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Chemistry > structure and bonding > Flashcards

structure and bonding Flashcards

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1
Q

What does bonding describe

A

how the outer electrons of atoms interact with each other

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2
Q

3 types of bonding

A

metallic, ionic, covalent

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3
Q

what does structure describe

A

the arrangement of the bonded atoms

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4
Q

2 types of structures

A

giant (lattice) – all metals and ionic, simple – gas or liquid

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5
Q

properties of metals x5

A

strong, high melting point, malleable, ductile, electric conductors

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6
Q

meaning of malleable and ductile

A

malleable – shaped when hit with hammer without breaking, ductile – stretched into wires/cables

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7
Q

how are metals held together?

A

electrostatic attraction between positive ions and delocalised electrons between them

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8
Q

what are alloys

A

mixtures of metals

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9
Q

properties of alloys x3

A

stronger, less malleable and less ductile

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10
Q

why are metals conductors of electricity

A

there are mobile delocalised electrons which carry charge

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11
Q

what is combined to form ionic compounds

A

metal and non-metal ( positive ion to a negative ion)

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12
Q

In an ionic compound, the _____ always transfers its outermost shell electrons to the _______

A

metal, non-metal

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13
Q

In ionic bonding, the metal gains/ loses the same number of electrons as its ____ _______

A

loses, group number

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14
Q

3 typical properties of ionic compounds

A

soluble in water, conducts electricity, high melting point

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15
Q

3 typical properties of covalent compounds

A

low melting point, electric insulator, insoluble in water

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16
Q

how are ionic compounds held together?

A

strong electrostatic forces of attraction between oppositely charged ions

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17
Q

why do ionic compounds have high melting points?

A

a lot of energy is required to overcome strong electrostatic forces of attraction

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18
Q

do ionic compounds conduct electricity

A

yes but only when molten

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19
Q

why do ionic compounds conduct electricity when molten/ in solution but not when solid

A

because ions are fixed in position when solid but are able to move in solution. Electrons can then flow through.

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20
Q

structure of ionic compounds

A

giant lattice

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21
Q

covalent bonding occurs between 2 or more ____________

A

non metals

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22
Q

each atom tries to achieve a _____ _______ _____ in covalent bonding

A

full outer shell

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23
Q

electrostatic attraction is between what and what in covalent bonding

A

positive nuclei and shared pair of electrons

24
Q

attraction forces between molecules are called

A

intermolecular forces

25
Q

what is the spontaneous movement of a gas to fill its container called

A

diffusion

26
Q

simple covalent bonds will not conduct electricity because

A

they don’t have delocalized electrons or charged mobile ions

27
Q

the strong covalent bonds do not break when liquid water boils into steam. What is broken then?

A

intermolecular forces

28
Q

properties of simple covalent molecules x2

A

low boiling point b.c. of weak intermolecular forces, do not conduct electricity

29
Q

examples of giant covalent structures

A

diamond, graphite

30
Q

different structural forms of the same element are called

A

allotropes

31
Q

in fullerenes, each carbon atom is _________ bonded to ______ other carbon stoms

A

covalently, 3

32
Q

example of fullerene

A

C60 – 60 carbon atoms

33
Q

graphene is

A

a sheet of carbon atoms with no fixed formula

34
Q

graphene is ____ atom thick

A

1

35
Q

is graphene a good electrical conductor and why

A

yes, it allows free electrons to move across its surface ( each carbon atoms is only bonded to 3 other carbons )

36
Q

is graphene strong or weak and why

A

covalent bonds make it extremely strong

37
Q

giant molecular structures of carbon have high/low melting points because …

A

high, many strong covalent bonds need to be broken

38
Q

does graphite or diamond conduct electricity

A

graphite does, diamond doesn’t

39
Q

how does graphite conduct electricity

A

has 3 covalent bonds for each carbon atom –> not all its electrons are held in covalent bonds –> delocalized electrons are free to move and can carry an electrical current

40
Q

uses of graphite x3

A

pencil, electrodes(conducts electricity but not very reactive), lubricant (layers can slide past each other)

41
Q

what is an ore

A

a rock containing mental compounds with enough metal in it to make it worth extracting

42
Q

what 3 metals are found pure in the ground (native)

A

gold, silver, platinum

43
Q

zinc, iron, tin, lead and copper are extracted by…

A

reduction (smelting)

44
Q

which 5 metals are extracted using electricity? what is the method called

A

potassium sodium calcium magnesium aluminium, electrolysis

45
Q

what happens in a displacement reaction

A

a more reactive element takes the place of a less reactive one in a compound

46
Q

is potassium or platinum more reactive

A

potassium

47
Q

meaning of reduction

A

loss of oxygen

48
Q

meaning of oxidized

A

gained oxygen

49
Q

why can only some metals be extracted by reduction?

A

they have a lower reactivity than carbon, which is used to displace the metal

50
Q

disadvantage of electrolysis

A

v. expensive as it requires lots of energy

51
Q

meaning of electrolysis

A

using electricity to split a compound

52
Q

2 methods of extraction for low grade ores

A

phytoextraction, bioleaching

53
Q

briefly explain phytoextraction

A

plants absorb metal ions and concentrate these ions in their cells. The plants are burnt leaving plant ash, and the ash is processed using electrolysis or displacement to produce a metal

54
Q

advantages of phytoextraction x2

A

conserves higher grade ores, reduces habitat destruction

55
Q

disadvantages of phytoextraction x2

A

long process, costly labour time

56
Q

briefly explain bioleaching

A

certain bacteria break down low grade ores to produce acidic solution ( leachate), metals can then be extracted by electrolysis or displacement

57
Q

disadvantages of bioleaching

A

toxic products formed

Chemistry (6 decks)

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