Atoms Molecules and Compounds

1. Atoms Molecules and Compounds • Matter is anything that takes up space and has mass. • Matter can come in four physical forms or phases; solid, liquid gas and plasma. • Matter is composed of Quarks, Leptons, neutrinos • Organic means it contains a carbon and usually found in living organisms. Inorganic is matter without a C.

2. Atoms are the smallest units of an element that still have its characteristics. • Atoms are composed of 3 types of particles, proton, neutron, electron • Ions are atoms that have lost or gained electrons, charged atoms • Cation + charge • Anion -charge • Atomic number is the number of protons • Atomic mass is the number of protons and neutrons • Isotope-atoms of the same element with a different number of neutrons.

3. Atomic particles

7. Electron Orbital filling • 1s2 • 2s2 2p6 • 3s2 3p6 3d10 • 4s2 4p6 4d10 4f14 • 5s2 5p6 5d10 5f14 • 6s2 6p6 6d10 • 7s2 7p6

9. Chemistry • Law of Conservation of Matter- matter cannot be created or destroyed but may be transformed from one form into another form. • States of Matter-Solid, liquid, gas, and plasma • Mixture is when elements keep there own identity ex solution • Type, single and double replacement (substitution), synthesis, decomposition • Chemical energy is stored in the bonds. • Catalyst-speeds up a chemical reaction with out being used up • Chemical reaction where two materials are combined and energy is exchanged and new material/s are formed. • Reactants are what are originally combined • Products are what is formed • Yield sign tells you which way the reaction will normally proceed. Lowest energy and highest enthalpy

11. Bonding • Covalent Bond-Sharing bond to complete the outer shell, usually resulting in a molecule • Ionic Bond-is a bond that actually has a transfer of electrons from one atom to another Making ions with a specific crystalline lattice, is the compound. • Metallic Bond-the ability of a metallic compound to bend, Sea of Electrons, that roll. • Hydrogen bond- a bond that contains hydrogen, • Van der waals Forces attractive forces between atoms

12. Garnet Fluorite Beryl Laboratory made Bismuth

13. Bauxite Aluminum Aluminum Can

14. Chem Quiz • 1.How many protons, neutrons and electrons does Ca45/20 have? • 2.What is I 127/53, and I 126/53? • 3.If a Na atom becomes an ion with a +1 charge explain what happened. • 4.What is a sharing bond called? • 5.Organic means…….

15. Chem Quiz • 1.How many protons, neutrons and electrons does Ca45/20 have? • 20Protons, 25 Neutrons, and 20 electrons • 2.What is I 127/53, and I 126/53? Isotopes of Iodine • 3.If a Na atom becomes an ion with a +1 charge explain what happened. The Na atom has lost 1 electron (-1) and is now a positive ion(cation) • 4.What is a sharing bond called? Covalent • 5.Organic means living or containing a carbon

16. Acid and Base • pH is the reciprocal log of the hydronium ion concentration. Alkaline (7-14), acidic(1-7), 7 is neutral • Alkalinity is how basic something is, Acidity is how acid some thing is. • Usually acid have a H3O+, or H+ (Hydronium) in the cation and bases usually have an OH- (Hydroxide) in the anion. • Acids may be vinegar, Acetic acid, Sulfuric Acid (H2SO4), Hydrochloric acid (HCl), Nitric Acid (HNO3) • Bases are Sodium Hydroxide (NaOH) Lye, drain cleaner, Magnesium hydroxide MgOH, Calcium hydroxide CaOH, antacids

18. Chemical Energy • Energy is the ability to do work • Energy can be divided into two types. • Kinetic energy-1/2 mv2 is the energy of motion. • Potential Energy-mgh is the energy of position. • Activation Energy-Energy needed to start a chemical reaction • Law of Conservation of energy- Energy cannot be created or destroyed but transformed.

19. Reactions • Most reactions are reversible, but tend toward lowest energy and greatest enthalpy (disorder). • Reactants are the materials that are put together • Products are the results of mixing chemically active elements • Reactants -> Products. Reactions can be reversed, depending on conditions. If one of the reactants is in limited supply that limits how much or many of the product/s will be produced. • To satisfy the Law of Conservation of Matter what ever you put into a reaction you will get out.

21. Type of Reactions • A. C6H12O6 -> 6H2O + 6CO2 • B. 6H2O + 6CO2 -> C6H12O6 • C. 2NaOH + Ca(C2H3O2) -> 2NaC2H3O2 + Ca(OH)2 • ZnSO4 + Cu -> Zn + CuSO4

22. Organic Compounds • Organisms use some elements in large amounts some in trace amounts • Organic compounds are composed of chains or circles or elemental C. Organic compounds form the materials that living organisms are composed of • The four major groups of organic compounds are carbohydrates, protein, lipids, and nucleic acids

23. Organic Compounds • Lipids-Oil,fat: stored or reserve energy and taste • Carbohydrates-sugars, breads, cereals: Energy everyday or immediate • Protein-”Meat”, beans, nuts: repair, maintenance, growth: • Nucleic Acids-DNA,RNA, all cells has nucleic acids: Heredity, codes for the proper proteins to be produced.

24. Organic Compounds-containing C or come from living things. • C electron configuration is 1s2 2sp3, forms 4 covalent bonds. Carbon can form single, double or triple bonds. • Structural formula- rings, chains or combinations can be formed. So many different ways carbon can combine, stereoscopic isomers (mitten) • Biosynthesis or Condensation-build up of organic compounds. Making of Polymers, or one large molecule from several smaller molecules. Monomers form polymers • Hydrolysis-splitting of molecules with water. Converting polymers to monomers.

25. Biosynthesis and Condensation • What elements are present in the compounds? • What are the building blocks or molecules that make up the compounds? • What compounds or molecules make up the building blocks?

29. Proteins • Examples are beef, pork, chicken, and fish muscle • Composed of Amino Acids(19), CHOSPN and Fe • Amine NH2 • Alkyl group R which is in the middle and is a variable • Organic Acid –COOH • Condensation • Hydrolysis • Sequence of AA shape thus determines the protein characteristics • Proteins are very species specific. Antibodies per person varies as an example.

30. Protein, Enzymes(organic catalysts) • Control specific reactions, controlling all of the chemical reactions in our bodies • How an enzyme works • Substrates-substance that enzyme causes to react. • Active site is the area on an enzyme that fits a certain substrate • Once reaction is finished, enzyme moves on • Enzyme system-team of enzymes • Coenzyme nonprotein enzyme

32. Fats and Lipids • More energy per mass, More bonds • Examples are oils, fats, waxes, butter • Composed of C,H, and O, insoluble in water • Formation- Condensation, Dehydration Synthesis • 3 fatty acids • glycerol • Decomposition-Hydrolysis (3 water + Fat -> 1 glycerol + 3 fatty acids) • Saturated all single bonds, Unsaturated double bonds

33. Trans Fats • Trans fat is the common name for unsaturated fat with trans-isomer (E-isomer) fatty acid(s). Because the term refers to the configuration of a double carbon-carbon bond, trans fats are sometimes monounsaturated or polyunsaturated, but never saturated. • Trans fats are not essential fatty acids; indeed, the consumption of trans fats increases the risk of coronary heart disease12 by raising levels of "bad" LDL cholesterol and lowering levels of "good" HDL cholesterol.3 Health authorities worldwide recommend that consumption of trans fat be reduced to trace amounts. Trans fats from partially hydrogenated oils are more harmful than naturally occurring oils.4 Some studies have shown natural trans fats in beef and dairy products can have the opposite health effect and can actually be beneficial, e.g. lowering total and LDL cholesterol and triglyceride levels.567 • Unsaturated fat is a fat molecule containing one or more double bonds between the carbon atoms. Since the carbons are double-bonded to each other, there are fewer bonds connected to hydrogen, so there are fewer hydrogen atoms, hence the name, 'unsaturated'. Cis and trans are terms that refer to the arrangement of the two hydrogen atoms bonded to the carbon atoms involved in a double bond. In the cis arrangement, the hydrogens are on the same side of the double bond. In the trans arrangement, the hydrogens are on opposite sides of the double bond. • The process of hydrogenation adds hydrogen atoms to unsaturated fats, eliminating double bonds and making them into partially or completely saturated fats. However, partial hydrogenation, if it is chemical rather than enzymatic, converts a part of cis-isomers into trans-unsaturated fats instead of hydrogenating them completely. Trans fats also occur naturally in a limited number of cases: Vaccenyl and conjugated linoleyl (CLA) containing trans fats occur naturally in trace amounts in meat and dairy products from ruminants, although the latter also constitutes a cis fat.

35. Carbohydrates • Make up most of your diet, composed of CHO, examples are sugar, starches, cellulose. • Sugars are organized in plants as food • Monosaccharide-simple sugar • Disaccharides-double sugar • Polysaccharides- starches • Dehydration synthesis • Hydrolysis • Carbohydrates if not used are converted to fats by the liver.

38. Nucleic Acids • Gives instructions to the cell to make proteins, heredity, these instructions are passed on from generation to generation • Composition Nucleotides • 5 carbon sugar • Deoxyribose (Ribose minus an Oxygen) • Ribose • Phosphoric acid • Nitrogen base • Pyrimadine- this is the single ring structure • Purines- this is the double ring structure • Types • Ribonucleic Acid (RNA) • Deoxyribonucleic Acid (DNA)

39. DNA Linear, Double helix, Thymine, Deoxyribose sugar 3 forms heredity, Biologically the Master Molecule of Life Nucleus, or rings RNA Linear, Single side ladder Urasil, Ribose sugar 4 forms involved in making proteins Found in all parts of the cell DNA, RNA

40. Groups, Names • Organic Acid(COOH) • Amine NH2 • Alkyl R • Alcohol (COH) • Alkanes • Alkenes • Alkynes

41. Protein Protein Amino Acid Peptide Bond Alkyl Organic Acid Amine

42. Lipids Lipids Fatty Acid Glycerol Fatty Acid Fatty Acid

43. Carbohydrates Monosaccharide Galactose Monosaccharide Fructose Monosaccharide Glucose Disaccharide Sucrose Polysaccharide Starches

44. Nucleic Acid RNA, DNA Nucleotide Hydrogen Bonding Phosphoric Acid 5 Carbon Sugar Ribose, Deoxyribose N- Base Purine Pyrimadeines

45. Organic Compounds

46. Organic Compounds

47. Dehydration Synthesis, Condensation Building up of large molecule with the release of water as a product. Hydrolysis Breaking apart of large molecules, with water as a reactant. Reactions