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Chemistry GCSE Revision > atomic structure and the periodic table > Flashcards

atomic structure and the periodic table Flashcards

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1
Q

what are isotopes?

A

atoms of the same element that have a different number of neutrons

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2
Q

what is an example of an isotope

A

chloride 35 and chloride 17

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3
Q

what are the characteristics of chloride 35

A

18 neutrons
17 protons
17 electrons
abundance 75%

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4
Q

what are the characteristics of chloride 37

A

20 neutrons
17 protons
17 electrons
abundance 25%

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5
Q

why is the chloride on the periodic table called chloride 35.5 and not chloride 36?

A

the relative atomic mass is the average value for the isotopes of an element therefore

75% x 35 + 25% x 37 = 35.5

(abundance x atomic mass)

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6
Q

The atomic charge of of protons,neutrons and electrons (numbers)

A 
Protons = +1
Neutron = 0
Electrons = -1
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7
Q

The atomic mass of protons,neutrons and electrons

A 
Protons = 1
Neutrons = 1
Electrons = 1/2000  or negligible
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8
Q

what is found in the nucleus of an atom

A

protons and neutrons

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9
Q

what is found in the shells of an atom

A

electrons

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10
Q

what charge do protons,electrons and neutrons have

A 
protons = positive
electrons = negative
neutron = neutral
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11
Q

why is an atom neutral?

A

Atoms are neutral because they have equal numbers of positive protons and negative electron.

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12
Q

what is the mass number

A

number of protons and neutrons

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13
Q

what is the atomic number

A

number of protons

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14
Q

how do you calculate the number of neutrons?

A

mass number - atomic number

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15
Q

what are the elements on the left side of the periodic table called?

A

alkali metals

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16
Q

what are the elements on the right side of the periodic table called

A

non metals (have intermidiate chemical properties)

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17
Q

what is the special name for group 7 elements

A

halogens

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18
Q

what is the special name for group 8 / 0

A

noble gases

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19
Q

what is the ‘staircase’ on the right side of the periodic table called

A

metaloids / semi metals

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20
Q

what are they called semi metals?

A

Because they have properties of both metals and non metals

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21
Q

what are the elements in the middle called

A

transition metals

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22
Q

How are the metals arranged

A

In increasing atomic order

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23
Q

Groups are …

periods are …

A

vertical

horizontal

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24
Q

what do elements in the same group have in common?

A

Elements in the same group have similar properties e.g group 1 and group 7 because they have the same number of electrons in the outer shell

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25
Q

what can the last number in an electric configuration tell you

A

Number of electrons in the outer shell is the group number

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26
Q

what can all the numbers in an electric configuration tell you

A

Number of shells is the period number

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27
Q

what is a chemical reaction

A

The loss or gain of electrons

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28
Q

what is an ion

A

An atom that has loss or gained electrons

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29
Q

Metals always …

A

metals always LOSE electrons to form POSITIVE ions

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30
Q

None metals always ….

A

Non metals always GAIN electrons to form NEGATIVE ions

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31
Q

what does the electronic configuration become of an ion?

A

e. g 2.8.1 to 2.8 for metals

e. g 2.8.7 to 2.8.8 for non metals

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32
Q

how do you write an atom as an ion?

A

put brackets around it and add the charge

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33
Q

what is the ionic symbol of a metal

A

+

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34
Q

what is the ionic symbol of a non metal

A

_

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35
Q

Example of ions

A

Aluminium 2.8.3 Loses 3 becomes 2.8 = Al 3+

Oxygen 2.6 gains 2 becomes 2.8 = O2-

36
Q

oxidation

A

A chemical reaction with oxygen

37
Q

Group one the alkali metals reactivity

A

increases as you go down

38
Q

Balanced equation for lithium oxide

A

lithium + oxygen = lithium oxide

4 Li + O2 (small 2) = 2 Li (small 2) 2O

39
Q

lithium burns with a

A

red flame

40
Q

sodium burns with an

A

orange flame

41
Q

potassium burns with a

A

lilac flame

42
Q

what do the group 1 metals look like?

A

dull

43
Q

what do group one metals look like after you cut it?

A

shiny

44
Q

why are group one metals dull on the inside and dull on the outside?

A

Because the outside is the part of the metal that has been oxidised giving the dark colour,the shiny bit has not been oxidised.

45
Q

why are group one metals stored in paraffin oil?

A

To prevent oxidisation with the oxygen in the air / prevent reaction with oxygen

46
Q

what is a characteristic of the group one metals after cutting them as you go down the periods?

A

As you go down group one after you cut the metal the metals react quicker with oxygen / oxidise quicker

47
Q

why are group one metals called the alkali metals

A

because when you react them they create an alkali which can be found when using universal indicator which turns it blue/purple

48
Q

when lithium reacts with water what 3 things does it do?

A

Fizz
Float
Moves

49
Q

when sodium reacts with water what 3 things does it do?

A

Fizz
Float
Melts into a ball

50
Q

when potassium reacts with water what 3 things does it do?

A

Fizz
Float
Catches fire with a lilac flame

51
Q

Why are lithium,sodium and potassium denser than water

A

Because they float and they’re less dense than 1

52
Q

What gas is produced during the reaction with group one metals reacting with water?

A

Hydrogen gas to show there has been a reaction.

53
Q

Is the reaction with group one metals and water endothermic or exothermic

A

exothermic - produces heat

54
Q

equation for sodium reacting with water

A

sodium + water = sodium hydroxide

2Na + 2 H (small 2) 2O = 2NaOH + H (small 2 ) 2

55
Q

what would happen if you add universal indicator to the troph of water

A

When universal indicator is added the water in the troph will turn blue/purple because it’s an alkali solution

56
Q

what kind of molecules are the halogens

A

diatomic molecules (has 2 atoms)

57
Q

what happens to the reactivity in group 7 as you go down

A

the reactivity decreases

58
Q

what is the equation for when lithium reacts with chlorine

A

lithium + chlorine = Lithium chloride

2 Li + Cl (small 2) = 2 Li Cl

59
Q

what is the equation when sodium reacts with chlorine?

A

sodium + chlorine = sodium chloride

2 Na + Cl (small 2) = 2NaCl

60
Q

what is the equation for potassium reacting with chlorine

A

potassium + chlorine = potassium chlorine

61
Q

what is unique about the colours of the group seven vapours as you go down the table?

A

The colours get darker (possibly as dark as black)

62
Q

colours of the vapours group seven elements going down from fluorine

A 
Fluorine = pale yellow
Chlorine = green
Bromine - orange / brown
Iodine = grey / purple
Astatine = black
63
Q

what do the halogens give off

A

poisonous vapors

64
Q

what is unique about the state of the halogens at room tempreture

A

gas to liquid to solid

65
Q

what happens to the density of the halogens as you go down

A

increases

66
Q

reaction with chlorine and iron wool

A

iron wool burns and glows brightly

67
Q

reaction with bromine and iron wool

A

iron wool glows but less brightly than chlorine

68
Q

reaction with iodine and iron wool

A

iron wool has a slight glow

69
Q

equation for chlorine reacting with iron

A

chlorine + iron = iron (III) chloride

3Cl (small 2) + 2Fe = 2FeCl (small 3)

Iron = Fe3+

70
Q

what is a flame test used for?

A

identifies the presence of a metal ion

71
Q

flame test for lithium

A

red / crimson

72
Q

flame test for sodium

A

yellow /orange

73
Q

flame test for potassium

A

lilac

74
Q

flame test for calcium

A

brick red

75
Q

flame test for copper

A

blue /green

76
Q

flame test for barium

A

Apple green

77
Q

what is the silver nitrate test used for

A

identifies the presences of a halide ion e.g chlorine, bromide,iodide

78
Q

what is the equation for silver nitrate

A

AgNo3 (small 3)

79
Q

equation for chlorine and silver nitrate

A

Ag+ + Cl- = AgCl

80
Q

equation for bromide and chlorine

A

Ag+ + Br- = AgBr

81
Q

equation for iodide and chlorine

A

Ag+ + I- = AgI

82
Q

precipitate of chlorine

A

white

83
Q

precipitate of bromide

A

cream

84
Q

precipitate of iodide

A

pale yellow

85
Q

How do you detect hydrogen gas

A

place a lit splint and listen for a sqeaky pop

86
Q

what is used in the sqeaky pop test

A

magnesium metal and hydrochloric acid

Chemistry GCSE Revision (1 decks)

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