C2 Periodic Table

Question 1

Why ordering of elements changed overtime

Answer 1

New elements were being found and scientists needed to rearrange them by relative atomic mass

Question 2

How the electronic structure of metals and non-metals are different

Answer 2

Atoms of metal give away electrons to form positive ions

Atoms of non-metal gain electrons to form negative ions

Question 3

How the electronic structure of metals and non-metals affects their reactivity

Answer 3

If an atom has more electrons than protons its reactivity increases

Question 4

How electronic structure is linked to the periodic table

Answer 4

The number of electrons in outermost shell depends on the group number the element is in

Question 5

How to use the periodic table to predict reactivity of elements

Answer 5

For metals reactiviy increases down a group

Reactivity decreases moving left to right along a period

Question 6

Why are noble gases unreactive

Answer 6

The atoms of noble gases already have complete outer shells so they have no tendency to lose, gain or share electrons

Question 7

How to predict which ions are stable

Answer 7

How easily an element can achieve a full outer electron shell

Question 8

Properties of group 1 metals

Answer 8

Soft

Reactive

Low melting points

Good conductors of heat and electricity

Low density

Question 9

Why elements in group 1 react similarly

Answer 9

They all have 1 electron in their outer shell

Question 10

Why do the first 3 elements of group 1 float on water

Answer 10

Less dense than water

Question 11

Equation for group 1 metals react with water

Answer 11

2X(s) + 2H2O(s) —> 2XOH(aq) + H2(g)

Question 12

How you can show that hydrogen and metal hydroxides are made when Group 1 metals react with water

Answer 12

Hydroxides dissolve in water to form alkaline solutions

They are purple showing they are strongly alkaline

Question 13

How Group 1 metals are stored and the safety precautions used when dealing with them

Answer 13

Stored in mineral oil or kerosene

Do not expse to air or water

Question 14

How to recognise a halogen displacement reaction

Answer 14

Reaction mixture turns darker and iodine solution forms

Question 15

Why elements in group 7 react similarly

Answer 15

Same number of electrons in outer shell

Question 16

Main properties of halogens

Answer 16

Form negative anions

More dense as go down group

Poor conductors of heat and electricity

Brittle

Question 17

How to complete a halogen displacement reaction

Answer 17

2 drops potassium chloride to each 3 dimples in column 1 of tile

2 drops potassium bromide solution to each of 3 dimples in column 2

2 drops potassium iodide solution to each of 3 dimples in column 3

Question 18

What happens in halogen displacement reaction

Answer 18

The more reactive halogen atoms oxidise the less reactive halide ions

causing halide ions to lose electrons and form halogen atoms

Question 19

Trend in reactivity group 1 metals

Answer 19

Increases as you go down the group

Question 20

Reactivity of group 7

Answer 20

Decreases as go down the group

Question 21

Why group 1 reactivity increases as go down the group

Answer 21

As go down the group

Atoms get larger

Outer electron gets further from nucleus

Attraction between nucleus and outer electron gets weaker so electron is easily more lost

Question 22

Why group 7 reactivity decreases as go down the group

Answer 22

As you go down the group

Atomic mass of halogens increases

Increases in electron shells

Atoms get larger as go down the group therefore attraction of outer electron to nucleus decreases as you go down group 7

Question 23

Trend in group 1 boiling point

Answer 23

Decreases

Question 24

Why group 1 boiling point decreases as go down the group

Answer 24

As go down the group there are more protons, electrons, neutrons and energy levels to the atoms

Atoms get larger

As atom increase in size attractive forces decrease since internuclear distance increases

This leads to lower boiling and melting temperatures

Question 25

Trend in group 7 boiling points

Answer 25

Increases

Question 26

Why trend in boiling point increases as you go down group 7

Answer 26

Atoms increase in size as they gain electron shells

Intermolecular forces are stronger

More energy required to break these forces
so higher boiling and melting points as go down the group

Halogens have covalent bonding

Question 27

How to use nuclear model to explain how the outer electrons experience different levels of attraction to the nucleus

Answer 27

Higher effective nuclear charge causes greater attractions to electrons

Question 28

Properties of transition metals

Answer 28

Hard

Strong

High melting boiling points

Good conductors of heat and electricity

Dense

Question 29

Use of transition metals

Answer 29

Iron used to make steel used to build buildings

Copper used for coins

Question 30

Why mercury is not a typical transition element

Answer 30

Neither the atom or its cations posses an incomplete d-subshell

Question 31

Why Group 1 metals have different properties compared to transition metals

Answer 31

Transition metals react slowly or not at all