Fundamentals of Atomic and Molecular Mass: Moles and Conversion Factors in Chemistry PDF

View this QuickTake in the app Fundamentals of Atomic and Molecular Mass: Moles and Conversion Factors in Chemistry Modified: Jan 27, 2025 11:02 AM 1. Outline Outline: Under...

View this QuickTake in the app Fundamentals of Atomic and Molecular Mass: Moles and Conversion Factors in Chemistry Modified: Jan 27, 2025 11:02 AM 1. Outline Outline: Understanding Atomic and Molecular Mass, Moles, and Conversion Factors I. Introduction Overview of key topics covered in the lecture II. Market Demand and Element Abundance A. Current market demand for cobalt B. Elemental abundance in the human body 1. Oxygen 2. Carbon 3. Hydrogen 4. Nitrogen III. Atomic Mass vs. Formula Mass A. Definition of Atomic Mass 1. Average mass of isotopes B. Definition of Formula Mass 1. Sum of atomic masses in a compound 2. Examples: nitrogen dioxide and glucose IV. Molar Mass A. Definition of Molar Mass 1. Mass of one mole of a substance in grams B. Calculation examples 1. Water 2. Carbon dioxide V. Understanding Moles A. Definition of a Mole 1. Unit of measurement (6.022 x 10²³ particles) B. Relationship between moles, grams, and atoms VI. Conversion Factors A. Importance in chemistry 1. Changing units (grams to moles, moles to atoms) B. Problem-solving examples using conversion factors VII. Practical Calculations A. Step-by-step approach to calculations 1. Calculating number of atoms from moles 2. Calculating moles from grams B. Emphasis on planning calculations VIII. Examples and Practice Problems A. Worked examples 1. Calculating moles from grams 2. Calculating atoms from moles B. Encouragement for practice and verification of answers IX. Critical Thinking in Problem Solving A. Importance of logical thinking B. Strategies for checking answer reasonableness X. Final Thoughts A. Reinforcement of practice and understanding basic concepts B. Encouragement for methodical problem-solving and unit usage XI. Conclusion Summary of the lecture’s key points and encouragement for further practice and critical thinking in chemistry. 2. Study guide www.quicktakes.io Fundamentals of Atomic and Molecular Mass: Moles and Conversion Factors in Chemistry Page 1/9  View this QuickTake in the app Study Guide: Understanding Atomic and Molecular Mass, Moles, and Conversion Factors Lecture Summary This lecture focused on the fundamental concepts of atomic and molecular mass, the definition and significance of moles, and the application of conversion factors in chemistry. Key topics included the market demand for elements, the distinction between atomic mass and formula mass, the definition of molar mass, and practical calculations involving moles. The importance of critical thinking and methodical problem-solving was emphasized, along with the encouragement for students to practice calculations to enhance their understanding. Key Topics 1. Market Demand and Element Abundance Current market demand for cobalt and its pricing. Elemental abundance in the human body: oxygen, carbon, hydrogen, nitrogen. 2. Atomic Mass vs. Formula Mass Atomic Mass: Average mass of all isotopes of an element. Formula Mass: Sum of the atomic masses of all atoms in a compound (e.g., nitrogen dioxide, glucose). 3. Molar Mass Definition: Mass of one mole of a substance (grams). Example calculations: Molar mass of water (H₂O) and carbon dioxide (CO₂). 4. Understanding Moles Definition: A mole is a unit of measurement for quantity (6.022 x 10²³ particles). Relationship between moles, grams, and atoms. 5. Conversion Factors Importance of conversion factors in chemistry for unit changes (grams to moles, moles to atoms). Examples of using conversion factors in calculations. 6. Practical Calculations Step-by-step approach to calculating the number of atoms from moles and vice versa. Emphasis on organizing information and planning calculations. 7. Examples and Practice Problems Worked examples on calculating moles from grams and atoms from moles. Encouragement for practice and verification of answers. 8. Critical Thinking in Problem Solving Importance of logical thinking in problem-solving. Strategies for checking the reasonableness of answers. 9. Final Thoughts Reinforcement of the need for practice and understanding of basic chemistry concepts. Encouragement to approach problems methodically and use units as guides. Useful Equations www.quicktakes.io Fundamentals of Atomic and Molecular Mass: Moles and Conversion Factors in Chemistry Page 2/9  View this QuickTake in the app Concept Equation Molar Mass ( \text{Molar Mass} = \frac{\text{mass (g)}}{\text{moles}} ) Number of Moles ( n = \frac{m}{M} ) Number of Particles ( N = n \times N_A ) Conversion from Moles to Grams ( \text{mass (g)} = n \times M ) Where: ( n ) = number of moles ( m ) = mass in grams ( M ) = molar mass in g/mol ( N ) = number of particles ( N_A ) = Avogadro’s number (( 6.022 \times 10^{23} ) particles/mol) Conclusion This study guide encapsulates the essential concepts discussed in the lecture on atomic and molecular mass, moles, and conversion factors. Students are encouraged to engage with practice problems and apply critical thinking to enhance their understanding of these fundamental chemistry topics. 3. Glossary Market Demand and Element Abundance Market Demand: The desire for a particular element or commodity in the market, which influences its price and availability. Element Abundance: The relative quantity of an element found in a specific context, such as its presence in the human body, with key elements including oxygen, carbon, hydrogen, and nitrogen. Atomic Mass vs. Formula Mass Atomic Mass: The weighted average mass of an element’s isotopes, typically expressed in atomic mass units (amu). Formula Mass: The total mass of a compound calculated by summing the atomic masses of all the atoms present in its chemical formula. Molar Mass Molar Mass: The mass of one mole of a substance, usually expressed in grams per mole (g/mol), which is used to convert between grams and moles. Understanding Moles Mole: A unit of measurement in chemistry representing 6.022 x 10²³ particles (atoms, molecules, etc.), allowing for the quantification of substances. Conversion Factors Conversion Factors: Ratios used to convert one unit of measurement to another, essential for changing between grams, moles, and atoms in chemical calculations. Practical Calculations Practical Calculations: The process of applying mathematical methods to determine quantities such as the number of atoms from moles or vice versa, emphasizing the importance of organization in problem-solving. Examples and Practice Problems www.quicktakes.io Fundamentals of Atomic and Molecular Mass: Moles and Conversion Factors in Chemistry Page 3/9  View this QuickTake in the app Worked Examples: Step-by-step demonstrations of calculations involving moles and grams, designed to help students understand the application of concepts. Practice Problems: Exercises provided to reinforce learning and encourage students to apply their knowledge to solve similar problems independently. Critical Thinking in Problem Solving Critical Thinking: The ability to analyze and evaluate information logically, which is crucial for solving complex problems in chemistry. Reasonableness Check: A strategy for assessing whether an answer is plausible based on known values and expected outcomes. Final Thoughts Reinforcement of Concepts: The emphasis on the importance of practice and a solid understanding of fundamental chemistry concepts to succeed in the subject. Methodical Approach: Encouragement to tackle problems systematically and to utilize units as a framework for calculations. 4. Practice Calculate the molar mass of glucose (C₆H₁₂O₆). If you have 2 moles of water (H₂O), how many grams do you have? Convert 50 grams of carbon dioxide (CO₂) to moles. How many atoms are in 3 moles of nitrogen (N)? Determine the number of moles in 75 grams of sodium chloride (NaCl). If you have 1.5 moles of oxygen gas (O₂), how many molecules do you have? Calculate the formula mass of nitrogen dioxide (NO₂). Convert 10 moles of hydrogen (H) to grams. If you have 200 grams of a substance with a molar mass of 50 g/mol, how many moles do you have? How many grams are in 0.25 moles of potassium chloride (KCl)? 5. Transcript It’s cold. Coble is the one that is the more expensive right now because it’s the one that is the most demand, right? They needed the most and they increase in prices. This cobal, for that after that it will be iron. And which element you think is the more abundant in yourself? Oh, give me a guess. It should be a good guess because if you look at your body, you should know. Yeah. Oxygen, no, very close. It’s very, very close. Which one? and now we don’t have that in what we have it in the body, but it’s not, carbon. And this is when I started thinking, remember the teaching is beyond what you see in chemistry. I want you to think properly. And I say, which one could be the more abundant element of that? If I said the same thing about your body, which one would be the more abundant? You can have a good guess. One of it would be oxygen, carbon, hydrogen, nitrogen, those are the more abundant, but in your cell phone it will be carbon. So now let’s go about this. Atomic mass and formula mass. We’re gonna start doing it. some numbers today and I want you to practice with me. Meaning you’re gonna do your calculator, you’re gonna be doing some numbers. So we’re gonna have two different things. Atomic mass. Atomic mass will be the average mass. Of all the atoms of a particular element, right? All of the same. So meaning you’re gonna add all the hydrogens and all the carbons and all individual atoms, you’re gonna add them all. And then we have formula mass, which is the sum of all the atomic masses. So when we have a compound, nitrogen dioxide, and then we’re gonna start doing atomic mass, the atomic mass of nitrogen, it will be just the mass of nitrogen because there’s only one. But the atomic mass of dioxide, meaning two oxygens, it will be you have the weight of two oxygen, you add them. That is atomic mass for oxygen. Formula mass will be all three together. So that’s how we work, right? In this case, we have a long example of glucose. You have the formula, they’re asking you to calculate the formula mass. So for you to calculate the formula mass, you need to calculate the atomic mass of individual atoms first. So you can have how many atoms of carbon? You have six. What’s the weight? 12. And then you have hydrogen. How many of them? Well, what’s the weight? One, plus how many oxygen do you have? Six was the weight? 60. Now you add everything together, and now you have one number, and this is an atomic mass. And now we’re going to have, at the end, the formula mass. We’re getting this, it is important to understand the difference so we can do that. Okay, molar mass. Have you ever hear of the world, molar or polarity before class? Right, molar mass. So we’re talking about what’s the mass of a mole. What’s a mole, by the way? Somebody can tell me, very, just, it should be a very short definition. What’s a mole? is a unit of measures. That’s it. It’s a unit. Give me an example or another unit. Somebody. Great. grams. Thank you. Units, kilograms, pounds, ounces, you know, you name it. That’s a unit. This is a unit. Mole is a unit. So when we are talking about moles, we’re talking about a unit. It’s a specific mass for that. So in this case, we have this example. It’s a molar mass. define as mass in grams of one more of pure substance, of one more. So the unit is a mass, right? And then you said one more of water contains two moles of hydrogen and one more of oxygen. Then you do the math, you know, you find the mass from the great table, you add them and then you have the formula mass for this. One more of carbon. Think about the relationship. Think about how we use in the words in here. I say one more of carbon dioxide. contains one mole of carbon and two moles of oxygen. So you see how weird it sounds? I already said it’s one mole of the entire compound and then I said, yeah, but the ratio is one mole of carbon, two moles of oxygen. Are we good at that? Because the unit of mold is related to the mass of individual atoms www.quicktakes.io Fundamentals of Atomic and Molecular Mass: Moles and Conversion Factors in Chemistry Page 4/9  View this QuickTake in the app and you start seeing that what we do calculations. Same thing in here, you have the mass of carbon and then multiply by two the mass of oxygen oxygen, and then you got the formula mass, which is the total. Now you do some calculations very quickly here. Just use that break table to be enough for you to calculate what I asking you for I don’t know. Talk to your neighbor and see if you match, the numbers match, right? Before we move on. I’m going to give you a few more seconds. Practice. Practice, do it because this is going to be in your exam, right? So you need to practice in here. Five seconds. Four, three, two, one, close. Aiden. Aiden? Let’s see. So this is how you start calculating things, right? You have a compound in there, which is an ion that has three calcium, three moles of calcium. And then remember that the parentheses is telling you, like, this group of atoms are double. So you have two molesose, and then you have a lot of phosphate. And then you have eight moles of oxygen. Are we good? Now that you have clear what is individually in there, now you find the molar masses of them in the break table, and then you multiply by each one of them and add them. And the number should be eight. Questions about this? Are we good? I’m going to be. I’m going to be. I’m going to I’m going to I’m going to be. I’m going to be. I’m going to be. I’m going to be. I’m going to be. I’m going to be. I’m going to be. I’m going to be. I’m going to I’m going to It’s a good. It’s a good. It’s I’m going to and so We’re good five seconds. Four, three, two, two, one. Close. Elliot. See. So let’s try it again. The first thing that I will do is get this number straight. Separate when you have four carbons, four oxygens, seven nitrogen, one nitrogen. Once you have that, you add them, and then of course all your numbers will give you this. Questions? It doesn’t really matter how big The only thing that my concern is, is about the last example that I gave you, when you have calcium three and then parentheses, phosphate, two. That people do not know what to do with the parentheses. And I want you to be aware that that parenthesis multiply everything inside by the number that is outside In that case what two Everything else should be very easy to do We good So we talk about a mole and I ask you a question about what’s a mole, and how we can understand the meaning of the mole. And then somebody told us about, yeah, it’s a unit. Yeah, it is a unit. It is like the same thing, like we said a dozen. It’s a 12 things. It could be a dozen of eggs, it could be a dozen of bread, it could be a dozen of oranges, it could be a dozen of anything. Still the same. One dozen means 12. Is that right? So one mole means that a particle, any atom molecule, this is the amount that one mole will possess. So every element in the break table, we have the same number. number, meaning one more of it, it will be 6.022 multiplied by 10 to the 23. Every atom has the same amount of moles, but it’s not the same way. Remember that this is the amount of particles that are in one atom, one piece. If I have, you know, we’re going to do calculations, right? But the idea of this, the Avogadro’s numbers is telling you the amount of particles present in that mass. That’s the unit because the unit is so huge. You see how huge it is? That’s why we use micrograms, milligrams, grams, kilograms, and then you start moving out. Bigger the amount of particles are, you increase the unit that you’re using. So it’s easier for us to tell, right? You never say, hey, how far is your house? Then you can tell me, oh, I live 21 miles away from the university. You will never tell me I leave a couple millions of inches away from the university. All right. You’re not using that unit. Same thing here. We’re going to use Avogadro’s number to tell you that that’s the amount of numbers of particles that are present in that. I mean, you can name it. We can have different examples. Like Legos, for instance. I don’t know if you ever play with Legos, but you may have Legos with different sizes, and those may be different weights. So you can have all red ones and all blue ones, and then you can have 12 of them represent one more. But when you weigh them, it will weigh differently because the shape and the mass they process are different. But we still can call them a mole of blue and more of red. Are we clear on that? So more, it shows a generic way to say how many particles are pressed. And that’s an easy number to remember, I think. But we normally give it to you. So how we get this specified value? And then they start using this by, you know, using the atom of carbon. And then he said it was in an atom of carbon, you have 12, carbon, fewer, you know, 12 grams. And then in that 12 grams of carbon, that’s the number of atoms that are present in that amount. So you see 12 grams of power. And I don’t know if you, have you ever weighed anything in your life like sugar or salt or anything in a little balance? Have you seen it? Try this. Take the soda that you like the most. Code or Sprite or whatever you like. Read the label and see how many grams of sugar it possess. Then go to a lab or ask for a little balance and trying to put the same gram, the same grams that they possess. that they possess like 34 grams of sugar, put it in a balance. So you visually see what you eat it. And now you have an idea, right? 12 grams, I can imagine how much is 12 grams of that carbon. So now, we’re going to start doing conversions. And we’re going to, I’m going to call these conversion factors. Remember that in education in any topic, you always need to create basic knowledge, right? Because if you have basic knowledge, you can process information, you can think critically, and then you can make decisions based on those basic knowledge. This is one of the basic knowledge that you need to have. You need to know how a conversion factor will work. So in this case, we already discussed the fact that one model of atoms, of any atom, equals 6.022 multiplied by 10.2. But I can express it in the different way. I can tell you too that 6.022 will be divided by 10 to the 23 atoms are present in one more. It’s the same thing, right? I’m just telling you the two different ways. Why do I have that in two ways? Somebody can tell me. Why they are different, even though they’re equal. I mean meaning yes Yes But they different because we using it in different ways Yes Yeah Yeah it about unit transformation Thank you What your name Nick Okay Thank you, Nick. That is absolutely right. Because, and this is, once again, I always mention this to you, the best friend for you in chemistry one or two is the units. That’s your best friend. What I’m telling you is because you will never fail. If you use the units properly in any math problem, you know that you’re gonna get the right answer because the units will cancel out in a way that show you what you’re looking for. So this conversion factor is one of the keys for this because you’re gonna use it as a conversion factor for units. And we will see plenty of examples today. So I’m gonna put examples in here, but believe me, I want you to do calculations with me. It’s not enough for you to look at this, I said, ah, I got it. I want you to do it in paper. So it says calculate the number of copper atoms. Asking you for copper atoms. And then they give you 2.45 more. I’m going to give you my advice as me as a human, not as an instructor, how I faced chemistry when I was younger than you. So I used to write what is given to me. Then I would write what was given to me. Then I would write what was given to me I would write again what is in their specific what was given 2.45 moles of copper that’s what it was given to me and now and then I will reflect okay what was asked find the number of atoms and then I started thinking about how can I get there right very simple process but believe me it works when you start thinking about what you have and what you need to go so now we have something that is called conversion factors. And that’s something that we already saw, and it’s right here, is in between. And remember that I wanted in two different ways, is because I will move it accordingly to the question. So my units will cancel out. Units will cancel out when they’re at opposite sites. One above, and other one below, you always cancel. And then you will check it out your units at the very end. So we’re going to do the math problem. I’m going to write down along the table. This is very short. At one point we’re going to do calculations that we’re going to do conversion factors like a long way. But we’re going to start by what was given to you. 2.45 balls www.quicktakes.io Fundamentals of Atomic and Molecular Mass: Moles and Conversion Factors in Chemistry Page 5/9  View this QuickTake in the app of copper. Now my conversion factor is right here. And I’m going to write it in a way that the moles will cancel. And I will get at the end atoms, because the question is, how many atoms I have? So you see I have to refer back again to what is the question okay so now I have moles and they are opposite side right one is multiplied the only one is dividing now those units are gone what is the remaining unit the unit that I need you the one that is asking me for atoms so now the answer is I would hear this you always right the conversion factor either way. Same thing for the molecular mass with the mass that you grab from the very table. You can move it either way so you can do calculations properly. Good questions. Yes. You’re talking about this 23 and this 24, which is the math. Do you use the calculator? It’s just a multiplication. It’s if you multiply 2 by 2, you get 4. It changed. It’s the same way. I mean, right now, you increase the amount of articles in it. Just does the amount of atoms. And it makes sense. Think about it. How many atoms we said that one more possess? 6.022 multiplied by 10 to the 24. 10 to the 24. One mold. How many moles I have? Two point something. So I’m expecting to have more than one. So when I see 24, it makes sense, increases. And that’s something, once again, is again to double check yourself, it makes sense the answer. Are we good? If that number by any chance is less than 23, you know that you’re doing something wrong, because it should be more. All right. Now, please go ahead. ahead and start working on this. A silver ring contains 1.1 time to the 22nd silver atoms. How many moles of silver are in the ring? We are going backwards. So you’re going to flip your conversion factor this time. So let’s go and write what was given. And what do you need to do? to find. Always in your exams, I mean, you can do whatever you want in the exam, but this is my advice for you to approach it in that way. What’s the concept behind this? What do you have to do? What was given? Atoms. And then you know you have to go from atoms to moles. And to do the change, you need a conversion factor. And you already know the conversion factor. We saw it. It’s right there. So now, based on this, Do it. I’ll give you a few seconds to work it up. All right, I’m going to proceed. So now the solution is you’re going to use the conversion factor in between the change, and what you’re going to do is you’re going to write it. What was given to you is 1.1 multiplied by 10 to the 22nd atoms of silver. This is my conversion factor. And look, I’m writing the units of that conversion factor in a way that you will cancel out the opposite, right? will cancel out atoms and the remaining unit would be more which that’s the question so now I have one more as unit and then my answer will come along and so I have yes questions Yes. You didn’t get a number that is in there? What was the question? Yes, you can. Absolutely. Now, she said if she can write instead of 1.8 to the minus 2, if she can write 0.018. That’s true. You can write it. right but remember we give you options in the exam this is a multiple choice so make sure that you match what we’re giving you if we’re giving you an explanation numbers you choose that one are we good now let’s do another conversion mass and the amount of molds this is where we can start using the molecular mass of elements coming from the break table So we’re going to increase now our conversion factors. Now we’re going to have one more conversion factor coming into play so we can answer questions. Remember that molar mass. Where you can find the molar mass? Where you can find the molar mass of an atom? Crateroic table, right? So now we’re going to use trade table to calculate that. And then like atomic mass of copper is, and the molar mass is the same. Remember what was atomic mass? We saw it a few slides ago. Atomic mass was just the addition of all the atoms of the same element. So we have carbon 4H2 and then you have four carbons, you multiply by that weight and that’s you atomic mass. Moolar mass is the mass of the moles of that atom, which represent the same. Are we figuring this? It’s just, remember the moles and atoms, we’re talking about units and that’s all, but the numbers will be the same. One is atomic mass unit. The only one is grams per mole. Yeah. Correct. So that will be a conversion factor, and then you’re gonna be using for calculations, molar mass, because molar mass possess two items in here that can be, used for conversions. So you see these grams over mole is telling you 63.55 grams per mole meaning that in one mole there are 63.55 grams. Are we good? I can tell you that in 63.5 grams is one more or one more weighs 63.55. It’s the same thing. Remember it is a conversion factor so you can write it in any way to do calculations. That’s what we’re going to be doing so it’s clear for you. We have 60, that’s the molecular weight of copper, and then we know that it’s one mole of copper, because that’s the weight. And then this is the amount of atoms that that mole possess Are we good Everything is the same You just looking for the different units that we look at So 63.5 grams of copper are in one mole of copper. That’s how much it weighs. Are we good? And possess 6.022 to the 23 copper atoms. Is everybody on the same page on here? So we’re talking about the same thing right now. We can do it. Then now, any conversion, we can go from one side to the other. We can just go around this three. And we will do it a lot. I can give you grams and ask you for atoms or ask you for moles. I can ask you for anything and you can just go back and do conversions based on this facts. Okay? Conversion factors. Example, calculate the amount of carbon in molds. Be aware of the question. contain on this amount of grams. So this is just how can you approach this problem? What do you have that is necessary to solve this problem? Yes. You look, that is absolutely too. You look, again, I will always start with what was given. What was given to me? Okay, I have 0.02 65 grams of carbon. And then what they’re asking me to calculate is the number of moles of carbon. So I need to do a conversion in here of units. What is my conversion factor? David? That is my conversion factor. Where is this conversion factors coming from? Very table. Remember the units. When you look at the break table, it’s telling you grams per mole. It’s telling you that in one mole of carbon, they weight 12.01 grams of carbon. Okay, so I’m going to remember I can use this same conversion factor. In either way, the idea here is to eliminate this, the units that I don’t want to and keep the units that I need to have at the end. So I’m going to multiply. I start with what was given. This is the amount of grams of carbon, and I’m going to multiply that by the conversion factor. I’m going to write it in a way that grams will be canceled out. So now, what’s the remaining unit? Moles. What was the question? What is the amount of moles? Now I have an answer. We’re good? So I want you to practice with me today. This is hands-on, right? This is how you practice chemistry. So let’s do it. This is not a click-up, but I want you to start. And then we’re going to continue doing it. Just calculate the number of moles, and I give you these graphs. But, you see, I didn’t give you the formula. What I gave you the spelling, right? I write it so you can just write it first. It’s a din nitrogen monoxide. What kind of compound is this? Ionic or colon? Just because of the way that I’m writing it, you should know. Molecular compound? Yes, absolutely, because I use them prefixes. So you should know how to do that. So the first thing, I need to write this down because otherwise how can I do calculations, right? Is it dye nitrogen? Die nitrogen, and then it’s monoxide. Mono means one. This is what I have now. So now, what I need to know is I need to calculate the molar mass. molar mass would be nitrogen multiplied by two and oxygen multiplied by one right so you get your numbers from here and you get the final number so what you get is 123 let me see sorry let me write let’s start this 44 you always start with what was given what was given was 12.3 grams of thineatrogen monoxide And you’re going to multiply that by the conversion factor, which is coming from the great table, right? The atomic masses that we already discovered how to do it, which is 44.02. Grams of nitrogen are gone, and now I have moles of dinitrogen monoxide. You see the conversion factor is just helping me to achieve the results just by writing it in the proper way So my units will www.quicktakes.io Fundamentals of Atomic and Molecular Mass: Moles and Conversion Factors in Chemistry Page 6/9  View this QuickTake in the app cancel out Remember if you have something on top it because they are multiplying and they can be cancelled with the ones that are dividing So that why this will go away. The only remaining unit would be moles. Talk about the mass of 1.3 moles of C none. You see I’m going in the opposite way. This is just more practice. And then you start with what was given. I would write it. C-NN and then dye fluoride, it will be two of this, which is right here. You do the same thing, you go to a predict table and find the formula mass. It will be two fluorine and then one C-N, that will give you the weight of 169.3. Then now you can see malls and the answer is in frames. So again, it’s very repetitive, but it’s a logic process. And it’s always the same, guys. It’s always the same. So don’t get in chalk. We can write questions in many ways, but the process will never change. And you start seeing it with questions. So now, it’s a click. Let’s start. Not out of the middle. Not out of any more. So, so. We’re going to be. Thank you. Thank you. We’re going to be. I’m going to be. We’re going to be able to be. Okay. I’m going to be. Thank you. I want you to discuss it with your neighbor. Come on, this should be simple. I know what it will give you two to three minutes for every math problem. So you have time to discuss it and see if the number is okay, if you match. What answer are you getting, because I’m getting E. I put the wrong one. I’m getting that because it’s like 154 or whatever, and that’s, and E’s like 1.5, that’s the only, I’m really getting, I’m probably wrong now. Um, um, I’m not. Um, All right, you guys have four seconds. Three, two, two, one. And it’s close. Vera. E. All right, let’s start with what I say always. You always start with what was given to you. You start with the number of moles given 2.63 moles of nickel. And then they’re asking you to find the mass. What’s the conversion factor? What’s the conversion factor? My mass, right? It’s right there. Mass of what? Nickel. Where is that coming from? Great table, 58.69. And then, now let’s do calculations because I can do that and then from there I can calculate the mass in milligrams. Do you know what’s the conversion factor from grass to milligrams? You should know it. It’s something that is, it’s not just chemistry, it’s just 1,000, right? So we’re going to go over all this and 1,000. So if you notice here, this mole will cancel with this mole and now I have only 2 multiplied by 58 grams That the unit that I have it here And then I have grams of Nico It will cancel out with this grams And now my unit will be milligrams So I have this multiply by 1 milligrams. So this is how you do the calculation. 2.63 multiplied by this and my multiplied by this will give you the answer, which is… Are we good? Actually, let me see the statistics of this one. Maybe I can not see it. Okay. Well done, yes. All right. 90% of you got it right. How many copper atoms are in a copper penny with this mess? Now think about what I’m saying because now we have I’m giving you I’m asking you how many atoms and I’m giving you grams can you go from grams to atoms? Yeah David said no and he’s right you can not go from grams to atoms How can you do it? It just told me two. So you go from grams to moles, because now we know moles are related to atoms. Moles are not related to grams, to atoms, right? So now we get into the process. What was given to us 3.10 grams of copper, and then now we’re going to, you know, this is the whole process, number of moles, number of parts. You always have that in between. So we’re going to be using two different conversion factors. The first one is we need to know how many moles are in one mole of copper and this is coming from the break table. So now we’re going to write my equation in this way. You see we now start extending the way that we do conversion factors right now. This is what’s given to us. This is my first conversion factor and grams and grams of copper are gone. Now my unit is mole. Now I can use the second conversion factor, which is the one putting together moles and atoms. This is my second conversion factor. And I know now moles will cancel out, and my answer will be in atoms. And this is the answer. We’re good? Now we use it. This is the maximum amount that we go on these conversions, right? Unless we ask you from growth from, from milligrams to grams and then grams to moles and moles to atoms. Are we good? But that will be it for you in Gen Kemp. This is what we’re going to be using all the way from Gen Kemp 1 to Gen Kemp 2. We’re always going to ask you the same things. Always. So don’t forget this. This is crucial for you for the continuation of the Gen Kemp 1 and 2. This is how we’re going to work it out. So you need to practice a lot. So I always encourage you. encourage you to create a logical process when you are answering questions. Do not rush to answer a question. Even when somebody asks you like face to face a question, trying to think first before you answer, those milliseconds that you have to process will stop you to get it in trouble many times. Because when you answer, sometimes you answer with feelings and then feelings can hurt people. I’m related this to the exam. I’ve been professor for one and ten years, and I’m telling you across the board when the students come to an exam, how you get here? Happy? No. You get excited and nervous. Those are two feelings that block your brain from proper thinking. So when you come and we ask you questions, I want you to pause, to think, to do a game change. You know, you’re gonna play a game in your brain. This is what I’m gonna do every time. I’m gonna read the question. I’m going to write down what they’re asking me for. I’m going to write out what they gave me. And I’m going to plan how can I get there. You see, take a few seconds to do that, and you will do it. This is how I’m asking you to plan you play day, right? So you can go from grounds to malls, to atoms, and all the way in between. You can not go from here to here. Are we good? You always have to use that. And what is the name of that we’re using to convert this? Conversion factors. One is coming from the break table, which is the atomic mass of the compound. You calculate the atomic mass. And then now you have the abogadros number, is the last conversion. Are we good? Another that it will be just units. When you have to change to pounds, to kilograms, to milligrams, micrograms, that’s something that we expect. to know. Let’s do this. How many aluminum atoms are in a can? You see, I’m asking you for all all conversions, right? So I’m asking you how many atoms you know that you need to use Avogatros number? And then I’m telling you that an aluminum can weighs 16.2 grams. So what I would do, I would write out the things that I need to know, right? What was given, what they asked for. Now I’m going to write down my plan. Once again, I’m teaching you how to solve your problems in not just chemistry in general. That’s how you should approach the problems to. So you have your plan. Okay, now I have the grams of aluminum. I need to go from moles. This is when you got the basic knowledge in place. You know that you can not go from grams to atom. You need to go from grams to moles first. And then moles are related to atoms, and then you can do that with Amogadros number. So what’s the relationships? You know it. The way the atomic mass is coming from the Greek table. If it’s only one atom, you just look it out and get it. If it’s a molecule, you calculate the entire mass first. Now you have it. Now you can go and do the solution. And that’s what we’re going to be doing. My conversion factors will be in between these two. Once again, this is my conceptual plan. This is what I need to do to get there. So now we’re gonna start doing the map. What was given, 60.2 grams of aluminum conversion factor is coming from the very table, knowing the molecular weight of my aluminum is 26.98. Now I can cancel the grams and I have moles. I know I am a mold right now, but my answer should be in atoms. So now I need to multiply by the conversion factor that joins my moles and atoms, which is avocado’s number, and I’m going to write it in a way. Remember, this is very important. You’re going to write it in a way that moles will cancel out. Now my answer should be in atoms. Are we good? Questions? This is just to double-check you thinking. You know, my first degree is in education. I just want to clarify that to you. My first degree is in education. Second degree is in chemistry. I have to. One education about chemistry, the www.quicktakes.io Fundamentals of Atomic and Molecular Mass: Moles and Conversion Factors in Chemistry Page 7/9  View this QuickTake in the app other one is in pure chemistry. So I’m teaching you how to do analysis of any question that you have, not just in chemistry. But when you have a question, you always have to have a plan to answer the question. And this is how I want you to start getting used to. to do it, right? So now you think about, is my answer right? Can I have some clues if my answer is right? Yes, one clue, is the unit right? What was the question? How many atoms? So my unit at the end should be atoms. Do I have atoms? Yes, I do. So it’s a good indication that my answer is okay. And then I can think again, how much a mole of aluminum weights. You already calculated it’s 26.98. That’s how much a mole. How much a can weight? 16.2. So what is the proper thinking here? My answer should be less than what a mole weights. Are we good? It is less? Yes, it is. Are you full of what I’m trying to say? It’s just clue or finding out if you answer is correct. It’s better than going outside of the exam, that’s what you guys used to do. You go outside and then you all chat together and see who got the right answer and not and then you get, you know, finding all these things. Now, before you go, you do this and you go happier home, right? Let’s do it again. Find the number of molecules. Remember the molecules and atoms, you can do it in the same way. So I’m going to write down what was given. 10.8 grams of carbon dioxide. I need to find the molecules. What’s my plan of action? Then I know I can go from grams to moles and moles to molecules, because that’s how the relationship will go. And in between, I will have two conversion factors that I can lay it down right there. If I don’t know the mass of CO2, of course, I have to go where to get it? Pretty table. So I can go on and do the formula mass for CO2. One carbon, two oxygens, you add them together, and that’s the molar mass, and then it will be 44.01 rest Now I after that my plan I have my numbers Now I going to solve my problem I going to start with what was given again 10.8, and then I multiply that by the first conversion factor, which is changing grams to moles. You have to be very logical why are you using that one. It’s because you want to change your grams to molds. Now, of course, these grams are gone. I have moles. I’m not done yet. Now I have to multiply by the second conversion factor, which is going to change my moles to molecules. So these moles, we go away, and my answer is in molecules now. Are we good? Questions about this? Now, you can do the same thing, a process, to check if the number makes sense. First thing is, is my unit correct? And I encourage you to first check you units because many mistakes that you knew. Okay, let me rephrase that. We’re about to finish. When we ask you a question in an exam, we sit together, we are four teachers, and we spread 20 questions among us. They say you take five learning objectives and we choose five. Each one of us choose five. Once we got together, we review the questions and accept or reject, depending on our feelings, right? Now it’s too hard, now it’s too easy, and then we should try to get an agreement. Once we get that, the answers that we give it to you are based on what we know, the mistakes that you may do. Are you guys clear on that? If we understand what is the struggle with you, we can give you different answers with different units, knowing that I know you’re gonna make the mistake of using this unit. So I’m gonna put it in there for you. So when you see it, you said, yeah, at it, it’s right, but it’s not right, because it’s a mistake. So what I’m trying to say, double check to answer first before you choose from what is displayed to you. Are we good? So in other words, I can give you a number that only involves the first multiplication. As one of the possible answers, I can choose multiply, divide this by this, and the number that comes out of it, I’m going to put it as an answer. So when somebody’s doing calculations in your exam and you see the number, oh, it’s right there. Done. That’s why a proper process of thinking and solving the problems in the same way, in a logical way, you save yourself on tragedy. Exam one is the strategy, always tragedy on Gen Camp, because everyone is confident. But I want you to be aware that you can make it very good this and I say. So let’s do it. Now once again, you see is grams and atoms. Lay down you plan. What are you going to be doing? What’s the conversion factor? This two that you have to use. Which ones are those? Write it down and solve it. Good, thank you for letting me no idea and open it. Sometimes I forget. You guys, I normally give you three minutes. So let’s speak with two and a half. For now, I think it’s enough time for you guys to solve it. If you struggle, raise your hand, I can go to you in doing this. minutes okay So, I’m going to be. We’re going to be. I’m going to be. I’m going to be. I’m going to be. So, I’m going to be able to be. So, I’m going to be. I’m sorry. What did you get that? I got a I think I man my son one like this. None. You have enough information to solve. We have enough information to solve. We have a lot of things. Very much. There you. We have a great. We have a great. We have a good. We have a lot of it. And I’m not right. This is a lot of it. I don’t get over. Wait. Why? I don’t know. You can go in this year? You can go in this year? You can use it. You can do it. Oh, yeah. I don’t know. I need a little. I’m a very. So, I’m going to take five. All right, guys, you have five seconds. Four, three, two, one, close. Julia. What is it? Is it? Did you answer? I already closed it. You didn’t send an answer? Okay. Somebody sent an answer, give me your answer. Huh? Hey, now let’s do this. This is very interesting. Remember that life will never give you exactly what you are prepared for. You have to prepare for the unknowns. This question, we haven’t seen it yet, but we have enough materials. have enough materials to do it. How? Just proper thinking. So now let’s think about this. It says three grams. Okay, three grams of a sample and an element, an element. So we don’t know the element. Let’s go back. Contains, this is the amount of atoms. So in the proper thinking, we know that we can go from grams to moles and to moles to atoms. Are we good? That’s the way we should go normally. Grams to moles to atoms. This is the direction. And here we have a conversion factor. And here we have a conversion factor. So we have two conversion factors to go from one side to the other. Are we clear this? This is basic knowledge that we have built so far. The question is asking me, identify the mass, which is right here. It’s telling me, identify the mass, which is in the middle of this conversion that we normally do. My question is, can I go from grams and find this? No, because I don’t know the element. I do not know the element. The question is, was the element? Are we going to hear? So this is once again, I want you to start learning how to think. One direction do not work. But can I go from the other direction? Can I go from atoms to moles? Yes, because I have atoms were given to me and I have the conversion factor. What’s the conversion factor? Avogadro’s number. So now let me erase that and then we’re going to see it. So I have the amount of atoms that was given and this is my conversion factor. Then atoms and atoms are gone. Now I have moles. Right? Now I have moles and I have grams. What is the atomic mass? What is the unit of atomic mass? Molever mass? Grams per mole. So now you just finish. And then now you have the grams that were given. divided by the mold that you choose found it and now the answer should be 52. Who is 52 Chrombium Did I do you guys send the answer for this one Yeah, right? Sorry, let me see if the statistics in this one is. 81% of you got it right. I’m very proud of you. This is good. Questions about this? Any questions? You see, I’m showing you everything that could be possible in an exam. And this is the one that is the more extraordinary, meaning it may happen if you know it, this is very good. If you know how to do this, it’s just you’re very good right now. Good? Questions for me? We’re going to be. I’m going to be. We’re going to be. So, I’m going to be. So, I’m going to be. And so on the So, I’m going to be. So, and So, I’m going to be able to So, I’m going to be. I’m going to be. I’m going to I’m going to I’m going to be. We’re going to be. I’m sorry. I’m going to be. We have a lot of it. Raise you know. with the math. I should want to see an average on timing. Five seconds, four, three, two, one, close. Neck. Nick. I’m sorry, I www.quicktakes.io Fundamentals of Atomic and Molecular Mass: Moles and Conversion Factors in Chemistry Page 8/9  View this QuickTake in the app didn’t necessarily. All the answer. Okay. So you already know the mass of aluminum. So what do you need to do is you start with what is given to you. 20 point grams of aluminum. And then what will be my first conversion factor? The motor mass of it. So I’m going to write it in a way that I can cancel out. I’m going to say that one mole of aluminum weights 26.98 grams. So this is going to cancel. Gramps, now I know I have the units of moles. So what will be my next step? Avogadro’s number, right? Because I need to go from moles to atoms, right? I’m saying they’re going to be doing this. Are we good? One more before you go home. I’m sorry. So we need to be able to be a good for the first of us. I don’t know how much. I’m going to be able to be. We’re going to be. I’m sorry. You’re going to be used in all the compression factors that we have seen as far plus one, which is changing grams to kilo. Thank you. www.quicktakes.io Fundamentals of Atomic and Molecular Mass: Moles and Conversion Factors in Chemistry Page 9/9