First post! I am going to use this blog as a place to post current assignments, links to useful resources, the text of the PowerPoint presentations, and other class-related information.
This first post will summarize Chapter 2 up to today's lesson/assignment
9/28 - Friday
Section 2.1 - PPT (PowerPoint) - Notes
Section Review 2.1 (in class, collected)
Chapter 2 Practice Problems - Section 2.1 only, turn in before test
10/1 - Monday
Section 2.2 - PPT - Notes
Section Review 2.2 (in class, collected)
Textbook questions 7-12, p. 35 at the end of the notes
Chapter 2 Practice Problems - Section 2.2 only, turn in before test
10/2 - Tuesday
Section 2.3 - PPT - Notes
Section Review 2.3 (in class, collected)
Textbook questions 14-18, p. 40 at the end of the notes
Chapter 2 Practice Problems - Section 2.3 only, turn in before test
Homework: Interpreting Graphics Chapter 2 - due 10/3
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All past PowerPoint presentations are available here. Download OpenOffice (a free version of Microsoft Office) if you need to view the presentations and don't already have MS Office.
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Chapter 2 - Matter and Change
Lecture Notes 2.1 - Matter
Properties of Matter
Matter - anything that has mass and takes up space
Mass - amount of matter an object contains
Example: a golf ball has more mass than a tennis ball, therefore a golf ball contains more matter than a tennis ball.
Properties of Matter, cont.
Substance - also called “Pure Substance” contains only one type of matter
Example: sugar is all sucrose
Non-example: lemonade is not a substance - it contains different types of matter in different combinations.
Properties of Matter, cont.
Physical property - a quality of a substance that can be observed or measured without changing the composition of the substance
Examples: color, solubility, odor, hardness, density, melting point, boiling point, physical state
States of Matter
There are 3 states of matter:
Solid - has a definate shape and volume, example - ice, coal, sugar, iron
Liquid - has a definate volume, but takes the shape of the container it is in, example - water, milk, blood
Gas - takes the shape and volume of the container it is in, example - steam, air
Vapor vs. Gas
A gas is something that is in the gas form at room temperature
Vapor - the gaseous state of a substance that is generally a liquid or solid at room temperature, example - steam = water vapor because water is a liquid at room temperature.
Physical Changes
Physical Change - when matter is changed without changing its composition
Examples = phase change (ice to water to steam)
Words that imply physical change: boil, freeze, dissolve, melt, condense, break, split, crack, grind, crush, bend
Chapter 2.2
Mixtures
Classifying Mixtures
Mixture - a physical blend of two or more substances
Examples: a tossed salad (lettuce, tomatoes, dressing, etc…), blood (water, cells, other chemicals)
Types of Mixtures
Heterogeneous Mixture - not uniform in composition
Example = salad - one sample might be different from another
Types of Mixtures, cont
Homogenous Mixture - has a completely uniform composition. It’s components are evenly distributed throughout the sample
Example=salt water
Solutions and Phases
Solutions - special name given to homogeneous mixtures
Phase - any part of a system with uniform composition
Homogeneous mixture=1 phase
Heterogeneous mixture=2+ phases
Separating Mixtures
Some mixtures can be separated physically: salad can be separated by a fork
A mixture of sulfur and iron filings could be separated with a magnet
Distillation
How could we separate a homogeneous mixture of tap water and the minerals and chemicals?
Distillation - liquid is boiled to a vapor then condensed again.
Practice
Complete problems 7-12 on page 35 at the end of your notes page.
These will be checked when you turn in your notes at the end of the chapter.
Section 2.3
Elements and Compounds
Distinguishing Elements and Compounds
Elements - the simplest forms of matter that can exist under normal laboratory conditions.
Examples: hydrogen, oxygen, carbon, lead
Distinguishing Elements and Compounds, cont
Compounds - consist of 2 or more elements. Can only be separated by chemical means.
Examples: hydrogen (element) and oxygen (element) makes water (compound), sugar (sucrose) is made from oxygen, carbon, and hydrogen
Symbols and Formulas
Chemical Symbol - a one- or two-letter symbol that stands for an element.
Many chemical symbols are obvious - they are the first letter or two of the element name.
Examples: 0 = oxygen, C = carbon, He = helium
Symbols and Formulas, cont
Some elements have chemical symbols that are not related to the English name of the element.
Examples: Fe = iron, Na = sodium, Pb = lead, K = potassium
Symbols and Formulas, cont
Chemical symbols are most useful in chemical formulas. Many compounds are made of many elements and to write them all out would be difficult.
Example: the sucrose (sugar) molecule is made of 12 carbon atoms, 22 hydrogen atoms, and 11 oxygen.
To shorten this, we write C12H22O11
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