Anatomy and physiology chap 2

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118 Terms

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Chemistry
The science of change: structure of atoms, basic chemical building blocks, atoms combine to form increasingly complex structures
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Matter
Made up of atoms; atoms join together to form chemicals with different characteristics; chemical characteristics determine physiology at the molecular and cellular levels
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Atoms
Building blocks of matter
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Subatomic particles
protons, neutrons, electrons
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Proton
Positive charge, 1 mass unit
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Neutron
Neutral, 1 mass unit
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Electron
Negative charge, low mass
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Atomic structure
atomic number, nucleus, electron cloud
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Atomic number
Number of protons
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Nucleus
Contains protons and neutrons
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Electron cloud
Contains electrons
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Hydrogen-1
A typical hydrogen nucleus contains a proton and no neutrons, mass number:1
A typical hydrogen nucleus contains a proton and no neutrons, mass number:1
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Hydrogen-2, deuterium
Nucleus contains a proton and a neutron, mass number: 2
Nucleus contains a proton and a neutron, mass number: 2
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Hydrogen-3, tritium
Nucleus contains a proton and two neutrons, mass number: 2
Nucleus contains a proton and two neutrons, mass number: 2
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Oxygen, O (65)
A component of water and other compounds; gaseous form is essential for respiration
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Carbon, C (18.6)
Found in all organic molecules
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Hydrogen, H (9.7)
A component of water and most other compounds in the body
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Nitrogen, N (3.2)
Found in proteins, nucleic acids, and other organic compounds
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Calcium, Ca (1.8)
Found in bones and teeth; important for membrane function, nerve impulses, muscle contraction, and blood clotting
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Elements
Determined by atomic number of an atom; most basic chemicals
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Isotopes
Specific version of an element based on its mass number
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Mass number
Number of proton plus the number of neutrons
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Why only are the number of neutrons different?
Because the number of protons determines the elements
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Atomic weight
Exact mass of all particles; measured in moles; average of the mass numbers of the isotopes
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Electrons in the electron cloud
Determine the reactivity of an atom
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Electron cloud
Contains shells, or energy levels, that hold a maximum number of electrons
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Valence shell
Outermost shell that determines bonding
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Chemical bonds
Involve the sharing, gaining, and losing of electrons in the valence shell; form molecules and/or compounds
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Three types of chemical bonds
Ionic, covalent, hydrogen
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Ionic bonds
Attraction between cations (electron donor) and anions (electron acceptor) then draws the two ions together
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Covalent bonds
Strong electron bonds involving shared electrons
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Hydrogen bonds
Weak polar bonds based on partial electrical attractions; bonds between adjacent molecules, not atoms, slightly positive and negative portions of polar molecules being attracted to one another
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Molecules
Two or more atoms joined by strong bonds
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Compounds
Two or more atoms OF DIFFERENT ELEMENTS joined by strong or weak bonds
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Explain: H2= Molecule only, H2O= molecule and compound
Compounds are all molecules, but not all molecules are compounds
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Electron donor
Loses one or more electrons and becomes a cation, with a positive charge
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Electron acceptor
Gains those same electrons from the donor and becomes an anion, with a negative charge
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Ion
A subscript plus or minus sign following the symbol of an element
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Single covalent bond
Sharing one pair of electrons
Sharing one pair of electrons
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Double covalent bond
Sharing two pairs of electrons
Sharing two pairs of electrons
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Triple covalent bond
Sharing three pairs of electrons
Sharing three pairs of electrons
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Nonpolar covalent bonds
Involve equal sharing of electrons because atoms involved in the bond have equal pull for the electrons
Involve equal sharing of electrons because atoms involved in the bond have equal pull for the electrons
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Polar covalent bonds
Involve unequal sharing of electrons because one of the atoms involved in the bond has a disproportionately strong pull on the electrons; ex: water
Involve unequal sharing of electrons because one of the atoms involved in the bond has a disproportionately strong pull on the electrons; ex: water
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Hydrogen bonds between H2O molecules causes
Surface tension
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Chemical reaction
Either new bonds are formed or existing bonds are broken; reactants, products, metabolism; in cells, cannot start without help
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Reactants
Materials going into a reaction
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Products
Materials coming out of a reaction
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Metabolism
All of the reactions that are occurring at one time
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Energy
Power to do work
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Work
A change in mass or distance
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Kinetic energy
Energy of motion
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Potential energy
Stored energy
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Chemical energy
Potential energy stored in chemical bonds
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Types of chemical reactions
Decomposition (catabolism), synthesis (anabolism), exchange, reversible
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Decomposition reaction (catabolism)
Breaks chemical bonds
Breaks chemical bonds
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Synthesis reaction (anabolism)
Forms chemical bonds
Forms chemical bonds
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Exchange reaction
Involves decomposition first, then synthesis
Involves decomposition first, then synthesis
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Reversible reaction
At equilibrium the amounts of chemicals do not change even though the reactions are still occurring; seek equilibrium, balancing opposing reaction rates; add or remove reactants
At equilibrium the amounts of chemicals do not change even though the reactions are still occurring; seek equilibrium, balancing opposing reaction rates; add or remove reactants
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Activation energy
The amount of energy needed to get a reaction started
The amount of energy needed to get a reaction started
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Enzymes
Protein catalysts that lower the activation energy of chemical reactions; are not changed or used up in the reaction
Protein catalysts that lower the activation energy of chemical reactions; are not changed or used up in the reaction
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Exergonic (Exothermic) Reactions
Produce more energy than they use; releases energy; reaction ends with lower energy than it started with
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Endergonic (Endothermic) Reactions
Use more energy than they produce; absorbs energy; reaction ends with higher energy than it started with
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Nutrients
Essential molecules obtained from food
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Metabolites
Molecules made or broken down in the body
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Inorganic compounds
Molecules not based on carbon and hydrogen; carbon dioxide, oxygen, water, and inorganic acids, bases, and salts
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Water
Accounts for up to two-thirds of your total body weight
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Solution
Uniform mixture of two or more substances; consists of a solvent, or a medium, in which atoms, ions, or molecules of another substance, called a solute, are individually dispersed
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Solubility
Water’s ability to dissolve a solute in a solvent to make a solution
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Reactivity
Most body chemistry occurs in water
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High heat capacity
Water’s ability to absorb and retain heat
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Lubrication
To moisten and reduce friction
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Colloid
A solution of very large organic molecules; ex: blood plasma
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Suspension
A solution in which particles settle (sediment); ex: whole blood
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Concentration
The amount of solute in a solvent (mol/L, mg/mL)
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PH
The concentration of hydrogen ions (H+) in a solution
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Neutral pH
A balance of H+ and OH-; pure water= 7.0
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Acidic
Lower than 7.0; high H+ concentration; low OH- concentration
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Basic (or alkaline)
Higher than 7.0; low H+ concentration; high OH- concentration
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pH of human blood
Ranges from 7.35 to 7.45
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pH Scale
Has an inverse relationship with H+ concentration; more H+ ions means lower pH, fewer H+ ions means higher pH
Has an inverse relationship with H+ concentration; more H+ ions means lower pH, fewer H+ ions means higher pH
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Acid
A solute that adds hydrogen ions to a solution; proton donor; strong ones dissociate completely in solution
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Base
A solute that removes hydrogen ions from a solution; proton acceptor; strong ones dissociate completely in solution
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Weak acids and weak bases
Fail to dissociate completely; help to balance the pH
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Salts
Solutes that dissociate into cations and anions other than hydrogen ions and hydroxide ions
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Buffers
Weak acid/salt compounds; neutralize either strong acid or strong base; sodium bicarbonate is very important in humans
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Antacids
Basic compounds that neutralize acid and form a salt; alka-seltzer, tums, rolaids, etc
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Organic molecules
Contain H, C, and usually O; covalently bonded; contain functional groups that determine chemistry; carbohydrates, lipids, proteins (amino acids), nucleic acids
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Amino group— NH2
Acts as a base, accepting H+, depending on pH; can form bonds with other molecules; ex: amino acids
Acts as a base, accepting H+, depending on pH; can form bonds with other molecules; ex: amino acids
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Carboxyl group— COOH
Acts as an acid, releasing H+ to become R—COO-; ex: fatty acids, amino acids
Acts as an acid, releasing H+ to become R—COO-; ex: fatty acids, amino acids
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Hydroxyl group— OH
May link molecules through dehydration synthesis (condensation); hydrogen bonding between hydroxyl groups and water molecules affects solubility; ex: carbohydrates, fatty acids, amino acids
May link molecules through dehydration synthesis (condensation); hydrogen bonding between hydroxyl groups and water molecules affects solubility; ex: carbohydrates, fatty acids, amino acids
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Phosphate group— PO4
May link other molecules to form larger structures; may store energy in high-energy bonds; ex: phospholipids, nucleic acids, high-energy compounds
May link other molecules to form larger structures; may store energy in high-energy bonds; ex: phospholipids, nucleic acids, high-energy compounds
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Carbohydrates
Contain carbon, hydrogen, and oxygen in a 1:2:1 ratio; monosaccharide, disaccharide, polysaccharide
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Monosaccharide
Simple sugars with 3 to 7 carbon atoms; ex: glucose, fructose, galactose
Simple sugars with 3 to 7 carbon atoms; ex: glucose, fructose, galactose
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Disaccharide
Two simple sugars condensed by dehydration synthesis; ex: sucrose, maltose
Two simple sugars condensed by dehydration synthesis; ex: sucrose, maltose
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Polysaccharide
Many monosaccharide condensed by dehydration synthesis; ex: glycogen, starch, cellulose
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Breakdown of sucrose into simple sugars by hydrolysis
Reverses the steps of dehydration synthesis; a complex molecule is broken down by the addition of a water molecule
Reverses the steps of dehydration synthesis; a complex molecule is broken down by the addition of a water molecule
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Lipids
Mainly hydrophobic molecules such as fats, oils, and waxes; made mostly of carbon and hydrogen atoms; fatty acids, eicosanoids, glycerides, steroids, phospholipids and glycolipids
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Fatty acids
Long chains of carbon and hydrogen with a carboxyl group (COOH) at one end; relatively nonpolar, except the carboxyl group; saturated and unsaturated
Long chains of carbon and hydrogen with a carboxyl group (COOH) at one end; relatively nonpolar, except the carboxyl group; saturated and unsaturated
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saturated fatty acid
With hydrogen, no covalent bonds
With hydrogen, no covalent bonds
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unsaturated fatty acid
One or more double bonds; monounsaturated, polyunsaturated
One or more double bonds; monounsaturated, polyunsaturated