Year 9 Science · Unit 2 · Lesson 10

Metallic Bonding and Bond Types

Foundation Worksheet

Name

Date

Class

Learning Goals

Describe how metallic bonding creates a "sea of delocalised electrons" around positive metal cations.
Identify the key properties of metals (conductivity, malleability, ductility, lustre) and link each to metallic bonding.
Sort substances and properties into ionic, covalent, or metallic categories using lesson knowledge.

Warm Up

Sort it!

Write each item from the pool below into the correct category box. Each item belongs to exactly one bond type.

NaCl high electrical conductivity forms molecules brittle when hit Cu metal H₂O delocalised electrons transfers electrons shares electron pairs malleable high MP lattice low melting point

Ionic

Covalent

Metallic

Your Turn

True or False? Fix the false ones

Circle T or F for each statement. If the statement is false, rewrite it correctly on the line below.

Metals conduct electricity because they have free electrons that flow through the structure.

Correct it:

Metallic bonding involves atoms sharing electrons in pairs, like covalent bonds.

Correct it:

Copper can be drawn into wire because the electron sea allows layers of ions to slide without breaking the bond.

Correct it:

Ionic compounds always have higher melting points than metals.

Correct it:

Metallic bonding only occurs in pure metals, not in alloys.

Correct it:

Show What You Know

1. In the metallic bonding model, what are the two types of particles present in a metal lattice? Describe what each one is.

Recall 2 marks

2. Use the sea-of-electrons model to explain why metals are good conductors of electricity but ionic compounds in solid form are not.

Recall 2 marks

Wrap Up

In one sentence, what was the main idea of this lesson?