Monatomic or monoatomic elements are elements that are stable as single atoms. Mon-or Mono-means one.In order for an element to be stable by itself, it needs to have a stable octet of valence electrons. Engaging math & science practice! Improve your skills with free problems in 'Drawing Lewis dot structures for monatomic ions' and thousands of other practice lessons.
EXAMPLE - Predicting Ion Charge:
Predict the charge or charges for the ions formed by atoms of (a) scandium, Sc, (b) gallium, Ga, and (c) sulfur, S. Write an abbreviated electron configuration for each ion and use it to explain why the ion acquires the charge it does.
Solution:
a. Because scandium is a metal in group 3 on the periodic table, we expect its atoms to lose three electrons each and form +3 cations with the stable 3s23p6 configuration of argon.
ScSc3++3e-
[Ar] 3d1 4s2[Ar] or [Ne] 3s2 3p6
b. Gallium is a metal, so we expect it to form cations. It is in group 13, so we follow the guidelines for cations other than Al3+ and those in groups 1, 2, or 3. The first step is to write the abbreviated electron configuration for an uncharged gallium atom. The noble gas preceding gallium on the periodic table is argon. Gallium atoms can lose one electron to form Ga+ ions with the stable 3d104s2 configuration.
GaGa++e-
[Ar] 3d10 4s2 4p1[Ar] 3d10 4s2
[Ar] 3d10 4s2 4p1[Ar] 3d10 4s2
Gallium atoms can also lose three electrons to form Ga3+ ions with the stable 3d10 configuration.
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GaGa3++3e-
[Ar] 3d10 4s2 4p1[Ar] 3d10
[Ar] 3d10 4s2 4p1[Ar] 3d10
c. Sulfur is a nonmetal, so we expect its atoms to gain electrons and form anions. Each atom gains two electrons to form a S2- ion with the stable, noble gas electron configuration of argon.
S+2e-S2-
[Ne] 3s2 3p4[Ar] or [Ne] 3s2 3p6
[Ne] 3s2 3p4[Ar] or [Ne] 3s2 3p6
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![Monatomic Ion Monatomic Ion](/uploads/1/1/9/3/119388900/857533563.png)
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Return to the Monatomic Ion Configurations Page.
Learning Objectives
1. Use the rules for naming ionic compounds.
Naming Ions
Naming the Cation
The name of a monatomic cation is simply the name of the element followed by the word ion. Thus, Na+ is the sodium ion, Al3+ is the aluminum ion, Ca2+ is the calcium ion, and so forth. Metals ions from Group 1 always have a 1+ charge, metals ions from Group 2 always have a 2+ charge, the only aluminum ion is 3+, zinc ions are 2+, and silver ions are 1+. These are the fixed-charge metals. The names for fixed-charge metal ions must never be given a Roman numeral.
Metals that can have several different charges as ions are referred to as variable-charge metals. Almost all transition metals plus the metals under the staircase are variable-charge metals. Iron, for example, can form two different cations, each of which, when combined with the same anion, makes a different compound with unique physical and chemical properties. For example, FeCl2 and FeCl3 differ in density, melting point, solubility, and color. Thus, we need a different name for each iron ion to distinguish Fe2+ from Fe3+. The same issue arises for all of the variable-charge metals.
In the modern approach to naming compounds containing variable-charge metals, called the Stock system, a variable-charge metal ion’s positive charge is indicated by a Roman numeral in parentheses after the element name, followed by the word ion. Thus, Fe2+ is called the iron(II) ion, while Fe3+ is called the iron(III) ion. The names for variable-charge metals must always be given a Roman numeral.
An older system used the endings -ic for when the metal had the larger of its possible negative charges and -ous for when the metal had the smaller of its possible negative charges instead of the Roman numerals. We will not use this older system.
Naming the Anion
The name of a monatomic anion consists of the stem of the element name, the suffix –ide, and then the word ion. Thus, as we have already seen, Cl− is “chlor-” + “-ide ion,” or the chloride ion. Similarly, O2− is the oxide ion, Se2− is the selenide ion, and so forth. Table 3.3 “Some Monatomic Anions” lists the names of some common monatomic ions.
Table 3.3 Some Monatomic Anions
Ion | Name |
---|---|
F− | fluoride ion |
Cl− | chloride ion |
Br− | bromide ion |
I− | iodide ion |
O2− | oxide ion |
S2− | sulfide ion |
P3− | phosphide ion |
N3− | nitride ion |
The polyatomic ions have their own characteristic names, as we saw in Table 3.1 “Some Polyatomic Ions”.
Example 6
Name each ion.
- Ca2+
- S2−
- SO32−
- NH4+
- Cu+
Solution
Show Answer- the calcium ion
- the sulfide ion (from Table 3.3 “Some Monatomic Anions”)
- the sulfite ion (from Table 3.1 “Some Polyatomic Ions”)
- the ammonium ion (from Table 3.1 “Some Polyatomic Ions”)
- the copper(I) ion : Copper can form cations with either a 1+ or 2+ charge, so we have to specify the charge by using a Roman numeral.)
SKill Building Exercise
Name each Ion
Example 7
Write the formula for each ion.
- the bromide ion
- the phosphate ion
- the copper 1+ ion
- the magnesium ion
How to clear memory on windows 7. Solution
Show Answer
SKILL-BUILDING EXERCISE
Write the formula for each ion.
- the fluoride ion
- the carbonate ion
- the tin4+ ion
- the potassium ion
Naming Compounds
Now that we know how to name ions, we are ready to name ionic compounds. We do so by placing the name of the cation first, followed by the name of the anion, and dropping the word ion from both parts.
For example, what is the name of the compound whose formula is Ba(NO3)2?
The compound’s name does not indicate that there are two nitrate ions for every barium ion. You must determine the relative numbers of ions by balancing the positive and negative charges.
If you are given a formula for an ionic compound whose cation can have more than one possible charge, you must first determine the charge on the cation before identifying its correct name. For example, consider FeCl2 and FeCl3. In the first compound, the iron ion has a 2+ charge because there are two Cl− ions in the formula (1− charge on each chloride ion). In the second compound, the iron ion has a 3+ charge, as indicated by the three Cl− ions in the formula. These are two different compounds that need two different names. By the Stock system, the names are iron(II) chloride and iron(III) chloride.
Example 8
Name each ionic compound. Use Roman numerals only when needed.
- Ca3(PO4)2
- (NH4)2Cr2O7
- KCl
- CuCl
- SnF2
Monatomic Ions Quizlet
Solution
Monatomic Ions Worksheet
Show Answer- calcium phosphate
- ammonium dichromate (the prefix di- is part of the name of the anion, as in Table 3.1 “Some Polyatomic Ions”)
- potassium chloride
- copper(I) chloride
- tin(II) fluoride
Skill-building Exercise
Name each ionic compound. Use Roman numerals only when neccessary.
- ZnBr2
- Fe(NO3)3
- Al2O3
- AuF3
- AgF
Figure 3.7 “A Guide to Naming Simple Ionic Compounds” is a synopsis of how to name simple ionic compounds.
Figure 3.7 A Guide to Naming Simple Ionic Compounds. Follow these steps to name a simple ionic compound.
Concept Review Exercises
- Briefly describe the process for naming an ionic compound.
- In what order do the names of ions appear in the names of ionic compounds?
- When do you need a Roman numeral in the name of an ionic compound? Give an example. When are you not allowed to have a Roman numeral in an ion compound name?
ANswers
Show Answer- Name the cation and then the anion.
- the cation name followed by the anion name
- An ionic compound in which the metal cation can have more than one possible charge must have a Roman numeral. For example FeCl3 is iron(III) chloride but FeCl2 is iron(II) chloride. Metals that always have the same charge as a cation are not given a Roman numeral, For example MgCl2 is simply magnesium chloride because the magnesium ion is always Mg2 .
Key Takeaway
- Each ionic compound has its own unique name that comes from the names of the ions.
Exercises
- Name each ion.
- Cs+
- As3−
- HSO4−
- Sn2+
- Name the ionic compound formed by each pair of ions.
- Na+ and Br−
- Mg2+ and Br−
- Mg2+ and S2−
- Name the ionic compound formed by each pair of ions.
- K+ and Cl−
- Mg2+ and Cl−
- Mg2+ and Se2−
- Name the ionic compound formed by each pair of ions.
- Na+ and N3−
- Mg2+ and N3−
- Al3+ and S2−
- Name the ionic compound formed by each pair of ions.
- Li+ and N3−
- Mg2+ and P3−
- Li+ and P3−
- Name the ionic compound formed by each pair of ions. Use both the Stock and common systems, where appropriate.
- Fe3+ and Br−
- Fe2+ and Br−
- Au3+ and S2−
- Au+ and S2−
- Name the ionic compound formed by each pair of ions. Use both the Stock and common systems, where appropriate.
- Cr3+ and O2−
- Cr2+ and O2−
- Pb2+ and Cl−
- Pb4+ and Cl−
- Name the ionic compound formed by each pair of ions. Use both the Stock and common systems, where appropriate.
- Cr3+ and NO3−
- Fe2+ and PO43−
- Ca2+ and CrO42−
- Al3+ and OH−
- Name the ionic compound formed by each pair of ions. Use both the Stock and common systems, where appropriate.
- NH4+ and NO3−
- H+ and Cr2O72−
- Cu+ and CO32−
- Na+ and HCO3−
- Name each compound.
- Co(HCO3)2
- LiHCO3
1. a. the radium ion
b.the phosphide ion
c. the dihydrogen phosphate ion
d. the tin(IV) ion
3. a. sodium bromide
b. magnesium bromide
c. magnesium sulfide
5. a. sodium nitride
b. magnesium nitride
c. aluminum sulfide
7. a. iron(III) bromide
b.iron(II) bromide
c. gold(III) sulfide
d. gold(I) sulfide
9. a. chromium(III) nitrate
b. iron(II) phosphate
Monatomic Ion Chart
c. calcium chromate
d. aluminum hydroxide
![Monatomic Monatomic](/uploads/1/1/9/3/119388900/639342481.png)
Monatomic Ions
11. a. aluminum hydrogen sulfate or aluminum bisulfate
b. magnesium hydrogen sulfate or magnesium bisulfate