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GCSE Science > Chemistry Paper 1- Major Focus Of Exam > Flashcards

Chemistry Paper 1- Major Focus Of Exam Flashcards

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1
Q

Why do elements in the same group react similarly?/ have similar properties?

A

Same number of electrons in their outer shell

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2
Q

What did dalton arrange elements in?

A

Order of atomic weight

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3
Q

What did John newlandd arrange elements in and what else did he notice?

A

Order of atomic weight

Noticed elements reacted in a similar way and that properties of every eighth element seemed similiar

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4
Q

What law did John new lands propose?

A

Law of octaves

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5
Q

What was a problem with newlands proposed idea?

A

Elements were grouped together when they had totally different properties

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6
Q

Why was Mendeleevs periodic table widely accepted?

A

Switched order of elements so they fitted the patterns of other elements in the same group
Left gals for undiscovered elements and predicted their properties

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7
Q

Are noble gases reactive or unreactive?

A

Unreactive

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8
Q

Why are nobles gases unreactive?

A

They have a full outer shell, so dknt need to react, so are stable

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9
Q

As the atomic masses of noble gases increases, what happens to their boiling point?

A

Increases

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10
Q

What groups of the periodic table contain highly reactive metals?

A

Group 1 and 2

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11
Q

When metals react, do they gain or lose electron to gain a full
Outer shell?

A

Lose

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12
Q

What type of ions do

Metals always form?

A

Positive ions

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13
Q

Are group 1 metals hard?

A

No, they are soft

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14
Q

Describe the trend of reactivity down group 1

A

Increases as you go down

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15
Q

Why does reactivity increase as you go down group 1?

A

Atoms get larger
Outer electron is further from nucleus
Attraction is weaker
Electron is more easily lost

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16
Q

What does the group number correspond to?

A

Number of electrons in outer shell

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17
Q

Do the melting and boiling points increase or decreases as we move down group 7?

A

Increase

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18
Q

What compounds do group 7 elements from when they react with non metals?

A

Covalent

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19
Q

When group 7 elements react with metal atoms, what type of compound do they form?

A

Ionic compoinds

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20
Q

What’s the trend of reactivity down group 7?

A

Decreases

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21
Q

Why does reactivity decrease as you go down group 7?

A

Atoms get larger
Outer shell get further from nucleus
Ability for nucleus to attract extra electron gets weaker
An extra electron is less easily attracted

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22
Q

When sodium is out in a gas jar of chlorine, what happens before/during/ after reaction

A

Before- yellow flame
During- white smoke
After- white solid

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23
Q

What are 2 reasons why in electrolysis, the mass of copper deposited was lower than the expected value?

A

Diff concentration of solution

Different current

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24
Q

Describe the observations/ what happens when lithium reacts with oxygen

A

Burn with a crimson flame

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25
Q

What happens when lithium reacts with water?

A

Floats on surface and release hydrogen as bubbles

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26
Q

What type of flame does sodium burn with when it reacts with oxygen?

A

Yellow

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27
Q

What happens when sodium reacts with water?

A

Floats on surface, releasing heat to melt the sodium, so it moves quickly across the surface

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28
Q

What happens when potassium reacts with water?

A

Similar to sodium but more vigourous

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29
Q

What is formed when alkali metals react with chlorine?

A

Metal chloride

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30
Q

Describe what happens when an alkali metal reacts with chlorine

A

Metal chloride is formed and dissolved in water to give a colourless solution

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31
Q

What are some differences with transition metals compared to alkali metals?

A 
Transition:
Higher density
Lower reactivity
Harder
High melting points
32
Q

What are 3 specials properties of transition metals?

A

Form ions with different charges
Form different colour compounds
Used as catalysts

33
Q

Give one use of transition metals(beside as catalysts) and explain why they are used

A

Used in cooking equipment due to their high melting point

34
Q

Why is graphite a good electrical conductor?

A

Contains 1 delocalised electron per carbon atom

It’s free to move to carry a charge

35
Q

Why is graphite soft and slippery?

A

No bonds between layers
Made of weak intermolecular forces
Layers Can slide over each other

36
Q

How can you find the total mass of copper produced?

A

Filter mixture
Wash and dry copper
Weigh copper collected
Add to increase in mass of electrode

37
Q

State some potential improvements for the titration practical

A

Add acid dropwise
White tile under flask
Swirl solution

38
Q

Which one of 0.1mil/dm3 or 1.0 mol/dm3 solution has a lower ph

A

1.0 mol/dm3

39
Q

What’s the difference between the processes in electrolysis and in a chemical cell?

A

Electrolysis uses electricity to produce a chemical reaction whereas a chemical cell uses a chemical reaction to produce electricity

40
Q

What are 2 properties of small covalent molecules?

A

Low melting/boiling points

Cannot conduct electricity

41
Q

Why do small covalent molecules have low melting and boiling points?

A

Weak intermolecular forces

Require little energy to break

42
Q

Why don’t small covalent molecules conduct electricity?

A

Molecules don’t have an overall charge

43
Q

Why are giant covalent molecules always solid at room temperature?

A

Have strong covalent bonds

44
Q

What element is diamond formed from?

A

Carbon

45
Q

In diamond what does the carbon atom do?

A

Each carbon atom forms 4 covalent bonds to 4 other carbon atoms

46
Q

Why does diamond have high melting and boiling points?

A

Main if of millions of carbon atoms bonded by strong covalent bonds
Requires lots of energy to be broken

47
Q

Why can’t diamond conduct electricity?

A

No free electrons to carry a charge

48
Q

What’s some properties of graphite?

A

High melting point
Soft and slippery
Conducts heat and electricity

49
Q

In graphite what does each carbon atom form?

A

3 covalent bonds

50
Q

In graphite, what do the carbon atoms form?

A

Hexagonal rings

51
Q

Why is graphite slippery?

A

Hexagonal rings are in layers
No covalent bonds between layers
Layers can slide

52
Q

Why can graphite conduct electricity?

A

Contains one delocalised electron

They can move and carry a charge

53
Q

What is graphene?

A

Single layer of graphite

54
Q

Is it true graphene is one atom thick?

A

Yes

55
Q

Why is graphene an excellent conductor of electricity?

A

Has delocalised electrons

They can move and carry and a charge

56
Q

Besides conducting electricity what’s another property of graphene?

A

Extremely strong

57
Q

What are fullerenes?

A

Molecules of carbon atoms with hollow shapes

58
Q

What shape is a buckminsterfullerene?

A

Spherical

59
Q

What are used of fullerenes?

A

Used as lubricants
Drug delivery
Catalyst

60
Q

What’s some properties of carbon nanotubes ?

A

Easily stretched

Conduct electricity and heat

61
Q

What are polymers?

A

Very large molecules

62
Q

What type of bonds do polymers contain?

A

Single covalent

63
Q

Why are most polymers solids at room temperature?

A

Intermolecular forces are strong

Require lots of energy to be broken

64
Q

Describe the bonding in metals

A

Consist of giant structure of atoms arranged in regular layers
Electrons in outer energy level is delocalised
Strong electrostatic attraction between sea of delocalised electrons and positive metal ions

65
Q

Why are metallic bonds strong?

A

Strong electrostatic attraction between sea of delocalised electrons and positive metal ions

66
Q

Why can metals be bent and shaped?

A

Layers of atoms can slide over each ither

67
Q

Why are alloys harder than pure metals?

A

Different sizes of atoms distorts layers, making it more difficult for them to slide

68
Q

What’s an advantage of a dot and cross diagram

A

Clear where electrons are coming from because we use dots and crosses

69
Q

Why are disadvantages of using a dot and cross diagram?

A

Don’t tell us shape of molecule

70
Q

What’s some disadvantages of a 2D stick model?

A

Can’t tell which electron in bind came from which atom
Give no idea of outer electrons that aren’t in bonds
Don’t give accurate information if shape of molecule

71
Q

What’s a benefit if a 3D stick diagram?

A

Show shape of molecule

72
Q

Benefit if ball and stick diagram

A

Can see ions in 3D

73
Q

Disadvantage of ball and stick diagram

A

Show ions are spaced apart but in reality they are packed together

74
Q

Benefit if spaced filling diagrams

A

See how closely packed ions are

75
Q

Disadvantage of spaced filling diagram

A

Difficult to see 3D

Only show tiny part of lattice

GCSE Science (8 decks)

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