Electronic Structure and I.E.

Electronic Structure and I.E.

1. Electronic Structure

   • Orbitals
     • There are different kinds of orbitals. The S, P, D and F. The S orbital forms a spherical shape surrounding the nucleus. The P orbital forms a shape like weights around the nucleus. Each orbital can hold a maximum of 2 electrons. However, there are more than one of each orbital in each shell. These are known as sub shells.
   • Sub-shells
     • A sub shell is a subdivision of a shell. They are labelled S, P, D and F. There is 1S orbitals in a subshell, 3P and 5D
   • Shells
     • The first shell contains the 1S subshell, the second 2S and 2P and the third the 3S 3P and 3D. Shells or energy levels hold different numbers of electrons. Shell 1 holds 2, shell 2 hold 8, shell 3 holds 18.

2. Ionisation energy.

   • Defecnitions
     • First ionisation energy: The energy required to remove one electron from each ion in one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions.
     • Second ionisation energy: The energy required to remove one electron from each ion in one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions.
     • Successive ionisation energy: A measure of the energy required to remove each electron in turn.
   • Factors affecting first ionisation energy:
     • The charge of the nucleus
     • Distance of electrons from nucleus
     • Number of shells between nucleus and electron
     • Across a period first ionisation energy generally increases.

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