ELECTRON CONFIGURATION

Question 1

Electronic configuration of Cu

Answer 1

1s2 2s2 2p6 3s2 3p6 4s1 3d10
(fully filled sub-level is stable)

Question 2

Electronic configuration of Cr

Answer 2

1s2 2s2 2p6 3s2 3p6 4s1 3d5
(half-filled is more stable)

Question 3

Distinguish ultraviolet light from visible light in terms of wavelength and energy

Answer 3

UV has a shorter wavelength and a higher energy than visible light

Visible light has a longer wavelength and a lower energy than UV

Question 4

Describe the hydrogen emission spectrum.

Answer 4

A series of lines of specific frequencies that converge at higher energies

Question 5

Analytical chemistry uses instruments to separate, identify and quantify matter. Outline how this spectrum is related to the energy levels in the H atom

Answer 5

1. Electrons transitions between higher energy levels to a lower energy level
2. Electron transitions into the first energy level causes UV series
3. Transitions into second energy level causes visible series
4. Transitions into second energy level causes infrared series

Question 6

Which experimental results support the theory that electrons exists in discrete energy levels?

Answer 6

Emission spectrum

Question 7

Outline the model of electron configuration deduced from the hydrogen line emission spectrum (Bhor’s model)

Answer 7

Electrons are in discrete energy levels and energy levels converge at higher energies/frequencies

Question 8

How is the emission spectrum formed

Answer 8

Photons are emitted when promoted electrons return to a lower energy level

Question 9

Contrast a line spectrum and a continuous spectrum

Answer 9

A line spectrum only shows discrete lines corresponding to specific wavelengths of light.

A continuous spectrum spectrum has no breaks or lines within the continuous bond of wavelengths and shows all wavelengths of light.

Question 10

Energy formula

Answer 10

6.63 x 10^-34 J (Planck constant) x f (frequency)

Question 11

Ionisation energy

Answer 11

Lower to higher energy level

Question 12

Limitations for model of electron energy levels

Answer 12

Does not represent sub-levels/orbitals
Only applies to atoms with one electron/hydrogen

Question 13

Wavelengths, Energy and Frequency relationship

Answer 13

1. Higher frequency, higher energy
2. Higher energy, shorter wavelength
3. longer wavelength, lower energy
4. Low frequency, longer wavelength