C1 Periodic Table

Question 1

Do metal ions lose or gain electrons?

Answer 1

Metal ions lose electrons and become positive

Question 2

Do non-metal ions lose or gain electrons?

Answer 2

Non metal ions gain electrons and become negative

Question 3

What has happened for an atom to become an ion?

Answer 3

When an atom becomes an ion it has either lost or gained an electron

Question 4

How do you work out the number of electrons in an ion?

Answer 4

The symbol/s next to the ion shows weather the atom has lost or gained electrons. Whatever this number/symbol is you add/take away from the number of electrons.

Question 5

What is the difference between Newlands periodic table and the modern periodic table?

Answer 5

Newlands Periodic Table:
Each period has 7 elements
Metals and non metals are mixed together
Some elements are in different groups eg Oxygen group 7
It is ordered by atomic mass
Fewer elements
There is no group 8, no noble gasses
Noble gasses haven’t been discovered yet

Modern Periodic Table:
Periods can have different amounts of elements in them
Metals and nonmetals are separate
Oxygen is in group 6
Ordered by atomic number
Group 8 included

Question 6

Who created the modern periodic table?

Answer 6

Mendeleev

Question 7

How did mendeleev arrange the elements in the periodic table?

Answer 7

He arranged the elements in order of increasing atomic weight and grouped elements that had similar properties. He also left gaps for elements that hadn’t been discovered yet.

Question 8

Why were there gaps in the periodic table?

Answer 8

There were gaps for elements that hadn’t been discovered yet.

Question 9

What predictions could be made about the gaps in the periodic table?

Answer 9

You could predict its: atomic weight, weather its a metal or nonmetal, melting point

Question 10

What properties do metals have?

Answer 10

Hard, stong, good at conducting heat, good at conducting electricity, shiny, ductile, malleable, sonorous, high melting point, mostly solid and room temperature.

Question 11

What properties do nonmetals have?

Answer 11

Soft, brittle, low melting point, mostly liquid or gas at room temperature, dull

Question 12

Why is copper good for making wires?

Answer 12

Copper is used to make electrical wires because they can be easily bent into the correct shape because metals are ductile. They also conduct electricity well so this makes copper good for a wire.

Question 13

What are the Trend in Group 8 elements

Answer 13

Density increases as you go down the group because the atoms become larger as they gain more protons and neutrons

Boiling point increases as you go down the group because the atoms get bigger so there are stronger intermolecular forces which means there is more energy required to overcome forces

Question 14

Trends in group 1 metals

Answer 14

Density decreases as you go down the group
Hardness decreases as you go down the group
Reactivity increases as you go down the group

Question 15

What forms when Lithium reacts with oxygen

Answer 15

Lithium oxide

Question 16

What forms when Lithium reacts with chlorine

Answer 16

Lithium chloride

Question 17

What forms when Lithium reacts with water

Answer 17

Lithium hydroxide + hydrogen

Question 18

What are electrons attracted to?

Answer 18

Electrons are negative they are attracted to the positive part of the atom, the nucleus

Question 19

What are electrons held in place by?

Answer 19

Electrons are held in place with electrostatic attractions between negative electrons and the positive protons in the nucleus

Question 20

What is electrostatic?

Answer 20

the attraction between the negative electrons the outer shells and the positive protons in the nucleus

Question 21

When group 1 metals react, they lose electrons this means:

Answer 21

there are more electron shells
the outer electron is further away from positive nucleus
The electrostatic attraction is weaker
The electron is lost more easily

Question 22

Which is more reactive, potassium or lithium?

Answer 22

Potassium is more reactive than lithium.
Potassium has more shells of electrons than lithium.
This means there’s more shielding between the positive nucleus and the negative electron in potassium’s outer shell.
There is weaker electrostatic attraction between the positive nucleus and negative electron in the outer shell.
This makes it easier for potassium to lose an electron than lithium.

Question 23

What are the properties of group 7?

Answer 23

Low melting points
Diatomic molecules
Poor conductors of heat and electricity
Darker as you move down the group

Question 24

What are the trends of group 7?

Answer 24

Melting point increases down the group
Reactivity decreases down the group

Question 25

When group 7 metals react, they gain electrons this means:

Answer 25

More electron shells
Outer electron is further away from positive nucleus
The electrostatic attraction is weaker
Harder to gain an electron

Question 26

What are the halogens?

Answer 26

group 7

Question 27

complete equation:
Metal + halogen →

Answer 27

metal halide

Question 28

What is displacement?

Answer 28

Displacement is where a more reactive element takes the place of a less reactive element in a compound.

Question 29

Fluorine + lithium bromide →

Answer 29

Bromine + lithium fluoride

Question 30

Chlorine + sodium fluoride →

Answer 30

NO REACTION

Question 31

Potassium bromide + chlorine →

Answer 31

Potassium chloride + bromine

Question 32

how do you work out a displacement equation?

Answer 32

1) work out which element in group 7 is more reactive (tip reactivity decreases as you go down the group)
2) if the element that is on its own is more reactive, it will replace the other element in the second part of the equation
3) the one that was on its own in the first part of the equation becomes ‘IDE’ in the second part of the equation

Question 33

What is an example of an alkali metal?

Answer 33

Sodium, potassium, lithium

Question 34

What is an example of a halogen

Answer 34

Fluorine, chlorine, bromine