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chemistry > 05 - states of matter > Flashcards

05 - states of matter Flashcards

1
Q

gas particles are:

A

. far apart (so can be compressed)
. are randomly arranged
. can move freely from place to place, in all directions

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2
Q

liquid particles are:

A

. close together (so have a fixed volume, can only be compressed slightly)
. mostly randomly arranged
. limited movement from place to place

LIQUIDS TAKE THE SHAPE OF THE CONTAINER

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3
Q

solid particles are:

A

. touching each other (can’t be compressed)
. usually in a regular arrangement
. can’t change positions with each other, only vibrate

SOLIDS HAVE A FIXED SHAPE AND VOLUME

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4
Q

what are the types of structures found in elements and compounds:

A

. simple molecular/simple atomic
. giant ionic
. giant metallic
. giant molecular (noble gases thought of having this structure, although they exist as isolated atoms)

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5
Q

what is the kinetic theory of gases?

A

. the theory that particles in gases liquids are in constant movement

. used to explain the effect of temperature and pressure on the volume of a gas as well as the rates of chemical reactions

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6
Q

what are the assumptions made by the kinetic theory of gases?

A

. gas molecules move rapidly and randomly
. dist. betwesn gas molecules&raquo_space;> diameter of molecules SO they have nelegible volume
. no intermolecular forces of attraction or repulsion between the molecules
. collisions between particles are elastic (no kinetic energy lost in collisions)
. temperature of the gas is related to avg. ke of the molecules

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7
Q

what is an ideal gas?

A

a gas whose volume varies in proportion to the temperature and in inverse proportion to the pressure

noble gas approach ideal gas behavior (due to their low intermolecular forces)

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8
Q

what is a real gas?

A

a gas that does not obey the ideal gas law, especially at low temps and high pressures

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9
Q

volume of a gas depends on:

A

. pressure in Pa
. temperature in K

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10
Q

volume relation to pressure?

A

volume = 1/pressure

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11
Q

volume relation to temperature?

A

volume is directly proportional to temp

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12
Q

in what ways do real gases not ovbey the kinetic theory?

A

. not zero attraction between molecules
. volume of molecules are not neligible

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13
Q

under high pressure and low temp, real gases:

A

. molecules are close to each other
. volume of the molecules not negligible
. there are id id or pd pd forces between molecules
. attractive forces pull mols towards each toher and away from container
. pressure lower than expected
. effective volume of gas is smaller than ideal gas

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14
Q

whats the formula?

A

pV=nRT

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15
Q

pV=nRT stands for?

A

p = pressure in Pa
V = colume of gas in cm3
n = no. of moles of gas
R = gas constant (8.31 J K-1 mol-1)
T = temperature in K

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16
Q

celsius to kelvin

A

+ 273

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17
Q

methods of calculating relative molecular mass?

A

. use a mass spectrometer, accurate
. use general gas eq, less accurate

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18
Q

melting for solids?

A

. energy transferred makes particles vibrate more vigorously
. forces of attraction between particles weaken
. solid beocmes liquid at its melting point

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19
Q

what is the melting point of a solid?

A

the temperature at which it changes to a liquid at 1atm

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20
Q

to melt ionic compounds, need…

A

high temp (strong bonds)

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21
Q

to melt molecular solids, need…

A

low temperature (weak intermolecular forces between particles)

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22
Q

what is vaporisation?

A

the change in state when a liquid changes to vapour

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23
Q

when heating a liquid?

A

. particles move faster
. forces for atrraction between particles weaken
. particles with most energy escape first
. liquid evaporates (at temp below boiling point)
. forces weaken for all the particles to become completely free from each other
. liquid boils at boiling point

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24
Q

what enthalpy change of vaporisation?

A

the energy required to change one mole of liquid to one mole of gas

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25
what is condensation?
the change in state when a vapour change to a liquid
26
are chnages in states reversible?
YES
27
what is vapour pressure?
the pressure exerted by a vapour in equilibrium with a liquid
28
as vapour pressure increases, temp increases because..
. gas particles have more ke . particles move faster and overcome intermolecular forces of attraction more easily
29
what is the boiling point of a liquid?
the temperature at which it chnage to a gas at one atm temperature at which vapor pressure = atmostpheric pressure
30
1 atmosphere =
101 325 Pa
31
why do crystals have a regular structure?
due to the regularly packed particles within the crystals - called a crystal lattice
32
what is a lattice?
a regularly repeatinv arrangement of ions, atoms or molecules in 3D
33
ionic lattices?
AKA giant ionic lattices . depends on ion sizes . MgO and NaCl have cubic lattices
34
ionic compound properties?
. hard - takes lot of energy to stratch surface, strong attractive forces . brittle - may split if hit in same direction as ion layers, ions may be displaces and same charge ions come together, repulsion . high mp and bp - strong attraction, increase with charge density (more attraction in 2+ and 2- than + and - ) . water soluble - can form ion-dipole bonds . only conduct electricity when molten or in solution
35
metals conduct electricity due to...
delocalised electrons
36
ionic giant structures conduct when liquid/aq solution due to...
mobile ions
37
metallic lattices?
. ions surrounded by a sea of electrons . often in hexagonal layers or in a cubic arrangement . malleable and ducile - forces acr in all directions, so bonds easily reform when layers slide . high tensile strength and hardness - strong attraction forces
38
what is an alloy?
a mixture of two or more metals or a metal with a non metal
39
brass
70% copper 30% zinc
40
why is brass stronger than copper
difference in Zn and Cu ion sizes makes lattice arrangement less regularly
41
pure aluminium properties
. softer than many metals . ductile . high electrical and thermal conductivity . low strength
42
aluminium alloys properties
. lightweight . strong . corrosion resistant
43
aluminium alloy uses
. aircraft bodies . cylinder blocks of car engines . bicycle frames
44
bronze
alloy of copper and tin
45
simple molecular lattices
. can form crystals . ice forms crystalline lattices . iodine has low melting point, weak im forces
46
giant molecular/covalent structure
. structures having a 3D network of covalent bonds throughout the whole structure . have high mps and bps - lots of covalent bonds . eg: graphite, diamond, silicon dioxide
47
what are allotropes?
different crystalline or moecular forms of the same element, eg graphite and diamond for carbon
48
graphite properties:
. high mp and bp - strong covalent bonding . soft - forces between carbon is weak, layers easily flake . good electrical conductor - has free electrons
49
graphite structure
. c atoms arranged in planar layers . within layers, c atoms in hexagons ONE C TO THREE C . fourth electrons of occupies p orbital . p orbitals overlap sideways . cloud of delocalised electrons clouds join form extended delocalised rings of electrons
50
diamond properties
. high mp and bp - strong covalent bonds . hard - hard to break 3D network of strong covalent bonds . doesn't conduct electricity - all four electrons bonded, no free . good heat conductor
51
diamond structure?
ONE C TO FOUR C . tetrahedral arrangement . network of C atoms extends unbroken . crystalline structure
52
artificial diamond
. too small of jewelry . used for drill tips . made by heating other forms of C under high pressure
53
silicon IV oxide
. many forms . found in mineral quartz . structure and properties to diamond . forms hard, colourless crystals with high mp and bp . doesn't conduct electricity . largely sand ONE SI TO FOUR O ONE O TO TWO SI
54
silicon IV oxide
. many forms . found in mineral quartz . structure and properties to diamond . forms hard, colourless crystals with high mp and bp . doesn't conduct electricity . largely sand ONE SI TO FOUR O ONE O TO TWO SI
55
what are fullerenes?
. allotropes of carbon in form of hollow spheres or tubes . structure of many is based on rings of carbon atoms, like graphite, in hexagons and sometimes pentagons . properties unlike graphite . dimensions between 0.1 and 100 nanometers ONE C TO THREE C
56
what is buckminsterfullerene?
. simple molecular structure of carbon . formula C60 . shape of football . C atoms arranged at corners at ends of 20 hexagons and 12 pentagons . bonds between two hexagons are shorter than those between hexagons and pentagons . has some delocalised electrons but less than graphite
57
what is buckminsterfullerene?
. simple molecular structure of carbon . formula C60 . shape of football . C atoms arranged at corners at ends of 20 hexagons and 12 pentagons . bonds between two hexagons are shorter than those between hexagons and pentagons . has some delocalised electrons but less than graphite
58
properties of buckminsterfullerene?
. low sublimation point - weak intermolecular forces . soft - not much energy required to overcome weak intermolecular forces . poor conductor of electricity - extent of electron delocalisation is lower . slightly soluble in solvents, unlike graphite and diamond . more reactive than graphite or diamond - bucky reacts with H, Cl, F, Br, O, due to relatively high electron density
59
what is a nanotube?
fullerene of hexagonally arranged carbon atoms like a single layer of graphite bent into the form of a cylinder
60
nanotube size
small diameter, long length
61
properties of nanotubes?
. have high electrical conductivity - have delocalised electrons . high tensile strength - 100 times stronger than steel . very high melting points - strong covalent bonding
62
uses of fullerenes
. buckminsterfullerene - trap small molecules in its cages, deliver drugs to certain parts of the body . nanotubes - as wires in tiny electrical circuits, electrons in thin batteries, treating types of cancer, clothing for added strength
63
what is graphene?
single isolated layer of graphite, layer is not entirely rigid and can be distorted
64
graphene properties
. most chemically reactive form of carbon . single sheets of graphene burn at very low temperatures, much more reative than graphite . extremely strong for its mass . conducts electricity and heat better than graphite
65
graphene uses
. uses in tiny electrical circuits . for tiny transistors . tiny touchscreen . tiny solar cells . tiny energy storages devices

chemistry (19 decks)

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