C1 Atomic Structure and Periodic Table

Question 1

Define atom

Answer 1

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

Question 2

Define element

Answer 2

A substance made of only one type of atom

Question 3

Define compound

Answer 3

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

Question 4

Define molecule

Answer 4

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

Question 5

Define mixture

Answer 5

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

Question 6

State the three subatomic particles

Answer 6

Protons, neutrons, electrons

Question 7

State the masses of the subatomic particles

Answer 7

Protons: 1, neutrons: 1, electrons: 0

Question 8

State the relative charges of the subatomic particles

Answer 8

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

Question 9

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

Answer 9

Protons and neutrons in the nucleus, electrons orbiting in shells

Question 10

What is the plum pudding model of the atom?

Answer 10

A ball of positive charge with negative electrons studded into it

Question 11

What did Rutherford’s alpha scattering experiment prove?

Answer 11

That atoms have a small dense nucleus with a positive charge

Question 12

How did Bohr adapt the model of the atom?

Answer 12

He said electrons orbit the nucleus at specific distances

Question 13

What did Chadwick’s work give evidence of?

Answer 13

That the nucleus also contained neutrons as well as protons

Question 14

What is the atomic number of an atom?

Answer 14

The number of protons in an atom

Question 15

What is the mass number of an atom?

Answer 15

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

Question 16

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

Answer 16

Mass number - atomic number

Question 17

How are the electrons arranged in atoms?

Answer 17

Orbiting the nucleus in shells

Question 18

How many electrons can go in the first shell?

Answer 18

2

Question 19

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

Answer 19

8

Question 20

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

Answer 20

By atomic weight

Question 21

How are elements in the periodic table arranged?

Answer 21

By atomic number

Question 22

What are groups in the periodic table?

Answer 22

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

Question 23

What do you know about elements in the same group?

Answer 23

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

Question 24

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

Answer 24

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

Question 25

What are periods in the periodic table?

Answer 25

The rows in the periodic table

Question 26

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

Answer 26

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

Question 27

Why did Mendeleev swap the order of some elements?

Answer 27

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

Question 28

Why did Mendeleev leave gaps in his periodic table?

Answer 28

For elements that had not been discovered yet

Question 29

What is an ion?

Answer 29

an atom which has lost or gained an electron

Question 30

How many electrons does calcium have?

Answer 30

20 (same as atomic number!)

Question 31

How many electrons does silicon have?

Answer 31

14 (same as atomic number!)

Question 32

How are the electrons in sulphur arranged?

Answer 32

2.8.6 (18 electrons total)

Question 33

How are the electrons in magnesium arranged?

Answer 33

2.8.2 (12 electrons total)

Question 34

How many electrons are in the outer shell of boron?

Answer 34

3 (it is in group 3!)

Question 35

How many electrons are in the outer shell of phosphorous?

Answer 35

5 (it is in group 5!)

Question 36

How many electrons are in the outer shell of sodium?

Answer 36

1 (it is in group 1!)

Question 37

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

Answer 37

Aluminium (group 3, period 3

Question 38

How many electrons are in the outer shell of Gallium?

Answer 38

3 (it is in group 3!)

Question 39

How can solids be separated from liquids?

Answer 39

Filtration

Question 40

What is crystallisation?

Answer 40

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

Question 41

What does distillation do?

Answer 41

Separates mixture of liquids with different boiling points

Question 42

What decides what element an atom is?

Answer 42

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

Question 43

Why do atoms have no charge?

Answer 43

They have the same number of protons and electrons

Question 44

What is the approximate radius of an atoms

Answer 44

0.1nm (1x10-10m)

Question 45

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

Answer 45

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

Question 46

What is an isotope?

Answer 46

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.

Question 47

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

Answer 47

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

Question 48

What type of ions do metals form?

Answer 48

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

Question 49

What type of ions do non-metals form?

Answer 49

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

Question 50

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

Answer 50

1 electron in the outer shell

Question 51

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

Answer 51

7 electrons in the outer shell

Question 52

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

Answer 52

Full outer shell

Question 53

What is more reactive, lithium or sodium?

Answer 53

Sodium

Question 54

What is more reactive, chlorine or bromine?

Answer 54

Chlorine

Question 55

Define inert

Answer 55

Unreactive

Question 56

Explain why the noble gases are inert

Answer 56

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

Question 57

What is a trend?

Answer 57

A pattern in properties

Question 58

State the trend in the melting points of the alkali metals

Answer 58

Gets lower down the group

Question 59

What state is fluorine at room temperature?

Answer 59

Gas

Question 60

What state is chlorine at room temperature?

Answer 60

Gas

Question 61

What state is bromine at room temperature?

Answer 61

liquid

Question 62

What state is iodine at room temperature?

Answer 62

solid

Question 63

Balance the equation: Li + H₂O → LiOH + H₂

Answer 63

2Li + 2H₂ → 2LiOH + H₂

Question 64

Balance the equation: K + H₂O → KOH + H₂

Answer 64

2K + H₂ → KOH + H₂

Question 65

Name LiOH

Answer 65

Lithium hydroxide

Question 66

Name KOH

Answer 66

Potassium hydroxide

Question 67

Explain why the group 1 elements are called alkali metals

Answer 67

They are metals that form alkalis when they react with water

Question 68

What is a displacement reaction?

Answer 68

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

Question 69

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

Answer 69

Iodine is less reactive than bromine so cannot displace it

Question 70

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

Answer 70

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

Question 71

Explain why fluorine is more reactive than chlorine

Answer 71

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

Question 72

Explain why potassium is more reactive than lithium

Answer 72

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

Question 73

Explain why bromine is less reactive than chlorine

Answer 73

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

Question 74

Explain why sodium is less reactive than caesium

Answer 74

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

Question 75

What is the equation for lithium reacting with oxygen?

Answer 75

4Li + O2 → 2Li2O

Question 76

What is the equation for sodium reacting with chlorine?

Answer 76

2Na + Cl2 → 2NaCl

Question 77

What are common properties of transition metals?

Answer 77

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

Question 78

Name some common transition metals

Answer 78

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

Question 79

How do transition metal properties differ from group 1 metals?

Answer 79

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