/*! 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 52 Sketch a periodic table that wou... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 9: Problem 52

Sketch a periodic table that would include all the elements in the main body of the table. How many "numbers" wide would the table be?

Short Answer

Expert verified
The periodic table would be 18 numbers wide.

Step by step solution

01

Identify Groups in the Periodic Table

The main body of the periodic table is made up of groups, which are columns running vertically down the table. Elements in the same group share similar properties due to having the same number of electrons in their outer shell. Staring from left to right, each group has a distinct number from 1 through to 18.
02

Count the Groups

Given that there are 18 distinct groups from 1 to 18 in the main body of the periodic table, you can count each group to validate this fact.
03

Determine the Width of the Periodic Table

The 'width' of the periodic table corresponds to the number of groups it has, as they are arranged horizontally. After counting, it becomes evident that there are 18 groups, thus the width of the periodic table that includes all the elements is 18 numbers wide.

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.

Groups of Elements
The periodic table is often organized into vertical columns, known as groups. These groups help categorize elements with similar physical and chemical properties. Here's why they are significant:
  • Arrangement: Each group corresponds to a specific column on the periodic table, numbered from 1 to 18.
  • Shared Characteristics: Elements within the same group tend to exhibit similar characteristics. This is because they have the same number of valence electrons, which are the electrons in the outermost shell of an atom.
  • Examples: The alkali metals (Group 1) like sodium and potassium are highly reactive, whereas noble gases (Group 18) such as helium and neon are known for being inert.
Understanding how groups are arranged enhances your ability to predict the behavior of an element based on its position in the table.
Electron Configuration
Electron configuration provides insight into the arrangement of electrons around an atom's nucleus. It is crucial for predicting how an element will interact chemically.
  • Defining Orbitals: Electrons exist within different energy levels, often visualized as "shells." These shells are divided into orbitals (s, p, d, f), each capable of holding a specific number of electrons.
  • Notation: Electron configurations are typically represented by numbers and letters, such as 1s虏 2s虏 2p鈦�, indicating the distribution of electrons among shells and orbitals.
  • Influence on Properties: An element's chemical properties are significantly determined by its electron configuration, particularly the valence electrons.
By understanding electron configurations, you can foresee how elements might bond or react based on their position in the periodic table.
Chemical Properties
The chemical properties of elements are directly related to their position on the periodic table. These properties dictate how an element will behave in chemical reactions.
  • Reactivity: The tendency of an element to engage in chemical reactions varies across the table. For example, alkali metals are highly reactive, whereas noble gases are mostly inert.
  • Acid-Base Behavior: Some groups exhibit characteristic acid-base behavior. For instance, elements in Group 1 (alkali metals) often form strong bases.
  • Bonding Patterns: The ability to form certain types of chemical bonds, such as ionic or covalent, depends on the element's electron configuration and its group.
Having a grasp on the chemical properties allows for predictions about how different elements will react with each other, leading to a deeper understanding of chemical phenomena.

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

All the isoelectronic species illustrated in the text had the electron configurations of noble gases. Can two ions be isoelectronic without having noble-gas electron configurations? Explain.

Which of the following species has the greatest number of unpaired electrons (a) \(\mathrm{Ge} ;\) (b) \(\mathrm{Cl} ;\) (c) \(\mathrm{Cr}^{3+}\) (d) Br -?

Compare the elements \(\mathrm{Al}, \mathrm{Si}, \mathrm{S},\) and \(\mathrm{Cl}.\) (a) Place the elements in order of increasing ionization energy. (b) Place the elements in order of increasing electron affinity.

In your own words, define the following terms: (a) isoelectronic; (b) valence- shell electrons; (c) metal; (d) nonmetal; (e) metalloid.

A method for estimating electron affinities is to extrapolate \(Z_{\text {eff }}\) values for atoms and ions that contain the same number of electrons as the negative ion of interest. Use the data in the table on the next page to answer the questions that follow. $$\begin{array}{lll} \hline \begin{array}{l} \text { Atom or lon: } \\ \text { I(kJmol }^{-1} \text {) } \end{array} & \begin{array}{l} \text { Atom or lon: } \\ \text { I(kJmol }^{-1} \text {) } \end{array} & \begin{array}{l} \text { Atom or lon: } \\ \text { I(kJmol }^{-1} \text {) } \end{array} \\ \hline \text { Ne: 2080 } & \text { F: 1681 } & \text { O: } 1314 \\ \text { Na }^{+}: 4565 & \text { Ne }^{+}: 3963 & \text { F }^{+}: 3375 \\ \text { Mg }^{2+} \text { : 7732 } & \text { Na }^{2+}: 6912 & \text { Ne }^{2+}: 6276 \\ \text { A1 }^{\text {3 }^{+}: 11,577} & \text { Mg }^{3+}: 10,548 & \text { Na }^{3+}: 9540 \\ \hline \end{array}$$ (a) Estimate the electron affinity of \(F\), and compare it with the experimental value. (b) Estimate the electron affinities of \(\mathrm{O}\) and \(\mathrm{N}\) (c) Examine your results in terms of penetration and screening.
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Kinetics

Read Explanation

Nuclear Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Chemical Reactions

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.