Two questions about bond polarity, anyone could help?

boiling points of discrete molecules depend on intermolecular forces between molecules. hbr , hcl both polar molecules, net dipole moment greater hcl, yet hbr has greater boiling point. due greater london dispersion forces, ldf. molecules, if other forms of intermolecular forces present, exhibit ldf's. strength of ldf's depend on polarizability of molecule, in turn depends on total number of electrons , area on spread. hbr has more electrons, has greater polarizabiltiy, , greater london dispersion forces, , greater boiling point.

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boiling point of 1-chlorohexane 135c
boiling point of 1-bromohexane 154c
1 bromohexane has greater boiling point, predict based on london dispersion forces.

silicon dioxide solid not exist in discrete molecules, co2, may comparing to. sio2 network solid each si atom covalently bonded 4 adjoining oxygen atoms form continuous lattice of si , o atoms. entire crystal of sio2 (quartz, when formed in nature) 1 giant macromolecule.

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unfortunately, john confused. there no hydrogen-bonding in of these compounds, not in hcl, hbr, 1-chlorohexane, or 1-bromohexane. hydrogen bonding intermolecular bond h 1 molecule bonded n, o or f, weakly covalently bonded n, o or f in adjacent molecule.

grief!!! 1234 out lunch, too. why these otherwise nice folks think there hydrogen bonding? also, ldf's not depend on mass, on number of electrons.

1. know hbr has higher boiling point hcl has larger molecular size.
when determine boiling points of 1-bromohexane , 1-chlorohexane, 1-bromohexane has lower boiling point. why?

2. , silicon dioxide contain single bonds rather double bonds?

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