topic 1 - structure and bonding Flashcards

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