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Chapter 1: Problem 13

(a) What are the systematic names for \((0) \mathrm{CS}_{2} ;(\mathrm{il}) \mathrm{Cl}_{2} \mathrm{O}_{7}\) (iii) \(\mathrm{XeF}_{6} ;(\mathrm{iv})\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4} ;(\mathrm{v}) \mathrm{CrCl}_{3} ;(\mathrm{vi}) \mathrm{KlO}_{4} ?\) (b) Write the formula of each of the following compounds: (i) sodium sulfite; (ii) barium carbonate; (iii) iron(II) chloride; (iv) sodium thiosulfate; (v) diiodine pentoxide; (vil) dinitrogen oxide. (Section 1.4 )

Short Answer

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(a) (i) Carbon disulfide (ii) Dichlorine heptoxide (iii) Xenon hexafluoride (iv) Ammonium sulfate (v) Chromium(III) chloride (vi) Potassium periodate. (b) Na鈧係O鈧�, BaCO鈧�, FeCl鈧�, Na鈧係鈧侽鈧�, I鈧侽鈧�, N鈧侽.

Step by step solution

01

Understand Systematic Naming Rules

To systematically name a compound, we need to understand IUPAC naming conventions. For binary compounds like CS鈧�, we name based on electronegativity order: the less electronegative element first as a prefix and add -ide to the more electronegative element. For oxohalide like Cl鈧侽鈧�, the prefix 'di-' and 'hepta-' indicate the number of atoms.
02

Name Each Compound Systematically

(i) CS鈧� is named carbon disulfide. (ii) Cl鈧侽鈧� is dichlorine heptoxide. (iii) XeF鈧� is xenon hexafluoride. (iv) (NH鈧�)鈧係O鈧� is ammonium sulfate. (v) CrCl鈧� is chromium(III) chloride due to the chromium ion's +3 oxidation state. (vi) KIO鈧� is potassium periodate due to the IO鈧勨伝 ion, known as periodate.
03

Identify Formula Components for Writing Formulas

To write the formula of a compound, identify the constituent ions or molecules and their charges. For example, sodium sulfite contains sodium ions (Na鈦�) and sulfite ions (SO鈧兟测伝). Balance the charges to write the correct formula.
04

Write Formulas for Given Compounds

(i) Sodium sulfite: Na鈧係O鈧�. (ii) Barium carbonate: BaCO鈧�. (iii) Iron(II) chloride implies Fe虏鈦� ions and Cl鈦� ions, so the formula is FeCl鈧�. (iv) Sodium thiosulfate: Na鈧係鈧侽鈧�. (v) Diiodine pentoxide: I鈧侽鈧�. (vi) Dinitrogen oxide: N鈧侽.

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Key Concepts

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

IUPAC Naming Conventions
To systematically name chemical compounds, the IUPAC naming conventions serve as the global standard, providing a uniform language for chemists worldwide. This system helps identify not just the elements within a compound but also their quantities and interactions. For binary compounds, we use prefixes like 'mono-', 'di-', 'tri-', etc., to indicate the number of each type of atom present. Additionally, in binary compounds, the element with less electronegativity is named first, followed by the more electronegative one with an '-ide' suffix. For example, in the compound carbon disulfide (CS鈧�), 'di-' indicates two sulfur atoms, and the '-ide' suffix is added to sulfur.
Binary Compounds
Binary compounds consist of exactly two different elements. They can be either ionic, composed of metals and non-metals, or covalent, involving only non-metals. When naming binary ionic compounds, the metal name comes first, followed by the non-metal name with an '-ide' ending. For example, sodium chloride (NaCl) combines sodium and chlorine. In covalent binary compounds, which often involve gases, the element names also reflect the number of atoms with prefixes such as mono-, di-, tri-, etc. For instance, dichlorine heptoxide (Cl鈧侽鈧�) and dioxgen (O鈧�) utilize this naming system effectively to denote the number of each atom.
Oxidation States
Oxidation states are an integral part of chemical nomenclature, providing information about the charge of ions within compounds. These states indicate the hypothetical charge that an atom would have if all bonds were ionic. In transition metals, oxidation states can vary and must be specified when naming. For example, in chromium(III) chloride (CrCl鈧�), the Roman numeral III indicates a +3 oxidation state for the chromium ion. Oxidation states help avoid ambiguity when multiple ionic forms are possible, ensuring the correct compound is identified in both written and spoken nomenclature.
Ionic Compounds
Ionic compounds consist of positively charged ions (cations) and negatively charged ions (anions) arranged in a lattice structure. Typically formed between metals and non-metals, they result from the transfer of electrons from one atom to another. In chemical formulas, it's crucial to balance the total positive and negative charges. For example, in ammonium sulfate \((NH_4)_2SO_4\), two ammonium ions each carrying a +1 charge balance the \(-2\) charge on the sulfate ion. This charge balance is vital to understanding how ionic compounds are structured and named.
Chemical Formula Writing
Writing chemical formulas requires understanding the components and charges in a compound. Firstly, identify the ions involved and their respective charges. For binary ionic compounds, swap and drop the charges to balance them as with sodium sulfite, Na鈧係O鈧�, which is made from sodium ions (Na鈦�) and sulfite ions (SO鈧兟测伝). The subscript numbers in a chemical formula ensure the overall neutrality of the compound. In molecular compounds such as diiodine pentoxide (I鈧侽鈧�), the prefixes indicate how many atoms of each element are interconnected, ensuring that the written formula precisely reflects the compound's structure.

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Most popular questions from this chapter

Sodium chromate \(\left(\mathrm{Na}_{2} \mathrm{CrO}_{4}\right)\) can be prepared by oxidizing a chromium(lil) salt with sodium peroxide (Na_O_) in alkaline solution. The \(\mathrm{Cr}^{3+}\) ions are oxidized to \(\mathrm{CrO}_{4}^{2-}\) ions. The \(\mathrm{O}_{2}^{2-}\) ions are reduced to OH' ions. Construct half equations and a balanced overall equation for the reaction. (Section \(1.4)\)

Nitrogen dioxide gas is heated in a sealed container at \(700 \mathrm{K}\) until the system comes to equilibrium. The nitrogen dioxide dissociates into nitrogen monoxide and oxygen in an endothermic process (Section \(1.9)\) $$2 \mathrm{NO}_{2}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g})$$ The equilibrium constant at \(700 \mathrm{K}\) is \(2.78 \times 10^{-2} \mathrm{moldm}^{-3}\) (a) Write an expression for \(K_{c}\) (b) State how the position of equilibrium would be affected by: (1) an increase in temperature (ii) an increase in the total pressure. (c) At equilibrium at \(700 \mathrm{K}\), the concentration of nitrogen monoxide was found to be \(0.017 \mathrm{moldm}^{-3}\). What was the concentration of nitrogen dioxide in the equilibrium mixture?

A stream running out from a copper mine contains a dilute solution of copper sulfate. As it passes over an iron grid, copper metal deposits on the grid. (Section \(1.4)\) (a) Write a balanced equation, with state symbols, for the reaction taking place. (b) Write an ionic equation for the reaction. (c) Assign oxidation states to the elements in each of the reactants and products in the equation in (b). Use these values to decide what has been oxidized and what reduced.

The standard enthalpy change of combustion of heptane, \(\left.\mathrm{C}_{7} \mathrm{H}_{16}, \text { at } 298 \mathrm{K}, \text { is }-4817 \mathrm{kJmol}^{-1} \text {. (Section } 1.6\right)\) (a) Write a thermochemical equation for the complete combustion of heptane to carbon dioxide and water. (b) What is the enthalpy change when \(50 \mathrm{g}\) of heptane are bumed? (c) What mass of heptane would be needed to provide \(100 \mathrm{MJ}\) of energy?

Oxygen gas liquefies at \(-183.0^{\circ} \mathrm{C}\) and freezes at \(-218.4^{\circ} \mathrm{C}\) Work out its melting point, \(T_{\mathrm{m}},\) and boiling point, \(T_{\mathrm{b}},\) in kelvin. (Section \(1.2)\)
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