Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 9: Problem 9

For each of the following pairs, indicate the atom that has the larger size: (a) Te or Br; (b) \(\mathrm{K}\) or \(\mathrm{Ca} ;\) (c) Ca or Cs; (d) \(\mathrm{N}\) or \(\mathrm{O} ;\) (e) \(\mathrm{O}\) or \(\mathrm{P} ;\) (f) \(\mathrm{Al}\) or \(\mathrm{Au}.\)

Short Answer

Expert verified
(a) Te, (b) K, (c) Cs, (d) N, (e) P, (f) Au.

Step by step solution

01

Identify the Position of Te and Br

From the periodic table, locate Tellurium (Te) and Bromine (Br). Both are in the same period, but Te is to the left of Br. Therefore, the atomic radii should decrease as we move to the right which implies Te is bigger.
02

Identify the Position of K and Ca

Looking at the periodic table, locate Potassium (K) and Calcium (Ca). Both of them are in the same period, but K is to the left of Ca. Therefore, as per the rule, K is bigger.
03

Identify the Position of Ca and Cs

From the periodic table, locate Calcium (Ca) and Cesium (Cs). Here, both are in the same group, but Cs is below Ca. Therefore, as per the rule, atomic size increases as you move down a group, which implies Cs is bigger.
04

Identify the Position of N and O

Looking at the periodic table, locate Nitrogen (N) and Oxygen (O). Both are in the same period, but N is to the left of O. Therefore, as per the rule, N is bigger.
05

Identify the Position of O and P

From the periodic table, locate Oxygen (O) and Phosphorus (P). Here, they are in the same group, but P is below O. Therefore, as per the rule, atomic size increases as you move down a group, indicating that P is bigger.
06

Identify the Position of Al and Au

Looking at the periodic table, locate Aluminum (Al) and Gold (Au). They belong to different groups and periods. However, Au is lower down than Al on the table. As a rule, atomic size increases as you move down, indicating that Au should be bigger.

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

The masses of individual atoms can be determined with great precision, yet there is considerable uncertainty about the exact size of an atom. Explain why this is the case.

Which of the following species would you expect tobe diamagnetic and which paramagnetic? (a) \(\mathrm{K}^{+}=\) (b) \(\mathrm{Cr}^{3+} ;\) (c) \(\mathrm{Zn}^{2+} ;\) (d) \(\mathrm{Cd} ;\) (e) \(\mathrm{Co}^{3+} ;\) (f) \(\mathrm{Sn}^{2+} ;\) (g) Br.

Compare the elements \(\mathrm{Na}, \mathrm{Mg}, \mathrm{O},\) and \(\mathrm{P}.\) (a) Place the elements in order of increasing ionization energy. (b) Place the elements in order of increasing electron affinity.

The highest first ionization energy of the following is that of (a) \(\mathrm{Cs}_{i}\) (b) \(\mathrm{Cl}_{i}\) (c) I; (d) Li.

Are there any atoms for which the second ionization energy \(\left(I_{2}\right)\) is smaller than the first \(\left(I_{1}\right) ?\) Explain.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Organic Chemistry

Read Explanation

Making Measurements

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

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