Explain the melting points of period 3 elements.

Going from Na to Si, the melting point increases. This is because from Na-Al, the charge of the metal ion and the number of delocalised electrons increases so the strength of the metallic bonding increases as well. Hence the energy required to break bonds increases. Si exists as macromolecule with strong covalent bonds between the atoms which require a lot of energy to break. From phosphorus to argon, the melting points decrease in order of S8 > P4 > Cl2 > Ar. I will show you on the whiteboard why sulphur has high melting point than phosphorus.  

AK
Answered by Amanpreet K. Chemistry tutor

5230 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

Consider the following reaction: C2H4 + HBr -> ?. a) What is the product of the reaction? Name the compound and give the structural formula. b) What is the type of the reaction? c) Draw a reaction mechanism.


Draw the shape of an SF6 and SF4 molecule, indicating bond angles and any lone pairs which may influence these. What shape is the SF6 molecule?


The reversible reaction 2 SO2 (g) + O2 (g) <-> 2 SO3 (g) has a delta H value of -197 kJ/mol. Use Le Chatelier's principle to explain what conditions would give the highest equilibrium yield and why industry uses different conditions. (5 marks)


What's the difference between an electrophile and a nucleophile?


We're here to help

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

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences