C2. The Periodic Table

Question 1

Define the term period in the context of the Periodic Table

Answer 1

A period is a horizontal row in the Periodic Table that shows the number of electrons

Question 2

What does the group number indicate in the Periodic Table?

Answer 2

Indicates the number of electrons in the outer shell of an element

Question 3

What is the relationship between group number and the number of electrons in the outer most shell of an atom

Answer 3

The group number is the same as the number of electrons in the outer most shell of an atom

Question 4

Define the term group in the context of the Periodic Table

Answer 4

Groups are the vertical columns that show how many outer electrons each atoms has

Question 5

What did the gaps in Mendeleev’s table represent?

Answer 5

The gaps in Mendeleev’s table represented undiscovered elements

Question 6

What is the modern basis for arranging elements in the periodic table?

Answer 6

Elements in the modern periodic table are arranged by increasing atomic number

Question 7

Before the discovery of protons, neutrons and electrons how was the early Periodic Table ordered?

Answer 7

Before the discovery of protons, neutrons and electrons the early Periodic Table was ordered by atomic weight

Question 8

What confirmed Mendeleev’s theories about his Periodic Table?

Answer 8

Mendeleev’s theories about his Periodic Table were confirmed when these elements were later discovered and found to fit in his pattern

Question 9

What change to the Periodic Table arrangement took place when subatomic particles were discovered?

Answer 9

The arrangement changed by ordering by atomic number rather than atomic mass

Question 10

In terms of their physical state at room temperature what is the difference between metals and non-metals?

Answer 10

At room temperature, metals are typically solid and non-metals cam be gases or solids

Mercury and bromine are exceptions as they are liquid at room temperature

Question 11

What properties are used to classify elements as metals or non-metals?

Answer 11

Conductivity
Melting/boiling point
Reaction with acid
Type of oxide formed

Question 12

Where are non-metals generally located on the Periodic Table?

Answer 12

On the right-hand side of the Periodic Table

Question 13

What type of oxide do metals normally form?

Answer 13

Metals normally form basic oxides

Question 14

Do metals or non-metals generally have low melting and boiling points?

Answer 14

Non-metals generally have low melting and boiling points

Question 15

State the characteristic properties of metals and non-metals?

Answer 15

Metals typically have high electrical conductivity, are malleable/ductile, reacts with acids and form basic oxides

Non-metals typically have lower electrical conductivity, are brittle, do not react with acids and form acidic oxides

Question 16

What is Group 0 of the Periodic Table called?

Answer 16

Noble gases

Question 17

Why are noble gases unreactive?

Answer 17

Noble gases are unreactive as they have full outer shells of electrons

Question 18

What is Group 1 of the Periodic Table called?

Answer 18

Alkali metals

Question 19

Name the two products formed when sodium reacts with water.

Answer 19

Sodium hydroxide and hydrogen

Question 20

Give two properties of Group 1 metals

Answer 20

They are soft
They have relatively low densities
They have relatively low melting points
They are very reactive

Question 21

Explain why the alkali metals share similar chemical properties

Answer 21

The alkali metals share similar chemical properties because they all have one electron/ the same number of electrons in their outer shell.

Question 22

Describe the trend in reactivity going down Group 1

Answer 22

Reactivity increases

Question 23

Apart from fizzing/effervescence, state two other observations that would be made when sodium is added to water

Answer 23

Floating
Moving
Melting/turning into a ball/sphere
Getting smaller/disappearing/dissolving
Leaving a white trail

Question 24

Give the charge of the ions formed when a Group 1 metals loses an electron

Answer 24

1+

Question 25

Name Group 7 of the Periodic Table

Answer 25

The Halogens

Question 26

Give the colour and state of chlorine at room temperature

Answer 26

Pale green gas

Question 27

Describe what happens to the melting points of the halogens going down the group

Answer 27

The melting point of the halogen increases

Question 28

What is meant by a halogen displacement reaction?

Answer 28

Where a more reactive halogen displaces a less reactive halogen form an aqueous solution of its halide

Question 29

Explain why chlorine has a higher melting point than fluorine

Answer 29

Chlorine has a higher melting point than fluorine because there are stronger intermolecular forces which need more energy to overcome

Question 30

Give the charge of the ion formed when a halogen reacts with Group 1 metal.

Answer 30

-1

Question 31

Why is fluorine the most reactive halogen?

Answer 31

It has the fewest shells so it easier for the nucleus to attract an electron

Question 32

Explain why reactivity decreases going down Group 7

Answer 32

Reactivity decreases going down Group 7 because the atoms have more shells. This means that there is a less attraction between an incoming electron and the positive nucleus, which makes it harder to gain an electron

Question 33

Where are the transition elements located in the Periodic Table

Answer 33

between Group 2 and Group 3

Question 34

What are the typical properties of transition elements

Answer 34

High densities
High melting points
Form coloured compounds
Act as catalysts

Question 35

Compare the hardness of transition metals to Group 1 metals

Answer 35

Transition metals are much harder than Group 1 metals which are very soft and light

Question 36

How do the melting points of transition metals compare to those of Group 1 metals?

Answer 36

Transition metals have much higher melting points than Group 1 metals

Question 37

How do Group 1 metals and transition metals differ in their reaction with oxygen?

Answer 37

Group 1 metals tarnish quickly in the presence of oxygen forming a metal oxide

Transition metals react much more slowly

Question 38

What are two key characteristics that define a transition element?

Answer 38

They form coloured compounds
They have multiple oxidation states

Question 39

Compare the reactivity of Group 1 metals and transition metals with water, oxygen and halogems

Answer 39

Group 1 metals react readily with water, oxygen, and halogens, while transition metals either react very slowly or do not react at all with these substances