Metallic bonding
Cambridge A-Level Chemistry (9701) · Unit 3: Chemical bonding · 9 flashcards
Metallic bonding is topic 3.3 in the Cambridge A-Level Chemistry (9701) syllabus , positioned in Unit 3 — Chemical bonding , alongside Electronegativity and bonding, Ionic bonding and Shapes of molecules. In one line: Metallic bonding is the electrostatic attraction between positive metal ions and delocalised electrons. These delocalised electrons are free to move throughout the metallic lattice, contributing to the metal's conductivity.
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 9 flashcards — 3 definitions and 6 key concepts — covering the precise wording mark schemes reward. Use the 3 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.
Metallic bonding
Metallic bonding is the electrostatic attraction between positive metal ions and delocalised electrons. These delocalised electrons are free to move throughout the metallic lattice, contributing to the metal's conductivity.
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.
- define metallic bonding as the electrostatic attraction between positive metal ions and delocalised electrons 3.4 Covalent bonding and coordinate (dative covalent) bonding Learning outcomes
- define covalent bonding as electrostatic attraction between the nuclei of two atoms and a shared pair of electrons (a) describe covalent bonding in molecules including: • hydrogen, H2 • oxygen, O2 • nitrogen, N2 • chlorine, Cl 2 • hydrogen chloride, HCl • carbon dioxide, CO2 • ammonia, NH3 • methane, CH4 • ethane, C2H6 • ethene, C2H4 (b) understand that elements in period 3 can expand their octet including in the compounds sulfur dioxide, SO2, phosphorus pentachloride, PCl 5 , and sulfur hexafluoride, SF6 (c) describe coordinate (dative covalent) bonding, including in the reaction between ammonia and hydrogen chloride gases to form the ammonium ion, NH4 + , and in the Al 2Cl 6 molecule
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 Metallic bonding
- › 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 metallic bonding.
Metallic bonding is the electrostatic attraction between positive metal ions and delocalised electrons. These delocalised electrons are free to move throughout the metallic lattice, contributing to the metal's conductivity.
Describe the structure of a typical metallic lattice.
A metallic lattice consists of a regular arrangement of positive metal ions surrounded by a 'sea' of delocalised electrons. These electrons are not associated with any single atom.
How does the charge and radius of a metal ion affect the strength of metallic bonding?
Higher charge density (higher charge and/or smaller ionic radius) leads to stronger electrostatic attraction between the metal ions and delocalised electrons, thus stronger metallic bonding.
Define covalent bonding.
Covalent bonding is the electrostatic attraction between the nuclei of two atoms and a shared pair of electrons. These shared electrons are attracted to both positive nuclei, holding the atoms together.
Draw a dot-and-cross diagram to show the covalent bonding in a molecule of oxygen, O2.
O2 contains a double covalent bond with each oxygen atom sharing two electrons, so that each oxygen atom achieves a stable octet of electrons in its outer shell.
Explain how elements in Period 3 can expand their octet.
Period 3 elements, such as sulfur and phosphorus, can expand their octet because they have available d-orbitals that can accommodate additional electrons, allowing them to form more than four covalent bonds. Examples include SF6 and PCl5.
Define coordinate (dative covalent) bonding.
Coordinate bonding occurs when one atom provides both electrons for the shared pair in the covalent bond. The resulting bond is essentially the same as a normal covalent bond, but its formation differs.
Describe the formation of the ammonium ion (NH4+) using a coordinate bond.
Ammonia (NH3) donates its lone pair of electrons to a proton (H+) to form NH4+. The bond between the nitrogen and the newly attached hydrogen is a coordinate bond, as both electrons originate from the nitrogen atom.
Describe the bonding in aluminium chloride dimer (Al2Cl6).
Aluminium chloride exists as a dimer (Al2Cl6) where each aluminium atom forms coordinate bonds with chlorine atoms on the other AlCl3 unit to achieve a more stable electron configuration. Thus each Aluminum has 4 bonds.
More Chemistry flashcards
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All Chemistry FlashcardsMore topics in Unit 3 — Chemical bonding
Metallic bonding 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 Metallic bonding deck
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