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chemistry > bonding structures and properties (p1) > Flashcards

bonding structures and properties (p1) Flashcards

1
Q

What are the three types of chemical bond?

A

Ionic, covalent and metallic

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2
Q

What bonding occurs in metals?

A

metallic

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3
Q

What bonding occurs in non-metals?

A

covalent

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4
Q

What bonding occurs between a metal and non-metal?

A

ionic

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5
Q

How do metals form ions?

A

lose electrons

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6
Q

How do non-metals form ions?

A

gain electrons

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7
Q

What charge do metal ions have?

A

positive

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8
Q

What charge do non-metal ions have?

A

negative

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9
Q

What charge do ionic compounds have?

A

neutral

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10
Q

What is an ionic bond?

A

Electrostatic forces of attraction between ions with opposite charges

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11
Q

What is a covalent bond?

A

A shared pair of electrons between two atoms

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12
Q

What is a metallic bond?

A

Electrostatic forces of attraction between postive metal ions and negative, delocalised electrons

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13
Q

In what type of bonding are electrons shared?

A

covalent

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14
Q

In what type of bonding are electrons transferred?

A

ionic

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15
Q

What charge are the ions of group 1 elements?

A

1+

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16
Q

What charge are the ions of group 2 elements?

A

2+

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17
Q

What charge are the ions of group 6 elements?

A

2-

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18
Q

What charge are the ions of group 7 elements?

A

1-

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19
Q

What structure do ionic compounds have?

A

giant ionic lattice

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20
Q

What substances contain covalent bonds?

A

Small molecules, giant covalent structures, polymers

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21
Q

What forces are found between molecules?

A

intermolecular forces

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22
Q

What side of the periodic table contains metals?

A

left

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23
Q

What side of the periodic table contains non metals?

A

right

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24
Q

How many pairs of electrons are shared in a single covalent bond?

A

1

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25
Q

How many pairs of electrons are shared in a double covalent bond?

A

2

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26
Q

If the temperature is below the melting point of a substance, what state will it be?

A

solid

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27
Q

If the temperature is between the melting and boiling point of a substance, what state will it be?

A

liquid

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28
Q

What does (s) mean?

A

solid state

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29
Q

What does aqueous mean?

A

dissolved in water

30
Q

What does (aq) mean?

A

aqueous state

31
Q

What does (l) mean?

A

liquid state

32
Q

What does (g) mean?

A

gaseous state

32
Q

If the temperature is above the boiling point of a substance, what state will it be?

A

gas

33
Q

What state change happnes when a solid changes to a liquid?

A

melting

34
Q

What state change happens when a liquid turns to a gas?

A

boiling or evaporating

35
Q

What state change happens when a liquid turns to a solid?

A

freezing

36
Q

What state change happens when a gas turns to a liquid?

A

condensing

37
Q

What structure do ionic substances have?

A

giant ionic

38
Q

What structure do metallic substances have?

A

giant metallic

39
Q

What structures do covalent susbtances have?

A

Giant covalent or simple covalent

40
Q

What do substances need to conduct electricity?

A

Charged particles that can move

41
Q

Why can’t ionic compounds conduct electricity when solid?

A

ions are not free to move

42
Q

Why can metals conduct electricity?

A

The delocalised electrons are free to move

43
Q

Why can ionic compounds conduct electricity when molten or aqueous?

A

ions are not free to move

44
Q

Why can’t simple covalent substances conduct electricity?

A

have no charged particles

45
Q

Which structures have substances with high boiling points?

A

Giant covalent, giant ionic and giant metallic

46
Q

Which structures have substances with low boiling points?

A

simple covalent

47
Q

When can ionic compounds conduct electricity

A

when molten or aqueous

48
Q

Why do giant covalent compounds have high melting and boiling points?

A

The strong covalent bonds require lots of energy to break

49
Q

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

A

The weak intermolecular forces do not require much energy to break

50
Q

What type of bond links the atoms in polymers?

A

covalent

51
Q

What are alloys?

A

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

52
Q

Why are metals mixed with other elements to form alloys?

A

Metals are too soft for many uses

53
Q

Why can metals conduct thermal energy?

A

energy is transferred by the delocalised electrons

54
Q

What element is diamond made up of?

A

carbon

55
Q

What element is graphite made up of?

A

carbon

56
Q

What element is graphene made up of?

A

carbon

57
Q

How many covalent bonds can a carbon atom form?

A

4

58
Q

Why does graphite conduct electricity?

A

has electrons that are free to move

59
Q

Why does graphene conduct electricity?

A

It has electrons that are free to move

60
Q

What bonds connect the carbon atoms in graphite?

A

covalent bonds

61
Q

What connects the layers in graphite?

A

weak forces

62
Q

What bonds connect the carbon atoms in diamond?

A

covalent bonds

63
Q

What bonds connect the carbon atoms in graphene?

A

covalent bonds

64
Q

How are the carbon atoms arranged in graphite?

A

Hexagonal rings in layers

65
Q

How are the carbon atoms arranged in graphene?

A

Hexagonal rings

66
Q

Why does diamond have a high melting and boiling point?

A

The millions of strong covalent bonds require lots of energy to break

67
Q

Why does graphite have a high melting and boiling point?

A

The millions of strong covalent bonds require lots of energy to break

68
Q

What are fullerenes?

A

Molecules of carbon atoms with hollow shapes

69
Q

What was the first fullerene to be discovered called?

A

Buckminsterfullerene

chemistry (15 decks)

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