Lesson 3.1.3.3
3.1.3.3 Metallic bonding Quiz: AQA Chemistry, Unit 1
20 questions
In partnership with Revision Ninja
Lesson 3.1.3.3, Metallic bonding: 20 multiple choice questions for the AQA Chemistry (7405), Unit 1: Physical chemistry, written with Revision Ninja.
Host it live on the board and students join with a game code on their own devices, or revise alone with Free Play. The answers are revealed in the game.
The 20 questions
-
Which particles are electrostatically attracted in a metallic bond?
- Protons and electrons
- Anions and cations
- Cations and electrons
- Nuclei and pairs
-
Which particles move through a metal lattice to conduct electricity?
- Delocalised electrons
- Protons and neutrons
- Shared electron pairs
- Positive metal ions
-
Where are delocalised electrons free to move in a metal?
- Between specific pairs
- Within single bonds
- Throughout the lattice
- Around one nucleus
-
Why can layers of ions in a metal slide without shattering?
- Rigid ionic lattice
- Directional covalent bonds
- Non-directional bonding
- Fixed shared pairs
-
Which metal in Period 3 has the most delocalised electrons per atom?
- Magnesium
- Aluminium
- Potassium
- Sodium
-
What force gives metals their high melting points?
- Strong electrostatic attraction
- Repulsive magnetic force
- Weak intermolecular force
- Directional covalent bond
-
Which particles form the fixed regular lattice in a metal?
- Delocalised electron pairs
- Negative non-metal ions
- Positive metal ions
- Neutral molecules
-
Why does magnesium have a higher melting point than sodium?
- Lower ion charge
- Weaker electrostatic force
- More delocalised electrons
- Larger ionic radius
-
Which property of solid metals is caused by delocalised electrons?
- Low melting point
- Extreme brittleness
- High density
- Electrical conductivity
-
Which cations are present in the metallic lattice of calcium?
- Ca+ ions
- Ca- ions
- Ca3+ ions
- Ca2+ ions
-
How many delocalised electrons does one atom of magnesium contribute to the metallic lattice?
- 1
- 0
- 2
- 3
-
How does metallic bonding differ from covalent bonding?
- Electrons are delocalised
- Electrons are transferred
- Electrons are lost
- Electrons are fixed
-
How do delocalised electrons transfer thermal energy through metals?
- By photon emission
- By kinetic energy
- By mass transport
- By nuclear decay
-
How many delocalised electrons does each atom of a Group 1 metal contribute?
- Two
- Three
- None
- One
-
Why are alloys usually harder than pure metals?
- Weaker metallic bonds
- Distorted ion layers
- Smaller overall lattice
- Fewer delocalised electrons
-
Why do Group 1 metals have lower melting points than Group 2 metals?
- Smaller ionic radius
- Higher atomic mass
- Lower cation charge
- More delocalised electrons
-
Comparing two metals with equal ionic charge, which has stronger metallic bonding?
- Equal ionic radii
- Smaller positive ions
- Uncharged atoms
- Larger positive ions
-
Why does electrical conductivity in a metal decrease as temperature increases?
- Bonds are broken
- Ions vibrate more
- Electrons are lost
- Ions move faster
-
How many moles of delocalised electrons are present in 1 mol of aluminium?
- 27 mol
- 1 mol
- 3 mol
- 2 mol
-
Why do metals usually have a high mass density?
- Delocalised protons
- Large atomic radii
- Closely packed lattice
- Weak metallic bonds
Related quizzes
- Fundamental particles Quiz · 3.1.1.1 · 20 questions
- Mass number and isotopes Quiz · 3.1.1.2 · 20 questions
- Electron configuration Quiz · 3.1.1.3 · 20 questions
- Relative atomic mass and relative molecular mass Quiz · 3.1.2.1 · 20 questions
- The mole and the Avogadro constant Quiz · 3.1.2.2 · 20 questions
- The ideal gas equation Quiz · 3.1.2.3 · 20 questions
- Empirical and molecular formula Quiz · 3.1.2.4 · 20 questions
- Balanced equations and associated calculations Quiz · 3.1.2.5 · 20 questions
- Ionic bonding Quiz · 3.1.3.1 · 20 questions
- Nature of covalent and dative covalent bonds Quiz · 3.1.3.2 · 20 questions