Unit One- Chapter 2 Chemistry of Life

1. Unit One- Chapter 2 Chemistry of Life Mrs. Cook Biology

2. A. How is Chemistry related to Biology? • Chemistry is the study of the composition and properties of matter. • Chemistry is related to Biology because all organisms are composed of chemical substances. • The structure of a DNA Molecule is a carbohydrate.

3. B. Nature of Matter The non-living components of cells begin with atoms. An atom is the smallest unit in a particular organism. Organization of Living things: Chemical (atomic) level Cellular Level Tissue Level Organ Level Organisms Level Ecological Level

4. 1. Four States of Matter a. Solid - particles are tightly packed - particles move very little - do not need a container b. Liquid - particles loosely arranged - particles move randomly - particles conform to container c. Gas - particles most loosely arranged - particles move the most - particles fill a container d. Plasma - exists between solid and liquid

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6. 2. Atom Configuration • Atoms are made up of 3 types of particles: a. Electrons - Located outside the nucleus - have a negative charge b. Protons - inside the nucleus - have a positive charge c. Neutrons - inside the nucleus - have no charge The number of electrons = the number of protons, net charge is neutral.

7. 3. Elements • An element is a pure substance made up of only one kind of atom.

8. Elements cont. a. The total number of Protons is called the atomic number. b. The total number of Protons + Neutrons is called the Atomic Mass. ***Remember: The number of Protons is equal to the number of electrons. Look on your periodic table. What is the atomic number for Carbon? What is the Atomic Mass? How many electrons does it have? How many neutrons?

9. 4. Chemical Bonding • Atoms can join with other atoms to form stable substances. a. Chemical Bond- is a force that joins atoms together. b. A compound is a substance made of the joined atoms of 2 or more different elements. • H2O • NaCl • C6H12O6 • CO2

10. Chemical Bonding cont. c. The arrangement of an element’s electrons determines how atoms bond together. i. Electrons are grouped into different levels. ii. The levels closer to the nucleus hold fewer electrons than those further away from the nucleus. • 1st energy level - 2 electrons • 2nd energy level -8 electrons • 3rd energy level -8 electrons

11. Chemical Bonding cont. d. A molecule is a group of atoms held together by covalent bonds. i. Covalent bonds form when two or more atoms shareelectrons.

12. Chemical Bonding cont. e. Atoms or molecules that gain or lose electrons are called ions. i. Ions have either a + charge, they loss electrons and now have more protons (+) than electrons(-), or ii. a – charge, they gained electrons and now have more electrons (-) than protons (+). iii. Ions with opposite charges can form ionic bonds.

13. Chemical Bonding cont. f. Hydrogen Bonds: i. A weak chemical attraction between hydrogen and fluorine, oxygen, or nitrogen. ii. These type of bonds are not true bonds but more of an attraction. They are easily broken. (Think Velcro) iii. The most common place to find hydrogen bonds is in DNA!!

14. Chemical Bonding cont. • Hydrogen bonds between water molecules cause the cohesion of liquid water. • Cohesion is the attraction between substances of the same kind. • Because of Cohesion- water and other liquid form drops . • This attraction between water molecules causes a condition known as surface tension, which prevents the water from breaking easily.

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16. Chemical Bonding cont. • Water Molecules are also attracted to many other similarly polar substances. • Adhesion is an attraction between different substances. • Because of adhesion, some substances get wet. • It also powers a process called capillary action, in which water molecules move upward through a narrow tube- such as the stem of a plant.

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18. 5. Chemical Formula • A chemical formula is used to show the binding and proportions of atoms that form compounds. • Examples: MgCl2 means 1 Mg and 2 Cl C6H12O6 means 6C,12H and 6O H2SO4 means Na2CO3 means

19. 6. Chemical Reactions • A chemical reaction is the process of breaking chemical bonds or of forming new bonds or both. • In a chemical reaction the atoms of the reactants combine to form the products of the reaction. • CHEMICAL Equations show how reactant change during chemical reactions.

20. Chemical Reactions a. Rules for Balancing Equations • In chemical reactions, matter cannot be created or destroyed- CONSERVATION OF MASS. • The quantity of the products must equal the quantity of the reactants. • Subscripts can NOT be changed • Subscripts only apply to the element that they followCO2 = 1 carbon and 2 Oxygen • Numbers placed in front of a compound carry through the whole compound 2CO2 = 2 carbon and 4 oxygen • Numbers before or after parenthesize get carried through to all the elements 2(NaCl2)2= 4 Na and 8Cl

21. Chemical Equations cont b. Balancing Equations Examples ** Remember - If there is a number in front of the compound then you have more than 1 molecule of that compound 6MgCl2 means 6 Mg and 12 Cl 2C6H12O6 means 12 C, 24 H, and 12 O 4Na2CO3 means Balance _____ H2 + _____ O2 _____ H2O _____ N2 + _____ O2 _____ N2O _____ HgO  _____ Hg + _____ O2

22. 7. Mixtures • Mixture is a composition of two or more substances that are not chemically combined with each other and are capable of being separated. • Types of Mixtures: 1. Solution 2. Suspensions

23. Types of Mixtures cont. a. Solution: • A solution is a mixture in which one or more substances are uniformly distributed in another substance. • The SOLUTE is the substance being dissolved in the solution. (may be ions, atoms, or small molecules). • The SOLVENT is the substance in which the solute is dissolved. • Examples: Soda is a solution. Water is the solvent, Carbon dioxide is the solute that causes the bubbles. Sugar is a solute in regular soda.

24. Type of Mixtures cont. b. Solute to Solvent Ratio: - Concentration: Ratio of solute to a set amount of solvent. High concentration = high solute, low solvent. Dilute= low solute, high solvent Saturated- When you get to a point where no more solute can be dissolved within the solvent, at a given temperature.

25. Type of Mixtures cont. c. Biologically the most important solutions are those in which gases, liquids, and solids, are dissolved in water. - These are referred to as Aqueous Solutions - Water is referred to as the “Universal Solvent.”

26. Aqueous Solution cont. • The polarity of water enables many substances to dissolve in water. • Ionic and polar molecules dissolve best in water • examples: salt, sugar • Nonpolar molecules do not dissolve in well in water. • The polar molecules are more attracted to each other than to the non polar molecules. The non polar molecules are shoved together. • Example: water and oil

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28. Types of Mixtures cont. d. Suspensions: - a suspension is a mixture in which particles spread through a liquid or a gas but settle out over time. - The particles in a suspension are larger than solute particles in a solution. Examples: Italian Dressing,

29. Acids and Bases • Scientists have developed a scale for measuring the relative concentration of hydrogen and hydroxide ions in a solution. • Called the pH SCALE it ranges from 0 to 14. 0- 6.9 = Acidic solution 7 = Neutral Solution 7.1- 14= a basic or alkaline solution Water molecules can break down forming Hydrogen ions, H+, and hydroxide ions, OH-.

30. Acids and Bases cont a. Compounds that form hydrogen ions when dissolved in water are called acids.

31. Acids and Bases cont. b. OH-, Hydroxide ions, are produced when a base is dissolved in a solution. • A basic solution is a solution that contains more hydroxide ions than hydrogen ions

32. pH Scale

33. Testing pH • Acidity can be tested using…. 1. electronic devices 2. Litmus paper (indicator paper that turns red in acids and blue in basic solutions) 3. pH paper (indicator paper that tells you the pH of a solution) * Control of pH is often very important for the survival of an organism

34. Chemistry of Life- Chapter 2 Part B Mrs. Cook Biology

35. A. Organic Compounds • Most matter in your body, besides water, is made up of organic compounds. • What makes a compound organic? • Contain carbon atoms • Forms covalent bonds • Carbon most often bonds with H, O, & C.

36. 1. Carbon Bonding

37. Carbon Bonding- Covalent bond a. Carbon forms covalent bonds with other elements. In this example it forms 4 covalent bonds with which element? _____

38. Carbon Bonding- Covalent bond b. Carbon can bond with other carbon atoms forming a double bond and still bond with hydrogen at the same time. CIRCLE ALL THE COVALENT BONDS

39. Carbon bonding- Carbon Chains c. Carbon and hydrogen can form chains. There are still 4 covalent bonds for each carbon atom.

40. Carbon Bonding- Carbon rings d. Carbon bonding can sometimes form rings. But there are still covalent bonds. FIND THEM!!

41. Carbon Variety- Carbon variety e. Find the Covalent bonds, which are double?

42. Monomers and Polymers • Monomers- small compound • Polymer- the joining of monomers by chemical compound bonds • Monomer Monomer Monomer Monomer Polymer We can create polymers from monomers, or break polymers apart into monomers.

43. Monomers and Polymers

44. Monomers and Polymers Look at all the LEGOS- think of each of these as a monomer. By themselves they are just LEGO bricks…… Put them together- like a polymer- and something else is created!!

45. B. Classification of Organic Compounds • Four classes of Organic molecules: • Carbohydrates • Lipids • Proteins • Nucleic Acids

46. 1. Carbohydrates- “Carbs” • Compound made of carbon, hydrogen and oxygen • Found in a 1:2:1 ratio • Found mainly in fruits, vegetable, and grains and provide energy for humans and animals, and make up cellulose in plants. a. Two Types of Carbs: i. Monosaccharide or simple carbohydrates. • Found in fruits, dairy, white breads, pasta, & white sugar • Body uses them up quickly. • Glucose C6H12O6 and fructose.

47. Carbohydrates cont. ii. Polysaccharides or complex carbohydrates • Found in vegetables, whole grains breads and pasta, brown rice and legumes (bean, peas & lentils.) • Takes longer to digest. • Starch is a long chain of many linked glucose molecules. Potato Cell w/Starch granules Wheat starch granules

48. b. Carbohydrate Monomer • One saccharide or monosaccarharide, the monomer of a carbohydrate

49. Carbohydrate polymers • 2 saccharides make a disaccharide • More than 2 saccharides make a polysaccharide

50. d. How does your body process Carbs? • The liver digests carbohydrates by breaking them down into simple sugars, or glucose, which stimulates the production of insulin in the pancreas. • The insulin functions to get the sugar into the body’s cells to be used as energy. • When digesting simple carbohydrates, insulin levels spike faster, and the carbs are used up more quickly for energy. “sugar high” • Complex carbohydrates take longer to digest, resulting in longer lasting energy, and less of an insulin reaction in the body.