Textbook Question
(d) If you remove a single electron from a P atom, which orbital will it come from?
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Ch.7 - Periodic Properties of the Elements
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not 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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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
(b) Repeat these calculations using Slater’s rules.
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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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