The Periodic Table

Question 1

What group is the alkali metals?

Answer 1

Group 1

Question 2

What side of the periodic table are the non-metals on?

Answer 2

Left

Question 3

What side of the periodic table are the metals on?

Answer 3

Right

Question 4

What are the elements between Group 2 and 3?

Answer 4

Transition metals

Question 5

What group is the halogens?

Answer 5

Group 7

Question 6

What group is the noble gases?

Answer 6

Group 0

Question 7

In the first list of elements, how were the elements ordered?

Answer 7

By atomic mass

Question 8

In the first list of elements, were there gaps?

Answer 8

No

Question 9

In the first list of elements, how were elements grouped?

Answer 9

They weren’t

Question 10

In the first list of elements, was there a distinction between metals and non-metals?

Answer 10

No clear distinction

Question 11

In the first list of elements, what was one of the problems?

Answer 11

Some elements organised inappropriately

Question 12

In Mendeleev’s Periodic Table, how were elements grouped?

Answer 12

Normally by atomic mass, but some swapped around

Question 13

In Mendeleev’s Periodic Table, were there gaps?

Answer 13

Yes, for undiscovered elements

Question 14

In Mendeleev’s Periodic Table, how were elements grouped?

Answer 14

By chemical properties

Question 15

In Mendeleev’s Periodic Table, how were metals and non-metals organised?

Answer 15

No clear distinction

Question 16

In Mendeleev’s Periodic Tale, what were some of the problems?

Answer 16

1. Incomplete
2. No explanation as to why some elements had to be swapped to fit in appropriate groups

Question 17

In the modern Periodic Table, how are elements grouped?

Answer 17

By atomic number

Question 18

In the modern Periodic Table, are there gaps?

Answer 18

No gaps - all elements up to a certain atomic number have been discovered

Question 19

In the modern Periodic Table, how are elements grouped?

Answer 19

Metals are on the left; non-metals are on the right

Question 20

How was Mendeleev able to accurately predict the properties of undiscovered elements?

Answer 20

By the position of gaps in his Periodic Table

Question 21

What did the discovery of electrons allow scientists to do?

Answer 21

Work out that the elements with the same number of electrons in their outer shell had similar properties

Question 22

What did the discovery of protons allow scientists to do?

Answer 22

Order the elements in the Periodic Table by their atomic number

Question 23

What did the discovery of neutrons allow scientists to do?

Answer 23

Discover isotopes. This helped them understand why some elements didn’t seem to fit when the Periodic Table was organised by atomic mass.

Question 24

What are the properties of noble gases?

Answer 24

1. Full outer shells with 8 electrons
2. Are very unreactive (inert)
3. Boiling points increase down the group

Question 25

What do Group 1 elements react with?

Answer 25

Oxygen, chlorine, water

Question 26

Why are Group 1 metals called alkali metals?

Answer 26

They react with water to form an alkali (a solution of their metal hydroxide)

Question 27

What is the reactivity like in Group 1?

Answer 27

As you go down the group, reactivity increases.

Question 28

Why does reactivity decrease down Group 1?

Answer 28

As you move down the group: 1. The atoms increase in size 2. So the outer electron is further from the nucleus 3. And there are more shells shielding the outer electron from the nucleus 4. *Electrostatic attraction between the outer electron and nucleus is weaker* 5. So it is easier to lose the outer electron

Question 29

What is the melting and bowling point like in Group 1?

Answer 29

As you go down the group, melting and boiling points decrease

Question 30

What are the halogens? (structure)

Answer 30

Non-metals that exist as molecules made up of pairs of atoms

Question 31

What is the reactivity like in Group 7?

Answer 31

As you go down the group, reactivity decreases

Question 32

Why does reactivity decrease down Group 7?

Answer 32

As you move down the group: 1. The atoms increase in size 2. So the outer electron is further from the nucleus 3. And there are more shells between the nucleus and the outer shell 4. *Electrostatic attraction between the outer electron and nucleus is weaker* 5. So it is harder to gain the one electron to fill the outer shell

Question 33

What is displacement in Group 7?

Answer 33

More reactive Group 7 elements can take the place of other, less reactive ones in a compound

Question 34

What is an example of displacement in Group 7?

Answer 34

Fluorine displaces chlorine as it is more reactive. Fluorine + potassium chloride -> potassium fluoride + chlorine

Question 35

Why are noble gases inert?

Answer 35

They have full outer shells so do not need to lose or gain an electron