Redox Reactions and Oxidation States Quiz

A chemical reaction where electrons are transferred from one reactant to another.

The flow of electrons through a circuit.

The study of how chemical energy is converted to electrical energy.

The part of an electrochemical cell where oxidation occurs.

The part of an electrochemical cell where reduction occurs.

A device that generates electrical energy from a chemical reaction.

The potential difference between the anode and cathode in an electrochemical cell.

A measure of the tendency of a substance to gain electrons.

A reaction in which a species loses electrons and increases its oxidation state.

A reaction in which a species gains electrons and decreases its oxidation state.

A species that gains electrons in a redox reaction, causing another species to be oxidized.

A species that loses electrons in a redox reaction, causing another species to be reduced.

A redox reaction occurs only when a strong oxidizing agent reacts with a strong reducing agent.

A reaction in which a metal displaces another metal from its salt solution.

A method for balancing redox reactions by balancing each half-reaction separately and ensuring that the number of electrons lost in the oxidation half-reaction is equal to the number of electrons gained in the reduction half-reaction.

A chemical equation showing the ionic species involved in a reaction.

A chemical equation showing only the species that directly participate in the reaction.

A reaction where the same element is both oxidized and reduced.

A reaction between a metal and a non-metal, forming an ionic substance.

The process of forming new hybrid orbitals by mixing atomic orbitals. This allows for more effective bonding, resulting in stable molecules.

A type of covalent bond formed by the overlap of two atomic orbitals along the axis connecting the two atoms.

A type of covalent bond formed by the sideways overlap of two atomic orbitals above and below the plane of the sigma bond.

The three-dimensional arrangement of atoms in a molecule, determined by the spatial orientation of bonds around a central atom in a molecule.

The angle between two adjacent bonds in a molecule.

Hybridization occurs when an atom's electron promotion is necessary to obtain the required number of unpaired electrons for bonding. This happens when there are fewer than four unpaired electrons in the valence shell.

The type of hybridization depends on the number of unpaired electrons in the central atom. For example, carbon's four hybrid orbitals are called sp3, indicating one s and three p orbitals combined.

The orbitals in hybridized atoms change their shape to create hybrid orbitals suitable for bonding. For example, sp3 orbitals are tetrahedral in shape.

The presence of lone pairs on the central atom influences the bond angles in the molecule due to repulsion. For example, the bond angle in water is 104.5° due to two lone pairs on the oxygen atom.

The ability of atoms to form bonds, especially with the same atom, allows for the formation of chains, rings, and diverse molecules.

Hybridization helps atoms form stable bonds with other atoms and allows molecules to adopt specific shapes.

The central atom in methane (CH4) undergoes hybridization because it requires four valence electrons to form four bonds. The hybridization of the carbon atom in methane is sp3 and results in a tetrahedral shape.

A model that predicts the geometric shape of molecules based on the number of electron pairs around the central atom.

A measure of the difference in electronegativity between two bonded atoms. It determines the polarity of a bond, ranging from 0 (nonpolar) to 4 (ionic).

The tendency of an atom in a molecule to attract shared electrons towards itself, influenced by factors like nuclear charge and shielding.

A molecule with a positive end and a negative end due to unequal sharing of electrons, leading to an overall dipole moment.

A molecule where the electron distribution is even, resulting in no overall dipole moment.

Weak forces of attraction between molecules due to temporary fluctuations in electron distribution, present in all molecules.

Forces of attraction between polar molecules due to the attraction of oppositely charged ends of the dipoles, stronger than LDF.

A special type of dipole-dipole interaction between a hydrogen atom bonded to a highly electronegative atom (O, N, or F) and an electron pair on an adjacent molecule, the strongest intermolecular force.

Forces of attraction between molecules, responsible for physical properties like boiling point, melting point, and viscosity. They are weaker than intramolecular forces that hold atoms together within a molecule.

Describes how strong a bond is between two atoms, based on how much of its valence electrons it shares with the other atom to reach a stable state.

The type of hybridization where an atom's atomic orbitals combine to form four equivalent sp³ hybrid orbitals, resulting in a tetrahedral shape.

The type of hybridization where an atom's atomic orbitals combine to form two equivalent sp hybrid orbitals, resulting in a linear shape.

The process of determining the molecular shape by considering the number of electron pairs around the central atom and using the VSEPR theory to predict the repulsion of electrons.