Chemistry Resonance and Bonding Concepts

The tendency of a substituent in a molecule to either withdraw or donate electron density through sigma bonds.

A measure of an atom's ability to attract electrons towards itself in a chemical bond.

The delocalization of electrons through a system of conjugated pi bonds, leading to stabilization of the molecule.

An inductive effect where electron density is withdrawn from a carbon atom by a substituent, making the carbon atom more electron deficient.

An inductive effect where electron density is donated to a carbon atom by a substituent, making the carbon atom more electron rich.

A positively charged carbon atom with three bonds, often stabilized by electron-donating groups.

Groups that increase electron density towards a carbon atom, making it more stable.

The stability of a carbocation increases as the number of electron-donating groups attached to it increases.

The effect of electron-donating groups decreases with distance from the positively charged carbon.

Ionic compounds are solid at room temperature due to the strong electrostatic forces holding the ions together in a rigid lattice structure.

The amount of energy released when one mole of an ionic compound is formed from its gaseous ions.

The energy required to convert one mole of a solid substance into its gaseous state.

The energy required to remove one electron from a gaseous atom.

The energy change when one mole of gaseous atoms gains one electron to form one mole of gaseous negative ions.

The process of delocalizing π-electrons or lone pairs through conjugation, creating multiple resonance structures.

Structures that contribute to the overall representation of a molecule, where electrons can be delocalized through resonance.

Electron-withdrawing groups that make a molecule more acidic by stabilizing the negative charge of the conjugate base through resonance.

A method used to determine the acidity of a compound by considering the stability of its conjugate base through resonance stabilization.

A representation of a molecule showing all possible positions of electrons, contributing to the molecule's overall stability. These structures differ in electron distribution but have the same arrangement of atoms.

The electron-donating effect of an atom or group within a molecule. It involves the movement of electron density from the substituent to the pi system of the molecule, increasing its electron density.

The electron-withdrawing effect of an atom or group within a molecule. It pulls electron density away from the pi system, making the molecule more 'electron-poor.'

A type of covalent bond where the electron pair sharing is uneven, resulting in a partial positive charge on one atom and a partial negative charge on the other. This arises due to differences in electronegativity between the atoms.

The electrons in the outermost shell of an atom that are available for bonding.

The atom in a molecule that forms bonds with other atoms, typically the one with the highest electronegativity.

Atoms tend to gain, lose, or share electrons to achieve a full outer electron shell with eight electrons (like noble gases).

The way positive and negative charges are distributed within a molecule.

Diagrams that show the arrangement of valence electrons in a molecule, using dots to represent electrons.

The formation of a covalent bond involves the overlap of atomic orbitals, where only half-filled orbitals with opposite spins can participate.

The degree of overlap between atomic orbitals determines the bond's strength. Greater overlap leads to a stronger bond and vice-versa.

Sigma bonds are formed by direct head-on overlap between s orbitals, or an s and a p orbital.

Pi bonds result from the sideways overlap of two p orbitals. Their formation depends on a pre-existing sigma bond framework.

Orbitals that overlap must have the same sign (+ or -) to result in bonding interaction.

The sharing of valence electrons between atoms to achieve a stable electron configuration, typically resembling a noble gas.

When atoms form a bond by sharing one pair of electrons. The shared electron pair occupies the region between the two bonded atoms.

Atoms share more than one pair of electrons, forming stronger bonds than single bonds. Sigma bonds are the strongest, while pi bonds are weaker and form sideways.

The process where atomic orbitals mix to form new hybrid orbitals, leading to specific shapes that influence molecular geometry and bond formation.

These are formed during hybridization and are involved in the formation of sigma bonds, explaining the geometry of molecules.

The type of bond formed directly between two atoms by overlapping orbitals.

The number of hybrid orbitals formed is equal to the number of atomic orbitals participating in the hybridization process.

Hybrid orbitals are named based on the type of atomic orbitals involved in their formation, such as sp, sp2, sp3, etc.