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Chapter 10: Problem 1

Name the following ionic compounds: (a) \(\mathrm{Ca}(\mathrm{CN})_{2}(s)\) (b) \(\mathrm{AgClO}_{4}(s)\) (c) \(\mathrm{KMnO}_{4}(s)\) (d) \(\operatorname{SrCrO}_{4}(s)\)

Short Answer

Expert verified
(a) Calcium cyanide; (b) Silver perchlorate; (c) Potassium permanganate; (d) Strontium chromate.

Step by step solution

01

Identify the Cation

For each compound, first identify the cation. In (a) \(\mathrm{Ca(CN)}_{2}(s)\), the cation is calcium (Ca). (b) \(\mathrm{AgClO}_{4}(s)\), the cation is silver (Ag). (c) \(\mathrm{KMnO}_{4}(s)\), the cation is potassium (K). (d) \(\operatorname{SrCrO}_{4}(s)\), the cation is strontium (Sr).
02

Identify the Anion

Determine the anion for each compound. In (a) \(\mathrm{Ca(CN)}_{2}(s)\), the anion is the cyanide ion (\(\mathrm{CN}^-\)). (b) \(\mathrm{AgClO}_{4}(s)\), the anion is the perchlorate ion (\(\mathrm{ClO}_{4}^-\)). (c) \(\mathrm{KMnO}_{4}(s)\), the anion is the permanganate ion (\(\mathrm{MnO}_{4}^-\)). (d) \(\operatorname{SrCrO}_{4}(s)\), the anion is the chromate ion (\(\mathrm{CrO}_{4}^{2-}\)).
03

Name the Compound

Combine the cation and anion names for each compound, maintaining the order as 'cation name + anion name'.(a) \(\mathrm{Ca(CN)}_{2}(s)\) is named calcium cyanide. (b) \(\mathrm{AgClO}_{4}(s)\) is named silver perchlorate. (c) \(\mathrm{KMnO}_{4}(s)\) is named potassium permanganate. (d) \(\operatorname{SrCrO}_{4}(s)\) is named strontium chromate.

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Key Concepts

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

Nomenclature
Nomenclature is the system of naming chemical compounds. It provides a standardized way to identify chemical substances. For ionic compounds, nomenclature involves naming both the cation and the anion part of the compound. The **cation name** is always mentioned first, followed by the **anion name**. This naming order helps in clear communication and understanding for chemists worldwide.
Important points to remember in nomenclature of ionic compounds:
  • Cations retain the element name, such as Calcium (Ca) and Potassium (K).
  • Anions often have names ending in '-ide', '-ate', or '-ite', such as Chloride (Cl-) or Sulfate (SO42-).
By adhering to these rules, you can accurately name any ionic compound given its chemical formula.
Cation Identification
In an ionic compound, the cation is the positively charged ion. Cations are typically formed from metals, and they possess a positive charge due to the loss of electrons. Understanding how to identify the cation in a formula is crucial because it is always listed first in the compound.
To identify the cation:
  • Look at the chemical formula and locate the metallic element. This is usually a single element or a polyatomic ion.
  • The cation's charge can often be inferred from the group number on the periodic table, like Group 1 metals having a +1 charge.
For instance, in (b) Silver perchlorate ( ext{AgClO}_4 ) , the cation is Silver ( Ag ), easily identified because silver is a transition metal.
Anion Identification
Anions are negatively charged ions and are usually nonmetals or polyatomic ions. These ions gain electrons, resulting in a negative charge. Identifying the anion is the next step after identifying the cation when working with ionic compounds.
To determine the anion:
  • After finding the cation in the chemical formula, the remaining part of the formula is the anion.
  • Common anions include single elements (e.g., Cl- for chloride), but they can also be polyatomic (e.g., NO3- for nitrate).
In the example of (d) Strontium chromate ( SrCrO_4 ) , the anion is the chromate polyatomic ion ( CrO_4^{2-} ). Identifying whether the anion is single- or multi-element helps label it correctly.
Chemical Formulas
A chemical formula represents the elements in a compound and the ratio of atoms. For ionic compounds, these formulas provide a shorthand way of showing how many of each ion is needed to balance charges and create a neutral compound. Understanding the structure of chemical formulas helps in both writing and naming ionic compounds.
Rules for interpreting chemical formulas:
  • The first part of the formula is the cation, which is followed by the anion.
  • Subscripts indicate the number of ions needed to balance the charge; e.g., CaCN _2_ shows two cyanide ions are needed per calcium ion.
    • li>Remember that the total charge must be zero, meaning positive charges from cations must cancel out negative charges from anions.
By applying these rules, one can correctly ascertain the composition and naming conventions of any ionic compound.

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Most popular questions from this chapter

Write the chemical formula for (a) sodium perchlorate (b) potassium permanganate (c) calcium sulfite (d) lithium cyanide

Complete and balance the equations for the following single-replacement reactions: (a) \(\mathrm{Ba}(s)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow\) (b) \(\mathrm{Fe}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow\) (c) \(\mathrm{Ca}(s)+\operatorname{HBr}(a q) \rightarrow\) (d) \(\mathrm{Pb}(s)+\mathrm{HCl}(a q) \rightarrow\)

Sodium hydroxide, \(\mathrm{NaOH}(s), \quad\) methanol, \(\mathrm{CH}_{3} \mathrm{OH}(l)\), and acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH}(a q)\), are highly water-soluble compounds that contain "OH" groups in their formulas. Use your knowledge of bonding and Lewis formulas to explain why sodium hydroxide forms highly basic solutions, solutions of methanol are essentially neutral, and acetic acid readily loses a hydrogen ion to form acidic solutions.

Name the following ionic compounds, which are used in silver-based photography: (a) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{~S}_{2} \mathrm{O}_{5}(s)\) (fixer) (b) \(\mathrm{Na}_{2} \mathrm{SO}_{3}(s)\) (preservative) (c) \(\mathrm{K}_{2} \mathrm{CO}_{3}(s)\) (activator) (d) \(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{5}(s)\) (fixer)

Write the balanced chemical equation for the following reactions: (a) When sulfuric acid is placed on chalk (calcium carbonate), the chalk bubbles, forming a gas. (b) When tin metal is placed in a solution of hydrochloric acid, bubbles form and the metal is slowly dissolved. (c) Magnesium ribbon burns in air with a bright blue flame, leaving behind a white powdery solid residue.
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