Chapter 6: Problem 96
Write the ground-state electron configurations for the following elements: \(\mathrm{B}, \mathrm{V}, \mathrm{C}, \mathrm{As}, \mathrm{I}, \mathrm{Au} .\)
Short Answer
Expert verified
B: 1s² 2s² 2p¹; V: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d³; C: 1s² 2s² 2p²; As: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p³; I: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁵; Au: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶ 6s¹ 4f¹⁴ 5d¹⁰.
Step by step solution
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Aufbau principle
The Aufbau principle is an essential rule when understanding how electrons fill the atomic orbitals of an element. The principle dictates that electrons occupy the lowest energy level orbitals available. Essentially, they build "upwards," step by step, starting from the lowest energy state available. It helps determine the order of electron filling by defining a sequence that leads to the correct distribution of electrons in an atom.
According to this principle, the order starts from 1s, then moves to 2s, followed by 2p, 3s, and so forth. The reason the order is not strictly sequential (i.e., 1s directly to 2s, etc.) is due to varying energy levels associated with different orbitals. For instance, 4s is lower in energy and thus fills before 3d.
Understanding the Aufbau principle is crucial as it forms the backbone for writing electron configurations, providing a structured approach to filling orbitals.
According to this principle, the order starts from 1s, then moves to 2s, followed by 2p, 3s, and so forth. The reason the order is not strictly sequential (i.e., 1s directly to 2s, etc.) is due to varying energy levels associated with different orbitals. For instance, 4s is lower in energy and thus fills before 3d.
Understanding the Aufbau principle is crucial as it forms the backbone for writing electron configurations, providing a structured approach to filling orbitals.
periodic table
The periodic table is more than a mere arrangement of elements; it is an incredible tool that provides valuable insights into an element's properties, including its electron configuration. Elements are arranged based on increasing atomic number, which corresponds to the number of protons in an atom's nucleus, but interestingly, it also aligns with electron distributions.
The horizontal rows in the periodic table are called periods and represent the number of electron shells an atom possesses. Meanwhile, the vertical columns are known as groups or families and share similar outer electron configurations resulting in similar chemical properties.
The position of an element in the table correlates with its electron configuration, highlighting which orbitals are filled as you move across a period or down a group, thus aiding in prediction of an element’s chemical behavior.
The horizontal rows in the periodic table are called periods and represent the number of electron shells an atom possesses. Meanwhile, the vertical columns are known as groups or families and share similar outer electron configurations resulting in similar chemical properties.
The position of an element in the table correlates with its electron configuration, highlighting which orbitals are filled as you move across a period or down a group, thus aiding in prediction of an element’s chemical behavior.
electron distribution
Electron distribution, or electron configuration, refers to how electrons are arranged within an atom's atomic orbitals. This distribution is fundamentally crucial as it determines how an element will chemically interact with others. Electrons are found in energy levels or shells, each consisting of one or more subshells or orbitals (like s, p, d, f).
The distribution follows a specific pattern guided by rules like the Aufbau principle, the Pauli Exclusion Principle, and Hund's Rule, each contributing to the final electron configuration of an element. For example, the electron configuration for Boron (B) is written as 1s² 2s² 2p¹, representing the completed filling of the s-orbitals and partial filling of the p-orbital, up to the total electron count.
Knowing how electrons are distributed in atomic orbitals helps predict physical and chemical properties of elements, including bonding, magnetism, and reactivity.
The distribution follows a specific pattern guided by rules like the Aufbau principle, the Pauli Exclusion Principle, and Hund's Rule, each contributing to the final electron configuration of an element. For example, the electron configuration for Boron (B) is written as 1s² 2s² 2p¹, representing the completed filling of the s-orbitals and partial filling of the p-orbital, up to the total electron count.
Knowing how electrons are distributed in atomic orbitals helps predict physical and chemical properties of elements, including bonding, magnetism, and reactivity.
atomic orbitals
Atomic orbitals are regions within an atom where electrons are most likely to be found. Each orbital type (s, p, d, f) has a different shape and energy level, contributing to the overall electron configuration of an element.
The simplest atomic orbital is the s-orbital; it is spherical and can hold a maximum of two electrons. Moving to more complex orbitals, the p-orbitals have a dumbbell shape and can accommodate up to six electrons across three orientations (px, py, pz).
Further complexity arises with d and f orbitals, which can hold 10 and 14 electrons respectively. These orbitals are crucial for transition metals and inner transition metals, influencing properties like color and conductivity.
Understanding the nature of atomic orbitals is vital for chemists as it helps explain and predict the behavior of atoms during chemical reactions and bonding processes, thereby playing a significant role in the study of chemistry.
The simplest atomic orbital is the s-orbital; it is spherical and can hold a maximum of two electrons. Moving to more complex orbitals, the p-orbitals have a dumbbell shape and can accommodate up to six electrons across three orientations (px, py, pz).
Further complexity arises with d and f orbitals, which can hold 10 and 14 electrons respectively. These orbitals are crucial for transition metals and inner transition metals, influencing properties like color and conductivity.
Understanding the nature of atomic orbitals is vital for chemists as it helps explain and predict the behavior of atoms during chemical reactions and bonding processes, thereby playing a significant role in the study of chemistry.
