Metallic Bonding

Metallic Bonding

By Hafiz Bin Mohd Saleh

Multiple Choice

What is the basis of a metallic bond?

• the attraction of neutral metal atoms.
• the attraction between protons and neutrons.
• the attraction between positive metal ions and interlocking electrons.
• the attraction between positive metal ions and free floating electrons.

Multiple Choice

Metallic bonding is...

• a type of covalent bond.
• a type of ionic bond.
• an attraction between positive ions and electrons.

Multiple Choice

In metals, the _______ electrons form a shared sea of electrons.

• Metallic
• Inner
• Outer
• Ionic

Multiple Choice

What does malleable mean?

• able to be shaped
• will break easily
• can be used for wire
• is shiny

Multiple Choice

What is the ability of a substance to be pulled into a thin strand?

• Malleability
• Ductility 
• Conductivity
• Solubility

Multiple Choice

What is the ability of a substance to allow heat, sound, or electricity to flow through it?

• Malleability
• Ductility
• Solubility
• Conductivity

Multiple Choice

Why do metals conduct

• They are shiny
• The electrons are held tightly within the lattice
• The electrons are delocalised and able to move
• The electrons are shared between two metal ions

Multiple Choice

Why do metallic compounds conduct electricity as solids?

• core electrons are mobile, allowing electricity to flow through the metal

• valence electrons are mobile, allowing electricity to flow through the metal

• protons are mobile, allowing electricity to flow through the metal

• the metal cations are mobile, allowing electricity to flow through the metal

Multiple Choice

Why are metals malleable? (They can bend without breaking.)

• Metals are very smooth.

• Metals have a sea of electrons.

• The sea of electrons form a strong metallic bond.

• Even though the metal ions repel each other, the electron sea holds all the atoms in place.

Multiple Choice

Why do metals have high melting points?

• The cations are weakly attracted to the sea of delocalised electrons

• Strong electrostatic forces of attraction between the electrons and cations

• All the electrons become delocalised and repel the metal body

Multiple Choice

Why are metals ductile?

• They are shiny

• The electrons are held tightly within the lattice structure making it strong

• The electrons are delocalised and are able to roll over each other into new positions without breaking the metallic bond.

• The electrons are shared between two metal ions and this holds the atoms together

Multiple Choice

The strength of the metallic bond depends on the _______ and the _______ of the metal cation.

• charge & ionisation energy

• radius and ionisation energy

• valency and charge

• ionisation energy & electronegativity

Multiple Choice

How many electrons are delocalised in a metal?

• 1

• 2

• as many as are in the valence shell

• as many as are in the first energy level

Multiple Select

What are some benefits of alloys? (choose all that apply)

• they can be stronger than pure metal

• they may not rust/corrode as easily

• they don't have electrons

• they form covalent bonds

Multiple Choice

Why are alloys generally used to make everyday objects?

• Alloys are often stronger and less active than pure metals.
• Alloys have higher melting point than pure metals.
• Alloys are less expensive to produce than pure metals.
• Alloys have ionic bonds instead of metallic bonds.

Multiple Choice

An alloy is harder than its pure metal because the foreign atoms in the alloy

• increase the bond strength between the atoms.

• increase the empty spaces between the atoms.

• react with the pure metal atoms to form a compound.

• reduce the ability of the atoms to slide across each other.