The ideal bond angle is 109.5, but because that lone pair is there, all you'd have to really say is, you would expect the bond angle to be less than 109.5. The electron-domain geometry around O is therefore tetrahedral, which gives an ideal angle of 109.5°. Although each molecule can be described as having a bent geometry the respective bond angles are different. The H—O —C angle will be compressed somewhat by the nonbonding pairs, so we expect this angle to be slightly less than 109.5° . Select the correct value for the indicated bond angle in each of the compounds. The O-H bond length is 95.84 pm and the S-H bond length is longer at 133.6 pm. See the website below to see the structure of methane. For the H—O—C bond angle, the middle O atom has four electron domains (two bonding and two nonbonding). Five Electron Pairs (Trigonal Bipyramidal) Transcript: We can draw O3 different ways. The bond length is more or less intermediate between #O=O#, #1.21xx10^-10*m#, and the peroxide bond in hydrogen peroxide, #1.49xx10^-10*m#, so our resonance description of ozone is appropriate. According to the valence shell electron pair repulsion theory, a trigonal planar molecular geometry is expected with an F-B-F bond angle of 120°. 1. ozone molecules are linear so the bond angle is 180 degree, 2. ozone molecules are tetrahedral so the bond angle is approximately 109 degree, the nonbonding electrons pair occupies greater space than the bonding pairs, the electrons in the double bond occupy more space that the non bonding electron pair Because of this, you can't have 2 pairs of double bonds, since it'd give you the incorrect number of electrons. The actual bond angle of O3 is about 116° For BF3, the three bond pairs of electrons are directed towards the corners of an equilateral triangle. A quick explanation of the molecular geometry of O3 including a description of the O3 bond angles. Answer link The HOH bond angle in water is 104.50, the HSH bond angle in hydrogen sulfide is less at 92.10. O 3 has 18 valence electrons (3 * 6e- = 18e-). For SO 2 the O-S-O angle is near 120 degrees, actually slightly less than 120, about 118 degrees, for H 2 O the H-O-H angle is near 105 degrees. It has eight valence electrons. And this works: we're using all 18 valence electrons for O3, and each of the atoms has a full outer shell. The bond angles of the molecules or ions from smallest to largest: O3- , O3 , O3+ Explanation: O3- has the smallest bond angle because the added electron makes two places for electron repulsion as it allocates time on the central O. 109.5˚ is the angle of a tetrahedron. First, we can draw it with a double bond on the left and a single bond on the right. The bond angle is a little less than 120˚, because the resonance bond is pulling the 2 O atoms a little bit closer to each other. :Ö=O=Ö: only has 16e- but the octets are already filled, so we have to use one sight with only one bond and another with 2 bonds. The bond angle is dependent on type of bonds in the molecule and relative attraction, which the 3 atoms have for each other.