Reaction nomenclature.

Stoichiometry is a toolbox for describing chemical change that employs the mass quantity relationships between reactants and products.

In the earlier chapters of Atomic Theory, Periodic Properties, Chemical Bonding, and Intermolecular Forces, we discussed the structure of matter and some of the changes in structure that can occur at the atomic, molecular, or intermolecular level. It is important to remember, however, that Chemistry is a laboratory practice, and the scale of the laboratory is much larger than atoms and molecules. In order to describe the measurable relationships governing chemical change, a system of accounting is necessary which describes the products and reagents in chemical equations in measurable terms like mass and moles. Stoichiometry describes the body of accounting techniques for the purpose of describing chemical reactions at the laboratory scale.

It is the right stage of the course to take the time to cover Stoichiometry. Already this week in the Main Sequence, we have learned how to describe the most basic kind of physical thermodynamic system, an Ideal Gas within its surroundiongs, and now we need to equip ourselves with Stoichiometry to begin building the bridge to systems composed of real substances and the chemical reactions such systems may undergo.

Stoichiometric problem solving is a major focus during the first semester of General Chemistry, and many students get the impression of chemistry as an endless variation on plugging and chugging grams and moles, and their conceptual understanding of chemistry can suffer. Although this type of problem solving is relatively minor on the MCAT (MCAT physical science questions are much more likely to involve conceptual reasoning than number crunching), there will be enough stoichiometric terminology to prevent from achieving a superior score if they don't understand it. You definitely need to understand stoichiometric nomenclature and the basics of stoichiometric problem solving for the MCAT.

WikiPremed Resources




Stoichiometry Practice Items
Problem set for Stoichiometry in PDF format

Answer Key
Answers and explanations

Stoichiometry Images
Image gallery for study with links to larger teaching JPEGs for classroom presentation

Question Drill for Stoichiometry
Conceptual Vocabulary Self-Test

Basic Terms Crossword Puzzle

Basic Puzzle Solution

Learning Goals

Proficiency 

Read chemical equations fluently. Understand the meaning of element symbols, coefficients, reaction conditions, reaction arrows and substance state symbols.

Distinguish empirical and molecular formulas.

Be able to solve percent composition problems.

Answer the question 'What is a Mole?' in clear simple terms. Explain the usefulness of the concept.

Understand how to balance chemical equations.

Confidently solve percent yield and limiting reagent problems.

Suggested Assignments

Warm up with a question drill on conceptual vocabulary in stoichiometry. To make sure you have the basic vocabulary down try to complete the fundamental terms crossword puzzle without pausing. Here is the solution to the puzzle.

Perform the Wikipremed practice items for stoichiometry. Here is the answer key for the practice items.

Review the stoichiometry web resources.

Conceptual Vocabulary for Stoichiometry

Stoichiometry
Stoichiometry is the calculation of quantitative relationships of the reactants and products in chemical reactions.
Mole
The mole is the SI base unit that measures an amount of substance, equal to Avogadro's number of entities.
Gram
Although the definition is more formal now, the gram was originally defined as the absolute weight of a volume of pure water equal to the cube of the hundredth part of a metre, and at the temperature of melting ice.
Reagent
A reactant or reagent is a substance consumed during a chemical reaction.
Product
A product is a substance that forms as a result of a chemical reaction.
Chemical reaction
A chemical reaction is a process that results in the interconversion of chemical substances.
Avogadro number
Avogadro's number is the number of entities in one mole
Chemical equation
A chemical equation is a symbolic representation of a chemical reaction.
Conservation of mass
The law of conservation of mass states that the total amount of matter within a closed system will remain constant, regardless of the processes acting inside the system.
Molecular mass
The molecular mass of a substance is the mass of one molecule of that substance, relative to the unified atomic mass unit (equal to 1/12 the mass of one atom of carbon-12).
Atomic mass
The atomic mass is the mass of an atom at rest, most often expressed in unifed amu.
Yield
Yield is the amount of product obtained in a chemical reaction.
Limiting reagent
The limiting reagent is the chemical that determines how far a reaction would go because the chemical in question is the reagent that would get completely used up, causing the reaction to stop.
Gram atomic mass
Gram atomic mass is the mass in grams of one mole of atoms in an element.
Chemical formula
A chemical formula is a concise way of expressing information about the atoms that constitute a particular chemical compound.
Structural formula
The structural formula of a chemical compound is a graphical representation of the molecular structure showing how the atoms are arranged.
Law of definite proportions
The law of definite proportions states that a chemical compound always contains exactly the same proportion of elements by mass.
Empirical formula
The empirical formula of a chemical compound is a simple expression of the relative number of each type of atom in it.
Equivalent
The equivalent is a measurement unit used in chemistry and the biological sciences, which measures of a substance's ability to combine with other substances, an expression frequently used in the context of normality.
Atom economy
Atom economy describes the conversion efficiency of a chemical process in terms of all atoms involved.
Gram equivalent
A gram equivalent is the mass in grams of a compound's equivalent weight.
Amedeo Avogadro
Lorenzo Avogadro (1776 - 1856) was an Italian scientist most noted for his contributions to the theory of molarity and molecular weight.
Law of multiple proportions
The law of multiple proportions, sometimes called Dalton's Law, states that if two elements form more than one compound between them, then the ratios of the masses of the second element which combine with a fixed mass of the first element will be ratios of small whole numbers.
Non-stoichiometric compound
Non-stoichiometric compounds are chemical compounds with an elemental composition that cannot be represented by a ratio of well-defined natural numbers, and therefore violate of the law of definite proportions.
Equivalent weight
Equivalent weight is the amount of an element that reacts with 1 mole of electrons.
Mass balance
A mass balance is an application of conservation of mass to the analysis of physical systems.