Final answer:
Electronegativity increases across a period from left to right in the periodic table due to the increasing number of protons. This general trend is influenced by effective nuclear charge and electron configuration, with certain exceptions. This trend allows us to predict bonding types and physical states in compounds.
Step-by-step explanation:
The general electronegativity trend within a period of the periodic table is that electronegativity increases as we move from left to right. This occurs because the number of protons (positive charges) in the nucleus of the atoms increases, enhancing the atom's ability to attract electrons. Consequently, elements to the right of a period have a greater pull on electrons, which corresponds with higher electronegativity.
Additionally, the trend is influenced by effective nuclear charge and the electron configuration of atoms, with exceptions found in group 2 (2A), group 15 (5A), and group 18 (8A). These instances can be explained by their distinctive electron configurations, disrupting the trend in electronegativity.
Overall, the general electronegativity trend enables us to predict the type of bonding and physical states in compounds, with higher electronegativities indicating stronger bonding capabilities and varying physical states.
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