Chemistry Exam Review

A set of vocabulary flashcards to help students review key terms and concepts in chemistry for their exam.

p bond

A bond formed from the overlap of two p orbitals.

sp3 hybridization

Hybridization involving one s orbital and three p orbitals, forming four equivalent sp3 hybrid orbitals.

sp2 hybridization

Hybridization involving one s orbital and two p orbitals, forming three equivalent sp2 hybrid orbitals.

sp hybridization

Hybridization involving one s orbital and one p orbital, forming two equivalent sp hybrid orbitals.

most stable structure

The molecular structure that has the lowest energy and highest stability among given pairs.

carbon hybridization

The concept of combining atomic orbitals on carbon to form new hybrid orbitals.

s orbital

A spherical atomic orbital that can hold a maximum of two electrons.

p orbital

A dumbbell-shaped atomic orbital that can hold a maximum of six electrons.

overlap

The interaction of atomic orbitals that leads to bond formation.

sp3 hybridization example

Methane (CH4) is an example of a molecule with sp3 hybridized carbon.

sp2 hybridization example

Ethylene (C2H4) is an example of a molecule with sp2 hybridized carbon.

sp hybridization example

Acetylene (C2H2) is an example of a molecule with sp hybridized carbon.

stable isomer

A chemical compound that differs in toxicity or reactivity from its isomer.

inherent stability

Stability that exists naturally due to molecular structure and bonding.

sigma bond

A bond formed by the head-on overlap of atomic orbitals.

diagram of overlap

A representation showing how atomic orbitals combine to form bonds.

orbital diagram

A graphical representation of the arrangement of electrons in the orbitals.

bond length

The distance between the nuclei of two bonded atoms.

bond angle

The angle formed between three atoms in a molecule.

energy minimization

The tendency of systems to move towards a state of lower potential energy.

electronic configuration

The distribution of electrons in an atom's orbitals.

Lewis structure

A diagram that shows the bonding between atoms in a molecule and any lone pairs of electrons.

molecular stability

The tendency of a molecule to maintain its structural integrity and resist decomposition.

polar covalent bond

A type of bond where two atoms share electrons unequally.

nonpolar covalent bond

A type of bond where two atoms share electrons equally.

ionic bond

A chemical bond formed through the transfer of electrons from one atom to another.

electronegativity

The ability of an atom to attract electrons in a bond.

orbital hybridization

The mixing of atomic orbitals to create new hybrid orbitals suitable for the pairing of electrons.

bonding pair of electrons

A pair of electrons that are shared between two atoms in a covalent bond.

lone pair of electrons

A pair of valence electrons that are not shared with another atom.

resonance structure

Different ways of drawing the same molecule that represent the delocalization of electrons.

stability of resonance

The concept that some resonance structures contribute more significantly to the hybrid than others.

conjugated system

A system in which there is alternating single and double bonds.

aromatic compound

A compound containing a ring of carbon atoms with delocalized pi electrons.

anti-bonding orbital

An orbital that has a higher energy than the corresponding bonding orbital.

bonding molecular orbital

An orbital formed by the combination of atomic orbitals that stabilizes the molecule.

free radical

An atom or molecule with an unpaired electron that is highly reactive.

reaction stability

The likelihood that a given chemical reaction will occur and achieve an equilibrium state.

thermodynamic stability

The stability of a substance under certain conditions, taking into account temperature and pressure.

kinetic stability

The stability of a reaction pathway, often influenced by activation energy.

bond dissociation energy

The energy required to break a bond in a molecule.

activation energy

The minimum energy required for a chemical reaction to occur.

transition state

The highest energy state during the conversion from reactants to products.

reaction intermediate

A species that is formed in one step of a reaction and consumed in another.

rate of reaction

The speed at which reactants are converted to products in a chemical reaction.

reaction kinetics

The study of the rates of chemical reactions.

catalyst

A substance that increases the rate of a reaction without being consumed.

enzyme

A biological catalyst that speeds up a chemical reaction.

substrate

The reactant in a chemical reaction that an enzyme acts upon.

oxygen atom hybridization

Oxygen typically exhibits sp3 hybridization in water (H2O).

double bond

A chemical bond involving the sharing of two pairs of electrons.

single bond

A chemical bond involving the sharing of one pair of electrons.

triple bond

A chemical bond involving the sharing of three pairs of electrons.

polar molecule

A molecule with a net dipole moment due to the presence of polar bonds.

nonpolar molecule

A molecule in which there is an equal distribution of electron charge.

intermolecular forces

Forces that occur between molecules, affecting physical properties.

hydrogen bonding

A strong type of intermolecular force that occurs between hydrogen and highly electronegative atoms.

van der Waals forces

Weak attractive forces between molecules or parts of molecules.

solubility

The ability of one substance to dissolve in another at a given temperature and pressure.

henry's law

A law stating that the amount of gas that dissolves in a liquid is proportional to the pressure of that gas.

molarity

Concentration measured by the number of moles of solute per liter of solution.

physico-chemical properties

Characteristics that define the physical and chemical behavior of a substance.

dilution

The process of reducing the concentration of a solute in a solution.

favored reaction pathway

The route a reaction takes that leads to the most stable product.

Lewis acid

A chemical species that acts as an electron pair acceptor.

Lewis base

A chemical species that acts as an electron pair donor.