The element lithium has two stable isotopes, lithium-7 with an atomic mass of 7.0160 u and lithium-6 with an atomic mass of 6.0150 u. From the atomic mass of Li = 6.94 u one can conclude that: lithium-7 has the highest percent natural abundance both isotopes have the same percent natural abundance lithium-6 has the highest percent natural abundance

The element lithium has two stable isotopes, lithium-7 with an atomic mass of 7.0160 u and lithium-6 with an atomic mass of 6.0150 u. From the atomic mass of Li = 6.94 u one can conclude that: lithium-7 has the highest percent natural abundance both isotopes have the same percent natural abundance lithium-6 has the highest percent natural abundance

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

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 43E: The element europium exists in nature as two isotopes: 151Eu has a mass of 150.9196 u and 153Eu has...

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Neon is an inert gas with three stable isotopes. It is used in gas lasers and in advertising signs. Its isotopes and their abundances are: Ne-20 19.9924 amu 90.51% Ne-21 20.9938 amu 0.27% Ne-22 21.9914 amu 9.22% What is the average atomic mass of neon?
See the definition for isobars in Question 15. Consider Cr-54, Fe-54, Fess, and Ni-S8. (a) Which of these are isobars? Which are isotopes? (b) What do Fe-S4 and Fe-58 have in common? (c) Which atoms have the same number of neutrons?
Chlorine has two isotopes, Cl-35 and Cl-37. Their abundances are 75.53% and 24.47%, respectively. Assume that the only hydrogen isotope present is H-1. (a) How many different HCI molecules are possible? (b) What is the sum of the mass numbers of the two atoms in each molecule? (c) Sketch the mass spectrum for HCI if all the positive ions are obtained by removing a single electron from an HCI molecule.
Uranium-235 is the isotope of uranium commonly used in nuclear power plants. How many (a) protons are in its nucleus? (b) neutrons are in its nucleus? (c) electrons are in a uranium atom?
Determine whether the statements given below are true or false. (a) The mass of an atom can have the unit mole. (b) In N204, the mass of the oxygen is twice that of the nitrogen. (c) One mole of chlorine atoms has a mass of 35.45 g. (d) Boron has an average atomic mass of 10.81 amu. It has two isotopes, B-10 (10.01 amu) and B-11 (11.01 amu). There is more naturally occurring B-10 than B-11. (e) The compound C6H12O2N has for its simplest formula C3H6ON1/2. (f) A 558.5-g sample of iron contains ten times as many atoms as 0.5200 g of chromium. (g) If 1.00 mol of ammonia is mixed with 1.00 mol of oxygen the following reaction occurs, 4NH3(g)+5O2(g)4NO(g)+6H2O(l)All the oxygen is consumed. (h) When balancing an equation, the total number of moles of reactant molecules must equal the total number of moles of product molecules.
The element europium exists in nature as two isotopes: 151Eu has a mass of 150.9196 u and 153Eu has a mass of 152.9209 u. The average atomic mass of europium is 151.96 u. Calculate the relative abundance of the two europium isotopes.
Mass spectrometric analysis showed that there are four isotopes of an unknown element having the following masses and abundances: Three elements in the periodic table that have atomic weights near these values are lanthanum (La), atomic number 57, atomic weight 138.9055; cerium (Ce), atomic number 58, atomic weight 140.115; and praseodymium (Pr), atomic number 59, atomic weight 140.9076. Using the data above, calculate the atomic weight, and identify the element if possible.
Argon has three naturally occurring isotopes: 0.3336% 36Ar, 0.063% 38Ar, and 99.60% 40Ar. Estimate the average atomic mass of argon. If the masses of the isotopes are 35.968 u, 37.963 u, and 39.962 u, respectively, calculate the average atomic mass of natural argon.
2.92 A candy manufacturer makes chocolate-covered cherries. Although all of the products look roughly the same, 3% of them are missing the cherry. The mass of the candy with a cherry is 18.5 g; those missing the cherry weigh only 6.4 g. (a) How would you compute the average mass of a box of 100 of these chocolate covered cherries from this manufacturer? (b) I low is this question analogous to the determination of atomic weights?