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Chemistry > All of year 9 > Flashcards

All of year 9 Flashcards

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1
Q

What are the 3 states of matter

A

liquid
solid
gas

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2
Q

what does each sate of matter depend on

A

how strong the forces of attraction are between the particles of the material

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3
Q

descirbe the arrangement in solids and why

A

very regular because of the strong forces of attraction holding them together

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4
Q

describe the movement of solid particles

A

they don’t move but do vibrate about a fixed point whilst keeping a definite shape and volume

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5
Q

what happens when materials are heated

A

the particles vibrate/move more gaining energy causing the material to expand

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6
Q

describe the arrangement and movement of liquids

A

weak forces of attraction cuase the particles to be random and free to move over each other and fill the bottom of the container

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7
Q

desribe the arrangement of gas particles

A

very weak forces allow the particles to be free to move and be far apart filling any container

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8
Q

What happens when gases are heated

A

they either expand or the pressure is increased

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9
Q

what is the process where a solid becomes liquid

A

melting

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10
Q

what is the process where a liquid becomes a solid

A

freezing

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11
Q

what is the process where a liquid becomes a gas

A

evaporating

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12
Q

what is the process where a gas becomes a liquid

A

condensing

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13
Q

what is the process where a solid becomes a gas

A

subliming

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14
Q

what is diffusion

A

the gradual movement of gas or liquid particles from places where there are lots to places where there are fewer

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15
Q

In a diffusion experiment with ammonia and hyrogen chloride why is the ring of ammonium chloride not in the center

A

becuase the hydrogen chloride particles are denser than the ammonium particles - they take longer to move

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16
Q

what is a solution

A

a mixture of solvent and solute that does not seperate out

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17
Q

what is a solute

A

the substance being dissolved

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18
Q

what is a solvent

A

the liquid the solute dissolves into

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19
Q

what is a saturated solution

A

a solution where the maximum amount of solute has been dissolved

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20
Q

what is solubility

A

the measure of how much solute will dissolve in 100g of solvent

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21
Q

how do you calculate solubility

A

(mass of solid / mass of water removed) x 100

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22
Q

How can you investigate how temperture affects solubility

A
  • weigh empty evaporating basin
  • pour some solution in basin
  • re-weigh basin
  • heat with bunsen burner
  • re-weigh pure substance once water evaportated
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23
Q

define isotope

A

isotopes are different atomic forms of the same element, which have the same number of protons but a different number of neutrons

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24
Q

what does the atomic number of an element tell you

A

how many protons

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25
Q

how can you find out the group number of an element

A

the number of electrons on the outer shell

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26
Q

how can you find out the period of an element

A

the number of occupied shells

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27
Q

what is an element

A

an element consists of only one atom

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28
Q

what is a compound

A

compounds are chemically boned elements (two or more)

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29
Q

what is a mixture

A

mixtures are easily seperated: there is no chemical bond

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30
Q

how can you tell if something is a pure substance

A

because it will have a speecific, sharp melting and boiling point

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31
Q

What is filtration used for

A

to seperate an insoluable solid from a liquid

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32
Q

what is crystallisation used for

A

to seperate a soluable solid from a solution

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33
Q

what do you need to perform filtration

A

beaker
funnel
filter paper

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34
Q

what is the mixture that stays in the filter paper call

A

the residue

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35
Q

how does crystallisation work

A
  • pour mixture into evapourating dish
  • heat solution ~ water will evapourate
  • once water evaporated leave dish to cool and dry
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36
Q

why does chromatography work when seperating mixtures

A

becuase dyes in the mixture move up the paper at different rates

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37
Q

how do you preform chromotagraphy

A
  • draw base line wiht pencil
  • add spots of ink to baseline
  • loosely roll paper and put in beaker with some water (ensure the baseline is above water level)
  • once dyes have spread take out to dry
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38
Q

how do you calculate the Rf value

A

distance travelled by solute / distance traveled by solvent

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39
Q

when is simple distillation used

A

to seperate out solutions

40
Q

when is fractional distillation used

A

to seperate out a mixture of liquids (with similar boiling points)

41
Q

how does simple distillation work

A
  • solution is heated
  • part of solution with lowest BP evapourates
  • vapour is cooled and condenses and collected in beaker
  • rest of solution is left in falsk
42
Q

What do you need to conduct distillation

A

flask
bung
thermometer
beaker
liebig condenser with water jacket
bunsun buner
tripod

43
Q

what is the relative charge of a proton

A

+1

44
Q

what is the relative charge of a neutron

A

0

45
Q

what is the relative charge of an electron

A

-1

46
Q

What is the relative mass of a proton

A

1

47
Q

What is the relative mass of a neutron

A

1

48
Q

What is the relative mass of an electron

A

0.0005

49
Q

what does the mass number of an element tell you

A

how many protons and neutrons there are

50
Q

how do you calculate the relative atomic mass of isotopes

A

((mass number x percentage) + (mass number x percentage)) / 100

51
Q

Why are the elements lower down in the group most reactive

A

becuase the outermost electron is further from the nucleus so the attraction is less

52
Q

What is a negative ion called

A

an anion

53
Q

what is a positive ion called

A

a cation

54
Q

what is an ion

A

an atom with a charge

55
Q

describe ionic bonding

A
  • metal + non-metal react to get complete outer shell
  • metal loses electron(s) forming a cation
  • non-metal gains the electron(s) forming an anion
  • oppositely charged ions are strongly attracted by ellectrostatic forces causing the bond
56
Q

define ionic bonding

A

the electrostatic forces of attraction between two oppositely charged ions

57
Q

why do ionic compounds have high MP and BP

A

becuase the a lot of energy is needed to overcome the strong attraction

58
Q

can ionic compounds conduct electricity

A

yes but only when molton or dissolved becuase the ions have to be free to maove and carry the charge

59
Q

How are metals held together

A

by metallic bonding

60
Q

describe a metallic bond

A

a giant structure of positive metal ions surrounded by a sea of delocalised electrons

61
Q

what does this diagram show

A

metallic bonding

62
Q

define metallic bonding

A

the strong electrostatic forces of attraction between metal ions and delocalised electrons

63
Q

why can metals conduct electricity

A

because the delocalised electrons can move to carry a charge

64
Q

why are metals malleable and ductile

A

becuase the layers of metal ions can slide as the atoms are all the same size

65
Q

what is the state symbol for solid

A

(s)

66
Q

what is the state symbol for liquid

A

(l)

67
Q

what is the state symbol for gas

A

(g)

68
Q

what is the state symbol for dissolved in water (aqueous)

A

(aq)

69
Q

what are metal ores

A

reactive metals found in the earths crust that have enough metal to be extracted from their ore

70
Q

what is the reactivity series

A

Potassium
Sodium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Silver
Gold

71
Q

how are metals more reactive than carbon extracted

A

using electrolysis

72
Q

what is the word equation for rusting

A

iron + oxygen + water –> hydrated iron(III) oxide

73
Q

What are the the two methods to prevent rusting

A

barrier methods
sacrificial methods

74
Q

What are barrier methods to pevent rusting

A

painting
oiling

75
Q

what are sacrificial methods to prevent rusting

A

galvanising

76
Q

what is galvanising

A

when a coating of zinc is sprayed onto an object so that the whole object will not rust

77
Q

define covalent bonding

A

the electrostatic forces of attraction between the shared pair of electrons and the nuclei of the bonding atoms

78
Q

describe covalent bonding

A
  • non-metals react together to get full outer shell
  • they share electrons
79
Q

what are intermolecular forces

A

simple covalent substances have intermoleccular forces, these are the forces between the covalent molecules themselves

80
Q

if a covalent molecule has a high melting point what are the intermolecular forces like

A

strong

81
Q

if a covalent molecule has a low melting point what are the intermolecular forces like

A

weak

82
Q

do covalent molecules conduct electricity

A

no becuase there are no free moving charged particles

83
Q

what are the three most important giant covalent structures

A

diamond
graphite
sand

84
Q

what is diamond made up of

A

carbon

85
Q

what is graphite made up of

A

carbon

86
Q

what is sand made up of

A

silicon and oxygen

87
Q

describe graphites intermolecular forces

A

weak but still present

88
Q

why can you write with graphite

A

becuase the weak intermolecular forces between the layers

89
Q

Why does graphite have a slippery feel

A

because weak intermolecular forces hold the layers of carbon atoms together, therefore making the layers able to slide and graphite has delocalised electrons as well so it can conduct

90
Q

why do giant molecular structures have high boiling and melting points

A

because they require a lot of energy to overcome the strong covalent bonds

91
Q

What is the structure of diamond like

A

tetrahedral

92
Q

what is the structure of graphite like

A

hexagonal layers

93
Q

Why is diamond hard

A

because the tetrahedral stucture allow external forces to be spread throughout the lattice and the forces of attraction are stong so they require a lot of energy to overcome

94
Q

why is graphite soft

A

because weak forces between layers allow to slide easily

95
Q

why does graphite conduct electricity

A

there are delocalised electrons between the layers

Chemistry (15 decks)

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