The Periodic table: 11.1 to 11.4 COMPLETE

Fluorine

Fluorine

________ and chlorine are gases, bromine is a liquid and iodine is a solid.

Helium

________ is used for filling balloons and weather balloons as it is less dense than air and does not burn.

Chlorine

________ is pale green, bromine is red- brown and iodine is black.

Astatine

________ is at the bottom of Group VII so will be a solid.

transition elements

The ________ form coloured compounds and often have more than one oxidation state, such as iron readily forming compound of both Fe2+ and Fe3+.

Neon

________ and argon are used as inert atmospheres for sensitive experiments where nitrogen is not appropriate.

Francium

________ is rare and radioactive so is difficult to confirm predictions.

vertical columns

Group: these are the ________ that show how many outer electrons each atom has.

Iron

________ for example can lose two electrons to form Fe2+ or three electrons to form Fe3+.

sodium

Group I metals are lithium, ________, potassium, rubidium, caesium and francium.

halide ions

They form ________ by gaining one more electron to complete their outer shells.

Halogens

________ are diatomic, meaning they form molecules of two atoms.

Argon

________ is used to provide an inert atmosphere for welding.

strong metals

They are very hard and ________ and are good conductors of heat and electricity.

Bromine

________ will therefore displace iodine from an aqueous solution of metal iodide.

outermost electrons

When atoms collide and react, it is the ________ that interact.

Eg elements

________ in Period 2 have two electron shells, elements in Period 3 have three electron shells.

Group VIII

The noble gases are in ________ (or Group 0); they are non- metals and have very low melting and boiling points.

medicine

They are used in ________ and surgical applications such as limb and joint replacement (titanium is often used for this as it can bond with bones due to its high biocompatibility)

reactivity of Group VII non metals

The ________ increases as you move up the group.

halogen displacement reaction

A(n) ________ occurs when a more reactive halogen displaces a less reactive halogen from an aqueous solution of its halide.

Astatine

________ is at the bottom of Group VII so will have the highest melting and boiling point.

Fluorine

________ is not allowed in schools so observations and experiments tend to only involve chlorine, bromine and iodine.

transition elements

The ________ have more than one oxidation state, as they can lose a different number of electrons, depending on the chemical environment they are in.

Chlorine

________ will therefore displace bromine from an aqueous solution of metal bromide.

Argon

________ is also used to fill electric light bulbs as it is inert.

Bromine

________ is above iodine in Group VII so is more reactive.

francium

As the reactivity of alkali metals increases down the group, rubidium, caesium and ________ will react more vigorously with air and water than lithium, sodium and potassium.

Fluorine

________ is at the top of Group VII so will have the lowestmelting and boiling point.

Astatine

________ is at the bottom of Group VII so the colour will be darker, so ________ is black.

transition elements

The ________ are used extensively as catalystsdue to their ability to interchange between a range of oxidation states.

argon

Neon, ________ and xenon are used in advertising signs.

Bromine

________ and iodine.

Chlorine

________ is above bromine in Group VII so is more reactive.

Fluorine

________ is at the top of Group VII so will be a gas.

Fluorine

________ is at the top of Group VII so the colour will be lighter, so ________ is yellow.

The table is arranged in vertical columns called Groupsnumbered I

VIII (numbers shown on the course's Periodic Table) and in rows called Periods (numbers not shown on the Periodic Table)

Period

these are the horizontal rows that show the number of shells of electrons an atom has

Group

these are the vertical columns that show how many outer electrons each atom has

The electronic configuration is the arrangement of electrons into shells for an atom (e.g

the electronic configuration of carbon is 2,4)

Example

Electronic configuration of chlorine

Lithium's electronic configuration

2,1

Sodium's electronic configuration

2,8,1

Potassium's electronic configuration

2,8,8,1

1

Form colored compounds

2

used as catalysts

3

high melting points

4

good conductors of heat and electricity

He

2

Ne

2,8

Ar

2,8,8

Kr

2,8,18,8

Xe

2,8,18,18,8