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  1. 1. WHAT IS CHEMISTRY?QBA Miguel A. Castro Ramírez
  2. 2. WHAT IS CHEMISTRY? Chemistry is the study of matter and the transformations it undergoes. What is matter? – Anything that has mass and takes up space.
  3. 3. IMPORTANCE OF CHEMISTRY Chemistry is all around you. – Air you breathe – Food you digest – Clothes you wear – Textbook you read Chemistry is often said to be the central science.
  4. 4. SCIENCE V.S. TECHNOLOGY How is science different from technology? Science: – Experimental investigation and exploration of natural phenomena – Pursues knowledge for its own sake – Does not cause change in itself Technology – The practical application of scientific knowledge – Leads to change (for better or for worse)
  5. 5. SCIENCE V.S. TECHNOLOGY (Cont) Examples of science: – What causes the flu? – How are atoms put together? – How is genetic information stored and transmitted? Examples of technology – Flu vaccine – Atomic bomb – Genetic engineering
  6. 6. SCIENTIFIC METHOD Step 1: Make observations – Example: I am sick with a stomachache. Step 2: Develop a hypothesis – Example: I am sick due to the spoiled food I ate for lunch. Step 3: Test hypothesis through experiments – Example: Ask others who ate the same food for lunch if they got sick.
  7. 7. SCIENTIFIC METHOD (Cont) Step 4: Develop a law – Law: Summarizes the outcome of several experiments that occur repeatedly and consistently. – Example: The spoiled food served at lunch makes people sick with a stomachache. Step 5: Develop a theory – Theory: Explanation for a why a law exists. – Example: It is the bacteria in the spoiled food that makes people ill.
  8. 8. SCIENTIFIC METHOD (Cont) Theories – Are never completely certain – May change as more experiments are performed. – A model is a physical picture or mathematical expression of a theory.  Example: Model of the atom The scientific method must be free of bias.
  10. 10. ELEMENTS Elemental substances contain only one type of atom Elements are the building blocks of matter There are 115 known elements today, 90 which occur naturally The periodic table displays the elements
  11. 11. ELEMENTS (Cont) Each element has a unique symbol – The first letter is always capitalized, the second letter is always lower case  Fluorine is F, not f  Cobalt is Co, not CO (which is carbon monoxide) The smallest unit of an element is the atom
  12. 12. COMPOUNDS Pure substances containing more than one different element. – NaCl (table salt)  Contains sodium (Na) and chlorine (Cl)  NaCl is the chemical formula – H2O (water)  Contains 2 atoms of hydrogen (H) and 1 atom of oxygen (O)  H2O is the chemical formula Elements in compounds are combined in a definite ratio – H2O is water but H2O2 is hydrogen peroxide
  13. 13. COMPOUNDS (cont) Are H2 and O3 considered elements or compounds? Why?
  14. 14. CLASSIFICATION OF MATTERClassify the following as an element, compound, homogeneous mixture, or heterogeneous mixture. a. Fog b. Gasoline c. Helium d. Sulfuric acid (H2SO4) e. Orange juice from squeezed oranges
  15. 15. STATES OF MATTER Solid Liquid Gas Copyright © 2005 by Pearson Education, Inc. Publishing as Benjamin Cummings
  17. 17. CHANGES IN STATE Melting: Solid to liquid Boiling: Liquid to gas Sublimation: Solid to gas – The above three require input of energy Condensation: Gas to liquid Freezing: Liquid to solid Deposition: Gas to solid – The above three release energy
  18. 18. PHYSICAL CHANGES Do not alter the chemical identity of the substance – Examples include:  Any change in the state of matter (e.g. freezing or boiling water)  Sawing wood  Crushing a tablet  Bending a wire  Dissolving salt in water
  19. 19. PHYSICAL PROPERTIES Characterize the physical state and physical behavior of a substance Each substance has unique physical properties Examples – Sulfur appears as a yellow powder – The boiling point of water is 100 oC – Carbon monoxide is odorless
  20. 20. CHEMICAL CHANGES Changes the identity of the substance as the chemical composition changes. – Also called chemical reactions Examples: – Tarnishing of silver (Ag forms AgS) – Rusting of iron (Fe forms Fe2O3)
  21. 21. CHEMICAL REACTIONS Are expressed using chemical equations. Rusting of iron: 4 Fe + 3 O2  2 Fe2O3 (rust) reactants products Meaning: Four atoms of iron react with three molecules of oxygen to form two molecules of rust
  22. 22. CHEMICAL REACTIONS (Cont)Zn + 2 HCl  ZnCl2 + H2Zinc hydrochloric acid zinc chloride hydrogen gasMeaning: One atom of zinc reacts with two molecules of hydrochloric acid to produce one molecule of zinc chloride and one molecule of hydrogen gas.
  23. 23. CHEMICAL PROPERTIES Describe ways pure substances behave when interacting with other pure substances. Examples – Iron reacts with oxygen to form rust. – Platinum does not react with oxygen at room temperature.
  24. 24. PRACTICE PROBLEMIdentify the following properties andchanges as physical or chemical. a. The copper sheets that form the “skin” of the Statue of Liberty have acquired a greenish coating over the years. b. Carbon appears as black powder. c. Adding food coloring to water. d. Wood burns in air.