/*! 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 119 Which part of the following stat... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 4: Problem 119

Which part of the following statement is true and which part is false? \(\mathrm{Mg}^{2+}\) and \(\mathrm{Na}^{+}\) have identical electron configurations, and they also have similar properties. Explain your answer fully.

Short Answer

Expert verified
The first part of the statement is true, as \(\mathrm{Mg}^{2+}\) (1s虏 2s虏 2p鈦�) and \(\mathrm{Na}^{+}\) (1s虏 2s虏 2p鈦�) have identical electron configurations. However, the second part of the statement is false; although both ions are cations, they have different properties due to their varying charges (+2 for Mg虏鈦� and +1 for Na鈦�) and sizes (Mg虏鈦� is smaller than Na鈦�).

Step by step solution

01

Part 1: Electron configurations of Mg虏鈦� and Na鈦�

To verify if the \(\mathrm{Mg}^{2+}\) and \(\mathrm{Na}^{+}\) have identical electron configurations, we need to write the electron configuration of each ion. For magnesium (Mg): Its atomic number is 12, so the electron configuration of a neutral atom is 1s虏 2s虏 2p鈦� 3s虏. When Mg loses two electrons to become \(\mathrm{Mg}^{2+}\), its electron configuration becomes: 1s虏 2s虏 2p鈦�. For sodium (Na): Its atomic number is 11, so the electron configuration of a neutral atom is 1s虏 2s虏 2p鈦� 3s鹿. When Na loses one electron to become \(\mathrm{Na}^{+}\), its electron configuration becomes: 1s虏 2s虏 2p鈦�. Now, comparing the electron configurations of \(\mathrm{Mg}^{2+}\) (1s虏 2s虏 2p鈦�) and \(\mathrm{Na}^{+}\) (1s虏 2s虏 2p鈦�), we find that they are identical. So, the first part of the statement is true.
02

Part 2: Comparing properties of Mg虏鈦� and Na鈦�

Now we will analyze the second part of the statement, which claims that Mg虏鈦� and Na鈦� have similar properties. Mg虏鈦� and Na鈦� are both positive ions (cations) formed by losing electrons. However, they differ in their charge and size: - Charge: Mg虏鈦� has a charge of +2, whereas Na鈦� has a charge of +1. - Size: Mg虏鈦� is smaller in size compared to Na鈦� because, after losing electrons, Mg虏鈦� has more protons (12) attracting the remaining electrons, while Na鈦� has fewer protons (11). These differences in charge and size lead to different chemical and physical properties: 1. Chemical properties: Even though both ions are cations, their reactivity and the stability of their compounds differ due to the difference in charge and size. 2. Physical properties: The difference in size and charge also affects their solubility, melting and boiling points, and other physical properties. From this analysis, we can conclude that even though Mg虏鈦� and Na鈦� have identical electron configurations, they have different properties due to their varying charges and sizes. So, the second part of the statement is false.

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.

Cation Properties
Cations are positively charged ions that form when an atom loses electrons. This loss of electrons results in a positive charge. The properties of cations are influenced by their charge and size.
  • A higher positive charge generally leads to stronger interactions with negatively charged species.
  • Smaller cations typically lead to stronger attractions between the ion and its surroundings.
Cations like \(\mathrm{Mg}^{2+}\) and \(\mathrm{Na}^{+}\) differ in charge (+2 vs +1, respectively), which significantly impacts their properties. Mg虏鈦�, with more protons for the same number of electrons, is smaller than Na鈦� and can form stronger ionic bonds.
Electron Loss in Ions
When an atom becomes a cation, it loses electrons. This changes its electron configuration and stabilizes the ion according to the octet rule, often resembling the configuration of noble gases.
For example:
  • Magnesium (Mg), with atomic number 12, loses two electrons to become \(\mathrm{Mg}^{2+}\), reducing its electron configuration to 1s虏 2s虏 2p鈦�.
  • Sodium (Na), with atomic number 11, loses one electron to become \(\mathrm{Na}^{+}\), also achieving a 1s虏 2s虏 2p鈦� configuration.
This identical electron configuration explains why ions like \(\mathrm{Mg}^{2+}\) and \(\mathrm{Na}^{+}\) can have similar stable structures, despite differing in other properties.
Chemical Properties of Ions
The chemical properties of ions, such as reactivity and the nature of the compounds they form, can be quite different even if they share the same electron configuration.
Consider the differences:
  • \(\mathrm{Mg}^{2+}\), having a higher charge, forms more stable ionic compounds compared to \(\mathrm{Na}^{+}\).
  • The greater charge density of \(\mathrm{Mg}^{2+}\) results in higher lattice energy in its compounds.
These distinctions arise from the ion鈥檚 charge and the size, affecting how they interact with other ions and molecules.
Physical Properties of Cations
Cations have distinctive physical properties based on their charge and size. These attributes dictate how ions behave in different physical contexts, such as:
  • Solubility: \(\mathrm{Na}^{+}\) salts are generally more soluble in water compared to \(\mathrm{Mg}^{2+}\) salts, due to the smaller lattice energies of the former.
  • Melting and boiling points: \(\mathrm{Mg}^{2+}\) compounds often have higher melting and boiling points, owing to stronger ionic bonds.
Even when two cations like \(\mathrm{Mg}^{2+}\) and \(\mathrm{Na}^{+}\) share the same electron configuration, these physical properties will differ because of the variations in charge and ionic size.

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

What is the highest value of \(n\) for the electrons in these atoms? (a) \(\overline{\mathrm{Co}}\) (b) As (c) \(\overline{\mathrm{Sr}}\) (d) \(\overline{\mathrm{Po}}\)

Circle the correct choice to indicate how many electrons each element must gain or lose to form an octet: \(\begin{array}{llll}\text { (a) } \mathrm{Mg} & \text { gains, loses } & 1,2,3 & \text { electrons }\end{array}\) \(\begin{array}{lll}\text { (b) Se gains, loses } 1,2,3 & \text { electrons }\end{array}\) (c) Al gains, loses \(1,2,3\) electrons \(\begin{array}{llll}\text { (d) Sr gains, loses } & 1,2,3 & \text { electrons }\end{array}\) (e) Br gains, loses \(1,2,3\) electrons (f) P gains, loses \(1,2,3\) electrons

Which subshell has the lowest energy? (a) \(4 s\) (b) \(3 p\) (c) \(2 p\) (d) \(3 s\) (e) \(2 s\)

Of the following atoms, which has the largest first ionization energy? (a) \(\mathrm{Br}\) (b) \(\overline{\mathrm{O}}\) (c) \(\mathrm{C}\) (d) \(\mathrm{P}\) (e) I

What is the wavelength in nanometers of electromagnetic waves that have an energy of \(1.00 \times 10^{-15} \mathrm{~J} ?\)
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Kinetics

Read Explanation

Chemical Reactions

Read Explanation

The Earths Atmosphere

Read Explanation

Making Measurements

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.