

Bonding domains: 2

nonbonding domains: 1

Number of electron domains: 3

Bond angle: 117.5

Tetrahedral

Bonding domains: 4

nonbonding domains: 0

Number of electron domains: 4

Bond angle: 109.5

Trigonal Pyramidal

Bonding domains : 3

nonbonding domains: 1

Number of electron domains: 4

Bond angle: 107

Bent (Double lone)

Bonding domains: 2

nonbonding domains: 2

Number of electron domains: 4

Bond angle: 104.5