Given The Name Of The Ionic Compound, Write The Formula For The Compound That Contains Transition Metals.1. Vanadium(IV) Sulfide - A. VS - B. $VS_2$ - C. $V(SO_4)_2$2. Copper(I) Nitrate - A. $CuNO_3$ - B.

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Introduction

Ionic compounds are formed when two or more elements with different charges combine to form a stable compound. Transition metals, in particular, are known for their ability to form a wide range of ionic compounds with various anions. In this article, we will explore the naming and formula writing of ionic compounds containing transition metals.

Naming Ionic Compounds with Transition Metals

When naming ionic compounds with transition metals, we need to follow a specific set of rules. The name of the compound is typically written in the following format:

  • The name of the cation (transition metal) is written first, followed by the Roman numeral in parentheses indicating the charge of the cation.
  • The name of the anion is written second, with its suffix changed to "-ide" if it is a monatomic anion.

Example 1: Vanadium(IV) Sulfide

The name of the compound is Vanadium(IV) sulfide. To write the formula for this compound, we need to determine the charge of the vanadium ion and the sulfide ion.

  • The charge of the vanadium ion is +4, as indicated by the Roman numeral in parentheses.
  • The charge of the sulfide ion is -2.

To balance the charges, we need to multiply the vanadium ion by 1 and the sulfide ion by 2. Therefore, the formula for Vanadium(IV) sulfide is VS2.

Example 2: Copper(I) Nitrate

The name of the compound is Copper(I) nitrate. To write the formula for this compound, we need to determine the charge of the copper ion and the nitrate ion.

  • The charge of the copper ion is +1, as indicated by the Roman numeral in parentheses.
  • The charge of the nitrate ion is -1.

To balance the charges, we need to multiply the copper ion by 1 and the nitrate ion by 1. Therefore, the formula for Copper(I) nitrate is CuNO3.

Common Transition Metal Compounds

Here are some common transition metal compounds with their formulas:

  • Iron(II) chloride: FeCl2
  • Iron(III) chloride: FeCl3
  • Copper(II) sulfate: CuSO4
  • Nickel(II) carbonate: NiCO3
  • Cobalt(II) nitrate: Co(NO3)2

Conclusion

In conclusion, writing the formula for ionic compounds containing transition metals requires a good understanding of the naming conventions and the charges of the ions involved. By following the rules outlined in this article, you should be able to write the formula for a wide range of transition metal compounds.

Common Mistakes to Avoid

Here are some common mistakes to avoid when writing the formula for ionic compounds containing transition metals:

  • Failing to include the Roman numeral in parentheses to indicate the charge of the cation.
  • Failing to balance the charges of the ions.
  • Using the wrong formula for a compound.

Practice Problems

Here are some practice problems to help you reinforce your understanding of writing the formula for ionic compounds containing transition metals:

  1. Write the formula for Manganese(II) carbonate.
  2. Write the formula for Chromium(III) nitrate.
  3. Write the formula for Iron(II) sulfate.
  4. Write the formula for Copper(II) chloride.
  5. Write the formula for Nickel(II) carbonate.

Answer Key

Here are the answers to the practice problems:

  1. MnCO3
  2. Cr(NO3)3
  3. FeSO4
  4. CuCl2
  5. NiCO3

References

Here are some references that you can use to learn more about ionic compounds and transition metals:

  • "Chemistry: The Central Science" by Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten
  • "General Chemistry" by Linus Pauling
  • "Transition Metal Chemistry" by F. Albert Cotton

Conclusion

Q: What is the difference between a transition metal and a non-transition metal?

A: Transition metals are a group of elements that are located in the d-block of the periodic table. They are characterized by their ability to form ions with different charges and their tendency to form complexes with other ions. Non-transition metals, on the other hand, are elements that are located in the s-block and p-block of the periodic table and do not exhibit these characteristics.

Q: How do I determine the charge of a transition metal ion?

A: To determine the charge of a transition metal ion, you need to look at the Roman numeral in parentheses that is written after the name of the metal. For example, if the name of the compound is Iron(II) chloride, the charge of the iron ion is +2.

Q: What is the difference between a monatomic anion and a polyatomic anion?

A: A monatomic anion is an anion that consists of a single atom, such as chloride (Cl-) or bromide (Br-). A polyatomic anion, on the other hand, is an anion that consists of multiple atoms, such as nitrate (NO3-) or sulfate (SO42-).

Q: How do I write the formula for an ionic compound with a transition metal?

A: To write the formula for an ionic compound with a transition metal, you need to follow these steps:

  1. Determine the charge of the transition metal ion.
  2. Determine the charge of the anion.
  3. Balance the charges by multiplying the transition metal ion by the appropriate number of anions.

Q: What is the difference between a cation and an anion?

A: A cation is a positively charged ion, while an anion is a negatively charged ion. Cations are typically formed by the loss of electrons from a metal atom, while anions are typically formed by the gain of electrons by a nonmetal atom.

Q: How do I determine the charge of a cation?

A: To determine the charge of a cation, you need to look at the Roman numeral in parentheses that is written after the name of the metal. For example, if the name of the compound is Copper(I) nitrate, the charge of the copper ion is +1.

Q: What is the difference between a strong acid and a weak acid?

A: A strong acid is an acid that completely dissociates in water to produce hydrogen ions (H+), while a weak acid is an acid that only partially dissociates in water to produce hydrogen ions.

Q: How do I write the formula for an acid?

A: To write the formula for an acid, you need to follow these steps:

  1. Determine the charge of the hydrogen ion.
  2. Determine the charge of the anion.
  3. Balance the charges by multiplying the hydrogen ion by the appropriate number of anions.

Q: What is the difference between a base and an acid?

A: A base is a substance that accepts hydrogen ions (H+) to form a salt and water, while an acid is a substance that donates hydrogen ions (H+) to form a salt and water.

Q: How do I write the formula for a base?

A: To write the formula for a base, you need to follow these steps:

  1. Determine the charge of the hydroxide ion.
  2. Determine the charge of the cation.
  3. Balance the charges by multiplying the hydroxide ion by the appropriate number of cations.

Conclusion

In conclusion, writing the formula for ionic compounds with transition metals requires a good understanding of the naming conventions and the charges of the ions involved. By following the rules outlined in this article and practicing with the practice problems, you should be able to write the formula for a wide range of transition metal compounds.