2.2 Definitions Flashcards
Electron pair repulsion theory
The shape adopted by a simple molecule or ion is that which keeps repulsive forces to a minimum
Bonding and lone pairs…
OF ELECTRONS!
Non-polar bond
Atoms have equal electronegativity
Polar bond
Different atoms with different electronegativities
When going to the right of the periodic table, nuclear charge…
Increases
When going to the right of the periodic table, electron shielding…
Stays the same
When going to the right of the periodic table, distance from the nucleus…
Decreases
When going up a group in the periodic table, nuclear charge…
Decreases
When going up a group in the period table, electron shielding…
Decreases
When going up a group in the periodic table, distance from the nucleus…
Decreases
2 bonds, 0 lone pairs
Linear, 180°
3 bonds, 0 lone pairs
Trigonal planar, 120°
4 bonds, 0 lone pairs
Tetrahedral, 109.5°
6 bonds, 0 lone pairs
Octahedral, 90°
4 bonds, 1 lone pair
Pyramidal, 107°
4 bonds, 2 lone pairs
Non-linear, 104.5°
London dispersion forces
Weakest, temporary dipole induced dipole interaction, non-polar, simple covalent molecules, more electrons=stronger
Dipole-dipole forces
Permanent dipole interaction, polar molecules
Hydrogen bonds
Strongest, H directly bonded to N, O, or F, causes higher boiling points
Why only N, O, and F?
They have high charge density because their high charges are packed into small sized atoms, making intermolecular attractions greater
