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Magazine Chapter 6: Problem 33
The following compounds contain ions that are required in small amounts by the body. Write the formula for each: a. potassium phosphide b. copper(II) chloride c. iron(III) bromide d. magnesium oxide
Short Answer
Expert verified
a. \(K_3P\) b. \(CuCl_2\) c. \(FeBr_3\) d. \(MgO\)
Step by step solution
01
- Identify the Ions for Potassium Phosphide
Potassium forms a cation with a +1 charge, represented as \(K^+\). Phosphide forms an anion with a -3 charge, represented as \(P^{3-}\). The formula should balance the total positive and negative charges.
02
- Write the Balanced Formula for Potassium Phosphide
To balance the charges, we need 3 potassium ions (\(K^+\)) for every phosphide ion (\(P^{3-}\)). Therefore, the formula is \(K_3P\).
03
- Identify the Ions for Copper(II) Chloride
Copper(II) indicates a copper ion with a +2 charge, \(Cu^{2+}\). Chloride forms an anion with a -1 charge, \(Cl^-\). The formula should balance these charges.
04
- Write the Balanced Formula for Copper(II) Chloride
To balance the charges, we need 2 chloride ions (\(Cl^-\)) for every copper ion (\(Cu^{2+}\)). The formula is \(CuCl_2\).
05
- Identify the Ions for Iron(III) Bromide
Iron(III) indicates an iron ion with a +3 charge, \(Fe^{3+}\). Bromide forms an anion with a -1 charge, \(Br^-\). The formula should balance these charges.
06
- Write the Balanced Formula for Iron(III) Bromide
To balance the charges, we need 3 bromide ions (\(Br^-\)) for every iron ion (\(Fe^{3+}\)). The formula is \(FeBr_3\).
07
- Identify the Ions for Magnesium Oxide
Magnesium forms a cation with a +2 charge, \(Mg^{2+}\). Oxide forms an anion with a -2 charge, \(O^{2-}\). The formula should balance these charges.
08
- Write the Balanced Formula for Magnesium Oxide
Since the charges are already balanced with one magnesium ion (\(Mg^{2+}\)) and one oxide ion (\(O^{2-}\)), the formula is \(MgO\).
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Potassium Phosphide
Potassium phosphide is a compound formed by the combination of potassium ions and phosphide ions. Potassium, a Group 1 element on the periodic table, is a metal that loses one electron to form a cation with a +1 charge, represented as K+. Phosphide, a non-metal, gains three electrons to form an anion with a -3 charge, represented as P3-.
To write the chemical formula for potassium phosphide, we need to balance the total positive and negative charges.
To write the chemical formula for potassium phosphide, we need to balance the total positive and negative charges.
- Since one phosphide ion carries a -3 charge, it will need to be balanced by three potassium ions, each with a +1 charge.
- The balanced chemical formula is K3P.
Copper(II) Chloride
Copper(II) chloride is formed by the combination of copper ions and chloride ions. The (II) in copper(II) chloride signifies that the copper ion has a +2 charge, represented as Cu2+.
The chloride ion, being a Group 17 element, forms an anion with a -1 charge, denoted as Cl-.
To write the chemical formula:
The chloride ion, being a Group 17 element, forms an anion with a -1 charge, denoted as Cl-.
To write the chemical formula:
- Since one copper ion carries a +2 charge, it will need to be balanced by two chloride ions, each with a -1 charge.
- Thus, the chemical formula is CuCl2.
Iron(III) Bromide
Iron(III) bromide involves the combination of iron ions with bromide ions. The (III) in iron(III) bromide indicates that the iron ion has a +3 charge, represented as Fe3+.
Bromide ions form from bromine, a Group 17 element, carrying a -1 charge, denoted as Br-.
To write the chemical formula for iron(III) bromide:
Bromide ions form from bromine, a Group 17 element, carrying a -1 charge, denoted as Br-.
To write the chemical formula for iron(III) bromide:
- A single iron ion carrying a +3 charge needs to be balanced by three bromide ions, each with a -1 charge.
- Thus, the balanced chemical formula is FeBr3.
Magnesium Oxide
Magnesium oxide is formed by the combination of magnesium ions and oxide ions. Magnesium, a Group 2 element, loses two electrons to form a cation with a +2 charge, represented as Mg2+.
Oxygen gains two electrons to form an anion with a -2 charge, denoted as O2-.
Writing the formula for magnesium oxide:
Oxygen gains two electrons to form an anion with a -2 charge, denoted as O2-.
Writing the formula for magnesium oxide:
- Since one magnesium ion carrying a +2 charge is perfectly balanced by one oxide ion carrying a -2 charge, they combine in a 1:1 ratio.
- Hence, the chemical formula for magnesium oxide is MgO.
