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Ch 10 Test Hints – Chemistry Chemical Quantities

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1)Define mole Were talking representative particles here. That could mean people, pickles, atoms, ions, molecules, etc. (Psssst….You should KNOW how many that is without us having to say so) Were talking representative particles here. That could mean people, pickles, atoms, ions, molecules, etc. (Psssst….You should KNOW how many that is without us having to say so)

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2) How to determine/calculate the number of atoms of an element in a given number of molecules of a compound So say we have 3 molecules of caffeine, C 8 H 10 N 4 O 2 in our coffee cup. (as if 3 molecules would be enough when were studying for a chemistry test!) Now, how many hydrogen atoms would we have in there? Hmmmm…. Each molecule of caffeine has 10 whole hydrogen atoms in it, so thats, C 8 H 10 N 4 O 2 plus, C 8 H 10 N 4 O 2 plus, C 8 H 10 N 4 O 2. Altogether that would be…? So say we have 3 molecules of caffeine, C 8 H 10 N 4 O 2 in our coffee cup. (as if 3 molecules would be enough when were studying for a chemistry test!) Now, how many hydrogen atoms would we have in there? Hmmmm…. Each molecule of caffeine has 10 whole hydrogen atoms in it, so thats, C 8 H 10 N 4 O 2 plus, C 8 H 10 N 4 O 2 plus, C 8 H 10 N 4 O 2. Altogether that would be…?

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3) The various quantities that Avogadros number represents. Check back to hint #1 and the examples of what a moles-worth of particles stands for. The key to this question is knowing the correct chemical formulas for atoms, molecules (even the diatomic ones), formula units, and ions. So, Avogadros number is the same for Na, Na +, NaCl, and Cl 2 (to name a few) [And youd still better know exactly what that number is!!] Check back to hint #1 and the examples of what a moles-worth of particles stands for. The key to this question is knowing the correct chemical formulas for atoms, molecules (even the diatomic ones), formula units, and ions. So, Avogadros number is the same for Na, Na +, NaCl, and Cl 2 (to name a few) [And youd still better know exactly what that number is!!]

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4) How to convert atoms of an element to moles of an element using Avogadros number. If we said you have 4.3 x 10 21 atoms of gold, nope, make that platinum. Would you be rich? How many moles is that? Look closely at the exponent. Is this quantity more than 1 moles-worth or less than 1 moles-worth? Once you figure that out, you will know if you need to multiply or divide by Avogadros number. [seriously! You need to know what that number is.] Remember, that a MOLE is a group that is a certain size. If we said you have 4.3 x 10 21 atoms of gold, nope, make that platinum. Would you be rich? How many moles is that? Look closely at the exponent. Is this quantity more than 1 moles-worth or less than 1 moles-worth? Once you figure that out, you will know if you need to multiply or divide by Avogadros number. [seriously! You need to know what that number is.] Remember, that a MOLE is a group that is a certain size.

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5) How to convert moles of an element to atoms of an element using Avogadros number This is just the opposite of number 4. If you have 1.50 moles (groups) of platinum, how many atoms is that? Mathematically, you do the opposite process compared to what you did in number 4. Think about it. This is more than one group, so it must be bigger than Avogadros number! This is just the opposite of number 4. If you have 1.50 moles (groups) of platinum, how many atoms is that? Mathematically, you do the opposite process compared to what you did in number 4. Think about it. This is more than one group, so it must be bigger than Avogadros number!

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6) How the atomic masses of 2 different elements are related The atomic masses of elements have something in common. They represent the same number of particles ! So, if you have 1.00797 g Hydrogen or 15.9994 g Oxygen or 140.9077 g of Praseodymium (just cuz that ones fun to say), they all have exactly _. _ _ _ x _ _ _ _ atoms. Yea! The atomic masses of elements have something in common. They represent the same number of particles ! So, if you have 1.00797 g Hydrogen or 15.9994 g Oxygen or 140.9077 g of Praseodymium (just cuz that ones fun to say), they all have exactly _. _ _ _ x _ _ _ _ atoms. Yea!

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7) How to calculate the molar mass of a diatomic (halogen) gas I know! I know! How about Fluorine gas? F 2 This is actually a molecule like H 2 O is a molecule. So, you have to add up the atomic masses of both fluorine atoms to get the molar mass! Simple. I know! I know! How about Fluorine gas? F 2 This is actually a molecule like H 2 O is a molecule. So, you have to add up the atomic masses of both fluorine atoms to get the molar mass! Simple.

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8) Define molar mass. Uh… the name says it all.

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9) How to calculate the molar mass of a given compound Well, weve practiced this a bazillion times in class, in labs, on homework. All you have to do is add up the atomic masses of the elements shown in the formula. Well, weve practiced this a bazillion times in class, in labs, on homework. All you have to do is add up the atomic masses of the elements shown in the formula.

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10) How to convert moles of a given compound to mass – molar mass will be given If 1.00 mole of water has a mass of 18.01534 g (You know how we got that. We used it in all the hydrate labs.), then how much would 2.00 moles of water be (by mass that is)? Just double it, right? As in multiply by 2.00. So what if the question actually has some weird number in it with decimals, like 4.56 moles or something? The math is the same. If 1.00 mole of water has a mass of 18.01534 g (You know how we got that. We used it in all the hydrate labs.), then how much would 2.00 moles of water be (by mass that is)? Just double it, right? As in multiply by 2.00. So what if the question actually has some weird number in it with decimals, like 4.56 moles or something? The math is the same.

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11) How to convert mass of a given compound to moles – molar mass will be given This one is just the opposite of number 10. You should be able to set up a factor-label problem. Some of you seemed to find using ratios easier, so go ahead and do that. The math is the same either way. If you are confused on how to start this problem, remember that one whole moles-worth of a compound is represented by the molar mass. If you are given a mass of something like 5.00 g H 2 O and a whole mole of water has a mass of 18.01534 g, you can see that the 5.00g is LESS than the mass of one mole. What mathematical operation is that then? This one is just the opposite of number 10. You should be able to set up a factor-label problem. Some of you seemed to find using ratios easier, so go ahead and do that. The math is the same either way. If you are confused on how to start this problem, remember that one whole moles-worth of a compound is represented by the molar mass. If you are given a mass of something like 5.00 g H 2 O and a whole mole of water has a mass of 18.01534 g, you can see that the 5.00g is LESS than the mass of one mole. What mathematical operation is that then?

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12) How to calculate the mass of a specific element in a given compound (% composition) – molar mass will be given. Ok. Now were talkin. This is a problem like #5 on the percent composition worksheet. Look back at the answers that you wrote down when we went over this in class. [Didnt do that? Then take a look at the practice problem on page 307 to get you started. Hey, the online textbook even has a Checkpoint problem that you can try!] Say you are asked to find the mass of Na in 7.80 g of NaCl. First, you have to find the % Na in NaCl and then take that percent of 7.80 g PS. If you get an answer over 300 g, you forgot to move the decimal. Ok. Now were talkin. This is a problem like #5 on the percent composition worksheet. Look back at the answers that you wrote down when we went over this in class. [Didnt do that? Then take a look at the practice problem on page 307 to get you started. Hey, the online textbook even has a Checkpoint problem that you can try!] Say you are asked to find the mass of Na in 7.80 g of NaCl. First, you have to find the % Na in NaCl and then take that percent of 7.80 g PS. If you get an answer over 300 g, you forgot to move the decimal.

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13) What information in general is needed to calculate the % composition of a compound. If we asked you to find the % composition of water, we mean find the % H and the % O. The whole % composition worksheet was about this. Can you describe how to calculate this? If we asked you to find the % composition of water, we mean find the % H and the % O. The whole % composition worksheet was about this. Can you describe how to calculate this?

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14) How to calculate the % composition of a binary compound when given the masses of each element. In this problem you will be given actual masses of elements. See page 306 #32 & 33 for examples. There is a sample problem in box 10.9. You will need to find the total mass of the compound first and then do a basic % of element example. Calculate the % of N. In this problem you will be given actual masses of elements. See page 306 #32 & 33 for examples. There is a sample problem in box 10.9. You will need to find the total mass of the compound first and then do a basic % of element example. Calculate the % of N. 9.03 g Mg 3.48 g N

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15) How to calculate the % of a given element in a specific compound – molar mass will be given. See your percent composition worksheet again. Example 10.10 on page 307. Something like what is the % N in NH 4 NO 3 See your percent composition worksheet again. Example 10.10 on page 307. Something like what is the % N in NH 4 NO 3

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16) How to set up the correct equation for finding % composition of an element. If you can calculate the % of an element like in #15, this one will be super easy. All you have to do is identify which problem is set up correctly. See, this is why we make you show your work all the time! If you can calculate the % of an element like in #15, this one will be super easy. All you have to do is identify which problem is set up correctly. See, this is why we make you show your work all the time!

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17) Define empirical formula. Hey, look in your glossary, or the notes, or on page 309 in your book. Its even on the online textbook. You know this! Weve asked you about it 100,000 times. [Oh, another way to say it is simplest formula] Hey, look in your glossary, or the notes, or on page 309 in your book. Its even on the online textbook. You know this! Weve asked you about it 100,000 times. [Oh, another way to say it is simplest formula]

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18) How to identify the molecular formula in a set of mostly empirical formulas. Check Table 10.3 on page 311. Mr. Sustin says its wonderful! Is the formula all nonmetals? Can the subscripts be reduced? If so, its a molecular formula and not an empirical formula. Hey, Ill bet there are podcasts posted on Mrs. Gregorys Moodle page that you ALL have access to. Practice problem #39 on page 312 rocks! Check Table 10.3 on page 311. Mr. Sustin says its wonderful! Is the formula all nonmetals? Can the subscripts be reduced? If so, its a molecular formula and not an empirical formula. Hey, Ill bet there are podcasts posted on Mrs. Gregorys Moodle page that you ALL have access to. Practice problem #39 on page 312 rocks!

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19) How to calculate the empirical formula of a compound when given the mass % of each element. Well now, this is the type of problem that involves the most math. On page 310, example problem 10.11 and two practice problems show you EXACTLY how to do this. Hey, the whole page is devoted to just this type of problem. In your notes, there is exactly the same type of example for Acetic Acid. Assume 100g sample – convert to moles – do a mole ratio. Well now, this is the type of problem that involves the most math. On page 310, example problem 10.11 and two practice problems show you EXACTLY how to do this. Hey, the whole page is devoted to just this type of problem. In your notes, there is exactly the same type of example for Acetic Acid. Assume 100g sample – convert to moles – do a mole ratio.

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20) How to distinguish between empirical and molecular formulas in general –basic characteristics/definitions of each. This is one of those Which of the following is NOT… questions. Make sure you really, really know the definitions of empirical formula and molecular formula. You have GOT to read all of the answer choices – twice, at least. How many times have you said to us during test corrections that you just misread the question? Well, dont do that. This is one of those Which of the following is NOT… questions. Make sure you really, really know the definitions of empirical formula and molecular formula. You have GOT to read all of the answer choices – twice, at least. How many times have you said to us during test corrections that you just misread the question? Well, dont do that.

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21) How to calculate the number of molecules in a given mass of a compound – molar mass will be given. You will be given a mass like 5.67 g H 2 O and then you need to figure out how many particles. So GO TO MOLES! Use the mole map that is on page 303, figure 10.12, and then convert to particles. Yes, you actually get to use Avogadros Number this time. You will be given a mass like 5.67 g H 2 O and then you need to figure out how many particles. So GO TO MOLES! Use the mole map that is on page 303, figure 10.12, and then convert to particles. Yes, you actually get to use Avogadros Number this time. KNOW THIS CHART! (x Avogadros #) (x Molar Mass) # of particles Mole Mass in grams

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22) How to calculate the % by mass of an element in a given compound – molar mass will be given. This is just like #15, but it is a short answer problem. You did a bunch of these on the % composition worksheet. Yea! This is just like #15, but it is a short answer problem. You did a bunch of these on the % composition worksheet. Yea!

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23) How to calculate the molecular formula of a compound when given the empirical formulas and molecular masses of each. If the empirical formula is HO and the molecular mass is 34 g/mole, what is the molecular formula? Well, add up the mass of H & O (1 + 16 as a quick example) = 17 17 is not 34 because 34 is twice as big. So just double the subscripts to get the molecular formula H 2 O 2. Yep, its that easy. If the empirical formula is HO and the molecular mass is 34 g/mole, what is the molecular formula? Well, add up the mass of H & O (1 + 16 as a quick example) = 17 17 is not 34 because 34 is twice as big. So just double the subscripts to get the molecular formula H 2 O 2. Yep, its that easy.

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24) How to calculate the number of moles of water in a hydrated compound when given the mass data (like the BaCl 2 lab and the MgSO 4 lab). This is a problem just like the hydrate labs. You will be given data for mass of the crucible, mass of crucible with chemical before heating and mass of crucible with chemical after heating. You need to know how to calculate the mass of water lost and the mass of the anhydrous (dry) chemical. Then, convert both of those to moles and do a mole ratio. You are filling in the question mark in a formula like MgSO 4 ? H 2 O Mrs. Gregory has a sample problem in her notes if you need that. This is a problem just like the hydrate labs. You will be given data for mass of the crucible, mass of crucible with chemical before heating and mass of crucible with chemical after heating. You need to know how to calculate the mass of water lost and the mass of the anhydrous (dry) chemical. Then, convert both of those to moles and do a mole ratio. You are filling in the question mark in a formula like MgSO 4 ? H 2 O Mrs. Gregory has a sample problem in her notes if you need that.

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25) How to calculate the empirical AND molecular formulas when given the mass percentages of each element and the molecular mass of the compound. This problem brings it all home. You will be given the %s of each element in a molecular compound. So, you need to convert each % to mass by assuming a 100.0 g sample. Change each mass to moles using molar mass. Calculate the mole ratio between the elements – always divide by the smallest number of moles so you get a whole number ratio. But! There is one more step. Once you get the mole ration, which is the subscripts for the empirical formula, you have to add up the molar mass. If that mass matches what is given as the molar mass, then the empirical formula = molecular formula. Chances are though that the molecular formula will be some multiple of the empirical (e.g. double, triple, etc.) so increase the subscripts by that much. 50.7% C, 4.2% H and 45.1% O with a molar mass of 110.0 g = ?? This problem brings it all home. You will be given the %s of each element in a molecular compound. So, you need to convert each % to mass by assuming a 100.0 g sample. Change each mass to moles using molar mass. Calculate the mole ratio between the elements – always divide by the smallest number of moles so you get a whole number ratio. But! There is one more step. Once you get the mole ration, which is the subscripts for the empirical formula, you have to add up the molar mass. If that mass matches what is given as the molar mass, then the empirical formula = molecular formula. Chances are though that the molecular formula will be some multiple of the empirical (e.g. double, triple, etc.) so increase the subscripts by that much. 50.7% C, 4.2% H and 45.1% O with a molar mass of 110.0 g = ??

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