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Chapter 2: Problem 136

Write formulas for the following compounds: (a) Calcium acetate (b) Iron(II) cyanide (c) Sodium dichromate (d) Chromium(III) sulfate (e) Mercury(II) perchlorate

Short Answer

Expert verified
(a) \(\text{Ca(CH}_3\text{COO})_2\), (b) \(\text{Fe(CN)}_2\), (c) \(\text{Na}_2\text{Cr}_2\text{O}_7\), (d) \(\text{Cr}_2(\text{SO}_4)_3\), (e) \(\text{Hg(ClO}_4)_2\).

Step by step solution

01

Identify Ions

Identify the ions involved in the compounds: (a) Calcium acetate is composed of calcium ions ( ext{Ca}^{2+}) and acetate ions ( ext{CH}_3 ext{COO}^-). (b) Iron(II) cyanide involves iron(II) ions ( ext{Fe}^{2+}) and cyanide ions ( ext{CN}^-). (c) Sodium dichromate involves sodium ions ( ext{Na}^+) and dichromate ions ( ext{Cr}_2 ext{O}_7^{2-}). (d) Chromium(III) sulfate involves chromium(III) ions ( ext{Cr}^{3+}) and sulfate ions ( ext{SO}_4^{2-}). (e) Mercury(II) perchlorate involves mercury(II) ions ( ext{Hg}^{2+}) and perchlorate ions ( ext{ClO}_4^-).
02

Balance Charges

Balance the charges to determine the correct ratio of ions for each compound: (a) Calcium acetate: ext{Ca}^{2+} balances with two ext{CH}_3 ext{COO}^- ions, so the formula is ext{Ca(CH}_3 ext{COO})_2. (b) Iron(II) cyanide: ext{Fe}^{2+} balances with two ext{CN}^- ions, so the formula is ext{Fe(CN)}_2. (c) Sodium dichromate: Two ext{Na}^+ ions balance one ext{Cr}_2 ext{O}_7^{2-}, so the formula is ext{Na}_2 ext{Cr}_2 ext{O}_7. (d) Chromium(III) sulfate: Two ext{Cr}^{3+} ions balance with three ext{SO}_4^{2-} ions, so the formula is ext{Cr}_2( ext{SO}_4)_3. (e) Mercury(II) perchlorate: ext{Hg}^{2+} balances with two ext{ClO}_4^- ions, so the formula is ext{Hg(ClO}_4)_2.

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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 atoms transfer electrons among each other, resulting in charged particles called ions. These ions are held together by strong electrostatic forces between oppositely charged ions, creating a lattice structure.
  • Cations are positively charged ions formed when an atom loses one or more electrons.
  • Anions are negatively charged ions formed when an atom gains electrons.
Ionic compounds are typically formed from a metal and a non-metal. Understanding the nature of ionic compounds is essential, especially when writing chemical formulas, as these require balancing of charges to achieve neutrality.
Balance Charges
When writing chemical formulas for ionic compounds, it's critical to ensure that the resultant compound is electrically neutral. This involves balancing the positive charges of the cations with the negative charges of the anions. For each compound:
  • Identify the charge of the cation and the anion.
  • Determine the ratio of ions that will result in zero net charge.
For example, calcium acetate results in the formula \(\text{Ca(CH}_3\text{COO})_2\) as two acetate ions each with a charge of \(-1\) are needed to balance one calcium ion with a charge of \(+2\). Always keep in mind that the total positive charge must equal the total negative charge.
Cation and Anion Identification
Identifying cations and anions is a foundational step for writing chemical formulas for ionic compounds. The cation is generally the metal and is listed first in the chemical name, while the anion is typically a non-metal or polyatomic ion.
  • The cation maintains its elemental name (e.g., sodium remains sodium).
  • Anions have modified names often ending in "-ide" for simple ions (e.g., chloride from chlorine) or take the name of the polyatomic ion (e.g., sulfate).
For instance, in chromium(III) sulfate, \(\text{Cr}^{3+}\) is the cation, and \(\text{SO}_4^{2-}\) is the anion. Recognizing the right composition of cations and anions ensures accurate formulation of chemical compounds.
Naming Chemical Compounds
Naming chemical compounds involves several rules that help in conveying the specific composition of the compound.
  • The cation is always named first, followed by the anion.
  • If the cation can have more than one possible charge (transition metals), the charge is specified in Roman numerals within parentheses.
  • For polyatomic ions, common names are used, such as acetate or cyanide.
Taking mercury(II) perchlorate as an example, "mercury(II)" indicates that mercury is in the +2 oxidation state, and "perchlorate" specifies the anion \(\text{ClO}_4^-\). This systematic approach to naming helps in identifying the proper ionic formula and understanding the composition of the compound.

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Most popular questions from this chapter

Write formulas for the following binary compounds: (a) Vanadium(III) chloride (b) Manganese(IV) oxide (c) Copper(II) sulfide (d) Aluminum oxide

Ibuprofen was initially synthesized by a process developed by Boots Co. in the \(1960 \mathrm{~s}\). Six reaction steps were utilized, and the percent atom economy was \(40 \%\). For every one mole of ibuprofen produced, 1 mole of Na, 23 moles of \(\mathrm{H}, 1\) mole of \(\mathrm{N}, 7\) moles of \(\mathrm{C}\), 8 moles of \(\mathrm{O}\), and 1 mole of \(\mathrm{Cl}\) were unused and considered as waste. (a) Calculate the mass (g) of each element wasted for every one mole of ibuprofen produced. (b) Calculate the total mass ( \(\mathrm{g}\) ) wasted for every one mole of ibuprofen produced. (c) Yearly production of ibuprofen is approximately 30 million lbs, which is equivalent to \(6.6 \times 10^{7}\) moles. Calculate the total mass (kg) of matter wasted in the annual production ibuprofen.

Write formulas for the following binary compounds: (a) Potassium chloride (b) Tin(II) bromide (c) Calcium oxide (d) Barium chloride (e) Aluminum hydride

What are the formulas of the compounds formed from the following ions? (a) \(\mathrm{Na}^{+}\) and \(\mathrm{NO}_{3}^{-}\) (b) \(\mathrm{K}^{+}\) and \(\mathrm{SO}_{4}^{2-}\) (c) \(\mathrm{Sr}^{2+}\) and \(\mathrm{Cl}^{-}\)

If the atomic weight of an element is \(x\), what is the mass in grams of \(6.02 \times 10^{23}\) atoms of the element? How does your answer compare numerically with the atomic weight of element \(x ?\)
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