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Stack #89249
Chemistry/Microbiology: Organic Chemistry Notes
| Question | Answer |
|---|---|
| 4 examples of inorganic acids | HCl, HNO3,H2SO4, H3PO4 |
| HCl is | Hydrochloric acid, cleans metals and cleans cement |
| HNO3 is | Nitric Acid: fertilizers, dyes, plastics, will turn skin yellow |
| H2SO4 os | Sulferic acid: fertilizers, gunpowder, auto bateries, burns skin |
| H3PO4 | phosphoric acid: flavoring agent in soda, fertilizers |
| An example of an Organic acid | CH3COOH: acetic acid, found in vinegar |
| CH3COOH is | Acetic acid: an organic acid, found in vinegar |
| 4 examples of bases | NaOH, Ca(OH)2,NH3, Mg(OH)2 |
| NaOH is | sodium hydroxide: lye, drain cleaners, caustic soap and celephane |
| Ca(OH)2 is | calcium hydroxide: used to manufacture cement |
| NH3 is: | ammonia: used in smelling salts and household cleaners |
| Mg(OH)2 is: | magnesium hydroxide: laxatives, antacids, milk of magnesia |
| 7 examples of salts | Ca3(PO4)2:calcium phosphate; Fe, Na, K, NaI: sodium iodide; Mg, and F |
| Ca(PO4)2 is: | a salt= calcium phosphate |
| NaI (capitol eye) is: | salt: sodium iodide |
| F is: | salt: fluorine salts |
| What can break covalent bonds? | Heat, electricity |
| In H2O, there are how many covalent bonds? | 2 |
| Form the compound: Ca(+2) and Cl(-1) | CaCl2 |
| Form the compound: Al(+3) and Cl (-1) | AlCl3 |
| 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 |
| Group 1A when they become ions they have a:_____ charge | +1 charge |
| Group 2A ions have a ____charge | +2 charge |
| Group 8A do not react, why? | they have full 8 electrons |
| GroupS 1A thru 3A _______electrons | loses |
| Group 6A GAIN ____electrons | 2; they have a -2 charge |
| Group 7A GAIN ___electron(s) | 1: they have a -1 charge |
| Groups 4A and 5A can ______or ________electrons | gain or lose: depending on what they combine with. |
| In a compound, is the positive or negative ion is written first? | Positive |
| 2 examples of writing the positive ions first in compound formation | Li(+1) and Cl (-1)= LiCl: Mg(+2) and Cl (-1) = MgCl2 |
| These three polyatomic groups have charges | Nitrate group, Sulfate Group, Phosphate Group |
| Nitrate Group | NO3- |
| The most common compound that shows up in the Nitrate group | HNO3 Nitric Acid does not have a charge |
| HNO3 | Nitric Acid formed by H+No3- |
| SO4(-2) | Sulfate Group |
| H2SO4 in the Sulfate Group is: | Sulferic acid |
| H3PO4 in the phosphate group is: | Phosphoric Acid |
| SO4(-2) is what group? | Sulfate Group |
| PO4(-3) is what group? | Phosphate Group |
| NO3(-) is what group? | Nitrate Group |
| Acids are bitter or sour? | sour |
| Bases are sour or bitter | bitter=base |
| What color does Litmus turns what color to indicate acids? | Red |
| Litmus turns what color to indicate bases? | blue = base |
| Acids and bases will react with each other and their products will always be a kind of: | Salt and H2O |
| Acid is a substance that releases _______in H2O? | Hydrogen ions |
| HCl put in H2O : | H(+) + Cl(-) |
| Scientist who first defined Base | Arrhenius |
| Scientist known for definition of acids | Bronstad |
| Base definition | A substance that releases OH(-) groups in H2O |
| NaOH put in H2O | Na(+) + OH(-) |
| Common name sometimes known for HCl | Muriatic acid |
| Formula for calculating pH | pH= -log[H+] |
| if it is in brackets [ ] it is: | [molar concentration] |
| Log of __ to exponent is equal to exponent | 10 |
| 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 |
| example of typical strong base | NaOH in water: Na(+) + OH(-) |
| Remember in determining concentration: | .01 = 10(-2) |
| A mixture is: | A combination of two or more substances that can be separated by PHYSICAL means |
| Name two types of mixtures | Heterogeneous and Homogeneous |
| Which type of mixture is a solution? | Homogeneous |
| Homogeneous mixture means | every part has the same properties |
| Salt water is an example of this kind of solution | Homogeneous |
| Heterogeneous mixture means: | different parts have different properties |
| Solution made from dissolving a solid in water is called | Aquaeous solution |
| SOLUTE | Substance which is dissolved ; ie. salt |
| SOLVENT | substance that does the dissolving (ie. H2O) |
| Liquid into liquid rule | the liquid in the greater amount is the solvent, the lesser is solute |
| CONCENTRATION | the ratio of solute to solvent |
| 3 ways to express the percentage of concentration | weight, volume, and weight/volume |
| SATURATED SOLUTION | A solvent that cannot hold anymore solute: won't dissolve further |
| Example of a strong acid | HCl |
| pH formula for solving for [OH-] | [OH-] = 10(-14)M divided by [H+] |
| Formula to solve pH for finding [H+] | [H+] = 10(-14)M divided by [OH-] |
| Group 1A is called: | Alkali metals or alkali elements |
| These elements produce a BASIC SOLUTION when added to H2O | Alkali metals or called alkali elements |
| The elements farthest to the right on the Periodic Table are the most: | Nonmetal |
| Column 8A on the Periodic Table are also known as: | Inert Elements/Noble gases; they do not react |
| Group 7A are | Halogens |
| Halogens refers to these elements | Salts |
| Group 2A on the Periodic table are | Alkalines |
| This group of elements are found in the earth's surface | Alkalines |
| These elements added into h2O produce what? | BASIC SOLUTIONS |
| MOLE FOR A COMPOUND = | molecular weight |
| MOLE OF AN ELEMENT = | ATOMIC WEIGHT |
| 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% |
| To calculate percentage of concentration by volume | %by Vol= vol of solute/total vol of solution X 100 ie. 62mL/210mL X100=29.5% |
| 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 |
| Calculate Molarity | Molarity=moles of solute/L of solution |
| Calculate the mole of compound for Molarity | NaCl= Na (23) + Cl (35) = 58g, 58g is 1 Mole of NaCl |
| Gas Laws: 2 predominant | Charle's Law and Boyle's Law |
| 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 |
| Charles's Law formula | Vi/Vf =Ti/Tf |
| Boyle's law means: | The volume of a gas at constant TEMPERATURE is indirectly po\roportional to its pressure. |
| Vi/Vf+ Pf/Pi | Boyle's Law: temperature remains constant |
| This acid breaks up completely into component ions | Strong acid |
| This acid does not break up completely into component ions. It is: | Weak |
| Give an example of a heterogeneous mixture | sand in water |
| the pH scale is a _______scale | logrythmic scale |
| on the pH scale 1-6.9 is | Acidic |
| On the pH scale, 7 is | Neutral |
| 7.1-14 on the pH scale is: | basic |
| Acidic on the pH scale has more or less H? | More |
| Substances made with elements that are present in a fixed proportion by mass and cannot be changed | Compounds |
| This basic building block of all substances cannot be boken down with a chemical reaction | Elements |
| ______have a varying composition and can be separated back to its components by PHYSICAL means | Mixtures |
| Physcially _____can be broken down into smaller substances or particles called ____but the properties do not change | Elements, Atoms |
| The ____is found under the symbol of an element, it is never a whole number | Atomic weight |
| Protons plus the number of neutrons = | atomic weight |
| O2 diatomic compounds | n2,H2,F2,Cl2,Br2,I(capital eye)2 |
| Gases behave to the rules of______even though they are in a different physical state | compounds |
| Predictive behavior of gases if temperature changes | + temp=molecules become more active, move faster , and occupy a greater volume |
| Predictive behavior of gases if pressure changes | + pressure = molecules bumping into each other; decrease volume by increasing pressure (Charles Law) |
| What is the Vf of a gas using Charles Law | Vf= Vi X Tf / Ti |
| Using Charles Law Vf= you must convert Celcius to | Kelvins |
| 50 degrees celcius is how many Kelvins? | 273+50= 323 degrees K |
| Boyle's Law: Temperature remains: | Constant; volume and pressure |
| Boyle's law using the fact that pressure has increased will cause and ________in volume | Increase |
| Solve for Pf using Boyle's Law | Pf=Vi x Pi / Vf |
| 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 |
| 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 |
| Liquid concept: | Evaporation: vapor phase little space above the water. |
| Dynamic Equalibrium | Molecules move from liquid to vapor to liquid and the rate of movement will become the same. |
| Equilibrium Vapor Pressure | Pressure exerted by vapor molecules; > temp = EVP increases |
| >EVP (higher) = | > Volatile, the more easily a liquid evaporates, it is more volatile. |
| two examples of less volatile liquids | motor oil, glycerine, because the lower the EVP, the harder it is to evaporate |
| The Vapor Point of a liquid VP = | atmp |
| atmP is like a giant weight pressing down on | molecules and keeping them down |
| Sublimation | Solid to a gas stage directly i.e. dry ice |
| 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. |
Created by:
tamiboren
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