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ELECTRONEGATIVITY - Coggle Diagram
ELECTRONEGATIVITY
Definition of Electronegativity
Atom's Ability to Attract Electrons
High Electronegativity: Grabs electrons tightly
Low Electronegativity: Shares electrons more easily
Factors Influencing Electronegativity
Atom's Size
Number of Protons
Trend: Smaller atoms with more protons are more electronegative
Electronegativity
Definition: Magnetism level for atoms
Role in Chemical Bonding: Determines how atoms stick together in molecules
Origin and Introduction
Scientist: Linus Pauling
Year: 1930s
Measurement of Electronegativity
Scale: Pauling Scale
Purpose: Quantifies atom's greed for electrons
Effect on Chemical Bond Type
Large Electronegativity Difference: Ionic or Polar Covalent Bond
Small Electronegativity Difference: Nonpolar Covalent Bond
Electronegativity and Molecular Polarity
Relationship: Hogging of electrons creates partial charge
Result: Molecule becomes polar (partial positive and negative ends)
Examples and Behavior in Reactions
High Electronegativity (e.g., Fluorine)
Behavior: Forms strong bonds, high reactivity
Low Electronegativity (e.g., Cesium)
Behavior: Less reactive due to lower electron-attracting tendency
Periodic Table Trends
Variation: Increases left to right and bottom to top
Significance in Reactivity
Highly Electronegative Elements: More reactive (desire to fill outer shells)