Chemistry: Week of 1/19
Chemistry: Week of 1/19 20002
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This 2 page Class Notes was uploaded by email@example.com Notetaker on Saturday January 30, 2016. The Class Notes belongs to 20002 at Indiana University of Pennsylvania taught by Charles Lake in Spring 2016. Since its upload, it has received 16 views. For similar materials see Principles of Chemistry I in Chemistry at Indiana University of Pennsylvania.
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Date Created: 01/30/16
Chemistry 111 M/W 3:30-4:45 Professor Lake Week of 1/19/16 1) Elements vs. Compounds a. Element: smallest part of matter; cannot be changed or broken down b. Compound: combination of two or more different elements c. Examples i. CO 2compound ii. Hg element iii. C4 compound iv. Fe element 2) Substances and Mixtures a. Substance: definite composition that does not vary from one sample to another i. Graphite ii. Distilled water b. Mixture: variable composition that may change between samples i. Ocean ii. Atmosphere 3) Physical and Chemical Changes a. Physical: compound doesn’t change i. Melting ice b. Chemical: compound changes i. Electrolysis for water in hydrogen and oxygen 4) States of Matter a. Solid: thermal vibrations are weaker than the forces holding the molecules together i. Definite shape ii. Definite volume b. Liquid: thermal vibrations are weaker (but not as much) than the forces holding the molecules together i. Definite volume ii. No definite shape c. Gas: thermal vibration is stronger than the forces holding the molecules together i. No definite volume ii. No definite shape 5) Changes of State a. Solid liquid: melting/ Liquidsolid: freezing b. Liquidgas: evaporation/ Gas liquid: condensation c. Solidgas: sublimation/ Gas solid: deposition 6) Intensive vs. Extensive Properties of Matter a. Intensive: does not depend on the amount of matter being considered i. Density ii. Temperature iii. Boiling/freezing points iv. Color** sometimes b. Extensive: depends on the amount of matter being considered i. Mass ii. Volume iii. Length iv. Color** sometimes
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