Chemistry Lecture Practice Questions

Flashcards covering fundamental chemistry concepts including atomic models, bonding, reaction types, and thermodynamics based on the lecture transcript.

Pure Substance

Matter that is classified as either an element or a compound, such as gold ($Au$).

Chemical Property

A property, such as flammability, that alters the composition of a substance and is generally irreversible.

Niels Bohr

The physicist known as the 'Architect of the Atom' who proposed the planetary model and that electrons move in specific energy levels.

Atomic Number

The value that represents the number of protons within an atom.

Nucleons

The collective term for the components of the nucleus, specifically protons and neutrons.

Isotopes

Atoms of an element that have the same number of protons but differ in the number of neutrons.

Compound

A molecule formed by atoms of different elements that are chemically bonded together.

Polar Molecule

A molecule, such as $H_2O$, that has two opposite charges or properties directed toward poles.

Saponification

The reaction between oily skin and a base like $NaOH$ that causes bases to feel slippery.

Neutralization

A reaction between an acid and a base that results in the formation of salt ($NaCl$) and water ($H_2O$).

Brønsted-Lowry Acid

A substance defined as a proton ($H^+$) donor.

Synthesis (Combination)

A chemical reaction represented by the formula $A + B \rightarrow AB$, where reactants combine to form a product.

Chemical Equilibrium

The state where the rate of the forward reaction is equal to the rate of the reverse reaction.

Dilution Equation

The formula $M_1V_1 = M_2V_2$ used to find the volume or molarity of a solution.

Exothermic Reaction

A chemical reaction that releases heat to its surroundings, often making them hotter.

Endothermic Reaction

A chemical reaction that absorbs energy from its surroundings, often making them cooler.

Orbitals

Regions that describe the probability of finding an electron, categorized into shapes like $s, p, d, f$.

Quantum Theory

The theory that explains the behavior of matter and energy at the atomic and subatomic level.

Heisenberg Uncertainty Principle

The principle stating that it is impossible to simultaneously measure both the exact position and the exact momentum of a microscopic particle.

Second Energy Level

The electron shell that can occupy a maximum of $8$ electrons.

Covalent Bond

A type of chemical bond characterized by the sharing of available valence electrons between atoms.

Ionic Bond

A chemical bond involving the transfer of electrons from a metal to a nonmetal.

Metallic Bond

The electrostatic attraction between electrons and metal ions.