chp 14 test Flashcards by meagan b

intermolecular forces vs intramolecular forces

intermolecular- between molecules, much weaker than intramolecular forces (dispersion, dipole-dipole, hydrogen bonds)

intramolecular- within a molecule (ionic, covalent, metallic)

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intramolecular forces

forces that exist within a molecule

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intermolecular forces

attractive forces between molecules

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neutral atom

equal number of protons and electrons

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how can an atom lose its symmetry?

electrons can randomly move to one side

a charged object near the atom can cause the electrons to shift

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what is the result of lost symmetry in an atom?

a dipole

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dipole

a mole in which the positive and negative charges are not evenly distributed

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induced dipole

one dipole can cause a neighboring atom to turn into a dipole; a neighboring atom of a dipole that becomes a dipole because of the neighboring dipole

resulting dipoles attract to each other

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(london) dispersion force

force of attraction between two neighboring temporary dipoles

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partial charges on atom cause blank dipoles

permanent

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dipole-dipole forces

attractions between neighboring permanent dipoles

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why are dipole-dipole forces much stronger than dispersion forces?

because they result from permanent (not temporary) dipoles

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hydrogen bond

a really strong dipole-dipole force

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weakest to strongest IF

dispersion forces
dipole-dipole forces
hydrogen bonds

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particles of a liquid

are in constant random motion
are sliding past each other
are tightly packed
are able to change positions
are NOT able to separate from one another

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what are properties of liquids determined by?

nature and strength of IF between the particles

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properties of liquids

definite volume- due to strong IF preventing them from separating
are fluids- IF are weak enough to allow liquids to flow
high density- IF are strong and the particles are tightly packed
incompressible- IF forces are sting and the particles are tightly packed
ability to dissolve- many solid will disolve in many liquids; IF are weak enough to allow the particles to move past each other
ability to diffuse- IF are weak enough to allow the particles to move past each other
tendency to evaporate
tendency to solidify
surface tension
viscosity

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surface tension

a force that pulls adjacent molecules on the surface of a liquid together

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relationship between surface tension and IF (and temp)

the greater the strength of the IF, the higher the surface tension

if temp increases, IF are weakened, surface tension decreases

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viscosity

the friction or resistance to motion, between particles of a liquid as they move past each other

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relationship between viscosity and IF (and temp)

the greater the IF, the higher the viscosity

if temp increases, IF are weakened, viscosity decreases

particles of a solid

can only vibrate in position

are not free to move around

have very strong IF

properties of a solid

high density

nonfluidity

incompressible

definitive volume and shape

tendency to melt

solids have tightly packed particles

types of solids

cristallin

amorphous

cristallin solids

particles arranged in a highly ordered, geometric repaying pattern

amorphous solids

no repeating pattern particles are randomly arranged when heated, solids softens and then melts

electron sea model

fixed positive ions surrounddd by mobile electrons

properties of metals

good conductors of heat and electricity malleable- easily shaped ductile- can be drawn into wires

what are the six state changes

vaporization (l—>g) melting (s—>l) sublimation (s—>g) condensation (g—>l) freezing (l—>s) deposition (g—>s)

which state changes are endothermic? why?

vaporization, melting, sublimation all require heat to weaken or break IF

which state changes are exothermic? why?

heat is released when IF get stronger

what happens to kinetic energy in state changes?

always remains constant because temp remains constant during state changes; if temp is constant, KE is constant

what happens to potential energy in state changes?

will increase or decrease depending on the kind of state change; PE increases in endothermic reactions and decreases in exothermic reactions

what does it mean to be in equilibrium?

equilibrium is reached when the rate of evaporation equals the rate of condensation (or any other state changes)

equilibrium

a dynamic condition in which two opposing changes occur at equal rates

what happens if the equilibrium is lost between condensation and evaporation is lost because the temp increases and evaporation increases

condensation increase to return the system to equilibrium

le châtelier’s principle

when the equilibrium of a system is lost, the system will adjust to return to equilibrium

equilibrium vapor pressure

pressure = equilibrium vapor pressure the pressure of a gas at equilibrium with its pressure (as temp increases, the vapor pressure increases; when vapor pressure equals atmospheric pressure, the liquid boils)

boiling point

when a vapor pressure equals atmospheric pressure, the liquid boils high altitude = lower atm pressure (a lower arm pressure is needed to boil; lower boiling pts)

phase diagram: triple point

all three states of matter are in equilibrium

phase diagram: critical point

the temp above which a substance will always be a gas

strong IF prevent liquid particles from separating; which property applies to this?

definite volume

IF forces in liquid particles are weak enough to allow liquids to flow; which property applies to this?

are fluids

IF in liquid particles are strong, which means the particles are tightly packed; which properties apply to this?

high density incompressible

IF in liquid particles are week enough to allow the particles to move past each other; which properties apply to this?

ability to dissolve- many solids will dissolve in many liquids ability to diffuse

solids have strong IF and tightly packed particles; which properties apply to this?

high density nonfluidity incompressible definite volume and shape

what is the state of matter of a substance determined by?

the strength of the forces (IF)

liquids: definitive volume

due to strong IF preventing them from separating

liquids: are fluids

IF are weak enough to allow liquids to flow

liquids: high density, incompressible

IF are strong, which means particles are tightly packed

liquids: ability to dissolve, ability to diffuse

IF are weak enough to allow the particles to move past each other