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GCSE Chemistry > Atomic Structure and The Periodic Table > Flashcards

Atomic Structure and The Periodic Table Flashcards

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1
Q

Who discovered neutrons

A

Chadwick

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2
Q

Who discovered electrons

A

Thompson

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3
Q

Who discovered protons

A

A series of experiments

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4
Q

Who discovered electron shells

A

Bohr

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5
Q

Who discovered the nucleus

A

Rutherford

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6
Q

What did Rutherford discover

A

nucleus

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7
Q

Who conducted the gold foil experiment

A

Rutherford

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8
Q

What order was each part of the atom discovered in

A

1) electrons (Thompson plum pudding model)
2) nucleus (Rutherford nuclear model)
3) electron shells (Bohr)
4) proton (series of experiments)
5) neutron (Chadwick)

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9
Q

What model did Rutherford create of the atom

A

Nuclear model (atom mostly empty space with electrons orbiting the positive nucleus)

(Electrons had already been discovered so they had to go somewhere in his model but not embedded as he found the atom was mostly empty space so he decided they would orbit around the edge- Bohr then finds that they orbit at set distances)

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10
Q

What model did Thompson create of the atom

A

Plum pudding
Positively charged atom with negative electrons embedded in it

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11
Q

True or false, in the nuclear model the electrons orbit the nucleus

A

True, but not at set distances as Bohr later discovers

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12
Q

What was concluded from the gold foil experiment and why

A

Atom is mostly empty space (most alpha particles went straight through)
Concentrated mass in centre of atom (some alpha particles deflected)
Concentrated mass is positive (some alpha particles reflected)

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13
Q

What is the radius of an atom in metres

A

1x10 ^-10m

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14
Q

What is the radius of a nucleus in metres

A

1x10^-14m

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15
Q

4 ways to separate mixtures

A

Chromotatography
Distillation (fractional and simple)
Crystallisation
Filtration

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16
Q

Properties of group 0 elements (Noble gases)

A

Unreactive due to full outer shell of electrons so they are stable (don’t need to lose or gain any electrons)
Exist as single atoms (are unreactive so don’t bond to form molecules)
Low melting/ boiling point
Boiling points increase down group

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17
Q

How does the boiling point change going down group 0 (Noble gases)

A

Increases

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18
Q

What is the name for group 1 metals

A

Alkali metals (react with water to form an alkali)

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19
Q

Why are group 1 elements very reactive

A

Have 1 electron in outer shell so it is easy to lose just this 1 outer electron and react

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20
Q

Does reactivity increase or decrease going down group 1 and why

A

Increase
- atom increases in size (larger radius)
- outer electron further away from nucleus
- more shells shielding outer electron from nucleus
- weaker electrostatic forces acting between negative outer electron and positive nucleus

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21
Q

What happens to boiling point going down group 1

A

Decreases

22
Q

What happens to boiling point going down group 7 (halogens)

A

Increases

23
Q

What happens to reactivity going down group 7

A

Decreases

24
Q

Why does reactivity decrease going down group 7 (but increases going down group 1)

A

More electron shells so more shielding between nucleus and outer electrons
Weaker electrostatic forces acting between nucleus and outer electrons so harder for an electron to be attracted to the nucleus and to be gained on the outer shell

(In group 7 the atom is trying to gain an electron so further away the electrostatic forces are weaker so there is less attraction meaning it is harder to gain the electron. But in group 1 if further away the electrostatic forces are weaker this means that the outer electron is less attracted to the nucleus so can be more easily lost)

25
Q

Difference between how reactivity changes going down group 1 and group 7

A

Group 1- increases
Group 7- decreases

26
Q

What do group 1 elements form when they react with water

A

Metal hydroxide + hydrogen

27
Q

What do all halogens exist as

A

Diatomic molecules
(Pairs of atoms chemically bonded together)

28
Q

When 3 or more elements combine with 1 being oxygen what does it end in

A

Ate

29
Q

Physical properties of alkali metals

A

Soft
Relatively low melting points
Low densities

30
Q

Chemical properties of alkali metals

A

Highly reactive
Reactive with water to form metal hydroxides (alkalis)

31
Q

True or false, group 7 elements get darker as you go down the group

A

True

32
Q

How did John Newlands initially arrange known elements

A

Order of increasing atomic weight
‘Law of Octaves’ as elements with similar properties repeated every 8 elements
Problem: some elements were grouped together with completely different properties

33
Q

How is the modern periodic table arranged

A

Increasing atomic number
Columns (groups)- all elements in same group have similar chemical properties (react in a similar way due to all having the same number of electrons in their outer shell)

34
Q

How did Mendeleev develop the first modern periodic table

A

Increasing atomic weight
Left gaps for elements yet to be discovered which he predicted the properties of
He swapped some elements around

35
Q

Physical Properties of transition metals

A

High density
High melting point
Hard
Strong
Good conductors of heat and electricity
Shiny

36
Q

Are alkali metals (group 1) hard or soft

A

Soft

37
Q

How many times smaller is the nucleus of the atom than the radius

A

10,000

38
Q

4 differences between physical properties of elements in group 1 and transition metals

A

Group 1 have lower melting and boiling points, lower densities, are less strong and are softer

39
Q

Further away from the nucleus is there more or less shielding

A

More (means electrostatic forces between outer electron and nucleus are weaker)

40
Q

Is boiling point chemical or physical property

A

Physical

41
Q

Fractional vs simple distillation

A

Fractional distillation separates multiple liquids from a solution based on boiling point (substances with similar boiling point)
Simple distillation separates a single liquid from a solution (substances with completely different boiling points) (the solution is heated, evaporated and condensed)

42
Q

What is a compound

A

2 or more different elements chemically bonded together

43
Q

Does a compound have to be 2 or more different elements

A

Yes

44
Q

What is a molecule

A

2 or more atoms chemically bonded together (can be the same type)

45
Q

What is a mixture

A

Contains 2 or more different substances not chemically joined

46
Q

Why Mendeleev reverse the order of some pairs of elements

A

So their properties matched the rest of the group

47
Q

4 differences between nuclear model and plum pudding model

A

Nuclear model has nucleus, plum pudding model does not
Nuclear model mostly empty space, plum pudding model is solid
Nuclear model positive charge is all in nucleus, plum pudding model atom has overall positive charge
Nuclear model electrons orbit nucleus, plum pudding model electrons are embedded into atom

48
Q

Physical property of noble gases (group 0)

A

Low melting point

49
Q

Why does boiling point increase going down group 0 (noble gases)

A

Atoms become larger
Intermolecular forces between atoms become stronger
More energy needed to overcome these forces

50
Q

Chemical properties of group 0 (noble gases)

A

Un reactive) Full outer shell of electrons)

GCSE Chemistry (18 decks)

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