Toluene undergoes electrophilic substitution most readily due to the electron-donating effect of the methyl group, which activates the benzene ring.

3-bromopentane undergoes elimination more readily due to the stability of the tertiary carbocation formed during the reaction.

3-bromopropane undergoes elimination more readily due to the stability of the tertiary carbocation formed during the reaction.

2-bromobutane undergoes elimination (E2) to form an alkene, while 2-bromo-2-methylpropane does not due to steric hindrance.

2-bromopentane can undergo E2 elimination because it has a beta-hydrogen available for elimination, while the others either do not or favor different mechanisms.

Nitrobenzene will not undergo electrophilic substitution readily because the nitro group is a strong deactivator and meta-director.

Toluene will undergo electrophilic aromatic substitution most readily due to the electron-donating effect of the methyl group.

Phenol will undergo electrophilic substitution more readily than benzene due to the electron-donating effect of the hydroxyl group.

Toluene will undergo electrophilic substitution more readily than benzene due to the electron-donating effect of the methyl group.

Ethylbenzene will undergo electrophilic substitution the fastest due to the electron-donating effect of the ethyl group.

2-butanol has a chiral center and can exist as two enantiomers, thus showing optical isomerism.

Aromatic compounds have delocalized π electrons that can absorb UV light, while alkanes and alcohols do not have such electronic transitions.

Ethanol would show a strong absorption in the IR region due to O-H stretching, characteristic of alcohols.

Aromatic compounds have delocalized π electrons that can absorb UV light, leading to strong absorption in the UV region, unlike alkanes which do not absorb UV light.

Real gases behave more ideally at low pressure and high temperature, where intermolecular forces and molecular volume become less significant.

Oxalate (C2O4) is a bidentate ligand that can form two bonds with a metal center.

[Ni(CN)4]2- is a square planar complex, while the others exhibit different geometries.

Ethylenediamine is a bidentate ligand that can form stable chelate complexes with transition metals.

The complex [Cu(NH3)4]2+ contains a transition metal with d-electrons that can be excited, resulting in color.

The complex [CoCl2(NH3)4] can exhibit geometric isomerism due to the presence of two different types of ligands.

Coordination numbers typically range from 2 to 6 in most coordination compounds, making 7 an unlikely coordination number.

A primary battery is designed for single-use and cannot be recharged, unlike secondary batteries.

The BET theory describes multi-layer adsorption on porous surfaces, extending the Langmuir model to account for multiple layers.

Oxygen can donate a lone pair to form a coordinate covalent bond, as seen in compounds like H2O and H3O+.

Phosphorus can form an expanded octet because it has available d orbitals to accommodate more than eight electrons in its valence shell.

Rubidium has the largest atomic radius due to its position in Group 1 and being the lowest in the group.

Boron has a lower first ionization energy than Be, C, and N due to its position in the periodic table.

Ionization energy decreases down a group; rubidium has the smallest ionization energy among these.

Ammonia (NH3) is a common ligand that can donate a pair of electrons to a metal center.

Neodymium is a lanthanide, which are the 15 elements from cerium (Ce) to lutetium (Lu) in the periodic table.