1. How do the delocalised electrons in metallic bonding effect the melting point?
- They make the bonding between atoms weaker
- Because the shared pair of electrons create a strong intermolecular force
- 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
1 of 10
Other questions in this quiz
2. What are three characteristics that ionic compounds have (when in a giant ionic structure)?
- always conducts electricity, low boiling point, cannot dissolve in water
- conduct electricity when molten or dissolved, have high boiling points, dissolve in water
- dissolve in water, low boiling point, can not conduct electricity
- high boiling point, always conducts electricity and cannot dissolve in water
3. What is the definition of the first ionisation energy?
- the energy needed to remove 1 electron from each atom in 1 mole of gaseous atoms to form one mole of gaseous 1+ ions.
- the energy needed to remove 1 electron from each ion in 1 mole of gaseous 1+ ions to form one mole of gaseous 2+ ions.
- a high attraction between the electron and the nucleus
- the ability to remove all the electrons from the outer shell in an exothermic process
4. What charge does the Sulfate SO4 ion carry?
5. What is a covalent bond?
- 1 shared electron
- the electrostatic attraction between ions with the same charge
- a shared pair of electrons
- the electrostatic attraction between two oppositely charged ions