Chemistry/Microbiology: Organic Chemistry Notes
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| 4 examples of inorganic acids | HCl, HNO3,H2SO4, H3PO4
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| HCl is | Hydrochloric acid, cleans metals and cleans cement
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| HNO3 is | Nitric Acid: fertilizers, dyes, plastics, will turn skin yellow
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| H2SO4 os | Sulferic acid: fertilizers, gunpowder, auto bateries, burns skin
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| H3PO4 | phosphoric acid: flavoring agent in soda, fertilizers
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| An example of an Organic acid | CH3COOH: acetic acid, found in vinegar
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| CH3COOH is | Acetic acid: an organic acid, found in vinegar
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| 4 examples of bases | NaOH, Ca(OH)2,NH3, Mg(OH)2
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| NaOH is | sodium hydroxide: lye, drain cleaners, caustic soap and celephane
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| Ca(OH)2 is | calcium hydroxide: used to manufacture cement
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| NH3 is: | ammonia: used in smelling salts and household cleaners
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| Mg(OH)2 is: | magnesium hydroxide: laxatives, antacids, milk of magnesia
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| 7 examples of salts | Ca3(PO4)2:calcium phosphate; Fe, Na, K, NaI: sodium iodide; Mg, and F
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| Ca(PO4)2 is: | a salt= calcium phosphate
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| NaI (capitol eye) is: | salt: sodium iodide
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| F is: | salt: fluorine salts
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| What can break covalent bonds? | Heat, electricity
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| In H2O, there are how many covalent bonds? | 2
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| Form the compound: Ca(+2) and Cl(-1) | CaCl2
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| Form the compound: Al(+3) and Cl (-1) | AlCl3
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| How do you form the compound when the charges do not cancel each other? i.e. Al(+3) and O(-2) | Find the lowest common multiple of the charges (6): to get a charge of 6 Aluminums X 2= 2Al(+3) and 3O(-2) together now form Al2O3
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| Group 1A when they become ions they have a:_____ charge | +1 charge
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| Group 2A ions have a ____charge | +2 charge
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| Group 8A do not react, why? | they have full 8 electrons
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| GroupS 1A thru 3A _______electrons | loses
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| Group 6A GAIN ____electrons | 2; they have a -2 charge
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| Group 7A GAIN ___electron(s) | 1: they have a -1 charge
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| Groups 4A and 5A can ______or ________electrons | gain or lose: depending on what they combine with.
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| In a compound, is the positive or negative ion is written first? | Positive
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| 2 examples of writing the positive ions first in compound formation | Li(+1) and Cl (-1)= LiCl: Mg(+2) and Cl (-1) = MgCl2
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| These three polyatomic groups have charges | Nitrate group, Sulfate Group, Phosphate Group
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| Nitrate Group | NO3-
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| The most common compound that shows up in the Nitrate group | HNO3 Nitric Acid does not have a charge
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| HNO3 | Nitric Acid formed by H+No3-
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| SO4(-2) | Sulfate Group
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| H2SO4 in the Sulfate Group is: | Sulferic acid
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| H3PO4 in the phosphate group is: | Phosphoric Acid
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| SO4(-2) is what group? | Sulfate Group
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| PO4(-3) is what group? | Phosphate Group
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| NO3(-) is what group? | Nitrate Group
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| Acids are bitter or sour? | sour
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| Bases are sour or bitter | bitter=base
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| What color does Litmus turns what color to indicate acids? | Red
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| Litmus turns what color to indicate bases? | blue = base
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| Acids and bases will react with each other and their products will always be a kind of: | Salt and H2O
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| Acid is a substance that releases _______in H2O? | Hydrogen ions
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| HCl put in H2O : | H(+) + Cl(-)
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| Scientist who first defined Base | Arrhenius
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| Scientist known for definition of acids | Bronstad
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| Base definition | A substance that releases OH(-) groups in H2O
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| NaOH put in H2O | Na(+) + OH(-)
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| Common name sometimes known for HCl | Muriatic acid
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| Formula for calculating pH | pH= -log[H+]
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| if it is in brackets [ ] it is: | [molar concentration]
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| Log of __ to exponent is equal to exponent | 10
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| Every unit on the pH scale is actually factor of | 10: i.e. difference of 5 and 7 on pH scale is 10x10=100, not 2 or 20
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| example of typical strong base | NaOH in water: Na(+) + OH(-)
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| Remember in determining concentration: | .01 = 10(-2)
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| A mixture is: | A combination of two or more substances that can be separated by PHYSICAL means
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| Name two types of mixtures | Heterogeneous and Homogeneous
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| Which type of mixture is a solution? | Homogeneous
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| Homogeneous mixture means | every part has the same properties
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| Salt water is an example of this kind of solution | Homogeneous
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| Heterogeneous mixture means: | different parts have different properties
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| Solution made from dissolving a solid in water is called | Aquaeous solution
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| SOLUTE | Substance which is dissolved ; ie. salt
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| SOLVENT | substance that does the dissolving (ie. H2O)
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| Liquid into liquid rule | the liquid in the greater amount is the solvent, the lesser is solute
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| CONCENTRATION | the ratio of solute to solvent
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| 3 ways to express the percentage of concentration | weight, volume, and weight/volume
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| SATURATED SOLUTION | A solvent that cannot hold anymore solute: won't dissolve further
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| Example of a strong acid | HCl
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| pH formula for solving for [OH-] | [OH-] = 10(-14)M divided by [H+]
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| Formula to solve pH for finding [H+] | [H+] = 10(-14)M divided by [OH-]
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| Group 1A is called: | Alkali metals or alkali elements
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| These elements produce a BASIC SOLUTION when added to H2O | Alkali metals or called alkali elements
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| The elements farthest to the right on the Periodic Table are the most: | Nonmetal
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| Column 8A on the Periodic Table are also known as: | Inert Elements/Noble gases; they do not react
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| Group 7A are | Halogens
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| Halogens refers to these elements | Salts
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| Group 2A on the Periodic table are | Alkalines
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| This group of elements are found in the earth's surface | Alkalines
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| These elements added into h2O produce what? | BASIC SOLUTIONS
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| MOLE FOR A COMPOUND = | molecular weight
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| MOLE OF AN ELEMENT = | ATOMIC WEIGHT
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| TO CALCULATE THE PERCENTAGE OF A CONCENTRATION BY WEIGHT | %by wt= massof solute divided by total mass of solution X 100 ie. 35g/100g = 35%
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| To calculate percentage of concentration by volume | %by Vol= vol of solute/total vol of solution X 100 ie. 62mL/210mL X100=29.5%
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| To calculate the % of a concentration by wt/vol | the units can be different: % by wt/vol=Mass of solute (g) / total vol of solution (ml) X 100 ie. 18g/75ml X 100= 24% by wt/volume
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| Calculate Molarity | Molarity=moles of solute/L of solution
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| Calculate the mole of compound for Molarity | NaCl= Na (23) + Cl (35) = 58g, 58g is 1 Mole of NaCl
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| Gas Laws: 2 predominant | Charle's Law and Boyle's Law
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| Charles's Law means: | Increase temp of a gas will cause the gas to occupy a greater volue. So the volume of a gas at a constant pressure is directly proportional to its Kelvin temperature
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| Charles's Law formula | Vi/Vf =Ti/Tf
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| Boyle's law means: | The volume of a gas at constant TEMPERATURE is indirectly po\roportional to its pressure.
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| Vi/Vf+ Pf/Pi | Boyle's Law: temperature remains constant
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| This acid breaks up completely into component ions | Strong acid
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| This acid does not break up completely into component ions. It is: | Weak
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| Give an example of a heterogeneous mixture | sand in water
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| the pH scale is a _______scale | logrythmic scale
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| on the pH scale 1-6.9 is | Acidic
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| On the pH scale, 7 is | Neutral
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| 7.1-14 on the pH scale is: | basic
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| Acidic on the pH scale has more or less H? | More
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| Substances made with elements that are present in a fixed proportion by mass and cannot be changed | Compounds
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| This basic building block of all substances cannot be boken down with a chemical reaction | Elements
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| ______have a varying composition and can be separated back to its components by PHYSICAL means | Mixtures
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| Physcially _____can be broken down into smaller substances or particles called ____but the properties do not change | Elements, Atoms
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| The ____is found under the symbol of an element, it is never a whole number | Atomic weight
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| Protons plus the number of neutrons = | atomic weight
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| O2 diatomic compounds | n2,H2,F2,Cl2,Br2,I(capital eye)2
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| Gases behave to the rules of______even though they are in a different physical state | compounds
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| Predictive behavior of gases if temperature changes | + temp=molecules become more active, move faster , and occupy a greater volume
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| Predictive behavior of gases if pressure changes | + pressure = molecules bumping into each other; decrease volume by increasing pressure (Charles Law)
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| What is the Vf of a gas using Charles Law | Vf= Vi X Tf / Ti
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| Using Charles Law Vf= you must convert Celcius to | Kelvins
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| 50 degrees celcius is how many Kelvins? | 273+50= 323 degrees K
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| Boyle's Law: Temperature remains: | Constant; volume and pressure
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| Boyle's law using the fact that pressure has increased will cause and ________in volume | Increase
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| Solve for Pf using Boyle's Law | Pf=Vi x Pi / Vf
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| Using Boyle's Law: An O2 cylinder of 5L (Vi) at 90atmp (Pi) has a final atmp of 1; what is the final volume | Vf=Vi X Pi / Pf = 5L X 90 atmp / 1 atmp = 450L
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| Using Boyle's Law: tipoff; change in pressure: if an O2 cylinder has 2.5L @ 5atmp, what is the pressure if the volume is changed to 10L? | Pf = Vi X Pi / Vf = 2.5 L X 5 atmp / 10L = 1.25 atmp
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| Liquid concept: | Evaporation: vapor phase little space above the water.
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| Dynamic Equalibrium | Molecules move from liquid to vapor to liquid and the rate of movement will become the same.
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| Equilibrium Vapor Pressure | Pressure exerted by vapor molecules; > temp = EVP increases
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| >EVP (higher) = | > Volatile, the more easily a liquid evaporates, it is more volatile.
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| two examples of less volatile liquids | motor oil, glycerine, because the lower the EVP, the harder it is to evaporate
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| The Vapor Point of a liquid VP = | atmp
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| atmP is like a giant weight pressing down on | molecules and keeping them down
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| Sublimation | Solid to a gas stage directly i.e. dry ice
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| Fractional Distillation | In a mixture of several liquids, upon heating it up, the one with lowest Boiling Pt will vaporize first, then th next lowest will vaporize, etc.
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