The Foundations of Chemistry

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Presentation transcript:

The Foundations of Chemistry CHAPTER ONE The Foundations of Chemistry

CHAPTER 1 The Foundations of Chemistry The rose on the right is in an atmosphere of sulfur dioxide, SO2. Gaseous SO2 and aqueous solutions of HSO3- and SO32- ions are used as bleaching agents. A similar process is used to bleach wood pulp before it is converted to paper.

Why is lemon often added to seafood? The odor that we associate with fish is due to the presence of amines. That is one reason why lemon is often added to seafood. The citric acid (a weak acid) neutralizes the odor of the amines.

Treatment of cancer Platinum

Matter and Energy - Vocabulary Chemistry Science that describes matter – its properties, the changes it undergoes, and the energy changes that accompany those processes Matter Anything that has mass and occupies space. Energy The capacity to do work or transfer heat.

States of Matter Solids

States of Matter Solids Liquids

States of Matter Solids Liquids Gases

Chemical and Physical Properties Chemical Properties - chemical changes rusting or oxidation chemical reactions Physical Properties - physical changes changes of state density, color, solubility Extensive Properties - depend on quantity (mass, volume) Intensive Properties - do not depend on quantity (color, temperature, density, melting point, etc.)

Chemical and Physical Properties Chemical Properties - chemical changes rusting of iron Fe + O2 Fe2O3 Burning gasoline C8H18 + O2 CO2 + H2O unbalanced unbalanced

Label each of the following as either a physical process or a chemical process?

Label each of the following as either a physical process or a chemical process?

Exothermic…Endothermic (a) Combustion is an exothermic process in which a chemical reaction releases heat. (b) The freezing of water is an exothermic process. Heat must be removed from the molecules in the liquid state to cause solidification. (c) The melting of ice is an endothermic process. The system requires heat to break the attractive forces that hold solid water together.

Exothermic…Endothermic (d) The boiling of water is an endothermic process. Molecules of liquid water must absorb energy to break away from the attractive forces that hold liquid water together in order to form gaseous molecules. (e) The condensing of steam is an exothermic process. The heat stored in water vapor must be removed for the vapor to liquefy. The condensation process is the opposite of boiling which requires heat.

Exothermic…Endothermic Water EXO EXO ENDO ENDO Ice Steam

Take-Home Vocabulary Endothermic: Describes processes that absorb heat energy. Exothermic: Describes processes that release heat energy. Energy: The capacity to do work or transfer heat.

Mixtures, Substances, Compounds, and Elements matter in which all samples have identical composition and properties Elements substances that cannot be decomposed into simpler substances via chemical reactions Elemental symbols found on periodic chart (Table 1-2)

Mixtures, Substances, Compounds, and Elements substances composed of two or more elements in a definite ratio by mass can be decomposed into the constituent elements Water is a compound that can be decomposed into simpler substances – hydrogen and oxygen

Mixtures, Substances, Compounds, and Elements composed of two or more substances homogeneous mixtures: e.g. solution (dissolved salt + water, brass, etc.) heterogeneous mixtures: e.g. soil (rocks, clay, organic matter, etc.)

Mixtures, Substances, Compounds, and Elements Matter Physical Change Pure Substance Mixture Chemical Change Homogeneous Mixture Heterogeneous Mixture Compound Element

Flow-Chart for Gasoline Mixture Homogeneous Mixture

Flow-Chart for Ink Ink Mixture Homogeneous Mixture

Flow-Chart for a Coin Coin Mixture Homogeneous Mixture

Flow-Chart for Seawater Mixture Homogeneous Mixture

Flow-Chart for CaCO3 CaCO3 Pure Substance Compound

Flow-Chart for Aluminum Foil Pure Substance Element

Flow-Chart for Toothpaste Mixture Heterogeneous Mixture

Classify each of the following as a homogeneous or a heterogeneous mixture? You do it ! Muddy river water Sugar dissolved in water

Take-Home Vocabulary Chemical change: A change in which one or more new substances are formed. Physical change: A change in which a substance changes from one physical state to another, but no substances with different compositions are formed.

Take-Home Vocabulary Mixture: A sample of matter composed of variable amounts of two or more substances, each of which retains its identity and properties. Heterogeneous mixture: A mixture that does not have uniform composition and properties throughout. Homogeneous mixture: A mixture that has uniform composition and properties throughout.

Measurements in Chemistry Quantity Unit Symbol length meter m mass kilogram kg time second s current ampere A temperature Kelvin K amt. substance mole mol

Measurements in Chemistry Metric Prefixes Name Symbol Multiplier mega M 106 kilo k 103 deka da 10 deci d 10-1 centi c 10-2

Measurements in Chemistry Metric Prefixes Name Symbol Multiplier milli m 10-3 micro  10-6 nano n 10-9 pico p 10-12 femto f 10-15

Density and Specific Gravity density = mass/volume What is density? Why does ice float in liquid water?

Density and Specific Gravity Example 1: Calculate the density of a substance if 742 grams of it occupies 97.3 cm3.

Density and Specific Gravity Example 1: Calculate the density of a substance if 742 grams of it occupies 97.3 cm3.

Density and Specific Gravity Example 2: Suppose you need 125 g of a corrosive liquid for a reaction. What volume do you need? liquid’s density = 1.32 g/mL You do it!

Density and Specific Gravity Water’s density is essentially 1.00 at room T. Thus the specific gravity of a substance is very nearly equal to its density. Specific gravity has no units.

Density and Specific Gravity Example 3: A 31.10 gram piece of chromium is dipped into a graduated cylinder that contains 5.00 mL of water. The water level rises to 9.32 mL. What is the specific gravity of chromium? You do it

Reading…. Please read section 1-12: HEAT AND TEMPERATURE

End of Chapter 1

Reading…. CHAPTER II Page 46 - 87