General Chemistry: Principles and Modern Applications (11th Edition)
11th Edition
ISBN: 9780132931281
Author: Ralph H. Petrucci, F. Geoffrey Herring, Jeffry D. Madura, Carey Bissonnette
Publisher: PEARSON
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Chapter 25, Problem 81SAE
Interpretation Introduction
Interpretation:
The element which has eight naturally occurring isotopes is to be determined.
Concept introduction:
The isotopes of atoms are determined by the same number of protons but have a different number of neutrons in their nucleus.
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Students have asked these similar questions
Consider the atoms (a) P-31, (b) S-33, and (c) P-33.
From greatest to least, rank them by the number of neutrons in the nucleus.
From greatest to least, rank them by the number of nucleons in the nucleus.
Nuclei differ in their stability, and some are so unstable thatthey undergo radioactive decay. The ratio of the number of neutrons to number of protons (N/Z) in a nucleus correlateswith its stability. Calculate the N/Zratio for (a) ¹⁴⁴Sm; (b) ⁵⁶Fe;(c) ²⁰Ne; (d) ¹⁰⁷Ag. (e) The radioactive isotope ²³⁸U decays ina series of nuclear reactions that includes another uranium isotope,²³⁴U, and three lead isotopes, ²¹⁴Pb, ²¹⁰Pb, and ²⁰⁶Pb. How manyneutrons, protons, and electrons are in each of these five isotopes?
How many protons, neutrons,and electrons are there in an atom of (a) 10
5B, (b) 36Ar, (c) 8538Sr, and
(d) carbon-11?
Chapter 25 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
Ch. 25 - Prob. 1ECh. 25 - Prob. 2ECh. 25 - Prob. 3ECh. 25 - Prob. 4ECh. 25 - Prob. 5ECh. 25 - Prob. 6ECh. 25 - Prob. 7ECh. 25 - Prob. 8ECh. 25 - Prob. 9ECh. 25 - Prob. 10E
Ch. 25 - Prob. 11ECh. 25 - Prob. 12ECh. 25 - Prob. 13ECh. 25 - Prob. 14ECh. 25 - Prob. 15ECh. 25 - Prob. 16ECh. 25 - Prob. 17ECh. 25 - Prob. 18ECh. 25 - Prob. 19ECh. 25 - Prob. 20ECh. 25 - Prob. 21ECh. 25 - Prob. 22ECh. 25 - Prob. 23ECh. 25 - Prob. 24ECh. 25 - Prob. 25ECh. 25 - Prob. 26ECh. 25 - Prob. 27ECh. 25 - Prob. 28ECh. 25 - Prob. 29ECh. 25 - Prob. 30ECh. 25 - Prob. 31ECh. 25 - Prob. 32ECh. 25 - Prob. 33ECh. 25 - Prob. 34ECh. 25 - Prob. 35ECh. 25 - Prob. 36ECh. 25 - Prob. 37ECh. 25 - Prob. 38ECh. 25 - Prob. 39ECh. 25 - Prob. 40ECh. 25 - Prob. 41ECh. 25 - Prob. 42ECh. 25 - Prob. 43ECh. 25 - Prob. 44ECh. 25 - Prob. 45ECh. 25 - Prob. 46ECh. 25 - Prob. 47ECh. 25 - Prob. 48ECh. 25 - Prob. 49ECh. 25 - Prob. 50ECh. 25 - Prob. 51ECh. 25 - Prob. 52ECh. 25 - Prob. 53ECh. 25 - Prob. 54ECh. 25 - Prob. 55ECh. 25 - Prob. 56ECh. 25 - Prob. 57IAECh. 25 - Prob. 58IAECh. 25 - Prob. 59IAECh. 25 - Prob. 60IAECh. 25 - Prob. 61IAECh. 25 - Prob. 62IAECh. 25 - Prob. 63IAECh. 25 - Prob. 64IAECh. 25 - Prob. 65IAECh. 25 - Prob. 66IAECh. 25 - Prob. 67IAECh. 25 - Prob. 68IAECh. 25 - Prob. 69IAECh. 25 - Prob. 70IAECh. 25 - Prob. 71IAECh. 25 - Prob. 72FPCh. 25 - Prob. 73FPCh. 25 - Radioactive decay and mass spectrometry are often...Ch. 25 - Prob. 75SAECh. 25 - Prob. 76SAECh. 25 - Prob. 77SAECh. 25 - Prob. 78SAECh. 25 - Prob. 79SAECh. 25 - Prob. 80SAECh. 25 - Prob. 81SAECh. 25 - Prob. 82SAECh. 25 - Prob. 83SAECh. 25 - Prob. 84SAECh. 25 - Prob. 85SAECh. 25 - Prob. 86SAECh. 25 - Prob. 87SAECh. 25 - Prob. 88SAECh. 25 - Prob. 89SAECh. 25 - Prob. 90SAECh. 25 - Prob. 91SAECh. 25 - Prob. 92SAECh. 25 - Prob. 93SAE
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- 2.86 For some uses, the relative abundance of isotopes must be manipulated. For example, a medical technique called boron neutron capture therapy needs a higher fraction of 10B than occurs naturally to achieve its best efficiency. What would happen to the atomic weight of a sample of boron that had been enriched in 10B? Explain your answer in terms of the concept of a weighted average.arrow_forwardBalance the following equations by filling in the blanks. (a) 92235U+01n54137_+201n+_ (b) 90232Th+612__01n+96240Cm (c) 24He+4296Mo43100_+_ (d) _+12H84210_+01narrow_forward2.10 Which isotope in each pair contains more neutrons? (A) 35Cl or 33S, (b) 19F or 19Ne, (c) 63Cu or 65Zn, (d) 126I or 127Tearrow_forward
- Who discovered the nucleus? Describe the experiment that led to this discovery.arrow_forwardWhich of the following is not a fundamental particle?(a) proton; (b) neutron; (c) beta particle; (d) alphaparticle; (e) all are fundamental particlesarrow_forwardAn isotope with atomic number 64 and mass number 158 is found to have a mass ratio relative to that of carbon-12 of 13.16034. What is the isotope, what is its atomic mass in u, and what is its mass relative to oxygen-16?arrow_forward
- 6. Which of the following nuclides have magic numbers of both protons and neutrons: (a) helium-4, (b) oxygen-18, (c) calcium-40, (d) zinc-66, (e) lead-208?arrow_forwardElement Atomic Number: 1 Name: Hydrogen Symbol: H Atomic Number 1 O'H O2H 25 50 75 Atomic Number An atom can be thought of as being formed from a number of combined 'H atoms with additional neutrons in the nucleus. The mass of an atom is less than that of the combined masses of the nuclear particles from which it is formed. This "mass loss" is an indication of the stablity of the atom's nucleus. In order to compare different atoms, the relative mass loss (in g/mol) is defined as: [(number protons x mass of 'H)+(number of neutrons x mass of n)] - atomic mass number of protons + number of neutrons The atom's binding energy (the energy associated with holding the nucleus together) can be calculated as: relative mass loss (kg/mol) x (2.998 x 10°m/s) The resulting units are joules/mole. Because calculating the relative mass loss involves dividing by the total number of nucleons (protons + neutrons), the binding energy is called the 'binding energy per nucleon.' (Previous Next) Relative…arrow_forwardYou are exploring the universe in your spaceship, and you land on a planet that is very similar to Earth. You encounter humanoid life forms that are comprised of molecules containing many carbon atoms (just like humans on Earth). And just like here on Earth, there are three isotopes of carbon: 12C, 13C, and 14C. However, on this new planet that you have discovered, the average isotopic mass of carbon is 13.101 amu. What can you conclude about this planet that you have discovered? Mark any/all that apply. Of the three isotopes of carbon, 14C has the greatest percent abundance. Half a mole of methane (CH4) on this new planet has a greater mass than half a mole of methane (CH4) on Earth. Of the three isotopes of carbon, 12C has the greatest percent abundance. Half a mole of methane (CH4) on this new planet has a lower mass than half a mole of methane (CH4) on Earth. Of the three isotopes of carbon, 13C has the greatest percent abundance.arrow_forward
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