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Chemistry GCSE > Atomic Structure and the Periodic Table > Flashcards

Atomic Structure and the Periodic Table Flashcards

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1
Q

What is in the nucleus?

A

Protons and Neutrons

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2
Q

Electrons _____ the nucleus in ______ ____

A

Orbit

Electron shells

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3
Q

Atoms have the same number of _______ and _______

A

Protons

Electrons

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4
Q

Why do atoms have no charge?

A

The positive charge of the protons cancel out the negative charge of the electrons
Neutrons have no charge

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5
Q

Mass of neutron:

A

1

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6
Q

Mass of proton:

A

1

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7
Q

Mass of electron:

A

Very small 0.000000005

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8
Q

Charge of proton:

A

+1

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9
Q

Charge of neutron:

A

0

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10
Q

Charge of electron:

A

-1

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11
Q

What is the mass number of an element?

A

The total number of protons and neutrons in the nucleus of the atom

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12
Q

What is the atomic number of an element?

A

The number of protons in the nucleus of the element

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13
Q

What are isotopes?

A

Different forms of an element, that have the same number of protons but a different number of neutrons

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14
Q

What is a compound?

A

A substance made from 2 or more elements that are chemically bonded

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15
Q

What is needed to separate compounds into its original elements?

A

A chemical reaction

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16
Q

What is a mixture?

A

Elements that are mixed together - no chemical reaction

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17
Q

Can a mixture be seperated out?

A

Yes by physical methods

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18
Q

Properties of ________ are usually different from the properties of the ________ element

A

Compounds

Original

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19
Q

Properties of ________ are a mix of the properties of the ________

A

Mixtures

Elements

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20
Q

What is chromatography used to separate?

A

Mixtures (of coloured compounds such as dyes)

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21
Q

What is the solvent?

A

The liquid

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22
Q

Why use a pencil to mark during chromotography?

A

Its insoluble

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23
Q

Why should the compounds NOT touch the solvent?

A

The compounds will dissolve in it

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24
Q

What will the movement of a dye be if its insoluble?

A

It will stay on the baseline

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25
Q

What is filtration used to separate?

A

Insoluble solids from liquids

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26
Q

What is evaporation used to separate?

A

Solids from solutions

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27
Q

What dish is used during evaporation?

A

An evaporating dish

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28
Q

What is crystallisation used to separate?

A

Soluble solids from solutions if the salt decomposes when heated

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29
Q

When does evaporation not work?

A

If the salt decomposes when heated

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30
Q

During crystallisation what do you do after evaporating the solution to form salt crystals?

A

Filter the crystals out of the solution

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31
Q

How do you separate rock salt?

A

Dissolve the salt in water
Filter the mixture - removes rock
Evaporate the water - leaves salt as crystal

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32
Q

What is distillation used to separate?

A

Mixtures which contain liquids

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33
Q

What is simple distilliation used to separate?

A

A liquid from a solution

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34
Q

What is fractional distillation used to separate?

A

A mixture of liquids (more than 1)

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35
Q

Simple distillation can only be used to separate things with …….

A

Very different boiling points

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36
Q

What happens during simple distillation?

A

The solution is heated - liquid with lowest boiling point evaporates
Vapour is cooled by a condenser and collected

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37
Q

What happens during fractional distillation?

A

Heat the mixture
Different liquids evaporate at different temps
When one liquid evaporates at its boiling point, it will reach the top of the column
Other liquids that start evaporating will only get a certain way before condensing

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38
Q

John _______ said that all matter was made up of ______ which are _____ ______

A

Dalton
Atoms
Solid spheres

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39
Q

What did JJ Thompson conclude?

A

The plum pudding model

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40
Q

Who thought of the plum pudding model?

A

JJ Thompson

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41
Q

What is the plum pudding model?

A

That an atoms a ball of positive charge with negatively charged electrons stuck inside it

42
Q

Who conducted the alpha particle scattering experiment?

A

Ernst Rutherford

43
Q

What did Ernst Rutherford do?

A

He fired positively charged alpha particles at a thin sheet of gold

44
Q

What was assumed would happen in the alpha particle scattering experiment?

A

That particles would pass through the sheet or be slightly deflected at most

45
Q

What actually happened in the alpha particle scattering experiment?

A

Some particles were deflected more than expected and a small number were deflected backwards while most did go straight through

46
Q

How is the nuclear model used to explain the alpha particle scattering experiment?

A

The atom has a tiny positively charged nucleus at the centre, where most of the mass is concentrated
A ‘cloud’ of negatively charged electrons surround the nucleus with most of the atom being empty space

47
Q

Why were some particles deflected backwards in the alpha particle scattering experiment?

A

Because, when the alpha particles came near the concentrated positive charge of the nucleus, they repelled (alpha particle is positively charged)

48
Q

What did Neils Bohr realise?

A

That if there is a ‘cloud’ of electrons, the electrons would be attracted to the nucleus, causing the atom to collapse

49
Q

What did Neils Bohr suggest?

A

That electrons orbit the nucleus in fixed shells

50
Q

Who suggested that electrons orbit the nucleus in fixed shells?

A

Niels Bohr

51
Q

Who discovered the nucleus?

A

James Chadwick

52
Q

How many electrons can go in each shell?

A

2
8
8

53
Q

Atoms want to have a ___ outer shell of electrons

A

Full

54
Q

Who had the atomic theory (periodic table)?

A

John Dalton

55
Q

Who decided to group elements into Traids?

A

Johann Dobereiner

56
Q

How did Johann Dobereiner group elements?

A

He grouped them into triads, based on similar appearance and reactions

57
Q

Who decided to group elements into the Law of Octaves?

A

John Newlands

58
Q

How did John Newlands group elements?

A

He grouped them into the Law of Octaves, in the order of their relative atomic mass

59
Q

Who arranged the Table of Elements?

A

Dimitri Mendeleev

60
Q

How did Mendeleev order elements?

A

In order of increasing atomic weight but switched and placed some out of order to appear in the same column as other elements with similar properties

61
Q

Why did Mendeleev reorder some elements?

A

So that elements would be in the same column as other elements with similar properties

62
Q

Why did Mendeleev leave spaces?

A

For atoms that are yet to be discovered - gaps allowed Mendeleev to predict the properties of these undiscovered elements

63
Q

What discovery confirmed that Mendeleev was correct to not place elements in a strict order of atomic mass?

A

Isotopes

64
Q

What did the discovery of isotopes confirm?

A

That Mendeleev was correct to not place elements in a strict order of atomic mass

65
Q

What are atoms in order of in the modern periodic table?

A

Increasing atomic (proton) mass

66
Q

What does the group number tell?

A

How many elements there are in the outer shell

67
Q

What does the way atoms react depend on?

A

How many electrons there are in the outer shell, groups reacts similarly

68
Q

Properties of metals:

A

Strong
Malleable
Good conductors of heat and electricity
High melting and boiling points

69
Q

Properties of non-metals:

A 
Dull
Brittle
Not always solid at room temp
Don't generally conduct
Generally have a lower density
70
Q

What are unique about transition metals?

A

They can have more than one ion
They are often coloured so compounds that contain them are colourful
They often make good catalysts

71
Q

What are Group 1 metals called?

A

Alkali metals

72
Q

Properties of alkali metals:

A

Soft

Low density

73
Q

As you go down Group 1:

A

Higher relative atomic mass
Lower melting and boiling points
Increasing reactivity

74
Q

Why does the reactivity of alkali metals increase as you go down the group?

A

The outer electron is lost more easily as the attraction between the outer shell electron and the nucleus decreases because the electron is further away from the nucleus as you go down the group, meaning there is more electron shielding, so not as much energy is needed to lose the other electron to form a full outer shell

75
Q

What do alkali metals react with?

A

Non-metals

76
Q

What do alkali metals form when they react with non-metals?

A

Ionic compounds

77
Q

What colour solution is generally formed when alkali metals when dissolves in water?

A

Colourless

78
Q

Alkali metals react ________ with water

A

Vigorously

79
Q

What is produced when alkali metals react with water?

A

Hydrogen gas and metal hydroxides

80
Q

What solutions do metal hydroxides produce when dissolved in water?

A

Alkaline

81
Q

Alkali metals react ________ with chlorine

A

Vigorously

82
Q

What is formed when alkali metals are heated in chlorine gas?

A

White metal chloride salts

83
Q

What is formed when alkali metals react with oxygen?

A

A metal oxide

84
Q

Alkali metals burn with a ________ flame when reacted with oxygen

A

Coloured

85
Q

Compared to transition metals, alkali metals…

A

Are less dense, strong and hard

Have lower melting points

86
Q

How many electrons are there in the outer shell of halogens?

A

7

87
Q

`As you go down Group 7:

A

Higher melting and boiling points
Higher relative atomic mass
Less reactive - harder to gain an extra electron - outer shell is further away

88
Q

Why does the reactivity decrease as you go down Group 7?

A

Because the outer electron shell is further away from the nucleus, meaning there is more electron shielding, meaning it is harder to attract an electron to the nucleus

89
Q

How do halogens share electrons?

A

Via covalent bonding

90
Q

How do halogens achieve a full outer shell?

A

They share electrons with other non-metals via covalent bonding

91
Q

What kind of compounds are formed when halogens react with non metals?

A

Compounds with simple molecular structures

92
Q

What charge ions do halogens form when they bond with metals?

A

1- ions

93
Q

What kind if compound is formed when metals and halogens bond?

A

Ionic compounds

94
Q

What are group 0 elements also called?

A

Noble gases

95
Q

Properties of noble gases:

A

Inert - unreactive

Colourless

96
Q

Why are noble gases inert?

A

They have a full outer shell that is energetically stable so they don’t need to gain or lose electrons

97
Q

Noble gases exist as _________ gases

A

Monatomic

98
Q

What are monatomic gases?

A

Single atoms not bonded to each other

99
Q

Why are noble gases colourless and non-flammable?

A

Because they are inert

100
Q

What is the trend in the boiling point of noble gases?

A

It increases as you go down the group

101
Q

Why does the boiling point of noble gases increase as you go down the group?

A

Because there is an increase in the number of electrons in each atom, meaning there are greater intermolecular forces that have to be overcome

Chemistry GCSE (10 decks)

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