Ch 10: States of Matter

equation for KE

KE=1/2mv^2

Among gas particles, the KE of the particles overcomes __between the molecules except when the temp. of the gas gets close to the point where gas will __

attractive forces, condense

ALL gases at the same temperature have the same...

average kinetic energy

what temperature is a measure for molecules?

average kinetic energy.

Kinetic Molecular Theory

based on the idea that particles of matter are always in motion

what is unusual about the density of H2O

becomes less dense when it solidifies

the change of a liquid to bubbles of vapor that appear throughout the liquid?

boiling.

the attraction of the surface of a liquid to the surface of a solid? This attraction tends to pull the liquid molecules upward along the surface of the solid and against the pull of gravity.

capillary action.

ability to greatly decrease the volume of a gas sample?

compressibility.

crystalline solid

consists of crystals- substance in which the particles are arranged in an orderly, geometric, repeating pattern

the process by which gas particles pass through a tiny opening?

effusion.

the pressure exerted by vapor on a liquid once the condensation and vaporization processes reach equilibrium?

equilibrium vapor pressure.

dynamic condition in which two opposing changes occur at equal rates, resulting in no net change?

equilibrium.

the process by which particles escape from the surface of a non boiling liquid and enter the gas state?

evaporation.

net release of heat? Deposition, Freezing, and Condensation are all examples.

exothermic

gases are the most ordered state of matter: t or f

false

under what conditions does deposition occur?

formation of frost

temperature at which the processes of freezing and melting are at equilibrium?

freezing point.

under what conditions does sublimation occur?

frost-free refrigerators

IMFs so weak you can ignore them

gas

able to effuse

gas

can be significantly compressed within an increase in pressure

gas

expand to fill container

gas

extremely mobile particles

gas

has the greatest distance between particles

gas

lowest density

gas

no definite shape or volume

gas

particles in constant motion

gas

phase of matter with the greatest disorder

gas

what happens to the gas particles as temperature increases?

gas particles move faster which increase KE and average speeds

Depostion

gas to solid

the state of matter that diffusion occurs more quickly in compared to liquids?

gases.

Enthalpy

heat

what volatile liquids have that is the reason why many molecules can go into the gas phase?

high equilibrium vapor pressure.

the high molar enthalpy of fusion and molar enthalpy of vaporization of water are die to water's __

hydrogen bonds

critical point

indicates the critical temperature and critical pressure

what occurs when the object(s) does not bounce away and kinetic energy is converted into other forms of energy (some of which, does not work) (ex. high speed car crash deforms the cars)?

inelastic collision.

a crystal structure consisting of positive and negative ions arranged in a regular pattern? These crystals are hard and brittle, have high melting points, and are good insulators.

ionic.

__ is transferred between two particles during collisions. However, the KE of the two particles remain the same as long as __ is constant.

kinetic energy, temperature

energy of motion

kinetic energy.

what nonvolatile liquids have that is the reason why many molecules cannot go into the gas phase?

low equilibrium vapor pressure.

factors that affect the rate of diffusion of one gas through another

low temperature and high pressure

how you would lower the boiling point of a liquid?

lower the atmospheric pressure

display surface tension

liquid

exhibit capillary action

liquid

has definite volume but takes the shape of its container

liquid

least common state of matter

liquid

moderately mobile particles

liquid

nearly incompressible

liquid

slightly less dense than solids

liquid

fluids

liquids and gases

the phase(s) of matter that act like fluids, being able to glide easily past one another (flow) and take the shape of its container?

liquids and gases (gas particles are so far apart that the attractive forces between the particles are weak, and thus the particles slide right past each other...think of air flowing out of a vent...it "pours" out)

why are liquids the least common state of matter?

liquids have a narrow range of temperatures and pressure for which a substance can remain in the liquid phase

volatile liquids

liquids that evaporate readily and have weak forces of attraction between particles

least common state of matter in the universe because they can only exist in a narrow range of temperatures and pressures?

liquids.

what is happening to the temperature of the liquid, when a substance is boiling?

nothing. It stays the same because the energy being absorbed is being used to vaporize the liquid (to overcome the attractive forces between the molecules of the liquid).

what the "m" stands for in the equation of kinetic energy?

mass

how are network covalent compounds bonded differently than melecular compounds?

melecular compounds contain individual molecules while network covalent compounds can be pictured as continuous, 3D networks of bonded atoms

crystal structure consisting of metal cations surrounded by a sea of delocalized valence electrons? The freedom of these delocalized electrons to move throughout the crystal explains the high electric conductivity of these crystalline solids.

metallic

higher kinetic energy between NH3 at 100°C or H2O at 100°C?

neither - they are the same.

a type of crystal in which each atom is covalently bonded to its nearest neighboring atoms? The covalent bonding extends throughout a network that includes very large number of atoms (making essentially giant molecules). Examples include diamond, quartz, and many compounds containing silicon. They have rather high melting points and are usually nonconductors or semiconductors.

network covalent.

amorphous solid and examples

particles are arranged randomly, glass and plastics

evaportation

particles escape from the surface of a non-boiling liquid and enter the gas phase, some surface particles with higher-than-average energies can overcome the liquid phase and escape into the gas state, liquids have to have enough KE to overcome the IMFs

graph with pressure on the y axis and temperature on the x axis? This graph shows the conditions under which the phases of a substance exist.

phase diagram.

although ideal gases do not exist, many gases behave almost ideally if...

pressure is not very high and temperature is not very low

what vapor molecules exert on a liquid in a closed container.

pressure.

how you would increase the equilibrium vapor pressure of a substance?

raise the temperature so more molecules have enough kinetic energy to enter the gas phase.

IMFs are the strongest between particles

solid

considerably more dense than gases

solid

generally the most dense state

solid

has a definite shape and volume

solid

has the smallest distance between particles

solid

incompressible

solid

least mobile particles

solid

particles are held in relatively fixed positions with only vibrational movement around fixed points

solid

phase of matter with the greatest order

solid

sublimation

solid to gas

nonvolatile liquids have...

strong forces of attraction

a force that tends to pull adjacent parts of a liquid's surface together, making droplets?

surface tension.

All liquids have a specific equilibrium vapor pressure at a given __

temperature

Evaporation and boiling are types of vaporization. what is the difference?

temperature of the liquid

fluid

the particles can easily glide past one another and can flow

equilibrium vapor pressure

the pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature

how are solids formed from a liquid

when a liquid cools, the average kinetic energy of its particles decrease and the effect of the IMFs increases, pulling the particles together to form a solid

6 properties of gas

1. expansion 2. fluidity 3. low density 4. compressibity 5. diffusion 6. effusion

5 assumptions of the KMT of an ideal gas

1. gases are mostly empty space 2. collision between gas particles and container walls are elastic 3. gas particles are in continuous rapid motion 4. there are no IMFs between gas particles 5. temperature is the average kenetic energy of particles

List 4 physical properties of network covalent compounds

1. hard 2. brittle 3. high melting points and boiling points 4. non/semi conductors

types of crystalline solids

1. ionic 2. metallic 3. molar covalent 4. network covalent

enemies of an ideal gas

1. strong IMFs 2. high pressure 3. low temperature (slow down particles)

what is capillary action responsible for? (3)

1. the transportation of water from the roots of a plant to its leaves 2. the meniscus that forms in a narrow glass tube (graduated cylinder) 3. water moving up paper in paper fibers (going against gravity)

normal boiling point

100 degrees Celsius

effusion

A process by which gas particles pass through a tiny opening

the molecule that behaves more ideally as a gas - H2 or H2O?

H2 . It's intermolecular forces are the weakest.

molecules that travel slower at 100°C - NH3 or H2O molecules?

H2O

equation of kinetic energy?

KE = ½ mv^2

the result of particles in a liquid being closer together?

IMF's will have a greater impact on the physical properties of the liquid (higher density, lower compressibility).

real: gas particles stick together because of __

LDF

molecule with a lower enthalpy of vaporization - water or methane (CH 4 )?

Methane (CH4) b/c the intermolecular forces are weak between molecules of CH4 (only LDF's) whereas the IMF's between water molecules are strong (LDF, D-D, and H bonding). So it would take more energy (enthalpy) to vaporize one mole of water than it would to vaporize one mole of methane.

diffusion

Movement of molecules from an area of higher concentration to an area of lower concentration.

the molecule with a greater rate of effusion - NH3 vapor or H2O vapor?

NH3

which substance would have a higher molar enthalpy of fusion? NH3 or H2

NH3, heavier???

vaporization

The change of state from a liquid to a gas

Equalibrium

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

surface tension

a force that tends to pull adjacent parts of a liquid's surface together, thereby decreasing surface area to the smallest possible size, as IMF increases so does the surface tension

vapor

a gas in contact with its liquid or solid phase

ideal gas

a hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory

able to diffuse

all

spontaneous mixing of the particles of two substances caused by their rapid, random motion?

diffusion. the movement of particles from an area of high concentration to an area of lower concentration without the input of energy.

net absorption of heat? Sublimation, Evaporation, and Melting are all examples.

endothermic.

the crystal structure consisting of metal cations surrounded by a sea of delocalized valence electrons? The freedom of these delocalized electrons to move throughout the crystal explains the high electric conductivity of these crystalline solids.

molecular covalent.

elastic collision

one in which there is no net loss of total kinetic energy

What is the KMT used to explain?

the PROPERTIES of solids, liquids and gases by taking into account the MOTION and ARRANGEMENT of molecules and the IMF between molecules

molar enthalpy of fusion

the amount of energy as heat required to melt one mole of solid at the solid's melting point

molar enthalpy of vaporization

the amount of energy as heat that is needed to vaporize one mole of liquid at the liquid's boiling point at constant pressure

capillary action

the attraction of the surface of a liquid to the surface of a solid

boiling

the conversion of a liquid to a vapor within the liquid as well as at its surface

critical pressure

the lowest pressure at which a substance can exist as a liquid at the critical temperature

relationship between polarity and ideal gas

the more polar the molecules of gas are the greater the attractive forces

critical temperature

the temperature above which a substance cannot exist in the liquid state

triple point

the temperature and pressure conditions at which the solid, liquid, and gaseous phases of a substance coexist at equilibrium

normal freezing point

the temperature at which the solid and liquid are in equilibrium at 1 atm

is the pot of boiling water hotter than the steam that is rising from the water?

the temperature is the same

boiling point

the temperature the equilibrium vapor pressure of the liquid equals the atmospheric pressure

the process by which a liquid or solid changes to a gas?

vaporization.

what the "v" stands for in the equation of kinetic energy?

velocity(speed+direction ex. 5 mph north)

higher enthalpy of fusion - water or methane(CH 4 )?

water b/c the IMF's are stronger between molecules of water (LDF's, D-D, and H bonding) than between molecules of CH 4 (LDF's only b/c a nonpolar molecule). So it would take more energy to melt one mole of water than it would to melt one mole of methane.

Is it true that all liquids freeze?

yes.