Question

Give the name of each of the following simple binary ionic compounds. a. \(\mathrm{NaBr}\) b. \(\mathrm{MgCl}_{2}\) c. AlP d. \(\operatorname{Sr} B r_{2}\) e. \(\mathrm{AgI}\) f. \(\mathrm{K}_{2} \mathrm{~S}\)

Short answer

The names of the simple binary ionic compounds are: a. Sodium Bromide b. Magnesium Chloride c. Aluminum Phosphide d. Strontium Bromide e. Silver Iodide f. Potassium Sulfide

Step-by-step solution

Determine the elements involved and their charges

First, we need to identify the elements in each compound using their symbols and determine their charges based on their position in the periodic table. a. NaBr: Sodium (Na) and Bromine (Br), Sodium forms a 1+ ion, Bromine forms a 1- ion b. MgCl₂: Magnesium (Mg) and Chlorine (Cl), Magnesium forms a 2+ ion, Chlorine forms a 1- ion c. AlP: Aluminum (Al) and Phosphorus (P), Aluminum forms a 3+ ion, Phosphorus forms a 3- ion d. SrBr₂: Strontium (Sr) and Bromine (Br), Strontium forms a 2+ ion, Bromine forms a 1- ion e. AgI: Silver (Ag) and Iodine (I), Silver forms a 1+ ion, Iodine forms a 1- ion f. K₂S: Potassium (K) and Sulfur (S), Potassium forms a 1+ ion, Sulfur forms a 2- ion

Combine element names

Now, we will combine the names of the elements in each compound using the appropriate rules for naming binary ionic compounds, which involve changing the ending of the second element to "-ide." a. Sodium Bromide b. Magnesium Chloride c. Aluminum Phosphide d. Strontium Bromide e. Silver Iodide f. Potassium Sulfide

Key concepts

Naming Ionic Compounds

When naming binary ionic compounds, the primary goal is to clearly communicate the specific combination of cations and anions. The first step is to identify the metal and non-metal components. Metals donate electrons and form positive ions (cations), while non-metals accept electrons to form negative ions (anions).
After identifying the elements, you combine their names. The metal name is said first, followed by the base name of the non-metal with an "-ide" suffix. For instance, in sodium bromide (\( \text{NaBr} \)), "sodium" is the metal, and "bromine" changes to "bromide" signaling it's the non-metal partner.
Specific rules exist for transition metals which may form various charged ions. In such cases, Roman numerals indicate the charge, but for simple binary ionic compounds, naming is straightforward as illustrated:

• Sodium Bromide - \( \mathrm{NaBr} \)
• Magnesium Chloride - \( \mathrm{MgCl}_2 \)
• Aluminum Phosphide - \( \mathrm{AlP} \)
• Strontium Bromide - \( \mathrm{SrBr}_2 \)
• Silver Iodide - \( \mathrm{AgI} \)
• Potassium Sulfide - \( \mathrm{K_2S} \)

Chemical Formulas

Chemical formulas represent the proportion of elements in a compound. They are abbreviated expressions of chemical compounds, showing exact relationships and ion counts.
A chemical formula is structured with element symbols and numeric subscripts. For instance, in magnesium chloride (\( \mathrm{MgCl}_2 \)), "Mg" represents magnesium and "Cl" represents chlorine.
The subscript "2" indicates two chlorine atoms are linked to one magnesium atom, due to magnesium's 2+ charge balancing two 1- chloride ions.Understanding chemical formulas involves:

• Identifying the chemical symbols.
• Recognizing subscripts which show the quantity of each ion.
• Knowing that the absence of a subscript implies a single atom.

Chemical formulas give insight into the arrangement and ratio of ions, helping predict compound properties such as reactivity and solubility.

Ion Charges

Ion charges are fundamental in forming ionic compounds as they influence how elements combine. A basic understanding of ion charges aids in predicting formula structure and compound balance.
Elements lose or gain electrons to attain stable electron configurations, resulting in charged ions.
The charge for each ion stems from the "group" or column in the periodic table.

• Group 1 elements (like sodium, Na) typically form 1+ ions.
• Group 2 elements (such as magnesium, Mg) form 2+ ions.
• Transition metals can form various charges, but silver (Ag) often has a 1+ charge.
• Non-metals like chlorine (Cl) and bromine (Br) tend to form 1- ions.

Ions join when total positive and negative charges neutralize each other, forming a stable compound.
For example, aluminum (\(\mathrm{Al}^{3+} \)) and phosphorus (\(\mathrm{P}^{3-} \)) neutralize by forming aluminum phosphide \(\text{AlP} \). Recognizing ion charges helps in deciphering molecular structures and ensures accurate compound naming.