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Understanding Chemistry: What Matter is Made of & How It Reacts

This chapter delves into the composition and reactions of matter, exploring elements, the periodic table, chemical bonding, free radicals, energy reactions, water importance, pH scale, organic compounds like carbohydrates, lipids, proteins, and nucleic acids.

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Understanding Chemistry: What Matter is Made of & How It Reacts

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  1. Chapter 2: Chemistry What is matter made up of and how does it react?

  2. What is Matter? • Anything that occupies space and has mass.

  3. Elements • Pure substance made up of only one kind of atom • 90 occur naturally • 25 essential to life: O, C, H, N • 0= 65%, C=18.5%, H=9.5%, N=3.2% • Atom: smallest unit of matter that cannot be broken down by chemical means.

  4. Periodic Table • Atomic Symbol: C = carbon, or Au = gold • Atomic Number: Number of Protons in an Atom. Carbon has ? Gold has ? • Atomic Mass: Number of Protons and Neutrons. • Isotope: Different numbers of Neutrons than Protons Periodic Table

  5. Atoms • Three major parts. • Protons:Positive Charge. Inside Nucleus • Neutrons: Neutral Charge. Inside Nucleus: • Electrons: Negative Charge. Outside Nucleus • 2 electrons in first shell • 8 electrons in the second shell • Eight is Great! Will not React with other atoms. • If the outer shell is not full it will react.

  6. Periodic Table Bonding Combining Chemicals • Compound: When two or more different elements combine. • Hydrogen Bond: H2O • When hydrogen bonds with another atom. Creates a polar molecule. • Covalent bond: CO2 • When atoms on the same side of the chart (same size) bond. Share electrons. • Both Hydrogen and Covalent bonds form molecules, ionic bonds do not. Ionic/ Covalent Bonds

  7. Combining Chemicals continued • Ionic Bonds: When atoms on different sides of the chart (different size) bond. Steal electrons. Create Ions. Make teeth and bones. • Ion: Charged particle either negative or positive. NaCl = table salt • Free Radical: Electrically charged ion with an unpaired electron in its outer shell.

  8. Antioxidants, What are they? • Subatances that inactivate oxygenderived free-radicals • Slows damage from free-radicals • Examples: Selenium, Zinc Beta-carotene, Viamins C & E Free Radicals Acai Berry

  9. Energy and Chemical Reactions • Reactants and Products • Co2 + H20 = H2C03 • Energy Transfer • Exergonic Rxns- Energy exits or released • Endergonic Rxns- Net absorption of energy • Activation energy • Energy needed to start the reaction. Catalysts reduce the energy needed. Often enzymes.

  10. More on Ionic Bonds • Ionic Bonds have 2 parts • Cation: Positively Charge, Ca+2 • Has lost 2 electrons • Anion: Negatively Charged, Cl- • Has Gained to electrons • Electrolytes: Ionic compounds that breaak into cations and anions when dissolved. (Salt)

  11. Solution • A mixture in which one or more substances are evenly distributed in another substance. • Solute: smaller word, smaller thing • Solvent: bigger word, bigger thing

  12. Importance of Water: an inorganic compound The Importance of Water • Polar molecule(it has a negative and positive charge.) • Can dissolve both Ionic and Polar-Covalent molecules • Surface Tension • Cohesion: Sticks to itself. • Adhesion: Like a band-aid. Sticks to stuff • Capillary Action: Climbs up thin tubes

  13. Importance of Water: an inorganic compound • Evaporates: Cooling, Water cycle, etc • Resists Temperature Change: Takes a lot of energy to heat or cool water • Expands as it Freezes.

  14. Ph Scale • Measured on grams of Hydrogen (H+) • pH of 1= 1g of H+, pH of 2= .01g of H+ • Acid: form hydronium ions (H+) • pH of less than 7 ( 1 to 6.9) • Base: form hydroxide ions (OH-) • pH of more than 7 (7.1 to 14) • Acid + Base: salt & water, the solution is neutral with a pH of 7. • NaOH + HCL = H2O + NaCl with a pH of 7

  15. What is a Buffer? • Chemical substances that neutralizes small amounts of an acid or base added to a solution. • Why are these important to your body?

  16. Carbohydrates Organic Compounds: C-H • Carbohydrate: fast energy • made of Carbon, Hydrogen, and Oxygen. 1:2:1 proportion. Sacchar = sugar • Monosaccharides:C6H12O6, glucose and fructose • Disaccharides: 2 sacchar’s: Sucrose, table sugar • Polysaccharides: Many sacchar’s: Cellulose (wood) and starch.

  17. Organic Compounds: C-H • Lipids: Fats long term energy storage • Have very few oxygen atoms • Saturated fats: All C bonded to H. Lard, and butter. • Unsaturated fats: C is double bonded to itself. Oil. Lipids

  18. Organic Compounds:All organic compounds contain Carbon. • Protein: the working molecule • 50 or more Amino Acids make a protein • Types of Proteins • Muscle • Enzymes: Control chemical reactions and can be re-used like a key in a lock • Hair Protein

  19. Organic Compounds:All organic compounds contain Carbon. • Nucleic Acids: pg. 37 DNA and RNA • Made of nucleotides: Sugar, Phosphate, and X • ATP: energy cells run on. DNA

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