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22 Cards in this Set
- Front
- Back
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Define elements and know the 6 most common elements in the body and their relative proportions. |
Elements: • Building blocks of matter • simplest units of matter that have unique properties. • Subatomic particles such electrons all have the same properties regardless of what element they are from. * 6 most common elements in the body: 98.5% of body weight.
- Oxygen, carbon, hydrogen, nitrogen, calcium, and phosphorus. -----CCHONP
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Know the following about atoms:
A) Definition of an atom B) Location, Mass, and charge of protons, neutrons and electrons. C) Explain how atomic # and mass are calculated D) Define isotopes and explain their contributions to the reported atomic mass of an atoms. E) Explain how electron shells are filled F) Define the valence shell and know its significance for chemical reactions. G) Define ions, cations, and anionsn and explain process that forms them. |
A) atom: smallest units if matter that retain properties and characteristics of the element.
B) Location: building blocks of molecules Mass #: the total # of protons and neutrons in an atom. Charge of Protons/Electrons/Neutrons: •P= + •E= - (# of e= # of p) •N= NO ELECTRICAL CHARGE
C) Atomic #: #protons Atomic Mass: # protons + # neutrons
D) Isotopes: varieties of an element that differ from one another only in the # of neutrons and therefore in atomic mass.
----extra neutrons increase atomic mass (p+n) ----isotopes of an element are chemically similar •have same valence electrons
* Relative Atomic mass: • accounts for the average atomic masses of the isotopes. • atomic mass of hydrogen is 1.008 amu instead if 1 amu.
E) Electron shells: • Volume of space around the nucleus that electrons occupy. • Shells are filled from innermost to outermost shell.
*1st shell: max of 2 electrons 2nd shell: holds 8 3rd shell: can hold 18 - successive shells can hold larger and larger # of electrons. - Outermost shell is called "valence shell"
F) Valence Shell: all electrons in the valence shell are called valence electrons.
• Octet Rule: - Valence electrons participate in chemical reactions to bring the total # of valence electrons to 8. - Unless there is only 1 shell, then the reaction produces 2 electrons.
G) Ions: are atoms or groups with either a + charge or a - charge.
--ionization: is the transfer of electrons from one atom to another. This creates charged atoms called ions.
Cations: positively charged - donated electrons so that: # protons > # electrons.
* cat is positively donating electrons to gain more protons.
Anions: negatively charged - gained electrons so that: # electrons > # protons
* Ana is negatively gaining electrons to gain more electrons.
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Define minerals and electrolytes and know common examples of both. |
Minerals: inorganic elements extracted from soil by plants and passed up the food chain to humans. • Ca, P, Cl, Mg, K, Na, I, Fe, Zn, Cu, and S * constitute about 4% of body weight ----- Structure (teeth, bones, etc.) ----- enzymes Electrolytes: chemical that dissociates when added to water and can conduct an electrical current; includes salts, bases, and acids. * Nacl and KCl, HCl, |
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Know the following about molecules and compounds. A) Definition of molecules and compounds B) Know how to categorize the following into either group: water, carbon dioxide, oxygen gas, methane gas, nitrogen gas, sodium chloride, and ammonia C) Know how to write a molecular and structural formula. D) Know how to calculate molecular weight (and know unit) |
A) Molecules: combinations of 2 or more atoms held together by chemical bonds.
Compounds: molecules composed of 2 or more different elements: H_2O, CH_4 . ---- compounds are also molecules. B) Compound: water, Carbon dioxide, methane gas, nitrogen gas, sodium chloride, Ammonia. Molecule: Oxygen gas, C) Molecular formula: identify the type and quantity of each element present in the molecule. --------- H_2O , C_6H_12O_6 Structural formula: (can see bonds) shows the location of each atoms, used to differentiate between molecules with the same molecular formula ----> called isomers. D) Molecular weight: of a compound is the sum of atomic weights of the atoms. *calculate: MW of glucose (C_6 H_12 O_6) ---> 6 C atoms x 12 amu each = 72 amu 12 H atoms x 1 amu each = 12 amu + 6 O atoms x 16 amu each = 96 amu =================================== Molecular weight (MW) = 180 amu |
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Explain how molecules form ionic, covalent (single, double, polar, non-polar) and hydrogen bonds. |
Ionic Bonds (s3): the attraction of a cation to an anion. • electron donated by one and received by the other. • relatively weak attraction that is easily disrupted in water, as when salt dissolves. Covalent Bond: formed by sharing electrons. • single- sharing of single pair of electrons • double (- sharing of 2 pairs of electrons • non-polar (s1)- shared electrons spend approximately equal time around each nucleus. ------> strongest of all bonds • polar (s2)- if shared electrons spend more time orbiting one nucleus than they do the other, they lend their - charge to the area they spend most time. -----> molecule will have + and - end. • Hydrogen Bonds (s4)w: a weak attraction between a slightly + hydrogen atom in one molecule and a slightly - oxygen or nitrogen atom in another. --- relatively weak bonds --- very important physiology • protein structure • DNA structure |
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Characterize the following features about water: solvency, cohesion, adhesion, chemical reactivity, thermal stability. |
Solvency: ability to dissolve other chemicals • water is called the Universal Solvent -- Hydrophilic- substances that dissolve in water. > molecules must be polarized or charged. -- Hydrophobic- substances that don't don't dissolve in water. > molecules are non-polar or neutral (fat). Cohesion: tendency of like molecules to cling to each other by forming H-bonds.... which creates surface tension. • water is very cohesive due to its hydrogen bonds. • H-bonds create force called surface tension. Adhesion: tendency of one substance to cling to another. • water adheres to body tissue to form lubricating film on membranes (pleura and pericardium) • Reduces friction as lungs and heart contract and expand against membranes.
Chemical Reactivity: is the ability to participate in chemical reactions, • water ionizes into H+ and OH- • water ionizes other chemicals -- Eg NaCl ionizes in water to form Na+ and Cl- . • Water involved in hydrolysis and dehydration synthesis reactions. Thermal Stability: water helps stabilize the internal temperature of the body. • has high heat capacity --- hydrogen bonds inhibit movement of molecules which prevents increases in temperature. --- Allows water to absorb heat without changing temperature very much. • Effective coolant --- as water changes to vapor, a lot of heat is lost from the surface of the body. |
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Know the following about mixtures A) Definition of mixtures B) Definition of solutes and solvents C) Solutions, colloids, and suspensions i) Size of particle ii) Appearance and properties after standing iii) Examples in the body |
A) Mixture: consists of substances physically blended, but not chemically combined. B) Solutes: substances present in less amounts ---Ex: iced tea- make a homogenous mixture where the solvent is the more in the drink "iced tea powder," and the solute is the tea mixed.
Solvent: the substance present in largest amount. or dissolving medium. --- 1) water is the body's chief solvent. 2) usually a liquid; like water. C) Solutions: consists of particles of matter called the solute mixed with more abundant substance (usually water) called the solvent. • usually transparent (tiny particles) • sugar water, oil, water Suspension: are heterogeneous mixtures. • blood- solute particles are very large, settle out, and may scatter light. Colloids: Also called emulsions • Heterogeneous mixtures • are larger than in solutions, solute particles do not settle out, they scatter light.
i) size of particle 1> smallest ----- solutions 2> I ----- suspension 3> Largest ----- colloid ii) appearance an properties after standing ---
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Know the following about concentrations A) how to calculate percentage concentrations B) Definition of mole C) Value of avogadro's # and its relevance to the definition of mole. D) How to calculate molarity (M) of a mixture E) Know the pros/cons of using percentage or molarity to characterize a solution. F) Know how to calculate equivalent concentrations of electrolytes. |
A) solutions are described in terms of their con concentration. Concentration is a measure of how much solute is present in a given volume of solvent. Physiological effects are based on the # of solutes in a solution, and not on the weight of the solute. Therefore concentration is most useful when it tells you how many pieces of solutes are dissolved • m/m, m/v, v/v, B) Mole: amount of any compound that is equal to its molecular weight in grams.
- Eg: molecular weight of glucose is 180 amu • therefore, 180 grams of glucose equal to 1 mole of glucose. C) 1 mole of any substance contains 6.023 x 10^23 units if that substance ----- this # is called Avogadro's #.
• 1 mole = 6.023x10^23 D) Molarity (M) = moles solute (mol)/ Liters solution (L) E) solutions are described in terms of their con concentration. Concentration is a measure of how much solute is present in a given volume of solvent. Physiological effects are based on the # of solutes in a solution, and not on the weight of the solute. Therefore concentration is most useful when it tells you how many pieces of solutes are dissolved F) |
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Define acids and bases |
Acids: is a molecule that releases H+ ions (called a proton) in water.
Bases: is a molecule that accepts H+ ions. |
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Know how to calculate pH and define pH ranges and relative concentrations of H+ and OH- of acidic and basic solutions. |
* The acidity of a mixture is based on the concentration (molarity) of H+ present in the mixture. Acidity is measured using the pH scale - pH= -loog [H+] (negative log of the molar concentration of H+) • ex: - a solution has[H+]= 0.0000001 molar=10^-7M -log [H+] = -7 - pH= -log [H+]= 7 |
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Define buffers and explain how they work using the carbonic acid- bicarbonate system as an example. |
Buffers: our body uses buffers to resist changes in pH. -Slight pH disturbances can disrupt physiological functions and alter drug actions. - pH of blood ranges from 7.35 to 7.45 - Deviations from this range cause tremors, paralysis or even death. * Carbonic Acid-Bicarbonate System: chemical reaction that can go in either direction to resist changes in pH. |
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ch. 2 Define energy and differentiate between potential and kinetic energy. |
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Know the following about chemical reactions A) Know how to write a chemical equation and define reactants and products. B) Know general definitions of decomposition, synthesis and exchange reactions. C) Definition of reversible reactions D) Definition of "Law of Mass Actions" and its role in predicting the direction of reactions. E) Predict the effects of concentration of reactants, temperature of reaction and presence of catalyst on the rate if reaction. |
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Define metabolism and distinguish between catabolism and anabolism. |
jn>cnl. |
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Definereduction and oxidation reactions. |
KNJ/LDN |
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Know the structural formula of the followingfunction groups: amine, carboxyl, hydroxyl, methyl, and phosphate |
ascac |
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Characterize hydrolysis and dehydrationsynthesis and explain their roles in synthesis and break-down of macromolecules |
scdacd |
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Know the four major organic molecules in ourbody. |
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Know the following aspects of carbohydrates A) Define the atomic make-up of carbohydrates B) know the building blocks C) Know common examples of monosaccharides,disaccharides and polysaccharides. |
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Know the following aspects of lipids A) Give 5 categories of lipids in the body B) Know the molecular components of triglycerides. i) Distinguish between saturated and unsaturated fats. C) Know the structural make-up of phospholipids. ii) Define the hydrophilic and hydrophobic regionsof phospholipids. D) Know the precursor material of all steroids andgive examples of steroid hormones. iii) Define LDL and HDL know their significance forcardiovascular health. |
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Knowthe building blocks of proteins A) Give the structural groups of amino acids and identify the portion that makes them unique. B) Know the names and 3 letter abbreviations forthe 20 amino acids. C) Identify the essential and non-essential amino acids D) Define the four levels of protein structure i) explain chemical bonds that contribute to their structure. ii) Give common examples of secondary structure. |
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Know the following aspects of nucleic acid A) Give the structural components of nucleotides. B) Know the structural make-up ATP and explain its significance. C) Compare and Contrast the structure and makeup of DNA and RNA. |
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