1. Explain atomic size, ionization potential, electronegativity and the general

Question

1. Explain atomic size, ionization potential, electronegativity and the general periodic trend for each of these properties. Arrange the following atoms: O, Se, C, Si, F in order of increasing atomic radius, in order of increasing electronegativity and in order of increasing ionization energy. Explain how you developed your list and explain the similarities or differences between the lists.

2.The successive ionization energies for boron are 801, 2430, 3670, 25,000, and 32,800 kJ/mole. Why does boron have a fairly low first ionization energy and why do the values increase with each successive ionization? Why is there a significant jump between the third and fourth value?

Explanation / Answer

1. Atomic size refers to size of atom which depends on no. of shells containing electrons

Electronegativity describes the tendency to accept electrons by a atom in it's valence shell

Ionization energy is the energy required to remove an electron from a neutral atom in its gaseous phase. Conceptually, ionization energy is the opposite of electronegativity.

2) Boron electronic configuration is 1s2 2s2 2px1 2py1 2pz1

boron has a low first ionization energy because it only has 5 protons so there is not as much a pull on the electrons. also it is not at a filled or half-filled sublevel. stability is associated with filled and half-filled sublevels so it is more difficult to remove electrons. ionization energy increases with each successive ionization because of the electrostatic force between the protons and electrons. the positively charged protons pull on the electrons, and as more electrons are removed, the protons gain more of a hold on the electrons making them more difficult to remove.

There is significant jump between third and fourth value becoz when third electron is removed, electron from outermost shell is removed, so not very high. but fourth electron is removed from 2s shell which is much closer to nucleus and therefore needs much more energy to remove electron.

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