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Name the following ionic compounds: (a) \(\mathrm{MgO}\), (b) \(\mathrm{AlCl}_{3}\), (c) \(\mathrm{Li}_{3} \mathrm{PO}_{4}\), (d) \(\mathrm{Ba}\left(\mathrm{ClO}_{4}\right)_{2}\), (e) \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\) (f) \(\mathrm{Fe}(\mathrm{OH})_{2},(\mathrm{~g}) \mathrm{Ca}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}\), (h) \(\mathrm{Cr}_{2}\left(\mathrm{CO}_{3}\right)_{3}\), (i) \(\mathrm{K}_{2} \mathrm{CrO}_{4}\) (j) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\)

Short Answer

Expert verified
(a) Magnesium oxide (b) Aluminum chloride (c) Lithium phosphate (d) Barium perchlorate (e) Copper(II) nitrate (f) Iron(II) hydroxide (g) Calcium acetate (h) Chromium(III) carbonate (i) Potassium chromate (j) Ammonium sulfate

Step by step solution

01

Identify cations and anions in each compound

For each compound, let's identify the cation and anion and list them for easier use in naming the compound. (a) \(\mathrm{MgO}:\) Cation = \(\mathrm{Mg}^{2+}\) (magnesium), Anion = \(\mathrm{O}^{2-}\) (oxide) (b) \(\mathrm{AlCl}_{3}:\) Cation = \(\mathrm{Al}^{3+}\) (aluminum), Anion = \(\mathrm{Cl}^{-}\) (chloride) (c) \(\mathrm{Li}_{3} \mathrm{PO}_{4}:\) Cation = \(\mathrm{Li}^{+}\) (lithium), Anion = \(\mathrm{PO}_{4}^{3-}\) (phosphate) (d) \(\mathrm{Ba}\left(\mathrm{ClO}_{4}\right)_{2}:\) Cation = \(\mathrm{Ba}^{2+}\) (barium), Anion = \(\mathrm{ClO}_{4}^{-}\) (perchlorate) (e) \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}:\) Cation = \(\mathrm{Cu}^{2+}\) (copper(II)), Anion = \(\mathrm{NO}_{3}^{-}\) (nitrate) (f) \(\mathrm{Fe}(\mathrm{OH})_{2}:\) Cation = \(\mathrm{Fe}^{2+}\) (iron(II)), Anion = \(\mathrm{OH}^{-}\) (hydroxide) (g) \(\mathrm{Ca}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}:\) Cation = \(\mathrm{Ca}^{2+}\) (calcium), Anion = \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\) (acetate) (h) \(\mathrm{Cr}_{2}\left(\mathrm{CO}_{3}\right)_{3}:\) Cation = \(\mathrm{Cr}^{3+}\) (chromium(III)), Anion = \(\mathrm{CO}_{3}^{2-}\) (carbonate) (i) \(\mathrm{K}_{2} \mathrm{CrO}_{4}:\) Cation = \(\mathrm{K}^{+}\) (potassium), Anion = \(\mathrm{CrO}_{4}^{2-}\) (chromate) (j) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}:\) Cation = \(\mathrm{NH}_{4}^{+}\) (ammonium), Anion = \(\mathrm{SO}_{4}^{2-}\) (sulfate)
02

Combine cation and anion names

Now that we have identified the cation and anion for each compound, let's combine their names to form the name of the compound. (a) Magnesium oxide (b) Aluminum chloride (c) Lithium phosphate (d) Barium perchlorate (e) Copper(II) nitrate (f) Iron(II) hydroxide (g) Calcium acetate (h) Chromium(III) carbonate (i) Potassium chromate (j) Ammonium sulfate

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Key Concepts

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

Naming Ionic Compounds
Naming ionic compounds can seem tricky at first, but with a few simple rules, it becomes straightforward. Ionic compounds consist of positive and negative ions held together by ionic bonds.
When naming these, first identify the cation (positive ion) and the anion (negative ion). The name of the cation is stated first followed by the name of the anion.
  • If the cation is a metal from groups 1, 2, or transitional metals with a known charge, simply write the metal's name (e.g., magnesium for \( \text{Mg}^{2+} \) ).
  • If the metal can form more than one type of cation, like copper (Cu), specify its charge using Roman numerals in parentheses, such as copper(II) for \( \text{Cu}^{2+} \) .
  • The name of the anion usually ends with "-ide" if it is a simple anion like chloride (\( \text{Cl}^{-} \) ), "-ate" or “-ite” if it’s a polyatomic ion such as sulfate (\( \text{SO}_4^{2-} \) ).

Examples include magnesium oxide (\( \text{MgO} \)) and lithium phosphate (\( \text{Li}_3 \text{PO}_4 \)). With practice, naming ionic compounds becomes much easier.
Cations and Anions
Cations and anions are the building blocks of ionic compounds. Cations are positively charged ions, while anions carry a negative charge.
These charges result from a metal losing electrons and a non-metal gaining those electrons, respectively.
  • Cations are often metals. For instance, a magnesium ion \( \text{Mg}^{2+} \) is a cation that has lost two electrons.
  • Anions are often non-metals or polyatomic ions, tables. Oxygen becomes an oxide ion \( \text{O}^{2-} \), by gaining two electrons.

In transition metals and some post-transition metals, multiple charges may be possible and are denoted using Roman numerals such as iron(II) \( \text{Fe}^{2+} \) . Unlike a trickle of water, ions engage in a captivating dance of attractions with their opposite charges guiding their every move.

The balance between these charges is crucial because it ensures the compound is neutral, having an overall charge of zero.
Polyatomic Ions
Polyatomic ions consist of multiple atoms bonded together that function as a single ion with a positive or negative charge. They are often critical components of ionic compounds.
The atoms in a polyatomic ion are covalently bonded, but the ion itself forms ionic bonds with cations or anions.
  • Common polyatomic ions include nitrate (\( \text{NO}_3^{-} \)), sulfate (\( \text{SO}_4^{2-} \)), and phosphate (\( \text{PO}_4^{3-} \)).
  • When included in ionic compounds, the polyatomic ion is treated as a single unit. For instance, in ammonium sulfate \( (\text{NH}_4)_2\text{SO}_4 \), ammonium \( \text{NH}_4^+ \) and sulfate \( \text{SO}_4^{2-} \) ions work together to create a stable compound.

These ions have their unique names, which are essential to learn, as their presence alters the naming and writing of chemical formulas. Polyatomic ions transform the naming game, asking you to find balance along with color connections in a complex world.

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Most popular questions from this chapter

Provide the name or chemical formula, as appropriate, for each of the following acids: (a) hydrobromic acid, (b) hydrosulfuric acid, (c) nitrous acid, (d) \(\mathrm{H}_{2} \mathrm{CO}_{3}\), (e) \(\mathrm{HClO}_{3}\), (f) \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\).

The compound cyclohexane is an alkane in which six carbon atoms form a ring. The partial structural formula of the compound is as follows: (a) Complete the structural formula for cyclohexane. (b) Is the molecular formula for cyclohexane the same as that for \(n\) -hexane, in which the carbon atoms are in a straight line? If possible, comment on the source of any differences. (c) Propose a structural formula for cyclohexanol, the alcohol derived from cycIohexane.

Write the correct symbol, with both superscript and subscript, for each of the following. Use the list of elements inside the front cover as needed: (a) the isotope of platinum that contains 118 neutrons, (b) the isotope of krypton with mass number \(84,(\mathrm{c})\) the isotope of arsenic with mass number 75, (d) the isotope of magnesium that has an equal number of protons and neutrons.

Carbonic acid occurs in carbonated beverages. When allowed to react with lithium hydroxide it produces lithium carbonate. Lithium carbonate is used to treat depression and bipolar disorder. Write chemical formulas for carbonic acid, lithium hydroxide, and lithium carbonate.

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

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