QQuestionChemistry
QuestionChemistry
How does electronegativity change going down and across the periodic table?
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Step 1:I'll explain how electronegativity changes across the periodic table systematically:
Step 2:: Understanding Electronegativity
Electronegativity is the ability of an atom to attract electrons in a chemical bond. It was first defined by Linus Pauling and varies systematically across the periodic table.
Step 3:: Trends Across a Period (Left to Right)
\text{Electronegativity Trend: } \leftarrow \text{Increasing}
As you move from left to right across a period: - Electronegativity generally increases - Atomic radius decreases - Nuclear charge increases - Valence electrons are pulled more tightly
Step 4:: Trends Down a Group (Top to Bottom)
\text{Electronegativity Trend: } \downarrow \text{Decreasing}
As you move down a group: - Electronegativity decreases - Atomic radius increases - Valence electrons are further from the nucleus - Shielding effect increases
Step 5:: Specific Observations
- Most electronegative element: Fluorine ($$F$$)
- Least electronegative elements: Francium (Fr) and Cesium (Cs)
Final Answer
Electronegativity increases from left to right across a period and decreases from top to bottom down a group of the periodic table.
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