Multiple Choice
What is the result when lead (II) nitrate is mixed with potassium bromide in an aqueous solution?
400
views
3. Chemical Reactions
Writing Ionic Compounds
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Which of the following is the correct formula for the ionic compound formed between magnesium and chlorine?
A
Mg_2Cl
B
Mg_2Cl_2
C
MgCl_2
D
MgCl
Verified step by step guidance1
Identify the charges of the ions formed by magnesium and chlorine. Magnesium typically forms a \(\text{Mg}^{2+}\) ion, and chlorine forms a \(\text{Cl}^{-}\) ion.
Determine the ratio of ions needed to balance the total positive and negative charges so that the compound is electrically neutral.
Since magnesium has a charge of +2 and chlorine has a charge of -1, you need two chloride ions to balance one magnesium ion.
Write the formula by placing the magnesium ion first, followed by the number of chloride ions needed, which is two, resulting in \(\text{MgCl}_2\).
Verify that the total positive charge (+2 from one \(\text{Mg}^{2+}\)) equals the total negative charge (2 × -1 from two \(\text{Cl}^{-}\) ions), confirming the compound is neutral.
3:09mWatch next
Master Rules for Writing Ionic Compounds with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
Writing Ionic Compounds practice set
Problem sets built by lead tutorsExpert video explanations