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What is a metallic bond?
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What is a metallic bond?
A metallic bond is the electrostatic attraction between a lattice of cations and delocalised electrons.
What are delocalised electrons?
Delocalised electrons are free-moving electrons in a metal lattice that are not bound to their atom.
Define malleability.
Malleability is the ability of a material to be hammered into shape.
Why do metals have high melting and boiling points?
Metals have high melting and boiling points due to the strong electrostatic forces of attraction between the cations and delocalised electrons in the metallic lattice. These forces need lots of energy to overcome.
What causes metals to be good thermal conductors?
Metals are good thermal conductors because when they are heated the positive ions vibrate and transfer kinetic energy to neighbouring ions and electrons.
What property of copper makes it suitable for electrical wiring?
Copper is used in electrical wiring because it is a good electrical conductor and malleable/ductile.
Why are metals malleable?
Metals are malleable because the positive metal ions are arranged in layers which can slide over each other when force is applied.
Why can metals conduct electricity?
Metals can conduct electricity because the delocalised electrons can move through the structure and carry a charge.
Why is aluminium used in food cans?
Aluminium is used in food cans because it is non-toxic and resistant to corrosion and acidic food stuffs.
True or False?
The strength of metallic bonds decreases as the number of outer electrons increases across a Period.
False.
The strength of metallic bonds increases as the number of outer electrons increases across a Period.
True or False?
Metallic compounds are brittle.
False.
Metallic compounds are malleable.
Give two factors that affect the strength of a metallic bond.
Two factors that affect the strength of a metallic bond are:
The charge on the metal ion
The radius of the metal ion.
True or False?
A greater charge difference between metal ions and electrons leads to a weaker metallic bond.
False.
A greater charge difference between metal ions and electrons leads to a stronger metallic bond.
How does the melting point of metals change across a period in the Periodic Table?
The melting point of metals increases moving across a period, from left to right.
How does the melting point of metals change down a group in the Periodic Table?
The melting point of metals decreases moving down a group.
Why does the strength of metallic bonding generally increase across a period?
The strength of metallic bonding generally increases across a period due to an increase in the number of delocalised electrons per atom and a decrease in atomic radius.
Why does the strength of metallic bonding decrease going down Group 1?
The strength of metallic bonding decreases going down Group 1 because:
Going down the group the size of the metal ion increases
There is a less attraction between the outer electrons and positive nucleus
Less energy is needed to overcome this weaker attraction.
What is a transition metal?
A transition metal is an element with an incomplete d-subshell or an element that can form at least one stable cation with an incomplete d-subshell.
Where are transition metals located on the Periodic Table?
Transition metals are located in the d-block of the Periodic Table.
True or False?
Scandium and zinc are considered transition metals.
False.
Scandium and zinc are not considered transition metals because they do not have an incomplete d-subshell as an element or ion.
Why do transition metals have high melting points?
Transition metals have high melting points because:
They can delocalise their d-electrons
So, there are strong electrostatic forces of attraction between the positive cations and the negative electrons
High amounts of energy is needed to overcome these forces
What causes transition metals to have high electrical conductivity?
Transition metals have high electrical conductivity because they have a large number of delocalised electrons that can move and carry a charge.
True or False?
Transition metals generally have lower melting points than s-block metals.
False.
Transition metals generally have higher melting points than s-block metals due to their ability to delocalise d-electrons.