Final Exam Notes - Inorganic Chemistry and Organic Chemistry Concepts

The flashcards cover key terms and definitions relating to chemical bonding, organic chemistry, reactions, and molecular structure.

Chemical Bonding

The attraction between atoms that allows the formation of chemical substances.

Ionic Bonding

formed through the transfer of electrons from one atom to another, resulting in the attraction between cations and anions.

Covalent Bond

type of intra-molecular bond. two atoms share one or more pairs of electrons.

Dative Covalent Bond

A type of covalent bond where one atom donates electron pair to a covalent bond.

are dative covalent bonds intra-molecular or inter-molecular

intra-molecular

Hydrogen Bonding

A type of strong intermolecular force that occurs between a hydrogen atom, covalently bonded to a highly electronegative atom, and another electronegative atom.

inter molecular forces

bonds between different molecules

van der waal 

non polar molecules, permanent electrostatic forces

dipole-dipole interactions

caused by presence of polar bonds

Valence Bond Theory

A theory that explains how atomic orbitals combine to form covalent bonds.

Sigma Bond

A covalent bond found in single bonds. 2 s-orbitals, 2 p-orbitals, or an s and p orbital 

Pi Bond

A type of covalent bond sharing 2 p-orbitals, found in double bonds. 

delta 

foud in quadruple bonds, formed when 2 d-orbitals overlap. 

properties of covalent bonds

low melting and boiling points, poor electrical conductors, mostly insoluble, can be gases liquids or solids,

valence bond theory

states that “the overlap between 2 atomic orbitals forms a covalent bond”

Hybridization

phenomenon of promoting electros up an orbital to allow to form a bond.

types of hybridization

sp, sp2,sp3

sp 

one electro from s1- orbital to p-orbital 

sp2

one electron from s1-orbital to p-orbital which already has 2 electrons.

sp3

one electron from s1 to p-orbital which already has 3 electrons.

what does an overlap of orbit;s ;had to

a covalent bond being formed

Coordination Compound

A complex composed of a central metal atom or ion bonded to one or more ligands.

Electronegativity

The tendency of an atom to attract electrons in a chemical bond.

Dipole Moment

A measure of the separation of positive and negative charge in a molecule.

Nucleophiles

An electron-rich species that donates an electron pair to form a chemical bond.

Electrophiles

Electron-deficient species that accept an electron pair to form a bond.

Carbocation

An ion with a positively charged carbon atom.

Aromatic Hydrocarbons

Compounds containing carbon atoms arranged in a ring with alternating double bonds, known for their stability.

Aliphatic Hydrocarbons

Hydrocarbons that consist of linear or branched chains of carbon atoms.

Phenolic Compounds

Compounds containing a hydroxyl group (-OH) attached to an aromatic hydrocarbon.

Cyclic Compounds

Compounds that contain carbon atoms arranged in a loop or ring.

Diels-Alder Reaction

A type of cycloaddition reaction between a diene and a dienophile to form a cyclic compound.

Dielectric Constant

A measurement of the ability of a substance to insulate charges from each other.

Redox Reaction

A chemical reaction that involves a transfer of electrons between two species.

Saponification

The process of making soap from the hydrolysis of fats or oils.

Glycosidic Bond

A type of covalent bond that joins a carbohydrate (sugar) molecule to another group.