What is the relationship between atomic radius and electronegativity?

Answer 1

Electron affinity is the energy change that occurs when an electron is accepted by an atom in the gaseous state. The electronegativity is a number that describes the relativity ability of an atom, when bonded, to attract electrons.

Answer 2

No they are not, although people constantly confuse them---just talk to your average biologist and ask them why O2 is important to life and most will talk about its high electronegativity contributing to its ability to pick up electrons. Electron affinity refers to the amount of energy released or required when an atom or ion gains an electron. The more energy released, the more favorable it is to add an electron. Electronegativity refers to how well an atom attracts electrons in a covalent bond. It is used to determine polarity of bonds and is a decent indicator of whether two atoms will form ionic or covalent bonds. It is not so surprising that people confuse these two. They sound the same, they both talk about attracting electrons (although in very different ways) and they both depend on the same things---effective nuclear charge (how well an atom attracts electrons given the inner electrons shielding it) and radius (how far the electrons that the nucleus is attracting are from the nucleus). That being said, there are some real differences in the two. Trends for electron affinity are somewhat jagged, as certain electron configurations are better at compensating for the added electron-electron repulsions than others. Electronegativity has a very smooth trend going across the Periodic Table. Also, noble gases have very unfavorable electron affinities---they don't get enough energy out of adding an electron to compensate for creating a new shell. However, Argon, Krypton, and Xenon have some of the highest electronegativities on the periodic table owing to their very high effective nuclear charges.

Answer 3

Electronegativity is the tendency of an atom to attract a bonding pair of electrons.

• No electronegativity difference between two atoms: non-polar covalent bond.

• A small electronegativity difference: polar covalent bond.

• A large electronegativity difference: ionic bond.

Answer 4

Electron Affinity:-It is defined as the energy given out when a neutral gaseous atom takes up an extra electron.

X(g) + e- ----> X-(g) where X is a neutral gaseous atom

Electron affinity is the measure of the tightness with which an atom bonds an electron to itself.

Electronegativity:-It is the measure of the ability of an atom in a combined state(i.e. in a molecule) to attract to itself the electrons in a chemical bond

Answer 5

If the electronegativity difference between the two atoms is above 1.7, then ionic bond is formed and if the difference is below 1.7, then covalent bond is formed.

Answer 6

The higher the electronegativity, the higher the ionization energy is.

Answer 7

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