Anatomy Unit 1: Inorganic Chemistry – Flashcards
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matter
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anything that occupies space and has mass
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composition of matter
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elements, atoms, molecule, compounds, formulas, chemical reactions
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elements
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fundamental units of matter. 92 occur naturally. living organisms require about 20 elements. 96% of the body is made from four elements- carbon, oxygen, hydrogen, nitrogen
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atoms
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building blocks of elements. BLANK of different elements vary in size and in how they interact.
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nucleus
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contain protons and neutrons, are about the same size and mass
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outside of nucleus
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contain electrons, have a much smaller mass and size than protons and neutrons
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neutral atoms
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have the same number of protons and neutrons
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atomic number
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the number of protons that the atoms contain
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atomic mass
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sum of the protons and neutrons
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molecule
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two or more atoms combined chemically
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compound
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two or more different atoms combined chemically. they always have a definite kind and numbers of atoms
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formulas
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two types: molecular and structural
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molecular formula
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represents the numbers and types of atoms in a molecule
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structural formula
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various representations can be used to illustrate molecules
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chemical reactions
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chemical bonds; electron shells; bonding; valence shells; ionic bonds; covalent bonds; hydrogen bonds; a BLANK occurs as bonds are formed or broken between atoms, ions, or molecules; those changed by the reaction are the REACTANTS; those formed are the PRODUCTS; REVERSIBLE REACTIONS are symbolized by using two arrows; CATALYSTS (enzymes in the body) influence the rates of reactions
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chemical bonds
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atoms are untied by BLANK by gaining, losing, or sharing electrons
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electron shells
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electons occupy energy levels called BLANK
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bonding
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involves interactions between electrons in the outer (valence) shell
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valence shells
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if BLANK are not full, they are unstable; the first energy shell holds 2 electrons, the other energy shells each hold 8 electrons when on the outside; tend to gain, lose, or share electrons; allows for bond formation, which produces stable BLANK
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ionic bonds
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form when electrons are completely transferred from one atom to another; contain ions
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ions
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charged particles formed when atoms gain or lose electrons
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covalent bonds
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atoms become stable through shared electrons; single BLANK share two electrons, double bonds share four electrons; have covalent molecules; some are non-polar and some are polar
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non-polar
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electrically neutral as a molecule
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polar
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have a positive and negative side
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hydrogen bonds
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hydrogen is attracted to negative portion of a polar molecule; weak chemical bonds; (provide attraction between molecules); between molecules of water, holds molecules of protein and DNA in their shapes
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synthesis reactions
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(A+B->AB); atoms or molecules combine; energy is absorbed for bond infomation, anabolic reaction
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anabolic reaction
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energy is absorbed for bond; ex: amino acids bond to form proteins
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decomposition reaction
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(AB->A+B); molecule is broken down; chemical energy is released, catabolic reaction
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catabolic reaction
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chemical energy is released; ex: ATP loses phosphate, releasing energy
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exchange reaction
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(AB+C->AC+B); involves both synthesis and decomposition reactions; switch is made between molecule parts and different molecules are made; ex: glucose 6 phospate gives up a phosphate to ADP to make ATP
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exchange reaction
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(AB+C->AC+B); involves both synthesis and decomposition reactions; switch is made between molecule parts and different molecules are made; ex: glucose 6 phospate gives up a phosphate to ADP to make ATP
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inorganic compounds
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tend to be simpler; lack carbon and hydrogen; ex: water, salts, some acids and bases, oxygen, carbon dioxide
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inorganic compounds
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tend to be simpler; lack carbon and hydrogen; ex: water, salts, some acids and bases, oxygen, carbon dioxide
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water
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most abundant compound in body (about 2/3 of the weight of adults) HIGH HEAT CAPACITY- does not change temperature easily; chemical reactivity; dehydration synthesis; hydrolysis; pH of 7=neutral; good solvent; cushion
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water
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most abundant compound in body (about 2/3 of the weight of adults) HIGH HEAT CAPACITY- does not change temperature easily; chemical reactivity; dehydration synthesis; hydrolysis; pH of 7=neutral; good solvent; cushion
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chemical reactivity
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serves as a base for reactions
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chemical reactivity
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serves as a base for reactions
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dehydration synthesis
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water is removed from adjacent atoms (H+ from one and OH- from another) to form a bond
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dehydration synthesis
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water is removed from adjacent atoms (H+ from one and OH- from another) to form a bond
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hydrolysis
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water is used to break bonds between molecules (H+ added to one and OH- added to another)
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hydrolysis
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water is used to break bonds between molecules (H+ added to one and OH- added to another)
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good solvent
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dissolves polar substances easily
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good solvent
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dissolves polar substances easily
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cushion
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mucus, internal organs, joints
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cushion
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mucus, internal organs, joints
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salts
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ionic compounds (metal with a nonmetal or an anion); easily break up into ions in the presence of water (dissociate); vital to many body functions; include electrolytes; ex: NaCl = sodium chloride and calcium phosphate
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salts
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ionic compounds (metal with a nonmetal or an anion); easily break up into ions in the presence of water (dissociate); vital to many body functions; include electrolytes; ex: NaCl = sodium chloride and calcium phosphate
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electrolytes
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conduct electrical currents
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electrolytes
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conduct electrical currents
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acids
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can release detectable hydrogen ions (H+); low pH (below 7); taste sour; ex: common- lemon juice, coffee, carbonic acid in soda; in body- gastric juice, uric acid, vitamin C, amino acids, nucleic acids, lactic acid, fatty acids, vaginal fluid
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acids
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can release detectable hydrogen ions (H+); low pH (below 7); taste sour; ex: common- lemon juice, coffee, carbonic acid in soda; in body- gastric juice, uric acid, vitamin C, amino acids, nucleic acids, lactic acid, fatty acids, vaginal fluid
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bases
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proton (H+) acceptors (most have hydroxide ions- OH-); high pH (above 7); taste bitter; slippery; ex: common- tums, baking soda, egg whites, sea water, draino, bleach, oven cleaner; in body- blood and semen
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bases
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proton (H+) acceptors (most have hydroxide ions- OH-); high pH (above 7); taste bitter; slippery; ex: common- tums, baking soda, egg whites, sea water, draino, bleach, oven cleaner; in body- blood and semen
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oxygen
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needed to release energy from nutrients and is used to drive the cells's metabolism; gas that is transported in the blood; it is taken in by inhaling
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oxygen
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needed to release energy from nutrients and is used to drive the cells's metabolism; gas that is transported in the blood; it is taken in by inhaling
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carbon dioxide
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released as a waste product during cellular respiration; removed by exhaling; cellular respiraction- glucose + oxygen -> water + carbon dioxide
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carbon dioxide
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released as a waste product during cellular respiration; removed by exhaling; cellular respiraction- glucose + oxygen -> water + carbon dioxide
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pH balance
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BLANK in the body is critical to physiology; measures relative concentration of hydrogen ions in solution; pH 7 = neutral, equal H+ and OH- ions; can be acidic, basic, or neutral
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pH balance
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BLANK in the body is critical to physiology; measures relative concentration of hydrogen ions in solution; pH 7 = neutral, equal H+ and OH- ions; can be acidic, basic, or neutral
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acidic
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pH 0-7
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acidic
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pH 0-7
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basic
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pH 7-14
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basic
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pH 7-14
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tenfold difference
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between each whole number on the pH scale, there is a BLANK in the H+ concentration
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tenfold difference
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between each whole number on the pH scale, there is a BLANK in the H+ concentration
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blood's normal pH
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between 7.35 and 7.45; when it drops below 7.0 or rises above 7.8 it is lethal
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blood's normal pH
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between 7.35 and 7.45; when it drops below 7.0 or rises above 7.8 it is lethal
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acidosis
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when it drops below 7.35
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acidosis
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when it drops below 7.35
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alkadosis
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when it drops below 7.45
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alkadosis
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when it drops below 7.45
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buffers
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compounds that minimize changes in pH; may be weak acids that donate H+ when pH rises or accepts H+ when pH drops; ex: carbonic acid- in water dissociates into bicarbonate and hydrogen ions
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buffers
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compounds that minimize changes in pH; may be weak acids that donate H+ when pH rises or accepts H+ when pH drops; ex: carbonic acid- in water dissociates into bicarbonate and hydrogen ions
