Basic Chemistry Revised

7/23/2019 Basic Chemistry Revised

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Copyright 2003 Pearson Education, Inc. publishing as Benjamin Cummings


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Matter anything that occupiesspace and has mass (weight)

Energy the ability to do work

Chemical

Electrical

Mechanical

Radiant



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Elements

Fundamental units of matter

96% of the body is made from 4 elements Carbon (C)

Oxygen (O) Hydrogen (H)

Nitrogen (N)

Atoms Building blocks of elements



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Nucleus

Protons (p+)

Neutrons (n0)

Outside ofnucleus

Electrons (e-)


Figure 2.1


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Atomic number

Equal to the numberof protons that the

atoms contain

Atomic massnumber

Sum of the protonsand neutrons



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Isotopes Have the same

number of protons

Vary in number of

neutrons

Atomic weight

Close to mass number

of most abundantisotope

Atomic weight reflectsnatural isotope

variationCopyright 2003 Pearson Education, Inc. publishing as Benjamin Cummings


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Radioisotope

Heavy isotope

Tends to be unstable

Decomposes to more stable isotope

Radioactivity Process of spontaneous atomic decay



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Molecule two or more atomscombined chemically

O2, H2O, CaCl2, CH4

Compound two or more differentatoms combined chemically

H2O, CaCl2, CH4



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Atoms are united by chemical bonds

Atoms dissociate from other atoms whenchemical bonds are broken



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Electrons occupy energy levels called

electron shells

Electrons closest to the nucleus are moststrongly attracted

Each shell has distinct properties

Number of electrons has an upper limit

Shells closest to nucleus fill first

Bonding involves interactions betweenelectrons in the outer shell (valence shell)

Full valence shells do not form bondsCopyright 2003 Pearson Education, Inc. publishing as Benjamin Cummings


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Have complete valence shells and arestable

Rule of 8s

Shell 1 has 2electrons

Shell 2 has 8electrons

10 = 2 + 8 Shell 3 has 18 electrons

18 = 2 + 8 + 8



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Valence shells arenot full and areunstable

Tend to gain, lose,or share electrons

Allows for bond

formation, whichproduces stable

valence.


Figure 2.4b


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Ionic Bonds Form when electrons are completely

transferred from one atom to another

Ions Charged particles

Anions are negative

Cations are positive Either donate or accept electrons



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Covalent Bonds Atoms become stable through shared electrons

Single covalent bonds share one electron

Double covalent bonds share two electrons


Figure 2.6c


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Covalent bonded

molecules Some are

non-polar

Electrically neutralas a molecule

Some arepolar

Have a positive andnegative side


Figure 2.7


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Hydrogen bonds

Weak chemical bonds

Hydrogen is attracted to negative portion ofpolar molecule

Provides attraction between molecules



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Synthesis reaction (A+B=AB)

Atoms or molecules combine

Energy is absorbed for bond formation



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Decomposition reaction (AB=A+B)

Molecule is broken down

Chemical energy is released


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Exchange reaction (AB + C = AC + B) Involves both synthesis and decomposition

reactions

Switch is made between molecule parts anddifferent molecules are made



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Slide 2.21Copyright 2003 Pearson Education, Inc. publishing as Benjamin Cummings

Organic compounds Contain carbon

Most are covalently bonded

E.g. C6H12O6 (glucose)

Inorganic compounds Lack carbon

Tend to be simpler compounds

E.g. H2O (water)


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Water Most abundant inorganic

compounds

Vital properties High heat capacity

Polarity/solvent properties

Chemical reactivity

Cushioning


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Salts

Easily dissociate into ions in the

presence of water Vital to many body functions

Include electrolytes which conductelectrical currents


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Acids

Can release detectable hydrogenions

Bases

Proton acceptors

Neutralization reaction

Acids and bases react to form waterand a salt


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Slide 2.25Copyright 2003 Pearson Education, Inc. publishing as Benjamin Cummings Figure 2.11

Measures relativeconcentration ofhydrogen ions

pH 7 = neutral

pH below 7 = acidic

pH above 7 = basic

Buffers

Chemicals that canregulate pH change

potenz Hydrogen -

power of Hydrogen


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Carbohydrates

Contain carbon, hydrogen, and oxygen

Include sugars and starches


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Monosaccharides simple sugars

glucose, fructose, ribose

Disaccharides two simple sugars joinedby dehydration synthesis

Maltose = glucose + glucose Sucrose = glucose + fructose

Lactose = glucose + galactose

Polysaccharides long branching chainsof linked simple sugars

Starch, glycogen, cellulose, chitin


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Lipids Contain carbon, hydrogen, and oxygen

Insoluble in water

E.g. neutral fats (stearic acid, oleic acid-palmoil, palmitic acid palm oil/lard)

Waxes (beeswax, lanolin oil used inointments, cosmetics & drugs)

Phosphoglycerides, Sphingolipids

sphingomyelins, cerebrosides, prostaglandin,steroids)


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Slide 2.33aCopyright 2003 Pearson Education, Inc. publishing as Benjamin Cummings

Proteins

Made of amino acids

Contain carbon, oxygen, hydrogen,nitrogen, and sometimes sulfur

Oxytocin, Vasopressin, Insulin,Glucagon, Antibodies


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Figure 2.16

Enzymes

Act as biological catalysts

Increase the rate of chemical reactions


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Nucleic Acids

Provide blueprint of life

Nucleotide bases

A = Adenine

G = Guanine

C = Cytosine

T = Thymine

U = Uracil Make DNA and RNA


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Figure 2.17c

Deoxyribonucleicacid (DNA)

Organized bycomplimentary

bases to form doublehelix

Replicates beforecell division

Provides instructionfor every protein inthe body


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Adenosine triphosphate (ATP) Chemical energy used by all cells

Energy is released by breaking high

energy phosphate bond

ATP is replenished by oxidation of foodfuels


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Basic Chemistry Revised

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