IB SL - Bonding - Strength of Metallic Bonds & m.p. Trends

The greater the ionic charge and the greater the ionic radius, the stronger the metallic bond. True or false?

• False

• True

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

• charge & ionisation energy

• radius and ionisation energy

• charge and radius

• ionisation energy & electronegativity

Identify which of the following shows the correct melting points in ascending order (i.e. from lowest to highest).

• Na < Mg < Al

• Al < Na < Mg

• Al < Mg < Na

• Mg < Na < Al

State which group 1 metal has the strongest metallic bond?

• Li

• Na

• K

• Rb

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

A mixture of two or more metals is called:

• mixture
• solution
• compound
• alloy

Why do group 1 metals exhibit a decrease in melting point going down the group ?

• Metallic radius increases -> charge density decreases -> electrostatic attraction to delocalised electrons increases -> metallic bonding increases

• Metallic radius increases -> charge density decreases -> electrostatic attraction to delocalised electrons increases -> metallic bonding decreases

• Metallic radius decreases -> charge density decreases -> electrostatic attraction to delocalised electrons increases -> metallic bonding increases

• Metallic radius increases -> charge density decreases -> electrostatic attraction to delocalised electrons decreases -> metallic bonding decreases

State which metal has the strongest metallic bond?

• K

• Ca

• Mg

• Cs

Select all the factors that affect the strength of metallic bonding

• Radius of metal

• Number of valence electrons

• Charge density of cation

• Charge of cation

Which sentence best explains why the difference in melting point for transition metals is slight ?

• The transition metals are similar

• Their D electrons are of similar energy

• Their oxidation states are similar

• The number of valence electrons they have is more similar than compared to metals in the s and p blocks