Atomic Structure

Question 1

What are the different types of subatomic particles

Answer 1

neutrons, electrons and protons

Question 2

Define atomic number

Answer 2

the number of protons in the nucleus of an atom

Question 3

Define mass number

Answer 3

the number of protons and neutrons in the nucleus of an atom

Question 4

Define isotopes

Answer 4

the atoms of the same element that have the same number of protons but different number of neutrons

Question 5

How many electrons can a main energy level hold

Answer 5

2n^2

Question 6

Properties of s orbitals

Answer 6

they are spherical in shape and can hold a max of 2 electrons

Question 7

Properties of p orbitals

Answer 7

they are dumbbell shaped (3) + can hold max of 6 electrons

Question 8

What are the main energy levels

Answer 8

s<p<d<f

Question 9

How to write electronic configuration for transition metals

Answer 9

they fill the 4s sub shell before the 3d sub shell AND they also lose from the 4s sub shell first

Question 10

What is the electronic configuration of Cr

Answer 10

4s1 3d5

Question 11

What is the electronic configuration of Cu

Answer 11

4s1 3d10

Question 12

Describe the electromagnetic spectrum

Answer 12

radio ways, microwaves, infrared, UV, X-rays, Gamma rays

Question 13

Describe the relationship between frequency, wavelength and energy

Answer 13

high frequency, shorter wavelength and high energy
low frequency, longer wavelength and low energy

Question 14

What is a continuous spectrum

Answer 14

It shows all the wavelengths, frequencies of visible light

Question 15

What does an absorption spectrum

Answer 15

it shows black lines on a coloured background because electrons gain energy, to go to higher energy levels

Question 16

What does an emission spectrum

Answer 16

it shows coloured lines on a black background because electrons release energy and return to a lower energy level

Question 17

The representation of each of the energy levels in the hydrogen spectrum

Answer 17

n1= UV
n2= visible light
n3= infrared

Question 18

How is the emission spectrum

Answer 18

It is produced when an electron emits energy and transitions to a lower energy level. The energy emitted corresponds to the wavelength/frequency of the energy level (visible light, infrared, UV)

Question 19

How is the absorption spectrum

Answer 19

It is produced when an electron absorbs energy and transition to a higher energy level. The energy absorbed corresponds to the wavelength/frequency of the energy level (visible light, UV, infrared)

Question 20

What does the arrow represent

Answer 20

the amount of energy absorbed or released
- the longer the arrow the more energy released or absorbed

Question 21

What is the limit of convergence

Answer 21

where the lines appear to meet, it represents the first ionisation energy

Question 22

How to calculate the ionisation energy

Answer 22

ΔE = h ν
h=plancks constant v=frequency
c = ν λ
c=speed of light, v=frequency, λ=wavelength

Question 23

Important thing to remember when calculating ionisation energy

Answer 23

multiply with the Avogadro constant and divide by 1000

Question 24

What are the 4 factors that affect ionisation energy

Answer 24

size of nuclear charge, distance of outer electrons from nucleus, shielding effect, spin-pair repulsion

Question 25

General trend in ionisation energy across the period

Answer 25

It increases

Question 26

General trend in ionisation energy down the group

Answer 26

It decreases

Question 27

The general equation for ionisation energy

Answer 27

X^(n-1)+ (g) → X(n)+ (g) + e-

Question 28

Explain the effect of nuclear charge on ionisation energy

Answer 28

As the size of the nuclear charge increases the force of attraction between the electrons the nucleus increases – greater ionisation energy

Question 29

Define ionisation energy

Answer 29

the minimum amount of energy needed to remove one mole of electrons from one moles of gaseous atoms

Question 30

Explain the effect of outer electrons on ionisation energy

Answer 30

the force of electrostatic attraction between the positive nucleus and negative electrons decreases as the distance increases between them – lower ionisation energy

Question 31

Explain the effect of the shielding effect on ionisation energy

Answer 31

electrons in the full inner shells repel the electrons in the outer shell, so the electrostatic force of attraction between the nucleus and the outer electrons weakens – lower ionisation energy

Question 32

Why does ionisation energy decrease across the period at certain moments in time (3 reasons)

Answer 32

1) electrons in p orbitals are of higher energy and further away from the nucleus than s orbitals - less energy is required to remove the electron (Be - B)
2) electron is in a doubly occupied orbital, so it is repelled by the other electron (N -O)
3) another shell is being added (He - Li)

Question 33

What are the 3 different types of spectrums

Answer 33

absorption, emission and continuous

Question 34

Why does successive ionisation energy increase across a period

Answer 34

electrons are being removed from increasingly more positive ions. The large increase in ionisation energy corresponds to a change of a new shell