BRAINCAKEBoiling Point of Hydrides
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 instantaneous dipoles inducing dipoles in neighbouring molecules.
- 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.
- Group
- A vertical column of the periodic table, containing elements with the same number of outer-shell electrons.
More in Bonding
- Polar Covalent Bonds
- Dipole-Dipole Forces
- Van der Waals forces
- Hydrogen Bonding
- The Importance of Hydrogen Bonding
- Electron Pair Repulsion Theory
- Two Pairs of Electrons
- Three Pairs of Electrons
All 30 lessons in Bonding · All AQA AS-level Chemistry topics