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Thornhill Academy Chemistry Combined (HGH) > Topic 2b - Bonding (Year 10) > Flashcards

Topic 2b - Bonding (Year 10) Flashcards

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1
Q

What does an ionic bond form between?

A

metal and non-metal

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2
Q

What does a covaltent bond form between?

A

non-metal and non-metal

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3
Q

What does a metallic bond form between?

A

metal and metal

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4
Q

How does an ionic bond form?

A

The metal loses electrons to become a positively charged ion, the non-metal gains electrons to become a negatively charged ion

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5
Q

How does a covalent bond form?

A

non-metals share pairs of electrons to gain full outer shells

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6
Q

How does a metallic bond form?

A

Metals lose their outer shell elctrons into a sea of delocalised electrons

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7
Q

If an atom loses two electrons to form an ion, what charge will the ion have?

A

+2

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8
Q

If an atom gains two electrons to form an ion, what charge will the ion have?

A

-2

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9
Q

Elements in group 1 will form ions with what charge?

A

+1

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10
Q

Elements in group 2 will form ions with what charge?

A

+2

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11
Q

Elements in group 3 will form ions with what charge?

A

+3

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12
Q

Elements in group 4 will form ions with what charge?

A

Group 4 don’t form ions because it is just as hard to lose 4 electrons, as it is to gain 4 electrons. Group 4 elements take part in covalent bonding.

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13
Q

Elements in group 5 will form ions with what charge?

A

-3

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14
Q

Elements in group 6 will form ions with what charge?

A

-2

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15
Q

Elements in group 7 will form ions with what charge?

A

-1

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16
Q

Elements in group 0 will form ions with what charge?

A

Group 0 don’t form ions because they already have a full outer shell

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17
Q

When are elements stable?

A

When they have a full outer shell of electrons

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18
Q

In ionic bonding, how are ions held together?

A

Electrostatic forces of attraction

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19
Q

Zinc Hydroxide is made up of Zn2+ ions and OH- ions. What is its formula?

A

Zn(OH)2

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20
Q

Sodium carbonate is made up from Na- and CO32-. What is its formula?

A

Na2CO3

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21
Q

Explain how Calcium Oxide forms. Remember Calcium is in gorup 2 and Oxygen is in group 6

A

Calcium loses 2 electrons becoming a 2+ ion and Oxygen gains 2 electrons becoming a 2- ion

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22
Q

Do ionic compounds have high or low melting points?

A

Ionic compounds have high melting points

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23
Q

Why do ionic compounds have high melting points?

A

Ions are held together by strong electrostatic forces of attraction

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24
Q

Give a limitation to the ball and stick models to represent ionic compounds

A

The model isn’t to scale. It shoes gaps between ions.

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25
Q

How are ions arranged in an ionic compound?

A

Giant ionic lattice

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26
Q

Can ionic compounds conduct electricity?

A

Yes but only when molten or dissolved in water

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27
Q

Why can ionic bonds only conduct electricity when molten or in a solution?

A

When solid, the ions in an ionic compounds can’t move. When molten or in solution th ions are free to move

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28
Q

Define the term: dissociate

A

To separate into separate ions. We talk about dissociation in terms of ions in ionic compounds dissociating when in a solution

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29
Q

Explain why carbon forms covalent bonds with 4 hydrogen atoms in CH4

A

Carbon has 4 electrons in its outer shell, so need for 4 covalent bonds to gain a full outer shell. Hydrogen has 1 electron in its outer shell and needs to form one single bond to gain a full outer shell. So you need 4 hydrogen atoms for each 1 carbon atom

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30
Q

Poly(ethene) is a polymer. Describe the structure of a polymer

A

A polymer is made up from a long chain of covalently bonded carbon atoms

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31
Q

True or False: All simple covalent molecular substances are insoluble in water

A

False, Some simple molecular substances are soluble and some are insoluble

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32
Q

True or False: O2 has a double bond

A

True, Oxygens structure is O=O

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33
Q

Is a covalent bond strong?

A

A single covalent bond is very strong. It is extremely hard to try and bbreak a bond where they are sharing electrons.

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34
Q

Why don’t simple molecular substances conduct electricity?

A

There is no charged ions and there is no free electrons that can move to carry electricity

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35
Q

Why do simple molecular substances have low melting and boiling points?

A

Simple molecular substances have low melting and boiling points because there was weak intermolecular force of attraction between moleculs that can easily be broken.

36
Q

H2 and CH4 are both covalent compounds. Which would have the highest boiling point?

A

CH4 would have the highest boiling point. The larger the molecule the stonger the intermolecular forces, meaning the more energy needed to break them.

37
Q

Define the term: allotrope

A

Different structural forms of the same element, for example diamond and graphite are both made from carbon

38
Q

What element is graphite made from?

A

Carbon

39
Q

What element is damond made from?

A

Carbon

40
Q

What is the structure of diamond?

A

Diamong is a tetraheadral structure, where each carbon is covalently bonded to 4 other carbons

41
Q

What is the structure of graphite?

A

Graphite is layers of graphene sheets, with forces acting between the sheets. Each carbon is bonded to 3 other carbon atoms in a hexagonal structure

42
Q

What is the difference between graphite and graphene?

A

Graphene is a single layer of hexagonal lattice structure, where a carbon is bonded to 3 other carbons. Graphite, is layers of graphene sheets

43
Q

Can diamond conduct electricity?

A

No. There are no free electrons in diamond

44
Q

Can graphite conduct electricity?

A

Yes. There are free electrons that can move throughout the structure

45
Q

Why do giant covalent substances have high melting points?

A

They have high melting points because of the strong covalent bonds between the atoms

46
Q

Explain how the structure and bonding of graphite makes it a suitable material for lubricants.

A

Graphite has a layered structure, with only weak forces of attraction between the layers. The layers can break away from each other, makng graphite soft and slippery

47
Q

Describe the structure of fullerenes

A

Fullerenes are molecules of carbon, shaped likeclosed tubes or hollow balls. They have a huge surface area, so many catalyst molecules could be attached to each fullerene

48
Q

Why is graphite used for electrodes?

A

Graphite has the ability to conduct electricity due to the free electrons. Carbon is also unreactive which makes it safer to use in electrodes

49
Q

Where on the periodic table are metals found?

A

Towards the left of the periodic table

50
Q

Describe the bonding in a metal

A

The bonding in a metal consists of strong electrostatic forces of attraction between positive metal ions and the delocalised electrons.

51
Q

Explain why metals can conduct electricity

A

The have delocalised electrons that can pass through the structure

52
Q

Explain why metals can conduct heat

A

The have delocalised electrons that can pass through the structure

53
Q

Explain why metals are malleable and ductile

A

Mtels have a layered structure. The layers can slide across each other, meaning when a pressure is applied the layers move.

54
Q

Explain why metals have a high melting and boiling point

A

Metals ions and the delocalised elctrons are held together by strong electrostatic forces of attraction. The electrostatic forces need a large amount of energy to be overcome

55
Q

Define the term: Alloy

A

An alloy is a mixture of metals or a mixture containing at least one metal.

56
Q

Why are alloys stonger than pure metas?l

A

An alloy has more than one type of atom. The atoms are different sizes, which makes it harder for the layers to pass over each other

57
Q

What type of ions do metals form?

A

Metals always form positive ions

58
Q

What type of ions do non-metals form?

A

Non-metals always form negative ions, due to them gaining electrons to gain a full outer shell.

59
Q

Which group of elements is stable and doesnt form compounds easily?

A

noble gases/group 0 in the periodic table

60
Q

Why do elements want to form bonds?

A

To gain a full outershell of electrons and become stable.

61
Q

How is an elements electron arrangement linked to its position in the periodic table?

A

Elements in the same group have the same number of electrons in their outer shell.

62
Q

How do positive and negative charges affect each other?

A

They attract each other.

63
Q

Which sub-atomic particles of atoms take part in chemical reactions?

A

Electrons

64
Q

What is an ion?

A

an atom that is charged because it has lost or gained one or more electrons

65
Q

What happens when an ionic bond is formed?

A

One atom (a metal) loses electrons to another atom (a non-metal) to form oppositely charged ions that attract each other.

66
Q

How is a positive ion formed and what is it called?

A

formed by the loss of electrons; cation

67
Q

How is a negative ion formed and what is it called?

A

formed by the gain of electrons; anion

68
Q

What are the forces called that hold ions together?

A

electrostatic forces of attraction

69
Q

Why do atoms form ions?

A

to become more stable (like a noble gas)

70
Q

What structure of regularly repeating ions do ionic compounds form?

A

lattice structure / ionic lattice

71
Q

What is the name of the ionic compound containing calcium and bromine only?

A

calcium bromide

72
Q

Describe the appearence of diamond

A

colourless and shiny

73
Q

Describe the appearence of graphite

A

dark black/silvery

74
Q

Describe the uses for diamond

A

Diamond is used for jewellery due to it’s appearance. Diamond is also used for drill bits - the covalent bonds mean that it extremely strong (one of the strongest known materials)

75
Q

Desrcibe a use for graphite

A

pencils, lubricants - due to the layered structure it allows for movement and the covalent bonds meann it has a high melting point.

76
Q

What is the molecular formula of the very common compound formed between hydrogen and oxygen?

A

H2O

77
Q

What are molecules?

A

groups of atoms held together by (covalent) bonds

78
Q

What happens to electrons between two atoms in a covalent bond?

A

they are shared

79
Q

What kinds of bonds are found in molecules?

A

covalent bonds are found holding the atoms together in molecules (intermolecular forces are found between molecules)

80
Q

Define: Intermolecular force of attraction

A

Forces of attraction between simple covalent compounds

81
Q

In oxygen and carbon dioxide, the atoms share two pairs of electrons. How do we describe these bonds?

A

double bonds (represented by = in a displayed formula)

82
Q

What is the name of the force that holds molecules together in gases and liquids?

A

intermolecular force

83
Q

How strong are the forces of attraction between molecules compared to the bonds within molecules?

A

They are relatively weak. (Covalent bonds holding atoms together are strong / Intermolecular forces holding molecules together are weak)

84
Q

Are simple molecules usually good conductors of electricity at room temperature?

A

No, they are poor conductors of electricity (as they have no charged particles or free electrons to move)

85
Q

What type of structure do diamond and graphite have?

A

Giant Covalent

86
Q

What type of structure does silicon dioxide have?

A

Giant covalent

Thornhill Academy Chemistry Combined (HGH) (8 decks)

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