Chemistry Paper 1- Major Focus Of Exam

Question 1

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

Answer 1

Same number of electrons in their outer shell

Question 2

What did dalton arrange elements in?

Answer 2

Order of atomic weight

Question 3

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

Answer 3

Order of atomic weight

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

Question 4

What law did John new lands propose?

Answer 4

Law of octaves

Question 5

What was a problem with newlands proposed idea?

Answer 5

Elements were grouped together when they had totally different properties

Question 6

Why was Mendeleevs periodic table widely accepted?

Answer 6

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

Question 7

Are noble gases reactive or unreactive?

Answer 7

Unreactive

Question 8

Why are nobles gases unreactive?

Answer 8

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

Question 9

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

Answer 9

Increases

Question 10

What groups of the periodic table contain highly reactive metals?

Answer 10

Group 1 and 2

Question 11

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

Answer 11

Lose

Question 12

What type of ions do

Metals always form?

Answer 12

Positive ions

Question 13

Are group 1 metals hard?

Answer 13

No, they are soft

Question 14

Describe the trend of reactivity down group 1

Answer 14

Increases as you go down

Question 15

Why does reactivity increase as you go down group 1?

Answer 15

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

Question 16

What does the group number correspond to?

Answer 16

Number of electrons in outer shell

Question 17

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

Answer 17

Increase

Question 18

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

Answer 18

Covalent

Question 19

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

Answer 19

Ionic compoinds

Question 20

What’s the trend of reactivity down group 7?

Answer 20

Decreases

Question 21

Why does reactivity decrease as you go down group 7?

Answer 21

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

Question 22

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

Answer 22

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

Question 23

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

Answer 23

Diff concentration of solution

Different current

Question 24

Describe the observations/ what happens when lithium reacts with oxygen

Answer 24

Burn with a crimson flame

Question 25

What happens when lithium reacts with water?

Answer 25

Floats on surface and release hydrogen as bubbles

Question 26

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

Answer 26

Yellow

Question 27

What happens when sodium reacts with water?

Answer 27

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

Question 28

What happens when potassium reacts with water?

Answer 28

Similar to sodium but more vigourous

Question 29

What is formed when alkali metals react with chlorine?

Answer 29

Metal chloride

Question 30

Describe what happens when an alkali metal reacts with chlorine

Answer 30

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

Question 31

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

Answer 31

``` Transition: Higher density Lower reactivity Harder High melting points ```

Question 32

What are 3 specials properties of transition metals?

Answer 32

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

Question 33

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

Answer 33

Used in cooking equipment due to their high melting point

Question 34

Why is graphite a good electrical conductor?

Answer 34

Contains 1 delocalised electron per carbon atom | It’s free to move to carry a charge

Question 35

Why is graphite soft and slippery?

Answer 35

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

Question 36

How can you find the total mass of copper produced?

Answer 36

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

Question 37

State some potential improvements for the titration practical

Answer 37

Add acid dropwise White tile under flask Swirl solution

Question 38

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

Answer 38

1.0 mol/dm3

Question 39

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

Answer 39

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

Question 40

What are 2 properties of small covalent molecules?

Answer 40

Low melting/boiling points | Cannot conduct electricity

Question 41

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

Answer 41

Weak intermolecular forces | Require little energy to break

Question 42

Why don’t small covalent molecules conduct electricity?

Answer 42

Molecules don’t have an overall charge

Question 43

Why are giant covalent molecules always solid at room temperature?

Answer 43

Have strong covalent bonds

Question 44

What element is diamond formed from?

Answer 44

Carbon

Question 45

In diamond what does the carbon atom do?

Answer 45

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

Question 46

Why does diamond have high melting and boiling points?

Answer 46

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

Question 47

Why can’t diamond conduct electricity?

Answer 47

No free electrons to carry a charge

Question 48

What’s some properties of graphite?

Answer 48

High melting point Soft and slippery Conducts heat and electricity

Question 49

In graphite what does each carbon atom form?

Answer 49

3 covalent bonds

Question 50

In graphite, what do the carbon atoms form?

Answer 50

Hexagonal rings

Question 51

Why is graphite slippery?

Answer 51

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

Question 52

Why can graphite conduct electricity?

Answer 52

Contains one delocalised electron | They can move and carry a charge

Question 53

What is graphene?

Answer 53

Single layer of graphite

Question 54

Is it true graphene is one atom thick?

Answer 54

Yes

Question 55

Why is graphene an excellent conductor of electricity?

Answer 55

Has delocalised electrons | They can move and carry and a charge

Question 56

Besides conducting electricity what’s another property of graphene?

Answer 56

Extremely strong

Question 57

What are fullerenes?

Answer 57

Molecules of carbon atoms with hollow shapes

Question 58

What shape is a buckminsterfullerene?

Answer 58

Spherical

Question 59

What are used of fullerenes?

Answer 59

Used as lubricants Drug delivery Catalyst

Question 60

What’s some properties of carbon nanotubes ?

Answer 60

Easily stretched | Conduct electricity and heat

Question 61

What are polymers?

Answer 61

Very large molecules

Question 62

What type of bonds do polymers contain?

Answer 62

Single covalent

Question 63

Why are most polymers solids at room temperature?

Answer 63

Intermolecular forces are strong | Require lots of energy to be broken

Question 64

Describe the bonding in metals

Answer 64

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

Question 65

Why are metallic bonds strong?

Answer 65

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

Question 66

Why can metals be bent and shaped?

Answer 66

Layers of atoms can slide over each ither

Question 67

Why are alloys harder than pure metals?

Answer 67

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

Question 68

What’s an advantage of a dot and cross diagram

Answer 68

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

Question 69

Why are disadvantages of using a dot and cross diagram?

Answer 69

Don’t tell us shape of molecule

Question 70

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

Answer 70

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

Question 71

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

Answer 71

Show shape of molecule

Question 72

Benefit if ball and stick diagram

Answer 72

Can see ions in 3D

Question 73

Disadvantage of ball and stick diagram

Answer 73

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

Question 74

Benefit if spaced filling diagrams

Answer 74

See how closely packed ions are

Question 75

Disadvantage of spaced filling diagram

Answer 75

Difficult to see 3D | Only show tiny part of lattice