Why do melting points decrease down the group 1 and increade down the group 7? (core syllabus: Periodicity)

Elements in the group one (i.e. alkali metals from lithium to francium) exhibit metallic bonding: the positive nuclei are held together thanks to the attraction to delocalised electrons. As the number of electron shells increases down the group, and consequently the atomic radii get bigger, the attraction between the nuclei and outer shell (valence) electrons decreases. Hence, the bonds are weaker and less energy is required to break them.

Elements in the group seven (i.e. the halides form fluorine to iodine) normally form diatomic covalently bound molecules. The only type of interaction between them are the London dispersion forces (momentary dipole interactions). The magnitude of London forces is proportional to the mass of the molecules, so as the molecular weights of the halides increase down the group, more energy is required to break the interactions between them.

PM
Answered by Paulina M. Chemistry tutor

73800 Views

See similar Chemistry IB tutors

Related Chemistry IB answers

All answers ▸

What is the charge of iron in the following complex: [Fe(H2O)6]Cl2 ?


What is the name of the compound with the formula CH3CH2CH(OH)CH3, and what is the name of its functional group?


How can we determine the molecular and electron geometry of H2O?


Describe how σ and π bonds form.


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