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Chapter 10: Problem 87

The lowest possible energy state of an atom is called the ________ state.

Short Answer

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ground state

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01

Identifying the term for the lowest energy state of an atom

The lowest possible energy state of an atom is called the "ground state." In the ground state, the electrons in an atom occupy the lowest available energy levels, and the atom is considered to be at its most stable configuration.

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Key Concepts

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

Atom Energy States
Atoms can exist at different energy levels, known as energy states. These states determine how much energy an atom and its electrons have. The most familiar energy states are:
  • Ground State: This is the lowest energy state an atom can be in. Here, all the electrons occupy the lowest possible energy levels. It's the "calm" state of an atom, where it's most stable and least reactive. Atoms prefer to stay in this state as it requires the least energy.
  • Excited States: When an atom absorbs energy, its electrons can jump to higher energy levels, putting the atom into an excited state. This state is temporary as electrons will eventually return to the ground state, releasing energy in the form of light or heat.
It's crucial to understand that the ground state reflects the natural, relaxed form of an atom. When atoms are in excited states, they seek to return to the ground state to regain stability.
Electron Configuration
Electron configuration describes how electrons are arranged in an atom's orbitals. Electrons fill the lowest available energy levels first, following the "Aufbau Principle." You can imagine this as a set of steps:
  • 1s, 2s, 2p, 3s, 3p, and so on. Electrons fill these orbitals from low to high energy.
  • Each orbital can hold a specific number of electrons, following the Pauli Exclusion Principle and Hund's Rule to ensure electrons fill the space efficiently and without violating any principles.
In the ground state, an atom's electrons are in their simplest, most energy-efficient configuration. This electron arrangement plays a crucial role in understanding how atoms interact and bond with each other. Understanding electron configurations also allows us to predict the chemical behavior of different elements. For example, elements with similar electron configurations exhibit similar chemical properties.
Atomic Stability
An atom's stability is primarily influenced by how its electrons are arranged. In general:
  • Atoms are most stable in their ground state because the electrons occupy the lowest energy levels, leading to a balanced, low-energy state.
  • When atoms are excited, they become less stable because the electrons are in higher energy levels or orbitals. Naturally, atoms strive to return to the more stable ground state.
  • Stable electron configurations, like a filled valence shell, often make atoms less reactive. Noble gases are perfect examples with their complete outer shells, making them relatively inert.
Stability is crucial for the atom's reactivity and the types of interactions it can undergo. More stable atoms react less vigorously compared to unstable ones, impacting their role in chemical reactions. Mechanisms like ionization, bonding, and excitation revolve around achieving or maintaining atomic stability.

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Most popular questions from this chapter

Into how many sublevels is the third principal energy level of hydrogen divided? What are the names of the orbitals that constitute these sublevels? What are the general shapes of these orbitals?

A student writes the electron configuration of carbon \((Z=6)\) as \(1 s^{3} 2 s^{3} .\) Explain to him what is wrong with this configuration.

Write the complete orbital diagram for each of the following elements, using boxes to represent orbitals and arrows to represent electrons. a. aluminum, \(Z=13\) b. phosphorus, \(Z=15\) c. bromine, \(Z=35\) d. argon, \(Z=18\)

Which elements in a given period (horizontal row) of the periodic table lose electrons most easily? Why?

When students first see a drawing of the \(p\) orbitals, they often question how the electron is able to jump through the nucleus to get from one lobe of the \(p\) orbital to the other. How would you explain this?
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