Chemistry Fundamental Concepts Quiz

Matter: Anything that has mass and occupies space; exists in solid, liquid, and gas states.
Atoms: Basic units of matter; consist of protons, neutrons, and electrons.
Molecules: Groups of two or more atoms bonded together.
Elements: Pure substances made of only one type of atom.

Atomic Number (Z): Number of protons in the nucleus; defines the element.
Mass Number (A): Total number of protons and neutrons.
Isotopes: Atoms of the same element with different mass numbers due to varying neutrons.

Groups: Vertical columns; elements have similar chemical properties.
Periods: Horizontal rows; represent energy levels of electrons.
Metals, Nonmetals, Metalloids: Classification based on physical and chemical properties.

Mole Concept: A mole is (6.022 \times 10^{23}) particles (Avogadro’s number).
Molar Mass: Mass of one mole of a substance (g/mol).
Balancing Equations: Ensuring the same number of each type of atom on both sides of a chemical equation.

Solid: Definite shape and volume; particles are closely packed.
Liquid: Definite volume but no definite shape; particles are close but can move.
Gas: No definite shape or volume; particles are far apart and move freely.

First Law of Thermodynamics: Energy cannot be created or destroyed, only transformed.
Enthalpy (H): Total heat content of a system; changes in enthalpy indicate heat exchange.

Reaction Rate: Speed at which reactants are converted to products.
Factors Affecting Rates: Concentration, temperature, catalysts, surface area.

Dynamic Equilibrium: Forward and reverse reactions occur at the same rate.
Le Chatelier's Principle: If a system at equilibrium is disturbed, it will shift to counteract the disturbance.

Arrhenius Theory: Acids produce (H^+) ions in solution; bases produce (OH^-) ions.
Brønsted-Lowry Theory: Acids are proton donors; bases are proton acceptors.

Functional Groups: Specific groups of atoms that determine the characteristics and reactivity of organic compounds.
Hydrocarbons: Compounds composed solely of hydrogen and carbon; can be aliphatic or aromatic.

Matter: Defined as anything with mass that occupies space; can manifest as solids, liquids, or gases.
Atoms: The fundamental building blocks of matter, composed of protons (positive charge), neutrons (no charge), and electrons (negative charge).
Molecules: Formed when two or more atoms bond together; can consist of the same or different elements.
Elements: Pure substances that contain only one type of atom; examples include hydrogen, oxygen, and gold.

Atomic Number (Z): Represents the number of protons in the nucleus, which uniquely identifies the element.
Mass Number (A): The sum of protons and neutrons within an atom's nucleus.
Isotopes: Variants of an element that share the same atomic number but differ in mass number due to a varying number of neutrons.

Groups: Vertical columns on the table indicating elements with similar chemical behavior.
Periods: Horizontal rows representing energy levels corresponding to the electrons in atoms.
Metals, Nonmetals, Metalloids: Classification based on distinct physical and chemical characteristics; metals are typically conductive, nonmetals are poor conductors, and metalloids possess properties of both.

Ionic Bonds: Occur when atoms transfer electrons, resulting in the formation of charged ions that attract each other.
Covalent Bonds: Form when atoms share electrons to achieve full outer electron shells, resulting in stable molecular structures.
Metallic Bonds: Characterized by the attraction between metal ions and a sea of delocalized electrons, allowing metallic properties such as conductivity.

Mole Concept: A mole contains (6.022 \times 10^{23}) particles, known as Avogadro’s number, used for quantifying atoms and molecules.
Molar Mass: The mass of one mole of a substance, expressed in grams per mole (g/mol), essential for conversions in chemical calculations.
Balancing Equations: The principle of maintaining equal numbers of atoms for each element on both sides of a chemical equation to reflect the law of conservation of mass.

Solid: Has a fixed shape and volume due to closely packed particles that vibrate in place.
Liquid: Maintains a definite volume but adapts to the shape of its container; particles are closely spaced but can move freely past one another.
Gas: Lacks definite shape and volume; particles are widely spaced and move independently, filling any available space.

First Law of Thermodynamics: States that energy cannot be created or destroyed but only transformed from one form to another.
Enthalpy (H): Refers to the total heat content of a system; changes in enthalpy (ΔH) indicate heat absorbed or released during chemical reactions.

Reaction Rate: Measures the speed at which reactants are converted into products; influenced by various factors.
Factors Affecting Rates: Include the concentration of reactants, temperature, presence of catalysts, and surface area of reactants.

Dynamic Equilibrium: Condition where forward and reverse reactions proceed at equal rates, resulting in stable concentrations of reactants and products.
Le Chatelier's Principle: Suggests that a system at equilibrium will adjust to minimize any imposed change or disturbance.

Arrhenius Theory: Defines acids as substances that release (H^+) ions in solution and bases as those that release (OH^-) ions.
Brønsted-Lowry Theory: Expands definitions, considering acids as proton donors and bases as proton acceptors.

Oxidation: Involves the loss of electrons by a substance, resulting in an increase in oxidation state.
Reduction: The gain of electrons by a substance, leading to a decrease in oxidation state.

Functional Groups: Specific clusters of atoms within molecules that determine the chemical properties and reactivity of organic compounds.
Hydrocarbons: Organic compounds composed solely of carbon and hydrogen; classified into aliphatic (straight or branched chains) and aromatic (ring structures) hydrocarbons.