S5 - Unit 1 Flashcards

1
Q

What happens in an oxidation reaction?

A

Electrons are lost

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What happens in a reduction reaction?

A

Electrons are gained

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What happens in an oxidation reaction apart from losing electrons?

A

Either hydrogen is lost or oxygen is added

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What are the steps involved in writing the equation for a reduction reaction in an acidic solution?

A
  • Balance the main element thats not oxygen
  • Balance the oxygen by adding water
  • Balance the hydrogen by adding hydrogen ions
  • Balance the charge by adding electrons
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What are titrations used for?

A

Measuring the concentration if a solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is atomic size?

A

The covalent atomic radius which is half the distance between the nuclei of two bonded atoms in an element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What happens to atomic size across a period and why?

A

Decreases due to increasing nuclear charge (protons)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What happens to the atomic size down a group?

A

Increases due to to increases no. of shells causing a shielding effect

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is electronegativity?

A

A measure of the tendency of an atom to attract a bonding pair of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What happens to the electronegativity across a period and why?

A

Increases due to the nuclear charge increasing

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What happens to the electronegativity down a group and why?

A

Decreases due to the increasing atomic size caused by extra shells, causing a shielding effect

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is ionisation energy?

A

The energy required to remove one mole of electrons from one mole of gaseous atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What happens to the ionisation energy across a period?

A

Increases due to increasing nuclear charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What happens to ionisation energy down a group?

A

Decreases due to the shielding effect

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is the second ionisation energy definition?

A

The energy required to remove one mole of electrons from one mole of positive gaseous ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Why is the second ionisation energy greater than the first?

A

Because the electrons are being pulled from a shell closer to the nucleus

17
Q

What is the definition of the third ionisation energy?

A

The energy required to remove one mole of electrons from one mole of two-positive gaseous ions

18
Q

Why is the third ionisation energy even greater than the second?

A

Because the electrons are being pulled from a shell even closer to the nucleus

19
Q

What happens to reducing agents in reactions?

A

They are oxidised and therefore lose electrons

20
Q

What happens to an oxidising agents in reactions?

A

they are reduced and therefore gain electrons