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chemistry > C2:Chemical bonds, ionic, covalent and metallic > Flashcards

C2:Chemical bonds, ionic, covalent and metallic Flashcards

1
Q

what happens in metallic bonding

A

grid off ions surrounded by a sea of delocalised electrons as the electrons can move the can bond with each other

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2
Q

what are ionic compound

A

giant structure of ions

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3
Q

what are ionic compound held together by

A

strong electrostatic attraction held together by oppositely charged ions

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4
Q

what are the limitations of using dot and cross, ball and stick, two and three-dimensional diagrams to represent a giant
ionic structure

A

gives no information about the forces of attraction between the ions,or the
movement of the electrons,

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5
Q

what do the ions have to do in an ionic compound

A

the charges on an ion have to cancel each other out to leave an overall charge of 0

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6
Q

what is the structure of ionic compounds

A

giant ionic lattice

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7
Q

why do ionic compounds have high melting and boiling points

A

need a lot of energy to break the strong bonds

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8
Q

how can ionic compounds conduct electricty

A

when they are molten or dissolved in an aqueous solution

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9
Q

why can they conduct electricity

A

ions are free to move so thye can carry a charge

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10
Q

Mg^2+ no3^-
what is this in an ionic compound

A

Mg(NO)3

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11
Q

what can covalent bonds consist of

A

small molecules

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12
Q

what are polymers an example of

A

large molecules

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13
Q

what do metallic bonds consist of

A

atoms arranged in a regular pattern

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14
Q

what happens during metallic bonding

A

electrons become delocalised and are free to move around.The sharing of delocalised electrons allow for strong metallic bonds

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15
Q

the amount of energy needed to change from a state of matter depends on

A

the strength of the forces acting on the particles of the substance

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16
Q

what does the nature of the particles depend on

A

type of bonding and structure of the substance

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17
Q

what are the limitations of the simple state model

A

there are no forces, all particles are represented as spheres and that they are solid

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18
Q

gasses don’t keep a definite …. whereas solids and liquids do

A

shape or volume

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19
Q

what are the forces between molecules called

A

intermolecular forces

20
Q

in simple molecular substances what is broken

A

intermolecular forces

21
Q

more molecules means

A

more intermolecular forces which gives a stronger attraction

22
Q

why cant simple molecular substances conduct

A

no free electrons and the molecules have no charge

23
Q

polymers have

A

large molecules and strong covalent bonds

24
Q

polymers are what at room temperature

A

solids

25
Q

giant covalent structure are

A

solids with high melting points

26
Q

what are giant covalent structures linked by

A

strong covalent bonds

27
Q

how can strong covalent bonds be broken down by

A

melting or boiling

28
Q

what is the structure of a pure metal

A

its arranged in layers

29
Q

why are pure metals mixed with other metals

A

they are too soft so they are mixed

30
Q

what are alloys

A

metals of different sizes mixed together which disrupt the lattice so layers cant slide over each other easily

31
Q

why are alloys stronger than pure metals

A

in alloys there are atoms of different sizes so a greater force is required to slide pver each other

32
Q

name the properties of a diamond

A

high melting and boiling points, hard

33
Q

what do covalent bonds form in a diamond

A

4 carbon bonds

34
Q

does diamond conduct electricity

A

NO

35
Q

what are the properties of graphite

A

hexagonal rings whih have no cvalent bonds in the layers

36
Q

what do covalent bonds form in graphite

A

3 carbon bonds

37
Q

in graphite what happens from each carbon atom

A

one electron from a carbon atom is delocalised

38
Q

what is graphene

A

single layer of graphite

39
Q

what are the uses of graphene

A

electronics and compsites

40
Q

what are the properties of graphene

A

hard,light with high resistance

41
Q

what are fullerenes

A

molecules of carbon atoms with hollow shapes

42
Q

what are the structures of fullerenes based on

A

hexagonal rings of carbon atoms

43
Q

give examples of fullerenes

A

carbon nanotubes and buckminsterfullerene

44
Q

what are carbon nanaotubes

A

cylindical fullerenes with very high length to diameter ratio

45
Q

how are carbon nanotubes useful

A

nanotechnology,electronics and materials

chemistry (4 decks)

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