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Given the data for hydrogen as it exists in nature: Isotope Atomic Mass Percent Abundance 99.985% 0.015% Hydrogen-1 1.0078 amu Hydrogen-2 2.0141 amu a) Make a prediction about the average atomic mass of hydrogen. I predict the average atomic mass of hydrogen will be the number of protons neutrons, while atomid mass (or isotopic mass) is the mass if you were to somehow weight on a balance ... To find the average atomic mass f neon, we will use the equation above and take the abundance of the inst isotope times the mass of the first isotope plus the abundance of the second isotope times the mass of the second isotope plus the abundance of the third isotope times the mans of the third isotope However, you might recall from your math courses that when y use a percentage in a calculation you always want to use the decimal form, meaning you must first divide the percentage by 100. The equation would then look (0.9048 x 19.9924 amu)-(00027 x 20.9038 amu)(0.0925x21.9914 amu) 18.009 amu -20.15 amu This is the average atomic mass of neon. Let's just take a second and see if 20.18 amu seems like a reasonable answer, given the initial data. According t the table, most neon (over 90%) has a mass of approximately 20 amu, a tiny bit has a mass of around 21 amu, and around 9% has a mass of 22 amu Based off this we would predict that the answer would be close to 20 amu, but sightly higher which it ist b) Calculate the average atomic mass of hydrogen and show all your work. c) Check your answer with a Periodic Table. What is the average atomic mass of hydrogen? d) Was your prediction correct? Explain.

Given the data for hydrogen as it exists in nature: Isotope Atomic Mass Percent Abundance 99.985% 0.015% Hydrogen-1 1.0078 amu Hydrogen-2 2.0141 amu a) Make a prediction about the average atomic mass of hydrogen. I predict the average atomic mass of hydrogen will be the number of protons neutrons, while atomid mass (or isotopic mass) is the mass if you were to somehow weight on a balance ... To find the average atomic mass f neon, we will use the equation above and take the abundance of the inst isotope times the mass of the first isotope plus the abundance of the second isotope times the mass of the second isotope plus the abundance of the third isotope times the mans of the third isotope However, you might recall from your math courses that when y use a percentage in a calculation you always want to use the decimal form, meaning you must first divide the percentage by 100. The equation would then look (0.9048 x 19.9924 amu)-(00027 x 20.9038 amu)(0.0925x21.9914 amu) 18.009 amu -20.15 amu This is the average atomic mass of neon. Let's just take a second and see if 20.18 amu seems like a reasonable answer, given the initial data. According t the table, most neon (over 90%) has a mass of approximately 20 amu, a tiny bit has a mass of around 21 amu, and around 9% has a mass of 22 amu Based off this we would predict that the answer would be close to 20 amu, but sightly higher which it ist b) Calculate the average atomic mass of hydrogen and show all your work. c) Check your answer with a Periodic Table. What is the average atomic mass of hydrogen? d) Was your prediction correct? Explain.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Avg Atomic Mass=(M1*A1)+(M2*A2)+(M3+A3)/100 Or. Using decimal abundances: Avg Atomic Mass=(M1*A1)+(M2*A2)+(M3*A3)
Given the data for hydrogen as it exists in nature: Isotope Atomic Mass Percent Abundance 99.985% 0.015% Hydrogen-1 1.0078 amu Hydrogen-2 2.0141 amu a) Make a prediction about the average atomic mass of hydrogen. I predict the average atomic mass of hydrogen will be Remember that mass number is not the same as the atomic mass or isotopic mass! The mass number is the number of protons neutrons, while atomsid mass (or isotopic mass) is the mass if you were to womehow weight on a balance To find the average atomic mass of neon, we will use the equation above and take the abundance of the inst isotope times the mass of the first isotope plus the abundance of the second isotope times the mass of the second isotope plus the abundance of the third isotope times the mans of the third isotope However, you might recall from your math courses that when you use a percentage calculation you always want to use the decimal form, meaning you must first divide the percentage by 100. The equation would then look like: (0.9048 x 19.9924 amu)-(00027 20.9038 amu)+(0.0925x21.9914 amu) 18.009 amu 0.0516 2.034 amu 20.15 amu This is the average atomic mass of neon, Let's just take a second and see if 20.18 amu seems like a reasonable answer, given the initial data. According to the table, most neon (over 90%) has a mass of approasemately 20 amu, a tiny bit has a mass of around 21 amu, and around 9% has a mass of 22 amu Based off this we would predict that the answer would be close to 20 amu, but slightly higher: which it ist b) Calculate the average atomic mass of hydrogen and show all your work. c) Check your answer with a Periodic Table. What is the average atomic mass of hydrogen? d) Was your prediction correct? Explain.
Transcribed Image Text:Given the data for hydrogen as it exists in nature: Isotope Atomic Mass Percent Abundance 99.985% 0.015% Hydrogen-1 1.0078 amu Hydrogen-2 2.0141 amu a) Make a prediction about the average atomic mass of hydrogen. I predict the average atomic mass of hydrogen will be Remember that mass number is not the same as the atomic mass or isotopic mass! The mass number is the number of protons neutrons, while atomsid mass (or isotopic mass) is the mass if you were to womehow weight on a balance To find the average atomic mass of neon, we will use the equation above and take the abundance of the inst isotope times the mass of the first isotope plus the abundance of the second isotope times the mass of the second isotope plus the abundance of the third isotope times the mans of the third isotope However, you might recall from your math courses that when you use a percentage calculation you always want to use the decimal form, meaning you must first divide the percentage by 100. The equation would then look like: (0.9048 x 19.9924 amu)-(00027 20.9038 amu)+(0.0925x21.9914 amu) 18.009 amu 0.0516 2.034 amu 20.15 amu This is the average atomic mass of neon, Let's just take a second and see if 20.18 amu seems like a reasonable answer, given the initial data. According to the table, most neon (over 90%) has a mass of approasemately 20 amu, a tiny bit has a mass of around 21 amu, and around 9% has a mass of 22 amu Based off this we would predict that the answer would be close to 20 amu, but slightly higher: which it ist b) Calculate the average atomic mass of hydrogen and show all your work. c) Check your answer with a Periodic Table. What is the average atomic mass of hydrogen? d) Was your prediction correct? Explain.
average atomic mass = [[relative abundance x mass of isotope) Remember that E is the symbol for sum. In other words, of each isotope multiplied by its mass Example Neon has three naturally occurring isotopes Symbol NIJO Ne-21 Mas Isotopic matt number (amu) 1904 21.9914 1992 Percent natural SPOMEN abundance 90.48% 027 Remember that muss number is not thUNK” jome mass or sdopić nau) Îv ras number is Se vise of probes • NEUTOES, WEVOZNUNZIOUNS)\TemassIWWED somehow weigh it on a balance To find the average atomic mass of neon, we will use the equation above and take the abundance of the first isotope times he mass of the first sobne nUSTH SUNCance of the second soʻope times the mass of the second isotope plus the abundanced tesed sclope treN-kd the third isolope However, you might recall from your math courses hart when you use a percentage in a calculation you always want to use the decimal form, meaning you must first övide the percentage by 100. The equation would then look like 9254 10.9048x 19.99024 amu) (0.0027 x 20 9936 amu) - (0.0325 x 21 0914 au) DVASININEN the sum of the relative abundance POSTIZE This is the average storeMge, Let's usi SEIZONTERETN0 18 aru seems the a PE POSVETS VANUSIIMNE DOTZ-V KIKUUT PENASIASI ŽIU PONTY
Transcribed Image Text:average atomic mass = [[relative abundance x mass of isotope) Remember that E is the symbol for sum. In other words, of each isotope multiplied by its mass Example Neon has three naturally occurring isotopes Symbol NIJO Ne-21 Mas Isotopic matt number (amu) 1904 21.9914 1992 Percent natural SPOMEN abundance 90.48% 027 Remember that muss number is not thUNK” jome mass or sdopić nau) Îv ras number is Se vise of probes • NEUTOES, WEVOZNUNZIOUNS)\TemassIWWED somehow weigh it on a balance To find the average atomic mass of neon, we will use the equation above and take the abundance of the first isotope times he mass of the first sobne nUSTH SUNCance of the second soʻope times the mass of the second isotope plus the abundanced tesed sclope treN-kd the third isolope However, you might recall from your math courses hart when you use a percentage in a calculation you always want to use the decimal form, meaning you must first övide the percentage by 100. The equation would then look like 9254 10.9048x 19.99024 amu) (0.0027 x 20 9936 amu) - (0.0325 x 21 0914 au) DVASININEN the sum of the relative abundance POSTIZE This is the average storeMge, Let's usi SEIZONTERETN0 18 aru seems the a PE POSVETS VANUSIIMNE DOTZ-V KIKUUT PENASIASI ŽIU PONTY
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