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78 Cards in this Set
- Front
- Back
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iso
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equal
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lip
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fat
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-lyt
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dissolvable
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mono
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one
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poly
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many
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-valent
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having power
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Atoms
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smallest particle of an element
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Matter
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anything that takes up space and has weight
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Elements
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Unique subtances; composed of chemically identical atoms; cannot be decomposed
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Atomic weight
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the number of protons plus the number of neutrons in one atom
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Isotopes
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Different atomic forms of the same element; they differ in the number of neutrons in the nucleus
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Half-life of an isotope
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The time it takes for one half of the isotope to decay to a non radioactive form
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Molecule
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two or more atoms
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Compound
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atoms of two different element combined to form
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Energy
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The ability to do work or to put matter into motion
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Kinetic energy
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energy of motion
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Potential energy
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Inactive or stored energy
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Three states of matter
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Gaseous, liquid, solid
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Two energy forms
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Kinetic and potential
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Four energy forms
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Chemical, electrical, mechanical, radiant
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When energy is converted from one form to another, is all the energy reusable?
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No, some is lost to the environment in the form of heat
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Three subatomic particles
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Protons, electrons, neutrons
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Number of protons in any atoms are equal to
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the number of its electrons
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Planetery model of the atom
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Protons and neutrons in center with electrons in specific orbits. There is an electron cloud around the nucleus
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Atomic number
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Identifier of each atom; the number of protons in the nucleus
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Radioisotopes uses in medicine
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Diagnosis and treatment; tagging in X-ray to trace anatomy
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Bond formation
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An energy relationship that involves interactions between tje electrons of the reacting atoms
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Valence shell
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Atom's outer most shell; the electrons of valence shell determine the chemical behavior of the atom
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8
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The number of electrons in the valence shell making the atoms stable
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Chemical reactions
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atoms combining with or dissociate from other atoms
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Differentiation between matter and energy
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Matter has mass; energy does not. Matter occupies space; energy does not
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Example of chemical energy
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Chemical energy harvested from food runs the body
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Example of electrical energy
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Nervous system uses electrical currents to conduct impulses throughout the body
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Example of mechanical energy
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Muscles in legs shorten and pull bones, causing limb to move
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Example of radiant energy
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Light energy stimulates retina to enhance vision
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ATP
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adenosine triphosphate; universal energy compound used; where chemical energy is trapped and transformed into electrical or mechanical energy
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Orbital model of an atom
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Depicts general location of electrons outside the nucleus as a haze of negative charge
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Four elements that make up 96% of body weight
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Carbon, oxygen, hydrogen and nitrogen
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Relationship between atoms and elements
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Elements are composed of more or less identical atoms
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Type of charge of a proton
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positive
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Type of charge of a neutron
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neutral
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Type of charge of an electron
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negative charge equal in strength to the positive charge of the protons
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Three types of chemical bonds
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Ionic, Covalent and Hydrogen
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Importance of hydrogen bond
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Help maintain the structure of protein molecules, which are essential functional molecules and body building materials
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Ionic bond formation
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when electrons completely transfer from one atom to another
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Ions
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Created when there is an imbalance of positive and negative charge in the atom
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Anions
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Negatively charged ions
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Cation
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Positively charged ions
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Salts
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NaCl and most other compounds formed by ionic bonding
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Covalent molecules
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Molecules in which atoms share electrons
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Nonpolar covalently bonded molecules
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Covalent molecules whose electrons have been shared equally between the atoms
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Polar molecules
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Contain electrically unbalanced atoms
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Importance of salts
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Nerve transmission, muscle contraction, blood clotting, transport of oxygen by hemoglobin, metabolism
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Electrolytes
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Substances that conduct an electrical current in solution. All salts are electrolytes
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2/3 of body weight
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Water
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Acid
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A substance that can release hydrogen ions in detectable amounts; have a sour taste
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Proton donors
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Acid
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Four vital properties of water
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1- high heat capacity 2-polarity/solvent properties 3-chemical reactivity 4-cushioning
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Proton acceptors
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Base
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Bases
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Bitter taste; feel slippery
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pH
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Relative acid-base concentration of hydrogen ions in body fluid
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Normal body pH
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7.35 to 7.45
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Carbohydrates
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Contain carbon, hydrogen and oxygen; sugars and starches
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Building blocks of carbohydrates
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Monosaccharides (glucose), disaccharides (lactose), polysaccharides (starch, glycogen)
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Inorganic compound
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Make up living things; do not contain carbon; Include: salts, water, some acids and bases
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Most abundant compound in the body
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Water
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Organic compound
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Carbon-containing compound that comprise living matter
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Lipids
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Triglycerides, phospholipids and steroids
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Importance of lipids
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Form the basis of certain hormines, bile salts and vitamin D
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Constructed from amino acids
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Protein
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Fibrous proteins
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Basic structural materials of the body
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Globular proteins
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functional proteins, including hemoglobin, some hormones and enzymes
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Enzymes
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Functional proteins that act as biological catalysts
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Two nucleic acids
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deoxyribonucleic acid (DNA) and ribonucleic acid (RNA)
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Maintains heritage by replicating itself before cell division
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DNA
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Acts in protein synthesis to ensure that DNA instructions are executed
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RNA
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Importance of ATP
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Provides cellular energy
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-saccharide
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sugar
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