VSEPR (Valence Shell Electron Pair Repulsion) theory explains molecular shapes by stating that electron pairs in the valence shell of a central atom repel each other, therefore arranging themselves to minimize repulsions.
• Lone pairs, triple bonds, double bonds and single bonds create a hierarchy of repulsive forces between electron pairs.
• Lone pairs: Experience the strongest repulsive forces because they are only held by one nucleus and occupy a large space around the central atom.
• Multiple bonds (triple and double bonds): They create more repulsion than single bonds because they have a higher electron density.
• Therefore, the order of repulsion is: Lone pair > Triple Bond > Double Bond > Single bond. Therefore, statements B and C are correct, and A and D are incorrect.
Consider the following reactions $ A + HCl + H_2SO_4 \rightarrow CrO_2Cl_2$ + Side Products Little amount $ CrO_2Cl_2(vapour) + NaOH \rightarrow B + NaCl + H_2O $ $ B + H^+ \rightarrow C + H_2O $ The number of terminal 'O' present in the compound 'C' is ______
An aqueous solution of Co(ClO4)2·6H2O is light pink in colour. Addition of conc. HCl results in an intense blue coloured solution due to the formation of a new species. The new species among the following is:
[Given: Atomic number of Co = 27]