Basics of Chemistry Quiz

Definition: The study of matter, its properties, composition, and changes it undergoes.
Branches:
- Organic Chemistry: Study of carbon-containing compounds.
- Inorganic Chemistry: Study of inorganic compounds, including metals and minerals.
- Physical Chemistry: Study of the physical properties and changes of matter.
- Analytical Chemistry: Techniques for analyzing substances to determine their composition.
- Biochemistry: Study of chemical processes within and related to living organisms.

Organization: Elements are arranged by atomic number and grouped by similar properties.
Groups: Vertical columns; elements in the same group share similar chemical behaviors.
Periods: Horizontal rows; represent energy levels of electrons.

Ionic Bonding: Transfer of electrons from one atom to another, resulting in charged ions.
Covalent Bonding: Sharing of electrons between atoms.
Metallic Bonding: Sea of electrons shared among a lattice of metal atoms.

Reactants: Substances that undergo a change.
Products: New substances formed from the reaction.
Types of Reactions:
- Synthesis: Two or more reactants combine to form a product.
- Decomposition: A single compound breaks down into two or more products.
- Single Replacement: An element replaces another in a compound.
- Double Replacement: Exchange of ions between two compounds.
- Combustion: Reaction with oxygen, producing heat and light.

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

Acids: Substances that donate protons (H⁺ ions); pH less than 7.
Bases: Substances that accept protons or donate hydroxide ions (OH⁻); pH greater than 7.
pH Scale: Measures acidity or alkalinity; ranges from 0 (acidic) to 14 (basic).

Definition: Study of the quantitative relationships in chemical reactions.
Mole Concept: 1 mole = 6.022 x 10²³ particles (Avogadro's number).
Balancing Equations: Ensures the law of conservation of mass; number of atoms on reactant side = number on product side.

Concentration: Amount of solute in a given volume of solution.
Equilibrium: State in which the forward and reverse reactions occur at the same rate.
Catalysts: Substances that speed up reactions without being consumed.

Chemistry studies matter, its properties, composition, and changes.
Organic Chemistry focuses on carbon-containing compounds.
Inorganic Chemistry deals with inorganic compounds, such as metals and minerals.
Physical Chemistry examines physical properties and changes of matter.
Analytical Chemistry involves techniques for substance composition analysis.
Biochemistry investigates chemical processes within living organisms.

Atoms are the fundamental units of matter, consisting of protons, neutrons, and electrons.
Protons are positively charged and located in the nucleus.
Neutrons, found in the nucleus, have no charge.
Electrons are negatively charged and orbit around the nucleus.
The atomic number signifies the number of protons and uniquely identifies an element.
The mass number is the sum of protons and neutrons in an atom.

Elements are organized according to atomic number and grouped by similar properties.
Groups are vertical columns where elements exhibit similar chemical behaviors.
Periods are horizontal rows corresponding to energy levels of electrons.

Ionic bonding involves the transfer of electrons, resulting in charged ions.
Covalent bonding entails the sharing of electrons between atoms.
Metallic bonding consists of a "sea of electrons" shared in a lattice of metal atoms.

Reactants are substances that undergo transformation while products are new substances formed.
Synthesis reactions involve combining multiple reactants to form a product.
Decomposition reactions occur when a single compound breaks down into multiple products.
Single replacement reactions feature one element replacing another in a compound.
Double replacement reactions involve an exchange of ions between two compounds.
Combustion reactions react with oxygen, generating heat and light.

Solids possess a definite shape and volume with particles closely packed together.
Liquids have a definite volume but take the shape of their container, with closely packed particles that can move past one another.
Gases do not have a definite shape or volume; particles are far apart and move freely.

Acids give away protons (H⁺ ions) with a pH lower than 7.
Bases accept protons or donate hydroxide ions (OH⁻) with a pH above 7.
The pH scale ranges from 0 (acidic) to 14 (basic) to measure acidity and alkalinity.

Stoichiometry studies the quantitative relationships in chemical reactions.
One mole equals 6.022 x 10²³ particles, referred to as Avogadro's number.
Balancing equations maintains the law of conservation of mass, ensuring equal atom counts for reactants and products.

Thermochemistry focuses on heat changes during chemical reactions.
Exothermic reactions, such as combustion, release heat.
Endothermic reactions, like photosynthesis, absorb heat from their surroundings.

Concentration indicates the amount of solute in a solution's volume.
Equilibrium describes a state where forward and reverse reactions occur at identical rates.
Catalysts enhance reaction rates without being consumed in the process.