LtCol W.G. Wickun, USMC (Ret) Native of Connecticut B. S. in Chemistry, Virginia Military Institute USMC, Regular Commission M.S. in Chemistry, Virginia Commonwealth University Began teaching at MECEP Prep Taught chemistry at Norwich University, Vermont Adjunct Faculty, State University of New York (SUNY) Ph.D. in Physical Chemistry, SUNY Taught chemistry at Whitworth College, Spokane, WA Teach chemistry and physics at Montana State University PT, cycling (mountain & road), backpacking, fly fishing, zymurgy

Chemistry

Introduction: Matter and Measurement Chapter 1

1. Matter - anything that occupies space and has mass. 2. Substance - a form of matter that has a definite composition and distinct properties. Chemistry - the study of matter and the changes it undergoes water, ammonia, sucrose, gold, oxygen

Mixture - a combination of two or more substances in which the substances retain their distinct identities. 1. Homogenous mixture – composition of the mixture is the same throughout. 2. Heterogeneous mixture – composition is not uniform throughout. soft drink, milk, solder cement, muddy water, iron filings in sand (Fig. 1.8)

Physical means can be used to separate a mixture into its pure components. magnet Also:filtration (Figure 1.12); paper chromatography (Figure 1.14) Distillation Figure 1.13

Element - a substance that cannot be separated into simpler substances by chemical means. 115 elements have been identified 83 elements occur naturally on Earth gold, aluminum, lead, oxygen, carbon 32 elements have been created by scientists technetium, americium, seaborgium

Table 1.2

Compound - a substance composed of atoms of two or more elements chemically united in fixed proportions. (Table 1.3) Compounds can only be separated into their pure components (elements) by chemical means. Water (H 2 O)Glucose (C 6 H 12 O 6 ) Ammonia (NH 3 )

Figure 1.9

States of Matter

Physical or Chemical? Physical change - does not alter the composition or identity of a substance. Chemical change - alters the composition or identity of the substance(s) involved: ice melting sugar dissolving in water Hydrogen gas burns in oxygen gas to form water (Fig. 1.10) Copper reacts with nitric acid to produce nitrogen dioxide (Fig. 1.11)

H2H2 O2O2 H2OH2O

Figure 1.7 Electrolysis of water

H2H2 O2O2 CathodeAnode