/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 18 The electronic configuration of ... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 2: Problem 18

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

Short Answer

Expert verified
(a) excited state

Step by step solution

01

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.
02

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.
03

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.
04

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.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

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

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.
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"鈥攚here 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.
  • 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.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Isotopes of an element differ in the number of \(\ldots \ldots \ldots \ldots .\) in their nuclei.

Which of the following statements is false? (a) Splitting of spectral lines in electrical field is called Stark effect (b) Frequency of emitted radiation from a black body goes from a lower wavelength to higher wavelength as the temperature increases (c) Photon has momentum as well as wavelength (d) Rydberg constant has unit of energy

When alpha particles are sent through a thin metal foil, most of them go straight through the foil because : (a) alpha particles are much heavier than electrons (b) alpha particles are positively charged (c) most part of the atom is empty space (d) alpha particle move with high velocity

What is the work function of the metal if the light of wavelength \(4000 \AA\) generates photoelectrons of velocity \(6 \times 10^{5} \mathrm{~ms}^{-1}\) from it ? (Mass of electron= \(9 \times 10^{-31} \mathrm{~kg}\) Velocity of light \(=3 \times 10^{\circ} \mathrm{ms}^{-1}\) Planck's constant \(=6.626 \times 10^{-34} \mathrm{~J}_{\mathrm{S}}\) Charge of electron \(=1.6 \times 10^{-19} \mathrm{JeV}^{-1}\) ) (a) \(0.9 \mathrm{eV}\) (b) \(3.1 \mathrm{eV}\) (c) \(2.1 \mathrm{eV}\) (d) \(4.0 \mathrm{eV}\)

The quantum number of four electrons are given below: I. \(n=4, l=2, m_{l}=-2, m_{s}=-1 / 2\) II. \(n=3, l=2, m_{l}=1, m_{s}=+1 / 2\) III. \(n=4, l=1, m_{l}=0, m_{s}=+1 / 2\) IV. \(n=3, l=1, m_{l}=1, m_{\mathrm{s}}=-1 / 2\) The correct order of their increasing energies will be : (a) IV \(<\mathrm{III}<\mathrm{II}<\mathrm{I}\) (b) \(\mathrm{I}<\mathrm{II}<\mathrm{III}<\mathrm{IV}\) (c) \(\mathrm{IV}<\mathrm{II}<\mathrm{III}<\mathrm{I}\) (d) \(\mathrm{I}<\mathrm{III}<\mathrm{II}<\mathrm{IV}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Making Measurements

Read Explanation

Chemical Analysis

Read Explanation

Inorganic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Nuclear Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.