Intermolecular forces, electronegativity and bond properties
Cambridge A-Level Chemistry (9701) · Unit 3: Chemical bonding · 6 flashcards
Intermolecular forces, electronegativity and bond properties is topic 3.6 in the Cambridge A-Level Chemistry (9701) syllabus , positioned in Unit 3 — Chemical bonding , alongside Electronegativity and bonding, Ionic bonding and Metallic bonding. In one line: Electronegativity is the measure of the ability of an atom in a chemical compound to attract electrons in a covalent bond. The Pauling scale is commonly used, with fluorine being the most electronegative element.
Marked as AS Level: examined at AS Level in Paper 1 (Multiple Choice), Paper 2 (AS Structured Questions) and Paper 3 (Advanced Practical Skills). The same content may also be assumed in Paper 4 (A Level Structured Questions).
The deck below contains 6 flashcards — 4 definitions and 2 key concepts — covering the precise wording mark schemes reward. Use the 4 definition cards to lock down command-word answers (define, state), then move on to the concept and calculation cards to handle explain, describe, calculate and compare questions.
Electronegativity
Electronegativity is the measure of the ability of an atom in a chemical compound to attract electrons in a covalent bond. The Pauling scale is commonly used, with fluorine being the most electronegative element.
What the Cambridge 9701 syllabus says
Official 2025-2027 spec · AS LevelThese are the exact learning outcomes Cambridge sets for this topic. The candidate is expected to be able to do each of these on the relevant paper.
- use the concept of electronegativity to explain bond polarity and dipole moments of molecules
- state that, in general, ionic, covalent and metallic bonding are stronger than intermolecular forces
Cambridge syllabus keywords to use in your answers
These are the official Cambridge 9701 terms tagged to this section. Mark schemes credit responses that use the exact term — weave them into your answers verbatim rather than paraphrasing.
Tips to avoid common mistakes in Intermolecular forces, electronegativity and bond properties
- › Only use 'intermolecular' when referring to simple molecules; use 'electrostatic attraction' for ionic, metallic, or giant covalent lattice forces.
- › Describe hybridisation as the mixing of atomic orbitals of similar energies to form a new set of equivalent hybrid orbitals.
- › Remember that a water molecule can form four hydrogen bonds: two through its lone pairs and two through its hydrogen atoms.
- › Count all single bonds and one bond from every double/triple bond as sigma bonds; ensure every C-H bond is included.
- › Recall that an octahedral structure has both 90 and 180 degree bond angles; visualize trans atoms to identify the 180 degree angles.
Define electronegativity.
Electronegativity is the measure of the ability of an atom in a chemical compound to attract electrons in a covalent bond. The Pauling scale is commonly used, with fluorine being the most electronegative element.
Explain how electronegativity differences lead to bond polarity.
When there's a significant electronegativity difference between two bonded atoms, the more electronegative atom attracts electron density, resulting in a partial negative charge (δ-) and the other atom a partial positive charge (δ+). This creates a polar covalent bond.
What is a dipole moment?
A dipole moment is a measure of the polarity of a molecule. It arises when there is an uneven distribution of electron density, creating a separation of charge. It's a vector quantity with both magnitude and direction.
How can a molecule with polar bonds be nonpolar overall?
If the individual bond dipoles within a molecule cancel each other out due to the molecule's symmetry, the overall dipole moment is zero, and the molecule is nonpolar. CO₂ is an example, despite having polar C=O bonds.
List the relative strengths of ionic, covalent, metallic bonding, and intermolecular forces.
Ionic, covalent and metallic bonds are stronger than intermolecular forces. The relative order is generally: Ionic > Metallic > Covalent >> Intermolecular forces.
Give examples of compounds with each of the following: ionic, covalent, and metallic bonding.
Ionic: NaCl (sodium chloride). Covalent: CH₄ (methane). Metallic: Fe (iron).
More Chemistry flashcards
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All Chemistry FlashcardsMore topics in Unit 3 — Chemical bonding
Intermolecular forces, electronegativity and bond properties sits alongside these A-Level Chemistry decks in the same syllabus unit. Each uses the same spaced-repetition system, so progress in one informs the next.
Key terms covered in this Intermolecular forces, electronegativity and bond properties deck
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