1. Introduction to Chemistry

2. Matter: Anything that has mass and volume States of Matter

3. Physical properties Properties that do not change the chemical nature of matter Boiling point Melting point Freezing point Color Density

4. Chemical Properties Properties that do change the chemical nature of matter Oxidation Oxidation Rusting of iron = Rusting of iron = Iron Oxide (FeO 2 ) Iron Oxide (FeO 2 ) pH pH Flammability Flammability Frying an egg Frying an egg

5. Physical & Chemical Changes

6. All Matter is composed of : Atoms – Means “unable to be cut” Atoms – Means “unable to be cut” The smallest particle of an element that still has the characteristics of that element The smallest particle of an element that still has the characteristics of that element

7. Elements Substances that can’t be broken down into simpler substances Substances that can’t be broken down into simpler substances 96% of human mass is made up of C, H, O, N

8. Periodic Table of The Elements

9. Atoms are made up of smaller subatomic particles Protons: positively charged (Located in the nucleus) Protons: positively charged (Located in the nucleus) Neutrons: neutrally charged (Located in the nucleus) Neutrons: neutrally charged (Located in the nucleus) Electrons: negatively charged (Located around the nucleus) Electrons: negatively charged (Located around the nucleus) Discovered by Ernest Rutherford in 1919 Discovered by J.J. Thomson in 1897 Discovered by James Chadwick in 1932

10. Each atom has the same number of protons and electrons Electrons have less mass than protons. 1 proton= 1870 electrons Electrons located farther away from the nucleus have more energy

11. Atomic number = number of protons Atomic mass = number of protons & neutrons Electron # = Proton # in Neutral elements

12. He 2 4.003 Atomic number: Atomic mass: # of Protons # of Electrons # of Neutrons

13. Isotopes Neutron #’s change Hydrogen: H 1 1 Deuterium : H 1 2 Tritium H 1 3

14. When elements combine to form substances with two or more atoms… Compounds are formed

15. Mixtures When one or more atoms are physically combined but NOT chemically combined (Individual atoms retain their own properties) Easily separated by non-chemical means

16. Solutions Solute – Substance dissolved Solute – Substance dissolved Solvent – Dissolves substances Solvent – Dissolves substances (Water is the universal solvent) (Water is the universal solvent) Colloids – light does not penetrate Colloids – light does not penetrate Suspensions Suspensions

17. Solubility of Solutions The amount of solute a solvent can dissolve The amount of solute a solvent can dissolve Solubility affected by: Temperature Temperature Concentration Concentration

18. Ions Ions are charged particles. Atoms have either lost or gained one or more electrons

19. Ionic bond CationAnion

20. Covalent Bond Occurs when atoms SHARE electrons Diatomic molecule Special Note Molecules are only formed with covalent bonds

21. Molecules A group of atoms held together by covalent bonds A group of atoms held together by covalent bonds Water, hydrogen gas, oxygen, carbon dioxide Water, hydrogen gas, oxygen, carbon dioxide

23. Uneven distribution of electrons results in a polar molecule

24. Hydrogen Bond A bond formed in polar molecules

25. Cohesion & Adhesion: Due to Hydrogen Bonding Cohesion – The ability of hydrogen bonds to attract like molecules Adhesion – The ability of hydrogen bonds to attract different types of molecules

26. Why can these animals walk on water?

27. Capillary Action is Due to Adhesion

28. Acids & Bases Acids are formed by hydrogen cations Bases are formed by hydroxide anions

29. Acids Donate protons (Hydrogen Ions) to water to form hydronium ions Donate protons (Hydrogen Ions) to water to form hydronium ions pH 0-6.99 pH 0-6.99 Taste Sour Taste Sour Turn litmus paper red Turn litmus paper red Strong acids completely dissociate to form ions Strong acids completely dissociate to form ions Strong acids Strong acids

34. Bases Donate hydroxide Donate hydroxide pH 7.01-14 pH 7.01-14 Accept protons Accept protons Taste bitter Taste bitter Feel slimy Feel slimy Turn litmus paper blue Turn litmus paper blue Strong bases completely dissociate to form ions Strong bases completely dissociate to form ions

35. pH

36. Buffers Compounds that tend to neutralize the pH of a solution by combining with either H+ ions or OH- ions to keep the solution neutral Compounds that tend to neutralize the pH of a solution by combining with either H+ ions or OH- ions to keep the solution neutral

37. Chemical Reactions Synthesis (A+B  C) Synthesis (A+B  C) Decomposition (C  A+B) Decomposition (C  A+B) Single Replacement (AB+C  AC+B) Single Replacement (AB+C  AC+B) Double Replacement (AB+CD  AC+BD) Double Replacement (AB+CD  AC+BD) Reactants are to the left of the arrow (Elements reacting) Reactants are to the left of the arrow (Elements reacting) Products are to the right of the arrow (Stuff made) Products are to the right of the arrow (Stuff made) Subscripts CANNOT be changed Subscripts CANNOT be changed Coefficients can be changed to balance an equation) Coefficients can be changed to balance an equation)

39. Chemical Reactions Endothermic rxn’s absorb heat Endothermic rxn’s absorb heat Exothermic rxn’s give off heat Exothermic rxn’s give off heat

40. Organic Chemistry Organic molecules are any molecules that contain atoms from three elements: carbon, hydrogen, and oxygen. Organic molecules are any molecules that contain atoms from three elements: carbon, hydrogen, and oxygen. For example, glucose is organic, since its molecular formula is C 6 H 12 O 6 For example, glucose is organic, since its molecular formula is C 6 H 12 O 6 Carbon dioxide (CO 2 ) is inorganic since it does not contain hydrogen. Carbon dioxide (CO 2 ) is inorganic since it does not contain hydrogen.

41. All organic molecules have two parts: The carbon backbone & the functional group Carbon atoms can form single, double, or triple bonds

42. 4 Groups of Organic Compounds Found in Living Things Carbohydrates (C-H-O 1:2:1 ratio) Carbohydrates (C-H-O 1:2:1 ratio) Lipids (C-H-O) Lipids (C-H-O) Proteins (C-H-O-N)…sometimes S Proteins (C-H-O-N)…sometimes S Nucleic Acids (C-H-O-N-P) Nucleic Acids (C-H-O-N-P)