Download Nutrition: A Closer Look at Nutrients

Chapter 2 - You matter! What are you made of?
A. Atoms - Smallest particle of an element that still has all the properties of that
element. All matter in the universe is composed of atoms.
States of matter: Solid-atoms are tightly packed in definite shape.
Liquids-atoms are packed loosely.
Gas-no definite shape or volume.
There are 500,000,000,000 billion atoms in this (.)
Three subatomic particles
In the nucleus
1. Proton (+)
2. neutron (n)
Outside the nucleus
3. electron (-)
If an atom is expanded to the size of Giant Stadium the nucleus would be the
size of a bee & electrons would be flying around in the nose bleed section.
B. Elements – found on the periodic table. Elements cannot
be broken down into smaller particles without losing its
properties.
Examples of elements: carbon C oxygen O hydrogen H nitrogen N phosphorous P sulfur S
90% of all living organisms are composed of just 6 elements C, O, H, N, P & S.
Above draw Neon(Ne)
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Ions – any atom or molecule with a charge, positive or negative.
In order for an atom to have a charge, it has to gain or lose election.
The process of making an ion is called ionization.
All elements on the periodic table are neutral. The # of positive charges from the
protons and the # of negative charges from the electrons make the atom neutral.
To figure out the
charge compare
protons to electrons.
Protons = _____
Electrons = ____
Charge? = _____
Add one electron:
To figure out the charge
compare protons to electrons.
Protons = _____
Electrons = ____
Charge? = _____
The loss of one electron:
To figure out the charge
compare protons to electrons.
Protons = _____
Electrons = ____
Charge? = _____
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C. Compounds – 2 or more kinds of atoms combined in a specific proportion.
The smallest part of a Compounds is a molecule.
Example: Water
Lolly Q
Name the
process that
releases energy
by breaking
bonds.
1. Bonds – hold atoms together to make compounds
 Bonds contain STORED ENERGY from the sun
Breaking these bonds releases energy
 2 types of bonds
Covalent – sharing of electrons
When carbon bonds with carbon it’s a covalent bond.
Water also bonds covalently.
Ionic bonding – transfer of electrons
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Water – is compound that is considered polar(an uneven charge)
Importance of water due to polarization & hydrogen bonding
1- universal solvent
2- high heat capacity (water temperature moderation)
3- capillary action-helps water up a tree
4- surface tension
Acids & Alkaline – depends upon the # of hydronium
ions and hydroxide ion
Acids produce H+(hydronium ion) in aqueous solutions
water
HCl
H+ (hydronium ion) + Cl-
Alkaline produce OH- (hydroxide ion) in aqueous solutions
water
Na+ + OH- (hydroxide ion)
NaOH
H2O
H2O
H2O
H+ H2O OH-
H2O
H2O
H+ H2O H+
H2O
H+ H2O OH-
H2O H2O
H2O H2O
H2O
H2O
OH-
OH-
OH-
OH-
H+
H+
H2O molecules = _______
H2O molecules = _______
H2O molecules = _______
H+
H+
H+
molecules = _______
molecules = _______
molecules = _______
OH- molecules = _______
OH- molecules = _______
OH- molecules = _______
Neutral, acid or alkaline
Neutral, acid or alkaline
Neutral, acid or alkaline
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II.
How do we diagram food as chemical compounds?
A. Diagramming Bonds between atoms
1. Single & multiple Bonds
C-C
O-O
C=C
O=O
C C
2. How do you know how many bonds an atom can make?
 C, H, O, N bonds determined by the number of valence
electrons
 Bond number + valence number of electrons = 8
B. Molecular Formulas for Compounds
C6 H12O6
- Uses letters and numbers
- Gives total number of each atom,
but NOT how they are arranged
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C. Structural Formulas for Compounds
C
H
C
H
C
Shows numbers of atoms
and how they are
combined
C
C
D. Chemical Reactions between Compounds
(Worksheets)
Practice:
- For each of the structural formulas below, write the molecular formula.
1.
3.
H2O
2.
NH3
NC2H5O2
4.
H
H
C6 H12O6
-Study the structural formulas. Figure out how many bonds hydrogen, oxygen, carbon and
nitrogen will normally form.
2
4
3
Hydrogen - _______
Oxygen - _______
Carbon - ________
Nitrogen - _________
1
-Label the reactants and the products in the chemical reaction diagrammed below See if you can
draw the structural formula for each reactant and product following the rules you figured out
above.
Reactants/Raw Materials
Products
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III. The Big Three of Organic Foods
CARBOHYDRATES: Saccharides
Prefix
Image
Base
Mono
Di
Poly
Saccharide
Saccharide
Simple
Sugar
Saccharide
Function
Store energy
Source of Energy
Make up Cell Structure
Examples
Simple Sugar (glucose),
Sucrose (table sugar),
Lactose
Starch
Cellulose
(Plants
only)
Glycogen (Animals
only)
Structure
See Worksheets
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Key Features
Hexagon Shape
2 H for 1 O
PROTEINS: Peptides
Prefix
Di
Poly
Image
Amino
Acid
Base
Function
Peptide
Building blocks for Proteins
Peptide
Structure (muscles)
Enzymes, Hormones, Antibodies
Examples
Amino Acid
Dipeptide
Polypeptide
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Structure
N-C-C----N-C-C
Key Features
N-C-C ---N-C-C --- N-C-C --- N-C-C ---N-C-C
N – the only one of R = Variable
the Big 3 with
group for 20
Nitrogen
different amino
acids
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FATS (lipids) also known as Triglycerides
Image
Base
Glycerol
Fatty Acid
Lipid (Fat)
Function
Holds Fat together
Builds Fat
Long Term Energy Storage and insulation
Also makes up cell membrane
Examples
Lard, Butter, Oil
Structure
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Key Features
Glycerol has 3 vertical
Carbons
Biochemistry in a Nutshell
Macromolecule
(Biological
Polymer)
Repeating Unit
(Building Block)
Function in Living Organisms
Molecular
Structure
Key Features
Mono and Disaccharides are used for
energy
Carbohydrates
Polysaccharides are used for storage
and cell structure (ex. Cell
membrane)
Simple Sugar
Amino Acid
Muscles
Proteins
Enzymes
N
Hormones
Antibodies
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Energy Storage
Lipids (Fat)
Insulation
E
Cell Structure (Cell membrane and
ER)
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