1. Chemistry of Life

2. Imagine this..
It has been a long day of school, and you are extremely frustrated because all of your teachers, except you’re wonderful Biology teacher, have assigned you tons of homework. “I’m gonna have to pull an all-nighter,” you think.

3. Imagine this..
You’re parents decides to make you dinner to help you get through the night. What should they cook?

4. Concept Map

5. Concept Map

6. Concept Map

7. Concept Map Carbon Compounds Carbohydrates Lipids Nucleic acids
include
Carbohydrates
Lipids
Nucleic acids
Proteins
that consist of
that consist of
that consist of
that consist of
Sugars and
starches
Fats and oils
Nucleotides
Amino Acids
which contain
which contain
which contain
which contain
Carbon,
hydrogen,
oxygen
Carbon,hydrogen,
oxygen, nitrogen,
phosphorus
hydrogen,oxygen,
nitrogen,

8. Why do we learn Chemistry in 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.

9. Ch. 2. Outline 2-1: Nature of Matter 2-2: Properties of Matter Atoms
Elements and Isotopes
Chemical Compounds
Chemical Bonds
2-2: Properties of Matter
Water Molecule
Solutions and Suspensions
Acids, Bases, and pH

10. Ch. 2. Outline 2-3: Carbon Compounds
Macromolecules
Carbohydrates
Lipids
Nucleic Acids
Proteins
2-4: Chemical Reactions and Enzymes
Chemical Reactions
Energy in Reactions
Enzymes
Enzyme Action

11. Section 1: Nature of Matter
What are Atoms?
The smallest unit of matter that cannot be broken down chemically
What composes Atoms?
Protons – positively charged (p+) particles, found in the nucleus
Neutrons – Particles with no charge (n0), found in the nucleus
Electrons – negatively charged (e-), found in energy levels

12. History of the Atom Democritus – “Atomos
Thomson Plum Pudding – “Plum pudding Model
Rutherford model – Planetary structure
Bohr Model – Discrete orbitals
Electron Cloud Model – Electrons orbit with specific clouds and shapes.

13. The Atom

14. Nature of Matter (con’t)
What are elements?
An element is a pure substance made up of only one kind of atom, represented by symbols, such as, H, O, N, C, etc.
What is an isotope?
Isotopes are atoms of an element that contain different numbers of neutrons
Carbon-12, Carbon-13, and Carbon-14

15. Chemical Bonding
Chemical Bonding describes the forces which joins atoms to form compounds.
A compound is a substance formed by the chemical combination of two or more elements in definite proportions
There are three types of bonds that you will learn about:
Covalent Bonds
Ionic Bonds
Van der Waals Forces

16. Chemical Bonding (con’t)
When do covalent bonds form?
Covalent bonds form when two or more atoms share electrons.
A molecule is a group of atoms held together by covalent bonds
What is a polar molecule?
A polar molecule has an unequal distribution of charge
I.e. H2O acts like a charge particle.

17. Covalent Bonds

18. Chemical bonding (con’t)
Van der Waals force or Hydrogen Bonding is a weak chemical attraction between polar molecules

19. Chemical Bonding (con’t)
What is an Ion?
An atom or molecule that has gained or loss one or more electrons.
How is an Ionic Bond formed?
When two or more ions of opposite charge are held together

20. Ionic Bonds Sodium atom (Na) Chlorine atom (Cl) Sodium ion (Na+)
Chloride ion (Cl-)
Transfer
of electron
Protons +11
Electrons -11
Charge
Protons +17
Electrons -17
Charge
Protons +11
Electrons -10
Charge
Protons +17
Electrons -18
Charge

21. Ionic Bonds

22. Water and Living Things
About 70% of our body is water, both inside and outside of all of our cells.
There are four major properties of water in biology:
Storage of Heat
Cohesion
Surface Tension
Adhesion

23. Properties of Water
Storage of Heat – Water helps cells maintain homeostasis by controlling internal body temperature because it retains heat
Cohesion – An attraction between substances of the same kind, I.e. water to form drops
Surface tension – forms drops of water because of attraction, prevents surface from breaking easily
Adhesion – an action between different substances, I.e water to walls of plant tube to cause capillary action.

24. Solutions and Suspensions
Water is not always pure—it is often found as part of a mixture
Mixture – a material composed of two or more elements that are physically combined not chemically combined.
Example: The Atmosphere, Your body, Water.

25. Solution and Suspensions
A solution is when a chemical change occurs that breaks apart bonds, usually in water.
Salt and Water
Two parts of a solution
Solute – the substance that is dissolved
Solvent – the substance that does the dissolving
Water is an excellent solvent because of it’s polar bonds.

26. Aqueous Solutions
An aqueous solution is a mixture in which one or more substances are distributed evenly in water or blood to be delivered in the body
There are two main properties of solution:
Polarity pH

27. Properties of Solutions
Polarity – Water is the universal solvent due to the fact that it is a polar substance. The polarity of water helps break apart bonds, especially ionic bonds. Nonpolar molecules, such as those found in oils, do not “mix” or dissolve in water.

28. Polarity of Water

29. Properties of Solutions (con’t)
The Acidity of solutions is a very important property in biology.
Acidity is measured using the pH scale
pH measure the amount of H+ ions in a solution
What would pOH measure?
Acids are solutions that range from 0 to 7 on the pH scale. They form hydrogren ions when dissolved in water
Bases are solutions that range from 7 to 14 on the pH scale. They form hydroxide ions when dissolved in water.

30. pH Scale
What are some acids and bases found in your body?

31. Section 3: Chemistry of Cells
As we go further into Biology, we will learn about cells and cell functions. An important aspect of biological cells are Carbon Compounds.
Carbon Compounds are made up of building blocks called Monomers.
Many monomers together are called a polymer

32. Carbon Compounds There are 4 main organic compounds found in the body:
Carbohydrates
Lipids
Protein
Nucleic Acids
Name an example of each.

33. Carbon Compounds (con’t)
Carbohydrates
Contains C,H, O with a 1:2:1 ratio.
Quick Source of energy, “carbo loading”
Basic monomers are monosaccharides
Glucose, Fructose, Galactose, etc.
Two monosaccharides form a disaccharide
Sucrose, more commonly known as Table Sugar
Many monosaccharides come together and make Polysaccharides
Starch – plants
Glycogen – animals
Cellulose in plants’ cell walls

34. Carbohydrates

35. Carbon Compounds (con’t)
Lipids
Also contains C, H, O, in no specific ratio
Include fats, oils, waxes, and steroids
Important in the structure and function of cell membrane, and light absorbing compounds called pigments
A long-term store for energy
Monomers are one glycerol and three fatty acids, called a triglyceride

36. Carbon Compounds (con’t)
Saturated fats: all the C atoms in the fatty acids are bonded to two Hydrogen atoms forming a straight chain.
Will they be solid or liquid at Room Temperature?
Unsaturated fats: some of the C atoms are linked by a double covalent bond with only one hydrogen atoms which forms kinks in the chain.

37. Carbon Compounds (con’t)
Proteins
Large macromolecules formed from monomers called amino acids
Generally fold into compact shapes on interaction with water
Many important functions in the body:
Collagen
Hemoglobin
Antibodies – aid immune system
Actin & Myosin
Enzymes – catalysts that speed up chemical reactions by lowering activation energy

38. Hemoglobin and Actin/Myosin Complex

39. Activation Energy Energy-Absorbing Reaction Energy-Releasing Reaction
Products
Activation energy
Activation
energy
Reactants

40. Enzyme and Substrate Enzyme (hexokinase) Substrates Products
Glucose
Substrates
ATP
bind to
enzyme
are converted
into products
Enzyme-substrate
complex
Enzyme
(hexokinase)
ADP
Products
Glucose-6-
phosphate
are released
Active site

41. Carbon Compounds Nucleic Acids Found in every cell
Made up of monomers called Nucleotides
DNA
Deoxyribonucleic Acid
RNA
Ribonucleic Acid
ATP
Adenosine Triphosphate
A high-energy storing molecule recycled in cells

42. DNA Structure

43. End of Organic Compounds