2.2 Electron configuration

Question 1

Electromagnetic spectrum

Answer 1

ELectromagnetic radiation varies in energy - different wavelengths

Question 2

Continuous spectrum

Answer 2

Continuous spectrum: an emission spectrum which contains all wavelengths

Question 3

Line spectrum

Answer 3

Line spectrum: an emission specturm consisting of separate lines

Question 4

Absorption spectrum

Answer 4

Absorption scpectrum: a spectrum of electromagnetic radiation transmitted through a substance, showing dark lines/bands due to absorption at specific wavelengths

Question 5

Bohr model of hydrogen

Answer 5

He proposed: when e absorbs E - e moves into higher E level further from the nucleus - excited state

When E is given out (electromag radiation) - e falls into lowest E level - ground state - for each e transition a photon is released (line spectrum)

In H - e fall to 2nd level (n=2) which is ground state - emit visible light; if to first (n=1) - higher E - ultraviolet; when falls to third (n=3+) - infrared

• • Oversimplification of atom strcuture - did not explain when more than one e acts in spectrum*
• • e trajectory cannot be simply described (uncertainty principle) - probability where it likely could be*

Question 6

Ionisation of an atom

Answer 6

When an electron is at the higher E level (n=∞) - no longer in the atom - ionisation

E needed to remove the e - ionisation E

Also supports Bohr’s model of H atom

Question 7

Principles used for orbital diagrams

Answer 7

1. Aufbau:
2. Hund’s 3rd rule:

Question 8

Atomic orbitals

Answer 8

ATOMIC ORBITALS: region around the atomic nucleus where it’s 90% chance to find the e

Different types of orbitals: s, p, d, f