Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

GCSE COMBINED SCIENCE > CHEMISTRY PAPER 1 > Flashcards

CHEMISTRY PAPER 1 Flashcards

You may prefer our related Brainscape-certified flashcards:
GCSE Religious Studies - Edexcel Route A flashcards GCSE Religious Studies - Eduqas Route A flashcards GCSE Geography - AQA flashcards Biology 101 flashcards GCSE Religious Studies - Edexcel Route B flashcards GCSE Religious Studies - Eduqas Route B flashcards
1
Q

What are the sub atomic structure of an atom

A

Proton
Electron
Neutron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is an ion

A

A charged atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is a Isotopes

A

An element that has the same amount of proton and different amount of neutron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is the atomic nucleus made up of

A

Proton and neutron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is the mass number

A

A total of proton plus neutron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What does the atomic number tell you

A

The amount of protons and electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What are on the outershell

A

Electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What are compounds

A

Two or more atoms that are chemically bonded together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

When making bonds what do they to

A

Either gain, loose or share an electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

How is ionic bonding made

A

When a metal gains and non metal loose electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

How is covalent bonding made

A

When two or more non metal share electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is a reactant in a word equation

A

The elements that will react together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is the product in a word equation

A

The products that is produced by the reactant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What are mixtures

A

They are mixtures that are easily separated unlike compounds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Types of method to separate mixtures

A

-filteration
-crystallisation
-simple distillation
-fractional distillation
-chromotography

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is the law of conservation?

A

no atoms can be created or destroyed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What happens is filtration

A

Separates mixtures that contain insoluble solids (can’t dissolve) and liquid (which are soluble)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

How is filtration performed

A
  • pouring mixture into filter paper
  • insouble is trapped by filter paper (solid)
  • soluble runs through paper and collected below
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is crystallisation

A

A separation of mixtures by the solute (dissolved solid) forming into a crystal.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

How would u preform crystallisation

A
  • add in solvent and a solid in a evaporating dish (and let the solid dissolve)
  • heating mixture (with bunsen burner) until some solvent (liquid) evaporates
  • eventually, crystal of the solute ( dissolved solid) will form
  • filter out crystals and leave it in a warm place to dry (could put in oven)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What is chromotography

A

Separates solution with a number of different solute (solids) in the solvent (liquid)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

How would you preform chromatography?

A
  • place a drop of solution near the bottom of the chromatography paper.
  • dip bottom of paper into suitable solvent (liquid)
  • solvent (liquid) moves up the paper and carried solute (solid) in the solution
  • some solutes moves at different speed
  • seperate on paper
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What is Simple distillation

A

A separates 2 liquids with different boiling point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

How is simple distillation preformed

A

-mixture starts to boil until liquid with the lower boiling point starts to boil
- vapour is released through condenser
-then gas cools back to liquid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What is fractional distillation

A

Separating lots of liquid with different amount of boiling point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

How is fractional distillation performed

A
  • slowly heat until the liquid with the lower boiling point starts to boil
  • than increase temperature to collect (boil then condense) the other fraction
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What is an alloy

A

Two or metals which are metallically bonded together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What is an alloy

A

Two or metals which are metallically bonded together

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What does diatomic mean

A

Element that can be alone like oxygen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What is a solvent

A

Liquid in which a solute is dissolved

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

What is a solute

A

The substance that is dissolved in the liquid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

What is a solution

A

The mixture formed when a solute dissolved into the solvent

33
Q

What is a souble

A

Something that can be dissolve

34
Q

What is insouble

A

Cant be dissolved

35
Q

What does chemical bonds create

A

A strong electromagnetic force

36
Q

What are the three main covalent structures

A
  • diamond
  • graphene
  • graphite
37
Q

What is a polmer

A

Large covalently bonded molecule

38
Q

What are the properties of an ionic structure

A

-giant ionic lattice
-strong electrostatic force
-high melting point and high boiling point
-when molten (melted) or dissolve it conducts electricity

39
Q

Why does a structure have a high melting and boiling point

A

Because energy is required to break many strong bonds

40
Q

Why does a melted or dissolved structure conduct electricity

A

Because of the free electron (delocalised)

41
Q

What are the properties of a small molecule

A

-has weak intermolecular force which is quickly broken in boiling and melting point
-intermolecular forces increases with the size of a molecule
-doesnt conduct electricity because they have no charge

42
Q

Why do gases and liquids have a low melting and boiling point

A

Because the attraction between molecules are easy to overcome

43
Q

What state is the gaint covalent bonds

A

Solid

44
Q

What is a diamond

A

4 carbon covalent bonded together

45
Q

What are the properties of a diamond

A

-very hard
-high melting point
-doesn’t not conduct electricity

46
Q

What are graphite

A

3 carbon covalently bonded together

47
Q

What are the properties of a graphite

A

-conducts electricity because of one free electron
-weak intermolecular force
-soft and slippery

48
Q

What is a graphene

A

A single layer of carbon atoms (tightly bonded in a hexagonal honeycomb lattice)

49
Q

The properties of graphene

A
  • extremely strong
  • lightweight
  • flexible
  • conductor of heat and electricity
50
Q

What is a relative formula mass of a compound

A

Sum of relative atomic masses of atoms (proton and neutron)

51
Q

What is a relative formula mass of a compound

A

Sum of relative atomic masses of atoms (proton and neutron)

52
Q

What is the number of atoms, molecule, or ions in a mole of a given substance in the Avogadro constant

A

6.02 x 10 to the power or 23 per mole

53
Q

What is the equation of moles

A

Mass= amount (mol) x relative fomula mass(gmol-1)

54
Q

how can you find the relative atomic mass in an isotope

A

sum of mass
——————————————- (divide)
how many elements there are

55
Q

how would we know that the relative atomic mass from the number of isotopes is correct

A

it will be the same as the relative atomic mass on the atomic table

56
Q

what is the calculation when finding the relative atomic mass by the percentage abundance

A

100

57
Q

what are group 1 elements known as

A

alkaline metals

58
Q

what are the properties of alkaline metals (3.5 points)

A
  • soft/ easy to cut through- gets softer down the table
    -low densities and low melting point (easy to melt when going down the group)
  • very reactive
59
Q

why does reactivity increase when going down group 1

A

number of shells increases by 1 when going down ( making it easier to loose)

60
Q

what happens when atomic number increases

A

-the atomic radius increase (creating distance between the outer shell an the nucleus)
-nucleus attraction decreases

61
Q

what happens when alkaline metals react with water

A

they react vigoursly ( reactive levels gets bigger down the group)

62
Q

when the alkaline reacts with water what does it produce

A

when fizzing the produce gas ( hydroxide and hydrogen)

63
Q

when group 1 metal reactive with water what do they loose

A

1 electron

64
Q

is the the reactant is = sodium+water, what will the product be

A

sodium hydroxide+ hydrogen

65
Q

how do group 1 react with oxygen

A

they react rapidly

66
Q

what do you call group 7

A

halogens

67
Q

what does is mean when halogen has a diatomic molecules

A

paired atoms

68
Q

how to the group 7 non metals present themsleves

A

as a coloured vapour/liquid

69
Q

what are the colour vapour/ liquid for the 4 main halogens

A

Fluorine- yellow poisonous gas
chlorine- green poisonous gas
bromine- red/brown volatile liquid
iodine- dark grey solid or purple vapour

70
Q

in a displacement reaction what will happen when one the halogen elements is more reactive that than the other ( e.g like how fluorine is more reactive then chlorine)

A

the less reactive one will get displaced by the more reactive halogen

71
Q

what is group 0 called

A

noble gasses

72
Q

why is group 0 unreactive

A

they have a full/ stable outershell

73
Q

what is the noble gas’s boiling point (which also makes them?)

A

lower then room temp (colourless and inflammable)

74
Q

when going down the noble gases what happens to the boiling point

A

increases

75
Q

why does the boiling point when going down group 0 increase

A

due to the increase number of electrons in each atom, creating a greater intermolecular force between them

76
Q

what are the physical changes of a halogen going down the group

A
  • colour gets darker
    -melting and boiling point increases
    -density increases
  • high relative atomic masses
77
Q

why is does the reactivity scale go down for halogens

A

as there are an increased of shells, the electrons on the outer shell would be far away from the nucleus creating a weak electrostatic force of attraction (making it harder for it to attract incoming electron to create a full shell)

78
Q

as halogens are a diatomic molecules, how will you write down the symbol for fluorine

A

F(small)2

79
Q
A

GCSE COMBINED SCIENCE (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions