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Chapter 2: Problem 44

Write formulas for the following ionic compounds. (a) hydrochloric acid (b) sodium nitrite (c) chromium(III) sulfite (d) potassium chlorate (e) iron(III) perbromate

Short Answer

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Question: Write the chemical formulas for the following ionic compounds: (a) Hydrochloric acid, (b) Sodium nitrite, (c) Chromium(III) sulfite, (d) Potassium chlorate, (e) Iron(III) perbromate. Answer: (a) HCl, (b) NaNO_2, (c) Cr_2(SO_3)_3, (d) KClO_3, (e) Fe(BrO_4)_3.

Step by step solution

01

(Identify Ions)

First, it is important to know the common ions and their charges. For each compound, determine the cation (positive ion) and the anion (negative ion) present, along with their respective charges. (a) Hydrochloric acid cation: H^+ (hydrogen ion) anion: Cl^- (chloride ion) (b) Sodium nitrite cation: Na^+ (sodium ion) anion: NO_2^- (nitrite ion) (c) Chromium(III) sulfite cation: Cr^{3+} (chromium(III) ion) anion: SO_3^{2-} (sulfite ion) (d) Potassium chlorate cation: K^+ (potassium ion) anion: ClO_3^- (chlorate ion) (e) Iron(III) perbromate cation: Fe^{3+} (iron(III) ion) anion: BrO_4^- (perbromate ion) ##Step 2: Write the chemical formulas for each compound##
02

(Write the Formulas)

To write the chemical formula for each compound, combine the cations and anions with subscripts according to their charges, so that the overall charge of the compound is neutral. (a) Hydrochloric acid Formula: HCl (since the charges of H^+ and Cl^- are equal and opposite) (b) Sodium nitrite Formula: NaNO_2 (since the charges of Na^+ and NO_2^- are equal and opposite) (c) Chromium(III) sulfite Formula: Cr_2(SO_3)_3 (requires 2 Cr^{3+} ions and 3 SO_3^{2-} ions to form a neutral compound) (d) Potassium chlorate Formula: KClO_3 (since the charges of K^+ and ClO_3^- are equal and opposite) (e) Iron(III) perbromate Formula: Fe(BrO_4)_3 (requires 1 Fe^{3+} ion and 3 BrO_4^- ions to form a neutral compound)

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Key Concepts

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

Chemical Formulas
Chemical formulas represent the composition of a chemical compound using symbols for the elements and numbers indicating the ratio of atoms. For ionic compounds, formulas are derived from the combination of cations and anions. Each formula reflects the specific ratio needed to balance the overall electrical charge of the compound.
  • In single-element ions or simple ionic compounds, the formula is straightforward, like in hydrochloric acid (HCl), where one hydrogen ion combines with one chloride ion.
  • For more complex compounds, the formula becomes a reflection of balancing the charges, such as in chromium(III) sulfite, Cr鈧�(SO鈧�)鈧�. This indicates that two chromium ions combine with three sulfite ions.
Understanding how to write these formulas is crucial for identifying the composition and structure of ionic compounds. Each compound has a unique formula that provides insight into the types and numbers of ions present.
Cation and Anion Identification
Ions are charged particles that form when atoms gain or lose electrons.
  • Cations are positively charged ions that form when atoms lose electrons.
  • Anions are negatively charged ions that form when atoms gain electrons.
Identifying the cation and anion within an ionic compound is the first step towards determining its chemical formula. For example:
  • In sodium nitrite, NaNO鈧�, sodium (Na) is the cation, while nitrite (NO鈧�) is the anion.
  • In iron(III) perbromate, Fe(BrO鈧�)鈧�, iron (Fe) acts as the cation, combined with perbromate (BrO鈧�) anions.
Correctly identifying these ions and their charges helps ensure that the resulting formula accurately reflects the compound's composition.
Neutral Charge Balancing
In ionic compounds, the total positive charge must balance the total negative charge to achieve neutrality. This neutral charge balancing is the foundation for writing correct chemical formulas. Each ion carries a specific charge, which must be considered when combining them.
To achieve neutrality in ionic compounds:
  • Identify the charge of each ion involved. For instance, chromium(III) has a charge of +3, while sulfite carries a charge of -2.
  • Calculate how many of each ion is needed to balance the charges. In chromium(III) sulfite, two +3 chromium ions are balanced by three -2 sulfite ions, resulting in the neutral formula Cr鈧�(SO鈧�)鈧�.
This balancing act ensures that all ionic compounds follow the fundamental rule of net zero charge.
Common Ions and Their Charges
Familiarity with common ions and their standard charges is essential when dealing with ionic compounds. Many elements form predictable ions, which can help in quickly constructing formulas.
Some typical cations include:
  • Hydrogen (H鈦�)
  • Sodium (Na鈦�)
  • Potassium (K鈦�)
  • Iron(III) (Fe鲁鈦�)
And typical anions include:
  • Chloride (Cl鈦�)
  • Nitrite (NO鈧傗伝)
  • Sulfite (SO鈧兟测伝)
  • Chlorate (ClO鈧冣伝)
  • Perbromate (BrO鈧勨伝)
Knowing these ions and their charges allows you to efficiently combine them in formulas, as seen with sodium nitrite (NaNO鈧�) and potassium chlorate (KClO鈧�). This foundational knowledge makes it easier to consistently perform charge balancing and write accurate chemical formulas.

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Most popular questions from this chapter

Identify the following elements: (a) A member of the same period as tellurium with two fewer protons than tellurium. (b) A transition metal in Group 5, period 4. (c) An alkali with 55 protons. (d) A metalloid in Group 15 with more than 40 protons.

Consider the elements oxygen, fluorine, argon, sulfur, potassium, and strontium. From this group of elements, which ones fit the descriptions below? (a) Two elements that are metals. (b) Four elements that are nonmetals. (c) Three elements that are solid at room temperature. (d) An element that is found in nature as \(\mathrm{X}_{8}\). (e) One pair of elements that may form a molecular compound. (f) One pair of elements that may form an ionic compound with formula \(\mathrm{AX}\) (g) One pair of elements that may form an ionic compound with formula \(\mathrm{AX}_{2}\) (h) One pair of elements that may form an ionic compound with formula \(\mathrm{A}_{2} \mathrm{X} .\) (i) An element that can form no compounds. (j) Three elements that are gases at room temperature.

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