Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 9: Problem 66

Refer only to the periodic table on the inside front cover, and arrange the following ionization energies in order of increasing value: \(I_{1}\) for \(\mathrm{F} ; I_{2}\) for \(\mathrm{Ba}\) \(I_{3}\) for \(\mathrm{Sc} ; I_{2}\) for \(\mathrm{Na} ; I_{3}\) for \(\mathrm{Mg}\). Explain the basis of any uncertainties.

Short Answer

Expert verified
Possible increasing arrangement: I1 for F < I2 for Na < I3 for Mg < I3 for Sc < I2 for Ba. Uncertainties might arise from the (n+l) rule and electron pair repulsion in elements with d and f block electrons.

Step by step solution

01

Understand the concept of ionization energy

The first ionization energy (I1) is defined as the energy required to remove the most loosely bound electron, the second ionization energy (I2) is the energy required to remove the second most loosely bound electron and the trend of ionization energies generally increases from left to right across a period and decreases down a group because the atomic radius is increasing, the nuclear charge is increasing, the number of energy levels/shells is increasing, and electron shielding is happening. However, there are exceptions to this
02

Locate the elements on the Periodic Table

Locate the elements Fluorine (F), Barium (Ba), Scandium (Sc), Sodium (Na), and Magnesium (Mg) on the Periodic Table. Note the Period (row) and Group (column) each element is in. It's also important to note the type of orbital (s,p,d,f) being filled with electrons in each of these elements.
03

Arrange the given ionization energies

Using the Periodic Table and understanding of ionization energy trends, arrange the ionization energies in increasing order. Since the first ionization energy is usually less than the second, and the second less than the third, I1 for F should be less than I2 for Na, which should be less than I3 for Mg. However, I3 for Sc and I2 for Ba are expected to be higher than I3 for Mg because they are the second and probably third ionization energies for the elements in their Period.
04

Reflect on uncertainties

Upon reflecting on uncertainties, it could arise from factors such as electron pair repulsion and the (n+l) rule when it comes to d and f block elements, which might cause some deviations from the general trend.
05

Final arrangement

Based on the information and understanding of ionization energy trends, a possible increasing arrangement could be: I1 for F < I2 for Na < I3 for Mg < I3 for Sc < I2 for Ba. However, there are still uncertainties because of possible exceptions for the d and f block elements.

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

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

Explain the important distinctions between each pair of terms: (a) actinide and lanthanide element; (b) covalent and metallic radius; (c) atomic number and effective nuclear charge; (d) ionization energy and electron affinity; (e) paramagnetic and diamagnetic.

In your own words, define the following terms: (a) isoelectronic; (b) valence- shell electrons; (c) metal; (d) nonmetal; (e) metalloid.

Assuming that the seventh period is 32 members long, what should be the atomic number of the noble gas following radon (Rn)? Of the alkali metal following francium (Fr)? What would you expect their approximate atomic masses to be?

Briefly describe each of the following ideas or phenomena: (a) the periodic law; (b) ionization energy; (c) electron affinity; (d) paramagnetism.

Plot a graph of the square roots of the ionization energies versus the nuclear charge for the two series \(\mathrm{Li}, \mathrm{Be}^{+}, \mathrm{B}^{2+}, \mathrm{C}^{3+},\) and \(\mathrm{Na}, \mathrm{Mg}^{+}, \mathrm{Al}^{2+}, \mathrm{Si}^{3+} .\) Explain the observed relationship with the aid of Bohr's expression for the binding energy of an electron in a one electron atom.
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Making Measurements

Read Explanation

Inorganic 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.

Sign-up for free