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
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 81c
(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?
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Understand the concept of effective nuclear charge (Z_eff), which is the net positive charge experienced by an electron in a multi-electron atom. It accounts for the shielding effect caused by other electrons.
Recognize that electrons in different orbitals experience different levels of shielding. The 3s and 3p orbitals have different shapes and distances from the nucleus, affecting their shielding and Z_eff.
Note that 3s electrons are closer to the nucleus and penetrate the inner electron shells more effectively than 3p electrons. This means 3s electrons experience less shielding and a higher Z_eff.
Understand that 3p electrons are further from the nucleus and are more shielded by inner electrons compared to 3s electrons, resulting in a lower Z_eff.
Conclude that the difference in Z_eff values for 3s and 3p electrons is due to their different orbital shapes and penetration levels, affecting the extent of shielding they experience.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Effective Nuclear Charge (Z_eff)
Effective nuclear charge (Z_eff) is the net positive charge experienced by an electron in a multi-electron atom. It accounts for the actual nuclear charge (the number of protons) minus the shielding effect of other electrons. This concept is crucial for understanding how electrons are held in an atom and why different types of electrons (like 3s and 3p) experience different levels of attraction to the nucleus.
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Effective Nuclear Charge
Electron Shielding
Electron shielding occurs when inner-shell electrons repel outer-shell electrons, reducing the effective nuclear charge felt by those outer electrons. This phenomenon explains why electrons in different subshells (like 3s and 3p) can experience different effective nuclear charges, as the spatial distribution and energy levels of these electrons influence how much they are shielded from the nucleus.
Subshell Energy Levels
Subshell energy levels refer to the different energy states of electrons within an atom, categorized into s, p, d, and f orbitals. The 3s and 3p subshells have different shapes and orientations, leading to variations in their energy and the extent to which they are shielded by other electrons. This difference in energy levels contributes to the distinct effective nuclear charges experienced by 3s and 3p electrons.
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Related Practice
Textbook Question
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?
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Textbook Question
(b) Repeat these calculations using Slater’s rules.
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Textbook Question
In Table 7.8, the bonding atomic radius of neon is listed as58 pm, whereas that for xenon is listed as 140 pm. A classmateof yours states that the value for Xe is more realisticthan the one for Ne. Is she correct? If so, what is the basisfor her statement?
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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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