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chemistry paper 1 > atomic structure and the periodic table > Flashcards

atomic structure and the periodic table Flashcards

1
Q

what is an element

A

made up of one type of atom

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2
Q

what is a compound

A

contain 2 or more different elements chemically bonded together

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3
Q

what does magnesium sulphide form

A

white crystals

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4
Q

what is a mixture

A

in a mixture there are different compounds or elements but are not chemically combined

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5
Q

how do we separate a mixture

A

physical separation

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6
Q

what are 4 types of physical separation

A

filtration
chromatography
crystallisation
distillation

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7
Q

what is a molecule

A

have the same element combine

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8
Q

what does insoluble mean

A

that the solid will not dissolve in a liquid

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9
Q

what is filtration used for

A

to separate an insoluble solid from a liquid

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10
Q

what is crystallisation used for

A

to separate a soluble solid from a liquid

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11
Q

what does aqueous mean

A

dissolved in water

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12
Q

what is fractional distillation used for

A

separate a mixture of different liquids

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13
Q

what happens if two liquids have a similar boiling point in fractional distillation

A

it will be harder to separate them

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14
Q

when were electrons discovered

A

1897

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15
Q

what is the plum pudding model

A

-ball of positive charge
-negative electrons embedded in it

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16
Q

what experiment was carried out to find out if the plum pudding model was correct

A

alpha scattering experiment

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17
Q

what is the alpha scattering experiment

A

-first scientist took a piece of gold foil
-scientist then fired alpha particles through the gold foil
-most particles passed through
some particle were deflected
-some particles bounced back

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18
Q

why was gold foil used

A

because gold can be hammered into very thin foil

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19
Q

what is the charge of the alpha particle

A

positive- so other positive particle will be repelled

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20
Q

what did they discover when most of the particle passed through

A

mostly empty space

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21
Q

what does it mean when some particles were deflected during the alpha scattering experiment

A

centre of the atom had a positive chargre

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22
Q

why did some particles bounce back

A

centre of atom must contain mass

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23
Q

what replaced the plum pudding model

A

the nuclear model

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24
Q

what is the nuclear model

A

mostly empty space
positive nucleus
negative electrons

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25
Q

why do atoms have no overall charge

A

number of protons is equal to number of electrons

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26
Q

what did Niels Bohr propose

A

that the electrons orbit the nucleus at specific distances

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27
Q

what did James Chadwick discover

A

the nucleus contained neutral particles that are called neutrons

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28
Q

radius of atom

A

1x10 -10m

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29
Q

radius of nucleus

A

1x10 -14

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30
Q

relative charge of proton

A

+1

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31
Q

relative charge of neutron

A

0

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32
Q

relative charge of electron

A

-1

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33
Q

relative mass of proton

A

1

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34
Q

relative mass of neutron

A

1

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35
Q

relative mass of electron

A

very small

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36
Q

what is an isotope

A

atoms of the same element with same number of protons different number of neutrons

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37
Q

what are ions

A

ions are atoms that have an overall charge, that is because ions have gained or loss electrons

38
Q

negative ions

A

gained electrons

39
Q

positive ions

A

lost electrons

40
Q

what does the mass number tell

A

total number of proton and neutrons

41
Q

what does the atomic number tell

A

number of protons

42
Q

what is paper chromatography

A

separates mixtures based on their different solubilities

43
Q

what is a solvent

A

liquid that will dissolve substances

44
Q

what is the mobile phase

A

solvent

45
Q

what is the stationary phase

A

paper

46
Q

what will a pure compound produce on chromatography paper

A

single spot

47
Q

what does the group number tell

A

number of electrons on the outer shell

48
Q

what are group 1

A

highly reactive metals

49
Q

what are the triads

A

elements with similar properties often occurred in threes

50
Q

what did Newlands do

A

arranged the elements in order of increasing atomic weight

51
Q

what is the law of octaves

A

every 8th element reacted in a similar way

52
Q

what were the problems with the law of octaves

A

-elements were grouped together with different propties

53
Q

what did Dmitri Mendeleev do

A

developed the first modern periodic table
-arranged elements in increasing atomic weight

54
Q

what did Dmitri Mendeleev do that other scientist had not done before

A

switch the order of elements so they fitted pattern of other elements in the same group
- he left gaps as he released some elements had not been discovered yet

55
Q

how is the modern periodic table

A

elements arranged in order of atomic number

56
Q

what had not been discovered when Mendeleev made his periodic table

A

protons

57
Q

what is a problem with ordering with atomic weight

A

elements can appear in wrong order due to isotopes
puts element in wrong group

58
Q

what is group 0 called

A

noble gases

59
Q

why are the noble gases unreactive

A

have a full outer shell
atoms are stable when they have a full outer shell

60
Q

what are noble gases boiling point

A

lower than room temperature

61
Q

how does the b.p of the noble gases change

A

the boiling point of noble gases increases down the group ( as the relative atomic mass increases)

62
Q

what happens when metal reacts

A

when metal reacts they loose electrons `to achieve a full outer shell

63
Q

what ions do metal form

A

positive

64
Q

what are group 1 metal called

A

alkali metals

65
Q

properties of group 1 metal

A

soft

66
Q

how do group 1 metals react with oxygen

A

react rapidly with oxygen

67
Q

what forms when oxygen reacts with group 1

A

oxide

68
Q

what happens when lithum reacts with oxygen

A

the outer shell of lithium moves to the oxygen atom lithium will now have a full outer shell lithium becomes an ion

69
Q

what do group 1 metals react rapidly with

A

-oxygen
-chlorine
-water

70
Q

what happens when a group 1 metal reacts with water

A

reacts rapidly with water
the water bubbles so therefore a gas is being produced
an alkali solution is produced because the universal indicator turns purple

71
Q

why does group 1 metals get more reactive going down the group

A

-radius of the atom of the increases this means there is a greater distance between positive nucleus and outer electron
- as the distance increases the outer electron is less attracted to the nucleus

72
Q

what is shielding

A

outer electron is repelled by electrons in internal energy level

73
Q

what are group 7 called

A

halogens

74
Q

what happens down the group 7

A

relative molecular mass increases

75
Q

what is a covalent bond

A

shared pair of electrons

76
Q

what has a melting point lower than 20 degrees

A

liquid

77
Q

what has a meting point and boiling point above 20 degrees

A

solid

78
Q

what has a boiling point lower than 20 degrees

A

gas

79
Q

what do group 7 elements form when they react with other non metals

A

covalent compounds

80
Q

what happens when halogens react with metals

A

they form ionic compounds

81
Q

when happens when a halogen reacts with a metal

A

halogen atom gains 1 electron and forms an ion with a -1 charge

82
Q

what are outer electrons attracted to

A

positive nucleus

83
Q

what happens down group 7

A

level of shielding increases

84
Q

what does an increased distance shielding mean

A

electrons in the internal level repel the outer electrons

85
Q

what can a reactive halogen replace

A

a less reactive halogen

86
Q

properties of group 1 metals

A

soft
low melting point
low density

87
Q

properties of transition metals

A

hard and strong
high melting point
high density
less reactive

88
Q

what do transition metals form

A

coloured compounds

89
Q

what transition elements useful for

A

catalyst

90
Q
A

chemistry paper 1 (4 decks)

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