III OCl2 OF2 The bond angle is greater in OCl2 than in OF2 because there are some pi interactions in OCl2 involving donation from the filled p-orbitals on oxygen into the empty d-orbitals on chlorine. No pi-bonding is possible for OF2 because all orbitals (2024)
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The bond angle is greater in OCl2 than in OF2 because there is some π interactions in OCl2 involving donation from the filled p-orbitals on oxygen into the empty d-orbitals on chlorine No π-bonding is possible for OF2 because all orbitals are filled on both atoms.
Explanation: Because oxygen in Cl₂O exhibits stronger electronegativity than chlorine, its bond angle is bigger than that of OF₂. As a result, oxygen and the shared electron pair are becoming closer to one another. Offer repulsion and an increase in angle as a result.
Answer. because in Cl2O oxygen has more electro-negativity than chlorine. Hence the shared electron pair is closer to oxygen which in turn get more closer to each other. Thus offer repulsion and increase in angle.
in case of clo2 there will be less repulsion hence bond angle will be greater and in case of cl2o there will be more repulsion hence bond angle will be be lesser in comparison to clo2.
OCl2 is a sp3 hybridized structure with 2 lone pairs . So resultant shape is V-Type . We know that in sp3 structure bond angle is 109.47 but high electro-negative oxygen atom, attracts Cl-O bonded electrons toward oxygen creating repulsions . So angle is slightly increases to 110.9.
And therefore the repulsion between bonding electrons is more in OBr2. Moreover the size of Br is bigger than Cl′s. So OBr2 has a greater bond angle than OCl2.
Therefore, VSEPR predicts that each molecule will be bent with the bonds and lone pairs taking the shape of a tetrahedron. This predicts an angle of 109.5 deg for each moleule. The observed angles are 111 deg for OCl2 and 103 deg for SCl2.
Bond angle refers to the angle between the two bonds i.e. the angle between two orbitals that contains a pair of bonding electron around the central atom in a complex molecule or an ion. This angle is usually measured in degrees, further calculated using the spectroscopic method.
In both the compounds O is the central atom but, Cl being excessively large with lone pairs causes strong repulsion with the other Cl atom in Cl2O thereby increasing the bond angle. However H is the smallest element and the repulsion between individual H atoms is very weak, thus it has a relatively smaller bond angle.
OCl2 is a sp3 hybridized structure with 2 lone pairs . So resultant shape is V-Type . We know that in sp3 structure bond angle is 109.47 but high electro-negative oxygen atom, attracts Cl-O bonded electrons toward oxygen creating repulsions . So angle is slightly increases to 110.9.
The molecules having sp hybridization will have largest bond angle because in sp hybridization bond angle is 180° and examples are CO2 , BeCl2 , BeH2 etc . Any molecule having “sp” hybridization or linear shape. So the largest possible angle in any molecule is 180°.
Introduction: My name is Aracelis Kilback, I am a nice, gentle, agreeable, joyous, attractive, combative, gifted person who loves writing and wants to share my knowledge and understanding with you.
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