Unit 1

Chemistry is the study of matter (physical stuff) and its behavior and interactions.  In our first topic, matter and measurements, you will learn how matter is described or classified, as well as the different ways matter can change or interact with other matter in different conditions.  As a science, the body of knowledge known to is as chemistry was developed using the scientific method, so we will next briefly review the scientific method.  This topic will then shift to ideas and concepts of measurement of properties of matter and a (hopefully) review of calculational tools we will use for the rest of the semester.

In the next topic, atoms, molecules, and ions, we will continue our look at matter begun in the previous topic, building on the large scale, macroscopic view discussed in the previous topic and quickly moving down to the smallest particles of matter — atoms, molecules and ions.

The unit will end with the topic of stoichiometry.  In the study of stoichiometry, you will learn ways to quantify amounts of substances as well as relationships between amounts (and masses) of substances that combine or react in chemical reactions.

Additionally, the first unit includes an introduction/review of chemical formulas and nomenclature (a set of rules for naming chemical compounds).  This will be essential as chemical formulas and names comprise the language of chemistry and is therefore needed for you to effectively study chemistry this semester.

Unit 1 Learning Objectives

Purpose of the Learning Objectives:

This is the list of learning objectives for Unit 1 from the course syllabus.  I know, it is long.  I don’t expect you to read it now before studying.  So how should you use it? Think of it as:

  1. An outline of the course and the material you will be studying in Unit 1 (and tested on the Unit 1 Exam).
  2. A list of things you should be able to do to demonstrate to me (and more importantly, yourself) that you have a good grasp of these concepts and skills in chemistry.  This will serve as a good review checklist – as you study for Exam 1, it’s worth giving these items a look to see if you can do them – if you can, you are likely well prepared.  If you can’t, that’s where you should focus your study and get help if needed.

Matter and Measurement

 

  1. Differentiate among the three states of matter:  gas, liquid, and solid.
  2. Distinguish among pure substances, compounds, elements, mixtures, heterogeneous, homogeneous and solutions.
  3. Distinguish between a physical or chemical change.
  4. Distinguish among hypothesis, theory, and law.
  5. Knowing the meaning of the prefixes used in the metric system, convert a value in one metric unit to another.
  6. Knowing that 2.54 cm = 1 in., 1.06 quarts = 1 liter and 1 lb = 454 grams, convert between English and Metric units.
  7. Interconvert degrees Fahrenheit, Celsius and Kelvin.
  8. Using the density formula, solve for density, mass or volume given the other two.
  9. Differentiate between exact numbers and measurements.
  10. Define and distinguish between precision and accuracy.
  11. Determine the correct number of significant figures in a measured or calculated quantity.
  12. Round off numbers to the correct number of significant figures.
  13. Express numbers and do calculations in exponential notation.
  14. Use dimensional analysis to solve unit conversion problems.
  15. Given the formula, name the elements and the binary compounds and vice versa (refer Nomenclature Handout: Sections I and II)

Atoms, Molecules, and Ions

  1. Apply the Law of Conservation of mass.
  2. State the basic postulates of Dalton’s Atomic Theory.
  3. Describe the studies made by Thomson, Millikan and Rutherford which helped develop our understanding of the subatomic nature of matter.
  4. Describe the composition of the atom in terms of protons, neutrons, and electrons;  describe the properties of these subatomic particles.
  5. Write the nuclear symbol of an isotope or, given the nuclear symbol, state the mass number, atomic number, and number of protons and neutrons.
  6. Given the atomic masses and the relative abundance of all the naturally occurring isotopes of an element, calculate the average atomic mass in amu.
  7. Given a periodic table, identify elements according to the following:  metals, nonmetals, transition metals, halogens, noble gases, alkali metals, alkaline earth metals, period families and groups.
  8. Given the chemical formula of any atom, ion or compound listed in the “”Formula and Nomenclature”” handout, give the name and vice versa.
  9. Identify the elements that exist as diatomic molecules.
  10. Given a molecular formula, indicate how many atoms of a given element are in the molecule.

Stoichiometry

  1. Write a balanced chemical equation from a word description of it.
  2. Identify a chemical reaction as combination, combustion, or decomposition.
  3. Given the atomic masses of all naturally occurring isotopes of an element, calculate the average atomic mass of the element in amu.
  4. Given the name or formula of an element or compound, determine its molar mass.
  5. Given a chemical formula or name, convert among moles, grams, amu, molecules and atoms.
  6. Determine the empirical formula of a compound from a molecular formula or percent composition.
  7. Given the chemical formula of a substance, calculate its percent composition.
  8. Given the empirical formula and molar mass of a compound determine its molecular formula.
  9. Calculate the mass of a particular substance produced or used in a chemical reaction.
  10. Given the amounts of two or more reactants and the chemical equation, determine the limiting reagent and the theoretical yield of the product.
  11. Given the theoretical yield and the actual yield, calculate the percent yield.

Unit 1 Topics

Study these in order:

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