Chapter 1: Matter, ENERGY and Measurement

Chapter 1 GIOs (General Instructional Objectives)

Section 1.1. The Study of Chemistry

1. Why study chemistry?

a. Define chemistry, explain why it's the central science and what chemistry (and thus, chemists) seek to understand or accomplish.

b. Provide specific reasons why chemistry ought to be studied and how chemistry specifically impacts our society.

2. Atomic and Molecular Perspective of Chemistry

a. Define matter and the role of properties in distinguishing matter from other matter.

b. Provide examples of what is and is not matter.

c. Distinguish between elements, atoms and molecules.

d. Explain the importance of using micro (or submicro) scopic models to predict and explain the behavior of the macroscopic realm. A critical skill as a chemist is to be able to visualize matter and to use models of atoms and molecules (figure 1.1) to explain why substances do what they do i.e. how does ethanol's molecular structure and composition affect its properties and what it does or doesn't do in the macroscopic world.

Section 1.2. Classifications of Matter

1. States of Matter

a. Describe specific properties of the three traditional states of matter (solid, liquid, gas)

b. Illustrate the differences (at the molecular level) between the states of matter.

2. Pure Substances

a. Define pure substance and differentiate between a pure substance and a mixture.

3. Elements

a. Define element and know how to properly write an element's symbol.

4. Compounds

a. Define compound and provide examples of a compound.

b. State the law of definite proportions and how it is applied and used in chemistry.

5. Mixtures

a. define mixture and provide examples of a mixture.

b. Be able to classify matter Use figure 1.9 as a study guide and visual aide!!

Section 1.3. Properties of Matter

1. Differentiate between physical and chemical properties (and give examples of each).

2. Physical and Chemical Changes

a. explain the difference between physical and chemical changes and provide examples of each.

3. Separation of Mixtures

a. Describe methods to separate a mixture. There is an ACT-type passage on Exam 1 over fractional distillation and lab 1 involves chromatography.

Section 1.4. The Nature of Energy

1. Define energy, work, heat and force.

2. Differentiate between potential and kinetic energy.

Section 1.5. Units of Measurement

1. Differentiate between quantitative and qualitative data.

2. Explain how the scientific method works.

a. Differentiate between a theory and a law.

b. Explain how the scientific method is used to gain knowledge about the natural world.

3. SI Units

a. know the SI base units (table 1.4) (you will not need to memorize them, but will have to use it!)

b. know the prefixes used in the metric system (table 1.5) (you will not need to memorize this them, but will have to use it!)

c. define mass.

4. Temperature

a. define temperature and how it is not heat.

5. Volume

a. define volume.

b. be able to calculate volume using various methods and units.

6. Density

a. define density.

b. be able to calculate and determine the density of objects.

7. Unit Conversions

a. be able to calculate metric and English unit conversions i.e. feet to meters, etc.

Section 1.6. Uncertainty in Measurement

1. Know that uncertainty always exist in measurement!

2. Accuracy v. Precision

a. know the difference between accuracy and precision

b. know how to improve both your accuracy and precision in an experiment.

Section 1.7. Dimensional Analysis

1. Be able to complete problems involving dimensional analysis by showing all work.

Lab 1: Chromatography

Be able to interpret the results of a chromatography lab i.e. identify which substances traveled the fastest (or slowest) up the chromatography paper, use the rf value to determine the identity of an unknown mixture, use tables to match rf value to the identity of an unknown mixture. Note: practice for this objective by completing the Chapter 1 Self Quiz (which contains the exact ACT-type passage you will be provided).

Lab 2: Mass/Charge of an Electron