2. What’s the Matter? All of the materials around you are made up of matter. You are made up of matter, as are the chair you sit on and the air you breathe. 1. Give an example of solid matter. 2. Give an example of liquid matter. 3. Give an example of gaseous matter. 4. Is all matter visible? 5. Does all matter take up space? Interest Grabber

3.  made of protons (+), neutrons, and electrons (-)  element = pure substance consisting of only one type of atom  compound = chemical combination of two or more elements

4. 6 C Carbon 12.011 Section 2-1 An Element in the Periodic Table : AN ELEMENT IN THE PERIODIC TABLE 6 electrons 6 protons 6 neutrons electrons = protons = atomic number Atomic mass - # electrons = neutrons

5. Nonradioactive carbon-12Nonradioactive carbon-13Radioactive carbon-14 6 electrons 6 protons 6 neutrons 6 electrons 6 protons 8 neutrons 6 electrons 6 protons 7 neutrons Section 2-1 Figure 2-2 Isotopes of Carbon ISOTOPES OF CARBON Vary in the number of neutrons

6.  Ionic Bonds  electrons transferred from one atom to another  anion = - charge  cation = + charge  Covalent Bonds  electrons shared by atoms  molecule is smallest unit of most compounds

7.  Van der Waals Forces  sharing of electrons not always equal  areas of molecule may have slight charge that can lead to slight attraction if in close proximity  weak but can hold large molecules together  geckos

8.  Hydrogen Bonds  see water info

10.  single most abundant compound in most living things  greatest solvent on Earth Polarity  Water molecule is polar because there is an uneven distribution of electrons between the oxygen and hydrogen atoms  Oxygen has a slight (-) charge; Hydrogen has slight (+) charge  like a magnet with 2 poles

11.  Attraction between the hydrogen of one water and the oxygen of another.  Allows for cohesion and adhesion  Because of polarity, hydrogen bonds usually form between oxygen, fluorine and nitrogen

12.  not as strong as covalent or ionic bonds  because water is polar it is able to form multiple hydrogen bonds – accounts for many of water’s special properties  expands slightly upon freezing  ice less dense than water  Hydrogen bonds allow water to dissolve many substances – critical to living cells

13.  Cohesion – attraction between molecules of the same substance  water is extremely cohesive  creates surface tension  Adhesion – attraction between molecules of different substances  water will adhere to the walls of a glass container

14.  ice is less dense than water so it floats on top  floating ice insulates the water underneath and prevents it from freezing  allows aquatic organisms that live in the water to survive during cold weather

16.  Heat capacity  amount of heat energy needed to increase temperature  requires large amount of heat to speed up molecules [raises temp]  heat capacity for water is high  body of water can absorb large amounts of heat without large temp changes  What are the benefits to this?

17.  composed of solute and solvent  solvent – substance in which solute dissolves  solute – substance that is dissolved

18.  water and non dissolved material  movement of water molecules keep small particles suspended  blood  water with blood cells and other undissolved particles

19. Oven cleaner Bleach Ammonia solution Soap Sea water Human blood Pure water Milk Normal rainfall Acid rain Tomato juice Lemon juice Stomach acid Neutral Increasingly Basic Increasingly Acidic pH Scale pH SCALE pH scale indicates the concentration of H+ ions H 2 O  H + + OH -  water hydrogen hydroxide ion ion Acid = contain higher concentrations of H + ions than pure water pH value below 7 Base = lower concentrations of H + ions than pure water pH value above 7

20.  weak acids and bases that react with strong acids and bases to prevent sudden changes in pH  blood pH = 7.4  changes prevented by buffers such as bicarbonate and phosphate ions  buffers play important role in homeostasis

21.  Organic Compounds  all contain the element carbon  study of organic compounds known as organic chemistry  4 groups Carbohydrates Lipids Proteins Nucleic Acids

22. MethaneAcetyleneButadieneBenzeneIsooctane Section 2-3 Figure 2-11 Carbon Compounds CARBON COMPOUNDS STRUCTURAL FORMULAS

23.  composed of carbon, hydrogen and oxygen  main source of energy for all living things  also used for structural purposes (cellulose)

24.  Terminology  monosaccharides simple sugars  ex. Glucose, fructose C 6 H 12 O 6 building blocks of complex carbs  disaccharides double sugars  ex. Sucrose, lactose, maltose C 12 H 22 O 11 glucose + fructose = sucrose glucose + glucose = maltose

25.  Polysaccharides  complex sugars  plants store sugar as starch  animals store sugar as glycogen  cellulose  starch used for structural purposes in plants [cell wall]

26.  Includes fats, waxes, oils  fats solid at room temp, produced by animals (except fish) saturated fats – cause heart disease  oils liquid at room temp, produced by plants unsaturated fats – better for you a few plant oils are saturated – coconut oil  waxes plants and animals

27.  stored as energy reserves  part of biological membranes and waterproofing  composed of fatty acid & glycerol molecules

28.  building blocks of living material  important in growth, maintenance, & repair  help run chemical reactions  made up of amino acids  20 of them  amino acids joined by peptide bonds  dipeptide = 2 amino acids  polypeptide = many amino acids  examples of amino acids = valine, lysine, glycine

30.  4 Levels  Primary  sequence of amino acids  Secondary  folding and coiling of the chain  Tertiary  three-dimensional arrangement  Quaternary  found in proteins with more than one polypeptide (chain)

32.  most complex biological compounds  DNA  deoxyribonucleic acid  RNA  ribonucleic acid  control heredity  composed of nucleotides which have 3 parts:  5 carbon sugar  nitrogen base  phosphate group

33. Nucleotide

34.  Monomer = smallest unit into which an organic compound can be broken  carbohydrates = monosaccharides  lipids = fatty acids and glycerol  proteins = amino acids  nucleic acids = nucleotides

35. Carbon Compounds include that consist of which contain that consist of which contain Section 2-3 Concept Map CarbohydratesLipidsNucleic acidsProteins Sugars and starches Fats and oilsNucleotidesAmino Acids Carbon, hydrogen, oxygen Carbon, hydrogen, oxygen Carbon,hydrogen, oxygen, nitrogen, phosphorus Carbon, hydrogen,oxygen, nitrogen, CONCEPT MAP FOR CARBON COMPOUNDS