What is the compound formed when Ag+ and Cl- combine?
Formation of Ionic Compounds: Silver Chloride
The question asks to identify the compound formed when silver ions ($\text{Ag}^+$) and chloride ions ($\text{Cl}^-$) combine.
Ionic compounds are formed by the electrostatic attraction between positively charged ions (cations) and negatively charged ions (anions). In this case, we have the silver cation ($\text{Ag}^+$) and the chloride anion ($\text{Cl}^-$).
The charge of the silver ion is $+1$ ($\text{Ag}^+$). The charge of the chloride ion is $-1$ ($\text{Cl}^-$).
To form a neutral ionic compound, the total positive charge must balance the total negative charge. Here, a $+1$ charge from one $\text{Ag}^+$ ion perfectly balances a $-1$ charge from one $\text{Cl}^-$ ion.
Therefore, one silver ion combines with one chloride ion. The chemical formula for the compound formed is $\text{AgCl}$.
The naming convention for simple ionic compounds is to state the name of the cation first, followed by the name of the anion with its ending changed to '-ide'. Thus, the compound formed from silver ($\text{Ag}^+$) and chloride ($\text{Cl}^-$) is called Silver Chloride.
Let's examine the given options:
- Argon Chlorate: Argon ($\text{Ar}$) is a noble gas and generally does not form chemical compounds easily. Chlorate is a polyatomic ion ($\text{ClO}_3^-$). This option is incorrect.
- Argon Chloride: Similar to Argon Chlorate, Argon does not readily form chlorides. This option is incorrect.
- Silver Chloride: This matches the compound formed from $\text{Ag}^+$ and $\text{Cl}^-$ ions, which is $\text{AgCl}$. This option is correct.
- Silver Chlorate: Silver combines with the chlorate ion ($\text{ClO}_3^-$) to form Silver Chlorate ($\text{AgClO}_3$). This is not the compound formed with just the chloride ion ($\text{Cl}^-$). This option is incorrect.
Based on the analysis, the compound formed when $\text{Ag}^+$ and $\text{Cl}^-$ combine is Silver Chloride.
Revision Table: Ionic Compound Formation
| Ion 1 | Ion 2 | Charge of Ion 1 | Charge of Ion 2 | Ratio for Neutrality | Formula | Compound Name |
|---|---|---|---|---|---|---|
| Silver ($\text{Ag}$) | Chloride ($\text{Cl}$) | $+1$ | $-1$ | $1:1$ ($\text{Ag}^+:\text{Cl}^-$) | $\text{AgCl}$ | Silver Chloride |
| Sodium ($\text{Na}$) | Chloride ($\text{Cl}$) | $+1$ | $-1$ | $1:1$ ($\text{Na}^+:\text{Cl}^-$) | $\text{NaCl}$ | Sodium Chloride |
| Magnesium ($\text{Mg}$) | Chloride ($\text{Cl}$) | $+2$ | $-1$ | $1:2$ ($\text{Mg}^{2+}:\text{Cl}^-$) | $\text{MgCl}_2$ | Magnesium Chloride |
Additional Information: Properties of Silver Chloride
Silver Chloride ($\text{AgCl}$) is an inorganic compound. It is a white crystalline solid. A key property of Silver Chloride is its very low solubility in water. This low solubility makes it useful in various applications, particularly in precipitation reactions used in chemistry to test for the presence of chloride ions.
- Chemical Formula: $\text{AgCl}$
- Appearance: White solid
- Solubility: Very low solubility in water
- Light Sensitivity: Silver chloride is sensitive to light and decomposes into silver and chlorine gas when exposed to light, which is why it was historically used in photography.
Understanding how ions combine based on their charges is fundamental to predicting the formulas and names of ionic compounds like Silver Chloride.
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