Increasing the size of the halogen atom generally increases the reactivity of haloalkanes due to the weaker C-X bond.

As the size of the halogen increases, the bond strength decreases due to the longer bond length and weaker overlap.

Increasing steric hindrance decreases the reactivity of ketones compared to aldehydes.

Electron-donating groups activate the aromatic ring, making it more reactive towards electrophilic substitution.

Substituents can either activate or deactivate the aromatic ring towards electrophilic substitution, depending on their electron-donating or electron-withdrawing nature.

The +M effect stabilizes the carbocation by donating electron density through resonance.

The -I effect increases acidity by stabilizing the negative charge on the conjugate base.

Electron-withdrawing groups (-I) increase the acidity of compounds by stabilizing the negative charge on the conjugate base.

The -M effect can stabilize a carbocation by delocalizing the positive charge.

-M groups destabilize carbocations by withdrawing electron density through resonance.

Hemoglobin is a protein that functions to transport oxygen from the lungs to tissues throughout the body.

Alcohols contain a hydroxyl (-OH) functional group.

Carboxylic acids contain the carboxyl group (-COOH), which is the defining feature of this class of compounds.

Ketones contain the functional group -CO- (carbonyl group) between two carbon atoms.

The general formula for alkanes is C_nH_(2n+2).

Alkenes are unsaturated hydrocarbons with the general formula CnH2n.

The general formula for alkynes is C_nH_(2n-2), where n is the number of carbon atoms.

The general formula for carbohydrates is C_n(H2O)_n, indicating that they are hydrates of carbon.

The general formula for carboxylic acids is C_nH_2nO_2.

The general formula for cycloalkanes is CnH2n.

The general formula for ketones is CnH2nO, where n is the number of carbon atoms.

The carbon atoms in benzene are sp2 hybridized, forming a planar structure with 120-degree bond angles.

The nitrogen in a primary amine is sp3 hybridized.

Nitrogen in amines is sp3 hybridized due to the presence of three substituents and a lone pair.

In ethylene, each carbon atom is sp2 hybridized, forming a double bond with the other carbon.

The carbon atoms in ethyne (C2H2) are sp hybridized due to the triple bond between them.

The carbon atoms in alkenes are sp2 hybridized due to the presence of a double bond.

In alkynes, the carbon atoms involved in the triple bond are sp hybridized.

The carbon atoms in benzene are sp2 hybridized, forming a planar structure with 120-degree bond angles.

The carbon atoms in ethylene (C2H4) are sp2 hybridized due to the presence of a double bond.