Pearson’s Anatomy and Physiology Chapter 2 – Flashcards
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Matter
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anything that occupies space and has mass
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States of Matter
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Solid, Liquid, Gas
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Electrical Energy
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results from the movement of charged particles. (The nervous system uses electrical currents)
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Elements
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Unique substances that cannot be broken down into simpler substances by ordinary chemical methods. 118 Elements are recognized, 92 of them occur in nature, the other 26 are man made.
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Carbon, Oxygen, Hydrogen and Nitrogen make up ________ % of the human body
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96%
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Periodic table
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provides a complete listing of known elements to help explain the properties of each element and how they react with one another
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Elements are made of small particles known as
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Atoms
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Atomic Symbol
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a 1 or 2 letter chemical short hand, usually the first letter(s) of an elements name.
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Nucleus
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Central structure that contains protons and neutrons that are tightly bound together. Protons and Neutrons are heavy particles and have the same mass, and are desginated as 1 amu (atomic mass unit). 99.9% of an atoms mass is located in the nucleus/
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Protons
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Have a positive electrical charge, located in the nucleus
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Neutrons
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Have a neutral charge, located in the nucleus,
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Atomic Mass
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The approximate total mass of an atom; also called atomic weight. Given as a whole number, the atomic mass approximately equals the mass number.
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Electrons
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Have a negative charge equal in strength to the positive charge of a proton. However the electron ony has about 1/2000 the mass of a proton, and is usually represented as 0 amu.
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Orbitals
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The regions around the nucleus in which a given electron pair is likely to be found
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Atomic Number
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Equal to the number of protons in the nucleus, and is written as a subscript to the left of the atomic symbol
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Mass Number
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The sum of the masses of it's protons and neutrons. The mass of electrons is so small that it's ignored. The Mass Number is written as a superscript on the left hand size of the Atomic Number.
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Isotopes
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Atoms of the same element that differ in the number of neutrons they contain.
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Atomic Weight
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Is an average of the relative weights (mass numbers) of all the isotopes of an element. Example the atomic weight of Hydrogen is 1.008
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Radioisotopes
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A heavier isotope that has an unstable nucleus and undergoes radioactive decay to decompose into a more stable form.
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Subatomic Particles
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Alpha (packets of 2p +2n), Beta (electron like negative particles), or Gamma (Electromagnetic energy that is ejected from the atomic nucleus)
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Molecule
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A combination of two or more of the same atoms that are held together by chemical bond.
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Compound
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A combination of two or more different kinds of atoms that bond together.
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Solutions
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Homogeneous mixtures of components that may be gases, liquids or solids.
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Homogeneous
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COMPOSED OF IDENTICAL PARTS; UNIFORM IN COMPOSITION
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Solvent
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The substance that presents in greatest amount, usually liquids.
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Solutes
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Components in smaller quantities within a solution
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Chemical Bonds
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A union between the electron structures of two or more atoms
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Electron Shells
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The formation of electrons in the electron cloud around the nucleus of an atom that occupy regions. Atoms known so far have electrons in seven shells, and the shells are numbered 1 - 7
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Energy Level
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Each electron shell represents a different energy level. In general the terms electron shell and Energy Level are used interchangeably.
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Valence Shell
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Indicates an atoms outermost energy level or that portion containing the electrons that are chemically reactive.
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Octet Rule / Rule of Eights
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Except for a shell of 1, which is full when it has 2 electrons, atoms tent to interact in such a way that have eight electrons in their Valence Shell.
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Ionic Bonds
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A chemical bond between atoms formed by the transfer of one or more electrons from one atom to another.
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Anion
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A negatively charged ion
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Cation
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A positively charged ion
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Covalent Bonds
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Electron sharing productes molecules in wich the shared electrons occupy a single orbital common to both atoms.
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Polar Molecules
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Unequal electron pair sharing, molecules in which the charges are unevenly distributed; they can attract each other
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Nonpolar Molecule
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Molecule that shares electrons equally and does not have oppositely charged ends
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electronegativity
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A measure of the ability of an atom in a chemical compound to attract electrons
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Molecular Formula
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A chemical formula that shows the number and kinds of atoms in a molecule, but not the arrangement of the atoms.
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Biochemistry
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Chemistry dealing with chemical compounds and processes in living plants and animals
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Organic Compounds
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Compounds that contain Carbon
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Inorganic Compounds
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Chemicals in the body that are do not contain carbon. (For example, Water, Salts, Acids and Bases.)
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Why is Water Vital to Life?
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High Heat Capacity, High Heat of Vaporization, Polar Solvent Properties, Reactivity, Cushioning.
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Universal Solvent
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Water is considered a Universal Solvent, due to its polarity and ability to dissolve many different solutes
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Hydration Layers
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water forms layers of molecules around large charged molecules such as proteins, shielding them from the effects of other charged substances in the vicinity and preventing them from settling out of solution; protein-water mixtures are biological colloids; blood plasma and cerebrospinal fluid
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Salt
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An ionic compunt that contains Cations other than H+ and Anions other than the hydroxl ion (OH-). A compound resulting from the formation of an ionic bond; also called an ionic compound.
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Electrolytes
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Substances that conduct an electrical current in solution
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Acids
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Releases Hydrogen Ions (H+) in Deductible amounts. Because the hydrogen ion is just a hydrogen nucleus, or "naked" proton, acids are also defied as proton donors.
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Bases
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Take up Hydrogen Ions.
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Bicarbonate Ion
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HCO3-, Carbon dioxide mixed with water in plasma in blood, particularly abundant in the blood.
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Ammonia
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A small, very toxic molecule (NH3) produced by nitrogen fixation or as a metabolic waste product of protein and nucleic acid metabolism.
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PH Units
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The relative concentration of hydrogen ions in various body fluids is measured in concentration units
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PH Scale
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measurement system used to indicate the concentration of hydrogen ions (H+) in solution; ranges from 0 to 14
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Neutralization Reaction
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a chemical reaction in which an acid and a base interact with the formation of a salt
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Strong Bases
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Dissociated completely into metal ions and hydroxide ions in aqueous solutions.
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Weak Bases
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React with water to form the hydroxide ion and the conjugate acid of the base.
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Strong Acids
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Completely dissociate in water
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Weak Acids
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Do not Dissociate completely, and dissociate in a predictable way.
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Carbohydrates
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Contain Carbon, Hydrogen, and Oxygen, and generally hydrogen and oxygen atoms occur in a 2:1 Ratio as in water.
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Classification of Carbohydrates
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Monosaccharide (one sugar), Disaccharide (two sugar), and Polysaccharide (many sugars)
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Monosaccharides
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Simple Sugars, or single chain or ring structure containing from three to seven carbon atoms. Generally carbon, hydrogen and oxygen occur in a 1:2:1 Ratio. Monosaccharides are named according to the number of carbon atoms they contain. (most important to the body are the pentose (5 carbon) and the hexose (six carbon) sugars. The Pentose Deoxyribose is part of DNA and the Glucose is a hexose, and is blood sugar.
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Disaccharides
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Double Sugar, is formed when two monosaccharides are joined by dehydration synthesis.
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Polysaccharides
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Carbohydrate containing more than two monsaccharides joined by glycosidic bonds. Starch, glycogen, and cellulose.
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Lipids
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Insoluble in water but dissolved in other lipids and in organic solvents such as alcohol and ether. Energy-rich organic compounds, such as fats, oils, and waxes, that are made of carbon, hydrogen, and oxygen.
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Triglycerides
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known as fats when solid or oils when liquid, composed of fatty acids and glycerol.
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Saturated Fats
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Fatty acid chains with only single covalent bonds between carbon atoms.
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Unsaturated Fats
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A Fatty acid that contains one or more double bond between carbon atom (monounsaturated and polyunsaturated)
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Trans Fats
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Common in types of margarines and baked products, oils have been solidified by the addition of H atoms at cites of Carbon Double bonds.
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Phospholipids
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A lipid made up of a glyerol joined to two fatty acids and a phosphate group; has two hydrophobic tails and a polar, hydrophilic head
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Steroids
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A type of lipid characterized by a carbon skeleton consisting of four rings with various functional groups attached.
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Proteins
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Compose 10-30% of cell mass and is the basic structural material of the body. Many play a vital roll in cell function, Proteins include enzymes (biological catalysts) hemoglobin of the blood, contractile proteins of the muscle. All proteins contain carbon, oxygen, and nitrogen and many contain sulfur.
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Amino Acids
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The building blocks of proteins, of which there are 20 common types. All Amino acids have two important function groups, amine group (-NH2) and an organic acid group (-cooh). Amino Acids can either be a base (proton acceptor) or a acid (proton donor).
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Fibrous Proteins
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bind structures together and for providing strength in certain body tissues. ex: collogen and keratin (Structural Proteins)
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Globular Proteins
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These proteins are small spheres with little to no water inside. They have hydrophobic amino acids in the inside and hydrophilic R groups on the outside. (Functional Proteins)
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Enzymes
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Globular Proteins that act as biological catalysts.
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Catalysts
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Substances that regulate and accelerate the rate of biochemical reactions but are not used up or changed in those chemical reactions.
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Nucleic Acids
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Composed of carbon, oxygen, hydrogen, nitrogen and phosphorus, and is the largest molecule in the body, and have two major classes, Deoxyribonucleic Acid (DNA) and Ribonucleic Acid (RNA)
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Necloutides
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The structural units of nucleic acid
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5 Types of Nucleotide Structure:
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Adenine (A), Guanine (G), Cytosine (C), Thymine (T), and Uracil (U)
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Double Helix
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The form of native DNA, referring to its two adjacent polynucleotide strands wound into a spiral shape.
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Complementary Bases
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Two bases that pair together. A is complementary to T and C is complementary to G.
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Adenosine Triphosphate
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ATP Molecule in cells that stores and releases chemical energy for use in body cells. ATP plays a role in rigor mortis.
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ADP
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(Adenosine Diphosphate) The compound that remains when a phosphate group is removed from ATP, releasing energy
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Chemical Properties are Determined primarily by Neutrons? T/F?
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False
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RNA
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A type of nucleic acid consisting of nucleotide monomers with a ribose sugar and the nitrogenous bases adenine (A), cytosine (C), guanine (G), and uracil (U); usually single-stranded; functions in protein synthesis and as the genome of some viruses.
