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GCSE Chemistry > Bonding Structure And Properties Of Matter > Flashcards

Bonding Structure And Properties Of Matter Flashcards

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1
Q

Name three types of chemical bonds

A

Ionic, covalent and metallic

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2
Q

What are the particles like in an ionic bond?

A

Oppositely charged ions

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3
Q

What do atoms do in a covalent bond to get a full outer shell?

A

Share pairs of electrons

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4
Q

What particles are involved in metallic bonding

A

Positive ions and delocalised electrons

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5
Q

What type of bond is formed between a metal and a nonmetal

A

Ionic bonds

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6
Q

What type of bonding is forms between just nonmetals?

A

Covalent

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7
Q

What type of bonding occurs in metals and alloys?

A

Metallic

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8
Q

What type of bonding involves gain or loss of electrons

A

Ionic

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9
Q

What happens when a metal and a nonmetal form an ionic bond?

A

Electrons in the outer shell of the metal atom are transferred to the nonmetal

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10
Q

What is the group number if an element forms of -2 ion

A

6

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11
Q

If an atom loses two electrons to form an ion, what charge will the ions have?

A

2+

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12
Q

What happens to a metal when forming an ionic bond?

A

Loses electrons and becomes positively charged - size of a charge is the same as the number of electrons lost. AKA lose one electron= +1 loses two electrons = +2

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13
Q

What happens to a nonmetal when forming an ionic bond

A

Gains electrons and becomes negatively charged -size of the charged is the same as the number of electrons gained. AKA gain one election = -1 charge and gain two electrons = -2

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14
Q

Why do metals and nonmetals form ionic bonds?

A

To get a full outer shell and therefore have the electronic structure of a noble gas

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15
Q

How can the transfer of electrons when forming an ion be represented?

A

Dot And cross diagram is

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16
Q

What are the limitations of using dot and cross diagram to represent ionic compounds?

A

It does not show how the ions are arranged in the space and does not show structure in 3-D.

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17
Q

What type of bonding is likely to occur between group one and two metals with group 6 and seven nonmetals

A

Ionic

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18
Q

Describe how magnesium and oxygen form an ionic bond

A

Magnesium loses two electrons and forms of 2+ ion magnesium gains two electrons and forms of 2- ion

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19
Q

What is a type of force that exist between oppositely charged ions?

A

Electrostatic

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20
Q

What type of structure is found in ionic compounds

A

Giant lattice

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21
Q

Describe the bonding and structure in an ionic compound

A

Giant lattice
Strong electrostatic attraction between oppositely charged ions with the forces acting in all directions

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22
Q

How can the structure of sodium chloride be represented, what are the limitations?

A

Space fill model: shows relative sizes of ions and regular pattern but can only see outer layer.

Ball and stick model: shows all the ions, bonds aren’t represented by lines, don’t show outer electrons.

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23
Q

What must the charges do when working out the formula of an ionic compound?

A

Cancel out

Eg

Na(+) and Cl(-)is NaCl

Mg(2+) and Cl(-) need 2 of cl- to cancel out the 2+ from mg

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24
Q

What are the properties of ionic compounds?

A

have a high melting points/high boiling point

Can conduct when molten (melted so liquid) or when in solution (dissolved in water)

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25
Q

Why do ionic compounds have high melting points?

A

Due to the strong electrostatic attraction between oppositely charged ions, which requires a lot of energy to break

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26
Q

Why do ionic compounds conduct when melted or dissolved in water?

A

Ions are free to move,they can’t move when they’re solid, and can carry a charge.

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27
Q

How do you workout the empirical formula of ionic compounds from a diagram?

A

Work out the chargers on the ions and balance them out

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28
Q

A compound is made up of calcium ions and chloride what is it empirical formula?

A

Calcium is in group 2, so forms of, 2+ ion
Chloride in group 7 so forms of 1- ion

Need two chlorides to balance out the charge on the calcium

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29
Q

How are covalent bonds formed?

A

By sharing electrons

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30
Q

How many electrons does each atom donate in a single covalent bonds?

A

One

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31
Q

What is the strength of a covalent bond?

A

Strong

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32
Q

What are the two types of covalent structure?

A

Small molecules and giant covalent

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33
Q

How are covalent bonds represented in small molecules?

A

Dot And cross - shows electrons shared
Displayed formula - shows covalent bonds as lines
Space fill - shows arrangement of atoms in 3-D

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34
Q

What type of structure is shown? H-C-H

A

Displayed - it shows covalent bonds as single lines between atoms

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35
Q

What are the limitations of using a displayed formula?

A

Does not show 3-D structure
Does not show where the electrons in a covalent bonds have come from

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36
Q

What type of bonding do you get in polymers?

A

Covalent, where N is a large number this is polyethylene

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37
Q

How are the atoms links in a polymer?

A

By strong covalent bonds between the atoms
weak intermolecular forces between the polymer chains

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38
Q

What are the properties of small covalent molecules?

A

Low melting points/boiling points, therefore gases mostly at room temperature
do not conduct electricity

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39
Q

Why do small covalent molecules have low boiling points, are gases and evaporate easily?

A

They have a weak intermolecular forces, which don’t require much energy to break

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40
Q

What happens to the boiling point of simple covalent molecules with increasing size?

A

Increases because there are more of the weak intermolecular forces present

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41
Q

Which has the highest boiling point of hydrogen or methane

A

Methane as it is a large molecule, so there are more intermolecular forces present so more energy need to break this

42
Q

Why don’t simple, covalent molecules, conduct electricity

A

they have no ions (charged particles), or free delocalised electrons

43
Q

Name three giant covalent structures

A

Diamond graphite silicon dioxide

44
Q

What are the melting point of the giant covalent structures?

A

Hi

45
Q

What are the properties of diamonds?

A

High, melting point
Hard
Does not conduct electricity

46
Q

Explain the properties of diamonds

A

High melting points/hard because it has lots of strong covalent bonds (each C atom bonded to 4 other atoms) which require a lot of energy to break

Does not conduct electricity because it has no free delocalised electrons

47
Q

Describe the structure and bonding in diamond

A

Giant covalent held together by lots of strong covalent bonds

48
Q

What are the properties of graphite?

A

High melting point

Soft/slippery

Does conduct electricity because only three out of four carbon electrons in valent shell are being used so has a delocalised electron

49
Q

Explain the properties of graphite

A

High melting point because it has a lot of strong covalent bonds (each C is bonded to 3 other atoms) which require a lot of energy to break

Soft/slippery because the layers are held together, by weak intermolecular forces, which can slide over each other

Does conducts electricity because it has delocalised electrons that are able to move through structure and carry charge

50
Q

Why is graphite soft and slippery?

A

Weak intermolecular forces between layers, which means the layers can slide past each other

51
Q

Why does graphite conduct?

A

As each C atom is bonded to 3 other C atoms leaves a delocalised electron which is able to move through the structure and carry a charge

52
Q

What is graphene

A

A single layer of graphite

53
Q

What are the properties of graphene?

A

Strong - strong, covalent bonds
Can conduct electricity for the same reason as graphite

54
Q

What are the uses of graphene?

A

Electronics Composites - as strong and light can be added as composite to improve strength without adding much weight

55
Q

What are carbon nanotubes

A

Sheet of graphene roles as a tube, call them a cylinder shape

56
Q

What are the properties of carbon nano tube?

A

Strong -strong, covalent bonds
Conducts electricity -delocalised electrons free to move through structure

57
Q

What are the uses of carbon nanoubes?

A

Electronics
Nanotechnology
Materials

58
Q

What are fullerenes?

A

Molecules of carbon atoms with hollow shapes based on hexagons of carbon atoms

59
Q

What was the first fullerene discovered?

A

Buckminsterfullerene C60 which is a spherical shape

60
Q

What are the properties of fullerenes?

A

Strong
Conduct electricity and thermal energy due to delocalised electrons

61
Q

What are the use of fullerenes?

A

Drug delivery
Catalysts

62
Q

What is the structure of metallic substances

A

Giant lattice

63
Q

What are the properties and bonding in a metal?

A

High melting points, (most)
Can conduct electricity
Malleable

64
Q

Describe the structure and bonding in metal

A

Giant lattice
Strong electrostatic attraction between positive metal ions and delocalised electrons

65
Q

Why do metals mostly have high, melting and boiling points

A

Strong electrostatic attraction between positive metal ions and delocalised electrons which require lots of energy to break

66
Q

Why do metals conduct?

A

They have Delocalised elections which are free to move through the structure and carry the current

67
Q

Why are metals malleable?

A

Layers of atoms can slide past each other

68
Q

Why are pure metals not suitable for many uses?

A

Too soft

69
Q

What is an alloy?

A

A mixture of metals

70
Q

Why are alloys harder than pure metals

A

Different size atoms disrupt the layers so layers of atoms can’t slide past each other as easily

71
Q

What are the three states of matter?

A

Solid liquid gas

72
Q

What takes place at the melting point

A

Melting and freezing

73
Q

What takes place at the boiling point

A

Boiling and condensing

74
Q

How can you represent the three states of matter?

A

Using a simple model represented small, solid spheres

75
Q

What does the energy needed to change the state depend upon?

A

The strength of force between the particles, the stronger the force, which depends upon the bonding and structure the higher, melting point and boiling point

76
Q

What are the limitations of the particle model

A

The model assumes no forces involved. All the particles represent as a spheres on the spheres are solid.

77
Q

What are the four state symbols?

A

Solid (s)
Liquid (l)
Gas (g)
Aqueous solution (aq) when something is dissolved in water

78
Q

How are the particles arranged in a solid?

A

Tightly packed
Regular arrangement and fix position
Have a definite shape and volume
Can’t be compressed

79
Q

How are the particles arranged in a liquid?

A

Close together
Disordered arrangement for free to move past each other
Able to flow
Have a fixed volume
Take the shape of its container
Can’t be compressed

80
Q

How are the particles arranged in a gas

A

Far apart
Random arrangement
No fixed volume or shape
Can be compressed

81
Q

What happens to bonds/forces when melting

A

They are weakened

82
Q

What happens to the bonds/forces when boiling

A

They are broken

83
Q

What is gains during melting and boiling?

A

Energy

84
Q

What is the name of the process turning a liquid to a gas?

A

Evaporation/boiling

85
Q

What is the name of the process turning a gas to a liquid?

A

Condensation

86
Q

What is the name of the process turning a liquid to a solid

A

Freezing

87
Q

What is the name of the process trying a solid to a liquid

A

Melting

88
Q

What is nano science?

A

Structures that are 1-100nm in size of the order of a few hundred atoms

(1x10(-9)m

89
Q

What size are fine particles PM2.5

A

Have diameters between 100-2500nm

90
Q

What size are coarse particles PM10

A

Have diameters between 1x10(-5) m - 2.5x10(-6) m
Referred to as dust

91
Q

Which particles are the smallest -
Nano particles, fine particles or coarse particles

A

Nano particles -have the smallest size

92
Q

Give some uses of nano particles

A

Many applications in medicine
Electronics
Cosmetics
Suncream
Deodorant
Catalysts

93
Q

Suggest a use for a nano particle which has antibacterial properties

A

Bandages
Wound dressings
Face masks
Deodorant
Socks

94
Q

Give a property of a nanoparticle if it is to be used in a computer chip?

A

Conduct electricity

95
Q

What are the suggest a possible risks of using nano particles in cosmetics?

A

Potential cell damage to the body(small enough to pass through the skin and remain in the body) harmful effects on the environment after being washed off the skin

96
Q

Why are catalysts in the form of nano particles more efficient?

A

A much higher surface area for reactions take place

97
Q

Why did the properties of nano particles differ to bulk materials

A

Due to the high surface area to volume ratio, smaller quantities are needed to be as effective as normal sized particles

98
Q

Suggest reasons why it costs less to use nano particles rather than fine particles in suncream

A

Greater surface area to volume ratio less can be used for the same affect

99
Q

Give me advantage of using nano particles in sun creams than other sun creams

A

Better coverage
More protection from the sun ultra Violet waves

100
Q

What happens to the surface area to volume ratio when the side of a cube decreases by a factor of 10

A

The area to volume ratio increases by a factor of 10

101
Q

How to workout the surface area to volume ratio

A
  1. Calculate the area of the cube.
  2. calculate the volume of the cube
  3. Divide areas by the volume.
  4. Write values in format surface area: volume
102
Q

Example of a calculation to determine the service area to volume ratio of a cube with side lengths of 50nm

A
  1. SurfaceArea = 50x50x6 —> 15000nm
  2. Volume is 50x50x50 —> 125000nm
  3. 15000/125000 —> 0.12nm
    Ratio = 0.12 : 1

GCSE Chemistry (7 decks)

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