Stoichiometry Quiz

Stoichiometry

• Definition: Stoichiometry is the study of the quantitative relationships between reactants and products in chemical reactions.
• Key Concepts:
  • Moles: a unit of measurement that represents 6.022 x 10^23 particles (atoms or molecules)
  • Molar Mass: the mass of one mole of a substance (in grams)
  • Empirical Formula: the simplest whole-number ratio of atoms in a compound
  • Molecular Formula: the actual number of atoms in a molecule
• Stoichiometric Calculations:
  • Mole-Mole Calculations: relate the number of moles of reactants to the number of moles of products
  • Mass-Mass Calculations: relate the mass of reactants to the mass of products
  • Limiting Reactant: the reactant that determines the amount of product formed
  • Percent Yield: the percentage of the theoretical amount of product that is actually formed

Atomic Structure

• Atomic Model:
  • Rutherford Model: an atom consists of a small, dense nucleus surrounded by electrons
  • Bohr Model: electrons occupy specific energy levels (shells) around the nucleus
• Subatomic Particles:
  • Protons: positively charged particles in the nucleus
  • Neutrons: particles with no charge in the nucleus
  • Electrons: negatively charged particles that orbit the nucleus
• Atomic Number and Mass Number:
  • Atomic Number (Z): the number of protons in an atom's nucleus
  • Mass Number (A): the sum of protons and neutrons in an atom's nucleus
• Isotopes: atoms of the same element with different mass numbers (different number of neutrons)
• Electron Configuration:
  • Valence Electrons: electrons in the outermost energy level
  • Core Electrons: electrons in the inner energy levels
  • Aufbau Principle: electrons occupy the lowest available energy level
  • Hund's Rule: electrons occupy degenerate orbitals with parallel spins

Stoichiometry

• Stoichiometry is the study of quantitative relationships between reactants and products in chemical reactions.
• A mole (mol) is a unit of measurement that represents 6.022 x 10^23 particles (atoms or molecules).
• Molar mass is the mass of one mole of a substance, measured in grams.
• Empirical formula is the simplest whole-number ratio of atoms in a compound.
• Molecular formula is the actual number of atoms in a molecule.
• Stoichiometric calculations involve mole-mole and mass-mass calculations.
• Mole-mole calculations relate the number of moles of reactants to the number of moles of products.
• Mass-mass calculations relate the mass of reactants to the mass of products.
• Limiting reactant is the reactant that determines the amount of product formed.
• Percent yield is the percentage of the theoretical amount of product that is actually formed.

Atomic Structure

• The Rutherford Model of the atom consists of a small, dense nucleus surrounded by electrons.
• The Bohr Model of the atom states that electrons occupy specific energy levels (shells) around the nucleus.
• Protons are positively charged particles in the nucleus of an atom.
• Neutrons have no charge and are found in the nucleus of an atom.
• Electrons are negatively charged particles that orbit the nucleus of an atom.
• Atomic number (Z) is the number of protons in an atom's nucleus.
• Mass number (A) is the sum of protons and neutrons in an atom's nucleus.
• Isotopes are atoms of the same element with different mass numbers (different number of neutrons).
• Electron configuration involves the arrangement of electrons in energy levels around the nucleus.
• Valence electrons are electrons in the outermost energy level.
• Core electrons are electrons in the inner energy levels.
• The Aufbau Principle states that electrons occupy the lowest available energy level.
• Hund's Rule states that electrons occupy degenerate orbitals with parallel spins.