/*! 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 45 In the following pairs of binary... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 8: Problem 45

In the following pairs of binary compounds, determine which one is a molecular substance and which one is an ionic substance. Use the appropriate naming convention (for ionic or molecular substances) to assign a name to each compound: (a) \(\mathrm{SiF}_{4}\) and \(\mathrm{LaF}_{3},(\mathbf{b}) \mathrm{FeCl}_{2}\) and \(\mathrm{ReCl}_{6},(\mathrm{c}) \mathrm{PbCl}_{4}\) and \(\mathrm{RbCl} .\)

Short Answer

Expert verified
(a) \(\mathrm{SiF}_{4}\): molecular substance, silicon tetrafluoride \(\mathrm{LaF}_{3}\): ionic substance, lanthanum fluoride (b) \(\mathrm{FeCl}_{2}\): ionic substance, iron(II) chloride \(\mathrm{ReCl}_{6}\): ionic substance, rhenium(VI) chloride (c) \(\mathrm{PbCl}_{4}\): ionic substance, lead(IV) chloride \(\mathrm{RbCl}\): ionic substance, rubidium chloride

Step by step solution

01

Identify the Ionic or Molecular Compound of each pair#a# For each compound in the pair, determine whether it is ionic or molecular.

(a) \(\mathrm{SiF}_{4}\): non-metal + non-metal, therefore molecular \(\mathrm{LaF}_{3}\): metal + non-metal, therefore ionic (b) \(\mathrm{FeCl}_{2}\): metal + non-metal, therefore ionic \(\mathrm{ReCl}_{6}\): metal + non-metal, therefore ionic (c) \(\mathrm{PbCl}_{4}\): metal + non-metal, therefore ionic \(\mathrm{RbCl}\): metal + non-metal, therefore ionic
02

Assign the Naming Convention#a# For each compound, apply the correct naming convention based on whether it is ionic or molecular.

(a) \(\mathrm{SiF}_{4}\): molecular, so we use prefixes Name: silicon tetrafluoride \(\mathrm{LaF}_{3}\): ionic, so we use the -ide suffix for the non-metal Name: lanthanum fluoride (b) \(\mathrm{FeCl}_{2}\): ionic, so we use the -ide suffix for the non-metal Name: iron(II) chloride (Roman numeral indicates the charge on the metal) \(\mathrm{ReCl}_{6}\): ionic, so we use the -ide suffix for the non-metal Name: rhenium(VI) chloride (Roman numeral indicates the charge on the metal) (c) \(\mathrm{PbCl}_{4}\): ionic, so we use the -ide suffix for the non-metal Name: lead(IV) chloride (Roman numeral indicates the charge on the metal) \(\mathrm{RbCl}\): ionic, so we use the -ide suffix for the non-metal Name: rubidium chloride Summary: (a) \(\mathrm{SiF}_{4}\): molecular substance, silicon tetrafluoride \(\mathrm{LaF}_{3}\): ionic substance, lanthanum fluoride (b) \(\mathrm{FeCl}_{2}\): ionic substance, iron(II) chloride \(\mathrm{ReCl}_{6}\): ionic substance, rhenium(VI) chloride (c) \(\mathrm{PbCl}_{4}\): ionic substance, lead(IV) chloride \(\mathrm{RbCl}\): ionic substance, rubidium chloride

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.

Ionic Compounds
Ionic compounds form when atoms transfer electrons from one to another, usually between metals and non-metals. This transfer creates ions, which are charged particles. Metals, which are positive ions (cations), transfer electrons to non-metals, which become negative ions (anions).
The positive and negative charges attract each other, creating a strong bond called an ionic bond. Common properties of ionic compounds include:
  • High melting and boiling points due to the strong forces between ions.
  • They conduct electricity when dissolved in water, as the ions are free to move.
  • They are usually solid at room temperature.
To name ionic compounds, the metal's name comes first, followed by the non-metal, which ends with "-ide". If the metal can have different charges (like transition metals), you specify its charge using Roman numerals. For example, in the compound FeCl鈧�, iron is in the +2 state, so it is called iron(II) chloride.
This helps distinguish it from iron(III) chloride, where iron would have a +3 charge.
Molecular Compounds
Molecular compounds, also known as covalent compounds, consist of atoms sharing electrons rather than transferring them. These bonds form typically between non-metal atoms. The shared electrons between these atoms hold them together in units called molecules.
This type of bonding results in different properties compared to ionic compounds. Characteristics of molecular compounds include:
  • Low melting and boiling points compared to ionic compounds, because the forces between the molecules are weaker.
  • They do not conduct electricity because there are no free ions or electrons.
  • Many exist as gases or liquids at room temperature.
Naming molecular compounds involves using prefixes to indicate the number of each type of atom present in the compound. For example, SiF鈧� is called silicon tetrafluoride where "tetra-" indicates four fluorine atoms. Understanding the system of prefixes (mono-, di-, tri-, tetra-, etc.) is key to proper naming of molecular compounds.
Binary Compounds
Binary compounds are simply those composed of exactly two different elements. These compounds can be either ionic or molecular.
The method of naming them varies depending on the nature of the bonds between the elements. For ionic binary compounds, you name the metal first followed by the non-metal with an "-ide" suffix. If it's a transition metal, remember to add a Roman numeral indicating its charge. For example, CoCl鈧� is called cobalt(II) chloride.
For molecular or covalent binary compounds, prefixes are used to specify the number of atoms. For example, in the molecular compound PCl鈧�, phosphorus is combined with five chlorine atoms, so the compound is named phosphorus pentachloride. In summary, recognizing whether a binary compound is ionic or molecular will guide you to the correct naming convention, aiding in understanding and communicating the compound鈥檚 composition effectively.

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

Which ionic compound is expected to form from combining the following pairs of elements? (a) barium and fluorine, (b) cesium and chlorine, (c) lithium and nitrogen, (d) aluminum and oxygen.

An ionic substance of formula MX has a lattice energy of \(6 \times 10^{3} \mathrm{k} / \mathrm{mol} .\) Is the charge on the ion M likely to be \(1+, 2+,\) or \(3+?\) Explain.

Consider the collection of nonmetallic elements \(\mathrm{O}, \mathrm{P}\) , Te, \(\mathrm{I},\) and \(\mathrm{B} .\) (a) Which two would form the most polar single bond? (b) Which two would form the longest single bond? (c) Which two would be likely to form a compound of formula \(\mathrm{XY}_{2} ?(\mathbf{d})\) Which combinations of elements would likely yield a compound of empirical formula \(\mathrm{X}_{2} \mathrm{Y}_{3}\) ?

(a) What is the trend in electronegativity going from left to right in a row of the periodic table? (b) How do electronegativity values generally vary going down a column in the periodic table? (c) True or false: The most easily ionizable elements are the most electronegative.

Although \(\mathrm{I}_{3}\) is a known ion, \(\mathrm{F}_{3}^{-}\) is not. (a) Draw the Lewis structure for \(\mathrm{I}_{3}^{-}\) (it is linear, not a triangle). (b) One of your classmates says that \(\mathrm{F}_{3}^{-}\) does not exist because \(\mathrm{Fis}\) too electronegative to make bonds with another atom. Give an example that proves your classmate is wrong. (c) Another classmate says \(\mathrm{F}_{3}^{-}\) does not exist because it would violate the octet rule. Is this classmate possibly correct? (d) Yet another classmate says \(\mathrm{F}_{3}^{-}\) does not exist because \(\mathrm{F}\) is too small to make bonds to more than one atom. Is this classmate possibly correct?
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Chemical Analysis

Read Explanation

The Earths Atmosphere

Read Explanation

Inorganic Chemistry

Read Explanation

Organic Chemistry

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.