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Chemistry Paper 1 Key Info > Chemistry Paper 1 > Flashcards

Chemistry Paper 1 Flashcards

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1
Q

What is an element?

A

A substance made up from only 1 type of atom

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2
Q

What is an atom?

A

the smallest part of an element that can exist

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3
Q

Total mass of products in a reaction =

A

Total mass of reactants

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4
Q

Why does total mass of products = total mass of reactants?

A

No atoms are lost or made

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5
Q

4 main separation techniques?

A

Filtration
Distillation (Simple//fractional)
Chromatography
Crystallisation

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6
Q

Who discovered the electron?

A

JJ Thomson

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7
Q

What did Thomson believe atoms contained? What was this model called?

A

negative electrons surrounded by a sea of positive charge. plum pudding model

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8
Q

What did Geiger and Marden do? What did this show Rutherford?

A

bombarded a thin sheet of gold foil with aloha particles&raquo_space; some bounced back/ were deflected&raquo_space; showed Rutherford that the positive charge in an atom must be concentrated in a very small area.

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9
Q

Who discovered the neutron?

A

James Chadwick

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10
Q

What did Bohr do?

A

Deduced that electrons must orbit the nucleus at a specific distance (otherwise they would spiral inwards)

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11
Q

Atomic radius of atoms?

A

0.1nm // 1x10^-10

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12
Q

what is the atomic number?

A

number of protons

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13
Q

what is the mass number?

A

number of nucleons (protons+neutrons)

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14
Q

How are element arrange in the modern periodic table/

A

In order of increasing mass number

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15
Q

What is an isotope?

A

An element with a different number of neutrons

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16
Q

what is an ion?

A

an atom that has lost or gained an electron

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17
Q

how did John Newlands order the periodic table?

A

KNOWN elements in order of atomic weight&raquo_space; notices patterns, but missing elements caused problems

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18
Q

What did Dimitri Mendeleev realise?

A

That some elements were yet to be discovered

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19
Q

what did Dimitri Mendeleev do?

A

LEFT GAPS for elements that were yet to be discovered

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20
Q

When subatomic particles were discovered, what was it revealed that Mendeleev had done?

A

Ordered them in increasing number of protons (atomic number)

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21
Q

What are group 0 elements called?

A

Noble Gases

22
Q

What are group 1 elements called?

A

Alkali metals

23
Q

What are group 7 elements called?

A

Halogens

24
Q

Noble Gases…

A

Full outer shell
Very stable and unreactive
Boiling points INCREASE as you go down group

25
Q

Alkali Metals…

A

1 electron in outer shell
LOW melting and boiling points&raquo_space; DECREASE as you go down
Become MORE reactive as you go down

26
Q

Why do alkali metals become more reactive as you go down?

A

Outer electron gets further away from influence of nucleus, so it can be lost more easily

27
Q

What are alkali metals stored under? Why?

A

Oil&raquo_space; react vigorously with oxygen and water (even moisture in air)

28
Q

When alkali metals react with water, what is given off and what is formed?

A

Hydrogen gas given off, a metal hydroxide formed

29
Q

Group 1 - low or high density?

A

Low

30
Q

Alkali metals react with non metals to form…

A

Ionic compounds

31
Q

When a metal hydroxide is dissolved in water, what is produced?

A

an alkaline solution

32
Q

Halogens…

A

7 electrons in outer shell
Pairs of atoms
Reactivity decreases down the group
Boiling and melting point INCREASE as you go down

33
Q

Why do halogens become less reactive as you go down?

A

Outer shell get further away from the influence of the nucleus, so it is less easy to gain an electron

34
Q

Halogens react with metals to produce….

A

ionic salts

35
Q

A more reactive halogen will displace a less reactive halogen…

A

From an aqueous solution of its salts

36
Q

What do transition metals form?

A

Coloured compunds

37
Q

Transition metals have ions…

A

With different charges eg - Fe2+ & Fe3+

38
Q

What can transition metals be used as?

A

Ctatalysts

39
Q

Properties of Transition metals

A

Good conductors of heat
Good conductors of electricity
Can easily be bent or hammered into shape

40
Q

What kind of force of attraction between IONIC COMPOUNDS?

A

STRONG ELECTROSTATIC FORCES

41
Q

Ionic bonding includes..

A

A metal and a non-metal

42
Q

Properties of ionic compounds?

A

STRONG ELECTROSTATIC FORCES
HIGH melting and boiling points
DO NOT conduct electricity when solid&raquo_space; ions cannot move
DO conduct electricity when MOLTEN&raquo_space; charges ions are free to move about and carry their charge

43
Q

What is a metallic bond?

A

The attraction between positive ions and delocalised electrons

44
Q

Why are metals good conductors?

A

They have FREE DELOCALISED ELECTRONS which are FREE TO CARRY THEIR CHARGE

45
Q

Uses and properties of aluminium

A

High voltage power cables, furniture, drinks cans, foil food wrap
Corrosion resistant, DUCTILE, MALLEABLE, good conductivity, low density

46
Q

Uses and properties of Copper

A

wires, water pipes, cooking equipment

DUCTILE, MALLEABLE, good conductivity

47
Q

Uses and properties of gold

A

jewellery, electrical junctions

DUCTILE, shiny, good conductivity

48
Q

What does malleable mean

A

can be easily bent or hammered into shape

49
Q

What does ductile mean?

A

can be easily bent or hammered into shape

50
Q

Covalent bond occurs between…

A

2 non metals

51
Q

What is a covalent bond

A

a shared pair of electrons between atoms

52
Q

A property of covalent bonds

A

very strong

Chemistry Paper 1 Key Info (1 decks)

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