Problem 41
Question
What are the charges on the ions in an ionic compound containing the elements barium and bromine? Write the formula for the compound.
Step-by-Step Solution
Verified Answer
The charges are \( \text{Ba}^{2+} \) and \( \text{Br}^- \). The formula is \( \text{BaBr}_2 \).
1Step 1: Identify the Elements and their Symbols
Barium is a metal with the chemical symbol \( \text{Ba} \) and bromine is a non-metal with the chemical symbol \( \text{Br} \). In an ionic compound, these two elements will form ions that combine to balance their charges.
2Step 2: Determine the Ion Charges
The first step in determining the charge of the ions is to look at their group numbers in the periodic table. Barium belongs to Group 2, which means it forms cations with a charge of \( +2 \), giving us \( \text{Ba}^{2+} \). Bromine is in Group 17, and typically forms anions with a charge of \( -1 \), resulting in \( \text{Br}^- \).
3Step 3: Balance the Charges to Write the Formula
To create a neutral ionic compound, the charges of the ions must balance. Since \( \text{Ba}^{2+} \) has a charge of +2 and \( \text{Br}^- \) has a charge of -1, you need two bromine ions to balance one barium ion. This gives the formula \( \text{BaBr}_2 \).
4Step 4: Write and Review the Chemical Formula
The correct formula for the ionic compound formed between barium and bromine is \( \text{BaBr}_2 \). This indicates the compound consists of one barium ion and two bromine ions, resulting in a neutral compound with balanced charges.
Key Concepts
Ion ChargesChemical FormulaPeriodic TableNeutral Ionic Compound
Ion Charges
Ion charges play a crucial role in forming ionic compounds. When elements form ions, they either lose or gain electrons to achieve a stable electron configuration. This process leads to the formation of charged particles called ions.
For example, metals like barium tend to lose electrons, forming positive ions or cations. Hence, barium, represented as \( \text{Ba} \), loses two electrons to form \( \text{Ba}^{2+} \) with a charge of +2. On the other hand, non-metals like bromine gain electrons to form negative ions or anions. Bromine forms \( \text{Br}^- \) by gaining one electron and attaining a charge of -1.
Understanding these charges is essential for predicting the formation of ionic compounds. It ensures that compounds are stable and neutral.
For example, metals like barium tend to lose electrons, forming positive ions or cations. Hence, barium, represented as \( \text{Ba} \), loses two electrons to form \( \text{Ba}^{2+} \) with a charge of +2. On the other hand, non-metals like bromine gain electrons to form negative ions or anions. Bromine forms \( \text{Br}^- \) by gaining one electron and attaining a charge of -1.
Understanding these charges is essential for predicting the formation of ionic compounds. It ensures that compounds are stable and neutral.
Chemical Formula
The chemical formula of an ionic compound provides the simplest ratio of the ions involved. It is essential to write the formula correctly to reflect the ratio that balances the overall charge to zero.
For instance, consider barium and bromine forming an ionic compound. Based on their charges, \( \text{Ba}^{2+} \) and \( \text{Br}^- \), the chemical formula is given as \( \text{BaBr}_2 \). This indicates one barium ion combines with two bromide ions to maintain charge neutrality.
The subscript indicates the number of ions needed to balance the charges. Hence, the chemical formula is a clear representation of how ions combine in a specific ratio to form a neutral compound.
For instance, consider barium and bromine forming an ionic compound. Based on their charges, \( \text{Ba}^{2+} \) and \( \text{Br}^- \), the chemical formula is given as \( \text{BaBr}_2 \). This indicates one barium ion combines with two bromide ions to maintain charge neutrality.
The subscript indicates the number of ions needed to balance the charges. Hence, the chemical formula is a clear representation of how ions combine in a specific ratio to form a neutral compound.
Periodic Table
The periodic table is a crucial tool for determining how elements form ions. It provides valuable information about the chemical properties and behavior of elements.
Elements are organized by groups or columns, and the group number helps predict the charge of the ions. For example, elements in Group 2, like barium, typically form ions with a +2 charge. Likewise, elements in Group 17, such as bromine, usually form ions with a -1 charge.
Understanding the arrangement of the periodic table helps determine how elements will react and combine, aiding in the prediction of chemical formulas and the behavior of ionic compounds.
Elements are organized by groups or columns, and the group number helps predict the charge of the ions. For example, elements in Group 2, like barium, typically form ions with a +2 charge. Likewise, elements in Group 17, such as bromine, usually form ions with a -1 charge.
Understanding the arrangement of the periodic table helps determine how elements will react and combine, aiding in the prediction of chemical formulas and the behavior of ionic compounds.
Neutral Ionic Compound
A neutral ionic compound is one where the total positive and negative charges equal zero, resulting in no overall charge.
When forming ionic compounds, ions combine so that the sum of their charges cancels out. For example, in the compound \( \text{BaBr}_2 \), one \( \text{Ba}^{2+} \) ion (with a +2 charge) combines with two \( \text{Br}^- \) ions (each with a -1 charge) to balance out to a neutral state.
This principle of charge balance is fundamental in chemistry, ensuring that compounds formed are stable and without net charge. The ability to form neutral ionic compounds explains much about the properties and stability of substances found in nature.
When forming ionic compounds, ions combine so that the sum of their charges cancels out. For example, in the compound \( \text{BaBr}_2 \), one \( \text{Ba}^{2+} \) ion (with a +2 charge) combines with two \( \text{Br}^- \) ions (each with a -1 charge) to balance out to a neutral state.
This principle of charge balance is fundamental in chemistry, ensuring that compounds formed are stable and without net charge. The ability to form neutral ionic compounds explains much about the properties and stability of substances found in nature.
Other exercises in this chapter
Problem 39
When a potassium atom becomes a monatomic ion, how many electrons does it lose or gain? What noble gas atom has the same number of electrons as a potassium ion?
View solution Problem 40
When oxygen and sulfur atoms become monatomic ions, how many electrons does each lose or gain? Which noble gas atom has the same number of electrons as an oxide
View solution Problem 42
What are the charges of the ions in an ionic compound containing cobalt(III) and fluoride ions? Write the formula for the compound.
View solution Problem 43
Give the formula and the number of each ion that makes up each of the following compounds: (a) \(\mathrm{K}_{2} \mathrm{S}\) (b) \(\cos \mathrm{O}_{4}\) (c) \(\
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