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Chemistry GCSE > topic 1 - structure and bonding > Flashcards

topic 1 - structure and bonding Flashcards

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1
Q

ion

A

a charge particle

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2
Q

anion

A

a negative ion

formed through electron gain

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3
Q

what groups form anions

A

6 and 7

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4
Q

cation

A

a positive ion

formed through electron loss

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5
Q

what groups readily form cations

A

1 and 2

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6
Q

how is an ionic bond formed

A

a metal atom loses electrons to form a cation
a non metal atom gains these electrons to form an anion
the two oppositely charged ions are strongly attracted to one another by ELECTROSTATIC FORCES

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7
Q

ions ending in -ate

A

negative

contain oxygen and at least one other element

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8
Q

ions ending in -ide

A

negative

only contain one element (excluding hydroxide)

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9
Q

structure of ionic compounds

A

regular, giant ionic lattice held together by strong electrostatic forces between oppositely charged ions

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10
Q

properties of ionic compounds

A

high melting and boiling points

conduct electricity when molten or aqueous

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11
Q

why do ionic compounds have high melting and boiling points

A

takes a lot of energy to overcome the strong electrostatic attraction

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12
Q

why do ionic compounds conduct electricity when molten or aqueous

A

when solid, the ions are held in place so can’t conduct electricity
when molten/aqueous, ions are free to move and therefore can carry electric current

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13
Q

covalent bond

A

a strong bond formed when a pair of electrons is shared between two atoms

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14
Q

covalent bond features

A

weak intermolecular forces
uses non metal atoms
creates molecules

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15
Q

properties of simple covalent compounds

A

low melting and boiling points

poor conduction of electricty

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16
Q

why do simple covalent compounds have low melting and boiling point

A

the intermolecular forces are weak so not much energy is needed to overcome them

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17
Q

why do simple covalent compounds not conduct electricity well

A

they contain uncharged atoms so there are no free ions or electrons to carry the current

18
Q

properties of giant covalent structures

A

very high melting and boiling points
don’t conduct electricity (apart from graphite and graphene)
insoluble in water

19
Q

what giant covalent structures can conduct electricity

A

graphite

graphene

20
Q

why do giant covalent structures have VERY high melting and boiling points

A

lots of energy is needed to overcome the strong covalent bonds

21
Q

give 4 examples of giant covalent structures

A

diamond
graphite
graphene
C60 - buckminsterfullerene

22
Q

diamond

A

network of carbon atoms that each form 4 covalent bonds

23
Q

properties of diamond and their reasons

A

high melting and boiling points - strong covalent bonds (strong intermolecular forces)

very hard - strong, rigid lattice structure

no conduction of electricity - no free ions or electrons

24
Q

use of diamond

A

cutting tools

25
Q

graphite

A

a carbon structure where carbon atoms have three covalent bonds and the 4th electron is delocalised
this creates sheets of carbon atoms arranged in hexagons

26
Q

properties of graphite and their reasons

A

high melting point - strong covalent bonds (strong intermolecular forces)

conduction of electricity - the delocalised electron is free to move

soft and slippery - layers don’t have covalent bonds between them, allowing them to slide over one another

27
Q

uses of graphite

A

electrodes

lubrication

28
Q

allotrope

A

multiple forms of the same element

29
Q

fullerene

A

carbon molecules shaped like a tube/cylinder or hollow ball

can trap molecules

30
Q

graphene

A

one layer of graphite

31
Q

properties of graphene

A

high melting point

conducts electricity

32
Q

what can graphene form and what can that be used for

A

can form carbon nanotubes
these have high tensile strength
used to strengthen lightweight sports equipment

33
Q

what does C60 look like

A

hollow sphere
20 hexagons
12 pentagons

34
Q

polymer

A

large molecules containing long chains of covalently bonded carbon atoms

formed by lots of monomers joining together

35
Q

metallic bond

A

bond between metal ions and delocalised electrons due to electrostatic attraction

36
Q

physical properties of metals

A 
shiny solids
high melting points
high density
good electrical conductors
malleable
37
Q

why are metals malleable

A

layers of pure metal can slide over one another

38
Q

what are the 4 kind of models

A

2D representations
dot and cross
3D models
ball and stick models

39
Q

evaluate 2d representations (2+, 2-)

A

simple and great
shows how atoms are connected

don’t show shape of substance
no indication of atom size

40
Q

evaluate dot and cross models

A

shows how compounds are formed
shows where electrons/ions came from

no indication of atom size
no indication of atom arrangement

41
Q

evaluate 3d models

A

shows arrangement of ions

only shows the outer layer of a substance

42
Q

evaluate ball and stick models

A

shows how the atoms are connected
good for visualising structures

makes it look like there are large gaps between atoms
doesn’t show correct scales of atoms or ions

Chemistry GCSE (15 decks)

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