Chemical Bonding And Molecular Structure

In the trigonal bipyramidal geometry, the central iron atom is surrounded by five ligands (carbon monoxide molecules). Three of these ligands are arranged in a trigonal plane, while the other two are located above and below the plane, making the shape trigonal bipyramidal.

So, the correct option is (C): Trigonal bipyramidal

The order of dissociation energy between and can be explained based on molecular and electronic structure.

N₂ (Nitrogen Molecule):

• is a stable diatomic molecule with a triple bond between two nitrogen atoms .
• In the molecule, there is a strong triple bond holding the two nitrogen atoms together.
• Breaking this bond to dissociate into two nitrogen atoms requires a significant amount of energy. This is because the bond is strong and stable.
• As a result, the dissociation energy of is relatively high.

N₂⁺ (Nitrogen Cation):

• refers to a nitrogen cation where one of the nitrogen atoms has lost an electron, leaving it with a positive charge.
• In , the positive charge destabilizes the molecule compared to because there are fewer electrons available for bonding.
• The N-N bond in is weaker than the triple bond in because it has lost one of its electrons.
• Due to the weaker bond in , less energy is required to dissociate it into two nitrogen atoms.

In summary, has a stronger and more stable triple bond, which means that it requires more energy to dissociate into its constituent nitrogen atoms. , on the other hand, has a weaker bond due to the loss of an electron, so it requires less energy for dissociation.

Therefore, the correct order of dissociation energy is option (A)

has a square planar molecular geometry. The central xenon atom is bonded to four fluorine atoms, and the molecule lies in a single plane. This arrangement results in a planar structure for .
In contrast, the other compounds have different molecular geometries. has a bent shape, has a seesaw shape, and has a tetrahedral shape.

So, the correct option is (A):

The statement "Bond energy of " is incorrect. The bond energy of is lower than that of because fluorine forms a stronger bond due to its higher electronegativity.

So, the correct option is (A): Bond energy of

The relationship between bond length and bond strength is inverse, while the relationship between bond strength and bond dissociation energy is direct. Since H₂ O₂ has a single bond, O₃ has a partial double bond due to resonance, and O₂ has a double bond, the right sequence is O₂ O₃H₂ O₂. O-O's bond length in O₂ is 1.21A⁰, O₃ is 1.2730A⁰, and H₂ O₂ is 1.49A⁰.

Therefore, the correct option is (C): O₂32O₂

The molecule of boron trifluoride, BF₃, has a trigonal planar shape.
Three bond pairs and no lone electron pairs make up the centre B atom. It goes through sp₂ hybridization.
The geometry of IF₃ is 'T' shaped. The geometries of PCl₃ and NH₃ are pyramidal.

Therefore, the correct option is (D) BF_{3 .}

We can observe that each of the supplied molecules has a chlorine anion linked to it, but the cations are different. And the cations' order of electronegativity is Na Li Be. Therefore, the covalent character will increase in the following order: NaCl, LiCl, and BeCl₂.

So, the correct option is (C): NaCl < LiCl < BeCl₂

Not every AB₅ molecule has a square pyramid structure. While some AB₅ molecules, such as phosphorus pentachloride (PCl₅), do have a square pyramid structure, others may have different structures depending on the atom involved and its geometry. For example, SF₅Cl has a trigonal bipyramidal structure, not a square pyramid. The actual structure depends on the specific molecular geometry and the arrangement of atoms and lone pairs around the central atom.

So, the correct option is (C): Every AB₅ molecule does in fact have square pyramid structure

The atomic number of the element is 16, which corresponds to sulfur (S). In a diatomic molecule of sulfur (S₂), each sulfur atom contributes six valence electrons (since sulfur is in group 16 of the periodic table). When two sulfur atoms bond together to form a diatomic molecule, they share their electrons, resulting in a total of 12 valence electrons in the molecule. To determine the number of unpaired electrons, you can use molecular orbital theory. In the case of a sulfur molecule (S₂), the molecular orbital diagram shows that there are 2 unpaired electrons.

So, the correct answer is (A): 2

adopts a tetrahedral structure due to the four chlorine atoms arranged symmetrically around the silicon atom. On the other hand, features four chlorine atoms and an additional lone pair on sulfur, causing it to assume a see-saw molecular geometry. The remaining molecules in the list maintain a tetrahedral geometry. Therefore, does not share the same structural arrangement as .

So, the correct option is (A):

Despite the fact that the electronegativity difference between nitrogen (N) and fluorine (F) is larger than that between nitrogen (N) and hydrogen (H), the dipole moment of NH₃ (1.5 D) exceeds that of NF₃ (0.2 D). This discrepancy arises because in NH₃, the atomic dipole moments and bond dipole moments align in the same direction, while in NF₃, they are oriented in opposite directions.

So, the correct option is (B): in NH₃ the atomic dipole and bond dipole are in the same direction whereas in NF₃ these are in opposite directions.

In ClF₃ (Chlorine trifluoride), the central chlorine atom forms three sigma (σ) bonds with three fluorine atoms. However, due to the lone pair of electrons on the chlorine atom, there is also a lone pair - lone pair repulsion, causing distortion in the molecular geometry. This results in unequal bond lengths, and not all the bonds are equal in ClF₃.

So, the correct option is (A): CIF₃