Periodic table

Question 1

Group names

Answer 1

1. Alkali metals
2. Alkaline earth metals
   Between 2 and 3. Transition metals
3. Boron family
4. Carbon family
5. Nitrogen family
6. Oxygen family
7. Halogens
8. Noble gases

Question 2

Periods

Answer 2

Go vertically down the group and tell us the number of electron shells in an atom

Question 3

Groups

Answer 3

Go horizontally and tell us the number of valence electrons

Question 4

Alkali metals properties

Answer 4

Silver, soft, low density

Question 5

Alkali metals

Answer 5

Reactivity increases down the group as there is a greater distance from the nucleus to valence electron (it is lost easier), weak bonds
Density increases down the group
Melting point decreases down the group

Question 6

Halogens

Answer 6

They are diatomic, 7 outer electrons
Fluorine and chlorine are yellow gases
Bromine is a dark red liquid
Iodine is shiny black
Melting and boiling points increase down the group 
Reactivity decreases down the group

Question 7

Noble gases

Answer 7

Boiling point increases down the group and so does density

Gets more reactive

Question 8

Transition metals

Answer 8

“oxidation state”= the charge on the metal ion

Question 9

Alloys

Answer 9

Alloys are mixtures of metals. The resulting material has properties of each metal and are useful in society. Pure metals are soft as the ions are the same size and can move over each other. Alloys are hard as the different sized ions do not allow movement

Question 10

Properties of metals

Answer 10

• conduct electricity and heat well (delocalised electrons)
• high melting point (strong metallic bonds)
• high density (ions are close together)
• malleable, shiny, ductile

Question 11

Reactivity series of metals

Answer 11

Lowest reactivity: Copper, tin, iron, zinc, magnesium, calcium, sodium and potassium (highest reactivity)

Question 12

Metal + oxygen

Answer 12

Magnesium + Oxygen = magnesium oxide