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THE TOP 10 ELEMENTS FOUND IN YOUR BODY
THE “BIG 4”
OTHER (4%)
96% of your body is composed of these 4 elements:
Nitrogen (3%)
Oxygen (65%)
Carbon (18.5%)
Hydrogen (9.5%)
Calcium
ChlorinePotassiumPhosphorus
SulfurSodium
• Trace amounts (less than 0.1%) of 15 other elements are also found in the body
Per
cent
age
(%)
of b
ody’
s co
mpo
siti
on
• Elements consist of atoms
atom: smallest unit of matter that still has properties of an element
• Atoms are made of subatomic particles:
1) protons: positive charge
2) electrons: negative charge
3) neutrons: no charge (neutral)
THE ATOM: BASIC STRUCTURE
Nucleus
Hydrogen atom1 Proton0 Neutrons1 Electron
Carbon atom6 Protons6 Neutrons6 Electrons
Proton Neutron
Nucleus:
Electron
Forces of attraction between positive and negative charges hold the fast-moving electrons (negative) close to the nucleus (positive).
• All atoms of a given element have same number of protons = atomic number
Helium = 2 protons = atomic number =2
Carbon = 6 protons = atomic number = 6
• Same # protons & electrons, electrical charge = 0, what is charge of He?
atomic mass: protons + neutrons
C = 6 protons + 6 neutrons = 12
isotope:
Importance of Electrons
• Determine how atoms interact
• Energy level differences, higher energy farther from nucleus
electron shell: energy levels around nucleus in which electrons are found
ELECTRON SHELLS AND ATOM STABILITY
ELECTRON SHELLSElectrons move around the nucleus in designated areas called electron shells. An atom can have as many as seven electron shells in total.
First electron shell(capacity: 2 electrons)
Second electron shell(capacity: 8 electrons)
Vacancy
The chemical characteristics of an atom depend upon the number of electrons in its outermost shell.
How does a Reaction Occur?
• 2 atoms with incomplete e- shells, give/take of e-, such that both atoms gain full shells
Chemical bond: 2+ atoms attracted to one another by a reaction
molecule: 2+ atoms held together by chemical bond, e.g., water H2O
Types of Chemical Bonds
1) Ionic Bonds (e.g., NaCl = salt)
1 atom loses e- & 1 atom gains e-
Result = form ions or charged atoms
ionic bond: 2 ions with opposite charges are attracted to each other
SODIUMATOM11 p+
11 e-
electron transfer
CHLORINEATOM17 p+
17 e-
SODIUMION
11 p+
10 e-
CHLORINEION
17 p+
18 e-
Types of Chemical Bonds
2) Covalent Bonds (e.g., H2O)
2 atoms share outer shell e-
- The number of single covalent bonds is dependent on the # of e- needed to fill the outer shell
COVALENT BONDSOTHER EXAMPLES OF COVALENT BONDS
Each oxygen atom shares two electrons. This is called a double bond.
There are several different ways of representing molecular structure.
O2 molecule
“Space-filling”model
“Lewis”model
“Ball-and-stick”model
CH4molecule(methane)
Water: The Basis of All Life
polar covalent bonds: 2 atoms with very different electronegativities (attraction for shared e- in covalent bond) – results in charged molecule (+ & - ends)
hydrogen bonds: H(+) attracted to O(-)\
WATER: HIGH SURFACE TENSION
Pressure applied to water surface
“V”-shaped water molecules are held together by hydrogen bonds. The bonds are just strong enough to give water a surface tension with net-like properties.
Hydrogenbond
WATER: STRONG COHESIVENESSBecause of the cohesive properties of water, trees such as the giant sequoia are able to transport water molecules from the soil to their leaves 300 ft. above.
As each water molecule evaporates, it pulls additional water up through the tree because of the “sticky-ness” of the hydrogen bonds that link the water molecules.
Water molecule released into the atmosphere
300 ft.
Water molecule pulled into root system
Water molecules pulled upward
6-ft.-tall man
Frozen water
WATER: LOWER DENSITY WHEN FROZEN
FROZEN WATERHydrogen bonding arranges water molecules into a crystalline lattice, keeping them slightly farther apart and, therefore, less dense.
LIQUID WATERWater molecules move about freely, allowing them to be closer to one another.
RELATIVE AREA OCCUPIED BY THE SAME NUMBER OF H2O MOLECULES: Liquid water
Blood
THE pH SCALE
ACIDS BASES
H+ ion Water OH– ion
Bases are fluids that have a greater proportionof OH– ions to H+ ions.• OH– ions bind with H+ ions, neutralizingacids.• Strong bases are caustic to your skin.• Bases can be found in many household cleaners.• Bases are generally bitter in taste and soapy.
Acids are fluids that have a greater proportion of H+ ions to OH– ions.• H+ ions are very reactive.• Strong acids are corrosive to metals.• Acids break down food in your digestive tract.• Acids are generally sour in taste.
Beer
Soda
Battery acid
Coffee
Water
Ammonia
BleachBaking soda
Soda, with a pH of about 3.0, is 10,000 times more acidic than a glass of water, with a pH of 7.0!
0 7 141312111098654321
SUMMARY: THREE TYPES OF BONDS
1 COVALENT BONDA strong bond formed when atoms share electrons in order to become more stable, forming a molecule.
2 IONIC BONDAn attraction between two oppositely charged ions, forming a compound.
3 HYDROGEN BONDAn attraction between the slightly positively charged hydrogen atom of one molecule and the slightly negatively charged atom of another.
H2 molecule
Bon
d S
tren
gth
Strongest
Weakest
NaCl compound
H2O molecule H2O molecule
Four Macromolecules of Life
1) Carbohydrates (sugars = alcohol & aldehyde or ketone)
2) Lipids (fats = alcohol & carboxylic acid)
3) Proteins (made of amino acids)
4) Nucleic Acids
How are Polymers Made?
Dehydration Synthesis
- “free” monomers have H & OH groups
- Add “free” monomers to polymer chain = 1 H2O released
- Form new covalent bond between monomers
* Make polymers (macromolecules) for storage/transport, but cells must break them down to monomers in order to use them
How are Polymers Broken Down?
Hydrolysis (hydro = water; lysis = to break
- Reverse of dehydration synthesis
- Break covalent bond by adding water
- OH group to 1 monomer & H to adjacent monomer
COMPLEX CARBOHYDRATES
FORMATIONBond(s) between simple sugars formed
Glucose Fructose
POLYSACCHARIDESComplex carbohydrates formed by the union of many simple sugars
DISACCHARIDESComplex carbohydrates formed by the union of two simple sugars
DIGESTIONBond(s) between simple sugars broken
Sucrose(table sugar)
Starch(consists of hundreds of glucose molecules)
ENERGY
Sugars broken down furtherSugars broken down further
ENERGY
Time
Blo
od s
ugar
leve
l
Time
Blo
od s
ugar
leve
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Complexcarbohydrates
Fructose
Depending on their structure, dietary carbohydrates can lead to quick-but-brief or slow-but-persistent increases in blood sugar.