1. How do the delocalised electrons in metallic bonding effect the melting point?
- They make the bonding between atoms weaker
- The more electrons there are, the stronger the bonding will be and the higher the meling point because the positive metal ions will have more electrons to be attracted to
- They make the melting point lower because it stops the positive ions being attracted togther
- Because the shared pair of electrons create a strong intermolecular force
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Other questions in this quiz
2. What affects ionisation energy?
- distance from the nucleus, shielding and intermolecular forces
- nuclear charge, distance from nucleus and sheilding
- the shape and size of an atom
- only nuclear charge
3. What charge does the Sulfate SO4 ion carry?
4. What is dative covalent bonding?
- When there are less than 8 electrons in outer shell
- When atoms share more than one pair of electron e.g. in N2
- When both electrons come from one atom
- When there are more than 8 electrons in outer shell
5. What is ionic bonding?
- the intermolecular forces between induced dipoles
- the intermolecular forces caused by an electronegative N,F,O, a lone pair and a hydrogen
- an electrostatic attraction between two oppositely charged ions
- an electrostatic attraction between two ions with the same charge