Ionisation energies and shells

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 2 electrons are likely to be found [1]

          b)    What is the maximum amount of electrons in an orbital? [1]  2 electrons [1]

          c)    How can 2 electrons occupy the same orbital when they both have a negative charge? [1]  They spin in opposite directions [1]

          d)    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]