bonding chemistry test

lemme class

types of bonding

ionic, covalent, metallic

ionic bonding

metal and non-metal

metal is giving to non-metal

covalent bonding

non-metal and non-metal

sharing electrons

metallic bonding

metal and metal

between 2 metals (cations) in the sea of delocalized electrons (electrons are just floating around to keep the protons together)

4 properties that metals have as a result of the electron sea

malleable

ductile

good conductors of heat

good conductors of electricity

ionic bonds

usually between a metal and a non-metal

bonds where a positively charged ion (cation) is attracted to a negatively charged ion (anion)

the bond is formed throughout the transfer of electrons

ionic compound

called salts

ammonium

NH4+

acetate

C2H3O2-

chlorate

CIO3-

cyanide

CN-

hydroxide

OH-

nitrate

NO3-

bicarbonate

HCO3-

carbonate

CO3-2

chromate

CrO4-2

sulfate

SO4-2

phosphate

PO4-3

exceptions (parentheses)

silver (Ag), zinc (Zn), and cadmium (Cd), aluminum (Al), gallium (Ga), indium (In)

silver

Ag⁺

zinc

Zn⁺²

cadmium

Cd⁺²

base

-ate

lose 1 oxygen

-ite

lose 2 oxygen

hypo- , -ite

add 1 oxygen

per-

metal + non-metal

criss-cross

transition metal + polyatomic

uncross to work out the charge on the transition metal

non-metal + non-metal

prefixes

1

mono

2

di

3

tri

4

tetra

5

penta

6

hexa

7

hepta

8

octa

9

nona

10

deca

stable electron configurations

all atoms react to achieve a noble gas configuration (8 electrons)

this is also known as the Octet Rule

single bond

2 atoms share 2 electrons (1 pair)

consists of 1 sigma bond

longest and weakest bond

double bond

2 atoms share 4 electrons (2 pairs)

consists of 1 sigma bond and 1 pi bond

medium length and medium strength

triple bond

2 atoms share 6 electrons (3 pairs)

consists of 1 sigma bond and 2 pi bonds

shortest bond and strongest bond

elements that often form double/triple bonds are carbon, oxygen, and nitrogen

elements that often form double/triple bonds are carbon, oxygen, and nitrogen

σ

sigma bond

π

pi bond

bond length and strength

as the number of bonds between 2 atoms increases, the bond grows shorter and stronger

the presence of pi bonds pulls the atom closer together, while also increasing bond strength

molecular structure

central atom will be least electronegative

hydrogen will not typically be a central atom

halogens will typically only form single bonds

exceptions for diagrams

boron (B) only needs 6 electrons

hydrogen (H) only need 2 electrons

linear VSEPR

2 elements around the center

0 lone pairs

2 electron domains

bond angle: 180 degrees

trigonal planar VSEPR

3 elements around the center

0 lone pairs

3 electron domains

bond angle: 120 degrees

bent linear VSEPR

2 elements around the center

1 lone pair

3 electron domains

bond angle: 117.5 degrees

tetrahedral VSEPR

4 elements around the center

0 lone pairs

4 electron domains

bond angle: 109.5 degrees

trigonal pyramidal

3 elements around the center

1 lone pair

4 electron domains

bond angle: 107 degrees

bent tetrahedral VSEPR

2 elements around the center

2 lone pairs

4 electron domains

bond angle: 104.5 degrees

formal charge equation

(valence electrons you start with) - (the dots and lines added together)

formal charge

the preferred lewis structure is the one in which the formal charge are closest to zero

resonance structures

when there is more than one way to draw the lewis structure of an ion/molecule depending on where you position the double bonds

the actual structures of the molecules are described as a hybrid of the individual resonance structures using double-headed arrows