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science end of chemistry test Flashcards

1
Q

what is the definition of an atom

A

the smallest neutral part of an element that can take part in chemical reactions

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2
Q

what is the definition of an element

A

made up of one type of atom

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3
Q

what is the definition of a compound

A

different types of elements that are chemically combined

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4
Q

what is the definition of a molecule

A

two or more elements joined together

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5
Q

what is the definition of a mixture

A

two or more substances/elements/compounds that are not chemically combined. can be separated

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6
Q

what is the definition of chemical change

A

when a reaction occurs between two or more substances to create a new chemical

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7
Q

what is the definition of physical change

A

a change where no new substances are formed

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8
Q

what is chromotography

A

used to separate mixtures of coloured compounds. separated based on density, lower the density the further it travels up the paper

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9
Q

what is magnetism

A

used to separate magnetic metals from non-magnetic substances

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10
Q

what is crystallisation

A

used to separate dissolved salts from their solvent. heating the solution evaporates the the solvent leaving the salt crystals

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11
Q

what is a separating funnel

A

used to separate immiscible liquids. opening the tap on the funnel allows the less dense bottom layer to flow through. tap can be closed when top layer reaches bottom

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12
Q

what is filtration

A

used to separate insoluble solids from liquids, solid residue left in filter paper and filtrate passes through

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13
Q

what is simple distillation

A

used to separate miscible liquids based on different boiling points. liquid with lower boiling point boils first and gas passes down condenser, cools and condenses again

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14
Q

what is fractional distillation

A

liquids will evaporate and rise up the column, liquid with the highest boiling point will condense on beads and drip back down while lowest boiling point will rise and pass into the condenser

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15
Q

who developed the atom in 460bc

A

democritus

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16
Q

what did democritus do

A

first to have the idea that everything was made of particles called atoms

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17
Q

who developed the atom in 1803

A

john dalton

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18
Q

what did john dalton do

A

he described atoms as like billiard balls and said atoms of the same element were identical. thought they could not be split

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19
Q

who developed the atom in 1897

A

jj thomson

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20
Q

what did jj thomson do

A

discovered the electron by passing high voltage electricity through gases. proposed the plum pudding model of atom, ball of positive charge with negative electrons embedded in it

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21
Q

who developed the atom in 1909

A

rutherford and marsden

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22
Q

what did rutherford and marsden do

A

fired positive alpha particles at a thin gold foil, expected all to pass through, some deflected and others bounced back. plum pudding model ditched for nuclear model, positive nucleus surrounded by negative atoms

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23
Q

who developed the atom in 1912

A

niels bohr

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24
Q

what did niels bohr do

A

agreed with the nuclear model and suggested that electrons orbited at specifiic distances. we call these shells

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25
Q

who devloped the atom in 1920

A

ernest rutherford

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26
Q

what did ernest rutherford do

A

suggested the name proton for hydrogen nuclei

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27
Q

who developed the atom in 1932

A

james chadwick

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28
Q

what did james chadwick do

A

proved the existence of the neutron and measured its mass

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29
Q

what is the radius of an atom

A

0.1nm

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30
Q

what proportion of a nucleas is that of an atom

A

1/10,000

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31
Q

how do you convert nm to m

A

multiple by 10^-9

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32
Q

how do you convert m to nm

A

divide by 10^-9

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33
Q

what are isotopes

A

atoms of the same element with the same number of protons and electrons but different numbers of neutrons

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34
Q

how do you work out relative atomic mass

A

total mass of all atoms of that element / total number of atoms of that element

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35
Q

what are the rules of electronic structure

A

always fill the shell from the centre
first shell can hold 2 electrosn
second can hold 8
third can hold 8 before the fourth starts to fill up

36
Q

who developed the periodic table in 1817

A

johann döbreiner

37
Q

what did john döbreiner do

A

noticed groups of elements of similar properties so put forward his law of triads. examples were lithium, sodium and potassium

38
Q

who developed the periodic table in 1864

A

john newlands

39
Q

what did john newlands do

A

ordered elements by atomic mass and noticed patterns every 8 elements so he proposed law of octaves. ideas were rejected order went wrong after calcium , unreactive copper in the same group as reactive lithium, sodium and potassium

40
Q

who developed the periodic table in 1869

A

dmitri mendeleev

41
Q

what did dmitri mendeleev do

A

also ordered elements by atomic mass but left gaps for elements that hadn’t yet been discovered. swapped order of some elements so that properties fit the pattern. mendeleev didn’t know about subatomic particles, we now know he put in order of atomic number. mendeleev’s table didn’t contain noble gases because they hadn’t been discovered

42
Q

how reactive are noble gases and why

A

they are unreactive because they have a full shell of outer electrons and don’t want to lose or gain any electrons

43
Q

how does density change with noble gases

A

increases as you go down the group

44
Q

how does boiling point change with noble gases

A

increases going down the group, more weak forces of attraction so more energy is required to break them apart

45
Q

how does lithium react with water

A

fizzes and floats

46
Q

how does sodium react with water

A

fizzes, floats, melts and sometimes a yellow flame is seen

47
Q

how does potassium react with water

A

fizzes, floats, melts and burns with a lilac flame

48
Q

word equation for alkali metal in water

A

metal + water –> metal hydroxide + hydrogen

49
Q

symbol equation for alkali metal in water

A

2Li + 2H⬇️20 –> 2LiOH + H⬇️2

50
Q

word equation for alkali metal with oxygen

A

metal + oxygen –> metal oxide

51
Q

symbol equation for alkali metal with oxygen

A

4Li + O⬇️2 –> 2Li⬇️2O

52
Q

word equation for alkali metal with chlorine

A

metal + chlorine –> metal chloride

53
Q

symbol equation for alkali metal with chlorine

A

2Li + Cl⬇️2 –> 2LiCl

54
Q

How do alkalis change as go down the group and why

A

They get more reactive because their outer electron is further away meaning it can be lost easier

55
Q

What is an ion

A

A charged particle that has either lost or gained an electron

56
Q

What ions do alkalis metals form

A

A +1 ion

57
Q

What is fluorine

A

A pale yellow gas

58
Q

What is chlorine

A

A pale green gas

59
Q

What is bromine

A

A dark brown liquid

60
Q

What is iodine

A

A grey solid with purple vapours

61
Q

How do halogens exist as

A

Diatonic molecules e.g. F⬇️2

62
Q

Word equation for halogen with hydrogen

A

Halogen + hydrogen –> hydrogen halide

63
Q

Symbol equation for halogen with hydrogen

A

Cl⬇️2 + H⬇️2

–> 2HCl

64
Q

Word equation for halogens with metals

A

Halogen + metal

–> metal halide

65
Q

Symbol equation for halogens with metals

A

Cl⬇️2 + 2Na –> 2NaCl

66
Q

What takes place during a halogen displacement reaction

A

A colour change

67
Q

What displaces what in a halogen reaction

A

A more reactive halogen displaces a less reactive one to form a compound

68
Q

How does reactivity change as you go down the halogens and why

A

They become less reactive because it is harder to gain an electron

69
Q

what is the order of reactivity for halogens

A

fluorine > chlorine > bromine > iodine

70
Q

example of word halogen displacement reaction

A

chlorine + sodium bromide –> sodium chloride + bromine

71
Q

example of symbol halogen displacement reaction

A

Cl⬇️2 + 2NaBr –> 2NaCl + Br⬇️2

72
Q

what type of ion do halogens form

A

a -1 ion because they all gain 1 electron

73
Q

melting point of transition and alkali metals

A

transition metals have high, alkali metals have low

74
Q

density of transition and alkali metals

A

transition metals have high, alkali metals have low

75
Q

physical structure of transition and alkali metals

A

transition metals are strong and hard, alkali metals are soft

76
Q

reactivity of transition and alkali metals

A

transition have low reactivity, alkali metals have high

77
Q

types of ions of transition and alkali metals

A

transition metals react to form ions with different charges, alkali metals react to form +1 ions

78
Q

compounds of transition and alkali metals

A

transition metals form coloured compounds, alkali metals form white ones

79
Q

what is a property that only transition metals have

A

they act as catalysts

80
Q

what properties do transition and alkali metals have in common

A
  • good conductors of heat
  • good conductors of electricity
  • shiny
81
Q

do transtion metals react with oxygen and chlroine like alkali metals do

A

yes but more slowly

82
Q

word equation for a metal reacting with oxygen

A

metal + oxygen –> metal oxide

83
Q

symbol equation for a metal reacting with oxygen

A

2Cu + O⬇️2 –> CuO

84
Q

word equation for a metal reacting with chlorine

A

metal + chlorine –> metal chloride

85
Q

symbol equation for a metal reacting with chlorine

A

2Fe + 3Cl⬇️2 –> 2FeCl⬇️2

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