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Chemistry GCSE > Chemistry GCSE: C1 Atomic Structure and the Periodic Table > Flashcards

Chemistry GCSE: C1 Atomic Structure and the Periodic Table Flashcards

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1
Q

What is a mixture?

Give examples of mixtures.

A

Two or more elements or compounds that are not chemically bonded.

Examples of mixtures:

Tap water (water and a variety of ions)

Sea water (water and a variety of ions including sodium and chloride ions)

Milk (water and a variety of fats, proteins and sugars)

Steel (iron, carbon and other metals)

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2
Q

What is a compound?

Give examples of compounds.

A

Two or more elements that are chemically bonded.

Examples of compounds:

Covalent compounds: Carbon dioxide, water, carbon monoxide, methane, sulfur dioxide, nitrogen dioxide etc.

Ionic compunds: Sodium chloride, sodium hydroxide, iron oxide, calcium carbonate etc.

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3
Q

What is the easiest way to identify whether something is an element?

A

Look in the periodic table.

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4
Q

What is a molecule?

A

Two or more atoms chemically bonded together.

These can be atoms of the same element (e.g O2) or atoms of different elements (CO2).

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5
Q

What three types of subatomic particle are atoms made from?

A

Protons

Neutrons

Electrons

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6
Q

What is the charge of a proton?

A

Positive

+1

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7
Q

What is the charge of an electron?

A

Negative

-1

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8
Q

What is the charge of a neutron?

A

Neutral

No Charge

0

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9
Q

What is the overall charge of an atom? Explain why atoms have this charge.

A

Neutral (no charge, 0)

Because all atoms have equal numbers of positively charged protons and negatively charged electrons, so they cancel each other out.

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10
Q

What is the mass of a proton?

A

1

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11
Q

What is the mass of an electron?

A

0 (no mass)

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12
Q

What is the mass of a neutron?

A

1 (the same as a proton)

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13
Q

Where are protons found in an atom?

A

In the nucleus

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14
Q

Where are neutrons found in an atom?

A

In the nucleus

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15
Q

Where are electrons found in an atom?

A

On the outer shells

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16
Q

How can you work out the number of protons in the atom of a named element (e.g carbon)?

A

Use the atomic/proton number in the periodic table.

This is the small number.

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17
Q

How can you work out the number of electrons in the atom of a named element (e.g carbon)?

A

Use the atomic/proton number in the periodic table.

This is the small number.

The number of electrons is always the same as the number of protons.

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18
Q

How can you work out the number of neutrons in an atom of a named element (e.g carbon)?

A

Mass number - atomic/proton number

The mass number is protons plus neutrons, so if you take the number of protons away from the mass number you are left with the number of neutrons.

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19
Q

Which of the following decides what element an atom is:

  1. The number of electrons
  2. The number of protons
  3. The number of neutrons
  4. The atomic mass
A

The number of protons.

For example, if an atom has 6 protons, it must be carbon.

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20
Q

What did scientists think atoms were like before electrons were discovered?

A

They thought that they were tiny spheres (balls) that could not be divided (broken into smaller pieces).

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21
Q

Who discovered electrons and what was his model of the atom called?

A

Thomson.

The Plum Pudding Model

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22
Q

What did Thompson (Plum Pudding Model) suggest the atom was like?

A

A ball of positive charge with negative electrons scattered in it.

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23
Q

Rutherford realised that the plum pudding model was wrong.

What was Rutherfords model of the atom like?

What did he call his model of the atom?

A

Rutherford thought the atom was made of a tiny positvely charged nucleus, surrounded by scattered eletrons.

He called it: The nuclear model

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24
Q
  1. What did Rutherford do to test the structure of the atom?
  2. What were his results and what did they show?

3. Extension: What had Rutherford expected to happen (if the Plum Pudding model was correct)?

A
  1. Rutherford fired positively charged alpha particles at a thin sheet of gold.
    2a. Most of the alpha particles went straight through the gold sheet: This showed that the atom was mainly empty space.
    2b. Some of the alpha particles were deflected, and a small number were deflected backwards: This suggested that the positive charge in the atom was focussed in a tiny area at the centre of the atom (the nucleus).
  2. Extension: Rutherford thought that all the alpha particles would pass straight through.
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25
Q

How did Bohr improve Rutherford’s nuclear model of the atom?

A

Bohr realised that electrons orbit the nucleus on shells.

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26
Q

After Bohr had realised that the electrons were on shells, Rutherford and Chadwick made further discoveries about the structure of the nucleus. What did they discover?

A

Protons were discovered: Rutherford realised that the nucleus could be divided into smaller positive particles.

Neutrons were discovered (20 years later): Chadwick showed that there were neutral particles in the nucleus.

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27
Q

How big is the nucleus of an atom compared to the whole atom?

A

The nucleus of the atom is 1/10,000 of the size of an atom.

28
Q

Where is most of the mass of the atom found?

A

In the nucleus.

Because this is where protons and neutrons are found.

29
Q

What do we call atoms of the same element (same number of protons) with different numbers of neutrons.

For example, carbon atoms with 6 neutrons and carbon atoms wiith 8 neutrons.

A

Isotopes

30
Q

If isotopes have different numbers of neutrons how else must they also be dfferent?

A

They must have different atomic masses.

31
Q

How are elements organised in the modern periodic table?

A

In order of their proton number.

32
Q
  1. How were elements organised in the early versions of the periodic table?
  2. What was the main problem with early versions of the periodic table?
A
  1. In order of relative atomic mass (electrons, protons and neutrons had not been discovered).
  2. Some elements were placed in groups with elements that had very different properties.
33
Q
  1. How did Mendeleev organise the elements in his periodic table?
  2. What unusual step did Mendeleev take to make this possible?
A
  1. Mainly order of relative atomic mass but he changed the order slightly to put elements with similar properties in the same group.
  2. He left gaps in his periodic table.
34
Q

How did the gaps in Mendeleevs periodic table hep to prove his ideas?

A

Elements were discovered that fitted the gaps and had similar properties to the other elements in the same group

For example, gallium fitted in a gap in group 3 and it had similar properties to aluminium.

35
Q

What do elements in the same group of the periodic table have in common?

A

The same number of electrons in their outer shell (e.g group 1 elements have 1 electron in their outer shell)

Similar properties (e.g all group 1 elements react with water producing hydrogen and metal hydroxides).

36
Q

Where are metals found in the peridic table?

A

On the left, in the middle and on the bottom right.

37
Q

Where are non-metals found in the periodic table?

A

On the right and towards the top.

38
Q

What properties do most metals have in common?

A
  1. They are strong
  2. They can be bent or hammered into shape (Malleable)
  3. They are good at conducting heat and electricity.
  4. They have high melting and boiling points.
39
Q

What properties do most NON-metals have in common?

A
  1. They are brittle
  2. Dull looking
  3. Often liquids or gases at room temperature.
  4. Poor conductors
40
Q

TRIPLE:

What do we call the metals in the middle of the periodic table?

A

The transition metals

41
Q

Is hydrogen a metal or non-metal?

A

Non-metal

42
Q

What do we call atoms that have lost or gained electrons and so have a positive or negative charge?

A

Ions

43
Q

How many electron can fit in the first (the one closest to the nucleus) electron shell of an atom?

A

2

44
Q

How many electrons can fit in the 2nd and 3rd electron shells of an atom?

A

8 in each shell

45
Q

If two elements are in the same group in the periodic table, what does this tell you about them?

A

That they have the same number of electrons in their outer shell (e.g all group 1 element have 1 electron in their outer shell).

That they have similar properties.

46
Q

What are group 1 elements called?

A

The alkali metals

47
Q

What are the properties of group 1 elements?

A
  1. Soft
  2. Low density
  3. React with non-metals (e.g chlorine and oxygen) to form ionic compunds.
  4. React with water.
48
Q

What charge do group 1 ions have (e.g sodium ions)?

A

+ 1

49
Q

What happens when group 1 elements react with water?

A
  1. They float and move around on the surface fizzing.
  2. Hydrogen (which may burst into flame) is made.
  3. Metal hydroxides (e.g sodium hydroxide) are made. These dissolve in the water making alkaline solutions.
  4. sodium + water → sodium hydroxide + hydrogen

HIGHER

2Na (s) + 2H2O (l) →2NaOH (aq) + H2 (g)

50
Q

Lithium + oxygen →

Sodium + oxygen →

HIGHER:

Li + O2 → (complete the equation, then balance it and add state symbols)

A

Lithium + oxygen →lithium oxide

Sodium + oxygen →sodium oxide (+ sodium peroxide)

HIGHER

4Li (s) + O2 (g) → 2Li2O (s)

51
Q

Sodium + chlorine →

Potassium + chlorine →

Higher:

Na + Cl2 → (complete the equation, then balance it and add state symbols)

A

Sodium + chlorine →sodium chloride

Potassium + chlorine →potassium chloride

Higher:

2Na (s) + Cl2 (g) → 2NaCl (s)

52
Q

How does the reactivity of the group 1 element (alkali metals) change as you go down the group?

A

The group 1 elements get more reactive as you go down the group.

53
Q

HIGHER:

Explain why the group 1 elements (alkali metals) get more reactive as you go down the group.

A
  1. The outer electron is further from the nucleus
  2. There is a weaker (electrostatic) attraction between the nucleus and outer electron.
  3. It is easier to lose the outer electron.
54
Q

TRIPLE:

Compare the properties of group 1 metals and transition metals

A

Group 1 are more reactive.

Transition metals are more dense, strong and hard.

Transition metals have much higher melting points.

55
Q

Fluorine and chlorine are both in group 7 of the periodic table, how many electrons do they have in their outer shell?

A

7

56
Q

What are group 7 elements called?

A

The halogens

57
Q

Group 7 elements form diatomic molecules? What are diatomic molecules?

A

Molecules made from two atoms bonded together.

58
Q

What is the colour and state at room temperature of fluorine, chlorine, bromine and iodine?

A
  • Fluorine: Yellow gas
  • Chlorine: Green gas
  • Bromine: Red-brown liquid (and gas)
  • Iodine: Grey solid and purple gas
59
Q

How does the reactivity of group 7 elements (halogens) change as you go down the group?

A

They get less reactive as you go down the group.

60
Q

Complete the equation below and exaplin why this happens:

Chlorine + sodium bromide →

HIGHER:

What is oxidised (loses electrons) and what is reduced (gains electrons) in this reaction.

A

Chlorine + sodium bromide →sodium chloride and bromine

Chlorine displaces bromine, because it is more reactive than bromine.

HIGHER:

Chlorine atoms are reduced (gain electrons) forming chloride ions.

Bromide ions are oxidised (lose electrons) forming bromine molecules.

61
Q

Explain why the group 7 elements (halogens) get less reactive as you go down the group.

A

Because the outer shell is further from the nucleus.

The (electrostatic) attraction between the nucleus and outer shell/electrons is waeker.

Its more difficult to attract electrons to the outer shell.

62
Q

What are group 0 elements called?

A

The noble gases

63
Q

How many electrons do the group 0 elements (noble gases) have in their outer shell.

A

8, except helium which has 2 electrons in its outer shell.

64
Q

Why are group 0 elements unreactive (inert)?

A

Because they have full outer shells of electrons.

Because they have a stable arrangement of electrons so they don’t need to gain/lose or borrow electrons from other atoms.

65
Q

What is the state and colour of group 0 eleemnts at room temperature.

A

They are all colourless gases.

66
Q

HIGHER:

Why does the boiling point of group 1 elements increase as you go down the group?

A

The atoms have more electrons.

There are stronger forces of (electrostatic) attraction between the atoms.

It takes more energy to break these forces.

67
Q

HIGHER:

Which elements form diatomic molecules (molecules made from tow atoms joined together)?

A

Oxygen (O2)

Hydrogen (H2)

Nitrogen (N2)

Group 7 elements (Fluorine F2, Chlorine Cl2, Bromine Br2, Iodine I2)

Chemistry GCSE (10 decks)

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