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Chemistry > Topic 2: bonding, structure, and properties of matter > Flashcards

Topic 2: bonding, structure, and properties of matter Flashcards

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1
Q

what is ionic bonding?

A

ionic bonding is the electrostatic attraction between positive and negative ions
it is a relatively strong connection

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2
Q

how are ionic compounds held together?

A
  • held together in a giant lattice
  • regular structure that extends in all directions in a substance
  • electrostatic attraction between positive and negative ions hold the structure together
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3
Q

state the properties of ionic substances

A
  • high melting and boiling point
  • strong electrostatic forces between positively charged ions
  • do not conduct electricity when solid (ions are in fixed proportions)
  • conduct when molten or dissolved in water (ions are free to move)
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4
Q

how are ionic compounds formed, explain in terms of MgO

A

reaction of a metal with a non-metal
electron transfer occurs - metal gives away its outer shell electrons to non-metals
Mg is in group II, so has 2 available outer shell electrons
O is in group VI, so can accept 2 electrons to get a full outer shell configuration
Mg becomes Mg2+ and O becomes o2-

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5
Q

what is a covalent bond?

A

covalent bond is a shared pair of electrons between 2 atoms

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6
Q

describe the structure and properties of simple molecular covalent substances

A
  • do not conduct electricity
  • small molecules
  • weak intermolecular forces, therefore
  • low melting and boiling point
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7
Q

how do intermolecular forces change as the mass/size of the molecule increase

A

they increase
cause melting and boiling points to increase as well

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8
Q

what are polymers

A

polymers are very large molecules with atoms linked by covalent bonds

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9
Q

what are thermosoftening polymers

A

a special type of polymer
they melt/ soften when heated
there are no bonds between polymer chains
strong intermolecular forces ensure that the structure is solid at room temp
these forces are overcome by heating - polymer melts

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10
Q

List the properties of giant covalent substances?

A
  • solids, atoms covalently bonded together in a giant lattice
  • high melting and boiling points
  • strong covalent bonds
  • mostly don’t conduct electricity (no delocalized electron)
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11
Q

examples of giant covalent substances

A

diamond, graphite, silicon dioxide

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12
Q

describe and explain the properties of allotropes of carbon:
Diamond

A
  • four very strong covalent bonds for each carbon atom
  • very hard (explanation: strong bonds)
  • very high melting point (explanation: strong bonds)
  • does not conduct electricity (explanation: no delocalised electrons)
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13
Q

describe and explain the properties of allotropes of carbon:
fullerenes:

A
  • hollow-shaped molecules
  • based on hexagonal rings
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14
Q

explain the buckminsterfullerne structure

A

-c60 has a spherical shape, a simple molecular structure

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15
Q

describe and explain the properties of allotropes of carbon:
nanotubes

A
  • cylindrical fullerene with a high length-to-diameter ratio
  • high tensile strength (strong bonds)
  • conductivity (delocalized electrons present)
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16
Q

describe and explain the properties of allotropes of carbon:
graphene

A

a single layer of graphite

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17
Q

describe and explain the properties of allotropes of carbon:
graphite

A
  • 3 layers of covalent bonds for each carbon atom
  • layers of hexagonal rings
  • high melting point
  • layers free to slide as weak intermolecular forces between layers: soft and can be used as a lubricant
  • conduct thermal energy and electrical energy due to one delocalized electron per carbon atom
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18
Q

what is metallic bonding?

A

forces of attraction between delocalized electrons and nuclei of metal ions

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19
Q

describe the properties of metals

A
  • high melting point and boiling point (explanation: strong forces of attraction)
  • good conductors of heat and electricity (explanation: delocalized electron present)
  • malleable, soft (explanation: layers of atoms can slide over each other whilst maintaining the attraction forces)
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20
Q

what are alloys

A

mixture of metal with other elements

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21
Q

why are alloys harder than pure metals?

A

different sizes of atoms distort the layers so they cannot slide over each other therefore alloys are harder than pure metals

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22
Q

what is the melting and boiling point of simple covalent bonds?

A

loe due to weak intermolecular forces between molecules

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23
Q

what is the conductivity when a solid of simple covalent bonds

A

poor, no ions to conduct

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24
Q

what is the conductivity when molten of simple covalent bonds?

A

poor due to no ions to conduct

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25
Q

what is the general description of simple covalent bonds?

A

mostly gases and liquids

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26
Q

what is the boiling point and melting? point of ionic bonds

A

high due to a giant lattice of ions with strong forces between oppositely charged ions

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27
Q

what are the melting and boiling points of giant covalent bonds?

A

high because of many strong covalent bonds between atoms in giant structure

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27
Q

what is the conductivity when a solid of ionic bonding

A

poor due to ions not being able to move

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28
Q

what is the conductivity when molten ionic compounds?

A

good due to ions are free to move

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29
Q

what is the general description of ionic bonds?

A

crystalline solid

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30
Q

what is the conductivity when a solid of giant covalent bonds

A

Diamond and sand: poor, because electrons cannot move
graphite: good as they have delocalized electrons between layers can move through the structure

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31
Q

what is the conductivity when molten of giant covalent bonds

A

poor

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32
Q

general description of giant covalent bonds

A

solids

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32
Q
A
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33
Q

boiling and melting point of metallic bonds

A

high due to strong electrostatic forces between positive ions and delocalized electrons

34
Q

conductivity when solid of metallic bonding

A

good as delocalized electrons are free to move through the structure

35
Q

what is the conductivity of molten metallic bonds?

A

good

36
Q

what is the general description of metallic bonds?

A

shiny metal solids

37
Q

what are the limitations of the simple model?

A

there are no forces between spheres and atoms, molecules and ions are solid spheres - this is not true

38
Q

what does the amount of energy needed to change state from solid to liquid or liquid to gas depending on

A

the strength of the forces between the particles of the substance
stronger forces means higher melting/boiling point so more energy will be needed

39
Q

what are the 3 states of matter?

A

solid, liquid, or gas

40
Q

what is nanoscience

A

science that studies particles that are 1-100nm in size

41
Q

state the uses of nanoparticles

A
  • medicine
  • electronics
  • deodorants
  • sun creams
42
Q

why are nanoparticles good for sun cream?

A

better skin coverage and more effective protection against cell damage
as it has a high surface area:volume ratio

43
Q

diameter of fine particles and give an example

A

100-2500nm
soot

44
Q

diameter of coarse particles

A

2500-10(5) nm diameters

45
Q

why do nanoparticles have high properties different from those for the same materials in bulk?

A

high surface area:volume ratio

46
Q

name 3 types of chemical bond

A

ionic, metallic, covalent

47
Q

define ionic bonding

A

electrostatic attraction between oppositely charged ions

48
Q

define covalent bonding

A

Electrostatic attraction between a positive nucleus and a shared pair of negative electrons.

49
Q

Define metallic bonding.

A

Electrostatic attraction between positively charged ions and delocalised electrons.

50
Q

What type of atoms form ionic bonds?

A

Non-metals with metals.

51
Q

What type of atoms form covalent bonds?

A

Non-metals only.

52
Q

What type of atoms form metallic bonds?

A

metals only

53
Q

What happens to the outer shell electrons when ionic bonds form?

A

Electrons are always transferred from the metal to the non-metal.

54
Q

What happens to the metal atoms in ionic bonding?

A

They lose their outer shell electrons to have a full shell and form a positively charged ion.

55
Q

How can you find out the size of the positive charge on a metal ion?

A

The group number except for transition metals, their charge is shown by Roman numerals.

56
Q

What happens to the non-metal atoms in ionic bonding?

A

They gain outer shell electrons to fill their shell and become negatively charged ions.

57
Q

How can you find out the size of the negative charge on a non-metal ion?

A

8 minus the group number is the size of the negative charge.

58
Q

What charge will a Group 1 metal have?

A

1

59
Q

what charge will a group 2 metal have?

A

2

60
Q

what charge will a group 3 metal have?

A

3

61
Q

what charge will a group 7 non-metal have

A

-1

62
Q

what charge will a group 6 non-metal have

A

-2

63
Q

what charge will a group 5 non-metal have

A

-3

64
Q

why do atoms become ions

A

to attain a full outer-shell of electrons

65
Q

how do you describe ionic bonding in terms of electron transfer

A

State what has happened to the electrons in the metal and then the non-metal. State the charges on the ions that form. Give the formula of the ionic compound formed. State why they transfer electrons.

66
Q

name the first 3 halide ions

A

fluoride, chloride, and bromide

67
Q

Name and write the formula of the GCSE
molecular positive ion

A

Ammonium, NH4+.

68
Q

Name and write the formula of the GCSE molecular 1- ions.

A

Hydroxide, OH- and nitrate, NO3-.

69
Q

Name and write the formula of the GCSE
molecular 2- ions.

A

Sulfate, SO42- and carbonate, CO32-.

70
Q

Name and write the formula of the GCSE
molecular 3- ion.

A

Phosphate, PO43-.

71
Q

Describe how you can work out the
molecular formula of an ionic
compound

A

Label each ions charge. Assign each ion the number of the oppositely charged ion.

72
Q

Describe how you should draw a covalent molecule.

A

Draw the outer electron shell of the atom present in the smallest amount. Draw overlapping circles for the other atoms present. Write x and o in the overlaps. Fill up any missing electrons.

73
Q

Describe how you should draw a metallic element.

A

Draw a box with dashed line circles inside, arrange them in rows, write a + in each circle, label the empty space in the box as delocalised electrons.

74
Q

At what point does a solid melt?

A

its melting point

75
Q

At what point does a gas condense?

A

its boiling point

76
Q

What determines the melting and boiling point of a material?

A

The strength of the forces between the particles.

77
Q

How can you work out the state of a material at a specific temperature?

A

Put the melting point and boiling point at two ends of a continuum, label all temperatures to the left of the melting point as solid, all to the right of the boiling point as gases. Liquids are in between.

78
Q

Write the names and symbols of all 4 state symbols.

A

Solid (s), liquid (l), gas (g) and aqueous (aq).

79
Q

Can an individual particle have a melting point?

A

No because it will not have the same properties as the bulk material and no bonds.

80
Q

State the structure of an ionic compound.

A

giant ionic lattice

81
Q

State the structure of a covalent compound.

A

Small molecule.

82
Q

Describe the melting points of small molecules.

A

weak

83
Q

What is the typical state of a small molecule?

A

liquid or gas

84
Q
A

Chemistry (10 decks)

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