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Chemistry - Paper 1 > STRUCTURE AND BONDING > Flashcards

STRUCTURE AND BONDING Flashcards

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1
Q

how are covalent bonds formed

A

by atoms sharing electrons

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2
Q

which type of atoms form covalent bonds between them

A

non metals

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3
Q

describe the structure and bonding of a giant covalent structure

A

billions of atoms bonded together by strong covalent bonds

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4
Q

describe the structure and bonding of small molecules

A

small numbers of atoms group together into molecules with strong covalent bonds between the atoms and weak intermolecular forces between the molecules

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5
Q

describe the structure and bonding of polymers

A

many identical molecules joined together by strong covalent bonds in a long chain with weak intermolecular forces between the chains

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6
Q

why do giant covalent substances have high melting points

A

it takes a lot of energy to break the strong covalent bond between atoms

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7
Q

why do small molecules have low melting points

A

only a small amount of energy is needed to break the weak intermolecular forces

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8
Q

why do large molecules have higher melting and boiling points than small molecules

A

the intermolecular forces are stronger

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9
Q

why do most covalent substances not conduct electricity

A

do not have delocalised electrons or ions

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10
Q

describe the structure and bonding in graphite

A

each carbon atom is bonded to three others in hexagonal rings arranged in layers - it has delocalised electrons and weak forces between layers

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11
Q

why can graphite conduct electricity

A

the delocalised electrons can move through the graphite

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12
Q

explain why graphite is soft

A

layers aren’t bonded so can slide over each other

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13
Q

what is graphene

A

one layer of graphite

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14
Q

2 properties of graphene

A

strong, conduct electricity

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15
Q

what is a fullerene

A

hollow cage of carbon atoms arranged as a sphere or a tube

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16
Q

what is a nanotube

A

hollow cylinder of carbon atoms

17
Q

2 properties of nanotubes

A

high tensile strength and conduct electricity

18
Q

3 uses of fullerenes

A

lubricants, drug delivery and high tech electronics

19
Q

what is an ion

A

atom that has lost or gained electrons

20
Q

what kind of elements form ionic bonds

A

metals and non metals

21
Q

name the force that holds oppositely charged ions together

A

electrostatic force of attraction

22
Q

describe the structure of a giant iconic lattice

A

regular structure of alternating positive and negative ions, held together by the electrostatic force of attraction

23
Q

why do ionic substances have a high melting point

A

electrostatic force of attraction between the positive and negative ions is strong and requires lots of energy to break

24
Q

why don’t ionic substances conduct electricity when solid

A

ions are fixed in position so cannot move and there are no delocalised electrons

25
Q

when can ionic substances conduct electricity

A

when melted or dissolved

26
Q

why do ionic substances conduct electricity when molten or dissolved

A

ions are free to move and carry charge

27
Q

describe the structure of a pure metal

A

layers of positive metal ions surrounded by delocalised electrons

28
Q

describe the bonding in a pure metal

A

strong electrostatic forces of attraction between metal ions and delocalised electrons

29
Q

4 properties of pure metals

A

malleable, high melting point, good conductors of electricity and thermal energy

30
Q

explain why pure metals are malleable

A

layers can slide over each other easily

31
Q

explain why metals having higher melting and boiling points

A

electrostatic force of attraction between positive and negative ions and delocalised electrons is strong and requires a lot of energy to break

32
Q

why are metals good conductors of electricity and of thermal energy

A

delocalised electrons are free to move through the metal

33
Q

what is an alloy

A

mixture of a metal with atoms of another element

34
Q

explain why alloys are harder than pure metals

A

different size atoms disturb layers, preventing them from sliding over each other

Chemistry - Paper 1 (5 decks)

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