Basic Concepts of Chemistry Quiz

Definition: The study of matter, its properties, composition, structure, and the changes it undergoes.
Matter: Anything that has mass and occupies space.
Types of Matter:
- Elements: Pure substances consisting of one type of atom (e.g., Hydrogen, Oxygen).
- Compounds: Substances formed from two or more elements chemically combined (e.g., Water - H2O).
- Mixtures: Combinations of two or more substances that are not chemically bonded (e.g., Air, Salad).

Atoms: Basic units of matter, consisting of protons, neutrons, and electrons.
- Protons: Positive charge, located in the nucleus.
- Neutrons: Neutral charge, located in the nucleus.
- Electrons: Negative charge, orbiting around the nucleus.
Molecules: Two or more atoms bonded together (e.g., O2, CO2).

Ionic Bonds: Formed when one atom transfers electrons to another, resulting in oppositely charged ions (e.g., Sodium Chloride - NaCl).
Covalent Bonds: Formed when two atoms share electrons (e.g., Methane - CH4).
Metallic Bonds: Characterized by a 'sea of electrons' that are shared among a lattice of metal atoms.

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

Definition: Process where substances (reactants) are transformed into different substances (products).
Types of Reactions:
- Synthesis: A + B → AB
- Decomposition: AB → A + B
- Single Replacement: A + BC → B + AC
- Double Replacement: AB + CD → AD + CB
- Combustion: Hydrocarbon + O2 → CO2 + H2O

Definition: A mole is 6.022 x 10^23 particles (atoms, molecules, ions).
Molar Mass: The mass of one mole of a substance, expressed in grams per mole (g/mol).

Acids: Substances that donate protons (H+) in solutions (e.g., HCl).
Bases: Substances that accept protons or donate hydroxide ions (OH-) (e.g., NaOH).
pH Scale: Measures the acidity or basicity of a solution (0-14 scale).

Law of Conservation of Mass: Matter is not created or destroyed in a chemical reaction.
Atomic Theory: All matter is made up of atoms; atoms of the same element are identical.
Periodic Law: Elements are arranged by increasing atomic number, resulting in periodic trends in properties.

Organization: Elements are arranged in rows (periods) and columns (groups).
Groups: Elements in the same group have similar chemical properties (e.g., Alkali metals, Halogens).
Metals, Nonmetals, and Metalloids: Metals are typically conductive and malleable; nonmetals are not conductive; metalloids have properties of both.

Filtration: Separating solids from liquids using a filter.
Distillation: Separating mixtures based on boiling points.
Titration: Method for determining concentration of an unknown solution by reacting it with a standard solution.

Elements are pure substances consisting of one type of atom, like hydrogen or oxygen.
Compounds are formed when two or more elements combine chemically, such as H2O (water).
Mixtures combine substances without chemical bonding, like air or salad.

The fundamental unit of matter is the atom.
Atoms consist of protons, neutrons, and electrons.
Protons are positively charged and located in the nucleus.
Neutrons have no charge and are also located in the nucleus.
Electrons are negatively charged and orbit the nucleus.
Molecules are formed by two or more atoms bonding together, e.g., O2 (oxygen) and CO2 (carbon dioxide).

Ionic bonds form when one atom transfers electrons to another, creating oppositely charged ions. This happens in compounds like sodium chloride (NaCl).
Covalent bonds occur when two atoms share electrons, as seen in methane (CH4).
Metallic bonds are characterized by a "sea of electrons" shared among a lattice of metal atoms.

Solids maintain a definite shape and volume due to tightly packed particles.
Liquids have a definite volume but take the shape of their container because particles are loosely packed.
Gases have no definite shape or volume and their particles are far apart, moving freely.

During a chemical reaction, substances called reactants transform into different substances called products.
Types of reactions include:
- Synthesis: A + B → AB
- Decomposition: AB → A + B
- Single Replacement: A + BC → B + AC
- Double Replacement: AB + CD → AD + CB
- Combustion: Hydrocarbon + O2 → CO2 + H2O

A mole represents 6.022 x 10^23 particles (atoms, molecules, or ions).
Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol).

Acids donate protons (H+) in solutions, such as hydrochloric acid (HCl).
Bases accept protons or donate hydroxide ions (OH-), like sodium hydroxide (NaOH).
The pH scale measures the acidity or basicity of a solution, ranging from 0 (most acidic) to 14 (most basic).

The Law of Conservation of Mass states that matter cannot be created nor destroyed during a chemical reaction.
The Atomic Theory explains that all matter is composed of atoms and that atoms of the same element are identical.
The Periodic Law organizes elements by increasing atomic number, leading to predictable trends in their properties.

Elements are arranged in rows called periods and columns called groups.
Elements within the same group share similar chemical properties, like the alkali metals or halogens.
Elements are classified as metals, nonmetals, or metalloids.

Filtration separates solids from liquids using a filter.
Distillation separates mixtures based on their boiling points.
Titration determines the concentration of an unknown solution by reacting it with a solution of known concentration.