Describe the difference in melting points for the elements Sodium and Magnesium

With these sort of questions, it's important to firstly think about what type of bonds make up the structure of the element. For this example, they both have metallic bonds which hold the structures together. Now we have to think about which what metallic bonds are and which element has the stronger bonds which will ultimately determine the melting point.
Metallic bonds can be defined as the attraction between positive metal cations and the delocalised electrons which flow through its structure. Sodium will delocalise 1 electron per atom (Na+) and Magnesium will delocalise 2 electrons per atom (Mg2+). Because magnesium has a greater charge, there will be greater attraction between delocalised electrons and the positively charged ions and so more energy will be needed to overcome this attraction. Magnesium will have a higher melting point than sodium.

Answered by Myles S. Chemistry tutor

12067 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

a sample of hydrated NiSO4 witha mass of 4.414g is heated to remove all water crystallisation. The resultant mass is 2.287g. How many H2O molecules to each NiSO4 were there in the original sample


In terms of Electrostatic Forces, Suggest why the ‘Electron Affinity’ of Fluorine has a Negative value.


How to answer the question: How does a bicarbonate buffer solution control pH when either an acid or a base is added?


Explain why the second ionisation energy of boron is higher than the first ionisation energy of boron?


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo
Cookie Preferences