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Chemistry GCSE > 4.2.1/2/3 Bonding, structure properties of matter (must know) PAPER 1 Part 2 > Flashcards

4.2.1/2/3 Bonding, structure properties of matter (must know) PAPER 1 Part 2 Flashcards

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1
Q

Structure of diamond

A

Giant lattice of carbon atoms
C atoms are covalently bonded to 4 others
Tetrahedral shape

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2
Q

Why does diamond have a high mtp

A

Lots of energy needed to break strong covalent bonds throughout giant lattice

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3
Q

Why are diamonds hard

A

Each C atom covalently bonded to 4 others by strong covalent bonds which stops atoms from moving

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4
Q

Why doesn’t diamond conduct electricity

A

No delocalised electrons to carry charge throughout the structure

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5
Q

Uses for diamonds

A

Drill bits

Cutting other diamonds

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6
Q

Structure of graphite

A

Giant lattice of carbon atoms

C atoms are covalently bonded to 3 others in hexagon layers which are held by weak forces of attraction

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7
Q

Why does graphite have a high mtp

A

Lots of energy needed to break strong covalent bonds throughout giant lattice

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8
Q

Why is graphite soft

A

Weak forces of attraction allows layers to slide

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9
Q

Why does graphite conduct electricity

A

Delocalised electrons carry charge through the structure

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10
Q

Uses for graphite

A

Pencil ‘lead’ (soft)
Lubricating machinery (slippery)
Electric motor contacts (conducts electricity)

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11
Q

Structure of fullerenes

A

Linked hexagonal/pentagonal rings of C atoms

Each C atom is bonded to 3 others

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12
Q

Why do fullerenes have low mtps

A

Little energy is needed to break weak intermolecular forces in the molecular structure

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13
Q

Why do fullerenes conduct electricity

A

Delocalised electrons carry charge through the structure

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14
Q

Uses of fullerenes

A

Delivering drugs to where needed in the body
Catalysts
Strengthening materials
Very small electrical circuits

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15
Q

Structure of graphene

A

One single layer of graphite

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16
Q

Why does graphene conduct electricity

A

Delocalised electrons carry charge through the structure

17
Q

Why does graphene have a high mtp

A

Lots of energy needed to break strong covalent bonds in giant lattice

18
Q

Why is graphene hard (unlike graphite)

A

No layers so no weak forces
Only strong covalent bonds
So atoms cannot move/slide

19
Q

Describe metallic bonding/structure of a metal

A

A giant lattice of positive metal ions attracted to delocalised electrons

Atoms in metals are arranged in a regular pattern

20
Q

What is the bonding like in metals

A

In metals, the outer shells contain delocalised electrons and can move throughout the whole structure
There are strong forces of electrostatic attraction between the positive metal ions and negative electrons. These forces hold the metal structure together

21
Q

What are the physical properties of metals and why

A

Malleable - Layers of metal ions are same size and slide over each other
Conduct heat - Delocalised electrons carry energy through the structure
Conduct electricity - Delocalised electrons carry charge through the structure
High mpt/bpt - Lots of energy needed to break strong metallic bonds throughout the giant lattice

22
Q

What are alloys

A

A mixture of metals or a metal + a non metal to make it stronger and harder

23
Q

Why are alloys harder than pure metals

A

They have atoms of different sizes which will distort the layers of metal atoms, making it harder for them to slide over each other

24
Q

Limitations of states of matter diagrams

A

No forces shown
All particles are represented as spheres
The spheres are solid

25
Q

What do stronger forces between particles mean

A

The stronger the forces between the particles the higher the melting point and boiling point of the substance.

26
Q

What does the amount of energy needed to change state depend on

A

The strength of the forces between the particles of the substance.

27
Q

How are atoms in polymers linked to eachother
What are the forces between polymer molecules
What state are polymers at room temperature

A

The atoms in the polymer molecules are linked to other atoms by strong covalent bonds
The intermolecular forces between polymer molecules are relatively strong
These substances are solids at room temperature

28
Q

Why are metals good conductors of thermal energy

A

Metals are good conductors of thermal energy because energy is transferred by the delocalised electrons

29
Q

What do the charges have to equal in ionic compounds

A

0, they have to cancel eachother out

Chemistry GCSE (28 decks)

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