4. Let's try another atomic mass problem. Suppose you have a mixture of two chlorine isotopes. The mixture is 40% Chlorine-37 and 60% Chlorine-35. Predict the atomic mass of this mixture. Hint: This is NOT nature's abundance of chlorine. You can check your answer by clicking "My Mixture" under isotope mixture. Next, create the mixture described in the problem. 35.8 amu 36.2 amu 36.0 amu

4. Let's try another atomic mass problem. Suppose you have a mixture of two chlorine isotopes. The mixture is 40% Chlorine-37 and 60% Chlorine-35. Predict the atomic mass of this mixture. Hint: This is NOT nature's abundance of chlorine. You can check your answer by clicking "My Mixture" under isotope mixture. Next, create the mixture described in the problem. 35.8 amu 36.2 amu 36.0 amu

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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Look at the first question to answer the second one
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Write the name of the following elements, ions, or compounds: (please answer all questions in order) a.) the element that has 16 protons b.) the ion with a -1 charge that has 18 electrons c.) the compound made from the alkali metal in the third period and the element with the atomic mass of 30.97 amu d.) the polyatomic ion that contains one sulfur and three oxygens e.) the compound made from the non-metal in group 1A and the polyatomic ion containing one nitrogen and three oxygens. f.) the element in which 0.274 moles weighs 24.01 g.
On earth, tin has 10 different stable isotopes. The heaviest, 124 Sn makes up 5.80% of naturally occurring tin atoms. a) How many atoms of 124 Sn are present in 42.7 g of a natural sample of tin? 124 Sn: 1.491e24 atoms Scientific Notation: 1.491 x 1024 Helpful tip: To enter a number in scientific notation, enter 0E5 or 1.0e5, for 1.0 x 105 where the E# (or e# ) denotes 10# b) Considering 124 Sn has an isotopic mass of 123.905 amu, calculate the mass of this isotope in the sample. Mass: 8.0 g
Before you Begin: Use your Periodic table to complete the table: Magnesium Name Hydrogen Oxygen Carbon socomsUlfor CI Symbol Na Atomic # Atomic .0079 Mass 15.999 # Protons # Electrons 17 Group 1 Period 1 3 Procedure: 1. Pick one color of bead to represent each of the elements below. Use map pencils to color the circle with the color you chose to represent the element. Hydrogen (H) Oxygen (O) Sodium (Na) s nodh to mote ono Sulfur (S) worlk oT belleo a senluomed ouc Carbon (C) Chlorine (CI) ebixoib nodt yolom Sis eor aneem ai w Juods Magnesium (Mg) a. Molecules with two atoms are linear: b. Molecules with two atoms on either side of a center atom are bent: c. Molecules with three atoms around a center atom are shaped like pyramids: 2. Given this information:
3. Two naturally occurring isotopes of silver are 107Ag (relative abundance 52.00%) and 109Ag (relative abundance Assume that the masses of the isotopes are 107 and 109 exactly. Determine the average atomic mass from these 48.00%). data. a. 107.48 b. 108.52 C. 107.52 d. 108.96 107.96 e. f. 109.48 g. 108.04 h. 110.54 PP
Element C has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ___amu?
Use the model to answer the following question. Element A Element C KEY Proton Element B Neutron Which of the following explanations are TRUE regarding the mass number and identity of Element C? OA Element C has only a different identity than elements A and B B. Element C has both a different mass number and identity than elements A and B C. Element C has the same mass number and identity as elements A and B O D. Element C has only a different mass number than elements A and B Lenovo DII @ 3 5 e r d f h k C V b
You have an unknown element consisting of two isotopes, one with mass = 36.9659 amu (24.22%), and one with mass = 34.9688 amu (75.78%). a. Use the weighted average calculation to obtain the atomic mass (weighted average). Show your calculations. Give final answer in 4 significant digits. b. What is the name of the element? c. What is the atomic symbol? d. Draw a similar table and fill in the table for the two isotopes. Please write Isotopes in the following format: = of Neutrons (no decimal numbers) Atomic Number # of Electrons Atomic Mass (no decimals) Isotope # of Protons ick Cancel to quit. Cancel Beg DELL insert prt sc end F12 home F5 F6 F8 F9 F10 F11 F4 4 7 8
Of all chlorine atoms, 75.771% are chlorine-35. Chlorine-35 atoms have a mass of 34.96885 amu. All other chlorine atoms are chlorine-37 and these have a mass of 36.96590. Calculate the average atomic mass of chlorine. Hint: Percentages must equal 100, so 100 - 75.771 = the missing percent.