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Ionic Compounds: Naming Ions and Formulas, Exercises of Chemistry

University of the Pacific (UOP)Chemistry

Instructions on how to name ions and write formulas for ionic compounds. It covers the basics of ionic bonding and explains how to determine the overall charge of an ionic compound. Critical thinking questions are included to test understanding.

What you will learn

  • What is the overall charge for the following ionic compounds: NaCl, MgF2, Ca3N2, AlN?
  • What is the symbol and name for each ion (positive or negative) for the following elements: Ca, Cl, N, K, S, B, P?
  • Why must the positive ion always be written first in the formula for an ionic compound?

Typology: Exercises

2021/2022

Uploaded on 09/27/2022

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ChemQuest 19 KEY
Name: ____________________________
Date: _______________
Hour: _____
Information: Naming Ions
To write an ion, you write the symbol of the atom and put the charge in the upper right corner.
Consider the following examples: Al3+, O2-, Mg2+. You should verify that each of the charges is
correct.
Positive and negative ions are named differently. Positive ions retain the same name as the
parent atom. For example, Al3+ is called the “aluminum ion” and Mg2+ is called the “magnesium
ion.” Negative ions are named a little differently. For negative ions, you change the ending of the
name to “-ide”. Therefore, O2- is named oxide and P3- is named phosphide.
Critical Thinking Questions
1. Write the symbol (including the charge) and name for each of the ions for each of the
following:
a) Ca b) Cl c) N d) K e) S f) B g) P
Ca2+ Cl- N3- K+ S2- B3+ P3-
calcium ion chloride nitride potassium ion sulfide boron ion phosphide
Information: Ionic Bonding and Formulas
There are two ways in which atoms can “bond” to each other and form a compound. The means
of
bonding that we will consider now is called ionic bonding, which occurs between a metal and a
nonmetal. As you know, opposite charges attract. Ionic bonding is when two ions of opposite
charge
attract and bond to each other forming an ionic compound. Consider the following examples of
formulas for ionic compounds:
• One Na+ (sodium ion) and one Cl- (chloride ion) bond to make NaCl, “sodium chloride.”
• One Mg2+ (magnesium ion) and two F- (fluoride ion) bond to make MgF2, “magnesium
fluoride.”
• Three Ca2+ (calcium ion) and two N3- (nitride ion) bond to make Ca3N2, “calcium nitride.”
• One Al3+ (aluminum ion) and one N3- (nitride ion) bond to make AlN, “aluminum nitride.”
The small numbers at the bottom right of each symbol in a formula are called “subscripts”.
Subscripts tell us how many of each type of atom are present. For example in the formula Mg3N2
there are three magnesium ions and two nitride ions.
Critical Thinking Questions
2. Consider the formula NaCl in the above example. It tells us that one Na+ ion is bonded to one
Clion.
What is the overall charge for NaCl? Is it positive, negative, or neutral?
Neutral: one +1 ion (Na+) and one -1 ion (Cl-) together are neutral.
60
3. Consider MgF2. This formula tells us that one Mg2+ ion bonds with two F- ions. What is the
overall charge on MgF2?
Neutral: one +2 ion (Mg2+) and two -1 ions (F-) together are neutral.
4. What is the overall charge on any ionic compound?
Neutral
pf3

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ChemQuest 19 KEY

Name: ____________________________ Date: _______________ Hour: _____

Information : Naming Ions

To write an ion, you write the symbol of the atom and put the charge in the upper right corner. Consider the following examples: Al3+, O2-, Mg2+. You should verify that each of the charges is correct. Positive and negative ions are named differently. Positive ions retain the same name as the parent atom. For example, Al3+ is called the “aluminum ion” and Mg2+ is called the “magnesium ion.” Negative ions are named a little differently. For negative ions, you change the ending of the name to “-ide”. Therefore, O2- is named oxide and P3- is named phosphide.

Critical Thinking Questions

  1. Write the symbol (including the charge) and name for each of the ions for each of the following: a) Ca b) Cl c) N d) K e) S f) B g) P Ca2+ Cl- N3- K+ S2- B3+ P3- calcium ion chloride nitride potassium ion sulfide boron ion phosphide

Information : Ionic Bonding and Formulas

There are two ways in which atoms can “bond” to each other and form a compound. The means of bonding that we will consider now is called ionic bonding, which occurs between a metal and a nonmetal. As you know, opposite charges attract. Ionic bonding is when two ions of opposite charge attract and bond to each other forming an ionic compound. Consider the following examples of formulas for ionic compounds:

  • One Na+ (sodium ion) and one Cl- (chloride ion) bond to make NaCl, “sodium chloride.”
  • One Mg2+ (magnesium ion) and two F- (fluoride ion) bond to make MgF 2 , “magnesium fluoride.”
  • Three Ca2+ (calcium ion) and two N3- (nitride ion) bond to make Ca 3 N 2 , “calcium nitride.”
  • One Al3+ (aluminum ion) and one N3- (nitride ion) bond to make AlN, “aluminum nitride.” The small numbers at the bottom right of each symbol in a formula are called “subscripts”. Subscripts tell us how many of each type of atom are present. For example in the formula Mg 3 N 2 there are three magnesium ions and two nitride ions.

Critical Thinking Questions

  1. Consider the formula NaCl in the above example. It tells us that one Na+ ion is bonded to one Clion. What is the overall charge for NaCl? Is it positive, negative, or neutral? Neutral: one +1 ion (Na+) and one -1 ion (Cl-) together are neutral. 60
  2. Consider MgF 2. This formula tells us that one Mg2+ ion bonds with two F- ions. What is the overall charge on MgF 2? Neutral: one +2 ion (Mg2+) and two -1 ions (F-) together are neutral.
  3. What is the overall charge on any ionic compound? Neutral
  1. Why is calcium nitride written like Ca 3 N 2 and not something like CaN 2 or Ca 2 N 3? In other words why do exactly three calcium ions bond with exactly two nitride ions? Three +2 ions (Ca2+) are required to go along with two -3 ions (N3-) so that the overall charge is neutral. Mathematically: 3(+2) + 2(-3) = 0
  2. The formula Ca 3 N 2 can never be written as N 2 Ca 3. To find out why, take note of each of the four example formulas given above. a) In terms of charge, what do the first ions named all have in common? They are positively charged. b) In terms of charge, what do the second ions named all have in common? They are negatively charged. c) Now, why can’t Ca 3 N 2 ever be written like N 2 Ca 3? The positive ion (Ca2+) must be written first.
  3. There are two rules to follow when writing formulas for ionic compounds. One has to do with charges (see questions 4 and 5) and the other has to do with which atom to write first and which one to write second (see question 6). What are these two rules?
  4. Ionic compounds need to be written with the ions combined so that the final compound is neutral.
  5. The positive ion must be written first.
  6. What is wrong with the following formulas? a) Al 2 S b) PNa 3 c) Mg 2 S 2
  7. Write the formula and name for the compound that forms when the following atoms form ionic compounds. The first is done for you. a) nitrogen and sodium b) barium and sulfur c) magnesium and iodine Na 3 N BaS MgI 2 sodium nitride barium sulfide magnesium iodide d) oxygen and aluminum e) calcium and phosphorus f) sodium and sulfur Al 2 O 3 Ca 3 P 2 Na 2 S aluminum oxide calcium phosphide sodium sulfide
  8. Given the following compounds, determine the charge on the unknown ion “X”. a) X 2 S b) MgX c) X 3 P 2 This compound is not neutral. Two Al3+ ions will combine with three S2- ions to give the correctly written, neutral compound: Al 2 S 3. Although this compound is neutral, the positive ion (Na+) is not written first. The correct way to write it would be Na 3 P. It is generally best to write ionic compounds in their lowest multiple so it should be written MgS and not Mg 2 S 2 or Mg 3 S 3 or Mg 4 S 4 , etc. X must be +1 since two + X ions would be needed to balance out the -2 sulfide ions.