Textbook Question
The natural abundance of 3He is 0.000137%. (b) Based on the sum of the masses of their subatomic particles, which is expected to be more massive, an atom of 3He or an atom of 3H (which is also called tritium)?
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Ch.2 - Atoms, Molecules, and Ions
Chapter 2, Problem 95b,c,d
Identify the element represented by each of the following symbols and give the number of protons and neutrons in each: (b) 12753X (c) 8636X (d) 6730X
Verified step by step guidance1
Step 1: The atomic number (the subscript) represents the number of protons in an atom. In this case, the atomic number is 53, which corresponds to the element Iodine (I) in the periodic table.
Step 2: The atomic mass number (the superscript) represents the total number of protons and neutrons in an atom. In this case, the atomic mass number is 127.
Step 3: To find the number of neutrons, subtract the atomic number (number of protons) from the atomic mass number. So, the number of neutrons is 127 - 53.
Step 4: Therefore, the element represented by the symbol 12753X is Iodine (I), with 53 protons and 74 neutrons.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Atomic Number
The atomic number of an element is the number of protons found in the nucleus of an atom. It uniquely identifies an element and determines its position on the periodic table. In the notation <sup>127</sup><sub>53</sub>X, the subscript '53' indicates that the element has 53 protons.
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02:10
Atom Structure
Mass Number
The mass number of an atom is the total number of protons and neutrons in its nucleus. It is represented by the superscript in the notation <sup>127</sup><sub>53</sub>X, where '127' signifies the combined total of protons and neutrons. To find the number of neutrons, subtract the atomic number from the mass number.
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02:19Atomic Mass
Element Identification
Each element is defined by its unique atomic number, which corresponds to its chemical properties. By knowing the atomic number (53 in this case), one can identify the element as iodine (I). Understanding the relationship between atomic number, mass number, and elemental identity is crucial for interpreting chemical symbols.
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01:15Chalcogen Identification Example
Related Practice
Textbook Question
The natural abundance of 3He is 0.000137%. (c) Based on your answer to part (b), what would need to be the precision of a mass spectrometer that is able to differentiate between peaks that are due to 3He+ and 3H+?
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Textbook Question
Identify the element represented by each of the following symbols and give the number of protons and neutrons in each: (a) 7433X
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Textbook Question
The nucleus of 6Li is a powerful absorber of neutrons. It exists in the naturally occurring metal to the extent of 7.5%. In the era of nuclear deterrence, large quantities of lithium were processed to remove 6Li for use in hydrogen bomb production. The lithium metal remaining after removal of 6Li was sold on the market. (b) The atomic masses of 6Li and 7Li are 6.015122 and 7.016004 u, respectively. A sample of lithium depleted in the lighter isotope was found on analysis to contain 1.442% 6Li. What is the average atomic weight of this sample of the metal?
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Textbook Question
The element oxygen has three naturally occurring isotopes, with 8, 9, and 10 neutrons in the nucleus, respectively. a. Write the full chemical symbols for these three isotopes.
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Textbook Question
The element lead (Pb) consists of four naturally occurring isotopes with atomic masses 203.97302, 205.97444, 206.97587, and 207.97663 amu. The relative abundances of these four isotopes are 1.4, 24.1, 22.1, and 52.4%, respectively. From these data, calculate the atomic weight of lead.
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