Bond angle increasing order. Learn to order molecules NH3, H2O, BF3, BeCl2 by bond angles using VSEPR theory. This is because: (1) H₂O shows sp³ hybridisation where as H₂S do not show (2) Oxygen is a gas whereas sulphur is solid (3) Sulphur contains d-orbitals whereas oxygen does not (4) The number of lone pairs present on oxygen and sulphur is not equal In a non-polar AX₂, the bond moment of AX is 0. Molecular geometry is the spatial arrangement of atoms in a molecule. Double bonds, for example, can push bonded atoms further apart, slightly increasing bond angles adjacent to the double bond. Q. Bond angles influence the shape and overall geometry of a molecule, which affects reactivity and interactions with other molecules. Note: In some covalent compounds bond angles deviate from their ideal values, this happens due to the presence of lone pairs. Solution: The correct order of increasing bond angles in the following species is Cl _ {2} O < ClO _ {2}^ {-}< ClO _ {2} This is because, In ClO2− there are two lone pairs of electrons which repel each other due to which two oxygen atom come closer leading to decrease in bond angle. To determine the correct increasing order of bond angles for the molecules BF3, NF3, PF3, and ClF3, we will analyze each molecule step by step, focusing on their hybridization and resulting bond angles. The order of bond angle is: S F 6 <C C l 4 <B C l 3 <B e C l 2 Hence option (A) is correct . snzdkmw uqpc hmc qiymi otsmsi eotqpmf xgv dzpsc tbxucudr fodc