groups

Question 1

Elements in Group 1 are

known as…?

Answer 1

The alkali metals

Question 2

State three characteristics of

the Alkali Metals

Answer 2

• All have one electron in their outer shell; have low density
• are stored under oil (to prevent reactions with oxygen or water)
• are soft (can be cut with knife).

Question 3

How do Group 1 elements react
with non-metals? Why are these
reactions similar for the different
Group 1 elements?

Answer 3

They form ionic compounds which are soluble white solids which form colourless solutions

– they all have one electron in their outer shell.

Question 4

How do Group 1 elements

react with water?

Answer 4

• They release hydrogen and form hydroxides which dissolve to form alkaline solutions
• react vigorously with water fizzing and moving around on the surface of the water.

Question 5

How does the reactivity
change moving down Group
1? Why?

Answer 5

• Reactivity increases as the atoms get larger and the distance between the nucleus and the outer electrons increases
• thus attraction from the nucleus decreases, allowing them to more easily lose electrons

Question 6

State five characteristics of
Group 7 (halogens)

Answer 6

• 7 electrons in outer shell
• Coloured vapours
• Diatomic molecules with covalent bond
• Form ionic salts with metals
• Form molecular compounds with non-metals

Question 7

State Group 7 elements and

their states of matter.

Answer 7

- Fluorine, F. F2
 is a pale yellow gas.
- Chlorine, Cl. Cl2
 is a pale green gas.
- Bromine, Br. Br2
 is dark brown liquid
- Iodine, I. I2
 is a grey solid.

Question 8

State three changes that
occur in Group 7 as one
moves down the group

Answer 8

• Higher relative molecular mass
• Higher melting and boiling point
• Less reactive – less easily gain electrons

Question 9

A more reactive halogen displaces a less reactive one from an aqueous solution of its salt; explain the trend in reactivity of halogens in these reactions

Answer 9

Reactivity decreases down the group. As we go down the group, the atoms get larger, so an incoming electron will be less tightly held by the attractive forces from the nucleus.

That’s why Cl2 displaces Br– and I–

Question 10

Compare Group 1 metals and

transition metals

Answer 10

• both heat and electricity conductors.
• shiny when polished and form ionic compounds with non metals.
• Transition metals have higher densities and higher melting points than Group 1 metals.
• They are less reactive and harder than Group 1 metals.

Question 11

State common
characteristics of transition
metals

Answer 11

• Hard and strong metals
• High density and m.p
• Less reactive than g1 metals
• Can form ions with different charges
• Form coloured compounds
• Catalytic properties

Question 12

What is a catalyst?

Answer 12

A catalyst is a chemical substance that increases the rate of a
chemical reaction.
It is not used up over the course of the reaction.

Question 13

State the colours of flames
observed when lithium,
sodium, and potassium burn
in oxygen

Answer 13

Crimson-red, Li
Yellow-orange, Na
Lilac, K

Question 14

Describe the properties of group 0, the noble gases. Discuss the trend in boiling
point down the group.

Answer 14

• Non-metals
• gases
• low boiling points
• unreactive because they have a full outer shell; they don’t easily accept or lose electrons, very stable
• The boiling point increases down the group, as the atoms get heavier.

Question 15

Whats a key fact to know ab metals?

Answer 15

• when metals react, they lose electrons to achieve a full outer shell
• to give them the same electronic structure as a noble gas
• always form positive ions

Question 16

What forms when group 7 elements react w other non metals?

Answer 16

Covalent compounds

Question 17

What forms when group 7 elements react w metals?

Answer 17

Ionic compounds, and the group 7 element gains one electron and forms a 1- ion