Chemistry- Properties of substances and mixtures

nonpolar

symmetrical, no charges

polar

asymmetrical, partial charges and dipole moments

the strongest intermolecular forces between ______ are less than ____ as strong as the bonds between ____

molecules, 5%, atoms

dipole-dipole force

partial positive and partial negative charges exist in molecule regions, forming a dipole.

london dispersion force

intermolecular forces are strong enough to cause solid and liquid phases to exist at any given time. electrons are unevenly distributed

what causes a temporary dipole?

the uneven distribution of electrons

every molecule experiences _____

london forces

force strength increases as _____

atomic/molecular weight increases

NPC is only

london dispersion

all hydrocarbons are

symmetrical

to pick which is the stronger forces between LDF, use

the number of electrons, whichever has more, is the strongest and more polarizable

all _________ have dipole-dipole forces

polar

hydrogen bondings involves hydrogen bonding with

N, O, F

strongest to weakest NPC and PC

HB, DD, LD

sometimes ___ can be stronger than ___ due to data given

LD, HB

viscous

strong force because its sticky— resistance to flow

for ionic compounds with high MP look at

charges

as force ______ BP +MP______

increase, Increases

ion dipole

between ions and polar covalent— a complete charge with a partial charge

ionic

between a metal and a nonmetal

ion-induced dipole

between ions and NPC— complete charge with a temporary dipole

dipole-induced dipole

between NPC and PC— partial charge and no charge to form a temporary dipole

strongest to weakest ION and covalent

ID, I-ID, D-ID

ionic solids

forces based on columbs law— strong force = high charge magnitude/small ions. high MP, conductive in water

metallic solids

metal, electron sea model, elements and alloys, conductive, malleable, lustrous

molecular solids

covalent molecular held together by relativley strong intermolecular forces, keeping it solid

molecular solids properties

low MP, volatile, nonconductive

network covalent solids

a huge molecule that has a network of covalent bonds

molecular solids examples

sugar, iodine

network covalent solids properties

hard, high MP, nonconductive except graphite

network covalent solids examples

diamond, graphite, quartz (SiO₂)

stages from strongest to weakest

solid, liquid, gas

When comparing elements boiling points use

whichever has the most electrons

This intermolecular force is caused by the formation of temporary dipoles

london dispersion

when looking at what would form the strongest ion-dipole force look at

radius

evaporation

volatility

capillary action

movement of a liquid through another of opposing force

vapor pressure

pressure of the vapor in a closed container

gases have no definite ____ and no definite ______

shape, volume

ideal gas

hypothetical gases that follow gas laws perfectly

real gases

have low pressures and/or high temperatures

boyles law

P₁V₁ = P₂V₂

charles law

V₁ / T₁ = V₂ / T₂

gay law

P₁ / T₁ = P₂ / T₂

avogadros law

V₁ / n₁ = V₂ / n₂

desnity and molar mass

MM= DRT / P

T is always in

Kelvin

density is always

g/L

collection over water

P_gas = P_total - P_H20

gas particles are ____ compared to the _____ between them

very small, distance

gas particles are in ____

constant motion

gas particles are assumed to exert ______ on each other

no forces

the kinetic energy of gas particles is _________ to the temperature of the gas

directly proportional

kinetic energy per molecule

energy due to the motion of a particle

kinetic energy per mole

energy due to motion of a group of particles

_____ molecules move faster than ____ ones

smaller, heavier

KE per mole of any gas depends on _____

temperature

pressure

gas particles coliding with walls of their containers

which is ideal? small or large molecules

small

which is ideal? few or many molecules

few

which is ideal? high temp, low pressure or low temp, high pressure

high temp, low pressure

which is ideal? very weak forces or strong

very weak