Textbook Question
The element argon has three naturally occurring isotopes, with 18, 20, and 22 neutrons in the nucleus, respectively. (a) Write the full chemical symbols for these three isotopes.
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Ch.2 - Atoms, Molecules, and Ions
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 2, Problem 92a
Identify the element represented by each of the following symbols and give the number of protons and neutrons in each: (a) 7433X
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 33, which corresponds to the element Arsenic (As) 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 74.
Step 3: To find the number of neutrons, subtract the atomic number (number of protons) from the atomic mass number. In this case, 74 (atomic mass number) - 33 (atomic number) = 41.
Step 4: Therefore, the element represented by the symbol 7433X is Arsenic (As), which has 33 protons and 41 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>74</sup><sub>33</sub>X, the subscript '33' represents the atomic number, indicating that the element has 33 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>74</sup><sub>33</sub>X, where '74' is the mass number. To find the number of neutrons, subtract the atomic number from the mass number: neutrons = mass number - atomic number.
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Isotopes
Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons. This results in different mass numbers for the isotopes of the same element. In the case of <sup>74</sup><sub>33</sub>X, knowing the mass number allows us to identify the specific isotope of the element with atomic number 33, which is arsenic.
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Related Practice
Textbook Question
(b) Using the mass of the proton from Table 2.1 and assuming its diameter is 1.0 * 10-15 m, calculate the density of a proton in g>cm3.
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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 diameter of a rubidium atom is 495 pm We will consider two different ways of placing the atoms on a surface. In arrangement A, all the atoms are lined up with one another to form a square grid. Arrangement B is called a close-packed arrangement because the atoms sit in the 'depressions' formed by the previous row of atoms:
(c) By what factor has the number of atoms on the surface increased in going to arrangement B from arrangement A?
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Textbook Question
(a) Assuming the dimensions of the nucleus and atom shown in Figure 2.10, what fraction of the volume of the atom is taken up by the nucleus?
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Textbook Question
The element chromium (Cr) consists of four naturally occurring isotopes with atomic masses 49.9460, 51.9405, 52.9407, and 53.9389 u. The relative abundances of these four isotopes are 4.3, 83.8, 9.5, and 2.4%, respectively. From these data, calculate the atomic weight of chromium.
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