What makes up everything in the universe?   2. Name 2 properties of all matter.   3. Define mass.   4. How does weight differ from mass?   5.What are elements?   6. Name the 4 elements that make up most of a living thing.   7. What is used to represent an element?   Matter Volume and Mass Quantity of matter an object has Weight is the pull of gravity on an object Pure substances that cannot be broken down into simpler kinds of matter C – H – O – N Chemical SYMBOL (1 or 2 letters)

Nucleus & Energy levels Center & Contains protons & neutrons 8. Name the smallest part of an element.   9. What are the 2 main regions of an atom?   10. Where is the nucleus of an atom found and what does it contain?   11. What is the charge on a proton?  A neutron?   12. All atoms of the same element have the ________ number of protons. 13. The number of protons in an atom determines the __________________.   14. What is the charge on an electron?   Atom Nucleus & Energy levels Center & Contains protons & neutrons + Neutral same Atomic # _

15. If you know the number of protons in an atom, how can you determine the number of electrons?   16. Do all the atoms of the same element have the same number of neutrons?   17. Atoms of the same element with different numbers of neutrons are called ___________.   18. The mass of an atom is centered in the ___________.   19. The number of protons PLUS neutrons in an atom determines its ___________________.   20. What atomic particle has a negative charge?   Usually equal No Isotopes Nucleus Atomic Mass Electrons

22. Where are electrons found? 21. Why isn’t the mass of an electron used to determine the atomic mass of an element? 22. Where are electrons found? 23. Which electrons in an atom have the most energy?   24. How many energy levels are there & name them?   25. How many electrons will each energy level hold?   26. Elements are arranged on a __________________ by their atomic _____________.   27. What are Periods & what do they tell you about elements?   28.What are Families & what do they tell you about elements?   e- have little to no mass Energy levels e- in the outer levels (7) - K – L – M – N – O - P - Q 2(n2) (n=energy level) K-2; L-8; M-18; etc. Periodic Table # Rows - # of energy levels Columns – Valence electrons

29. Two or more elements combined together make a _____________.   30. Chemical ______________ represent compounds.   31. _____________ are the smallest part of a compound.   32. ______________ in chemical formulas tell the number of atoms of each element.   33. _____________ in a formula tell the number of molecules.   34. Compounds have ____________ properties than its elements.   35.  The outermost _______________ in elements determine if they will combine.   36. Elements with ___________ outer energy levels are stable & won’t react.   Chemical compound Formulas Molecules Subscripts Coefficients Different Energy “Full” 2 or 8 e-

Chemical Bonds Ionic Covalent NH4 H20 NaCl KCl Sharing valence electrons Single, double or triple bonds can occur Very strong Transferring valence electrons Creates ions (charged particles) that are attracted to each other Van der Waals (forces) Attraction between whole molecules H-bonds are van der Waals attraction between H and other molecules.

(breaking down glucose) Ch.3 Energy in Reactions Exothermic Endothermic Cellular Respiration (breaking down glucose) Photosynthesis (creating glucose)

-ASE Enzymes Act as a catalyst Lower the activation energy 2. Are not used up or changed during a reaction 3. Are sensitive to changes in heat & pH 4. Work for only one specific reaction Enzyme animation

Ice is less dense than liquid water AMAZING WATER!! Water is fundamental to all life on Earth The Properties of Water: Polar molecule “Universal Solvent” Ice is less dense than liquid water Surface Tension Adhesion (other) Cohesion (self)

Non-polar particles eventually settle out of solution Mixtures with Water Homogeneous Heterogeneous Suspensions Colloids Solutions Non-polar particles eventually settle out of solution Non-polar particles do not settle out of solution Solute Solvent Polar molecules dissociate in water (form ions) Paint Ink Milk

ACIDS BASES Mixtures with Water pH – measure of H+ ions in solution Some solutes release H+ ions into solution ACIDS Some solutes release OH- (hydroxide) ions into solution BASES pH Scale Acidic H+ = OH- Basic (Alkaline) H+ > OH- OH- > H+

Organic Chemistry

-determines some properties and reactions of that class of molecule. Organic Chemistry Functional Groups -determines some properties and reactions of that class of molecule. *Functional groups will undergo the same type of reactions regardless of the compound of which they are a part *Functional groups can be used to distinguish similar compounds from each other. Acetic Acid Ethanol

Organic Chemistry Functional Group Formula Example Alcohols Hydroxyl R-OH Carbonyl R - C = O - H Aldehydes R –C–R = O Ketones R - C = O - OH R - C = O - O Carboxylic Acid Carboxyl

Organic Chemistry Group Formula Example Functional Group Formula Example R-N - H R-N - H Amino Acids Amino Sulfhydryl R-SH Thiols Phosphate R-O-P-O -O O= Organic Phosphates

Organic Chemistry 3. Identify Which group(s) What group is do you see? boxed in? Which group(s) do you see? Ketone Carboxyl Aldehyde Amino 5. Which group(s) do you see? RNA 4. Which group(s) do you see? Amino Phosphate Carboxyl Hydroxyl

Biological Macromolecules Polymers Monomers H2O Condensation Reaction Carbohydrates Monosaccharides Fatty Acids & Glycerol (Dehydration Synthesis) Lipids H2O Hydrolysis Proteins Amino Acids Nucleic Acids Nucleotides

Biological Macromolecules Amino Acids Polypeptide Hydrolysis/enzyme animation

Carbohydrates

Carbohydrates Small sugar molecules to large sugar molecules. Examples: A. monosaccharide B. disaccharide C. polysaccharide

Carbohydrates Monosaccharide: one sugar unit Examples: glucose (C6H12O6) deoxyribose ribose Fructose Galactose glucose

Carbohydrates Disaccharide: two sugar unit Examples: Sucrose (glucose+fructose) Lactose (glucose+galactose) Maltose (glucose+glucose) glucose

Carbohydrates Polysaccharide: many sugar units Examples: starch (bread, potatoes) glycogen (beef muscle) cellulose (lettuce, corn) glucose cellulose

Lipids

Lipids General term for compounds which are not soluble in water. Lipids are soluble in hydrophobic solvents. Remember: “stores the most energy” Examples: 1. Fats 2. Phospholipids 3. Oils 4. Waxes 5. Steroid hormones 6. Triglycerides

Lipids Six functions of lipids: 1. Long term energy storage 2. Protection against heat loss (insulation) 3. Protection against physical shock 4. Protection against water loss 5. Chemical messengers (hormones) 6. Major component of membranes (phospholipids)

Lipids Triglycerides: composed of 1 glycerol and 3 fatty acids. = = H H-C----O glycerol O C-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH3 = O C-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH3 = fatty acids O C-CH2-CH2-CH2-CH =CH-CH2-CH2-CH2-CH2-CH3 =

C-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH3 Fatty Acids There are two kinds of fatty acids you may see these on food labels: 1. Saturated fatty acids: no double bonds (bad) 2. Unsaturated fatty acids: double bonds (good) O C-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH2-CH3 = saturated O C-CH2-CH2-CH2-CH =CH-CH2-CH2-CH2-CH2-CH3 = unsaturated

Proteins

Proteins (Polypeptides) Amino acids (20 different kinds of aa) bonded together by peptide bonds (polypeptides). Six functions of proteins: 1. Storage: albumin (egg white) 2. Transport: hemoglobin 3. Regulatory: hormones 4. Movement: muscles 5. Structural: membranes, hair, nails 6. Enzymes: cellular reactions

Proteins (Polypeptides) Four levels of protein structure: A. Primary Structure B. Secondary Structure C. Tertiary Structure D. Quaternary Structure

Primary Structure Amino acids bonded together by peptide bonds (straight chains) aa1 aa2 aa3 aa4 aa5 aa6 Peptide Bonds Amino Acids (aa)

Secondary Structure 3-dimensional folding arrangement of a primary structure into coils and pleats held together by hydrogen bonds. Two examples: Alpha Helix Beta Pleated Sheet Hydrogen Bonds

Tertiary Structure Secondary structures bent and folded into a more complex 3-D arrangement of linked polypeptides Bonds: H-bonds, ionic, disulfide bridges (S-S) Call a “subunit”. Alpha Helix Beta Pleated Sheet

Quaternary Structure Composed of 2 or more “subunits” Globular in shape Form in Aqueous environments Example: enzymes (hemoglobin) subunits

Nucleic Acids

Nucleic acids Two types: a. Deoxyribonucleic acid (DNA- double helix) b. Ribonucleic acid (RNA-single strand) Nucleic acids are composed of long chains of nucleotides linked by dehydration synthesis.

Nucleic acids Nucleotides include: phosphate group pentose sugar (5-carbon) nitrogenous bases: adenine (A) thymine (T) DNA only uracil (U) RNA only cytosine (C) guanine (G)

Nucleotide O O=P-O Phosphate Group N Nitrogenous base (A, G, C, or T) CH2 O C1 C4 C3 C2 5 Sugar (deoxyribose)

DNA - double helix P O 1 2 3 4 5 P O 1 2 3 4 5 G C T A

C, O & H in straight chains or chains of rings Carbohydrates C, O & H in straight chains or chains of rings Lipids C, O & H Fatty acids held together by a glycerol or rings and chains

Proteins Nucleic Acids (Amino Acids) Look for an Amino group and carboxyl group Nucleic Acids (Nucleotides) Look for a sugar ring, phosphate, and amino group