/*! 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 113 Describe electronegativity trend... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 8: Problem 113

Describe electronegativity trends in the periodic table.

Short Answer

Expert verified
In the periodic table, electronegativity generally increases as we move from left to right across a period due to an increasing number of protons and a decreasing atomic radius. However, it decreases as we go down a group because of an increasing number of energy levels and larger atomic radius. The most electronegative element is fluorine, while the least electronegative is francium. Transition elements show slight or no variation in electronegativity, and noble gases have no electronegativity values due to their stable electron configurations.

Step by step solution

01

Understanding Electronegativity

Electronegativity is the ability of an atom in a molecule to attract electrons towards itself. It is a dimensionless quantity introduced by Linus Pauling and is a useful concept to understand the polarity and reactivity of chemical bonds. The electronegativity values for elements range from 0.7 for francium to 3.98 for fluorine on the Pauling scale.
02

Trend Across a Period (Horizontally)

As we move from left to right across a period in the periodic table, the electronegativity of elements generally increases. This is because the number of protons in the nucleus increases as we move across a period, which leads to a stronger positive charge attracting electrons. Moreover, the atomic radius decreases across a period due to an increase in the effective nuclear charge. As a result, electrons are held more tightly to the nucleus and are drawn closer, making the atom more electronegative.
03

Trend Down a Group (Vertically)

Going down a group in the periodic table, the electronegativity of elements generally decreases. This is because the number of energy levels or electron shells is increasing as we move down a group. These additional energy levels place the valence electrons further away from the nucleus, reducing their attraction to the protons in the nucleus. The atomic radius also increases, and since electronegativity is strongly related to atomic radius, the electronegativity decreases.
04

Exceptions and Notable Trends

There are a few exceptions to the general electronegativity trends, one of which is the transition elements. Electronegativity tends to vary slightly or remain relatively constant within a series of transition elements. Additionally, noble gases like helium, neon, and argon have no electronegativity values as they do not form bonds with other elements due to their stable electron configurations. It is important to note that the most electronegative element is fluorine, which is located in the top right corner of the periodic table (excluding noble gases), while the least electronegative element is francium, which can be found in the bottom-left corner. By understanding these trends and exceptions in electronegativity, students can better predict the behavior of elements and their chemical bonds in various chemical reactions.

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!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Periodic Table
The periodic table is an organized chart that displays all known chemical elements. Elements are arranged by increasing atomic number, which is the number of protons in an element's nucleus.

The layout enables us to see patterns in element properties, such as electronegativity, ionization energy, and atomic radius.
  • Elements in the same vertical column are called groups and share similar chemical properties.
  • Elements in horizontal rows are periods, and display gradual changes in properties across each row.
Understanding the periodic table helps predict how elements will react and bond with each other in chemical reactions.
Trends in Electronegativity
Electronegativity is a key concept in chemistry. It measures how strongly an atom can attract electrons towards itself. Different elements have varying electronegativities based on their positions in the periodic table.

  • As you move from left to right across a period, electronegativity tends to increase. This happens because elements have more protons, thus a greater positive nuclear charge attracting electrons.
  • Moving down a group, electronegativity generally decreases. This is due to the increased distance between the nucleus and valence electrons as additional electron shells are added, weakening the attraction.
Familiarizing yourself with these trends can help you understand chemical properties and reactiveness.
Chemical Bonds
Chemical bonds are forces that hold atoms together in compounds. Electronegativity plays a significant role in determining the type of bond that forms between atoms. There are three main types of chemical bonds:

  • Ionic bonds: Form between atoms with a large difference in electronegativity, usually between metals and non-metals.
  • Covalent bonds: Occur when atoms share electrons. If sharing is equal, it's a nonpolar covalent bond; if unequal, it's a polar covalent bond.
  • Metallic bonds: Found in metals, where electrons are shared across many atoms, creating a "sea of electrons."
The type of bond impacts the physical properties and reactivity of substances in chemical reactions.
Reactivity
Reactivity refers to how readily an element can participate in a chemical reaction.

Electronegativity is crucial in determining reactivity, especially for non-metals. Highly electronegative elements, like fluorine, are very reactive because they strongly attract electrons.

  • Non-metals generally have higher electronegativities and tend to gain electrons in reactions.
  • Metals usually have lower electronegativities and tend to lose electrons.
Understanding an element's electronegativity helps predict its behavior and reactivity in forming chemical compounds.
Pauling Scale
The Pauling Scale is a numerical scale that measures the electronegativity of elements. Introduced by Linus Pauling, it is named in his honor. The scale helps quantify electronegativity differences between elements, which is essential for predicting bond types.

  • The scale ranges from 0.7 to 4.0, with fluorine, the most electronegative element, at 3.98.
  • Francium has the lowest electronegativity value of 0.7, indicating weak attraction for electrons.
The Pauling Scale is a valuable tool for chemists in analyzing molecular structures and predicting bond behavior in compounds.

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

Summarize the rules for naming binary molecular compounds.

Challenge The \(\mathrm{ClO}_{4}-\) ion contains numerous lone pairs. Draw its Lewis structure.

Rank each of the molecules below in order of the shortest to the longest sulfur-oxygen bond length. a. \(\mathrm{SO}_{2} \quad\) b. SO_ \(_{3}^{2-} \quad\) c. \(\mathrm{SO}_{4}^{2-}\)

What must you know in order to draw the Lewis structure for a molecule?

Draw the resonance structures for the dinitrogen oxide \(\left(\mathrm{N}_{2} \mathrm{O}\right)\) molecule.
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemical Analysis

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.