Textbook Question
(b) Repeat these calculations using Slater’s rules.
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Ch.7 - Periodic Properties of the Elements
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 7, Problem 79
Consider the stable elements through lead (Z = 82). In how many instances are the atomic weights of the elements out of order relative to the atomic numbers of the elements?
Verified step by step guidance1
Identify the atomic weights and atomic numbers of all stable elements up to lead (Z = 82).
Arrange the elements in order of increasing atomic number and note their corresponding atomic weights.
Compare the atomic weights of each element with those of the elements immediately preceding and succeeding it in the list.
Count the number of instances where an element has a higher atomic number but a lower atomic weight than the element that follows it.
Summarize the total number of such instances to find the answer.
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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 its atoms, which determines the element's identity and its position in the periodic table. Elements are arranged in order of increasing atomic number, which reflects their increasing positive charge and the number of electrons in a neutral atom.
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Atom Structure
Atomic Weight
Atomic weight, or atomic mass, is the weighted average mass of an element's isotopes, measured in atomic mass units (amu). It reflects the mass of an atom relative to the mass of carbon-12 and can vary due to the presence of isotopes, which are atoms of the same element with different numbers of neutrons.
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Periodic Trends
Periodic trends refer to the patterns observed in the properties of elements as one moves across or down the periodic table. These trends include variations in atomic size, ionization energy, and electronegativity, and they can also affect the relationship between atomic number and atomic weight, leading to instances where atomic weights do not increase consistently with atomic numbers.
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Related Practice
Textbook Question
(c) Detailed calculations indicate that the effective nuclear charge is 5.6+ for the 3s electrons and 4.9+ for the 3p electrons. Why are the values for the 3s and 3p electrons different?
Textbook Question
Write a balanced equation for the reaction that occurs in each of the following cases: (a) White phorphrous, P4(s), reacts with chlorine gas. (b) Sodium metal reacts with water. (c) Sulfur reacts with hydrogen gas.
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Textbook Question
Figure 7.4 shows the radial probability distribution functions for the 2s orbitals and 2p orbitals. (a) Which orbital, 2s or 2p, has more electron density close to the nucleus?
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Textbook Question
Write a balanced equation for the reaction that occurs in each of the following cases: (d) Fluorine reacts with water.
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