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Chemistry > C3 > Flashcards

C3 Flashcards

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1
Q

Liquid and solid changing state

A

When a solid heats up, it’s particles vibrate faster until they break free from neighbouring particles

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2
Q

Energy transfers whilst changing state

A

When heating a solid, the temperature stops rising at the melting point. At the melting point, the energy transferred from the surroundings goes into breaking the bonds

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3
Q

What is a compound

A

A substance containing two or more elements, chemically bonded together

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4
Q

What ion forms when loosing electrons

A

Positive

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5
Q

What ion forms when gaining electrons

A

Negative

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6
Q

How do we represent ionic structure

A

(2,8,4

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7
Q

How do we represent ionic bonding

A

Dot and cross diagrams

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8
Q

How does ionic bonding work

A

Atoms react to from negative and positive ions. These ions are held together by very strong forces of attraction between the oppositely charged ions acting in all directions

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9
Q

What is a giant ionic lattice

A

Arrangement of ions in ionic bonding in a steady, repeated pattern

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10
Q

What ions do each group produce

A

Group 1 - 1+
Group 2 - 2+
Group 3 - 3+
Group 4 - don’t
Group 5 - 3-
Group 6 - 2-
Group 7 - 1-
Group 8/0 - don’t

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11
Q

Properties of a giant, ionic lattice

A

Very tightly packed, forces act in all directions, hard to break up due to the electrostatic forces, high melting and boiling points

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12
Q

What happens when ionic compounds melt

A

The ions are free to move so can carry an electrical charge

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13
Q

What happens when an ionic compound mixes with water

A

Most will dissolve to form an ionic compound solution which can carry an electrical charge

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14
Q

What type of atoms are involved in ionic bonding

A

Non metal and a metal

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15
Q

What charge do metal ions have

A

Positive

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16
Q

What charge do non metals have

A

Negative

17
Q

Explain simple covalent bonding

A

When two non metals react together, they both want to gain electrons but neither can give them away. They complete their full outer shell by sharing electrons. These strong bonds are known as covalent bonds

18
Q

How to draw covalent bonding

A

Dots and crosses putting the shared electrons in the overlap between the atoms

19
Q

Cons of ball and stick diagrams

A

Does not show the true shape of the molecule, bonds aren’t in the right places

20
Q

Intermolecular bonds in covalent bonding

A

Each covalent bond is very strong but the individual molecules are quite spread out. This is because the force of attraction between molecules is weak or the intermolecular bonding is weak

21
Q

How do intermolecular forces in covalent structures change with the size of molecule

A

As the size of molecule increases, so does the intermolecular bond so large structures like polymers actually have quite strong intermolecular forces

22
Q

Giant covalent structures

A

Formed from large networks of atoms held together by covalent bonds

23
Q

Diamond

A
  • carbon atoms
  • 4 covalent bonds on each
  • does not conduct electricity
  • hard
  • high melting and boiling points
24
Q

Graphite

A
  • made of carbon
  • 3 covalent bonds on each
  • layers of delocalised electrons
  • made of layers of hexagonal rings of carbon atoms
  • layers slide over each other
  • conducts electricity
25
Q

What are fullerenes

A

Carbon structures where the atoms join together to form large, hollow cages in all different shapes

26
Q

What are cylindrical fullerenes

A

Fullerenes where their length is much longer than their diameter

27
Q

Properties of cylindrical fullerenes

A

High tensile strength and high electrical and thermal conductivity

28
Q

Uses of fullerenes

A

Deliver drugs in bodies, lubricants, catalysts due to their very high surface are to volume ratio

29
Q

Metallic bonding

A
  • between metals
  • lattice of positively charged ions
  • arranged in regular layers
  • outer electrons form a sea of freely moving electrons holding positive ions in place
  • actually delocalised electrons surrounding positive ions
30
Q

Properties of metallic bonding

A

Pure metals can be bent/ hammered into shape as the layers of ions slide easily over each other

31
Q

Alloys

A

A mixture of two or more element, at least on is a metal (usually both are metal)

32
Q

Properties of metals

A
  • conduct electricity due to delocalised electrons
  • malleable due to layers
  • ductile (can be made into wires)
  • good thermal conductors due to delocalised electrons
33
Q

Nano particles and nano science

A
  • 1nm = 1x10^-9 m
  • nano science deals with structures between 1-100 nm
  • high SA:V ratio makes them highly reactive
34
Q

Nano tube

A
  • like a layer of graphene rolled into a tube
  • very long compared to width
  • withstand high tensions
  • conduct electricity due to delocalised elecrtrons
35
Q

What is graphene and it’s properties

A
  • single sheet of carbon atoms from graphite
  • very good electrical conductor
  • low density
  • most reactive form of carbon
  • strong for its mass
36
Q

Uses for nano particles

A
  • used in windows to trigger break down of dirt
  • used in sunscreen, coat nano particles in silica
  • used in face creams as they are absorbed further into the skin
  • deliver drugs through blood stream
37
Q

Risks of nano particles

A
  • highly reactive
  • could get into the atmosphere
  • breathing them in could damage the lungs
38
Q

Limitations of particle model

A

Assumes particles are solid spheres with no forces operating between them

Chemistry (6 decks)

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