BRAINCAKEBoiling Points of Hydrides and Intermolecular forces
The boiling points of hydrides generally increase across a period from groups 4 to 7. Group 4 hydrides are tetrahedral, non-polar covalent molecules such as methane. From group 5 to 7 the electronegativity increases and the molecules become more polar.
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Key terms in this lesson
- Electronegativity
- The attraction of a bonded atom for the pair of electrons in a covalent bond, measured on the Pauling scale.
- Dipole
- A separation of opposite partial charges caused by an uneven distribution of the bonding electron pair.
- London forces
- Weak intermolecular forces caused by an instantaneous dipole inducing a dipole in a neighbouring molecule.
- Hydrogen bond
- A strong permanent dipole-dipole interaction between a hydrogen atom bonded to N, O or F and a lone pair on an electronegative N, O or F atom of another molecule.
- Periodicity
- The repeating trend in the properties of elements across each period of the periodic table.
More in Shapes and Intermolecular Forces
- More examples.
- Electronegativity
- Bond Polarity
- Polar Solvents and Solubility
- Induced Dipole-Dipole Interactions (London Forces)
- Permanent dipole-dipole interactions
- Solubility of Simple Molecules
- Hydrogen Bonds
All 13 lessons in Shapes and Intermolecular Forces · All OCR AS-level Chemistry topics