Domanda del libro di testo
According to the aufbau principle, which orbital is filled immediately after each of the following in a multielectron atom?
(a) 4s
(b) 3d
(c) 5f
(d) 5p
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Ch.5 - Periodicity & Electronic Structure of Atoms
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
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McMurry 8th EditionCh.5 - Periodicity & Electronic Structure of AtomsProblema 98
McMurry 8th EditionCh.5 - Periodicity & Electronic Structure of AtomsProblema 98Capitolo 5, Problema 98
Why does the number of elements in successive periods of the periodic table increase by the progression 2, 8, 18, 32?
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1. The periodic table is organized based on the electron configuration of atoms. The electron configuration of an atom is determined by the distribution of electrons in its atomic orbitals.
2. The atomic orbitals are grouped into different energy levels or shells, and each shell is divided into subshells. The first energy level has one subshell (s), the second and third levels have two subshells (s and p), the fourth and fifth levels have three subshells (s, p, and d), and the sixth and seventh levels have four subshells (s, p, d, and f).
3. The s subshell can hold up to 2 electrons, the p subshell can hold up to 6 electrons, the d subshell can hold up to 10 electrons, and the f subshell can hold up to 14 electrons.
4. The progression 2, 8, 18, 32 in the number of elements in successive periods of the periodic table corresponds to the maximum number of electrons that can be accommodated in the subshells of each energy level. The first period has one energy level (1s) that can hold 2 electrons. The second period has two energy levels (2s and 2p) that can hold 2 + 6 = 8 electrons. The third period has three energy levels (3s, 3p, and 3d) that can hold 2 + 6 + 10 = 18 electrons. The fourth period has four energy levels (4s, 4p, 4d, and 4f) that can hold 2 + 6 + 10 + 14 = 32 electrons.
5. Therefore, the number of elements in each period of the periodic table increases by the progression 2, 8, 18, 32 because this reflects the increasing capacity of the atomic orbitals to hold electrons as we move down the periods.
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Electron Shells and Energy Levels
Elements in the periodic table are arranged according to their electron configurations, which are organized into shells or energy levels. Each shell can hold a specific maximum number of electrons, determined by the formula 2n², where n is the principal quantum number. This structure explains why the first shell holds 2 electrons, the second holds 8, and so forth.
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00:46
Number of Electrons in Shells
Subshells and Orbital Types
Within each electron shell, there are subshells (s, p, d, f) that further define the distribution of electrons. As you move to higher energy levels, additional subshells become available, allowing for more electrons to occupy the shell. For example, the third shell includes s and p subshells (totaling 8) and the d subshell (adding 10), leading to a total of 18 electrons.
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02:06d Orbital Orientations
Periodic Trends and Grouping
The periodic table is structured in periods (rows) and groups (columns) that reflect similar chemical properties. The increase in the number of elements in successive periods (2, 8, 18, 32) corresponds to the filling of these electron shells and subshells, which influences the chemical behavior and reactivity of the elements. This systematic arrangement helps predict element properties based on their position in the table.
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01:55Periodic Trends