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Chapter 4: Problem 8

Distinguish between the ground state and an excited state of an atom.

Short Answer

Expert verified
The ground state is the lowest energy state of an atom, while an excited state is any energy state higher than the ground state.

Step by step solution

01

Define Ground State

The ground state of an atom is its lowest energy state. In this state, the electrons occupy the closest possible orbitals to the nucleus according to the Pauli exclusion principle and Hund's rule.
02

Define Excited State

An excited state of an atom is any state with energy higher than the ground state. In this condition, one or more electrons have absorbed energy and moved to higher energy orbitals.
03

Compare Energy Levels

In the ground state, the atom is at its minimum energy level. In an excited state, the atom has absorbed energy and is at a higher energy level than the ground state.
04

Understand Transition Between States

Atoms can transition from the ground state to an excited state by absorbing energy (e.g., from photons). They can return to the ground state by releasing this energy, often as light.
05

Real-world Example

Consider the hydrogen atom: When its electron is in the lowest energy orbital (n=1), the atom is in the ground state. If the electron absorbs energy and jumps to a higher orbital (n=2, n=3, etc.), the atom is in an excited state.

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Key Concepts

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

headline of the respective core concept
Atoms are made up of a nucleus surrounded by electrons. These electrons occupy specific energy levels or orbitals. The ground state of an atom is its lowest energy configuration, where the electrons lie in the closest possible orbitals to the nucleus. The Pauli exclusion principle states that no two electrons can have the same set of quantum numbers in an atom, and Hund's rule asserts that electrons must fill each orbital in a sublevel singly before pairing.
headline of the respective core concept
When an atom absorbs energy (for instance, from absorbing a photon), one or more of its electrons can jump to higher energy orbitals. This new arrangement, with the electrons in higher energy levels, is called the excited state. The excited states have more energy compared to the ground state, and the electrons are further away from the nucleus.
headline of the respective core concept
Electron transition refers to the movement of an electron between energy levels within an atom. When an electron absorbs energy, it moves from a lower energy level to a higher one (excitation). Conversely, when the electron returns to a lower energy level, it releases energy, often in the form of light (emission). These transitions are fundamental to the understanding of atomic spectra and the behavior of atoms in different conditions.
headline of the respective core concept
Energy absorption is a process where an atom takes in energy from its surroundings. This energy can come from different sources such as light (photons), heat, or electrical energy. When atoms absorb energy, their electrons move to higher energy states, leading to excited states. This process is crucial in phenomena like photosynthesis in plants and the functioning of solar cells. The absorbed energy is later released, often as light or heat, when the electrons transition back to lower energy levels.

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Most popular questions from this chapter

a. What is the principal quantum number? b. How is it symbolized? c. What are shells? d. How does n relate to the number of electrons allowed per main energy level?

What are the frequency and wavelength ranges of visible light?

a. What is the relationship between n and the total number of orbitals in a main energy level? b. How many total orbitals are contained in the third main energy level? in the fifth?

Given that the electron configuration for oxygen is \(1 s^{2} 2 s^{2} 2 p^{4},\) answer the following questions: a. How many electrons are in each oxygen atom? b. What is the atomic number of this element? c. Write the orbital notation for oxygen’s electron configuration. d. How many unpaired electrons does oxygen have? e. What is the highest occupied energy level? f. How many inner-shell electrons does the atom contain? g. In which orbital(s) are these inner-shell electrons located?

Given that the electron configuration for phosphorus is \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{3},\) answer the following questions: a. How many electrons are in each atom? b. What is the atomic number of this element? c. Write the orbital notation for this element. d. How many unpaired electrons does an atom of phosphorus have? e. What is its highest occupied energy level? f. How many inner-shell electrons does the atom contain? g. In which orbital(s) are these inner-shell electrons located?
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