/*! 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 51 Use the third period of the peri... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 8: Problem 51

Use the third period of the periodic table as an example to illustrate the change in first ionization energies of the elements as we move from left to right. Explain the trend.

Short Answer

Expert verified
As we move from left to right across the third period of the periodic table, the first ionization energy increases due to increasing nuclear charge and decreasing atomic radius. However, exceptions to this trend occur due to the electron configuration of some elements (Al, S).

Step by step solution

01

Identify the Elements of the Third Period

The third period of the periodic table consists of the elements from sodium (Na) to argon (Ar). These elements are: Na, Mg, Al, Si, P, S, Cl, and Ar.
02

Define First Ionization Energy

The first ionization energy is the energy required to remove the most loosely bound electron, the valence electron, from a neutral atom in its gaseous phase.
03

Analyze the Trend

As we move from left to right across the third period of the periodic table, the first ionization energy generally increases. This trend is mainly due to two effects: nuclear charge and atomic radius. As we go across the period, the atomic number increases, which means an increase in nuclear charge. This greater nuclear charge pulls the electrons in the atom closer, reducing the atomic radius and thus making electrons harder to remove, thereby increasing ionization energy.
04

Consider Exceptions

Although the general trend is for the first ionization energy to increase as you move from left to right, there are some exceptions. For sodium (Na) to magnesium (Mg), and phosphorus (P) to sulfur (S), the first ionization energy increases. However, aluminum (Al) and silicon (Si) do not follow this pattern, as the first ionization energy of aluminum is less than that of magnesium. This also occurs with phosphorus and sulfur.
05

Explain the Exceptions

These exceptions occur because of the structure of the electron shells. For Al and S, an electron is being removed from a higher-energy subshell (3p), which is easier to remove than from a lower-energy subshell (3s). This explains why the first ionization energy decreases from Mg to Al and from P to S.
06

Conclusion

On the whole, as you move from left to right across the third period of the periodic table, the first ionization energy tends to increase due to increasing nuclear charge and decreasing atomic radius. However, there are exceptions due to the electron configuration of some 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.

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

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

Write ground-state electron configurations for these transition metal ions: (a) \(\mathrm{Sc}^{3+}\) (b) \(\mathrm{Ti}^{4+}\) (c) \(\mathrm{V}^{5+}\) (d) \(\mathrm{Cr}^{3+}\) , (e) \(\mathrm{Mn}^{2+},\) (f) \(\mathrm{Fe}^{2+}\) (h) \(\mathrm{Co}^{2+}\) (g) \(\mathrm{Fe}^{3+}\) (i) \(\mathrm{Ni}^{2+}\) (i) \(\mathrm{Cu}^{+}\) (k) \(\mathrm{Cu}^{2+}\) (1) \(\mathrm{Ag}^{+}\) \((\mathrm{m}) \mathrm{Au}^{+}\) (n) \(\mathrm{Au}^{3+},\) (o) \(\mathrm{Pt}^{2+}\)

Give the physical states (gas, liquid, or solid) of the representative elements in the fourth period at 1 atm and \(25^{\circ} \mathrm{C}: \mathrm{K}, \mathrm{Ca}, \mathrm{Ga}, \mathrm{Ge}, \mathrm{As}, \mathrm{Se}, \mathrm{Br}\).

Why do elements that have high ionization energies usually have more positive electron affinities?

Acidic oxides are those that react with water to produce acid solutions, whereas the reactions of basic oxides with water produce basic solutions. Nonmetallic oxides are usually acidic, whereas those of metals are basic. Predict the products of the reactions of these oxides with water: \(\mathrm{Na}_{2} \mathrm{O}, \mathrm{BaO}, \mathrm{CO}_{2}\), \(\mathrm{N}_{2} \mathrm{O}_{5}, \mathrm{P}_{4} \mathrm{O}_{10}, \mathrm{SO}_{3} .\) Write an equation for each of the reactions.

Define ionic radius. How does the size change when an atom is converted to (a) an anion and (b) a cation?
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Making Measurements

Read Explanation

Physical Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Kinetics

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.