Shells, levels and orbitals |
1) Line emission spectra's give a unique spectra to each elements. Explain how they arise. Use the following terms in your answer: [4]
Excited Emit Energy Light Frequency absorb Energy level
When electrons absorb energy are excited [1] to a higher energy level [1] when they drop to a lower energy level [1] the emit light [1]
at specific frequencies unique to that element [1] any 4
2) The picture shows part of a spectra for an element.
a) What do you notice about the spectral
lines as you move to the left? [1]
The lines converge / get closer together [1] b) Explain how this spectra has changed the structure of the atom. [1] The electron shells / energy levels get closer as you move away from the nucleus [1] |
3) Sketch an energy level diagram showing the first 3 principle quantum numbers and write on how many electrons each energy level can hold. [4]
The energy levels converge / get closer together [1] n = 1 has 2e [1] n = 2 has 8e [1] n = 3 has 18e [1] |
4) The following question is about atomic orbitals:
a) What is an atomic orbital? [1] A region in space around a nucleus where electrons are likely to be found [1]
b) What is the maximum amount of electrons in an orbital? [1] 2 electrons [1]
c) Sketch a p orbital [1]
[1]
d) How can 2 electrons occupy the same orbital when they both have a negative charge? [1] They spin in opposite directions [1]
e) What can you say about the electron density of an orbital containing 2 electrons rather than 1 electron? [1]
The electron density would be twice as much [1]