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Chapter 7: Problem 88

Use the Aufbau principle to obtain the ground-state electron configuration of technetium.

Short Answer

Expert verified
The ground-state electron configuration of Technetium is 1s\(^2\), 2s\(^2\), 2p\(^6\), 3s\(^2\), 3p\(^6\), 4s\(^2\), 3d\(^{10}\), 4p\(^6\), 5s\(^2\), 4d\(^5\).

Step by step solution

01

Understanding Technetium's Atomic Number

Technetium is the 43rd element on the Periodic table, so it has 43 electrons in its ground state.
02

Aufbau Principle Application

The Aufbau principle stipulates that lower energy orbitals are filled before higher energy orbitals. The order for filling is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, and 6d. Using this sequence, fill up the energy levels until there are no more electrons left.
03

Implementation For Technetium

Follow the order of the Aufbau principle until all 43 electrons are used up. The electron configuration becomes: 1s\(^2\), 2s\(^2\), 2p\(^6\), 3s\(^2\), 3p\(^6\), 4s\(^2\), 3d\(^{10}\), 4p\(^6\), 5s\(^2\), 4d\(^5\).

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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 a fundamental guideline for writing electron configurations in chemistry. It helps us understand the sequence in which atomic orbitals are filled with electrons.
This principle comes from the German word "Aufbau," meaning "building up" or "construction."
According to this concept, electrons occupy the lowest energy orbitals first before moving to higher ones.
  • Starting from the lowest energy level and moving step-by-step to higher ones is key.
  • The sequence used is based on increasing energy levels: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, etc.
  • This order helps to predict how electrons are arranged around an atom, which impacts an element's chemical properties.
For Technetium, with 43 electrons, we use the order from the Aufbau principle to compose its electron configuration. This process involves filling the orbitals systematically until we reach the total electron count of Technetium.
Technetium
Technetium is a unique element found in the middle of the periodic table. It is represented by the symbol Tc and has an atomic number of 43. This makes it a part of the transition metals group.
Transition metals are known for their versatility and ability to form various compounds.
Despite being widely used in scientific fields, technetium is not found naturally in the Earth's crust in large amounts. It is typically a byproduct of nuclear reactions.
  • Technetium is essential in several applications, especially in the medical field for imaging and diagnostic procedures.
  • Its electron configuration and unique properties come from its position in the periodic table.
  • The knowledge of its electron configuration helps scientists utilize technetium effectively in various fields.
For students, knowing Technetium's atomic structure helps tie together concepts of electron configuration and its practical impacts.
Atomic Number
The atomic number is an essential concept in chemistry representing the number of protons found in the nucleus of an atom of an element. This number is unique to each element and determines its identity on the periodic table.
For example, Technetium has the atomic number 43, meaning it has 43 protons. This directly correlates to the number of electrons in a neutral atom, helping to establish its electron configuration.
  • Atomic number increases progressively as you move through the periodic table.
  • It helps with the determination of electron configuration, defining how electrons fill available orbitals.
  • Atomic number is used to predict chemical properties and reactivity.
Understanding the atomic number offers a clear pathway to comprehending more about how elements behave and interact chemically, solidifying the building blocks of chemistry knowledge.

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Most popular questions from this chapter

Indicate the number of unpaired electrons present in each of the following atoms: \(\mathrm{B}, \mathrm{Ne}, \mathrm{P}, \mathrm{Sc}, \mathrm{Mn}, \mathrm{Se}\) \(\mathrm{Kr}, \mathrm{Fe}, \mathrm{Cd}, \mathrm{I}, \mathrm{Pb}\)

The radioactive \(\mathrm{Co}-60\) isotope is used in nuclear medicine to treat certain types of cancer. Calculate the wavelength and frequency of an emitted gamma photon having the energy of \(1.29 \times 10^{11} \mathrm{~J} / \mathrm{mol} .\)

In 1996 physicists created an anti-atom of hydrogen. In such an atom, which is the antimatter equivalent of an ordinary atom, the electrical charges of all the component particles are reversed. Thus, the nucleus of an anti-atom is made of an anti-proton, which has the same mass as a proton but bears a negative charge, while the electron is replaced by an anti-electron (also called positron) with the same mass as an electron, but bearing a positive charge. Would you expect the energy levels, emission spectra, and atomic orbitals of an antihydrogen atom to be different from those of a hydrogen atom? What would happen if an anti-atom of hydrogen collided with a hydrogen atom?

An electron in an atom is in the \(n=3\) quantum level. List the possible values of \(\ell\) and \(m_{\ell}\) that it can have.

What is the difference between a \(2 p_{x}\) and a \(2 p_{y}\) orbital?
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