Bond Angles And Shapes In Chemistry

BOND ANGLES AND SHAPES lt;/b>

Any shape with four areas of electron density (a lone pair of electrons, or a bonded pair of electrons) will begin with an angle of 109.5, every lone pair that is present removed 2.5 degrees from the angle as lone pairs repel more than bonded pairs of electrons on the central atom. All other shapes and starting angles are:

120= 3 areas of electron density, no lone pairs, TRIGONAL PLANAR.

109.5= 4 areas of electron density, no lone pairs, TETRAHDERAL.

90= 6 areas of electron density, no lone pairs, OCTAHEDRAL.

90 and 120= 5 areas of electron density, no lone pairs, TRIGONAL BYPYRAMIDAL

180= 2 areas of electron density, no lone pairs, LINEAR.

107.5= 4 areas of electron density, one lone pair, PYRAMIDAL.

104= 4 areas of electron density, two lone pairs, NON-LINEAR.