Select correct order of bond angle ;
In case of 'F' bond angle always least.
CH4 = SiH4 = 109° 28'
BF3 = BCl3 = 120°
NO2+ = CO2 = 180°
Bond angles in molecules are influenced by factors such as electronegativity, lone pair-bond pair repulsion, and atomic size. Let's evaluate each option step by step.
Both PF3 and PCl3 have a trigonal pyramidal geometry with one lone pair on phosphorus. Chlorine is less electronegative than fluorine, so in PCl3, the bond pair is pulled less towards chlorine, reducing lone pair-bond pair repulsion. This results in a larger bond angle in PCl3 than in PF3. Thus, PF3 < PCl3 is correct.
Both BF3 and BCl3 are trigonal planar with no lone pairs on boron. The bond angle is exactly 120° in both due to identical geometry and no lone pair influence. Electronegativity differences do not affect the angle here. So, BF3 < BCl3 is incorrect; they are equal.
Both CH4 and SiH4 are tetrahedral with bond angles of approximately 109.5°. Since carbon and silicon are in the same group, and both molecules have identical geometries with no lone pairs, the angles are nearly the same. Silicon has a larger size, but this does not significantly reduce the angle. Thus, CH4 > SiH4 is incorrect; they are very similar.
NO2+ is linear with no lone pairs on nitrogen (sp hybridization), and CO2 is also linear with no lone pairs on carbon (sp hybridization). Both have bond angles of 180°. Thus, NO2+ > CO2 is incorrect; they are equal.
The correct order is PF3 < PCl3, as it is the only option where the bond angle difference is justified by electronegativity and repulsion effects.
Bond angle is determined by the number of bonding pairs and lone pairs around the central atom. According to VSEPR theory:
Example: In NH3 (with one lone pair), bond angle is 107°, while in CH4 (no lone pairs), it is 109.5°.
Which properties is related to given graph?
Select the correct option regarding following figure:
