Problem 18
Question
The electronic configuration of an element is \(1 s^{2}, 2 s^{2} 2 p^{6}, 3 s^{2} 3 p^{6} 3 d^{3}, 4 s^{1} .\) This represents its [2000S] (a) excited state (b) ground state (c) cationic form (d) anionic form
Step-by-Step Solution
Verified Answer
(a) excited state
1Step 1: Understand the given electronic configuration
Analyze the given electronic configuration: \(1s^2, 2s^2 2p^6, 3s^2 3p^6 3d^3, 4s^1\). Identify the total number of electrons. Count the total electrons as follows: \(1s^2 = 2\), \(2s^2 2p^6 = 8\), \(3s^2 3p^6 3d^3 = 11\), and \(4s^1 = 1\). Thus, the total is \(2 + 8 + 11 + 1 = 22\) electrons.
2Step 2: Determine the element
Using the periodic table, identify the element with an atomic number of 22, which corresponds to Titanium (Ti). Titanium in its neutral state has an atomic number of 22 and thus 22 electrons.
3Step 3: Analyze the electronic configuration for ground state
Check the standard ground state configuration for Titanium: \([Ar] 3d^2 4s^2\). The provided configuration \(1s^2, 2s^2 2p^6, 3s^2 3p^6 3d^3, 4s^1\) differs by having more electrons in the \(3d\) orbital and fewer in the \(4s\) orbital than expected.
4Step 4: Conclude the state of the element
Since the electronic arrangement deviates from the typical ground state configuration by having an altered \(3d\) and \(4s\) configuration, this electron arrangement corresponds to an excited state of Titanium.
Key Concepts
Excited StateGround StateTitanium
Excited State
In atomic physics, an excited state of an atom refers to any electronic configuration that has higher energy than the ground state. When an atom absorbs energy, its electrons can be moved to higher energy levels, creating an excited state.
This state is usually unstable and temporary. Electrons tend to revert to lower energy levels, releasing energy in the form of light or other electromagnetic radiation. In the case of titanium's electronic configuration, the rearrangement of electrons from the representative ground state into \(3d^3 4s^1\) shows an electron in a higher energy state.
Usually, the energy causes an electron to shift from the lower energy 4s orbital to the higher energy 3d orbital, which creates this excited state. What is important to remember is that excited states explain a lot about how and why atoms emit light or interact with other atoms, critical to understanding chemical reactions and color emission.
This state is usually unstable and temporary. Electrons tend to revert to lower energy levels, releasing energy in the form of light or other electromagnetic radiation. In the case of titanium's electronic configuration, the rearrangement of electrons from the representative ground state into \(3d^3 4s^1\) shows an electron in a higher energy state.
Usually, the energy causes an electron to shift from the lower energy 4s orbital to the higher energy 3d orbital, which creates this excited state. What is important to remember is that excited states explain a lot about how and why atoms emit light or interact with other atoms, critical to understanding chemical reactions and color emission.
Ground State
The ground state of an atom is the most stable and low-energy configuration of electrons around its nucleus. It is the typical arrangement of electrons when there is no external energy affecting the atom.
For titanium, the ground state is represented by the electron configuration \([Ar] 3d^2 4s^2\). This means, when all electrons are in their lowest energy states without external excitation.
Looking at the periodic table and the expected electronic configurations helps to understand the normal distribution of electrons. If "ground state" sounds too scientific, think of it as the "resting state"—where electrons would naturally settle when left undisturbed.
For titanium, the ground state is represented by the electron configuration \([Ar] 3d^2 4s^2\). This means, when all electrons are in their lowest energy states without external excitation.
Looking at the periodic table and the expected electronic configurations helps to understand the normal distribution of electrons. If "ground state" sounds too scientific, think of it as the "resting state"—where electrons would naturally settle when left undisturbed.
- Electron configurations in the ground state are vital for predicting bonding behavior and the chemical properties.
- The closer the electrons remain to their nucleus, the more stable the atom is in its ground state.
Titanium
Titanium is a transition metal with the chemical symbol Ti and an atomic number of 22. It is a lightweight, strong metal, commonly used in aerospace and medical industries due to its excellent strength-to-weight ratio and corrosion resistance.
When it comes to electronic configuration, Titanium typically has the ground state configuration \([Ar] 3d^2 4s^2\). This characteristic configuration is due to its 22 electrons being distributed in a way that fills the lower energy levels first.
Understanding titanium's electronic position reveals why it forms certain kinds of chemical bonds. As a metal, it readily loses electrons to form positive ions.
When it comes to electronic configuration, Titanium typically has the ground state configuration \([Ar] 3d^2 4s^2\). This characteristic configuration is due to its 22 electrons being distributed in a way that fills the lower energy levels first.
Understanding titanium's electronic position reveals why it forms certain kinds of chemical bonds. As a metal, it readily loses electrons to form positive ions.
- Properties like hardness and melting point are determined largely by its electronic configuration.
- Though its typical configuration is \(3d^2 4s^2\), changes in electron distribution occur under excited states or in various chemicals.
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