The central carbon atoms in both molecules have four bonding electron pairs. So, VSEPR theory predicts tetrahedral geometry Since this gives maximum separation. The H-C-H bond angles are all 109 degree and 28`.

There are five groups around the central atom, three bonding pairs and two lone pairs.

Hint: The shape of AB3 with one lone pair on central atom can be pyramidal . if there is no lone pair of electrons present on the central atom then the shape will be trigonal planar. In AB3 molecules there are 3 atoms attached to the central A atom….

There is a defined optimal distance between the nuclei in which the potential energy is at a minimum, meaning that the combined attractive and repulsive forces add up to the greatest overall attractive force. This optimal internuclear distance is the bond length; the distance is 74 pm for H2.

In addition to tetrahedral, another common shape for AB4 molecules is square planar. All five atoms lie in the same plane, with the B atoms at the corners of a square and the A atom at the center of the square.

Hence, due to small size and absence of d and f orbitals, Aluminium does not show inert pair effect.

The inert-pair effect is the tendency of the two electrons in the outermost atomic s-orbital to remain unshared in compounds of post-transition metals. As a result, the inert pair of ns electrons remains more tightly held by the nucleus and hence participates less in bond formation.

Answer. Inert pair effect is mostly shown by the 15-17th group elements. That is, the oxidation state reduces by 2 for elements below (As, Sb), which is more stable than the other oxidation states. The reason for this is the inertness of the inner s electrons due to poor shielding.

ii AlCl3 is more stable. Anhydrous state is covalent while aqueous state is ionic in nature. +3 oxidation state is more stable than +1 oxidation state. Inert pair effect is negligible.

Dear student, If you want to know why AlCl3 is more stable than TiCl3, it is because, +1 oxidation state increases down the group and +3 oxidation state decreases down the group due to increase in inert pair effect.

TlCl is more stable because it shows +1 oxidation state while TlCl3 shows +3 oxidation state due to inert pair effect.

AlCl3 achieves stability by forming a dimer. In trivalent state the compound is hydrolysed in water.

The answer is because the presence of half filled SP3 hybrid orbitals. The boron chloride is the electron deficient compound and the need of electrons is fulfilled by the chlorine which is electron rich. Due to this Cl atoms are more closely packed in BCl3 than in AlCl3 and hence it is more stable.

AlCl3 exists as a dimer as the Al atom in the molecule is electron deficient due to presence of only 6 electrons in its’ valence shell ie it has an incomplete octet due to which it is quite unstable.

Answer. BCl3 is more covalent due to its basic nature. PbCl4 is more covalent as it contains more chloride ions.

Which is more covalent nacl BeCl2 or AlCl3? This means that AlCl3 has stronger bonds than BeCl2 that require more energy to break down, thus the lattice enthalpy of AlCl3 is more exothermic (as the ions lie closer together) so AlCl3 is at a lower energy level and therefore more stable.

BeCl2 is more covalent than LiCl. As per the Fajan’s rule, more the polarisation, more will be the covalent character.

actually, smaller cations have higher charge density due to higher charge density , polarisation will be larger and hence, covent character will be higher. here four ionic compound are ; FeCl2, SnCl2, AlCl3 and MgCl2 . so, covalent character will be maximum in AlCl3 compound.

According to the Fajan’s rule, AlCl3 is more covalent in nature.

Hence, CaI2 has the largest covalent character.

Because of the high polarization capability of Li+ ion, lithium halides are somewhat covalent. Since anion with large size can be easily distorted, among halides, LiI is the most covalent in nature. The order of covalent character is LiI>LIBr>LiCI>LiF because larger the anion, greater is its polarizability.

LiI

Hence the order of increasing covalent character is: KCl< CaCl2