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Chem gcse > structure and bonding > Flashcards

structure and bonding Flashcards

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1
Q

Traits of solids

A

Very packed together
Cannot flow freely
Can vibrate
Fixed space
Hard to compress

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2
Q

Traits of liquids

A

Not much space between
Hard to compress
Flow freely
Take shape of their container

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3
Q

Traits of gases

A

Widely spaced
Easy to compress
Moves quickly and randomly

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4
Q

What has to be given to a solid to be a liquid

A

Energy so it can break the forces of attraction and move freely as a liquid

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5
Q

Stronger the forces of attraction…

A

More energy needed to be put it, higher melting/ boiling point

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6
Q

Limitations of a single particle model

A

Particles are not a solid sphere
Particles have forces between them

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7
Q

metals make..

A

positive ions

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8
Q

non metals make…

A

negative ions

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9
Q

what is ionic between

A

a metal and a non metal

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10
Q

what do ionic compounsds form

A

giant lattice structures

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11
Q

properties of iomic compounds

A

very strong electrostatic forces of attraction
very high melting and boiling points
cant conduct whilsta solid

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12
Q

diagram to show ionic bonding

A

dots and crosses

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13
Q

ionic compound in solution

A

does conduct
ions can become mobile when separated by water

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14
Q

molten ionic compound

A

does conduct
high temps overcome the strong force
ions can move

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15
Q

what is coveylant bonding between

A

two non metals

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16
Q

what happens in coveylant bonding

A

the two atoms share a pair of electrons, each pair shared is asingle coveylant bind.

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17
Q

dif types of bonding models

A

dot and cross
stick bonds
ball and stick

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18
Q

why are smaller coveylant molecules so volatile

A

because the bond between each bond is very tight however the intermoleculaar force is weak, meaning they are easy to overcome with a raise in temp.
larger the size of the molecule the stronger the forces are

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19
Q

do covelylant compounds conduct

A

no not even as a liquid because there is no electrical charge/ electrons are shared so none are free
unless theyre reacted w water or molten

20
Q

properties of giant coveylant structures

A

high m and b points
insoluable
hard and dont condutc except graphite

21
Q

formation of diamond

A

each carbon atom is bonded to 4 others in a huge huge structre

22
Q

why cant diamond/ silicon di conduct

A

all the electrons are bonded so there are no electrons free to conduct

23
Q

formation of silicon di

A

silicon and oxygen bonded

24
Q

formation of graphite

A

carbon atom bonded to three other carbon atoms

25
Q

properties of graphite

A

high m and b point
soft and slippery
v good conductor

26
Q

why is graphite slippery

A

the bonds are very strongly bonded but they are in layers that are weakly joined so they can easily slide

27
Q

why is graphite a strong conductor

A

because only three elctrons are bonded there is one delocalised electron that can move freely and conduct

28
Q

why is graphite similar to metal

A

good conductor of electricity
have delocalised electrons

29
Q

whats a fullerene

A

carbon atoms bonded together in shexagons or pentagons that makes huge hollow shapes

30
Q

what is nanotubes

A

large cylinder fullerenes

31
Q

properties of nanotubes

A

very strong and bendable
very strong conductor because its bonded like graphite

32
Q

uses of fullerenes

A

delivery of pharmacuticals into body because of cage structure
lubricants- slippery
catalysts- high SA/V ratio

33
Q

what is graphene

A

a single atom thick layer of graphite

34
Q

uses of graphene

A

very good conductor
very strong so can be used for computers and electromics- like a 2d screen

35
Q

what are metal structures like

A

huge lattice of pos ions as the outer layer of electrons are delocalised and move throughout
the pos ions are very compact and regularly arranged

36
Q

what bonds the metal lattice

A

strong atraction between the positively charged ions and the neg electrons that move

37
Q

why are metals easily bent

A

the atoms are in layers that can slide

38
Q

what are alloys and what do they do

A

a mixture of metals that are larger sp they distort the layers and block them from sliding. makes them harder than pure metals

39
Q

uses of metal

A

cooking stuff because it conducts thermal energy and melts high
wires because it conducts electricity

40
Q

properties of metals

A

high melting and boiling points bc the electrons can move and hold the pos ions
greeat conductors becasue of delocalised electrons
ductile because layers can slide

41
Q

how do ionic structures work in a liquid for electrolysis

A

the water molecules have enough enrgy to dissolve them, leaving them free to move and marry their charge- which are attracted to the oposite anode/ cathode

42
Q

what are macromolecules

A

giant coveylant structures

43
Q

whats an electrostatic force

A

the force of attraction between pos and neg ions that hold them toegther, as well as the force between protons and electrons in an atom

44
Q

whats an allotrope

A

substances made from the same element in the same state with dif structures eg graphite and diamond

45
Q

whats a polymer

A

large molecule made up of lots of smaller units called monomers

Chem gcse (17 decks)

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