The Chemical Level of Organization Chapter 2. Chemistry Review Matter – anything that occupies...
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Transcript of The Chemical Level of Organization Chapter 2. Chemistry Review Matter – anything that occupies...
The Chemical Level of Organization
Chapter 2
Chemistry Review Matter – anything that occupies space and has
weight
Atom – smallest stable unit of matter Protons – positive electrical charge Neutrons - uncharged Electrons – negative electrical charge
Atomic Number Number of protons in the nucleus
Atomic Weight (Mass) Approx. number of protons + neutrons
Chemistry Review Atom with a full outer electron shell is stable
helium, neon, argon, krypton, xenon, and radon
Atoms without full shell can achieve stability by sharing, gaining, or losing electrons through chemical reactions Many of these reactions produce molecules Molecules called compounds contain atoms of
more than one element
What are valence electrons
Chemistry Review Element
Consists of entirely one type of atom
Many found in the body Oxygen
65% Carbon
18.6% Hydrogen 9.7% Nitrogen
3.2% Calcium
1.8% Phosphorus 1% Potassium <1% Chlorine, Magnesium,
Sodium, Sulfur, Iron, Iodine
Compound Molecules containing
more than one type of atom
Water - H2O Salt - NaCl Methane - CH4
Chemistry Review Compounds have properties that can be very
different from their components. A mixture of hydrogen and oxygen is a flammable
gas Combining hydrogen and oxygen produces water
Bonding Ionic Bonds Covalent Bonds
Single Double Polar
Hydrogen Bonds
Ionic Bonding Ions are charged atoms – having lost or
gained electron(s) Atoms are held together by the attraction
between positive and negative charges
Ionic Bond - Sodium Chloride NaCl
Covalent Bonding Atoms share electrons to complete outer
electron shells Resulting bond is called a covalent bond
Ethane
Hydrogen chloride
Single covalent bond Sharing of one pair of electrons
Double Covalent Bond Sharing of two pairs of electrons
Polar Covalent An unequal sharing of electrons In water:
The oxygen atom has a stronger attraction for the electrons – the electrons spend more time there – so there is a negative charge
The hydrogen side is positively charged
Hydrogen Bond Within molecules some hydrogen atoms are
positively charged and some are negatively charged
Hydrogen bonding does not form molecules but can alter shapes or pull molecules together
Acids Bases
A solute Releases hydrogen
ions
HCl H+ + Cl-
A solute Removes hydrogen
ions
NaOH Na+ + OH-
Hydroxide ions have an affinity for hydrogen ions
OH- + H+ H20
pH pH is the concentration of hydrogen ions in a
solution
pH range is 0-14, pure water is 7 Below 7 is acidic…hydrogen ions outnumber
hydroxide ions Above 7 is basic….hydroxide ions outnumbers
hydrogen ions
In excessive amounts H+ will disrupt cell and tissue function
Blood pH ranges from 7.35-7.45 Below 7 can produce a coma Over 7.8 causes uncontrolled, sustained muscular
contractions
Buffers Compounds responsible for stabilizing pH
Remove or replace Hydrogen ions Antacids
Alka-Seltzer, Rolaids, Tums Tie up excess Hydrogen ions in the stomach
Extracellular - Sodium bicarbonate, ammonia Intracellular – proteins, phosphate
H2O + CO2 H2CO3 H+ + HCO3-
carbonic acid (H2CO3) - bicarbonate (HCO3-)
Nutrients and Metabolites Nutrients are essential elements and
molecules absorbed from foods
Metabolites are all molecules synthesized or broken down by chemical reactions in our body
Nutrients and metabolites can be categorized as inorganic or organic
Inorganic Compounds Generally do not contain carbon
Carbon Dioxide, Oxygen
Water
Inorganic Acids and Bases
Salts