The Periodic Table - Group I properties

Front

What trends can be seen in group I elements (lithium, sodium and potassium)?

Back

-        All relatively soft metals.

-        Decrease in melting point down the group

-        Increases in density down the group

-        Increase in reactivity with water down the group.

Front

How does melting point change down Group I?

Back

Melting point decreases down the group because the strength of the metallic bonds decreases so less energy is required to break these bonds to turn the solid into a liquid.

Front

How does density change down Group I?

Back

Density increases down the group.

All Group I elements have low densities and will float on water.

Front

What is the trend in the reactivity with water down Group I?

Back

Reactivity increases down the group.

Front

Why does reactivity increase down Group I?

Back

Group I elements lose an electron when they react. Atomic radius and electron shielding increase down the group so there is weaker attraction between the nucleus and outer shell electron. This means less energy is required to remove this electron from elements further down the group.

Front

Describe the general reaction of a Group I element with water

Back

Vigorous reaction with water, producing hydrogen and an alkaline solution. Bubbles will be seen due to the production of hydrogen.

Front

Using the trend in melting points, predict which element in Group I has the highest melting point

Back

Lithium

Front

Using the trend in density, predict which element has the highest density out of sodium, lithium and caesium

Back

Caesium