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GCSE AQA Chemistry > C3- Structure And Bonding > Flashcards

C3- Structure And Bonding Flashcards

1
Q

Elements react together to form compounds by gaining or losing electrons or by _________ electrons

A

Sharing

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2
Q

How are ionic compounds held together?

A

By strong forces of attraction between thie roppositely charged ions

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3
Q

A solid turns into a liquid at its __________

A

Melting point

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4
Q

The hotter the gass is the _______ the particles move

A

Faster

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5
Q

What is the pressure of a gas caused by?

A

The particles colliding with the sides of the container.

The more frequent and energetic the collisions, thr higher thr pressure of gas.

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6
Q

In a sealed container the pressure of gas_____ with temperature

A

Increases

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7
Q

The hotter the solid is, the ____ its particles vibrate

A

Faster

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8
Q

Liquid turns to gas at ________ point

A

Boiling

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9
Q

As the _________ rises, more and more energy is transferred from the sorroundings to the particles and the particles escape from the surface of the liquid,

the rate of evaporation increases.

A

Temperature

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10
Q

___________ are formed in changes of state

A

No new substances

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11
Q

What affects the arrangements of particles?

A

The temperature

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12
Q

When you monitor the temperature of a soild as you heat it beyond its melting point what happens?

A

The temperature stops rising at the solid’s melting point.

  • the tempurature remains constant until the solid has melted
  • only then the tempurature starts to rise again
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13
Q

What happens at a solids melting point?

A

Enougg energy is transferred from the surroundings to the solid for the forces between particles in the solid to break.

-this enables particles to break away from their fixed positions and start moving around

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14
Q

What does the simple particle model show?

A

Particles are made up of solid spheres with no forces operating between them

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15
Q

What is the particle model useful for?

A

Comparing the properties of solids, liquids and gases.

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16
Q

In melting and boiling, energy is transferred from the _______ to the ________

A
  1. Surroundings

2. Substance

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17
Q

In freezing and condensing energy is transferred from the _______ to the ________

A
  1. Substance

2. Surroundings

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18
Q

What does a compound contain?

A

Two or more elements that are chemically combined

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19
Q

The noble gases have an arrangement of electrons that make them__.

A

Stable

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20
Q

What is ionic bonding?

A

Transferring electrons

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21
Q

What is covalent bonding?

A

Sharing electrons

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22
Q

You lose electrons to form____

A

Positive ions

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23
Q

You gain electrons to form?

A

Negative ions

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24
Q

Metal atom which tend to _____ electrons react with non-metal atoms which tend to _______ electrons

A
  1. Lose

2. Gain

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25
Q

How can you show transferred electrons?

A

Dot and cross diagram

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26
Q

Elements in group _ react with elements in group _

A

1

7

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27
Q

Why do elements want to lose/gain electrons?

A

To get a stable electronic structure

A compound will have the same electronic structure as a noble gas

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28
Q

How are ionic compounds usually formed?

A

When metals react with non-metals

In this the metals form positive ions and the non-metals form negative ions

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29
Q

Ions formed are held next to each other are held by_________

A

Very strong forces of attraction between the oppositely charged ions

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30
Q

The electrostatic force of attraction which acts in all directions is called?

A

Ionic bonding

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31
Q

What ions do Group 1 atoms form?

A

1+ ions

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32
Q

What do group 7 atoms form?

A

1- ions

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33
Q

Besides the elements in Group 1 and Group 7 that can form ionic compounds include______

A

Those in Group 2 (forming 2+ ions)

Those in Group 6(forming 2- ions)

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34
Q

It takes a lot of energy to break up a ___________

A

Giant ionic lattice

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35
Q

Why do ionic compoundd have a high melting point?

A

Because to seperate the ions you have to overcome all the elecrtostatic forces of attraction acting in all directions.

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36
Q

What are ionic metals as liquids attracted to?

A

Oppositely charged electrodes held in the molten compound.

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37
Q

Can a soild ionic compound conduct electricity, explain why.

A

No beacuse its ions afe held in foxes positions in the lattice

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38
Q

Do ionic compounds dissolve in water?

A

Most but not all

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39
Q

Do ionic compounds dissolved in water conduct electricity?

A

Yes because the ions are able to move to an oppositely charged electrode dipped in the solution

40
Q

Does molten ionic compounds conduct electricity?

A

Yes

41
Q

Simple: why can ionic compounds conduct electricity when molten or dissolved in water?

A

Because their ions can become mobile and carry charge through the liquid

42
Q

What do reactions between metals and non-metals usually result in?

A

Ionic bonding

43
Q

Non-metals react together, their atoms shair pairs of electrons to for, molecules. What is this called?

A

Covalent bonding

44
Q

The atoms of non-metals tend to ____ electrons to achieve stable electron structures

A

Gain

45
Q

What are covalent bonds?

A

When the atoms in the molecules are held together by shared pairs of electrons.- the strong bonds between the atoms are called covalent bonds

46
Q

How can you show covalent bonds in substances such as water?

A
  • the number of covalent bonds
  • the highest energy levels(outer shells)
  • the outer electrons in dot and cross diagram
47
Q

What are giant covalent structures sometimes referred to as?

A

Macromolecules

48
Q

Does Diamond have a giant covalent structure?

A

Yes

49
Q

Describe diamond’s giant covalent structure:

A

Each carbon atoms forms four covalent bonds with its neighbours. -it results ina rigid giant covalent structure lattice

50
Q

How are covalent bonds formed?

A

When atoms of non-metals share pairs of electrons with each other

51
Q

Each shared pair of electron is a ______

A

Covalent bond

52
Q

Many substances containing covalent bonds consist of simple molecules but some have giant covalent structures

A

This is true 👍🏻

53
Q

Are electrons in covalent bonds constantly moving?

A

Yes

54
Q

In covalent bonds are the molecules held tightly together?

A

Yes

55
Q

How big is the force of attraction between the individual molecules?

A

Small (weak intermolecular forces)

56
Q

Why do larger molecules have higher melting and boiling points?

A

Because intermolecular forces increase with the size of the molecules.

57
Q

Why can’t simple molecules conduct electricity

A

They have no overall charge so they cannot carry an electrical charge

58
Q

Do substances made up of simple molecules have low melting points and boiling points?

A

Yes

59
Q

What is the problems with using models?

A

Each one has its limitations in representing reality

60
Q

What do Diamonds and other huge covalent structures have?

A

Huge networks of atoms arranged in simple molecules- the huge networks pf atoms are held together by strong covalent bonds in giant covalent structures

61
Q

What are some examples of giant covalent structures?

A

Graphite
Silicon dioxide
Diamond

62
Q

What are the properties of Giant covalent structures?

A
  • high melting and boiling points
  • insoluble in water (can’t dissolve in water)
  • apart from graphite they are hard and do not conduct electricity
63
Q

Im diamond how many covalent bonds does each atom form?

A

4

64
Q

What is Graphite used in?

A

Pencil lead

65
Q

How many carbon atoms is each carbon atom bonded to?

A

3

66
Q

What ks there between layers in graphite?

A

Weak intermolecular forces(no covalent bonds)

67
Q

Carbon has 4 atoms in its outer shell. If 3 are used in graphite what happens to the other one?

A

They move freely along the layers of carbon atoms.

The mobile elctrons in Graphite are called Delocalised electrons

68
Q

How do delocalised elelctrons behave?

A

Like electrons in metallic structure

69
Q

The delocalised electrons allow Graphite to ______

A

Conduct elelctricity

70
Q

Why is Graphite a good conductor of thermal energy?

A

As more energy is transferred to the delocalised electrons, they move around faster and rapidly transfer the energy along the layers of the Graphite

71
Q

As well as Diamond and graphite carbon also exaits as ________ which can form large cage-like structures and tubes based on hexagonal rings of carbon atoms

A

Fullerenes

72
Q

How are fullerenes finding uses?

A

As transport mechinism for drugs to specific sites in the body, as catalysts and as a reinforcement for composite matierals

73
Q

What are catalysts?

A

The process of increasing the rate of a chemical reaction without undergoing a chemical change itself

74
Q

What is graphene?

A

A single layer of graphite one layer thick.

Properties: very good at conducting electricity and it will help create new developments in the electronic industry in the future.

75
Q

What are Cylindrical fullerenes?

A

Very thin cylinders

  • high tensile strength
  • high electrical conductivity
76
Q

You can see ____ crystals on the surface of some steel that has been dipped into molten ____ to prevent it

A

Zinc
Zinc

-this is called galvanised steel

77
Q

Are the atoms in metals closely packed together and arranged in regular layers?

A

Yep

78
Q

What is metallic bonding?

A

Positively charged electrons

-held together by electrons from the outermost shell of each metal atom. These delocalised electrons are free to move throughout the giant metallic littice

79
Q

The ____ electrons from each metals atom can easily move throughout the giant structure

A

Outer

80
Q

Why are the layers of metal in a pure atom able to slide over each other?

A

Because metals can be hammered and bent into diffrent shales and drawn out into wires

81
Q

Atoms in a pure metal such as iron are held together by what?

A

A Giant metallic structure

82
Q

In giant metallic structures the atoms are arranged closely in packed layers this allows them to do what?

A

It allows the atoms to slide over one and other easily

83
Q

What is an alloy?

A

A mixture of two or more elelments, at least of one which is a metal

84
Q

The positive ions in a metlas giant structure are binded together by______

A

A sea of delocaslised electrons

( they act almost like a glue- the negatively charged between the positively charged ions hold the the metal ion in position by electrostatic forces of attraction.)

85
Q

Can delocalised electrons move throughout the whole lattice?

A

Yes

86
Q

Are alloys harder than pure metals if so why?

A

Yes because the regular layers in a pure metal are distorted by atoms of diffrent sizes in an alloy

87
Q

What allows electricity and thermal energy to be transferred through a metal easily?

A

Delocalised elelctrons

88
Q

What group tend to become stable by sharing electeons(covalent bonding)

A

Group 4

89
Q

How do you know if a compound is covalent or ionic?

A

ionic bond is between a metal and a nonmetal, and a covalent bond is between 2 nonmetals.

90
Q

What is the line that represents covalent bonding in 2 florine atoms?

A

F-F

91
Q

how do you know if something is a giant covalent structure, a giant ionic structure or a simple molecule?

A

If it is a gas, liquid or low melting point solid then you are talking about a simple molecular substance. … If it is a high melting point solid, it will be a giant structure - either ionic, metallic or giant covalent

92
Q

What are giant metallic structures?

A

Metals are giant structures with metal ions arranged in a regular, repeating lattice with layers of metal ions.

93
Q

Metallic bonding?

A

Positively charged metals ions with a sea of delocaslised electrons

94
Q

What is metallic bonds

A

Electrostatic attraction in a metal

95
Q

What is a giant ionic lattice

A

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

GCSE AQA Chemistry (22 decks)

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