honors chemistry states of matter

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Chemistry

94 Terms

1

kinetic theory

all matter consists of tiny particles that are in constant motion

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2

elastic collisions

A collision in which no kinetic energy is lost; gas particles have same speed before and after the collision

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3

hydrogen bonding

strong type of intermolecular dipole-dipole attraction that occurs between hydrogen and F, O or N

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4

london dispersion forces

the intermolecular attraction resulting from the uneven distribution of electrons and the creation of temporary dipoles

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5

dipole-dipole forces

intermolecular forces that exist between polar molecules, the strength of intermolecular attractions increase when polarity increases

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6

translational motion

movement in which an entire molecule moves in a definite direction (gas)

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7

vibrational motion

periodic motion of atoms within a molecule (solids)

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8

rotational motion

motion of a body that spins about an axis (liquids)

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9

compressibility

a measure of how much the volume of matter decreases under pressure

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10

difussion

movement from an area of higher concentration to an area of lower concentration

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11

effusion

a process by which gas particles pass through a tiny opening

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12

pressure

force per unit area

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13

manometer

instrument that measures pressure

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14

barometer

instrument that measures atmospheric pressure

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15

temperature

a measure of how hot or cold something is

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16

vacuum

a space where no particles of matter exist

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17

phase diagram

a graph showing the conditions at which a substance exists as a solid, liquid, or vapor

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18

triple point

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

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19

position of particles in a liquid [are fixed/can vary]

can vary

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20

total volume of a liquid is [fixed/variable]

fixed

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21

why is the density of a liquid higher than that of a gas of the same substance?

because of the intermolecular forces that hold liquid particles together

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22

liquids are considered to be [incompressible/compressible]

incompressible, because particles are already tightly packed

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23

viscosity

a liquid's resistance to flow (thickness)

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24

stronger intermolecular forces result in [higher/lower] viscosity

higher, due to strong bonds

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25

bigger particle size and shape result in [higher/lower] viscosity

higher, because big particles move more slowly

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26

higher temperature results in [higher/lower] viscosity

lower (indirect relationship), think oil spreads faster on a pan when it is heated, or cold maple syrup travels slower than warm

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27

surface tension

the energy required to increase the surface area of a liquid by a given amount

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28

why is water's surface tension so high?

because water has hydrogen bonds, which causes strong intermolecular forces

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29

surfractant

any substance that interferes with the hydrogen bonding between water molecules and thereby reduces surface tension

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30

cohesion

attraction between molecules of the same substance

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31

adhesion

attraction between molecules of different substances

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32

crystalline solid

a solid whose atoms, ions, or molecules are arranged in an orderly, geometric structure

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33

lattice

regular arrangement of particles

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34

unit cell

the smallest group of particles within a crystal that retains the geometric shape of the crystal

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35

allotrope

an element with different forms with different molecular structures (ex. carbon)

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36

ionic solid

solid composed of positive and negative ions held together by strong electrostatic attractions

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37
  • hard, brittle, high melting point, poor conductivity

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38

ex. NaCl, KBr, CaCO3

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39

molecular solid

a solid composed of neutral molecules at the lattice points

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40
  • soft, low to moderately high melting point, poor conductivity

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41

ex. I2, H2O, NH3, CO2, C12H22O11

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42

covalent network solid

a solid that consists of atoms held together in large networks or chains by covalent bonds

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43
  • very hard, very high melting point, often poor conductivity

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44

ex. diamond and quartz

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45

metallic solid

solid composed of metal atoms surrounded by mobile valence electrons

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46
  • soft to hard, low to high melting point, malleable or ductile, good conductivity

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47

ex. all metallic elements

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48

amorphous solid

a solid made up of particles that are not arranged in a regular pattern

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49

ex. glass, rubber, plastics

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50

5 differences between amorphous and crystalline solids

  • amorphous solids lack a definite geometric shape

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51
  • unclean cleavage when cut

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52
  • isotropic (physical properties are the same in all directions)

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53
  • non-definite melting point

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54
  • non-definite heat of fusion

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55

evaporation

  • when vaporization occurs only at the surface of a liquid

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56
  • doesn't require liquid to be above boiling point

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57
  • can occur from collision of air particles

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58

vaporization

  • the change of state from a liquid to a gas

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59
  • occurs when liquid is above boiling point

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60

dynamic equilibrium

when the rate of evaporation is equal to the rate of condensation

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61

vapor pressure

the pressure exerted by a vapor over a liquid in dynamic equilibrium

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62

volatility

the tendency of a substance to vaporize

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63

substances with high vapor pressures are [more/less] volatile

more because there are less intermolecular forces

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64

substances with low vapor pressures are [more/less] volatile

less because there are less intermolecular forces

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65

IMFs and vapor pressure have a [direct/indirect] relationship

indirect, as IMFs increase, vapor pressure decreases

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66

(because higher IMFs means higher boiling point)

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67

boiling point and vapor pressure have a [direct/indirect] relationship

indirect, as boiling point increases, vapor pressure decreases (because less vapor pressure makes a substance difficult to boil)

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68

temperature and vapor pressure have a [direct/indirect] relationship

indirect, related to boiling point. lower boiling point means lower IMFs, so vapor pressure increases and the substance is more volatile

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69

normal boiling point

the boiling point of a liquid at a pressure of 1 atm

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70

critical point

the temperature and pressure at which the gas and liquid states of a substance become identical and form one phase

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71

volume (v) and gas pressure have a [direct/indirect] relationship

indirect, as one increases the other decreases

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72

temperature (T) and gas pressure have a [direct/indirect] relationship

direct, as one increases so does the other

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73

amount of gas (n) and gas pressure have a [direct/indirect] relationship

direct, as one increases so does the other

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74

boyle's law

P1V1=P2V2

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75

T and n are constant

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76

isothermal system

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77

charles' law

V1/T1=V2/T2

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78

P and n are constant

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79

isobaric system

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80

gay-lussac's law

P1/T1=P2/T2

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81

V and n are constant

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82

isochoric system

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83

combined law

P1V1/T1=P2V2/T2

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84

n is constant

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85

avogadro's law

V1/n1=V2/n2

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86

T and P are constant

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87

isothermal and isobaric system

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88

ideal gas law

PV=nRT

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89

using ideal gas law to determine molar mass

M = mRT/PV

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90

(m is in g)

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91

using ideal gas law to determine density

p = MP/RT

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92

graham's law of effusion

rate A/rate B = square root of Mb/Ma

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93

dalton's law of partial pressures

states that the total pressure of a mixture of gases is equal to the sum of the pressures of all the gases in the mixture

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94

Ptotal = P1 + P2 + P3...

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