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Worksheets4.5 Metallic bonding
Total questions: 20
Worksheet time: 11mins
Why does the melting point of metals increase across period 3, from Sodium (Na) to Aluminium (AI)?
Size of atoms gets smaller
Attraction force between nuclei and free electron increases
Increased space between the valence electrons in the "sea"
Increased number of valence electrons contributed to the "sea"
Metals have positive ions in a ‘sea of electrons’. Which metal atom provides the most electrons for the sea?
Aluminium
Sodium
Calcium
Magnesium
Which statement describes metallic bonding?
The attraction between a lattice of negative ions and delocalised protons.
The attraction between a lattice of positive ions and delocalised electrons.
The attraction between delocalised protons and electrons.
The attraction between oppositely charged ions.
The diagram shows metallic bonding.
Which labels are correct?
X: atomic nucleus
Y: outer electron
X: metal atom
Y: mobile electron
X: metal cation
Y: mobile electron
X: positive ion
Y: negative ion
Metals are malleable. Which statement explains why metals are malleable?
Metallic bonding is very strong.
Metals are good conductors of electricity.
Positive metal ions are arranged in a regular lattice structure
The layers of positive metal ions can slide over each other.
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
Which of these describes the arrangement of particles in a metal?
Closely packed electrons with delocalised ions
Alternating layers of metal ions and electrons
Layers of metal ions surrounded by delocalised electrons
What does a metallic bond consist of?
Forces between metal ions and delocalised electrons
Pairs of metal atoms joined together by strong bonds
Forces between oppositely charged metal ions
Why are metals ductile?
Because the metal is arranged in layers
Because the metal ions are closely packed
Because the metal can conduct electricity
Why do metals conduct electricity?
They have free-moving atoms
They have free-moving ions
They have free-moving electrons
Why do metals have high melting points?
Metallic bonds are weak and metals have a simple structure
Metallic bonds are strong and metals have a lattice structure
Metallic bonds are strong and metals have a simple structure
What does 'malleable' mean?
Able to be drawn into wires
Able to conduct electricity
Able to be hammered into thin sheets
