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Magazine Chapter 2: Problem 86
Write the formula for each of the following compounds: a. ammonium hydrogen phosphate b. mercury(1) sulfide c. silicon dioxide d. sodium sulfite e. aluminum hydrogen sulfate f. nitrogen trichloride g. hydrobromic acid h. bromous acid i. perbromic acid j. potassium hydrogen sulfide k. calcium iodide I, cesium perchlorate
Short Answer
Expert verified
a. \((NH_4)_2HPO_4\)
b. \(Hg_2S\)
c. \(SiO_2\)
d. \(Na_2SO_3\)
e. \(Al_2(HSO_4)_3\)
f. \(NCl_3\)
g. \(HBr\)
h. \(HBrO_2\)
i. \(HBrO_4\)
j. \(KHS\)
k. \(CaI_2\)
l. \(CsClO_4\)
Step by step solution
01
a. ammonium hydrogen phosphate
Write the formula using the ions ammonium (NH鈧勨伜), hydrogen (H鈦�), and phosphate (PO鈧劼斥伝). The compound contains one phosphate ion, two ammonium ions, and one hydrogen ion to balance the charges, so the formula is (NH鈧�)鈧侶PO鈧�.
02
b. mercury(1) sulfide
Write the formula with mercury(I) ion (Hg鈧偮测伜) and sulfide ion (S虏鈦�). In this case, there is one mercury(I) ion and one sulfide ion, giving the formula Hg鈧係.
03
c. silicon dioxide
Create a formula using silicon (Si) ions and oxygen ions (O虏鈦�), remembering that silicon typically has a charge of +4. Since two oxygen ions with a charge of -2 balance the charge of silicon, the formula is SiO鈧�.
04
d. sodium sulfite
Write the formula using sodium ions (Na鈦�) and sulfite ions (SO鈧兟测伝). The compound contains one sulfite ion and two sodium ions to balance the charges, resulting in the formula Na鈧係O鈧�.
05
e. aluminum hydrogen sulfate
Make a formula considering aluminum ions (Al鲁鈦�), hydrogen ions (H鈦�), and sulfate ions (SO鈧劼测伝). The compound must have two aluminum ions, one hydrogen ion, and three sulfate ions to achieve a neutral charge, leading to the formula Al鈧�(HSO鈧�)鈧�.
06
f. nitrogen trichloride
Combine nitrogen (N) ions (with a typical charge of -3) with chlorine (Cl) ions (with a charge of -1) to form a neutral compound. The formula is NCl鈧� due to the 1:3 ratio of nitrogen to chlorine atoms, required to balance the charge.
07
g. hydrobromic acid
Write the formula using hydrogen ions (H鈦�) and bromide ions (Br鈦�). Hydrobromic acid is a binary acid, so the formula directly reflects the ions involved: HBr.
08
h. bromous acid
Use hydrogen ions (H鈦�) and bromite ions (BrO鈧傗伝) to form the formula. Bromous acid is an oxyacid with the formula HBrO鈧�.
09
i. perbromic acid
Combine hydrogen ions (H鈦�) with perbromate ions (BrO鈧勨伝) to form the formula. The formula for perbromic acid is HBrO鈧�.
10
j. potassium hydrogen sulfide
Create a formula using potassium ions (K鈦�), hydrogen ions (H鈦�), and sulfide ions (S虏鈦�). For a neutral compound, combine one potassium ion, one hydrogen ion, and one sulfide ion, resulting in the formula KHS.
11
k. calcium iodide
Write the formula using calcium ions (Ca虏鈦�) and iodide ions (I鈦�). The compound consists of one calcium ion and two iodide ions to balance the charges, yielding the formula CaI鈧�.
12
I. cesium perchlorate
Formulate the compound using cesium ions (Cs鈦�) and perchlorate ions (ClO鈧勨伝). The neutral formula consists of one cesium ion and one perchlorate ion, giving the formula CsClO鈧�.
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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 through the electrostatic attraction between positively charged ions (cations) and negatively charged ions (anions). These opposites attract, creating a stable compound. When writing the chemical formula for an ionic compound, it's key to ensure the total positive charge equals the total negative charge, leading to a neutral compound. For example, when combining sodium (
Na鈦�
) with sulfite (
SO鈧僞{2-}
), you need two sodium ions to balance with one sulfite ion, resulting in the formula
Na鈧係O鈧�
. This balance of charges is the cornerstone of writing ionic formulas. It's not only about the elements involved but how their charges interact.
Polyatomic Ions
Polyatomic ions are ions composed of two or more atoms covalently bonded together, carrying an overall charge. Understanding these ions is crucial for the chemistry of compounds. A common example is the ammonium ion (
NH鈧刕+
) and the sulfate ion (
SO鈧刕{2-}
). Polyatomic ions act as a single entity when forming compounds. For instance, ammonium hydrogen phosphate involves ammonium (
NH鈧刕+
), hydrogen (
H^+
), and phosphate (
PO鈧刕{3-}
). Combining these to form a neutral compound gives
(NH鈧�)鈧侶PO鈧�
. Recognizing and remembering the formulas of common polyatomic ions is a useful skill in chemistry.
Acid Nomenclature
Acid nomenclature involves naming compounds that release hydrogen ions,
H^+
, in solution. Different naming laws apply to binary acids, like hydrobromic acid (
HBr
), and oxyacids, which are acids containing oxygen. In oxyacids, the suffix changes depending on the central element's oxidation state. For example, HBrO鈧� is named bromous acid, indicating an intermediate level of oxygen, while HBrO鈧� is perbromic acid, showing a higher oxidation state. Mastery of acid nomenclature requires practice with identifying the type and charge of the acid in question.
Neutral Compound Formation
Neutral compound formation is the balancing act of creating compounds that have no net charge. Each compound's positive and negative components must cancel each other out. Take, for instance, the formation of aluminum hydrogen sulfate,
Al鈧�(HSO鈧�)鈧�
, where you have aluminum (
Al^{3+}
) ions and hydrogen sulfate (
HSO鈧刕{-}
) ions. Achieving neutrality involves ensuring that the total positive charges match the total negative charges: with two aluminum ions (3+ each) and three hydrogen sulfate ions (-1 each), the compound balances to zero. This process is vital for writing correct chemical formulas.
