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Jasmines class > Chemistry SLOPS > Flashcards

Chemistry SLOPS Flashcards

1
Q

define atom

A

The smallest part of an element that can still be recognised as that element

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2
Q

define element

A

a substance made of only one type of atom

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3
Q

define compound

A

a substance made of two or more different atoms chemically bonded together

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4
Q

what does soluble mean?

A

dissolves in water

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5
Q

what does insoluble mean?

A

does not dissolve in water

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6
Q

describe the plum pudding model

A

ball of positive charge with electrons embedded in it

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7
Q

which scientist developed the plum pudding model

A

JJ Thomson

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8
Q

which discovery did the alpha particle scattering experiment lead to?

A

that atoms have dense nucleuses with a positive charge

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9
Q

what did Bohr propose about electrons

A

electrons orbit at set energy levels

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10
Q

which scientist provided evidence for neutrons in the nucleus

A

James Chadwick

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11
Q

3 subatomic particles

A

protons
neutrons
electrons

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12
Q

masses of subatomic particles

A

protons: 1
neutrons: 1
electrons: very small

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13
Q

the relative charges of the subatomic particles

A

protons: +1
neutrons: 0
electrons: -1

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14
Q

how are the subatomic particles arranged in an atom

A

protons and neutrons in the nucleus
electrons orbiting in shells

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15
Q

what is an isotope

A

atoms of the same element with a different number of neutrons

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16
Q

what is the overall charge of an atom neutral

A

there are the same number of protons as electrons

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17
Q

the overall charge of the nucleus

A

positive
only made up of protons and neutrons

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18
Q

what is the atomic number of an atom

A

the number of protons in an atom

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19
Q

what is the mass number of an atom

A

the number of protons and neutrons

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20
Q

the name of group 1

A

the alkali metals

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21
Q

the name of group 7

A

the halogens

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22
Q

the name of group 0

A

the noble gases

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23
Q

the trend in reactivity down group 1

A

increases down

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24
Q

the trend in reactivity down group 7

A

decreases down

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25
Q

how is the periodic table organised

A

atomic number and groups of elements with similar chemical properties

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26
Q

how was the old periodic table organised

A

by atomic weight

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27
Q

name the scientist who developed the modern periodic table

A

Mendeleev

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28
Q

what did Mendeleev do for undiscovered elements

A

he left gaps

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29
Q

what can the group number tell you about the electrons in an atom?

A

how many electrons in the outer shell

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30
Q

what are periods in the periodic table

A

the rows in the periodic table

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31
Q

what charge do electrons have

A

negative

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32
Q

why did Mendeleev leave gaps in his periodic table

A

for elements that had not been discovered yet

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33
Q

why did Mendeleev put some elements in groups

A

because they had similar chemical properties

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34
Q

why is group 0 highly unreactive

A

the have a stable arrangement of electrons
(full outer shell)

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35
Q

sodium + water ➡️

A

sodium hydroxide + hydrogen

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36
Q

sodium + chlorine ➡️

A

sodium chloride

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37
Q

sodium + oxygen ➡️

A

sodium oxide

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38
Q

the trend in boiling point down group 7

A

increases down the group

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39
Q

potassium bromide + chlorine ➡️

A

potassium chloride + bromine

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40
Q

what type of reaction is this?
potassium bromide + chlorine ➡️ potassium chloride + bromine

A

displacement reaction

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41
Q

how do you calculate the number of neutrons in an atom

A

mass number - atomic number

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42
Q

what is an ion

A

an atom which has lost or gained electrons

43
Q

how many electrons can go in the first shell

A

2

44
Q

how many electrons can go in the 2 and 3 shell

A

8

45
Q

what is the definition of a displacement reaction

A

a more reactive element will displace a less reactive element from a compound

46
Q

are halogens metals or non metals

A

non metal

47
Q

what colour flame is produced when potassium reacts with water

A

lilac

48
Q

group 7 are diatomic
what does this mean

A

they exist in molecules made up of pairs of atoms

49
Q

the colour and state of chlorine at room temperature

A

green gas

50
Q

the colour and state of iodine at room temperature

A

grey solid

51
Q

what happens to the number of electron shells down the group

A

increase in the number of shells

52
Q

state the charge of all elements in group 1 when they become ions

A

+1

53
Q

state the charge of all the elements in group 7 when they become ions

A

-1

54
Q

explain why group 1 gets more reactive down the group

A

atoms get bigger down the group
electrons are further away from the nucleus
lose an electron more easily

55
Q

explain why group 7 gets less reactive down the group

A

more shielding down the group
atoms get bigger down the group
electron further away from the nucleus
electron is gained less easily

56
Q

state the observation of sodium with water

A

fizzes
melts
floats
moves around the surface
disappears

57
Q

describe the structure of a giant ionic lattice

A

strong electrostatic forces of attraction between oppositely charged ions acting in all directions

58
Q

state the general melting/boiling points of ionic substances

A

high melting and boiling points

59
Q

why do ionic substances have high melting points

A

large amounts of energy needed to break the many strong bonds

60
Q

when can ionic compounds conduct electricity

A

when they are molten or dissolved
because the ions will be free to move

61
Q

state the type of bonding between non metals

A

covalent

62
Q

describe covalent bonding in terms of electrons

A

sharing of electrons

63
Q

do small covalent substances have high or low boiling points

A

low boiling points

64
Q

why do small molecules have low melting points

A

the weak intermolecular forces are easily overcome by a small amount of energy

65
Q

state the trend in intermolecular forces as molecules get bigger

A

as the molecule gets bigger, the intermolecular forces get stronger

66
Q

do small covalent molecules conduct electricity

A

no

67
Q

state the type of bonding in metals

A

metallic bonding

68
Q

describe the metallic bonding structure

A

strong electrostatic forces of attraction between positive ions and delocalised electrons

69
Q

state the general melting point of metals

A

high melting point

70
Q

four properties of metals

A

malleable
ductile
good conductors of heat and electricity
high melting points

71
Q

why are metals good conductors of thermal energy

A

energy is transferred by delocalised electrons

72
Q

what is an alloy

A

a mixture containing at least one metal

73
Q

describe why alloys are harder than pure metals

A

layers of atoms are distorted so layers cannot easily slide over eachother

74
Q

why are metals good conductors of electricity

A

delocalised electrons carry a charge and flow through the metal

75
Q

state the element, diamond, graphite and fullerenes are made from

A

carbon

76
Q

state the type of bonding between carbon atoms

A

covalent

77
Q

how many bonds does each carbon have in a diamond

A

4

78
Q

state 4 properties of diamond

A

very hard
high melting point
does not conduct electricity
insoluble

79
Q

how many bonds does each carbon have in graphite

A

3

80
Q

why is graphene soft

A

it has weak intermolecular forces between the layers so layers easily slide over each other

81
Q

state 4 properties of graphite

A

good conductor of electricity and heat
soft
high melting point and boiling point
insoluble

82
Q

what is one layer of graphite called

A

graphene

83
Q

what is a fullerene

A

molecules of carbon atoms with hollow shapes

84
Q

what is the name of the fullerene that has 60 carbons

A

buckminsterfullerene

85
Q

describe a carbon nanotube

A

a cylindrical fullerene with a very high length to diameter ratio

86
Q

what are nanotubes used for

A

electronics
nanotechnology
materials

87
Q

what is the law of conservation of mass

A

no atoms are lost or made during a chemical reaction
the mads of the products is equal to the mass of reactants

88
Q

what is crude oil

A

a mixture of very large number of compounds

89
Q

what is a finite resource

A

one that will run out

90
Q

first 4 alkanes

A

methane
ethane
propane
butane

91
Q

what is fractional distillation

A

a process used to separate mixtures of substances with different boiling points

92
Q

what is combustion

A

the reaction of fuel with oxygen

93
Q

when does incomplete combustion occur

A

when there is not enough oxygen present

94
Q

what are the 2 types of cracking

A

catalytic
steam

95
Q

how do you test for an alkene

A

react it with bromine water

96
Q

5 fuels we obtain from crude oil

A

petrol
diesel
kerosene
heavy fuel oil
liquified petroleum gases

97
Q

the longer the alkane, the ………. its boiling point

A

higher

98
Q

the longer the alkane, the ……….. it is

A

thicker or viscous

99
Q

the longer the alkane, the less ……………. it is

A

flammable

100
Q

are alkenes saturated or unsaturated

A

unsaturated

101
Q

what are the 2 types of chemical bonding

A

ionic
covalent
metallic

102
Q

what is the arrangement of ionic bonding

A

non metal and metal

103
Q

what is the arrangement of covalent bonding

A

2 non metals

104
Q

what is the arrangement of metallic bonding

A

2 metals

Jasmines class (6 decks)

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