1. Biochemistry

2. Atoms
An atom that has either gained or lost an electron is called an Ion
CONSERVATION OF MASS –
Things can move / change position. But ALL the mass that is available is ALL the mass that will ever be available.
Periodic Table
Mass Number – how much it weighs in grams
Atomic Number – location on the periodic table (number of protons)
Isotopes – variations in elements based on number of neutrons

3. Atomic Mass = # Protons + # Neutrons The atomic mass of carbon = 12 The atomic # of carbon = 6 = the # of protons # neutrons = Atomic Mass - # protons # neutrons = = 6

4. Label your Periodic Table
s- block
p- block 1 2 3 4 5 6 7 2 3 4 5 6 7 3 4 5 6
d- block (n-1) 4 5
f- block
(n-2)

5. Compound-2 or more elements combined chemically
A compound is made up of different elements
The smallest particle of a compound with independent existence is: The molecules of that compound Ex: A CO2 Molecule as opposed to millions of CO2 Molecules

6. Nobel Gases: always have their outside electron shell full: They never bond with other atoms

7. Covalent Bonds:
When Atoms share electrons in their outer energy levels:
O2 H20

8. Atoms that have gained or lost an electron are called ions. NaCl HCl
Ionic Bonds: an electric attraction between two or more differently charged atoms or groups
Atoms that have gained or lost an electron are called ions.
NaCl HCl

9. Properties of Matter Physical Properties
Properties that do not change the chemical nature of matter
Examples
Color, Smell, Freezing Point, Boiling Point, Melting Point, Polarity, and Density
Physical change – change in its state

10. Properties of Matter Chemical Properties
Properties that DO change the chemical nature of matter
Examples
PH, Combustion, reactivity with water, explosions!
Compounds put together that create a new compound

11. States of Matter Physical Changes Chemical Changes Solid, Liquid, Gas
Changes properties of matter all together
Ex. Spoiling Milk

12. Properties of Chemical Change
Forms or breaks chemical bonds
Energy is taken (endothermic) or energy is released (exothermic)
One or more new chemical substances are formed
The process is usually difficult to reverse

13. Examples of Chemical Change
Digestion
Photosynthesis
Respiration
Burning
Decomposition

14. Structure of Atoms Protons: Neutron: Electron:
A sub atomic particle that is located in the nucleus and has a positive charge
Neutron:
A sub atomic particle that is located in the nucleus and has a neutral charge
Electron:
The smallest of the subatomic particles that carry a negative charge and surround the nucleus.

15. Energy and Chemical Change
Any energy an object has because of its position is called Potential energy.
The energy in motion (actual) is called Kinetic energy.

16. Atoms Electrons circle the nucleus in the electron shell
Noble gases all have there outer most electron full of electrons.

19. Mixtures Solution Suspension
Homogenous (same) mixture of components that stay mixed
Sugar and water
Suspension
Mixture of two substances that may mix right away, but do NOT stay mixed up
Starch and water

20. Mixtures
Colloid
A suspension of small particles that are dispersed into another substance
Partial Mix

21. Types of Bonds Cation- Anion –
A positivily charged ion (more protons than electrons)
Anion –
Negatively charged ion that contains more electrons in its outer shell compared to the protons.

22. Bonds
Ionic Bond
Sending an electron to an atom that is positively charged (opposing charges attract)
EX.
Na (+) = Cl (-)
Salt
H (+) = Cl (-)
Hydrochloric Acid

23. Bonds Covalent Bonds Sharing of electrons for the benefit of both EX.

24. Bonds Hydrogen Weaker bond
It is the type of bonds that hold our DNA molecules together.
Must include a Hydrogen molecule
Also, usually attaches to a electronegative atom

25. Properties of Water Polarity of water
Water is made up of two polar covalent bonds, but the molecule has no overall net charge
Oxygen slightly negative (heavier)
Hydrogen slightly positive (lighter)
Allows for cohesion of other water molecules

26. Properties of water Temperature stabilizing effects
Water is warm – hydrogen electrons move about and break leading to evaporation
Water is cold – Hydrogen molecules get closer together and form a lattice (solid) structure that we know as ICE

27. Properties of water Water Cohesion-
Water molecules binding to other water molecules
Hydrogen bonds attracted to each other and stick together!
Ions and polar molecules easily dissolve in water. The water molecules surround and separate the solute being dissolved.

28. Acids, Bases, and Buffers
pH – “Potential Hydrogen ions”..
Measurement of how many concentrated H+ ions there are.
1 – very acidic
14 – very basic
7 – Neutral

29. Acids, Bases, and Buffers
Acids – donate H+ to a solution increasing the conc. of H+ in the solution
Bases – Absorb / accept H= and they lower their concentration in the solution
Buffers – Are compounds that help absorb or donate H+ at the appropriate time as to keep a solution balanced
Salts – Can be formed by the combination of a strong acid and a strong base

30. Carbon Compounds All life organisms are made up of Carbon
Organic Molecules
Organisms consist mostly of which atoms?
Carbon, Nitrogen, Hydrogen, Oxygen, Phosphorous, trace elements

31. Chemistry of Carbon Carbon has how many bonds?
How many valence electrons does carbon have?
Carbon can bond to 4 other molecules
Carbon can form a single, double, or triple bond

32. Functional Groups of Carbon
A chain of carbon and hydrogen is called a hydrocarbon.
EX. Methane, Ocatane
Just C and H
There is ENERGY in these bonds!!! Do you recognize the molecules?

33. Other important carbon based groups:
Hydroxyl Group: OH
Carboxyl Group:
COOH
Amino Group:
NH2 or NH3
Phosphate Group:
PO3 or PO4

34. Hydroxyl –OH organic compounds with OH = alcohols
names typically end in -ol
ethanol

35. Carboxyl –COOH C double bonded to O & single bonded to OH group
compounds with COOH = acids
fatty acids
amino acids

36. Amino -NH2 N attached to 2 H compounds with NH2 = amines
amnio acids
NH2 acts as base
ammonia picks up H+ from solution

37. Phosphate –PO4 P bound to 4 O connects to C through an O
PO4 are anions with 2 negative charges
function of PO4 is to transfer energy between organic molecules (ATP)

38. How do cells build organic compounds?
Reactions: the use of raw materials “atoms”, energy, and enzymes to do one of the following
Functional group transfer – One molecule gives up a functional group which is then attached to another molecule
Electron transfer – One or more electrons is stripped from one molecule and donated to another molecule
Rearrangement – A juggling of internal bonds converting one type of organic compound into another
Condensation (Hydrolysis) – the removal or addition of water to create new bonds and break existing ones
Cleavage – A molecule splits into two smaller ones.

39. Important construction terms
Monomer : a molecule that is building block for something larger
Dimer : two monomer stuck together
Polymer : more than two monomers stuck together
Dehydration : Pulling water out of two molecules so as to bind them together
Hydrolysis : Adding water to a molecule to break it apart

40. Carbohydrates Contain – Carbon, Hydrogen, and Oxygen in a 1:2:1 ratio
Example: Glucose (C6H12O6)
The monomers that make them up are called monosaccharides

41. What are Carbs used for? Uses – Energy, Structure, Signals
These monomers usually form a ring structure, especially in water.
Examples Glucose and Fructose

42. Carbohydrates When do you notice about glucose and fructose?
They have the same number of atoms but they are in a different arrangement.
They are called isomers
The condensation of two monosaccharides is called a disaccharide.
Example - Sucrose

43. Carbohydrates
The largest carbohydrates are starches

44. Carbohydrates
The reaction that breaks down complex molecules – reverse condensation is called hydrolysis.
We have an enzyme in our body to do this process
Amylase (found in saliva)
New Study in sleep deprivation

45. Starch VS. Cellulose
We can break down starches, but our body cannot break down cellulose.

46. Tests for Carbohydrates
Monosaccharides
Disaccharides
Polysaccharides
Iodine
No Change
Turns Black
Benedicts Solution
Color changes with heat

47. Lipids Lipids contain Carbon, Hydrogen, and Oxygen
EX – Fats, Phospholipids, waxes, sterols “Steroids”

48. Lipids
They are used in living things for energy storage, structural molecules, and signaling molecules
Basic Structures
Tail and Head

49. Triglycerides

50. Saturated Fats:
Only form single bonds with Carbon Atoms: No room for more hydrogen atoms
Unsaturated Fats:
Form double bonds in Carbon atoms

51. All lipids are insoluble in water – A good test?
Water Solubility
Paper smear test

52. Phospholipids
Found in the cell membrane

53. Cell Membrane

54. Test for Fats TEST FAT NOT A FAT Brown Paper Paper Changes
(transparent)
Dries the same
Water Solution
They separate
They Mix

55. Proteins Proteins are made up of: Carbon, Hydrogen, Oxygen, & Nitrogen
Ex. – Eggs, seeds, hair, and meat
Basic Monomers – Amino Acids (aa)

56. Amino Acids (aa) Each aa is going to contain four distinct groups
Carboxyl Group – COOH
Amino Group – NH3
R Group (20 different R groups)
A Hydrogen atom – H
If there are twenty different amino acids

57. Protein Structure
Through a series of dehydration reactions, aa are joined into a chain to form a protein.
A special bond is formed
Peptide Bond
Polypeptide – polymer of aa

59. Protein Structure When you have two aa together Three or more aa
Dipeptide
Three or more aa
Polypeptide
These are used by living organisms for:
Enzymes, structures, transport, and signaling

60. 3D structure of proteins
Level 1
Level 2
Level 3
Level 4

62. Proteins DENATURATION Is the breaking down of molecules
Other molecules can be attached to proteins
Glycoproteins and Lipoproteins

63. Test for Proteins: Xanthopoetic test
NOT A PROTEIN
Nitric Acid
Turns Yellow
No Color Change

64. Enzymes A chemical that speeds up a reaction is called a
Catalyst
Proteins that do this process are called
Enzymes
Ex. – Sucrase, Amylase, Lactase

65. Nucleic Acids
All instructions for cellular activity are in the Nucleic Acids
Two kinds of Nucleic Acids
DNA
Holding genetic information
Where is it found?
In nucleus on chromosomes
RNA
Holding info for building proteins
Where are they found?
Everywhere in a cell

66. What makes them up? Complex monomers – Nucleotides
Bonds between them are called phosphodiester bond
Formed by a phosphate