The -OCH3 group shows +M effect as it donates electrons through resonance.

The –OH group donates electron density through resonance, exhibiting a +M effect.

-NO2 is a strong electron-withdrawing group that decreases electron density on the benzene ring.

Iodobutane can be converted to an alcohol by hydrolysis, while bromobenzene requires a different mechanism due to its aromatic nature.

Iodoethane has the highest boiling point due to the larger size and polarizability of iodine.

Iodoethane is least soluble in water due to its larger size and lower polarity compared to the others.

3-bromopropane is more reactive due to the stability of the tertiary carbocation formed during the reaction.

3-bromopropane is a tertiary haloalkane, which is more reactive towards nucleophilic substitution due to steric hindrance and stability of the carbocation formed.

3-chloropropane is a tertiary haloalkane and will undergo elimination more readily due to the stability of the resulting alkene.

2-bromopropane undergoes elimination readily due to the formation of a stable alkene.

All of the listed haloarenes can undergo nucleophilic substitution under suitable conditions.

Nitrochlorobenzene is most reactive due to the electron-withdrawing nitro group, which stabilizes the negative charge in the intermediate.

Iodobenzene is the most reactive towards nucleophilic substitution due to the weaker C-I bond compared to the other haloarenes.

23.40 has 4 significant figures, while 0.0450 has 3.

25.00 has 4 significant figures due to the trailing zeros.

H2O has two lone pairs and two bonding pairs, resulting in a bent geometry.

BF3 has a trigonal planar geometry with bond angles of approximately 120 degrees.

He2 has a bond order of 0, calculated as (2 bonding electrons - 2 antibonding electrons)/2 = 0.

H2 has a bond order of 1, calculated as (2 bonding electrons - 0 antibonding electrons)/2 = 1.

In PCl5, the phosphorus atom is dsp3 hybridized, resulting in a trigonal bipyramidal geometry.

In BrF5, bromine undergoes sp3d hybridization to form five bonds with fluorine and has one lone pair.

In BrF5, the bromine atom is sp3d2 hybridized, allowing it to form five bonds with fluorine.

BeCl2 has two bonding pairs and no lone pairs, resulting in a linear geometry.

NH3 has a trigonal pyramidal shape, which is not symmetrical due to the lone pair.

NH3 has three bonding pairs and one lone pair, resulting in a trigonal pyramidal shape.

SF4 has four bonding pairs and one lone pair, resulting in a seesaw molecular geometry.

SF4 has four bonding pairs and one lone pair, resulting in a seesaw shape.

SF4 has four bonding pairs and one lone pair, resulting in a seesaw shape.

XeF4 has four bonding pairs and two lone pairs, resulting in a square planar geometry.

CH4 has a tetrahedral shape due to the sp3 hybridization of the carbon atom.