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The Science of Chemistry

The Science of Chemistry. Chapter 1 Section Reviews 1-1 (pg 9 #1-4);1-2 (pg 19 #1-4, 8); 1-3 (pg 24 #1-7); 1-4 (pg 32 #1-5). 1-1 (pg 9 #1-4). What are the common physical states of matter? The common physical states of matter are solid, liquid and gas.

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The Science of Chemistry

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  1. The Science of Chemistry Chapter 1 Section Reviews 1-1 (pg 9 #1-4);1-2 (pg 19 #1-4, 8); 1-3 (pg 24 #1-7); 1-4 (pg 32 #1-5)

  2. 1-1 (pg 9 #1-4) • What are the common physical states of matter? The common physical states of matter are solid, liquid and gas. • How do the particle models for the states of matter differ? The particles of solids are closely packed; Liquid particles are close together but free to move around; Gas particles are separated by empty space and move freely.

  3. 1-1 (pg 9 #1-4) • What is the difference between an endothermic reaction and an exothermic reaction? An endothermic reaction absorbs energy. An exothermic reaction releases energy.

  4. 1-1 (pg 9 #1-4) • In what ways do the three fundamental states of matter differ? Solids have a fixed volume and shape. Liquids have a fixed volume but can flow and take the shape of the container. Gases have no fixed shape or volume.

  5. 1-2 (pg 19 #1-4, 8) • What two physical properties characterize matter? Two physical properties that characterize matter are mass and volume. • What SI unit is usually used to express the density of liquids? Density of liquids is usually expressed in grams per milliliter (g/mL) or cubic centimeter (cm3).

  6. 1-2 (pg 19 #1-4, 8) • How does mass differ from weight? Weight is a measure of downward force due to gravitational attraction. Mass is the quantity of matter. • Why is density considered a physical property rather than a chemical property of matter? The density of a material may be observed and measured without any change in chemical nature.

  7. 1-2 (pg 19 #1-4, 8) • Perform the following conversions • Milliliters in 21.59L = 21,590 mL • Centimeters in 1.62 m = 162 cm • Nanometers in 0.064 mm = 6.4 x 104 nm • Kilograms in 2648 cg = 0.02648 kg

  8. 1-3 (pg 24 #1-7) • How does an atom differ from an element? The atom is the fundamental particle of matter; a subunit of an element. • How is an atom related to a molecule? A molecule may consist of two or more atoms of the same element or different elements.

  9. 1-3 (pg 24 #1-7) • What are allotropes? An allotrope is one of a number of molecular forms of an element. • How do you think the symbols for newly discovered elements are determined? The symbols for newly discovered elements are based on the locations of their discovery as well as on the people who discover them.

  10. 1-3 (pg 24 #1-7) • List the symbols for the following elements: a. Carbon = C b. Nitrogen = N c. Hydrogen = H d. Gold = Au e. Neon = Ne f. Astatine = At

  11. 1-3 (pg 24 #1-7) • Write the names of the elements with the following symbols: a. He = Helium b. Na = Sodium c. Cl = Chlorine d. S = Sulfur e. Mg = Magnesium f. Sb = Antimony

  12. 1-3 (pg 24 #1-7) • Why don’t we use As as the symbol for astatine? As is already in use for Arsenic.

  13. 1-4 (pg 32 #1-5) • Define the term compound. Compounds are pure substances composed of two or more elements. • What are some of the properties of an acid? Acids have a sour taste, turn blue litmus paper red, have a pH lower than 7, and react with bases and some metals to form salts.

  14. 1-4 (pg 32 #1-5) • What element do all organic compounds contain? All organic compounds contain the element carbon. • What information is shown in a molecular formula? The overall arrangement of the atoms in a molecule is shown in a structural formula.

  15. 1-4 (pg 32 #1-5) • How is a homogeneous mixture different from a heterogeneous mixture? In a heterogeneous mixture, substances are not evenly mixed. In a homogeneous mixture, the substances are uniformly mixed at the molecular level.

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