Elements of Life - Atomic Structure

Question 2

What is relative mass measured in comparison to?

Answer 2

The relative mass of a proton or neutron is measured in comparison to (1/12 x carbon¹²)

Question 3

What is the relative mass of an electron?

Answer 3

1/1840

Question 4

What is the general formula for the relative mass?

Answer 4

(mass of isotope x % abundance) + (repeat for all isotopes) divided by 100

Question 5

What is the formula for relative abundance?

Answer 5

peak height / total peak height x100

Question 6

After which element does nuclear fusion usually stop and why?

Answer 6

Iron (Fe) too big

Question 7

Complete the nuclear equation: Hydrogen 1 + Hydrogen 1 ->

Answer 7

Helium 2

Question 8

Complete the nuclear equation: Helium 2 + a neutron ->

Answer 8

helium 3

Question 9

under which conditions can nuclear fusion occur?

Answer 9

very high temperatures and pressure due to the electrostatic repulsion of the positive nuclei

Question 10

What physical state must elements be in for mass spectroscopy?

Answer 10

gas

Question 11

What is mass spectroscopy used for?

Answer 11

Calculating the masses of different isotopes of the same element

Question 12

What equation links speed of light, wavelength and frequency?

Answer 12

Speed of light = wavelength x frequency C = λν

Question 13

What equation links energy, frequency and planck’s constant?

Answer 13

Energy = frequency x planck’s constant E = hν

Question 14

What is the quantisation of energy?

Answer 14

the theory that subatomic particles have no ‘in between’ speeds -> they go from one to the other instantaneously energy exists in specific packets called quanta

Question 15

Describe what an absorption spectra looks like

Answer 15

Coloured background with black lines

Question 16

Draw an example of an absorption spectra graph

Answer 16

Question 17

Draw an example of an absorption spectra graph

Answer 17

Question 18

Describe what an absorption spectra looks like

Answer 18

Coloured background with black lines

Question 19

Describe what an emmision spectra looks like

Answer 19

A black background with coloured lines

Question 20

Describe how an atomic emmission spectrum is produced

Explain why atomic emission spectrums are unique to particular elements

Answer 20

Excite the atoms to a higher energy level with energy (eg heat)

They then fall from a higher to lower energy level

Energy is quantised and coloured lines are produced as a result of E=hν

Energy levels are unique to the atom and therefore the ν emitted is unique to the atom

Question 21

How many electrons can S, D and P orbitals hold?

Answer 21

S -> 2

P -> 6

D -> 10

Question 22

After which element can the outer energy level hold more than 8 electrons?

Answer 22

Beyond Calcium, energy levels can take up to 18 electrons

Question 23

Define isoelectronic

Answer 23

When two different elements have the same electron configuration

eg K⁺ = Ar

Question 24

What is the wave theory of light?

Answer 24

As light is a form of EM radiation, it behaves like a wave

The speed of light is always constant despite wavelength and frequency changing

Question 25

What is the particle theory of light?

Answer 25

Light exists in packets of energy called photons

Question 26

How are the wave and particle theories of light linked?

Answer 26

energy of a photon = planck’s constant x frequency

Question 27

Describe Bohr’s theory about electrons

Answer 27

• > electrons only exist in specific energy levels
• > a photon of light is emitted when an electron changes energy levels
• > the energy of the photon is equal to the energy difference between the 2 energy levels
• > E = hν

Question 28

Describe how absorption spectras work

Answer 28

White light is passed through a cool sample of a gaseous element

The black lines on the spectrum represent the light absorbed by the atoms

Question 29

Explain how the atomic emission spectra shows that elements exist in energy levels

Answer 29

Each energy level has a specific frequency due to E = hv

The energy drops between each energy levels produce specific lines

Question 30

state the major trend in the first ionisation enthalpies across a period

explain in terms of electron energy levels, how this occurs

Answer 30

(from left to right) the ionisation enthalpie increases throughout the period

all electrons are in the same energy level, but as you go across they have more protons and therefore more electrostatic attraction so more energy is required to break them

Question 31

What is the EM spectrum?

(highest to lowest wavelength)

Answer 31

Radio, Infrared, Visible Light, Ultraviolet, X-Ray, Gamma