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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: \((\mathbf{a}) \mathrm{SiF}_{4}\) and \(\mathrm{LaF}_{3},(\mathbf{b}) \mathrm{FeCl}_{2}\) and \(\mathrm{ReCl}_{6},(\mathbf{c}) \mathrm{PbCl}_{4}\) and RbCl.

Short Answer

Expert verified
(a) SiF _{4}: Silicon tetrafluoride (molecular), LaF _{3}: Lanthanum fluoride (ionic); (b) FeCl _{2}: Iron(II) chloride (ionic), ReCl _{6}: Rhenium(VI) chloride (ionic); (c) PbCl _{4}: Lead(IV) chloride (ionic), RbCl: Rubidium chloride (ionic).

Step by step solution

01

Determine Compound Type for Part (a)

SiF _{4} is a compound formed by silicon (a non-metal) and fluorine (a non-metal). This makes SiF _{4} a molecular substance. LaF _{3} , on the other hand, is comprised of lanthanum (a metal) and fluorine (a non-metal), classifying it as an ionic compound.
02

Name the Compounds for Part (a)

The molecular compound SiF _{4} is named using prefixes: **Silicon tetrafluoride**. The ionic compound LaF _{3} is named by the metal followed by the non-metal with an -ide suffix: **Lanthanum fluoride**.
03

Determine Compound Type for Part (b)

FeCl _{2} is a compound of iron (a metal) and chlorine (a non-metal), which is an ionic compound. ReCl _{6} is a compound with rhenium (a metal) and chlorine (a non-metal), also making it an ionic compound.
04

Name the Compounds for Part (b)

For ionic compounds with transition metals, specify the metal's charge. FeCl _{2} is named **Iron(II) chloride** because iron has a +2 charge here. ReCl _{6} is named **Rhenium(VI) chloride** because the charge on rhenium is +6.
05

Determine Compound Type for Part (c)

PbCl _{4} is composed of lead (a metal) and chlorine (a non-metal), making it an ionic compound. RbCl is made from rubidium (a metal) and chlorine (a non-metal), classifying it as another ionic compound.
06

Name the Compounds for Part (c)

PbCl _{4} is named using the charge of the lead: **Lead(IV) chloride**. RbCl is named simply as **Rubidium chloride**.

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Key Concepts

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

Ionic Compounds
Ionic compounds are formed when metals and non-metals chemically combine by the transfer of electrons. Metals lose electrons to form positively charged ions, while non-metals gain these electrons to become negatively charged ions.
These ions attract each other due to opposite charges, creating ionic bonds.
  • They typically consist of a metal and a non-metal.
  • Usually solid at room temperature.
  • Have high melting and boiling points due to strong ionic bonds.
  • Conduct electricity when dissolved in water or melted due to free-moving ions.
To name ionic compounds:
  • Start with the name of the metal.
  • Followed by the non-metal, altering its ending to "-ide".
  • If the metal can have multiple charges, specify the charge with Roman numerals in parentheses.
Molecular Compounds
Molecular compounds, also known as covalent compounds, form when two or more non-metals share electrons. Unlike ionic compounds, there is no transfer of electrons.
This sharing allows each atom to achieve a stable electron configuration.
  • Typically consist of only non-metals.
  • Can be gases, liquids, or solids at room temperature.
  • Have relatively low melting and boiling points compared to ionic compounds.
  • Do not conduct electricity because they have no charged particles.
Naming molecular compounds involves using prefixes to denote the number of each type of atom present:
  • "Mono-" is sometimes omitted for the first element.
  • "Di-", "tri-", "tetra-", and so on indicate two, three, four, etc.
  • Change the ending of the last element to "-ide".
Naming Conventions
Naming conventions in chemistry help identify and communicate about compounds effectively.
Depending on whether a compound is ionic or molecular, different rules apply for naming them.
  • Ionic Compounds: Name the metal first, then the non-metal with its ending changed to "-ide". For transition metals, indicate the charge in Roman numerals.
  • Molecular Compounds: Use prefixes to indicate the number of atoms. Only the second element's name is altered to "-ide", and "mono-" is often dropped for the first element.
  • For polyatomic ions, such as sulfate (SO鈧劼测伝) and nitrate (NO鈧冣伝), use the ion name without modification.
Following these conventions ensures clarity and precision in communication among chemists worldwide.
Binary Compounds
Binary compounds are composed of exactly two different elements.
They can be either ionic or molecular depending on the nature of the elements involved.
An ionic binary compound consists of a metal and a non-metal, whereas a binary molecular compound comprises two non-metals.
  • Ionic Binary Compounds: Example: NaCl (sodium chloride) where Na is a metal and Cl is a non-metal.
  • Molecular Binary Compounds: Example: CO鈧� (carbon dioxide) composed of two non-metals, carbon and oxygen.
Naming is straightforward when these conventions are known:
  • Recognize the compound type first and apply respective naming rules.
  • For ionic, use the metal name first followed by the non-metal with "-ide".
  • For molecular, use appropriate prefixes for the number of atoms and alter the second element to end in "-ide".
Understanding and applying the principles behind naming binary compounds ensures effective learning and communication in chemistry.

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Most popular questions from this chapter

1,2-dihydroxybenzene is obtained when two of the adjacent hydrogen atoms in benzene are replaced with an OH group. A skeleton of the molecule is shown here. (a) Complete a Lewis structure for the molecule using bonds and electron pairs as needed. (b) Are there any resonance structures for the molecule? If so, sketch them. (c) Are the resonance structures in (a) and (b) equivalent to one another as they are in benzene?

Draw the dominant Lewis structures for these chlorineoxygen molecules/ions: \(\mathrm{ClO}, \mathrm{ClO}^{-}, \mathrm{ClO}_{2}^{-}, \mathrm{ClO}_{3}^{-}, \mathrm{ClO}_{4}^{-}\). Which of these do not obey the octet rule?

(a) Is lattice energy usually endothermic or exothermic? (b) Write the chemical equation that represents the process of lattice energy for the case of NaCl. (c) Would you expect salts like NaCl, which have singly charged ions, to have larger or smaller lattice energies compared to salts like \(\mathrm{CaO}\) which are composed of doubly-charged ions?

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: \((\mathbf{a}) \mathrm{TiCl}_{4}\) and \(\mathrm{CaF}_{2},(\mathbf{b}) \mathrm{ClF}_{3}\) and \(\mathrm{VF}_{3},(\mathbf{c}) \mathrm{SbCl}_{5}\) and \(\mathrm{AlF}_{3} .\)

(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.
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