C2:The periodic table

Question 1

Why did Mendeleev leave gaps?

Answer 1

Prediction of future elements.

Question 2

Who invented the modern periodic table?

Answer 2

Mendeleev

Question 3

What is the period table organised by?

Answer 3

Atomic mass

Question 4

How can you determine the amount of electrons in the outer shell?

Answer 4

Group number

Question 5

Common properties of metals:

Answer 5

-Conduct electricity
-Higher B+M points
-Ductile
-Malleable

Question 6

Common properties of non-metals:

Answer 6

-Brittle
-Low B+M points
-Electrical insulators

Question 7

What is different about the noble gases?

Answer 7

They are extremely unreactive.

Question 8

Why are group 0 elements unreactive?

Answer 8

They already have a full outer shell.

Question 9

Properties of alkali metals:

Answer 9

-Very reactive
-Low density (float on water)
-Soft and shiny (until react with oxygen and go dull)

Question 10

Why are alkali metals stored in oil?

Answer 10

So they don’t react with the oxygen in the air.

Question 11

Equation for alkali metals and water:

Answer 11

alkali metal + water =
metal hydroxide + hydrogen

Question 12

What are the melting and boiling points like for alkali metals?

Answer 12

Low, they are reactive. Get lower down the group.

Question 13

As you go down the alkali metals, what happens to the reactivity?

Answer 13

Goes up

Question 14

What do we expect to happen when alkali metal reacts with water?

Answer 14

Fizzing (hydrogen gas), metal floats and moves around.
Potassium’s reaction is so vigorous that the hydrogen produces a lilac flame.

Question 15

What colour does universal indicator turn the water after alkali metal + water?

Answer 15

Purple (alkali)

Question 16

Reaction of alkali metals with halogens:

Answer 16

metal halide (e.g sodium chloride)

Question 17

What does a metal halide produce when formed?

Answer 17

Dissolve in water to form colourless solutins.

Question 18

Properties of halogens:

Answer 18

-low melting and boiling points (goes up going down the group)
-poor conductors of heat and electricity
-all exist in pairs of atoms (diatomic molevules)

Question 19

What do halogens need to do to become an ion?

Answer 19

Gain 1 electron on their outer shell.

Question 20

What happens to the reactivity of halogens as you go down the group?

Answer 20

It goes down.

Question 21

What is a displacement reaction?

Answer 21

A more reactive halogen will displace a less reactive halogen from solutions of its salts.

Question 22

As you go down a group in the periodic table, the number of shells occupied by electrons ______.

Answer 22

Increases

Question 23

Larger atoms lose electrons _____ going down a group.

Answer 23

easier

Question 24

Larger atoms gain electrons ____ going down a group.

Answer 24

Less easier

Question 25

What is the attraction between electron and nucleus callled?

Answer 25

Electrostatic attraction.

Question 26

What effect can shells on inner shells have on the outer shell electrons?

Answer 26

Shielding effect, less electrostatic attraction.

Question 27

What are groups 2 and 3 also known as?

Answer 27

Transition elements.

Question 28

Properties of transition metals:

Answer 28

-good conductors of electricity and heat
-hard and strong
-high densities
-high melting points (other than mercury)

Question 29

Transition metals typically have very _____ reactions.

Answer 29

slow (e.g rusting)

Question 30

What are transition metals useful as?

Answer 30

Structural materials.

Question 31

Transition metals often form very ____ compounds.

Answer 31

Colourful (like copper sulfate being blue)