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Chemistry > C3 bonding > Flashcards

C3 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 boding of a giant covalent substance

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 inter molecular forces between the molecules

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5
Q

describe the structure and boning of polymers

A

many identical molecules joined together by strong covalent bonds in a long chain, with weak intermoecular 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 bonds between the 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 intermlecular 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 in large molecules

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9
Q

why do most covalent substances not conduct electricity

A

do not have delocalised electron or ions

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10
Q

describe the structure an bonding of graphite

A

each carbon atom is bonded to three others in hexagonal rings arranged in layers- it has delocalised electrons and weak forces between the 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 are not 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

give two properties of graphene

A

strong, conducts 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

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17
Q

give two properties of nanotubes

A

high tensile strength, conduct electricity

18
Q

what is an ion

A

atom that has lost or gained electrons

19
Q

which kinds of elements form ionic bonds

A

a metal with a non-metal

20
Q

what charges do ions from group 1 and 2 form

A

group 1 forms 1+, group 2 forms 2+

21
Q

what charges do ions from group 6 and 7 form

A

group 6 forms 2-, group 7 forms 1-

22
Q

name the force that holds oppositely charges ions together

A

electrostatic force of attraction

23
Q

give three uses of fullerenes

A

lubricants, drug delivery (spheres), high-tech electronics

24
Q

describe the structure of giant ionic lattice

A

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

25
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

26
Q

why do ionic substance have higher melting points

A

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

27
Q

when can ionic substances conduct electricity

A

when melted or dissolved

28
Q

why do ionic substances conduct electricity when melted or dissolved

A

ions are free to move and carry charge

29
Q

describe the structure of a pure metal

A

layers of positive metal ions surrounded by delocalised electrons

30
Q

describe the bonding in a pure metal

A

strong electrostatic forces between metal ions and delocalised electrons

31
Q

what are four properties of pure metals

A

malleable, high melting/boiling points, good conductors of electricity, good conductor of thermal energy

32
Q

explain why pure metals are malleable

A

layers can slide over easily

33
Q

explain why metals have high melting and boiling points

A

electrostatic forces between positive metal ions and delocalised electrons is strong and requires a lot of energy to break

34
Q

why are metals good conductors of electricity and of thermal energy

A

delocalised electrons are free to move through the metal

35
Q

what is an alloy

A

mixture of a metal with atoms of another element

36
Q

explain why alloys are harder than pure metals

A

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

37
Q

how big are nano particles

A

1-100 nm

38
Q

how are nanomaterials different from bulk materials

A

nanomaterials have a much higher surface area to volume ratio

39
Q

what is the relationship between side length and surface area to volume ratio

A

as side length decreases by a factor of ten, the surface area to volume ratio increases by a factor of ten

40
Q

what are nano particles used for

A

used in healthcare, electronics, cosmetics, and catalysts

Chemistry (13 decks)

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