Electronegativity

In this episode of the 'Chemical Bonding' course, we explore electronegativity, a fundamental concept in chemistry that describes an atom's ability to attract electrons in a bond. Building on previous discussions of ionic, covalent, and metallic bonds, this episode explains how electronegativity influences bond types, molecular polarity, and reactivity. We also discuss how it varies across the periodic table and its role in predicting chemical behavior. This episode lays the groundwork for upcoming topics like bond energy and bond length, deepening your understanding of chemical interactions.

Check your understanding

These are the same multiple-choice questions you will see in the Quiz section after you listen to the episode. Use them here to preview or review the answers.

What does electronegativity measure?

  1. The size of an atom.
  2. An atom's ability to attract shared electrons in a bond.
  3. The energy required to remove an electron from an atom.
  4. The number of valence electrons in an atom.
  5. The stability of an atom's nucleus.
  6. The type of bond an atom forms.

Which element has the highest electronegativity on the Pauling scale?

  1. Hydrogen
  2. Oxygen
  3. Fluorine
  4. Chlorine
  5. Cesium
  6. Nitrogen

How does electronegativity change across a period on the periodic table?

  1. It decreases.
  2. It increases.
  3. It remains constant.
  4. It fluctuates randomly.
  5. It depends on the group number.
  6. It increases, then decreases.

What type of bond forms when two atoms have a large electronegativity difference?

  1. Nonpolar covalent bond
  2. Polar covalent bond
  3. Ionic bond
  4. Metallic bond
  5. Hydrogen bond
  6. Van der Waals force

Which factor decreases electronegativity down a group in the periodic table?

  1. Increasing nuclear charge
  2. Increasing atomic radius
  3. Decreasing electron shielding
  4. Decreasing number of energy levels
  5. Stronger attraction to electrons
  6. Smaller ionic size

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