Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 6: Problem 59

List the following species in order of decreasing radius. (a) \(\mathrm{C}, \mathrm{Mg}, \mathrm{Ca}, \mathrm{Si}\) (b) Sr, Cl, Br, I

Short Answer

Expert verified
Question: Arrange the following elements in order of decreasing radius: (a) C, Mg, Ca, Si and (b) Sr, Cl, Br, I. Answer: (a) Ca > Mg > Si > C and (b) Sr > I > Br > Cl.

Step by step solution

01

Identify the positions in the periodic table

Place each element in its respective position in the periodic table. C is a group 14 element, Mg is a group 2 element, Ca is also a group 2 element, and Si is a group 14 element.
02

Apply the atomic radius trend

As you move from left to right across a period, atomic radius generally decreases due to the increasing effective nuclear charge. As you move down a group, atomic radius generally increases due to the addition of electron shells.
03

List the elements in order of decreasing radius

Knowing the trends in atomic radius, we can order the elements as follows: \(\mathrm{Ca} \gt \mathrm{Mg} \gt \mathrm{Si} \gt \mathrm{C}\). (b) Sr, Cl, Br, I
04

Identify the positions in the periodic table

Place each element in its respective position in the periodic table. Sr is a group 2 element, Cl is a group 17 element, Br is also a group 17 element, and I is a group 17 element.
05

Apply the atomic radius trend

Similar to the first part, as you move from left to right across a period, atomic radius generally decreases due to the increasing effective nuclear charge. As you move down a group, atomic radius generally increases due to the addition of electron shells.
06

List the elements in order of decreasing radius

Knowing the trends in atomic radius, we can order the elements as follows: Sr \(\gt\) I \(\gt\) Br \(\gt\) Cl.

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

Select the larger member of each pair. (a) \(\mathrm{K}\) and \(\mathrm{K}^{+}\) (b) \(\mathrm{O}\) and \(\mathrm{O}^{2-}\) (c) \(\mathrm{Tl}\) and \(\mathrm{Tl}^{3+}\) (d) \(\mathrm{Cu}^{+}\) and \(\mathrm{Cu}^{2+}\)

Explain why (a) negative ions are larger than their corresponding atoms. (b) scandium, a transition metal, forms an ion with a noble-gas structure. (c) electronegativity decreases down a group in the periodic table.

Magnetic resonance imaging (MRI) is a powerful diagnostic tool used in medicine. The imagers used in hospitals operate at a frequency of \(4.00 \times 10^{2} \mathrm{MHz}\left(1 \mathrm{MHz}=10^{6} \mathrm{~Hz}\right) .\) Calculate (a) the wavelength. (b) the energy in joules per photon. (c) the energy in kilojoules per mole.

Give the number of unpaired electrons in an atom of (a) mercury (b) manganese (c) magnesium

The ionization energy of rubidium is \(403 \mathrm{~kJ} / \mathrm{mol}\). Do X-rays with a wavelength of \(85 \mathrm{~nm}\) have sufficient energy to ionize rubidium?
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Chemical Analysis

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

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.

Sign-up for free