Anatomy & Physiology Chpt 2

Front 1

Chemistry

Back 1

Is the science of change

-The structure of atoms

-The basic chemical buildings blocks

-How atoms combine to form increasingly complex structures

Front 2

Matter

Back 2

Is made up of atoms

-Atoms joined together to form chemicals with different characteristics

-Chemical characteristics determine physiology at the molecular and cellular levels

Front 3

Subatomic Particles

Back 3

Proton

-Positive charge, 1 mass unit

Neutron

-Neutral, 1 mass unit

Electron

-Negative charge, low mass

Front 4

Atomic Structure

Back 4

Atomic number

-Number of protons

Nucleus

-Contains protons and neutrons

Electron cloud

-Contains electrons

Front 5

Chemical Bonds

Back 5

Involve the sharing, gaining, and losing of electrons in the valence shell

3 major types of chemical bonds

1. Ionic bonds

-Attraction between cations (electron donor) and anions (electron acceptor)

2. Covalent bonds

-Strong electron bonds involving shared electrons

3. Hydrogen bonds

-Weak polar bonds based on partial electrical attractions

Front 6

Chemical Bonds

Back 6

Forms molecules and/or compounds

Molecules

- 2 or more atoms joined by strong bonds

Compounds

- 2 or more atoms OF DIFFERENT ELEMENTS joined by strong or weak bonds

-Compounds are all molecules, but not all molecules are compounds

- H2= molecule only H2O= molecule and compound

Front 7

Ionic bonds

Back 7

One atom the electron donor loses one or more electrons & becomes a cation, w/ a positive charge

- Another atom the electron acceptor gains those same electrons and becomes an anion, w/ a negative charge

-Attraction between the opposite charges then draws the ions together

Front 8

Elements and Isotopes

Back 8

Isotopes are the specific version of an element based on its mass number

-Mass number= number of protons plus the number of neutrons

-Only neutrons are different because the number of protons determines the element

Front 9

Atomic Weights

Back 9

Exact mass of all particles

-Measured in moles

-Average of the mass numbers of the isotopes

Front 10

Covalent Bonds

Back 10

Involve the sharing of pairs of electrons between atoms

-1 electron is donated by each atom to make the pair of electrons

-Sharing 1 pair of electrons is a single covalent bond

-Sharing 2 pairs of electrons is a double covalent bond

-Sharing 3 pairs of electrons is a triple covalent bond

Front 11

Nonpolar covalent bonds

Back 11

Involve equal sharing of electrons because atoms involved in the bond have equal pull for the electrons

Front 12

Polar covalent bonds

Back 12

Involve the unequal sharing of electrons because 1 of the atoms involved in the bond has a disproportionately strong pull on the electrons

-Form polar molecules, like water

Front 13

Hydrogen Bonds

Back 13

Bonds between adjacent molecules, not atoms

-Involves slightly negative portions of polar molecules being attracted to one another

-Hydrogen bonds between H2O molecules cause surface tension

Front 14

Molecular weights

Back 14

The molecular weight of a molecule is the sum of the atomic weights of its component atoms

-H: approximately 1

-O: approximately 16

-H2: approximately 2

-H2O: approximately 18

Front 15

Chemical Reaction

Back 15

Either new bonds are formed or existing bonds are broken

Reactants

-Materials going into a reaction

Products

-Materials coming out of a reaction

Metabolism

-All of the reactions that are occurring at one time

Front 16

Basic Energy Concepts

Back 16

Energy

-The power to do work

Work

-A change in mass or distance

Kinetic energy

-Energy of motion

Potential energy

-stored energy

-chemical energy

-Potential energy stored in chemical bonds

Front 17

Chemical Reactions

Back 17

Types of Chemical Reactions

1. Decomposition reaction (catabolism)

2. Synthesis reaction (anabolism)

3. Exchange reaction

4. Reversible reaction

Front 18

Decomposition Reaction (Catabolism)

Back 18

-Breaks chemical bonds

-AB : A+B

-Hydrolysis A-B+H2O: A-H+HO-B

Front 19

Synthesis Reaction (Anabolism)

Back 19

-Forms chemical bonds

- A+B: AB

-Dehydration synthesis (condensation reaction)

A-H+HO-B: A-B+H2O

Front 20

Exchange Reaction

Back 20

-Involves decomposition first, then synthesis

-AB+CD : AD+CB

Front 21

Reversible Reaction

Back 21

-A+B <---> AB

-At equilibrium the amounts of chemical do not change even though the reactions are still occurring

-Reversible reactions seek equilibrium, balancing opposing reaction rates

-Add or removed reactants

-Reaction rates adjust to reach a new equilibrium

Front 22

Chemical Reactions

Back 22

-In cells cannot start without help

-Activation energy is the amount of energy needed to get reaction started

-Enzymes are protein catalysts that lower the activation energy of reactions

Front 23

Exergonic (Exothermic) Reactions

Back 23

-Produce more energy than they use

Front 24

Endergonic (Endothermic) Reactions

Back 24

Use more energy than they produce

Front 25

Nutrients

Back 25

Essential molecules obtained from food

Front 26

Metabolites

Back 26

Molecules made or broken down in the body

Front 27

Inorganic Compounds

Back 27

Molecules not based on carbon and hydrogen

-Carbon dioxide, oxygen, water and inorganic acids, bases and salts.

Front 28

Water

Back 28

Accounts for up to 2/3's of total body weight

-A solution is a uniform mixture for 2 or more substances

-It consists of solvent, or medium, in which atoms, ions, or molecules of another substance, called solute, are individually dispersed

Front 29

Solubility

Back 29

Water's ability to dissolve a solute in a solvent to make a solution

Reactivity

-Most body chemistry occurs in water

High Heat capacity

-Water's ability to absorb and retain heat

Lubrication

-To moisten and reduce friction

Front 30

The properties of Aqueous Solutions

Back 30

Ions and polar compounds undergo ionization or, dissociation in water

-Polar water molecules form hydration spheres around ions and small polar molecules to keep then in solution

Front 31

The properties of Aqueous Solutions

Back 31

Electrolytes and body fluids

-Electrolytes are inorganic ions that conduct electricity in solution

-Electrolyte imbalance seriously disturbs in vital body functions

Front 32

Hydrophilic

Back 32

Hydro= water, philos= loving

-Interacts with water

-Includes ions and polar molecules

Front 33

Hydrophobic

Back 33

Phobos= fear

-Does not interact with water

-Includes nonpolar molecules, fats, and oils

Front 34

Colloid

Back 34

A solution of very large organic molecules

-For ex. blood plasma.

Front 35

Suspension

Back 35

A solution in which particles settle (sediment)

-For ex. whole blood

Front 36

Concentration

Back 36

The amount of solute in a solvent (mol/L, mg/mL)

Front 37

pH

Back 37

The concentration of hydrogen ions (H+) in a solution

Front 38

Neutral pH

Back 38

A balance of H+ and OH-

-Pure water =7.0

Front 39

Acidic pH lower Than 7.0

Back 39

High H+ concentration

-Low OH- concentration

Front 40

Basic or (alkaline) pH Higher Than 7.0

Back 40

Low H+ concentration

-High OH- concentration

pH of Human Blood

-Ranges from 7.35 to 7.45

Front 41

Acid

Back 41

A solute that adds hydrogen ions to a solution

-Proton donor

-Strong acids dissociate completely in solution

Front 42

Base

Back 42

A solute that removes hydrogen ions from a solution

-Proton acceptor

-Strong base dissociate completely in solution

Front 43

Weak acids and Weak Bases

Back 43

Fail to dissociate completely

-Help to balance the pH

Front 44

Salts

Back 44

Solutes that dissociate into cations and anions other than hydrogen ions and hydroxide ions

Front 45

Buffers

Back 45

-Weak acid/salt compounds

-Neutralize either strong acid or strong base

-Sodium bicarbonate is very important in humans

Front 46

Antacids

Back 46

-Basic compounds that neutralize acid and from a salt

-Alka-Seltzer, tums, rolaids, etc.

Front 47

Carbohydrates

Back 47

-Contains carbon, hydrogen, and oxygen in a 1:2:1 ratio

-Monosaccharide ---- Simply sugar

-Disaccharide -----two sugars

-Polysaccharide---- many sugars

Front 48

Monosaccharides

Back 48

-Simple sugars with 3 to 7 carbon atoms

-Glucose, fructose, galactose

Front 49

Disaccharides

Back 49

-Two simple sugars condensed by dehydration synthesis

-Sucrose, maltose

Front 50

Polysaccharides

Back 50

-Many monosaccharides condensed by dehydration synthesis

-Glycogen, starch, cellulose

Front 51

Fatty Acids

Back 51

-Long chains of carbon & hydrogen w/ a carboxyl group (COOH) at one end

-Are relatively nonpolar, except the carboxyl group

Fatty acids may be:

-Saturated w/ hydrogen (no covalent bonds)

-Unsaturated (one or more double bonds)

-Monounsaturated=one double bond

-Polyunsaturated=two or more double bonds

Front 52

Eicosanoids

Back 52

-Derived from the fatty acid called arachidonic acid

-Leukotrienes

-Active in immune system

Front 53

Porstaglandins

Back 53

-Local hormones, short chain fatty acids

Front 54

Glycerides

Back 54

-Fatty acids attached to a glycerol molecule

Front 55

Triglycerides

Back 55

-are the 3 fatty acid tails

-Also called triacylglycerols or neutral fats

-Have 3 important functions

1. Energy source

2. Insulation

3. Protection

Front 56

Steroids

Back 56

-Four rings of carbon & hydrogen w/ and assortment of functional groups

Front 57

Cholesterol

Back 57

Component of plasma (cell) membranes

Front 58

Estrogens and testosterone

Back 58

-Sex hormones

Front 59

Corticosteroids and calcitriol

Back 59

-Metabolic regulation

Front 60

Bile salts

Back 60

-Derived from steroids

Front 61

Phospholipids and Glycolipids

Back 61

-Diglycerides attached to either a phosphate group (phospholipid) or a sugar (glycolipid)

-Generally, both have hydrophilic heads and hydrophoboic tails & are structural lipids, components of plasma (cell) membranes

Front 62

Proteins

Back 62

-Are the most abundant & important organic molecules

-Contain basic elements

-Carbon (C), hydrogen (H), oxygen (O), and nitrogen (N)

-Basic building blocks

-20 amino acids

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Back 63

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