quantisation of energy

Question 1

Quantised

Answer 1

Electrons can only exist in energy levels

Question 2

How do electrons jump between discrete energy levels

Answer 2

By absorbing or emitting energy

Question 3

Ground State

Answer 3

lowest energy state, most stable

Question 4

exited state

Answer 4

jumping to a higher energy level

Question 5

electromagnetic spectrum

Answer 5

range of different forms of electromagnetic radiation

Question 6

radiation from each portion can be described

Answer 6

in terms of frequencies, wavelengths and energy

Question 7

what happens when atoms return to ground state

Answer 7

absorb certain amount of electromagnetic radiation

Question 8

absorption

Answer 8

electrons can jump up to a higher energy level if it absorbs energy that corresponds exactly to the difference in energy between the lower and higher energy level

Question 9

absorption lines

Answer 9

represents electron jumping from one shell to another by absorbing specific wavelength energy. this wavelengths can respond to specific colours and energy that provide exact quantity required to promote electrons

Question 10

emission

Answer 10

electron returns to lower shell and emits energy in the form of light that corresponds to the exact distance from higher to lower shells/

Question 11

transition of electron

Answer 11

each electron makes an emission of specific quantities energies in the form of different colours

Question 12

emission lines

Answer 12

specific colours of light that perfectly correspond to the energy difference between two levels are emmited

Question 13

explain how emission spectra provide evidence for electron shells in the Bohr model

Answer 13

Each emission line correspond to a specific energy emited when electrons transition from a higher energy level to a lower energy level. This shows differences in energy levels and shows that electrons are found in shells with discrete energy levels.

Question 14

describe how the emission spectra can be used to identify elements.

Answer 14

emission lines show specific colours that are emitted when electrons move from higher energy levels to lower. the colours correspond to specific wavelengths and frequencies and tell us the quantities energy that is emitted when transitioning from higher to lower. these quantities of energy emitted is specific to each element and can therefore identify the element.

Question 15

describe how the absorption spectra can be used to identify elements.

Answer 15

absorption lines represents colours that are absorbed by the element when transitioning from ground state to a higher energy level. The colour corresponds to specific wavelengths and frequencies and energy levels. the quantity of the energy absorbed directly match the difference in energy from the lower to higher energy level. each element has unique quantities of energy absorbed when transitioning from lower to higher energy shells and therefore can identify elements