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Chemistry-Paper1 > C3:Structure And Bonding > Flashcards

C3:Structure And Bonding Flashcards

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1
Q

What are the three states of matter

A

Solids, liquids and gases

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2
Q

Structure of a solid

A

Particles are packed closely together and vibrate around fixed positions, they have strong intermolecular forces, can’t be compressed

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3
Q

Structure of a liquid

A

Particles are close together but they can slip and slide across each other in random motion as their intermolecular forces are weaker, can’t be compressed, take the shape of their container

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4
Q

Structure of a gas

A

Weak intermolecular forces, lots of energy, lots of space between particles, can be compressed

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5
Q

What happens to the energy transferred in melting and boiling

A

Energy is transferred from the surroundings to the substance

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6
Q

What happens to the energy transferred in freezing and condensing

A

Energy is transferred from the substance to the surroundings

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7
Q

Advantage of the simple particle model

A

Useful

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8
Q

Disadvantages of the particle model

A

The atoms, molecules and ions that make up all substances are not solid spheres with no forces between them

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9
Q

What do elements react together to form

A

Compounds

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10
Q

How are compounds formed

A

When elements react together by gaining or losing or sharing electrons

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11
Q

What group do group 1 elements react with

A

Group 7

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12
Q

Why does group 1 elements react well with group 7

A

As group 1 elements lose one electron to gain the stable electronic striction of a noble gas, this electron can be given to an atom from group 7 which also achieves the stable electronic structure of a Noble has

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13
Q

Ionic bonding

A

Ionic compounds held together by strong forces of electrostatic attraction between the positively and negatively charged ions

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14
Q

What groups can react to form ionic compounds

A

1 and 7

2 and 6

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15
Q

What do group 2 elements form in ionic bonding

A

2+ ions as they lose 2 outer shell electrons

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16
Q

What do group 6 elements form in ionic bonding

A

2- ions as they gained 2 electrons

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17
Q

Name for giant ionic compound

A

Giant ionic lattice

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18
Q

Why do giant ionic compounds have high melting points

A

As it takes a lot of energy to break the many string ionic bonds

19
Q

What state are giant ionic lattices At room temperature

A

Solids

20
Q

When will ionic compounds conduct electricity

A

When molten or dissolved in water as their ions can become mobile and carry charge through the liquid

21
Q

When are covalent bonds formed

A

When atoms of non-metals share pairs of electrons with each other

22
Q

What do many substances containing covalent bonds consist of

A

Simple molecules but some have giant covalent structures

23
Q

Properties of substances made of simple molecules

A

Low melting and boiling points

24
Q

What are ions

A

Charged particles

25
Q

Why do simple molecules have low melting and boiling points

A

As the intermolecular forces are weak

26
Q

Charge of a simple molecule

A

No charge so they can’t carry and electrical charge or conduct electricity

27
Q

Describe graphite

A

Contains giant layers of covalently bonded to 3 carbon atoms. However, there are no covalent bonds between the layers. This means they can slide over each other making graphite soft and slippery

28
Q

Describe diamond

A

Covalently bondéd to 4 carbon atoms they have a rigid giant covalent structure making it a hard substance

29
Q

How can graphite conduct electricity and thermal energy

A

As the third carbon atom that isn’t covalently bonded is lost between the layers to form a sea of delocalised electrons which conducts electricity

30
Q

Structures of fullerenes

A

Form cage-like structures and tubes based on hexagonal rings of carbon atoms

31
Q

What are fullerenes used for

A

A transport mechanism for drugs to specific sites in the body as catalysts and as reinforcement for composite materials

32
Q

What is graphene

A

A single layer of graphite

33
Q

Properties of graphene

A

One atom thick, excellent electrical conductivity will help create new developments in the electronic industry in the future

34
Q

What shows how ionic bonding is formed

A

Dot and cross diagrams

35
Q

Structures of metals

A

Atoms are closely packed together and arranged in regular layers

36
Q

Metallic bonding

A

Positively charged metal ions which are held together by electrons from the outermost shell of each metal atom, these delocalised electrons are free to move throughout the giant metallic lattice

37
Q

Why can metals be shaped and bent

A

As the layers of atoms/ positively charged ions in a giant metallic structure can slide over each other

38
Q

Why are alloys harder than pure metals

A

As the regular layers in a pure metal are distorted by atoms of different sizes in an alloy

39
Q

What do delocalised electrons in metals allow

A

Electricity and thermal energy to be transferred easily

40
Q

What is nano science

A

The study of small particles that are between 1 and 100 nanometers in size

41
Q

Properties of nanoparticles

A

High surface area to volume ratio, high percentage of their atoms exposed at their surface

42
Q

What will nanoparticles resolve in

A

Much smaller quantities of materials such as catalysts being needed for industrial processes

43
Q

What does new development In nanoparticulate materials mean

A

It’s exciting and could improve aspects of modern life

44
Q

What does The increased use of nanoparticles need

A

More research into possible issues that might arise in terms of health and the environment

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