C2 Periodic Table

Question 1

Why are group one metals stores in oil?

Answer 1

To keep air and water away from them

Question 2

Are group one very reactive or no?

Answer 2

Very reactive

Question 3

What happens when alkali metals react with water?

Answer 3

When dissolved, they form metal hydroxides which are alkaline (ph above 7, universal indicator purple)

Question 4

Give some physical properties of alkali metals

Answer 4

Low melting points (as opposed to to normal metals)
Very soft
Low densities (less than 1g/cm^3, so they can float on water)
Silvery shiny surface (quickly goes dull)

Question 5

As you go down group one…

Answer 5

Melting points decrease
Elements are more reactive

Question 6

What happens when an element in group 1 takes part in a reaction?

Answer 6

It’s atoms loose their outer electron and form positive ions (called cations). The more easily this happens, the more reactive the metal

Question 7

Why does reactivity in group 1 increase as you go down the group?

Answer 7

• Atoms become larger
• Outer electron is further from the nucleus
• Force of attraction between nucleus and outer electron decreases
• Outer electron is lost more easily

Question 8

What is the equation for Alkalis in water?

Answer 8

Metal hydroxide + hydrogen gas

Question 9

When you go down the Halogens group-

Answer 9

Boiling and melting points increase
Reactivity decreases

Question 10

What is Fluorine?

Answer 10

A poisonous yellow gas

Question 11

What is chlorine?

Answer 11

A poisonous green gas

Question 12

What is Bromine?

Answer 12

A poisonous brown liquid

Question 13

What is Iodine?

Answer 13

A dark grey solid/poisonous purple vapours
Can be antiseptic

Question 14

Halogens can exist in pairs of atoms called ———

Answer 14

Diatomic molecules
They do this by sharing electrons in the outer shell and forming a covalent bond.

Question 15

When you go down the Noble gases group-

Answer 15

The boiling points increase
The density increases

Question 16

Give some physical properties of Noble gases

Answer 16

• Non-reactive
• Non- flammable
• Colourless gases

Question 17

Do Noble gases bond with other elements?

Answer 17

Noble gases exist alone and don’t bond with other elements.
They have full outer shells

Question 18

Why do Nobel gases not easily form molecules?

Answer 18

They are stable with a full outer shell

Question 19

What is Halogen displacement?

Answer 19

This includes a more reactive halogen displacing (or takeoff the place of) a less reactive one.
For example, fluorine would take the place of chlorine in a reaction and equation.

Question 20

Give an example of a halogen displacement equation

Answer 20

Cl^2 (g) + 2kBr (aq) ➡️ Br^2 (g) + 2kCl (aq)

Question 21

Where are transition metals located?

Answer 21

In the middle of the periodic table

Question 22

Give some properties of transition metals

Answer 22

• Shiny (lustrous)
• Hard
• High density
• Maleable (bendable)
• Ductile (can be stretched into wires)
• Good conductors of heat
• High melting and boiling points (except Mercury)
  (All you would expect metals to be)

Question 23

Compare transition metals with alkali metals

Answer 23

• Harder and stronger
• More dense
• Higher melting and boiling points

Question 24

Are transition metals as reactive as alkali metals? Explain

Answer 24

Transition metals are much less reactive than alkali metals.
They react slowly, for example with air, water and acid.
For example copper doesn’t react with water but alkali metals such as sodium, react vigorously. This is the same with air

Question 25

What are the reactivity patterns in transition metals?

Answer 25

They mostly decreases in reactivity from left to right There are exceptions such as Zinc

Question 26

What are the colours of metal ions?

Answer 26

Cu^2+ Blue 🦋 Ni^2+ Pale green 🍋‍🟩 Cr^3+ Dark green 🌲 Mn^2+ Pale pink 🌸 Fe^2+ Pale green 🍋‍🟩 Fe^3+ Yellow 🌼

Question 27

What can transition metals react with?

Answer 27

- Oxygen (copper oxide) - Water (Iron and oxygen = hydroated iron oxide (rust)) - Halogens (Iron and chlorine = iron chloride)

Question 29

How are chemical elements placed in the periodic table?

Answer 29

Order of their atomic (proton) number This arranges them so that they line up in groups with similar properties

Question 30

Why do elements in the same group of the periodic table react in similar ways?

Answer 30

Their atoms have the same number of electrons in the highest occupied energy level (outermost shell)

Question 31

What are the differences between metals and non metals?

Answer 31

Metals conduct electricity but non metals are electrical insulators generally (exceptions are forms of carbon) Metals generally have higher melting and boiling points Comparing solid examples metals are ductile and malleable whereas non metals are brittle (can break easily)

Question 32

What ions do non metals and metals form ?

Answer 32

Metals- positive Non metals- negative

Question 33

Why are alkali metals so reactive?

Answer 33

Electronic structure Having one electron on the outer shell makes them very reactive as they only need to lose one electron to get a stable structure of a noble gas (so they react with non metals to loose the electron, always forming ionic compounds)

Question 34

What happens when alkalis react with non metals such as chlorine gas?

Answer 34

They produce metal chlorides which are white solids that can dissolve in water to form a colourless solution

Question 35

Why do alkali reactions get more vigorous going down the group?

Answer 35

It is easier to lose the single electron in the outer shell

Question 36

Give some properties of Halogens

Answer 36

Low melting and boiling points Poor conductors of heat and electricity

Question 37

How do Halogens gain one electron?

Answer 37

Through reacting with metals

Question 38

Halogens all react with —

Answer 38

Metals

Question 39

Page 28 for displacement practical

Question 40

The atoms get larger going down any group what two effects does this have?

Answer 40

- larger atoms lose electrons more easily going down a group - larger atoms gain electrons less easily going down a group This happens because the outer electrons (neg.) are further away from the attractive force of the nucleus (pos.) Also, the inner shells of electrons ‘screen’ or ‘shield’ the outer electrons from the positive charge of the nucleus.

Question 41

Why does reactivity increase going down group one?

Answer 41

Atoms get larger so single electron in the outermost shell is attracted less strongly to the positive nucleus. The electrostatic attraction with the nucleus gets weaker because the distance between the outer electron and nucleus increases Ask the outer electron experiences the shielding effect from inner shells of electrons.

Question 42

Why does the bigger positive charge in bigger atoms not make the force of attraction bigger between the nucleus and the outermost proton?

Answer 42

The greater the distance and mostly the shielding effect of inner electrons outweigh the increasing nuclear charge

Question 43

What does the size of the atoms, the shielding effect and nuclear charge mean for alkalis and halogens?

Answer 43

Group 7- Going down the group, it is harder to attract and gain an extra incoming electron. Group 1- Going down the group, the outer electron is easier to remove (so they get more and more reactive)

Question 44

What is an alloy? Give examples:

Answer 44

A mixture of a metal Eg: Steel (contains iron) Brass (containing copper and zinc)

Question 45

What are some physical properties of transition metals?

Answer 45

- Good conductors of electricity and thermal energy - Hard and strong - High densities - High melting points (except Mercury which is liquid at room temperature)

Question 46

What are some chemical properties of transition metals?

Answer 46

- Less reactive than G1 - They don’t react as readily with oxygen, chlorine and water as alkali metals - If transition metals corrode they do so very slowly - (Some can rust)

Question 47

How do you know if a compound contains a transition element?

Answer 47

It will usually include a Roman number like copper(II) sulfate This is because transition elements can form more than one ion (eg- Fe^2+ and Fe^3+). Compounds of these different ions are different colours.