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chemistry questions > C1 Atomic Structure and Periodic Table > Flashcards

C1 Atomic Structure and Periodic Table Flashcards

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AP® Chemistry flashcards Periodic Table flashcards
1
Q

Define atom

A

The smallest part of an element that can still be recognised as that element

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2
Q

Define element

A

A substance made of only one type of atom

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3
Q

Define compound

A

A substance made of two or more different atoms chemically bonded together

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4
Q

Define molecule

A

A substance made of more than one atom chemically bonded together (can be atoms of the same type!)

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5
Q

Define mixture

A

A substance made of more than one thing not chemically bonded together

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6
Q

State the three subatomic particles

A

Protons, neutrons, electrons

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7
Q

State the masses of the subatomic particles

A

Protons: 1, neutrons: 1, electrons: 0

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8
Q

State the relative charges of the subatomic particles

A

Protons: +1, neutrons: 0, electrons: -1

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9
Q

How are the subatomic particles arranged in an atom? (3 marks)

A

Protons and neutrons in the nucleus, electrons orbiting in shells

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10
Q

What is the plum pudding model of the atom?

A

A ball of positive charge with negative electrons studded into it

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11
Q

What did Rutherford’s alpha scattering experiment prove?

A

That atoms have a small dense nucleus with a positive charge

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12
Q

How did Bohr adapt the model of the atom?

A

He said electrons orbit the nucleus at specific distances

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13
Q

What did Chadwick’s work give evidence of?

A

That the nucleus also contained neutrons as well as protons

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14
Q

What is the atomic number of an atom?

A

The number of protons in an atom

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15
Q

What is the mass number of an atom?

A

The number of protons + the number of neutrons in an atom

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16
Q

How do you calculate the number of neutrons in an atom?

A

Mass number - atomic number

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17
Q

How are the electrons arranged in atoms?

A

Orbiting the nucleus in shells

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18
Q

How many electrons can go in the first shell?

A

2

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19
Q

How many electrons can go in the second and third shells?

A

8

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20
Q

How were elemets arranged in the early attempts of the periodic table?

A

By atomic weight

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21
Q

How are elements in the periodic table arranged?

A

By atomic number

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22
Q

What are groups in the periodic table?

A

The columns, numbered 1, 2, 3, 4, 5, 6, 7, 0/8

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23
Q

What do you know about elements in the same group?

A

They have similar properties (reactions) as they have the same number of electrons in the outer shell

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24
Q

What can the group tell you about the electrons in an atom?

A

How many electrons in the outer shell. E.g. carbon is in group 4 so has 4 electrons in the outer shell

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25
Q

What are periods in the periodic table?

A

The rows in the periodic table

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26
Q

What can the period tell you about the electrons in an atom?

A

How many shells an atom has. E.g. carbon is in the second period so has two shells

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27
Q

Why did Mendeleev swap the order of some elements?

A

So they were in the same group as elements they had similar chemical properties with

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28
Q

Why did Mendeleev leave gaps in his periodic table?

A

For elements that had not been discovered yet

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29
Q

What is an ion?

A

an atom which has lost or gained an electron

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30
Q

How many electrons does calcium have?

A

20 (same as atomic number!)

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31
Q

How many electrons does silicon have?

A

14 (same as atomic number!)

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32
Q

How are the electrons in sulphur arranged?

A

2.8.6 (18 electrons total)

33
Q

How are the electrons in magnesium arranged?

A

2.8.2 (12 electrons total)

34
Q

How many electrons are in the outer shell of boron?

A

3 (it is in group 3!)

35
Q

How many electrons are in the outer shell of phosphorous?

A

5 (it is in group 5!)

36
Q

How many electrons are in the outer shell of sodium?

A

1 (it is in group 1!)

37
Q

An element has three shells and three electrons in the outer shell. What element is it?

A

Aluminium (group 3, period 3

38
Q

How many electrons are in the outer shell of Gallium?

A

3 (it is in group 3!)

39
Q

How can solids be separated from liquids?

A

Filtration

40
Q

What is crystallisation?

A

When a solution is heated until crystals start to form then left to cool until all the water evaporates

41
Q

What does distillation do?

A

Separates mixture of liquids with different boiling points

42
Q

What decides what element an atom is?

A

The number of protons. E.g. carbon always has 6 protons

43
Q

Why do atoms have no charge?

A

They have the same number of protons and electrons

44
Q

What is the approximate radius of an atoms

A

0.1nm (1x10-10m)

45
Q

How big is the radius of the nucleus compared to that of the atom?

A

1/10000 the size (so 1x10-14m)

46
Q

What is an isotope?

A

A version of the same element with a different mass. Or an atom with the same number of neutrons but a different number of protons.

47
Q

How do you calculate the relative atomic mass of an isotope?

A

multiply the isotope mass by the abundance for each isotope, add them together and divide the answer by 100

48
Q

What type of ions do metals form?

A

Positive ions as they lose electrons to get a full outer shell

49
Q

What type of ions do non-metals form?

A

Negative ions as they gain electrons to get a full outer shell

50
Q

In terms of electrons, what do group 1 (the alkali metals) elements have in common?

A

1 electron in the outer shell

51
Q

In terms of electrons, what do group 7 elements (the halogens) have in common?

A

7 electrons in the outer shell

52
Q

In terms of electrons, what do group 0 elements (the noble gases) have in common?

A

Full outer shell

53
Q

What is more reactive, lithium or sodium?

A

Sodium

54
Q

What is more reactive, chlorine or bromine?

A

Chlorine

55
Q

Define inert

A

Unreactive

56
Q

Explain why the noble gases are inert

A

They have full outer shells, so do not need to gain or lose electrons

57
Q

What is a trend?

A

A pattern in properties

58
Q

State the trend in the melting points of the alkali metals

A

Gets lower down the group

59
Q

What state is fluorine at room temperature?

A

Gas

60
Q

What state is chlorine at room temperature?

A

Gas

61
Q

What state is bromine at room temperature?

A

liquid

62
Q

What state is iodine at room temperature?

A

solid

63
Q

Balance the equation: Li + H₂O → LiOH + H₂

A

2Li + 2H₂ → 2LiOH + H₂

64
Q

Balance the equation: K + H₂O → KOH + H₂

A

2K + H₂ → KOH + H₂

65
Q

Name LiOH

A

Lithium hydroxide

66
Q

Name KOH

A

Potassium hydroxide

67
Q

Explain why the group 1 elements are called alkali metals

A

They are metals that form alkalis when they react with water

68
Q

What is a displacement reaction?

A

A reaction in which a more reactive element takes the place of a less reactive element in a compound

69
Q

Explain why the following reaction does not proceed: KBr + I₂

A

Iodine is less reactive than bromine so cannot displace it

70
Q

Balance the below equation and explain why it is a displacement reaction: KBr + Cl₂ → KCl + Br₂

A

2KBr + Cl₂ → 2KCl + Br₂ , chlorine has displaced bromine as it is more reactive

71
Q

Explain why fluorine is more reactive than chlorine

A

Fewer shells/electrons, less shielding (or stronger attraction from nucleus), easier to gain electrons

72
Q

Explain why potassium is more reactive than lithium

A

More shells/electrons, less shielding (or weaker attraction from nucleus), easier to lose electrons

73
Q

Explain why bromine is less reactive than chlorine

A

More shells/electrons, more shielding (or weaker attraction from nucleus), harder to gain electrons

74
Q

Explain why sodium is less reactive than caesium

A

Fewer shells/electrons, less shielding (or stronger attraction from nucleus), harder to lose electrons

75
Q

What is the equation for lithium reacting with oxygen?

A

4Li + O2 → 2Li2O

76
Q

What is the equation for sodium reacting with chlorine?

A

2Na + Cl2 → 2NaCl

77
Q

What are common properties of transition metals?

A

Many transition elements have ions with different charges, form coloured compounds and are useful as catalysts.

78
Q

Name some common transition metals

A

Chromium (Cr), Manganese (Mn), Iron (Fe), Cobalt (Co), Nickle (Ni), Copper (Cu)

79
Q

How do transition metal properties differ from group 1 metals?

A

They have higher melting points, densities, strength and hardness and are also less reactive with oxygen, water and halogens

chemistry questions (10 decks)

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