For each of the following pairs of elements, identify which...

For each of the following pairs of elements, identify which element would be expected to be more electronegative. It should not be necessary to look at a table of actual electronegativity values.
a. Be or Ba
b. $\mathrm{N}$ or $\mathrm{P}$
c. F or Cl

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Key Concepts

Atomic Radius

Atomic radius is a measure of the size of an atom, usually influenced by the number of electron shells. A larger atomic radius, which is common when moving down a group, generally results in a lower electronegativity because the outer electrons are further from the nucleus and less strongly attracted.

Electronegativity

Electronegativity refers to the tendency of an atom to attract electrons in a chemical bond. It is a fundamental property that influences how electrons are distributed in molecules, affecting bond polarity and molecular reactivity.

Periodic Trends

Periodic trends provide insights into how properties like electronegativity change across the periodic table. Typically, electronegativity increases moving from left to right across a period due to increasing effective nuclear charge, and it decreases moving down a group because of the increasing distance between the nucleus and the bonding electrons.

Effective Nuclear Charge

Effective nuclear charge is the net positive charge experienced by an electron in an atom, taking into account the shielding effect of inner electrons. A higher effective nuclear charge generally holds electrons more tightly and is a key factor in increasing an atom's electronegativity.

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