S1.3

Question 1

What units does Wavelengths have

Answer 1

m

Question 2

What units does frequency have

Answer 2

Hz

Question 3

Frequency and Wavelength are

Answer 3

Inversely Proportional

Question 4

Energy and Frequency are

Answer 4

directly proportional

Question 5

What are the 7 regions of EM spectrum increasing frequency

Answer 5

Radio waves
Microwaves
Infrared
Visible Light
Ultra Violet
X-rays
Gamma rays

Question 6

What has the highest frequency and highest energy , shortest wavelength in the EM spectrum

Answer 6

Gamma Rays

Question 7

What has the lowest frequency , lowest energy and longest wavelength

Answer 7

Radio waves

Question 8

Red is on the right with

Answer 8

lowest energy lowest frequency and longest wavelength

Question 9

Violet is on the left with

Answer 9

highest energy
highest frequency
shortest wavelength

Question 10

What is the difference between a continuous spectrum and emission line spectrum

Answer 10

Continuous spectrum shows all the wavelengths or frequencies of visible light

Emission line only shows specific wavelengths or frequencies

Question 11

Lines converge at

Answer 11

higher frequencies

Question 12

n= 1 is
and has

Answer 12

closest to the nucleus
lowest energy

Question 13

n=6 is
and has

Answer 13

furthest from the nucleus
highest energy

Question 14

Main energy levels

Answer 14

converge at higher energy

Question 15

How do electrons move between energy levels

Answer 15

By absorbing or emitting energy and getting excited

Question 16

What happens if an electron absorbs an amount of energy

Answer 16

it will transfer from a lower energy level to a higher energy level and be in its excited state
e.g n=2 to n=3

Question 17

What happens after the electron becomes excited

Answer 17

It becomes unstable and emits the same amount of energy that it absorbed and it transitions back down to n=2

Question 18

When the the electron transfers from n=3 to n=2 what colour does it correspond to

Answer 18

red

Question 19

The amount of energy emitted also depends on the

Answer 19

size of the transition

Question 20

When is emission line spectra produced

Answer 20

when electrons transition from higher to lower energy levels

Question 21

Four discrete lines on the spectrum suggest

Answer 21

Electrons can only exist at certain energy levels

Question 22

What radiation correspond when electron transitions from higher energy levels to n=1

Answer 22

UV radiation

Question 23

What radiation corresponds when electron transitions from higher energy levels n=2

Answer 23

visible light

Question 24

What radiation corresponds to when electron transitions from higher energy levels to n=3

Answer 24

Infrared Radiation (lowest energy)

Question 25

What does n= ♾️ represent

Answer 25

The point when the electron has been completely removed from the attraction of the nucleus and the atom has been ionised

Question 26

the larger the transition the

Answer 26

more energy emitted

Question 27

What are the sublevels divided into

Answer 27

s p d f

Question 28

How many electrons can a single atomic orbital hold

Answer 28

two

Question 29

How many atomic orbitals are each sublevel made of

Answer 29

s - 1 atomic orbital
p - 3 atomic orbitals
d - 5 atomic orbitals
f - 7 atomic orbitals

Question 30

How many electrons can each sublevel hold

Answer 30

s - two
p - six
d - ten
f - fourteen

Question 31

The maximum number of electrons in an energy level is

Answer 31

2n squared

Question 32

What are the exceptions to the Aufbau Principle

Answer 32

Copper and Chromium

Question 33

What would you expect electronic configuration of CU 29 to be vs what it actually is

Answer 33

thought : Cu 1s2 2s2 2p6 3s2 3p6 4s2 3d9
Actual : Cu 1s2 2s2 2p6 3s2 3p6 4s1 3d10

Question 34

What’s would be the actual electronic configuration of Cr 24

Answer 34

1s2 2s2 2p6 3s2 3p6 4s1 3d5

Question 35

Why does boron have a lower ionisation energy then Be ?

Answer 35

Be has electronic configuration of 1s2 2s2

B has electronic configuration of 1s2 2s2 2p1

Higher nuclear charge
electrons in p orbitals are of higher energy and further from the nucleus than electrons in s orbitals , therefore require less energy to remove (weaker electrostatic forces of attraction)

Question 36

Why has oxygen got a lower IE than nitrogen
1s2 2s2 2p4
1s2 2s2 2p3

Answer 36

Nitrogen has three singly occupied p orbitals but in oxygen one orbital is doubly occupied. An electron is repelled by the second electron and requires less energy to remove than an electron in a half -filled orbital

Question 37

What happens at the convergence limit

Answer 37

The electron has been removed from the attraction of the nucleus and the atom has been ionised

Question 38

What is Energy measured in

Answer 38

J

Question 39

What is wavelength measured in

Answer 39

m

Question 40

From energy in joules to ionisation energy what do you do

Answer 40

multiply by avogadros constant and divide by 1000

Question 41

Define successive ionisation energy

Answer 41

The energies required to remove more and more electrons from an ion that is becoming increasingly positive

Question 42

What is the first and second ionisation energy equation of Allumium.

Answer 42

Al(g) > Al+ (g) + e- 1st
Al + (g) > Al 2+ (g) + e-

Question 43

The order in which electrons are removed is from

Answer 43

the higher energy levels first

Question 44

After the first ionisation energy why do all successive ionisation energies show an increase ?

Answer 44

After the first ionisation, the electrons are being removed from an increasingly positive ion. This leads to an increase in the electrostatic attraction between the nucleus and the remaining electrons and an increase in the IE

Question 45

How do you determine from the large increase what group an element belongs to

Answer 45

Count the number of electrons before first large increase

Question 46

How can the number of occupied energy levels be identified ?

Answer 46

By the number of jumps +1

Question 47

Identify energy levels

Answer 47

n=1
n=2
n=3
n=4
n=5
n=6