The Effect of Different Isotopes on Atomic Mass (Chemistry Lab)

The Effect of Different Isotopes on Atomic Mass Introduction An isotope is a variation of an atom that already exists. An isotope is different from an atom because of the moment of neutrons in its nucleus. considering the amount of neutrons in an atom can be calculated by subtracting the atomic frame of a specific atom from its atomic pickle. When looking at the semestral table, the atomic potbelly in the top left corner of each box is a decimal. The pile is in decimal format because the outlet listed is an amount of that atom, plus all of its isotopes.Isotopes set about different bookes because neutrons consider 1 amu where as an electrons weight would be negligible. The prove described under shows how including all isotopes of one and only(a) element effect the second-rate atomic push-down stack of the element. Materials 1. Calculator 2. Whitium adjudicate 3. Brownium sample 4. Blackium sample 5. 3 plastic cups 6. electronic balance 7. Data table Procedure 1. Se parate the whitium, brownium, and blackium samples from each other. 2. Find the mass of 1 cup with the electronic balance. 3.Put the different samples in snap off cups and count the number of beans in each cup write those come in the data table. 4. Find the total number of beans. 5. Find the mass of each cup of beans (using the electronic balance) and subtract the mass of the cup. issue these total in the data table. 6. Divide the mass of each sample by its respective amount of beans to find the reasonable mass of one bean. Write these numbers in the data table. 7. Divide the number of beans from 1 sample by the total number of beans to find the percent of the total that that bad-tempered isotope takes up.Do this for each of the samples. Record these numbers in the data table. 8. To find the average atomic mass of beanium, use the following formula percent of balckium atomsaverage mass of blackium percent of brownium atoms average mass of brownium +percent of whitium atoms ave rage mass of whitium atomic mass of beanium Record this number in the data table. Results Isotope make out of beans (atoms) Mass of beans (g) second-rate mass of one bean (g) Percent of beans Average atomic mass of beanium Blackium 293 65. 8 . 224 62. 7% . 43 gBrownium 104 62. 5 . 60 22. 3% Whitium 70 69. 2 . 99 15% essence 467 To calculate the percentage of beans Number of Beans of 1 IsotopeTotal Number of Beans To calculate the atomic mass of beanium percent of balckium atomsaverage mass of blackium percent of brownium atoms average mass of brownium +percent of whitium atoms average mass of whitium atomic mass of beanium Conclusion In conclusion, an isotope is a variation of an element that already exists. It is different because it has more or less neutrons in its nucleus.Depending on how many isotopes one element has, the average atomic mass will change. When calculating the average atomic mass, you must(prenominal) include all of the isotopes which have more or les s neutrons than the reliable element. Since neutrons have a mass of 1amu, the isotopes masses will vary, thus bear upon the average atomic mass of an element. When performing this experiment, the mass of the beans were measured plot the number of beans, average mass and percent of beans had to be calculated. The average mass of he beans, or isotopes, was a decimal because the weight of the beans in one sample divided by the number of beans of the same sample was not an even number. This lab simulates the various isotopes of an element because all of the beans were in the same family however, they all looked different and had different masses. This is an example of how real elements have isotopes that whitethorn not look alike or have the same mass, exclusively theyre still a part of that one element. As this experiment whitethorn have gotten the results shown above, when performing this experiment a second time, the results may vary.This is because not every bean is identical. If larger samples are used accordingly the difference may be smaller because the larger the sample you have to work with, the closer your average will be to the actual mass. 1 source of flaw in this experiment may have been miscounting the number of beans. This may change the results of the 2, 4, and 5 columns of the data table. Another source of error may have been miscalculating the average mass of one bean. This would affect the final result for the atomic mass of beanium.