The following electron configurations represent excited states. Identify the element and write its ground-state condensed electron configuration. (b) 3Ne43s13p44p1.

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Identify the atomic number of the element by summing the total number of electrons in the given excited state configuration. In this case, count the electrons in each orbital: 2 electrons in each of the first three 2p orbitals, 1 electron in the fourth 2p orbital, 2 electrons in the 3s orbital, 3 electrons in the 3p orbitals, and 1 electron in the 4p orbital.

Determine the element by matching the total number of electrons to the atomic number on the periodic table. The sum of the electrons will give you the atomic number of the element.

Understand that the ground state electron configuration is the lowest energy configuration and typically fills orbitals starting from the lowest energy level to higher, following the Aufbau principle, Hund's rule, and the Pauli exclusion principle.

Write the ground-state electron configuration for the element. Begin with the lowest energy orbitals and fill them according to the number of electrons up to the atomic number of the element, ensuring to fill the 1s, 2s, 2p, 3s, and 3p orbitals completely before moving to higher energy orbitals.

Condense the electron configuration by using noble gas notation for the core electrons (those electrons in the energy levels below the valence electrons) and then listing the valence electrons explicitly.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It is typically represented in a specific notation that indicates the energy levels and sublevels occupied by electrons. Understanding how to read and write electron configurations is essential for identifying the state of an atom, whether it is in a ground or excited state.

Excited State vs. Ground State

The ground state of an atom is its lowest energy configuration, where electrons occupy the lowest available energy levels. In contrast, an excited state occurs when one or more electrons have absorbed energy and moved to higher energy levels. Recognizing the difference between these states is crucial for determining the correct electron configuration of an element.

Condensed Electron Configuration

Condensed electron configuration is a shorthand notation that simplifies the representation of an atom's electron arrangement by using the nearest noble gas to represent core electrons. This method makes it easier to write and understand electron configurations, especially for larger elements, and is particularly useful when identifying the ground state of an element from its excited state configuration.

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Condensed Electron Configuration

Related Practice

Textbook Question

Identify the specific element that corresponds to each of the following electron configurations and indicate the number of unpaired electrons for each: (d) 3Kr45s24d105p4.

Textbook Question

(a) What does the term paramagnetism mean? (b) How can one determine experimentally whether a substance is paramagnetic? (c) Which of the following ions would you expect to be paramagnetic: O2+ , N22 -, Li2+ , O22 - ? For those ions that are paramagnetic, determine the number of unpaired electrons.

Textbook Question

The following do not represent valid ground-state electron configurations for an atom either because they violate the Pauli exclusion principle or because orbitals are not filled in order of increasing energy. Indicate which of these two principles is violated in each example. (a) [Ne]3s²3p⁶3d⁵ (b) [Xe]6s³ (c) 1s²3s¹.

Textbook Question

Consider the two waves shown here, which we will consider to represent two electromagnetic radiations: (a) What is the wavelength of wave A?

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Textbook Question

Consider the two waves shown here, which we will consider to represent two electromagnetic radiations: (b) What is the frequency of wave A?

Textbook Question

If a sample of calcium chloride is introduced into a nonluminous flame, the color of the flame turns to orange ('flame test'). The light is emitted because calcium atoms become excited; their return to the ground state results in light emission. (b) What is the energy of 1.00 mol of these photons (a mole of photons is called an Einstein)?

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