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Physics And Chemistry 2024 Year 10 > C3-Structure And Bonding > Flashcards

C3-Structure And Bonding Flashcards

1
Q

What is an ionic bond

A

Ionic bond is force that hold them together and ionic compound is everything.

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2
Q

What are ionic compounds held by

A

Ionic compounds are held by strong electrostatic forces of attraction by there oppositly charge ionic bonding.Between a metal and a non metal

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3
Q

Ionic charges Group 1,2,3

A

1+,2+,3+

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4
Q

Ionic charges group 5,6,7

A

3-,2-,1-/-

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5
Q

Ammonium

A

NH4+
+1 ion

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6
Q

Nitrate

A

No3 -
-1 ionic charge

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7
Q

Sulfate

A

So4 2-
2- ionic charge

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8
Q

Carbonate

A

Co3
2- ionic charge

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9
Q

Phosphate

A

Po4
3- ionic charge

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10
Q

Zinc

A

Zn
2+ ionic charge

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11
Q

States of matter

A

Solid,liquid,gas,aqueos

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12
Q

Ionic solids

A

Fixed in position in a giant lattice.Vibrate but no movement.Cannot conduct electricity

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13
Q

Molten ionic compounds

A

High temperatures provides enough energy to overcome the many strong attractive forces between ipns.Ions are free to move.
Conducts electricity

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14
Q

Ionic compound in solution

A

Water molecules seperate ions from the lattice.Ions are free to move around within the solution.
Conducts electricity

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15
Q

When do ionic compounds conduct electricity

A

When they are molten or dissolved in water.This is because their ions can then become mobile and can carry charge throughout the liquid

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16
Q

Lattice

A

The electrostatic forces of attraction between the oppositely charged ions in an ionic compound are veru strong. operating in all directions. The regular arrangement of ions in the giant lattice results in ionic compounds forming crystals.
The ball and stick model shows the 1: 1 ratio of Na and Cl ions in NaCl

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17
Q

What is a covalent bond

A

A bond between a non metal where they share electrons

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18
Q

What is an alloy

A

a mixture of two or more elements, at least one of which is a metal

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19
Q

What is a delocalised electrom

A

bonding electron that is no longer associated with any one particular atom

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20
Q

What is a dot and cross diagram

A

a drawing to show only the arrangement of outer shell electrons of the atoms or ions in a substance

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21
Q

What is fullerene

A

form of the element carbon that can exist as large cage-like structures, based on hexagonal rings of carbon atoms

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22
Q

What is a giant covalent structure

A

a huge 3D network of covalently bonded atoms

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23
Q

What is a giant lattice

A

a huge 3D network of atoms or ions

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24
Q

What is the intermolecular force

A

the attraction between the individual molecules in a covalently bonded substance

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25
Q

What is a liquid

A

substances that have a fixed volume, but they can flow and change their shape

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26
Q

What is an ionic bond

A

the electrostatic force of attraction between positively and negatively charged ions

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27
Q

What is particle theory

A

a theory that explains the properties of solids, liquids and gases based on the fact that all matter is made from tiny
particles. It describes the movement of particles and the distance between them

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28
Q

What is a polymer

A

a substance made from very large molecules made up of many repeating units

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29
Q

What is the state of matter

A

the forms in which matter can exist. A substance can be solid, liquid or gas

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30
Q

How are ionic compounds held together?

A

• They are held together in a giant lattice.
• It’s a regular structure that extends in all directions in a substance.
• Electrostatic attraction between positive and negative ions holds the structure together.

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31
Q

How are ionic compounds formed? Explain in terms of MgO case.

A

Reaction of a metal with a non-metal.
Electron transfer occurs - metal gives away its outer shell electrons to non-metal.
Mg is in Group Il, 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 Mg?* and O becomes O2- (oxide).

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32
Q

How do intermolecular forces change as the mass/size of the molecule increases?

A

They increase. That causes melting/boiling points to increase as well (more energy needed to overcome these forces).

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33
Q

What are thermosoftening polymers

A

Thermosoftening polymers - special type of polymers; they melt/soften when heated. There are no bonds between polymer chains. Weak intermolecular forces ensure that the structure is solid at room temperature. These forces are overcome with heating - polymer melts.

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34
Q

What are giant covalent substances? Give examples

A
  • Solids, atoms covalently bonded together in a giant lattice.
  • High melting/boiling points - strong covalent bonds.
  • Mostly don’t conduct electricity (no delocalised e )
  • Diamond, graphite, silicon dioxide.
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35
Q

Describe and explain the properties of allotropes of carbon. Diamond

A

Diamond
- four, strong covalent bonds for each carbon atom
- very hard (Strong bonds)
- very high melting point (strong bonds)
- does not conduct (no delocalised electrons)
-Giant covalent structure.

36
Q

Describe and explain the properties of the allotropes of carbon,fullerenes and nanotubes

A

Fullerenes
- hollow shaped molecules
- based on hexagonal rings but may have
5/7-carbon rings
- C6o has spherical shape, simple molecular structure (Buckminsterfullerene)
-Have a large surface area to volume ratio
Nanotubes
- cylindrical fullerene with high length to diameter ratio
- High tensile strength (strong bonds)
- Conductivity (deloc. electrons)
Graphene - a single layer of graphite.

37
Q

What is metallic bonding

A

Forces of attraction between delocalised electrons and nuclei of metal ions.

38
Q

Describe the properties of metal

A

High melting/boiling points (strong forces of attraction)
- Good conductors of heat and electricity (delocalised electrons)
- Malleable, soft (layers of atoms can slide over each other whilst maintaining the attraction forces)

39
Q

Why are alloys harder than pure metals?

A

different sizes of atoms distorts the layers, so they can’t slide over each other, therefore alloys are harder than pure metals

40
Q

Properties of simple covalent bonda

A

Low melting point and boiling,does not conduct electricity when solid pr molten.

41
Q

Propertys of ionic

A

High melting and boiling due to strong forces between oppositley charged ions,no conductivity when solid but when molten conductablw

42
Q

Properties of giant covalent bonds

A

High melting and boiling points,diamond and sand poor(cannot move),graphite conduct when solid as delocalised electrons can move,when molten poor conductor

43
Q

Properties of mettalic

A

High melting and boiling points,good conducter when solid and molten

44
Q

Limitations of the simple model

A

No forces between spheres and atoms,molecules and ipns are solid spheres-this is not true

45
Q

What does the amount of energy needed to change state from solid to liquid or liquid to gas depend on?

A

The strength of the forces between the particles of the substance. The nature of the particles involved depends on the type of bonding and the structure of the substance. The stronger the forces between the particles the higher the melting point and boiling point of the substance

46
Q

A pure substance will melt or boil at…?

A

A fixed temperature.
A mixture will melt over a range of temperatures.

47
Q

What is nanoscience

A

Science that studies that are 1-100nm in size

48
Q

Why do nanoparticles have properties different from those for the same materials in bulk

A

Higher surface area to volume ratio

49
Q

Ionic bonding

A

Metal + Non-metal: electrons in the outer shell of the metal atom are transferred
• Metal atoms lose electrons to become positively charged ions
• Non-metal atoms gain electrons to become negatively charged ions
• An ion is an atom that has lost or gained electron(s).

50
Q

Metallic bonding

A

The bonding in a metal consists of positive ions (atoms that have lost electron(s)) and delocalised electrons arranged in a regular pattern.
• The delocalised electron system consists of the electrons ‘lost’ from the atoms to form positive ions.
• Del dalised slectrons are free to move through the structure.
The delocalised electrons are shared through the structure so metallic bonds are strong.

51
Q

Properties of ionic compounds

A

Ionic compounds have regular structures (giant ionic lattices) in which there are strong electrostatic forces of attraction in all directions between oppositely charged ions.
• They have high melting and boiling points, because a lot of energy is required to break the many strong bonds.
• When melted or dissolved in water, ionic compounds conduct electricity because the ions are free to move and carry current. But they can’t conduct electricity when solid because the ions are fixed in place.

52
Q

Properties of small molecules

A

Substances that consist of small molecules are usually gases or liquids that have low boiling and melting.
• They have weak intermolecular forces between the molecules. These are broken in boiling or melting, not the covalent bonds.
• The intermolecular forces increase with the size of the molecules, so larger molecules have higher melting and boiling points.
• Substances that consist of small molecules don’t conduct electricity, because small molecules do not have an overall electric charge.

53
Q

Uses of nanoparticles

A

They have a high surface area to volume ratio, and therefore would make good catalysts.
• They can also be used to produce highly selective sensors.
• Nanotubes could make stronger, lighter building materials.
• New cosmetics, e.g sun tan cream and deodorant. They
• Lubricant coatings, as they reduce friction. These can be used for artificial joints and
Nanotubes conduct electricity, so can be used in small electrical circuits for
possible disadvantages: there are some concerns that nanoparticles may be toxic to people. They may be able to enter the brain from the bloodstream and cause harm.

54
Q

Possible risks of nanoparticles

A

Due to there large surface area If a spark is made by accident near a large quantity of the catalyst, there could be a violent explosion.

Higher risk of finding their way into the atmosphere. In general, Breathing in tiny particles could damagethe lungs.

55
Q

How to calculate surface area to volume ratio

A

Sa=basexheightx6cm^2
V=basexheightxwidth

56
Q

1 nanometre

A

1x10-9 meters

57
Q

Why does nano particles save money

A

Its costs less as you need a smaller amount of it due to its larger suface area to volume ratio

58
Q

Properties of metals

A

Male-able,bendable,ductile,strechable

59
Q

Bonding between metals

A

Closely packed together,delocalised electrons are free to move throughout thr giant mettalic lattice

60
Q

What is a metal bonding considered with delocalised electrons in it

A

A sea of delocalised electeons

61
Q

Formula for diamond,graphite,buckminsterfullerene,graphene

A

Diamond=c,graphite=c,buckminsterfullerene=c60,graphenevc

62
Q

Graphite-giant covalent structure

A

Giant layers of covalently bonded carbon atoms.No covalent bonds between layers.This means they can slide over eachother.

63
Q

For simple molecules describe its forces within

A

Strong covalent bonds but weak force between molecules(weak intermolecular force

64
Q

Charge of simple molecules

A

No overallcharge

65
Q

What is a simple molecular substance

A

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

66
Q

Common examples of simple molecules

A

H2-hydrogen
O2-oxygen
Ch4-methane
Cl2-Chlorine
N2-Nitrogen
H20-Water
Hcl-Hydrogen Chloride

67
Q

Properties of simple molecular substances

A

Contain and are held by strong covalent bonds,forces of attraction are week(intermolecular forces),low melting and boiling point,Most molecular substances are gases or liquids at room temperature,as the molecules get bigger there intermolecular force increases increasing there melting and boiling point,do not conduct electricity

68
Q

Explain why oxygen is a gas at room temperature

A

Because of irs weak intermolecular forces are broken allowing them to move freely.

69
Q

What state is a polymer at room temperature

A

Solid

70
Q

What is an allotrope

A

Different structural form of the same element in the same physical state eg.diamond

71
Q

Explain and show the properties of the allotropes of carbon graphite

A

Graphite
- three covalent bonds for each carbon atom
- contains layers of hexagonal rings
- high melting point
- layers free to slide as weak intermolecular forces between layers; soft, can be used as a lubricant
- conduct thermal and electricity due to one delocalised electron per each carbon atom
-Sheets of carbon
-Has three out of the four carbons used so it has a extra carbon which is delocalised and can move so therefore it can conduct electricity

72
Q

Describe and explain the properties of the allotropes of carbon-graphite

A

Graphene - a single layer of graphite joined together in hexagons
-Very strong covalent bonds
-Very light
-Can be added to a composite material to improve their strength without adding much weight
-Contains a delocalised electron so therefore can conduct electricity
-Potential to be used in electrons

73
Q

How strong the forces of attraction depends on three things

A

-the material
-temperature
-pressure

74
Q

Properties of solids

A

Strong forces of attraction,form a very regular lattice arangement
-particles do not move from their positions
-particles vibrate in a fixed position

75
Q

Properties of liquids

A

Weak forces of attraction,tend to stick closely to eachother,Have a definite volume but dont keep a definite shape,particles are constantly moving with a random motion,hotter the liquid the faster they move

76
Q

What is an aqueous solution

A

aqueous solution” is a solution in which water is the solvent, such as salt dissolved in water

77
Q

Properties of gases

A

Weak forces of attraction,free to move,don’t keep a definite shape or volume,move constantly,gases either expand when heated or their pressure increased

78
Q

Defintion of physical change

A

The changing of a particles arrangement or their energy

79
Q

What happens when a solid is heated

A

When a solid is heated the particles vibrate more,which weakens the forces of attraction,at certain temperatures called the melting point the particles have enough energy to break free.This is when it turns into a liquid,when its heated again it gets even more energy,Which makes it move even fastee and then this breaks its bond again passing its boiling point turning into a gas

80
Q

What happens when a gas is cooled

A

When a gas is cooled the particles no longer have enough energy to overcome the forces of attraction,bonds form between the particles,at the boiling point so many bonds have formed between the gas particles that the gas condenses and becomes a liquid,when a liquid cools the particles have even less energy and then once it has not enough energy to overcome the attraction so more bonds are formed then it turns into a solid and is known as frozen/freezing

81
Q

What is it if a substance is below the melting point of a substance

A

Solid

82
Q

What if a substance is above the boiling point

A

Gas

83
Q

If its between two points

A

Liquid

84
Q

Surface area to volume ratio

A

Surface area/volume

85
Q

What happens if a particles size decreases

A

The size of their surface area in relation to their volume will increase

Physics And Chemistry 2024 Year 10 (5 decks)

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