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Chapter 6: Problem 30

Write the ground state electron configuration for (a) \(\mathrm{B}\) (b) \(\mathrm{Ba}\) (c) \(\mathrm{Be}\) (d) \(\mathrm{Bi}\) (e) \(\mathrm{Br}\)

Short Answer

Expert verified
Answer: The ground state electron configurations for the given elements are as follows: - Boron (B): 1s虏 2s虏 2p鹿 - Barium (Ba): 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦� 4p鈦� 5s虏 4d鹿鈦� 5p鈦� 6s虏 - Beryllium (Be): 1s虏 2s虏 - Bismuth (Bi): 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦� 4p鈦� 5s虏 4d鹿鈦� 5p鈦� 6s虏 4f鹿鈦� 5d鹿鈦� 5f鹿鈦� 6p鲁 - Bromine (Br): 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦� 4p鈦�

Step by step solution

01

Find the atomic number of Boron

Using the periodic table, we can see that the atomic number of Boron is 5. This means that Boron has 5 electrons in its ground state.
02

Determine the electron configuration using the Aufbau Principle

Following the Aufbau Principle, we fill the subshells in order of increasing energy. The electron configuration for Boron with 5 electrons is: 1s虏 2s虏 2p鹿 #b) Barium (Ba)#
03

Find the atomic number of Barium

Using the periodic table, we can see that the atomic number of Barium is 56. This means that Barium has 56 electrons in its ground state.
04

Determine the electron configuration using the Aufbau Principle

Following the Aufbau Principle, we fill the subshells in order of increasing energy. The electron configuration for Barium with 56 electrons is: 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦� 4p鈦� 5s虏 4d鹿鈦� 5p鈦� 6s虏 #c) Beryllium (Be)#
05

Find the atomic number of Beryllium

Using the periodic table, we can see that the atomic number of Beryllium is 4. This means that Beryllium has 4 electrons in its ground state.
06

Determine the electron configuration using the Aufbau Principle

Following the Aufbau Principle, we fill the subshells in order of increasing energy. The electron configuration for Beryllium with 4 electrons is: 1s虏 2s虏 #d) Bismuth (Bi)#
07

Find the atomic number of Bismuth

Using the periodic table, we can see that the atomic number of Bismuth is 83. This means that Bismuth has 83 electrons in its ground state.
08

Determine the electron configuration using the Aufbau Principle

Following the Aufbau Principle, we fill the subshells in order of increasing energy. The electron configuration for Bismuth with 83 electrons is: 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦� 4p鈦� 5s虏 4d鹿鈦� 5p鈦� 6s虏 4f鹿鈦� 5d鹿鈦� 5f鹿鈦� 6p鲁 #e) Bromine (Br)#
09

Find the atomic number of Bromine

Using the periodic table, we can see that the atomic number of Bromine is 35. This means that Bromine has 35 electrons in its ground state.
10

Determine the electron configuration using the Aufbau Principle

Following the Aufbau Principle, we fill the subshells in order of increasing energy. The electron configuration for Bromine with 35 electrons is: 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦� 4p鈦�

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Atomic Number
The atomic number of an element is a fundamental property that tells us the number of protons in an atom's nucleus. It also indicates the number of electrons in a neutral atom. This is crucial because electrons determine how an atom will interact (or bond) with others. Each element on the periodic table has a unique atomic number.
For example:
  • Boron (B) has an atomic number of 5, meaning it has 5 protons and, in its neutral state, 5 electrons.
  • Barium (Ba) has an atomic number of 56.
  • Beryllium (Be) is 4.
  • Bismuth (Bi) is 83.
  • Bromine (Br) is 35.

Knowing the atomic number, we can proceed to determine the electron configurations for these elements using additional principles like the Aufbau principle.
Aufbau Principle
The Aufbau Principle is a fundamental guide for determining the electron configuration of an atom. It states that electrons occupy orbitals starting from the lowest energy level to the highest. Simply put, you fill up the lower energy levels first before moving to higher ones. This is similar to filling seats in a theater from the front row to the back.
For example:
  • Boron with 5 electrons would fill electrons like this: start in the 1s orbital, move to 2s, and then the rest in 2p: 1s虏 2s虏 2p鹿.
  • Beryllium with 4 electrons has 1s虏 2s虏 as its configuration, finishing as soon as the 2s orbital is filled.
The principle helps in building the electron configuration systematically and remains consistent across different elements in the periodic table.
Ground State
The ground state of an atom is its most stable and lowest energy state. In this state, all the electrons are arranged in the lowest possible energy levels, according to the Aufbau Principle. This is the natural configuration for an atom, meaning they are not excited by external energy sources.
  • Electrons will always try to return to the ground state if they have been excited to higher energy levels.
  • Only when an atom is given energy, typically as heat or light, do its electrons move to an excited state.

The electron configurations mentioned earlier are for atoms in their ground state. When studying chemistry, and particularly electron configurations, the ground state is the typical reference point. This stability is important for predicting chemical behavior and reactivity.
Periodic Table
The periodic table is a systematic arrangement of elements based on increasing atomic number and their chemical properties. It groups elements into rows called periods and columns called groups or families, where elements share similar properties and electron configurations.
  • The table helps us easily find an element like Boron (B) and provides its atomic number, essential for determining its electron configuration.
  • It showcases trends in element properties, such as electronegativity and atomic size, which can influence how elements form bonds.

The periodic table is an invaluable tool for chemists, allowing them to predict and explain the chemical behavior of elements. By referencing the table, we can determine facts such as which orbitals will be filled first according to the Aufbau Principle and confirm our electron configurations.

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Most popular questions from this chapter

For the following pairs of orbitals, indicate which is lower in energy in a many-electron atom. (a) \(3 \mathrm{~d}\) or \(4 \mathrm{~s}\) (b) \(4 \mathrm{f}\) or \(3 \mathrm{~d}\) (c) \(2 \mathrm{~s}\) or \(2 \mathrm{p}\) (d) \(4 \mathrm{f}\) or \(4 \mathrm{~d}\)

Write the symbol of each element described below. (a) largest atomic radius in Group 17 (b) smallest atomic radius in period 3 (c) largest first ionization energy in Group 2 (d) most electronegative in Group 16 (e) element(s) in period 2 with no unpaired p electron (f) abbreviated electron configuration is \([\mathrm{Ar}] 4 \mathrm{~s}^{2} 3 \mathrm{~d}^{3}\) (g) A \(+2\) ion with abbreviated electron configuration [Ar] \(3 \mathrm{~d}^{5}\) (h) A transition metal in period 4 forming \(\mathrm{a}+2\) ion with no unpaired electrons

Which of the following electron configurations are for atoms in the ground state? In the excited state? Which are impossible? (a) \(1 s^{2} 2 s^{2} 2 p^{1}\) (b) \(1 s^{2} 1 p^{1} 2 s^{1}\) (c) \(1 s^{2} 2 s^{2} 2 p^{3} 3 s^{1}\) (d) \(1 s^{2} 2 s^{2} 2 p^{6} 3 d^{10}\) (e) \(1 s^{2} 2 s^{2} 2 p^{5} 3 s^{1}\)

Given the following sets of electron quantum numbers, indicate those that could not occur, and explain your answer. (a) \(1,0,0,-\frac{1}{2}\) (b) \(1,1,0,+\frac{1}{2}\) (c) \(3,2,-2,+\frac{1}{2}\) (d) \(2,1,2,+\frac{1}{2}\) (e) \(4,0,2,+\frac{1}{2}\)

For the following pairs of orbitals, indicate which is higher in energy in a many-electron atom. (a) \(3 \mathrm{~s}\) or \(2 \mathrm{p}\) (b) 4 s or \(4 \mathrm{~d}\) (c) \(4 \mathrm{f}\) or \(6 \mathrm{~s}\) (d) 1 s or \(2 \mathrm{~s}\)
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