Chemical Bonding And Molecular Structure

In general, the bond length decreases as the bond order increases. The shortest bond length is found in CO because it has a triple bond, which results in a shorter bond compared to the others.

An empirical formula represents the simplest whole-number ratio of elements in a compound. PCl is already in its simplest form, making it an empirical formula.

The percent ionic character of a molecule can be calculated using the following formula: where: - is the measured dipole moment of the molecule, - is the ideal dipole moment assuming complete ionic character. The ideal dipole moment is given by: where: - is the charge of the electron, , - is the interatomic separation, . Substituting the values: Now, calculate the percent ionic character:
Thus, the correct answer is (c).

In Cl O , the molecular geometry around each chlorine atom is tetrahedral due to the bonding with oxygen atoms.
In such a geometry, the bond angle is typically around 109.5°, but due to the presence of lone pairs, the bond angle slightly deviates.
The bond angle in Cl-O-Cl in Cl O is 119°, which is slightly less than the ideal tetrahedral angle due to repulsion between the lone pairs on the oxygen atoms.
Thus, the correct answer is (b).

The correct Lewis structure for the ionic compound Ca(ClO2)2 is represented by option (c).
In this structure, calcium (Ca) has a 2+ charge and is bonded to two chlorite ions ( ) with each chlorine atom in the chlorite ion having two lone pairs of electrons.

In the isoelectronic series, the species with the least nuclear charge (lowest effective nuclear charge) will require the least energy to remove an electron. Since has the most electrons and the smallest nuclear charge, it will require the least energy to remove an outer electron. Thus, the correct answer is (a) .

In species I ( ) and II (acetone), electrons are delocalised over the entire structure, as seen in their resonance forms. In , the electron density is shared between the two oxygens and the carbon atoms, forming a delocalised system. This delocalisation stabilises the ion and contributes to its overall chemical properties. In acetone, the carbonyl group ( ) allows for electron delocalisation via resonance with the oxygen atom, further stabilising the molecule.

In contrast, species III does not have delocalised electrons because it is a simple molecule with no resonance structures. This lack of delocalisation means that the electrons are more localized, which affects its reactivity and stability compared to species I and II.

Thus, species I and II exhibit delocalised electrons, while species III does not.