Unit 1

1. Unit 1 Basic Chemistry

2. Watching Youtube Videos • When you click on the video it will play within the power point • Once you’ve viewed the video you must click somewhere on the slide outside of the video box to advance to the next slide

3. Scientific Method

4. Scientific Method • Is the process employed by scientist to support or reject an idea, by accumulating data, and testing the data under conditions which are controlled in ways to give credible results. • If an idea or hypothesis withstands substantial independent testing it becomes a theory, then a law or principle.

5. Scientific Method • This site has a nice explanation and a quiz for you to test yourself • http://www.biology4kids.com/files/studies_scimethod.html

6. States Of Matter • SolidDefinite shape and volume. • LiquidTakes shape of container; definite volume. • GasTakes shape of container. (compressible).

7. Properties • PhysicalWhat a substance is. • Color, density, odor, solubility in water. • DensityWeight per unit volume. • ChemicalWhat a substance does • +/- Reactivity with water or air. • +/- Burning in a flame.

8. Physical change: Although some extensive properties (like shape, phase, etc.) of the material change, the material itself is the same before and after the change. The change can be “undone.” Chemical change: The atoms have been altered. What was there at the beginning is no longer the same. Chemical changes cannot be undone. Physical vs Chemical Changes Steel rusting is an example of a chemical change Ice melting is an example of a physical change

9. Kinetic Energy The energy of motion Potential Energy Stored energy Energy

10. Conservation Laws • Matter is neither created or destroyed, only arranged from one form to another. • Energy is neither created or destroyed, only changed from one form to another. • PotentialKineticHeat. http://www.youtube.com/v/dExpJAECSL8&playnext_from=TL&videos=PAn7NmYhHVw

11. Elements • Substances which cannot be broken into simpler substances by ordinary means. • Are homogeneous in compositionthe same throughout. • Each element represented by a symbol. • O = Oxygen • C = Carbon • AU = Gold.

12. Periodic Table Another version at http://www.ptable.com/

13. Atomic Structure • Atoms are electrically neutral • Composed of protons, neutrons & electrons

14. The Nucleus of the Atom • Protons • Positive charge • Number of protons is the atomic # • All atoms of same element have same atomic # • Neutron • No charge ie neutral • Same mass as a proton • located in nucleus • Number of protons + neutrons = atomic weight Number of Protons Number of Protons + Neutrons

15. Isotopes • Different # of neutrons than normal, i.e., different atomic weight. Normal Carbon 6 protons + 6 neutrons Atomic Mass = 12 Carbon 14 Isotope 6 protons + 8 neutrons Atomic Mass = 14

16. Electrons • 1/1837, the mass of a proton • orbit the nucleus • Directly involved in chemical reactions • Determines the chemical property of the atom • Negative charge • Equal in number to the number of protons • Arranged in energy levels or shells around nucleus; • 1st shell holds two—all others hold eight • Happiness is a full outer shell 

17. Atomic Structure

18. Electron Arrangement • Arranged in energy levels or shells around nucleus; • 1st shell holds two—all others hold eight • Happiness is a full outer shell  • Atoms will share, give away or pick up electrons to achieve a full outer shell

19. Electron Arrangement • For example: Carbon • Atomic Number 6, Atomic Mass 12 • This tells us there are 6 protons (atomic number) • 6 neutrons (atomic mass – atomic number) • And 6 electrons (equal to the number of protons) • The first shell holds a maximum of 2 • The other 4 will be in the second shell • So Carbon has 4 electrons in its outer shell

20. Electron Arrangement • For example: Cobalt (Co) • Atomic Number 27, Atomic Mass 58.93 (round up to 59) • This tells us there are 27 protons (atomic number) • 32 neutrons (atomic mass – atomic number) • And 27 electrons (equal to the number of protons) • 2 in the first shell • Remember all other shells hold a maximum of 8 • 8 in the second, 8 in the third, 8 in the fourth • We still have one left so that 1 electron is in the fifth • Cobalt has 1 electron in its outer shell

21. Electron Arrangement Cobalt 27 Protons 32 Neutrons 27 Electrons electrons Protons and Neutrons In the nucleus 2 in the first shell 8 in shells 2, 3, and 4 1 in shell 5

22. Electron Arrangement • Now would be a good time for you to work on the Periodic Table Assignment! 

23. Atomic Bonding • Ionic Bonding • Results from the transfer of electrons • Atoms gain/lose electrons. • Results in ions • Atom with a charge. • The charge difference holds the resulting molecule together http://www.youtube.com/v/xTx_DWboEVs&playnext_from=TL&videos=Prgzu17ouAM

24. Atomic Bonding • Covalent Bonding • Results from a sharing of electrons b/t two atoms. • Each atom provide an electron • The Shared electron pair orbits both nuclei this is what keeps the molecule together • Larger nuclei will hog the shared electrons from smaller nuclei http://www.youtube.com/v/1wpDicW_MQQ&playnext_from=TL&videos=tqqVAiDEMWo

25. Atomic Bonding Covalent Bond Between Oxygen and Hydrogen • Hydrogen Bond • Special bond—very weak • Bond between molecules NOT between atoms • Results from a covalent bond involving hydrogen • Shared electron spends more time around the bigger nucleus of the Oxygen atom • This leaves the hydrogen end with a net positive charge & the Oxygen end with a net negative. • A polar molecule due to the charge difference from one end of the molecule to the other. Between two Water molecules

26. Compounds • Combination of elements. • Can be separated into their parts by chemical means. • Homogeneous in composition. • Definite composition • Have different properties than their parts • Example: Oxygen +Hydrogen= H2O water. • Oxygen and Hydrogen at room temperature are gasses • Neither conduct electricity • Water is a liquid at room temperature and does conduct electricity

27. Mixture • Combination of substances • Can be separated by physical means • No set composition • Heterogeneous in composition • Parts retain their own character • Example: Italian Salad Dressing • The vinegar and oil can be mixed together with spices but they can be separated from one another

28. Macromolecules: Proteins • Compound of amino acids joined together. • Each protein has a definite structure. • Primary—linear sequence of amino acids • Secondary-Initial folding to sequester hydrophobic • (water hating) amino acids. • Alpha Helix • Beta Pleated Sheet • Tertiary—Complex folding to created final 3D shape

29. Macromolecules: Proteins Protein Structure http://www.youtube.com/v/lijQ3a8yUYQ

30. Macromolecules: Proteins • Denaturation • To destroy the shape of a protein • Heat, ph, salt concentrate on • Maybe reversible or not • Cook an egg: the heat denatures the albumin protein in egg white

31. Macromolecules: Carbohydrates • Carbohydrates • Sugars, Starches, Cellulose • All contain carbon, hydrogen, & oxygen in a 1:2:1 ratio • Glucose C6H12O6 • Monosaccharide: Single Sugar, glucose. • Disacharide: Double Sugar, sucrose

32. Macromolecules: Carbohydrates • Polysacharride : • Many sugar molecules joined together • Starch • Plant form of energy storage. • Insoluble in water. • Digestible by animals. • Detected by iodine. • Celluose • wood, cotton, paper; • insoluble in water; • not digestible by animals. • Glycogen • Animal form of energy storage

33. Macromolecules: Nucleic Acids • Information storage • DNA: DeoxyriboNucleic Acid) • Organism’s instructions for assembly • Double stranded • Located in nucleus • BASES • Adenine Guanine • Thymine Cytosine

34. Macromolecules: Nucleic Acids • RNA: RiboNucleic Acid • Information Use, daily operation of organism. • Single stranded • Made in nucleus, exported for work throughout cell • BASES • Adenine Guanine • Uracil Cytosine

35. Macromolecules: Lipids / Fats • Insoluble in water. • Combination of fatty acids and glycerol. • Reserve energy storage. • Make up cell membranes and some hormones

36. Saturated All carbon atoms linked by single bond. “Saturated with hydrogen” Solid at room temp Most of the animal fats responsible for increasing the amount of cholesterol Unsaturated At least one double bond between 1 pair of carbon atoms. Liquid at room temperature Most vegetable fats Macromolecules: Lipids / Fats

37. Enzymes • Biological catalyst. • Increases the rate of chemical reaction. • Lowers the activation energy required for reaction. • All enzymes are proteins. • Have specific active site to bind to substrates. • These active sites are created by the 3D structure of the protein. • What would you expect if an enzyme was subjected to extreme heat? http://www.youtube.com/v/V4OPO6JQLOE&playnext_from=TL&videos=I91ovDgWCys

38. Acids • Donate H+ ions to solution • Can be in solid or liquid form • Sour taste • The more H+ ions released the stronger the acid • Common Acids • HCl Hydrochloric (in stomach) • H2SO4 Sulfuric (battery acid) • HNO3 Nitric (Medical Testing) • H2CO3 Carbonic (Soda)

39. Bases • Donate OH-, hydroxide ions to solution • Slippery feel • Bitter taste • Common Bases • NaOH Sodium Hydroxide (Drain cleaner) • NH4OH Ammonium Hydroxide (Cleaning) • NH3 Ammonia (Cleaning)

40. pH Scale • A measure of the H+ ion concentration in a solution. • Each whole number change in PH value is a 10 fold d/f in H+ concentration • pH Scale 0-14 • <7 is acid • =7 is neutral • >7 is base • The farther away from 7 the stronger the acid or base

41. pH Scale http://www.youtube.com/v/gwFR_Iph5R0

42. Indicators Compounds which look different according to the pH pH paper; litmus paper. Phenolphalein, bromthymol Blue. All change color in response to pH Buffers Compounds which resist changes in PH serve as reservoir for H+ ions. Can donate or accept H+ ions Very important in maintaining homeostasis in living organisms Indicators and Buffers

43. CHEMICAL REACTIONS • Dehydration Synthesis • Synthesis: to make • A+B  C • In the animation notice the water molecule bouncing away from the sucrose http://www.youtube.com/v/UyDnnD3fMaU&feature=PlayList&p=5DD6329BBE0DE93F&playnext_from=PL&playnext=1&index=1

44. CHEMICAL REACTIONS H2O • Hydrolysis • to split apart using water • The water wedges itself against the A-B bond until it breaks B A A B +

45. Metabolism • We use both hydrolysis & dehydration synthesis • Hydrolysis breaks down the food we eat. • Dehydration synthesis builds what our bodies need