CHEMISTRY:MOLECULAR NATURE (LL)W/ACCESS
7th Edition
ISBN: 9781119497325
Author: JESPERSEN
Publisher: WILEY
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Textbook Question
Chapter 0, Problem 9RQ
What elements were formed (a) during the first moments of the big-bang, (b) in red giant stars, and (c) during a supernova?
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Consider the nuclide cobalt-59 (5927Co).
(a)
The mass of 5927Co in atomic mass units is 58.933200 u. (Note this is the mass of the entire atom, not just the nucleus.) This mass is lower than the total mass of its constituent protons, neutrons, and electrons.
Find the difference, in atomic mass units, between the total mass of the constituent particles, and the actual mass of the nuclide. (This is sometimes called the "mass defect.") The mass of a proton is 1.007276 u, the mass of a neutron is 1.008665 u, and the mass of an electron is 5.486 ✕ 10−4 u. (Round your answer to at least four decimal places.)
b) Since, according to special relativity theory, mass and energy are "equivalent," the mass defect, or "missing" mass found in part (a), is measurement of the energy it would take to break the bound 5927Co atom into its constituent particles. In other words, it is equivalent to the binding energy.
Using the result of part (a), find the binding energy per nucleon, Eb/A for 5927Co in…
Element
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
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Relative…
A small fraction of all the carbon in living things is radioactive.
True or false
Chapter 0 Solutions
CHEMISTRY:MOLECULAR NATURE (LL)W/ACCESS
Ch. 0 - Practice Exercise 0.1
Using the chapter titles...Ch. 0 - Prob. 2PECh. 0 - Prob. 3PECh. 0 - Prob. 4PECh. 0 - Prob. 5PECh. 0 - Prob. 6PECh. 0 - Prob. 7PECh. 0 - Prob. 8PECh. 0 - Prob. 9PECh. 0 - Practice Exercise 0.10 Aluminum atoms have a mass...
Ch. 0 - Practice Exercise 0.11 How much heavier is the...Ch. 0 - Practice Exercise 0.12 The definition of the size...Ch. 0 - Practice Exercise 0.13 Naturally occurring boron...Ch. 0 - Practice Exercise 0.14
Neon, the gas used in neon...Ch. 0 - Prob. 1RQCh. 0 - 0.2 Knowing what we know today, which of the...Ch. 0 - 0.3 In what ways does the atomic theory affect the...Ch. 0 - Shake a few crystals of salt into your hand and...Ch. 0 - Are there any examples of crystals in nature that...Ch. 0 - 0.6 Heat is one form of energy. If a reaction...Ch. 0 - Can you think of a chemical reaction that starts...Ch. 0 - 0.8 Some large biological molecules rely on...Ch. 0 - 0.9 What elements were formed (a) during the first...Ch. 0 - Prob. 10RQCh. 0 - 0.11 What is the predominant element in the solar...Ch. 0 - Prob. 12RQCh. 0 - What physical factors caused elements and minerals...Ch. 0 - Is this separation still occurring on the earth?Ch. 0 - 0.15 What measuring devices did early chemists...Ch. 0 - 0.16 In your own words, describe how Daltons...Ch. 0 - Which of the laws of chemical combination is used...Ch. 0 - Prob. 18RQCh. 0 - Where in an atom is nearly all of its mass...Ch. 0 - What is a nucleon? Which ones have we studied?Ch. 0 - 0.21 How was the charge-to-mass ratio of the...Ch. 0 - 0.22 How did Robert Millikan determine the charge...Ch. 0 - How was the proton discovered?Ch. 0 - What experiment did Rutherford carry out to...Ch. 0 - Why dont we count the electrons when determining...Ch. 0 - Define the terms atomic number and mass number....Ch. 0 - Prob. 27RQCh. 0 - Write the symbols of the isotopes that contain the...Ch. 0 - What is wrong with the following statement? The...Ch. 0 - 0.30 The atomic number of silver, Ag, is 47 and it...Ch. 0 - A certain element X forms a compound with oxygen...Ch. 0 - Nitrogen reacts with a metal to form a compound in...Ch. 0 - Give the numbers of neutrons, protons, and...Ch. 0 - 0.34 Give the numbers of electrons, protons, and...Ch. 0 - Iodine-131 is used to treat overactive thyroids;...Ch. 0 - Prob. 36RQCh. 0 - 0.37 One chemical substance in natural gas is a...Ch. 0 - 0.38 Carbon tetrachloride contains one carbon and...Ch. 0 - If an atom of carbon-12 had been assigned a...Ch. 0 - 0.40 One atom of has a mass that is 9.0754 times...Ch. 0 - Naturally occurring copper is composed of 69.17%...Ch. 0 - Naturally occurring magnesium (one of the elements...Ch. 0 - N2O is often called nitrous oxide or laughing gas,...Ch. 0 - An element has 24 protons in its nucleus. (a)...Ch. 0 - Iron is composed of four isotopes with the...Ch. 0 - 0.46 What color are the protons, neutrons, and...Ch. 0 - 0.47 Immediately after the big bang, helium and...Ch. 0 - Prob. 48RQCh. 0 - Scientists often validate measurements, such as...Ch. 0 - Sir James Chadwick, discovered the neutron. The...
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Who discovered the nucleus? Describe the experiment that led to this discovery.arrow_forwardThe atomic masses of hydrogen-2 (deuterium), helium-4, and lithium-6 are 2.014102 amu, 4.002602 amu, and 6.0151228 amu, respectively. For each isotope, calculate (a) the nuclear mass,arrow_forwardDetermine the number of protons and neutrons in uranium-235. Enter your answers numerically separated by a comma.arrow_forward
- You 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_forwardThe decay series of uranium- 238 includes 3 different isotopes of polonium. Which of these isotopes you would expect to find with the greatest abundance in a sample pitchblende?arrow_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
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