1. Science 10

2. Chemistry of Life Hydrogen Oxygen Carbon Gold Silver
Element - any substance that is comprised of one type of atom and cannot be broken down into another substance.
Examples
Hydrogen
Oxygen
Carbon
Gold
Silver

3. Chemical Bonds
Ionic bonds - formed through the transfer of electrons between two atoms. The bond is due to the attraction of oppositely charged ions (atoms with a negative or positive charge).

4. Chemical Bonds
Covalent bonds - formed through the sharing of atoms between atoms.

5. Mixture - a substance composed of two or more elements or compounds which are physically mixed together, but not chemically combined.

6. Solute - substance that is dissolved.
Solution - mixture of two or more substances in which the substances are evenly distributed.
Solute - substance that is dissolved.
Solvent - substance in which the solute is dissolved.

7. Can it be physically separated?
Matter Flow Chart
MATTER
yes no
Can it be physically separated?
MIXTURE
PURE SUBSTANCE
Is the composition uniform? no
yes
Can it be chemically decomposed? no
yes
Homogeneous Mixture
(solution)
Heterogeneous Mixture
Compound
Element
Colloids
Suspensions

8. Water is the solvent of life

9. Chemical elements and water
Elements of life (most common)
Carbon, hydrogen, oxygen
Other necessary elements & function
Nitrogen (amino acids),
Calcium (bones, teeth),
Phosphorous (ATP, DNA),
Iron (hemoglobin),
Sodium (nerve transmision)

10. Like no other common substance, water exists in nature in all three physical states:
as a solid
as a liquid
as a gas

11. Properties of water Transparency: Cohesion:
Light can easily pass through
Reach inside cytoplasm (water) to
chloroplast, retina
Reach organisms in water
Cohesion:
Water molecules stick together (surface)
Water can be pulled up trees
Small animals can live on water surface (mosquito)

12. Properties of water Solvent Properties (universal solvent)
Allow substance carried in water
blood, sap
Thermal properties (large heat capacity)
requires large amounts of energy to heat
remains stable temperature
fish, blood (carry heat to cold parts)

13. Properties of water Thermal properties (cooling from evaporation)
evaporate at temperatures below boiling
heat energy required to break hydrogen bonds, taken from liquid water cooling it down

14. Hydrophobic Hydrophilic Properties of Water
Cohesion - attraction between molecules of the same substance.
Adhesion - attraction between molecules of different substances.

15. Cohesion:
Water molecules stick together
surface tension

17. Polarity
Polar: Uneven distribution of charge within the molecule. Example: H2O (water)
Non-polar: Even distribution of charge within the molecule. Example: BF3 (boron trifluoride)
Like dissolves like
Something polar dissolves something polar
Something nonpolar dissolves something nonpolar

18. Polar molecules are also soluble in water because they can also form hydrogen bonds with water.
Even large molecules, like proteins, can dissolve in water if they have ionic and polar regions.
Fig. 3.8
Copyright © 2002 Pearson Education, Inc., publishing as Benjamin Cummings
Fig. 3.7
Copyright © 2002 Pearson Education, Inc., publishing as Benjamin Cummings

19. Biochemistry The chemistry of Life Bio-molecules Proteins
Carbohydrates
Lipids (fats, membranes…)
Nucleic Acids (DNA…)

20. Trace elements May be needed in only small amounts but may cause
goiter
May be needed in
only small amounts
but may cause
harm if absent
(iodine)

21. Organic Compounds Contain carbon & found in living organisms
Inorganic Carbon compounds: CO2,
Many inorganics found in living organisms
Iron in blood

22. Macromolecules - large molecules formed through the joining of many monomers (small molecular units) into polymers (larger molecules).
We will be studying 4 important macromolecules: Carbohydrates, lipids, proteins, nucleic acids.

23. Monosaccharides - single sugar molecules (glucose, galactose).
Carbohydrates - sugars which contain C, H and O and are the main energy source for all living things (some organisms also use carbohydrates for structural purposes).
Monosaccharides - single sugar molecules (glucose, galactose).
Disaccharides - carbohydrates composed of two sugar molecules (lactose).
Polysaccharides - large carbohydrates composed of many monosaccharide monomers (starch, cellulose, glycogen).

24. Condensation Reaction: monomers form chains
Remove water to form bonds
Protein synthesis
Fatty acid synthesis 1 2 3
Short polymer
Unlinked monomer
Removal of water molecule 1 2 3 4
Longer polymer
Figure 3.3A

25. Hydrolysis - reverse process of condensation polymers are broken down to monomers
Using water 1 2 3 4
Addition of water molecule 1 2 3

26. Carbohydrate Polymers
Monomer: Monosacccharide
Glucose – the most basic unit of sugar (energy)
The building block
Polysaccharides:
Glycogen: energy storage
Animal muscles
Starch: plant energy storage
Cellulose: plant structure

27. The structure of glucose

28. Starch: plant energy storage Cellulose: plant structure
A polysaccharide is made by linking two (or more) monosaccharides together.
Glycogen:
energy storage
animal muscles
Starch: plant energy storage
Cellulose: plant structure
glucose fructose = sucrose
glucose galactose = lactose

29. Functions of Lipids (fats)
A group of organic compounds, including fats oils, and waxes that are soluble insoluble in water.
Energy storage:
Insulation:
Protection:
Membranes (phospholipids):

30. Glycerol & fatty acid

31. Proteins - macromolecules that contain N, H, O and C
Proteins - macromolecules that contain N, H, O and C. Are comprised of amino acid (the order and combination of these amino acids determines the role of the protein) subunits.
Types of proteins:
Enzymes - carry out the chemical reactions in the organism (lactase, DNA helicase, catalase).
Structural Proteins - aid in building muscles, bones and other components of the organism (keratin, collagen).
Functional Proteins - assist in organism’s daily functioning such as messengers (hemoglobin, insulin), defense or transport.

32. Dehydration synthesis
Protein Synthesis
amino acids link
dipeptides
polypeptide chains (Proteins)
The bonds are called peptide bonds
Dehydration synthesis
Figure 3.13

33. Proteins have levels of organization. Proteins can be denatured.
Primary structure refers to the sequence of amino acids joined by peptide bonds. Secondary structure is any folding or twisting of the chain in space. Tertiary structure comes about when proteins fold into globular shapes. Quaternary structure occurs in proteins that have more than one polypeptide chain twisted together.
Extremes in temperature or pH, or chemicals, radiation, and so forth can cause proteins to unfold, thus denaturing them.

34. Enzymes Enzyme Active Site Protein Biological catalyst
Example: amylase
Active Site
Location where substrate (reactant) binds

35. Lock and Key Model (enzyme-substrate specificity)

40. Effects of variables on enzymes
Temperature pH

41. Nucleic Acids - macromolecules that contain H, O, N, C and P
Nucleic Acids - macromolecules that contain H, O, N, C and P. The 2 kinds of nucleic acids are DNA and RNA which store and transmit genetic information (the “blueprint” to make you).
Comprised of nucleotide (5-C sugar, phosphate group and nitrogenous base) monomers.