Atomic Structure and Periodic Table Quiz

Atomic Structure

• Atoms are the fundamental building blocks of matter.
• Atoms consist of a nucleus containing positively charged protons and electrically neutral neutrons, surrounded by negatively charged orbiting electrons.
• The number of protons determines the element's atomic number.
• The mass number is the sum of protons and neutrons.
• Isotopes are atoms of the same element with different numbers of neutrons and thus, different mass numbers.
• Atomic orbitals describe the probability of finding an electron in a specific region around the nucleus, organized into energy levels (shells) and sublevels (subshells).
• Electron arrangement follows the Aufbau principle, Hund's rule, and the Pauli exclusion principle.

Periodic Table

• The periodic table arranges elements in order of increasing atomic number.
• Elements are grouped (vertical columns) and periods (horizontal rows).
• Elements in the same group share similar chemical properties because of similar outer shell electron configurations (valence electrons).
• Metals (left side) are typically good conductors of heat and electricity, malleable, and ductile.
• Nonmetals (right side) are usually poor conductors of heat and electricity and are brittle.
• Metalloids (along the stair-step line) exhibit properties intermediate between metals and nonmetals.

Chemical Bonding

• Chemical bonds hold atoms together to form molecules or compounds.
• Covalent bonds result from electron sharing between atoms.
• Ionic bonds form from the transfer of electrons between atoms, creating oppositely charged ions that attract each other.
• Metallic bonding involves the sharing of delocalized electrons throughout a network of metal atoms, leading to the characteristic properties of metals.
• Bonds form to achieve a more stable electron configuration.

Chemical Reactions

• Chemical reactions involve the rearrangement of atoms.
• Chemical equations represent reactions using symbols to denote reactants and products.
• The law of conservation of mass dictates that the total mass of reactants equals the total mass of products.
• Reactants undergo changes, while products are new substances created.
• Factors impacting reaction rates include temperature, concentration, surface area, and catalysts.
• Reaction types encompass synthesis, decomposition, single replacement, double replacement, and combustion.

States of Matter

• Matter exists as solids, liquids, and gases.
• Solids have fixed shape and volume due to strong intermolecular forces.
• Liquids have a fixed volume but take the shape of their container due to weaker intermolecular forces than solids.
• Gases have neither fixed shape nor volume, completely filling their container due to weak intermolecular forces.
• State changes involve energy absorption or release.

Solutions

• Solutions are homogeneous mixtures of two or more substances.
• The solute is dissolved, and the solvent does the dissolving.
• Solutions can contain dissolved solids, liquids, or gases.
• Concentration describes the amount of solute in a given amount of solution.
• Concentration can be expressed in molarity, molality, or percentage by mass.

Acids and Bases

• Acids release hydrogen ions (H+) in solution, while bases release hydroxide ions (OH-).
• The pH scale measures acidity or basicity (0 to 14).
• An acidic solution has a pH less than 7, a basic solution has a pH greater than 7, and a neutral solution has a pH of 7.
• Strong acids/bases fully dissociate in water, while weak ones partially dissociate.
• Neutralization reactions produce a salt and water when acids and bases react.

Thermodynamics

• Thermodynamics studies energy changes during chemical and physical processes.
• The first law of thermodynamics states that energy cannot be created or destroyed, only transferred or changed.
• The second law of thermodynamics states that the total entropy of an isolated system always increases.
• The third law of thermodynamics states that the entropy of a perfect crystal at absolute zero is zero.

Stoichiometry

• Stoichiometry quantifies the relationships between reactants and products in chemical reactions.
• Chemical equations allow calculating product formation or reactant consumption.
• Stoichiometry uses mole ratios to relate quantities of substances in a reaction.

Kinetics

• Chemical kinetics studies reaction rates and influencing factors.
• Reaction rates quantify the change in concentration of reactants or products over time.
• Reaction mechanisms detail the sequence of steps in a chemical reaction.
• Reaction rates depend on temperature, reactant concentration, catalysts, and surface area.