Stoichiometry Quiz

Study Notes

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 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 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.

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.