The anomalous behavior of oxygen can be attributed to its small size and high electronegativity. Let us understand why:
Small Size:
Oxygen is one of the smaller atoms due to its position in the periodic table (it is a second-period element).
The smaller atomic size results in a stronger attraction between the nucleus and the valence electrons, increasing its ability to attract electrons towards itself.
High Electronegativity:
Oxygen is the second most electronegative element after fluorine. This high electronegativity leads to the formation of highly polar covalent bonds.
The high electronegativity is due to the strong pull from the nucleus due to the small atomic radius, making oxygen excel at attracting shared electrons in a chemical bond.
These characteristics distinguish oxygen from other elements in its group, leading to its unique or anomalous behavior. As a result, oxygen is able to form multiple types of oxides and has distinctive reactivity patterns compared to its group counterparts like sulfur, selenium, etc.
Thus, the correct answer is: Small size and high electronegativity.
Options Analysis:
Large size and high electronegativity: Oxygen does not have a large size; hence this option is incorrect.
Small size and low electronegativity: While the size is correct, oxygen exhibits high electronegativity, not low; thus, this option is incorrect.
Large size and low electronegativity: Both characteristics are incorrect for oxygen, making this option incorrect.
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The anomalous behavior of oxygen in the periodic table is attributed to its small atomic size and high electronegativity, which influence its chemical properties distinctively compared to other elements in its group. The Correct Answer is: Small size and high electronegativity
