VSEPR and Types of Bonds

2 electron groups, 0 lone pairs

2 electron groups, 0 lone pairs

e⁻ geo: linear molecular geo: linear hybridization: sp bond angle: 180°

3 electron groups, 0 lone pairs

e⁻ geo: trigonal planar molecular geo: trigonal planar hybridization: sp² bond angle: 120°

3 electron groups, 1 lone pair

e⁻ geo: trigonal planar molecular geo: bent hybridization: sp² bond angle: <120°

4 electron groups, 0 lone pair

e⁻ geo: tetrahedral molecular geo: tetrahedral hybridization: sp³ bond angle: 109.5°

4 electron groups, 1 lone pair

e⁻ geo: tetrahedral molecular geo: trigonal pyramidal hybridization: sp³ bond angle: <109.5°

4 electron groups, 2 lone pairs

e⁻ geo: tetrahedral molecular geo: bent hybridization: sp³ bond angle: <109.5°

5 electron groups, 0 lone pairs

e⁻ geo: trigonal bipyramidal molecular geo: trigonal bipyramidal hybridization: sp³d bond angle: 120° & 90°

5 electron groups, 1 lone pair

e⁻ geo: trigonal bipyramidal molecular geo: see saw hybridization: sp³d bond angle: <120° & <90°

5 electron groups, 2 lone pairs

e⁻ geo: trigonal bipyramidal molecular geo: t-shaped hybridization: sp³d bond angle: <120° & <90°

5 electron groups, 3 lone pairs

e⁻ geo: trigonal bipyramidal molecular geo: linear hybridization: sp³d bond angle: 180°

6 electron groups, 0 lone pairs

e⁻ geo: octahedral molecular geo: octahedral hybridization: sp³d² bond angle: 90°

6 electron groups, 1 lone pair

e⁻ geo: octahedral molecular geo: square pyramidal hybridization: sp³d² bond angle: <90°

6 electron groups, 2 lone pairs

e⁻ geo: octahedral molecular geo: square planar hybridization: sp³d² bond angle: 90°

6 electron groups, 3 lone pairs

e⁻ geo: octahedral molecular geo: t-shaped hybridization: sp³d² bond angle: <90°

6 electron groups, 4 lone pairs

e⁻ geo: octahedral molecular geo: linear hybridization: sp³d² bond angle: 180°

ionic=

metal + nonmetal

covalent=

non-metal + non-metal

metallic

metals only

ionic bond strength=

strong

covalent bond strength=

weak

metallic bond strength=

strong

ionic is called...

compounds

covalent is called...

molecule or molecular compound

what happens to the electrons of ionics?

transfers electrons from metals to non-metals

what happens to the electrons of covalents?

shares electrons (equally= non-polar, unequal= polar)

what happens to the electrons of metallics?

delocalized (sea of electrons)

ionic: formed from cations/anions?

made of cations (metal) and anions (non-metal)

covalent: formed from cations/anions?

made only of anions

metallic: formed from cations/anions

made only of cations

ionic conductivity

conducts when dissolved in aqueous solution

covalent conductivity

does NOT conduct electricity

metallic conductivity

good conductors of heat and electricity

ionic state of matter

solids at room temp (stronger bonds)

covalent state of matter

liquids or gasses (weaker bonds)

metallic state of matter

solids at room temperature

ionic melting and boiling points

high

covalent melting and boiling points

low

metallic melting and boiling points

high

ionic reason for forming a bond

forms a bond to become stable

covalent reason for forming a bond

forms to become stable

metallic reason for forming a bond

forms to become stable

ionic characteristics include

brittle

covalent characteristics include

network covalent

network covalent

diamond and silicon are very strong bonds

metallic characteristics include

shiny (luster), malleable/ductile

ionic electronegativity values

high electronegativity difference

covalent electronegativity values

low electronegativity difference

metallic electronegativity values

low

ionic bond energy

high

covalent bond energy

low

metallic bond energy

high

ionic bond length

short

covalent bond length

long

metallic bond length

short

Metallics have a short bond length because

electrons don't belong to any atom (= sea of electrons (delocalized))

electricity=

flow of electric charges

cations...

lose electrons and become positive (metals)

anions...

gain electrons and become negative (non-metals)

valence electrons...

involved in bonding and found in the outer most shell

molecular orbit=

region in which shared electrons are found

bond length=

average distance due to electrons moving in the form of a wave

single bond length is

long

single bond strength is

weak

double bond length is

shorter than a single bond

double bond strength is

stronger than a single bond

triple bond length is

the shortest

triple bond strength is

the strongest

bond energy=

the amount of energy required to break the bond in 1 mole of a substance

polar=

unequal sharing of electrons

nonpolar=

equal sharing of electrons

are diatomics polar or nonpolar?

always nonpolar

polar=

opposites