![]() However, if there are lone pairs on a linear shape, I just memorize it is always 180 degrees. If a molecular geometry shape has lone pairs, the bond angle will have a less than sign since the lone pairs push down on the terminal atoms, decreasing the bond angle. For the 6th row, I memorize that all of them have 90 degree angles. For the 5th row, I memorize that the first two have 120 degree and 90 degree angles, but then a T shape has 90 degree angles (based on its shape). If there are three, then it is 120 degrees. This is the chart I use as well! For me, I memorize how many electron densities (number of terminal atoms + number of lone pairs). And as previously mentioned, linear is always 180 degrees, so a geometry with 6 electron domains and 4 lone pairs is 180 degrees. If you are having trouble with the last row, notice that the angles are 90 degrees, < 90 degrees, 90 degrees, and <90 degrees respectively. The way I committed these to memory was by remembering that linear always equates to 180 degrees and that T-shape always equates to <90 degrees. Thus we can say hybridization of H3O+ is Sp3. As this is a cationic molecule thus, C 1. 3 hydrogen atoms are bonded to oxygen, so the number of the monovalent atoms (M) 3. ![]() ![]() The discrepancies to this pattern lie toward the bottom of the table which contains molecules of 5 or 6 domains with 2 to 4 lone pairs. In hydronium ion, the central atom is oxygen and it has 6 valence electrons. For a VSEPR model with four electron domains, you simply need to know that 2 lone pairs require an extra (<<) symbol, which makes sense because the more electrons there are, the greater distortion of the bond angle. Every bond angle value listed under 1 lone pair is always denoted as less than (<) the values listed in the basic geometries from which they were derived. As you can see below, the basic geometries (0 lone pairs) of each model all have solid values of 180 degrees, 109.5 degrees, etc. ![]() Discussed below are the electron pair and molecular geometries. The way I memorized the bond angles was by finding a pattern within the VSEPR geometry chart. In fact for NO 2, a bent molecular geometry, the bond angle is 115.4 o. ![]()
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