QuestionMay 5, 2025

Which of the following properties generally decreases from left to right across a period (from potassium to bromine)? (A) Electronegativity (B) Electron affinity (C) Atomic number (D) Atomic radius (E) Maximum value of oxidation number

Which of the following properties generally decreases from left to right across a period (from potassium to bromine)? (A) Electronegativity (B) Electron affinity (C) Atomic number (D) Atomic radius (E) Maximum value of oxidation number
Which of the following properties generally decreases from left to right across a period (from potassium to bromine)? (A) Electronegativity (B) Electron affinity (C) Atomic number (D) Atomic radius (E) Maximum value of oxidation number

Solution
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Answer

(D) Atomic radius Explanation 1. Analyze the periodic trends Across a period in the periodic table (from left to right), several properties exhibit predictable trends: - **Electronegativity** generally increases because atoms have a stronger pull on electrons as their nuclear charge increases. - **Electron affinity** generally becomes more negative (increases) due to the higher attraction for additional electrons. - **Atomic number** always increases since it represents the number of protons in the nucleus. - **Atomic radius** decreases because the increasing nuclear charge pulls the electron cloud closer to the nucleus. - **Maximum oxidation number** generally increases across a period as elements gain more valence electrons, but this trend is not consistent for all periods. 2. Identify the property that decreases From the analysis above, the only property that consistently **decreases** from left to right across a period is the **atomic radius**, as the effective nuclear charge increases and pulls the electrons closer to the nucleus.

Explanation

1. Analyze the periodic trends<br /> Across a period in the periodic table (from left to right), several properties exhibit predictable trends:<br />- **Electronegativity** generally increases because atoms have a stronger pull on electrons as their nuclear charge increases.<br />- **Electron affinity** generally becomes more negative (increases) due to the higher attraction for additional electrons.<br />- **Atomic number** always increases since it represents the number of protons in the nucleus.<br />- **Atomic radius** decreases because the increasing nuclear charge pulls the electron cloud closer to the nucleus.<br />- **Maximum oxidation number** generally increases across a period as elements gain more valence electrons, but this trend is not consistent for all periods.<br /><br />2. Identify the property that decreases<br /> From the analysis above, the only property that consistently **decreases** from left to right across a period is the **atomic radius**, as the effective nuclear charge increases and pulls the electrons closer to the nucleus.
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