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Chemistry > Bonding, Structure and Properties of Matter > Flashcards

Bonding, Structure and Properties of Matter Flashcards

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1
Q

Ion

A

Charged particle formed when an atom/molecule loses/gains electrons to get a full outer shell

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2
Q

What happens when metals form ions

A
  • lose electrons
  • form positive ions
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3
Q

What happens when non-metals form ions

A
  • gain electrons
  • form negative ions
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4
Q

How is charge of an ion determined

A

number of an electrons lost

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5
Q

Most likely groups to form ions

A
  • group 1
  • group 2
  • group 6
  • group 7
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6
Q

Types of bonds

A
  • ionic
  • covalent
  • metallic
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7
Q

ionic bond

A

Strong attraction between oppositely charged ions by electrostatic forces, caused by metals and non-metals reacting together

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8
Q

What happens in an ionic bond

A
  • metal atom loses electrons
  • electrons transferred to non-metal
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9
Q

What diagram shows ionic bonds

A

Dot and cross

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10
Q

Limitations of dot and cross diagram

A

Doesn’t show 3 dimensional nature of structure

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11
Q

Structure of ionic compound

A

Giant ionic lattice

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12
Q

Structure of giant ionic lattice

A
  • ions form closely packed regular lattice arrangement
  • strong electrostatic forces of attraction between oppositely charged particles in all directions in lattice
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13
Q

Properties of ionic compounds

A
  • high melting points
  • high boiling points
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14
Q

Why do ionic compounds have high melting/boiling points

A

There are strong electrostatic forces of attraction between ions that take a lot of energy to overcome

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15
Q

When can ionic compounds conduct electricity

A

When molten

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16
Q

Molten

A

Metled

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17
Q

Why can ionic compounds conduct electricity when molten

A

Ions are free to move and carry a charge

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18
Q

When can’t ionic compounds conduct electricity

A

When solid

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19
Q

Why can’t ionic compounds conduct electricity when solid

A

ions held in place so can’t carry a charge

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20
Q

What happens to some ionic compounds in water

A
  • they dissolve
  • ions separate and are free to move in solution
  • carry electric charge and conduct electricity
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21
Q

Empirical formula

A
  • what atoms are in an ionic compound
  • includes number of each atom
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22
Q

Covalent bond

A
  • bond between non-metals
  • electrons shared to get full outer shells
  • positive nuclei attracted to shared electrons through electrostatic forces
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23
Q

Diagram to show covalent bonds

A

Dot and cross

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24
Q

Simple molecular substances

A

Substances made up of molecules containing a few atoms joined together by covalent bonds

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25
Q

Properties of simple molecular substances

A
  • atoms within molecules held together by very strong covalent bonds
  • forces of attraction between molecules very weak
  • low melting/boiling points
  • usually gas/liquid at room temperature
  • melting/boiling points increase as molecules get bigger
  • don’t conduct electricity
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26
Q

Why do simple molecular structures have low melting/boiling points

A

To melt/boil, only have to break weak intermolecular forces (easy to do)

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27
Q

Why do melting/boiling points of simple molecular substances increase as they get bigger

A
  • strength of intermolecular forces increases
  • more energy needed to break them
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28
Q

Why can’t simple molecular structures conduct electricity

A

Not charged so there are no free electrons to carry a charge

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29
Q

Polymers

A

Long chains of repeating small units, forming a long molecule that has repeating sections

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30
Q

How are atoms in polymers linked

A

Strong covalent bonds

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31
Q

How are polymers drawn

A
  • repeating section in brackets
  • ‘n’ outside brackets showing number of sections
32
Q

State of polymers at room temperature

A

Solid

33
Q

Why are polymers solid at room temperature

A

Stronger intermolecular forces, requiring more energy to break them

34
Q

What type of molecule are giant covalent structures

A

Macromolecules

35
Q

Properties of giant covalent structures

A
  • all atoms bonded to each other by strong covalent bonds
  • high melting/boiling points
  • usually can’t conduct electricity
36
Q

Why do giant covalent structures have high melting/boiling points

A

Lots of energy needed to break covalent bonds between atoms

37
Q

Why don’t giant covalent structures usually conduct electricity

A

Don’t contain charged particles

38
Q

Examples of giant covalent structures

A
  • diamond
  • graphite
  • silicon dioxide
39
Q

Allotrope

A

Different structural forms of the same element in the same physical state

40
Q

Allotropes of carbon

A
  • diamond
  • graphite
  • fullerene
41
Q

Properties of diamond

A
  • very hard
  • high melting point
  • doesn’t conduct electricity
42
Q

Why is diamond very hard

A

Each carbon atom forms 4 covalent bonds

43
Q

Why does diamond have a high melting point

A

Covalent bonds are strong and need a lot of energy to break

44
Q

Why doesn’t diamond conduct electricity

A

No free electrons/ions to carry a charge

45
Q

Properties of graphite

A
  • each carbon atom forms 3 covalent bonds, creating sheets of carbon atoms arranged in hexagons
  • layers held together weakly (no covalent bonds) so it is soft and slippery - good lubrication
  • high melting point
  • conducts electricity + thermal energy
46
Q

Why does graphite have a high melting point

A

Covalent bonds require much energy to break

47
Q

Why does graphite conduct electricity and thermal energy

A

Only 3 of carbons electron used in bonds - 1 electron delocalised and free to move

48
Q

Graphene

A
  • 1 layer of graphite
  • sheet of carbon atoms joined together in hexagons
  • 1 atom thick
  • contains delocalised electrons to conduct electricity
49
Q

Fullerene

A
  • molecules of carbon shaped liked closed tubes or hollow balls
  • made up of carbon atoms arranged in hexagon sometimes containing pentagons (rings of 5 carbon atoms) or heptagons (rings of 7 carbon atoms)
  • can form nanotubes
50
Q

Uses of fullerene

A
  • delivering a drug into body - fullerene structure forms around other atoms/molecules and traps them inside
  • industrial catalyst - large surface area, individual catalyst molecules could be attached to fullernes
  • lubrication
51
Q

First fullerene to be discovered

A

Buckminsterfullerene

52
Q

Molecular formula of Buckminsterfullerene

A

C₆₀

53
Q

What does Buckminsterfullerene form

A

Hollow tubes

54
Q

Nanotubes

A

Tiny carbon cylinders

55
Q

Properties of nanotubes

A
  • high ration between length and diameter
  • conduct electricity + thermal energy
  • high tensile strength so don’t break when stretched
56
Q

nanotechnology

A

Technology that uses very small particles like nanotubes

57
Q

Uses of nanotubes

A
  • strengthening materials without adding much weight
  • used in electronics
58
Q

Metallic bonding

A

Strong electrostatic forces of attraction between positive metal ions and shared negative electrons, holding atoms together in a regular struture

59
Q

Properties of metals

A
  • mostly solid at room temperature - high melting/boiling points
  • good conductors of electricity
  • good conductors of heat
  • malleable
  • strong and hard to break
60
Q

Why are most metals solid at room temperature

A

electrostatic forces between metal atoms and sea of delocalised electrons need lots of energy to be broken to melt/boil

61
Q

Why are metals good conductors of electricity/heat

A

delocalised electrons carry electrical charge + thermal energy through whole structure

62
Q

Why are metals malleable

A

Layers of atoms can slide over each other

63
Q

Why aren’t metals always right for certain jobs

A

Often too soft when pure

64
Q

How to deal with metals being too soft for certain jobs

A

Mix them with other metals to make them harder

65
Q

Alloy

A

Mixture of 2 or more metals or a metal and another element

66
Q

Why are alloys harder than pure metals

A
  • different metals have different sized atoms
  • when another element is mixed with a pure metal, new metal atoms will distort layers of metal atoms, making it more difficult fore layers to slide over each other
67
Q

What determines what state something is a certain temperature

A

Strength of forces of attraction between particles of the material

68
Q

What determines strength of forces of attraction between particles in a material

A
  • material - structure of substance + types of bonds holding particles together
  • temperature
  • pressure
69
Q

Criticisms of the particle theory model

A
  • uses inelastic/spherical particles instead of atoms/ions/molecules
  • doesn’t show forces between particles so can’t see how strong they are
70
Q

Aqueous

A

dissolved in water

71
Q

What happens when a solid is heated

A
  • particles gain more energy and vibrate more, this weakens the forces holding the solid together
  • at certain temperature (melting point), particles have enough energy to break free from their positions (melting) and turn into a liquid
72
Q

What happens when a liquid is heated

A
  • particles gain more energy and move faster
  • bonds holding liquid together weaken and break
  • at certain temperature (boiling point), particles have enough energy to break bonds (boiling) and turn into a gas
73
Q

What happens when gases cool

A
  • particles no longer have enough energy to overcome forces of attraction between them
  • bonds form between particles
  • as boiling point, so many bonds have formed between gas particles, it has condensed and become a liquid
74
Q

What happens when liquids cool

A
  • particles have less energy so move around less
  • not enough energy to overcome forces of attraction between particles so bonds form between them
  • at melting point, so many bonds have formed between particles, they’re held in place
  • liquid had frozen to become a solid
75
Q

What determines amount of energy needed for a substance to change state

A

How strong forces between particles are

Chemistry (6 decks)

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