Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 6: Problem 56

Which of the four atoms \(\mathrm{Na}, \mathrm{P}, \mathrm{Cl}\), or \(\mathrm{K}\) (a) has the largest atomic radius? (b) has the highest ionization energy? (c) is the most electronegative?

Short Answer

Expert verified
Answer: Potassium (K) has the largest atomic radius, Chlorine (Cl) has the highest ionization energy, and Chlorine (Cl) is the most electronegative element.

Step by step solution

01

Understanding atomic radius

The atomic radius is the distance from the center of an atom's nucleus to its outermost electron. In a periodic table, atomic radii generally decrease from left to right within a period and increase from top to bottom within a group.
02

Understanding ionization energy

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. The ionization energy generally increases from left to right within a period and decreases from top to bottom within a group of the periodic table.
03

Understanding electronegativity

Electronegativity is the tendency of an atom to attract electrons to itself when it forms a chemical bond with another atom. Electronegativity generally increases from left to right within a period and decreases from top to bottom within a group of the periodic table.
04

Locating the four elements in the periodic table

Now, let's identify the positions of Na, P, Cl, and K in the periodic table. - Sodium (Na) is in Group 1 and Period 3 - Phosphorus (P) is in Group 15 and Period 3 - Chlorine (Cl) is in Group 17 and Period 3 - Potassium (K) is in Group 1 and Period 4
05

Determine the element with the largest atomic radius (a)

Based on the position of the given elements in the periodic table, we can determine which element has the largest atomic radius. We know that atomic radius increases from top to bottom within a group and decreases from left to right within a period. Therefore, Potassium (K), which is in Period 4 and Group 1, has the largest atomic radius among these four elements.
06

Determine the element with the highest ionization energy (b)

Since ionization energy increases from left to right within a period and decreases from top to bottom within a group, the element with the highest ionization energy will be Chlorine (Cl), which is in Group 17 and Period 3.
07

Determine the most electronegative element (c)

Electronegativity increases from left to right within a period and decreases from top to bottom within a group. Therefore, the most electronegative element among these four elements will be Chlorine (Cl), which is in Group 17 and Period 3. So, to summarize the answers: (a) Potassium (K) has the largest atomic radius. (b) Chlorine (Cl) has the highest ionization energy. (c) Chlorine (Cl) is the most electronegative element.

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

Give the symbol of the element of lowest atomic number whose ground state has (a) a p electron. (b) four felectrons. (c) a completed d subshell. (d) six s electrons.

Select the smaller member of each pair. (a) \(\mathrm{N}\) and \(\mathrm{N}^{3-}\) (b) \(\mathrm{Ba}\) and \(\mathrm{Ba}^{2+}\) (c) Se and \(\mathrm{Se}^{2-}\) (d) \(\mathrm{Co}^{2+}\) and \(\mathrm{Co}^{3+}\)

Write the ground state electron configuration for (a) \(\mathrm{B}\) (b) \(\mathrm{Ba}\) (c) \(\mathrm{Be}\) (d) \(\mathrm{Bi}\) (e) \(\mathrm{Br}\)

Give the number of unpaired electrons in an atom of (a) phosphorus (b) potassium (c) plutonium (Pu)

Write the ground state electron configuration for (a) \(\mathrm{N}\) (b) Na (c) Ne (d) Ni (e) Si
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Inorganic Chemistry

Read Explanation

Making Measurements

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Analysis

Read Explanation

Organic 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