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Chemistry Paper 1 > Topic 2 Using Spec > Flashcards

Topic 2 Using Spec Flashcards

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1
Q

What happens when an atom loses one or more electrons

A

It becomes a cation - a positively charged ion

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2
Q

What happens when an atom gains one or more electrons

A

Becomes an anion - a negatively charged ion

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3
Q

How are ionic bonds formed

A

When the transfer of electrons occurs an electrostatic attraction between the two ions of opposite charge takes place and an ionic bond is formed.

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4
Q

What is an ion

A

An ion is an atom or group of atoms with a positive or negative charge .

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5
Q

When do materials with ionic bonds conduct electricity

A

When molten and high melting points

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6
Q

When do ionic compounds end in -ide

A

When made from 2 different elements

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7
Q

When do ionic compounds end in -ate

A

When the ionic compound is made from 3 or more different elements

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8
Q

Explain the structure of an ionic compound as a lattice structure

A

Oppositely charged ions are held together in ionic lattices. Ionic lattices are giant structures that are held together by strong electrostatic forces between the positive and negative ions.

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9
Q

Deduce the formula for sodium carbonate.

A

Sodium carbonate contains Na+ and CO32- ions:

this is one positive charge and two negative charges
to balance, two Na+ ions and one CO32- ions are needed
so the formula is Na2CO3

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10
Q

Explain how a covalent bond is formed when a pair of electrons is shared between two atoms

A

Covalent bonds are formed when 2 non-metal atoms share pairs of electrons.
These electrons are found on the outer shell of the atoms. Covalent bonds are strong because the shared electrons are attracted to the nucleus of both atoms

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11
Q

covalent bonding results in the formation of what molecules?

A 
Small molecules (water)
Large molecules (polymers)
Giant covalent structures (diamond)
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12
Q

What kind of covalent bond is hydrogen

A

Single covalent bond as each hydrogen atom shares 1 electron with the other

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13
Q

What kind of covalent bond is water

A

Single covalent with 2 hydrogen atoms

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14
Q

What type of covalent bond is oxygen

A

Double covalent bond as it needs 2 electrons to get a full outer shell

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15
Q

What are the properties of the lattice structure in the ionic compounds

A

High melting and boiling points
Don’t conduct electricity if solid
Conduct electricity if liquid or in solution

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16
Q

Why do lattice structures have a high melting and boiling point

A

Because to break the ionic bonds, a lot of energy is needed to overcome the electrostatic forces between the ions and electrons.

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17
Q

Why can’t the lattice structure conduct electricity if solid

A

When solid the ions are fixed in place therefore charges cannot flow so electricity cannot be conducted

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18
Q

Why can the lattice structure conduct electricity if liquid or in solution

A

When molten or dissolved in water, the ions in the lattice can move freely therefore charges can flow and electricity can be conducted

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19
Q

What is an example of a small molecule

A

Chlorine as it has weak intermolecular forces between its molecules

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20
Q

What is an example of a bigger molecule

A

Sucrose as its intermolecular forced are strong

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21
Q

What are the properties of small covalent molecules

A

Lower melting/boiling points

Don’t conduct electricity

22
Q

What are the properties of large covalent molecules

A

High melting/boiling point

Don’t conduct electricity

23
Q

Why are small covalent molecules liquid or gases at room temperature

A

When small molecules melt or boil, it’s the weak intermolecular forces that break.
Since these intermolecular forces are weak and break easily, simple covalent molecules have very low melting and boiling points.
Therefore, they exist as liquid and gases at room temperature.

24
Q

What are the properties of giant covalent structures

A

Very high melting points

1 large molecule

25
Q

Why does giant covalent structures have very high melting points

A

As the string covalent bonds between atoms make them solid at room temperature
High temperatures and significant energy are required to break the structures covalent bonds

26
Q

Why is 1 large molecule a property of giant covalent structures

A

There are no intermolecular forces because there is only 1 molecule

27
Q

What are some example of giant covalent structures

A

Graphite and diamond

28
Q

Explain why elements and compounds can be classified as metallic

A

As they only have a few atoms

29
Q

Explain why elements and compounds can be classified as ionic

A

As the Ionic compounds contain ions and are held together by the attractive forces among the oppositely charged ions.

30
Q

Explain why elements and compounds can be classified as simple molecular

A

Simple molecules contain only a few atoms held together by covalent bonds

31
Q

What is diamond

A

An allotrope of carbon

32
Q

What are the properties of diamond

A

Covalent bonds
High melting point
Hard
Does not conduct electricity

33
Q

Describe the covalent bonds in diamond

A

Each carbon atom is bonded to 4 other carbon atoms by strong covalent bonds which creates a giant covalent structure

34
Q

Why does diamond have a high melting point

A

Lots of strong covalent bonds so requires a lot of energy to break the bonds

35
Q

Why is diamond hard

A

Lots of strong covalent bonds

36
Q

Why does diamond not conduct electricity

A

As there are no delocalised electrons

37
Q

Why are graphite and diamond different types of carbon

A

Graphite conducts electricity as there is one delocalised electron from every carbon atom
Diamond is hard whereas graphite is soft
Each carbon atom in graphite is bonded to 3 other carbon atoms by strong covalent bonds.

38
Q

Why is graphite useful as a lubricant and as pencil lead

A

As the layers can easily slide over one another as the intermolecular forces keeping the layers together are weak so graphite is very soft

39
Q

Why is diamond used for cutting tools

A

As diamond is very hard due to its strong covalent bonds

40
Q

What is fullerenes

A

Molecules of carbon atoms that take up hollow structures

41
Q

Describe the structure of fullerenes

A

Carbon atoms arranged in a hexagonal rings but pentagonal and heptagon all rings can be found as well

42
Q

What was the first fullerene to be discovered

A

Buckiminsterfullerane - spherical shape and formula c60

43
Q

What are the properties of graphene

A

Conducts electricity- each carbon atom has a delocalised electron
Light but strong- almost a two dimensional structure but has strong covalent bonds between carbon atoms

44
Q

What can graphene be used for

A

Solar panels

Batteries

45
Q

What are polymers

A

Large chain like molecules
Held together by strong covalent bonds between atoms in molecules
Weak intermolecular forces between molecules

46
Q

Why do many polymers melt easily

A

The intermolecular forces remain less strong than chemical bonds

47
Q

What is poly (ethane)

A

An addition polymer

48
Q

What are the properties of pure metals

A

Soft and malleable- ions are arrange in layers that easily move over each other when a force is applied
High melting and boil point strong electrostatic forces between metal ions and delocalised electrons.

49
Q

What are the advantages and disadvantages of dot and cross model

A

Pro - shows the bonding

Con - doesn’t show how the ions are arranged in space

50
Q

Ball and stick advantages and disadvantages

A

Pro - illustrates arrangement of atoms in 3D space

Con - doesn’t show movement of electrons

51
Q

2-3 dimensional representation model advantages and disadvantages

A

Pros - Shows how much space and atom uses

Con- hard to see structure of whole molecule clearly

52
Q

Properties of non metals

A

Low boiling points

Poor conductors of electricity

Chemistry Paper 1 (4 decks)

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