Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

volume of a gas depends on:

A

. pressure in Pa
. temperature in K

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

volume relation to pressure?

A

volume = 1/pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

volume relation to temperature?

A

volume is directly proportional to temp

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

whats the formula?

A

pV=nRT

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

celsius to kelvin

A

+ 273

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

methods of calculating relative molecular mass?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

what is the melting point of a solid?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

to melt ionic compounds, need…

A

high temp (strong bonds)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

to melt molecular solids, need…

A

low temperature (weak intermolecular forces between particles)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

what is vaporisation?

A

the change in state when a liquid changes to vapour

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

what enthalpy change of vaporisation?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

what is condensation?

A

the change in state when a vapour change to a liquid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

are chnages in states reversible?

A

YES

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

what is vapour pressure?

A

the pressure exerted by a vapour in equilibrium with a liquid

28
Q

as vapour pressure increases, temp increases because..

A

. gas particles have more ke
. particles move faster and overcome intermolecular forces of attraction more easily

29
Q

what is the boiling point of a liquid?

A

the temperature at which it chnage to a gas at one atm

temperature at which vapor pressure = atmostpheric pressure

30
Q

1 atmosphere =

A

101 325 Pa

31
Q

why do crystals have a regular structure?

A

due to the regularly packed particles within the crystals - called a crystal lattice

32
Q

what is a lattice?

A

a regularly repeatinv arrangement of ions, atoms or molecules in 3D

33
Q

ionic lattices?

A

AKA giant ionic lattices
. depends on ion sizes
. MgO and NaCl have cubic lattices

34
Q

ionic compound properties?

A

. 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
Q

metals conduct electricity due to…

A

delocalised electrons

36
Q

ionic giant structures conduct when liquid/aq solution due to…

A

mobile ions

37
Q

metallic lattices?

A

. 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
Q

what is an alloy?

A

a mixture of two or more metals or a metal with a non metal

39
Q

brass

A

70% copper
30% zinc

40
Q

why is brass stronger than copper

A

difference in Zn and Cu ion sizes makes lattice arrangement less regularly

41
Q

pure aluminium properties

A

. softer than many metals
. ductile
. high electrical and thermal conductivity
. low strength

42
Q

aluminium alloys properties

A

. lightweight
. strong
. corrosion resistant

43
Q

aluminium alloy uses

A

. aircraft bodies
. cylinder blocks of car engines
. bicycle frames

44
Q

bronze

A

alloy of copper and tin

45
Q

simple molecular lattices

A

. can form crystals
. ice forms crystalline lattices
. iodine has low melting point, weak im forces

46
Q

giant molecular/covalent structure

A

. 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
Q

what are allotropes?

A

different crystalline or moecular forms of the same element, eg graphite and diamond for carbon

48
Q

graphite properties:

A

. high mp and bp - strong covalent bonding
. soft - forces between carbon is weak, layers easily flake
. good electrical conductor - has free electrons

49
Q

graphite structure

A

. 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
Q

diamond properties

A

. 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
Q

diamond structure?

A

ONE C TO FOUR C

. tetrahedral arrangement
. network of C atoms extends unbroken
. crystalline structure

52
Q

artificial diamond

A

. too small of jewelry
. used for drill tips
. made by heating other forms of C under high pressure

53
Q

silicon IV oxide

A

. 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
Q

silicon IV oxide

A

. 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
Q

what are fullerenes?

A

. 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
Q

what is buckminsterfullerene?

A

. 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
Q

what is buckminsterfullerene?

A

. 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
Q

properties of buckminsterfullerene?

A

. 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
Q

what is a nanotube?

A

fullerene of hexagonally arranged carbon atoms like a single layer of graphite bent into the form of a cylinder

60
Q

nanotube size

A

small diameter, long length

61
Q

properties of nanotubes?

A

. have high electrical conductivity - have delocalised electrons
. high tensile strength - 100 times stronger than steel
. very high melting points - strong covalent bonding

62
Q

uses of fullerenes

A

. 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
Q

what is graphene?

A

single isolated layer of graphite, layer is not entirely rigid and can be distorted

64
Q

graphene properties

A

. 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
Q

graphene uses

A

. uses in tiny electrical circuits
. for tiny transistors
. tiny touchscreen
. tiny solar cells
. tiny energy storages devices

chemistry (19 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions