Chemistry Basics Quiz

Matter: Anything that has mass and occupies space; exists in solid, liquid, and gas states.
Atoms: Basic units of matter; composed of protons, neutrons, and electrons.
Elements: Pure substances made up of only one type of atom; listed in the periodic table.

Nucleus: Central part of an atom; contains protons (+1 charge) and neutrons (neutral).
Electrons: Negatively charged particles that orbit the nucleus in electron shells.
Atomic Number: Number of protons in an atom; defines the element.
Mass Number: Total number of protons and neutrons in the nucleus.

Ionic Bonds: Formed when electrons are transferred from one atom to another, resulting in positive and negative ions.
Covalent Bonds: Formed when atoms share electrons.
Metallic Bonds: Occur between metal atoms; electrons are shared in a "sea" of electrons.

Reactants and Products: Starting materials (reactants) transform into new materials (products) during a reaction.
Balancing Reactions: Conservation of mass dictates that the number of atoms must remain the same on both sides of the equation.
Reaction Types:
- Synthesis: Two or more substances combine to form a new compound.
- Decomposition: A compound breaks down into simpler substances.
- Single Replacement: An element replaces another in a compound.
- Double Replacement: Exchange of components between two compounds.
- Combustion: Reaction with oxygen producing heat and light.

Solid: Definite shape and volume; particles closely packed.
Liquid: Definite volume but takes the shape of its container; particles less tightly packed than solids.
Gas: No definite shape or volume; particles are far apart and move freely.

Acids: Substances that donate protons (H+) in a solution; have a pH less than 7.
Bases: Substances that accept protons or donate hydroxide ions (OH-); have a pH greater than 7.
pH Scale: Measures the acidity or basicity of a solution, ranging from 0 (strong acid) to 14 (strong base).

Solutions: Homogeneous mixtures where one substance (solute) is dissolved in another (solvent).
Concentration: Amount of solute in a given volume of solution; expressed in molarity (M).
Solubility: Maximum amount of solute that can dissolve in a solvent at a given temperature.

Energy: The capacity to do work; can be in the form of heat (thermal energy).
Endothermic Reactions: Absorb heat from the surroundings.
Exothermic Reactions: Release heat to the surroundings.

Groups/Families: Vertical columns with similar chemical properties.
Periods: Horizontal rows indicating increasing atomic number.
Metals, Nonmetals, and Metalloids: Classification based on physical and chemical properties.

Boyle's Law: Pressure and volume are inversely related at constant temperature.
Charles's Law: Volume and temperature are directly related at constant pressure.
Ideal Gas Law: PV = nRT, where P = pressure, V = volume, n = number of moles, R = gas constant, T = temperature in Kelvin.

Mole Concept: 1 mole = 6.022 x 10²³ particles; used for counting atoms and molecules.
Mole Ratio: Derived from balanced equations; used to convert between moles of reactants and products.

Matter has mass and occupies space, existing in solid, liquid, and gas states.
Atoms are the smallest units of matter, consisting of protons, neutrons, and electrons.
Elements are pure substances consisting of a single type of atom, represented in the periodic table.

The nucleus is the atom's central part, containing positively charged protons and neutral neutrons.
Electrons are negatively charged particles that orbit around the nucleus in distinct electron shells.
The atomic number indicates the number of protons in an atom, which defines the element.
The mass number is the total count of protons and neutrons within the nucleus.

Ionic bonds form through the transfer of electrons between atoms, creating charged ions.
Covalent bonds arise when atoms share electrons to achieve stability.
Metallic bonds occur among metal atoms, characterized by a "sea" of shared electrons.

Reactants are the starting materials in a reaction, which convert to products.
Balancing reactions necessitates that the number of atoms remains equivalent on both sides of the equation, reflecting conservation of mass.
Types of chemical reactions include:
- Synthesis: Combination of substances to form a new compound.
- Decomposition: Breakdown of a compound into simpler substances.
- Single Replacement: One element substitutes another in a compound.
- Double Replacement: Exchange of components between two compounds.
- Combustion: Reaction involving oxygen that produces heat and light.

Solids feature a definite shape and volume, with particles closely packed together.
Liquids have a definite volume but adapt to the shape of their container, with particles less tightly packed than in solids.
Gases lack a fixed shape or volume; particles are widely spaced and move freely.

Acids donate protons (H+) in solution, resulting in a pH less than 7.
Bases accept protons or release hydroxide ions (OH-), yielding a pH greater than 7.
The pH scale ranges from 0 (strong acids) to 14 (strong bases), measuring the acidity or basicity of a solution.

Solutions are homogeneous mixtures of a solute dissolved in a solvent.
Concentration refers to the amount of solute in a certain volume of solution, commonly expressed in molarity (M).
Solubility is the maximum amount of solute that can dissolve in a solvent at a specified temperature.

Energy represents the ability to perform work and can exist as thermal energy (heat).
Endothermic reactions absorb heat from their surroundings.
Exothermic reactions release heat into their surroundings.

Groups or families are vertical columns of elements sharing similar chemical properties.
Periods are horizontal rows representing elements with increasing atomic numbers.
Elements are categorized into metals, nonmetals, and metalloids based on their physical and chemical properties.

Boyle's Law states that pressure and volume are inversely related when temperature is constant.
Charles's Law expresses that volume and temperature are directly related at constant pressure.
The Ideal Gas Law is articulated as PV = nRT, connecting pressure (P), volume (V), number of moles (n), gas constant (R), and temperature (T) in Kelvin.

The mole concept establishes that 1 mole equals 6.022 x 10²³ particles, facilitating the counting of atoms and molecules.
The mole ratio, obtained from balanced chemical equations, allows conversion between moles of reactants and products.