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Chapter 2: Problem 69

Give the names and charges of the cation and anion in each of the following compounds: $(\mathbf{a}) \mathrm{CaO},(\mathbf{b}) \mathrm{Na}_{2} \mathrm{SO}_{4},(\mathbf{c}) \mathrm{KClO}_{4},$ (d) \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}\), (e) \(\mathrm{Cr}(\mathrm{OH})_{3}\)

Short Answer

Expert verified
a) \(\mathrm{CaO}\): Cation: Calcium ion \(\mathrm{(Ca^{2+})}\), Anion: Oxide ion \(\mathrm{(O^{2-})}\) b) \(\mathrm{Na_2SO_4}\): Cation: Sodium ion \(\mathrm{(Na^{+})}\), Anion: Sulfate ion \(\mathrm{(SO_4^{2-})}\) c) \(\mathrm{KClO_4}\): Cation: Potassium ion \(\mathrm{(K^{+})}\), Anion: Perchlorate ion \(\mathrm{(ClO_4^{-})}\) d) \(\mathrm{Fe(NO_3)_2}\): Cation: Iron(II) ion \(\mathrm{(Fe^{2+})}\), Anion: Nitrate ion \(\mathrm{(NO_3^{-})}\) e) \(\mathrm{Cr(OH)_3}\): Cation: Chromium(III) ion \(\mathrm{(Cr^{3+})}\), Anion: Hydroxide ion \(\mathrm{(OH^{-})}\)

Step by step solution

01

a) CaO (Calcium Oxide)

Calcium oxide has two elements: Calcium (Ca) and Oxygen (O). Calcium is in Group 2 of the periodic table, so it loses two electrons and forms a cation with a charge of +2. The chemical symbol with its charge for the cation is: \(\mathrm{Ca^{2+}}\). Oxygen is in Group 6 and gains two electrons to complete its octet, forming an anion with a charge of -2. The chemical symbol with its charge for the anion is: \(\mathrm{O^{2-}}\). Cation: Calcium ion \(\mathrm{(Ca^{2+})}\) Anion: Oxide ion \(\mathrm{(O^{2-})}\)
02

b) Na2SO4 (Sodium Sulfate)

Sodium sulfate has three elements: Sodium (Na), Sulfur (S), and Oxygen (O). Sodium is in Group 1 of the periodic table, so it loses one electron and forms a cation with a charge of +1. The chemical symbol with its charge for the cation is: \(\mathrm{Na^{+}}\). The anion in the compound is the sulfate ion (SO4). Sulfate is a polyatomic ion with a charge of -2. The chemical symbol with its charge for the anion is: \(\mathrm{SO_4^{2-}}\). Cation: Sodium ion \(\mathrm{(Na^{+})}\) Anion: Sulfate ion \(\mathrm{(SO_4^{2-})}\)
03

c) KClO4 (Potassium Perchlorate)

Potassium perchlorate has three elements: Potassium (K), Chlorine (Cl), and Oxygen (O). Potassium is in Group 1 of the periodic table, so it loses one electron and forms a cation with a charge of +1. The chemical symbol with its charge for the cation is: \(\mathrm{K^{+}}\). The anion in the compound is the perchlorate ion (ClO4). Perchlorate is a polyatomic ion with a charge of -1. The chemical symbol with its charge for the anion is: \(\mathrm{ClO_4^{-}}\). Cation: Potassium ion \(\mathrm{(K^{+})}\) Anion: Perchlorate ion \(\mathrm{(ClO_4^{-})}\)
04

d) Fe(NO3)2 (Iron(II) Nitrate)

Iron(II) nitrate has two elements: Iron (Fe) and the polyatomic ion Nitrate (NO3). The charge of Iron (Fe) in this compound is +2 as given in the name. The chemical symbol with its charge for the cation is: \(\mathrm{Fe^{2+}}\). The anion in the compound is the nitrate ion (NO3). Nitrate is a polyatomic ion with a charge of -1. The chemical symbol with its charge for the anion is: \(\mathrm{NO_3^{-}}\). Cation: Iron(II) ion \(\mathrm{(Fe^{2+})}\) Anion: Nitrate ion \(\mathrm{(NO_3^{-})}\)
05

e) Cr(OH)3 (Chromium(III) Hydroxide)

Chromium(III) hydroxide has two elements: Chromium (Cr) and the polyatomic ion Hydroxide (OH). The charge of Chromium (Cr) in this compound is +3 as given in the name. The chemical symbol with its charge for the cation is: \(\mathrm{Cr^{3+}}\). The anion in the compound is the hydroxide ion (OH). Hydroxide is a polyatomic ion with a charge of -1. The chemical symbol with its charge for the anion is: \(\mathrm{OH^{-}}\). Cation: Chromium(III) ion \(\mathrm{(Cr^{3+})}\) Anion: Hydroxide ion \(\mathrm{(OH^{-})}\)

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Most popular questions from this chapter

There are two different isotopes of bromine atoms. Under normal conditions, elemental bromine consists of \(\mathrm{Br}_{2}\) molecules, and the mass of a \(\mathrm{Br}_{2}\) molecule is the sum of the masses of the two atoms in the molecule. The mass spectrum of \(\mathrm{Br}_{2}\) consists of three peaks: $$ \begin{array}{lc} \hline \text { Mass (u) } & \text { Relative Size } \\ \hline 157.836 & 0.2569 \\ 159.834 & 0.4999 \\ 161.832 & 0.2431 \\ \hline \end{array} $$ (a) What is the origin of each peak (of what isotopes does each consist)? (b) What is the mass of each isotope? (c) Determine the average molecular mass of a \(\mathrm{Br}_{2}\) molecule. (d) Determine the average atomic mass of a bromine atom. (e) Calculate the abundances of the two isotopes.

The element chromium (Cr) consists of four naturally occurring isotopes with atomic masses 49.9460,51.9405,52.9407 , and \(53.9389 \mathrm{u}\). The relative abundances of these four isotopes are \(4.3,83.8,9.5,\) and \(2.4 \%\), respectively. From these data, calculate the atomic weight of chromium.

Two substances have the same molecular and empirical formulas. Does this mean that they must be the same compound?

How many of the indicated atoms are represented by each chemical formula: (a) carbon atoms in \(\mathrm{C}_{4} \mathrm{H}_{9} \mathrm{COOCH}_{3}\),(b) oxygen atoms in \(\mathrm{Ca}\left(\mathrm{ClO}_{3}\right)_{2}\), (c) hydrogen atoms in \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4} ?\)

(a) Define atomic number and mass number. (b) Which of these can vary without changing the identity of the element?
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