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Chemistry > PAPER 1 GCSE > Flashcards

PAPER 1 GCSE Flashcards

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1
Q

What is an ELEMENT?

A

A substance containing only one type of atom
eg. Mg, O2

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2
Q

What is a COMPOUND?

A

A substance containing two or more different types of atoms which are CHEMICALLY BONDED
eg. H20

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3
Q

Why must equations be balanced?

A

Atoms cannot be created or destroyed due to CONSERVATION OF MASS

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4
Q

What is a PRO TIP when balancing equations?

A

Start with atoms in a compound; end with elements.

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5
Q

What is a MIXTURE?

A

A mixture consists of different substances NOT CHEMICALLY BONDED
eg. air, solutions.

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6
Q

What does FILTRATION do?

A

Removes large, insoluble particles from a liquid
eg. sand from water

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7
Q

What does CRYSTALLISATION do?

A

Leaves behind crystals of a dissolved substance (solute)

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8
Q

What does SIMPLE DISTILLATION do?

A

Involves condensing the evaporated solvent and collecting it

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9
Q

What does FRACTIONAL DISTILLATION do?

A

Can separate liquids due to their different boiling points

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10
Q

What does CHROMATOGRAPHY do?

A

Separates mixtures of soluble substances in a solution

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11
Q

What are the 3 main states of matter?

A

Solid
Liquid
Gas

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12
Q

What is MELTING?

A

Solid -> Liquid

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13
Q

What is SOLIDIFICATION/ FREEZING?

A

Liquid -> Solid

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14
Q

What is EVAPORATION/ BOILING?

A

Liquid -> Gas

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15
Q

What is CONDENSATION?

A

Gas -> Liquid

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16
Q

What is SUBLIMATION?

A

Solid -> Gas

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17
Q

Particles in a SOLID:

A
  • Regular arrangement (lattice) and vibrate about fixed positions.
  • Cannot be compressed
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18
Q

Particles in a LIQUID:

A
  • Irregular arrangement and are able to move past each other
  • Cannot be compressed
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19
Q

Particles in a GAS:

A
  • Far apart, move randomly at fast speeds (high energy)
  • Can be compressed
20
Q

Are new substances made after a physical change?

A

No

21
Q

What is needed to overcome the electrostatic forces of attraction between particles to melt/ evaporate?

A

Energy (heat)

22
Q

What are the state symbols?

A

(s) = SOLID
(l) = LIQUID
(g) = GAS
(aq) = AQUEOUS (dissolved or in a solution)

23
Q

Atomic Structure HISTORY (briefly):

A

ANCIENT GREEKS: thought matter to be made of invisible particles

JJ THOMPSON: Created the ‘plum pudding’ model

ERNEST RUTHERFORD: Discovered that the nucleus was small and positively charged by finding that most alpha particles went straight through a gold ‘leaf’; very few deflected back.. Atoms mostly empty space

NEILS BOHR: Deduced that electrons exist in ‘shells’. JAMES CHADWICK determined that the nucleus must contain NEUTRONS as well as protons.

24
Q

What are the RELATIVE CHARGES of the three subatomic particles?

A

Proton = +1
Neutron = 0
Electron = -1

25
Q

What are the RELATIVE MASSES of the three subatomic particles?

A

Proton = 1
Neutron = 1
Electron = 0.0005

26
Q

What is the ATOMIC NUMBER?

A

The number of protons/ electrons in a nucleus

27
Q

What is an ISOTOPE?

A

Atoms with the same number of protons but a different number of neutrons.

28
Q

What happens if an atom has a different number of protons and electrons?

A

It is an ION.

29
Q

What is the MASS NUMBER also known as?

A

RELATIVE ATOMIC MASS/RAM/Ar

30
Q

What is the MASS NUMBER?

A

The number of PROTONS and NEUTRONS in a nucleus.

31
Q

Why might some MASS NUMBERS on your periodic table be decimals?

A

They are the AVERAGE mass of all isotopes

32
Q

How do you work out the AVERAGE MASS?

A

Average mass = total mass of 100 atoms/ 100

33
Q

The RELATIVE ABUNDANCE of
Chlorine-35 is 75%
Chlorine-37 is 25%

How would this look in the formula for average mass?

A

(35x75)+(37x25)/ 100 = 35.5

34
Q

How were the elements initially ordered in the periodic table?

A

According to their atomic ‘weight’

35
Q

How did Dmitri Mendeleev organise the periodic table?

A

He grouped elements together based on their properties.

36
Q

Why did Dmitri Mendeleev believe there were gaps in his table?

A

Elements had yet to be discovered.
In time, this was proven to be largely correct, and is the basis of the modern periodic table.

37
Q

Electron configuration?

A

2,8,8,2

38
Q

Which ions do metals form?

A

Positive

39
Q

Which ions do non-metals form?

A

Negative

40
Q

What is Group 1 called?

A

The Alkali Metals

41
Q

What is Group 7 called?

A

The Halogens

42
Q

What is Group 0/8 called?

A

The Noble Gases

43
Q

How does the reactivity of Group 1 change throughout the group?
Why?

A

Group 1 gets more reactive as you go down the group.
This is because the outer electron is further from the nucleus so the attraction between the outer electrons and the nucleus decreases.

44
Q

How does the reactivity of Group 7 change throughout the group?
Why?

A

They get less reactive as you go down the group.
This is because the number of electron shells increases, so the attraction between the nucleus and outer electrons decrease which makes it harder to gain an electron.

45
Q

How does the reactivity of Group 0/8 change throughout the group?
Why?

A

The are unreactive as they already have an empty outer shell.

46
Q
A

Chemistry (13 decks)

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