Chemistry Unit 12 Test Review

linear, 180 degrees

trigonal planar, 120 degrees

Bent, <120°

tetrahedral, 109.5 degrees

trigonal pyramidal, <109.5

Bent 109.5

trigonal bipyramidal, 90 or 120

See-saw, <90° and <120°

T-structure, <90°

Linear 180

octahedral, 90 degrees

square pyramidal 90

square planar, 90 degrees

-if there are lone pairs

-if there 2 or more different elements (excluding the core element)

-if there are no lone pairs

-if there is only two elements including the core element

-dipoles in opposite directions creates even distribution of charge in the molecule

Covalent Network: Carbon, Silicon or silicon with carbon or oxygen

Metallic Interactions: Metals only

Ionic bonds: metals and nonmetals

Nonmetals with N, O or F bonded with H: Hydrogen bonding(LDF)

Nonmetals with polar structure: Dipole-Dipole (LDF)

Just nonmetals: LDF

London dispersion force and is the weakest of the IMFs and all nonmetals have this

attractive forces between the positive end of one polar molecule and the negative end of another polar molecule

Hydrogen bonding is the strongest intermolecular force. it only happens when hydrogen is covalently bonded to fluorine, nitrogen or oxygen because they're very electronegative and can pull the bonding electrons away from the hydrogen. Substances with hydrogen bonding have higher melting and boiling points because of the extra energy needed to break the hydrogen bonds.

Electrostatic attractions between cations and anions in an ionic compound. A metal bonded to a non-metal. In some cases we can compare the relative strength of ionic IMF's. Ionic IMF's increase as the charge on the ions increase.

It occurs when one or more metals are combined. There are a sea of valence electrons that holds the cations together.

When the number of atoms joining together is huge and the number of atoms is not fixed and a giant lattice forms containing billions of atoms

the volume occupied by one mole of a gas

The volume decreases

The temperature increases

Energy needed to undergo a phase change

increase

the pressure exerted by a vapor over a liquid

decrease

the energy required to completely separate a mole of a solid ionic compound into its gaseous ions

increase

An attraction between molecules of different substances

Attraction between molecules of the same substance

Spontaneous rising of a liquid in a surface area

the resistance of a liquid to an increase in its surface area

-Conduct electricity

-High melting point

-malleable

-ductile

-excellent heat conductors

-shiny