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Chapter 9: Problem 33

Define electronegativity, and explain the difference between electronegativity and electron affinity. Describe in general how the electronegativities of the elements change according to position in the periodic table.

Short Answer

Expert verified
Electronegativity refers to an atom's tendency to attract a bonding pair of electrons, while electron affinity is the energy change when an electron is added to a neutral atom. Electronegativity tends to increase across a period (left to right) and decrease down a group or column on the periodic table, as a result of changes in atomic structure and electron configuration.

Step by step solution

01

Definition of Electronegativity

Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. It's a vital concept for understanding the nature of chemical bonds.
02

Comparison of Electronegativity and Electron Affinity

While both electronegativity and electron affinity refer to how eager an atom is to accept electrons, they differ subtly. Electron affinity refers to the energy change that occurs when an electron is added to a neutral atom forming a negative ion, while electronegativity represents an atom's eagerness to attract electrons in a covalent bond.
03

Explaining Electronegativity Trend in the Periodic Table

The electronegativity generally increases from left to right across a period, and decreases down a group. Going across a period, the number of protons (nuclear charge) increases, yet the electrons are held in the similar energy level, leading the electron cloud to be drawn closer to the nucleus and increase the electronegativity. Conversely, going down a group, an extra energy level is added with each new period and the outer electrons are further away from the nucleus, decreasing the electronegativity. But there are exceptions too such as noble gases which have low electronegativity as they already have a full valence shell and are not eager to accept more electrons.

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Most popular questions from this chapter

The following species have been detected in interstellar space: (a) \(\mathrm{CH},(\mathrm{b}) \mathrm{OH},(\mathrm{c}) \mathrm{C}_{2},(\mathrm{~d}) \mathrm{HNC},(\mathrm{e}) \mathrm{HCO} .\) Draw Lewis structures for these species and indicate whether they are diamagnetic or paramagnetic.

Write Lewis structures for the following molecules: (a) ICl, (b) \(\mathrm{PH}_{3}\), (c) \(\mathrm{P}_{4}\) (each \(\mathrm{P}\) is bonded to three other \(\mathrm{P}\) atoms (d) \(\mathrm{H}_{2} \mathrm{~S}\), (e) \(\mathrm{N}_{2} \mathrm{H}_{4}\), (f) \(\mathrm{HClO}_{3}\), (g) \(\mathrm{COBr}_{2}\) (C is bonded to \(\mathrm{O}\) and \(\mathrm{Br}\) atoms).

Explain the concept of formal charge.

Draw a Lewis structure for nitrogen pentoxide \(\left(\mathrm{N}_{2} \mathrm{O}_{5}\right)\) in which each \(\mathrm{N}\) is bonded to three \(\mathrm{O}\) atoms.

Draw Lewis structures for the following organic molecules. In each there is one \(\mathrm{C}=\mathrm{C}\) bond, and the rest of the carbon atoms are joined by \(\mathrm{C}-\mathrm{C}\) bonds. \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{~F}, \mathrm{C}_{3} \mathrm{H}_{6}, \mathrm{C}_{4} \mathrm{H}_{8}\)
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