3.1.1 Atomic structure

Question 1

Nucleons

Answer 1

Nucleons are protons and neutrons in the nucleus.

Question 2

Position of protons

Answer 2

Nucleus

Question 3

Relative mass of a proton

Answer 3

1

Question 4

Relative charge of a proton

Answer 4

+1

Question 5

Position of neutrons

Answer 5

Nucleus

Question 6

Relative mass of a neutron

Answer 6

1

Question 7

Relative charge of a neutron

Answer 7

0

Question 8

Position of electrons

Answer 8

Orbitals

Question 9

Relative mass of an electron

Answer 9

1/1800

Question 10

Relative charge of an electron

Answer 10

-1

Question 11

Mass number

Answer 11

Sum of protons and neutrons

Question 12

Atomic number

Answer 12

The amount of protons in the nucleus

Question 13

Number of neutrons is worked out by…

Answer 13

Subtracting the atomic number from the mass number

Question 14

Isotopes

Answer 14

Atoms of the same element with the same number of protons but a different amount of neutrons

Question 15

Isotopes have similar chemical properties because…

Answer 15

they have the same electron configuration

Question 16

Isotopes have varying physical properties because…

Answer 16

they have different masses

Question 17

Ions

Answer 17

A charged particle formed when an atom or molecule gains

or loses one or more electrons

Question 18

Relative Isotopic Mass

Answer 18

The mass of an atom of a particular isotope compared to 1/12

the mass of an atom of carbon-12

Question 19

Relative Atomic Mass (Ar)

Answer 19

The average mass of an atom compared to 1/12 the mass of

an atom of carbon-12

Question 20

Relative Molecular Mass (Mr)

Answer 20

The average mass of a molecule compared to 1/12 the mass

of an atom of carbon-12

Question 21

Mass Spectrometer: Why is it kept in vacuum conditions?

Answer 21

To prevents the ions produced colliding with molecules of air

Question 22

Mass Spectrometer: What happens during ionisation?

Answer 22

The sample is dissolved in a volatile solvent and forced
through a fine, hollow needle which is connected to a
positive terminal of a high voltage supply. The sample is shot
with an electron gun, which knocks off an electron,
producing positively charged ions.

Question 23

Mass Spectrometer: What happens during acceleration?

Answer 23

Positive ions are attracted to a negatively charged plate,
causing them to accelerate. Lighter ions with a higher charge
move faster

Question 24

Mass Spectrometer: What happens during ion drift?

Answer 24

The ions pass through a hole in the negatively charged plate,
forming a beam, which drift towards the detector

Question 25

Mass Spectrometer: What happens during detection?

Answer 25

The lighter ions which have the fastest velocities arrive at the detector first. The positive ions pick up an electron, causing a current to flow

Question 26

Mass Spectrometer: What happens during data analysis?

Answer 26

Signals from the detector are passed to a computer which | generates a mass spectrum

Question 27

Mass Spectrometer: What is the mass spectrometer | measuring?

Answer 27

M:Z ratio and abundance

Question 28

How do you calculate R.A.M from a mass spectrum?

Answer 28

You multiply the m:z ratio and abundance together for each peak. You then add the totals together and divide by the total relative abundance.

Question 29

What sub-level can principle level 1 hold?

Answer 29

1s

Question 30

What sub-levels can principle level 2 hold?

Answer 30

2s, 2p

Question 31

What sub-levels can principle level 3 hold?

Answer 31

3s, 3p, 3d

Question 32

What sub-levels can principle level 4 hold?

Answer 32

4s, 4p, 4d, 4f

Question 33

How many electrons can sub-level S hold?

Answer 33

2

Question 34

How many electrons can sub-level P hold?

Answer 34

6

Question 35

How many electrons can sub-level D hold?

Answer 35

10

Question 36

How many electrons can sub-level F hold?

Answer 36

14

Question 37

What shape are S sub-levels?

Answer 37

Spherical

Question 38

What shape are P sub-levels?

Answer 38

Dumbbells

Question 39

Why is the 3d sub-level filled after the 4s sub-level?

Answer 39

Because 3d is higher in energy, so 4s is filled first and then when 3d is filled, the energy level drops to below 4s

Question 40

First Ionisation Energy

Answer 40

The enthalpy change when one mole of gaseous atoms forms one mole of gaseous atoms with a singe positive charge by losing one electron

Question 41

Second Ionisation Energy

Answer 41

The enthalpy change when one mole of gaseous ions with a single positive charge forms one mole of gaseous ions with a 2+ charge by losing one electron

Question 42

Factors affect ionisation energy: Nuclear Charge

Answer 42

The higher the nuclear charge (the more protons there are) | the greater the attraction of the outer electrons to the nucleus

Question 43

Factors affect ionisation energy: The distance of the outer | electrons to the nucleus

Answer 43

The larger the atom, the further the outer electrons are away from the nucleus, making the attraction weaker

Question 44

Factors affect ionisation energy: Shielding

Answer 44

Electrons in the outer shell are repelled by electrons in complete inner shells, weakening the attraction of the nucleus

Question 45

Factors affect ionisation energy: In-orbital Repulsion

Answer 45

Once the electrons are paired, they start repelling each other, the degree of repulsion affects how easy it is to remove electrons

Question 46

Why are the successive ionisation energies always higher?

Answer 46

Because a positive ion is formed from the first ionisation energy, meaning the nuclear attraction increases, making it harder for the second electron to be removed

Question 47

Why is He's ionisation energy bigger than H's?

Answer 47

- Increased nuclear charge (gone from + to +2) - Same shielding - Same distance from nucleus to outer electron

Question 48

Why is there such a large drop of ionisation energy between | He and Li?

Answer 48

- Increased shielding (Li enters 2s orbital, He still on 1s) - Increased nuclear charge - Outer electrons are further away from the nucleus

Question 49

Why is Be's ionisation energy greater than Li?

Answer 49

-Increased nuclear charge -Shielding same as Li -Outer electrons are the same distance away from the nucleus in both

Question 50

Why is Be's ionisation energy higher than B?

Answer 50

-Increased nuclear charge -Increased shielding (B enters 2p orbital) so is shielded by 1s and 2s orbitals -Outer electrons are further away in B

Question 51

Why is there a drop of ionisation energy between N and O?

Answer 51

- Increased nuclear charge - Shielding same (still in 2p orbital) - Same amount of shielding