Chemistry

1. Section 2.8
Naming Simple Compounds
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2/2/2024
Chemistry
1
Vocabulary - Review
Q: What is a cation?
A: A positive ion formed by a metal
Examples: Na+ Ca 2+ Al 3+
Q: What is an anion?
A: A negative ion formed by a nonmetal.
Examples: H- F- O 2- P 3-
Q: What is a polyatomic ion?
A: A group of charged atoms NH4
+ SO4
2-
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2. Section 2.8
Naming Simple Compounds
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Ionic Compounds
 Attraction between + ions and - ions
 Electrons go from metals to nonmetals
electron transfer
metal nonmetal ion+ ion–
Electrons lost = Electrons gain
NOTE: the net charge on the compound is zero
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3. Section 2.8
Naming Simple Compounds
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3
Formation of Ionic Compounds

4. Section 2.8
Naming Simple Compounds
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Ionic Bonding
What happens when an atom of sodium reacts with an
atom of chlorine?
Na Na+ + 1e-
Cl + 1e- Cl-
Na + Cl + 1e- Na+Cl- + 1e-
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5. Section 2.8
Naming Simple Compounds
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Ionic Bonding
We write Na+Cl- as simply NaCl
• The ionic compound is neutral – this means the net
(overall) charge is = 0.
• Now let’s try for cesium reacting with sulfur.
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6. Section 2.8
Naming Simple Compounds
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Ionic Bonding
Cs Cs+ + 1e-
S + 2e- S2-
Cs + S + 2e- Cs+S2- + 1e-
This equation is not balanced. What must be done to
correct this?
Solution:
1. Write the symbol for each ion present
2.Make sure you include the charge of each ion
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7. Section 2.8
Naming Simple Compounds
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Writing a Formula
Write the formula for the ionic compound that
will form between Ba2+ and Cl.
Solution:
1. Balance charge with + and – ions
2. Write the positive ion of metal first, and the
negative ion Ba2+ Cl
3. Write the number of ions needed as
subscripts BaCl2 (NOTE WE CRISSCROSSED THE CHARGES)
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8. Section 2.8
Naming Simple Compounds
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Ionic Compounds--Example: Sodium and oxygen react
1. You have to balance the charges.
2. You do this by criss-crossing the value of the charge
(not the + or -)
Sodium oxide
Na+ O2-
Na2O
we do not write the 1 as a subscript
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9. Section 2.8
Naming Simple Compounds
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Ionic Compounds
Lithium iodide
Li+ I –
LiI
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10. Section 2.8
Naming Simple Compounds
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Ionic Compounds
Magnesium oxide
Mg2+ O2-
Mg2O2 MUST be reduced to MgO
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11. Section 2.8
Naming Simple Compounds
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Ionic Compounds
Let’s try a few:
Barium nitride
Ba3N2
Aluminum oxide
Al2O3
Cesium iodide
CsI
Sodium fluoride
NaF
Strontium bromide
SrBr2
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12. Section 2.8
Naming Simple Compounds
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Learning Check
Write the correct formula for the
compounds containing the following ions:
A. Na+, S2-
B. Al3+, Cl-
C. Mg2+, N3-
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13. Section 2.8
Naming Simple Compounds
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Solution
A. Na+, S2-
Na2S
B. Al3+, Cl-
AlCl3
C. Mg2+, N3-
Mg3N2
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14. Section 2.8
Naming Simple Compounds
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• Binary Compounds
 Composed of two elements
 Ionic and covalent compounds included
• Binary Ionic Compounds
 Metal—nonmetal
• Binary Covalent Compounds
 Nonmetal—nonmetal
Naming Compounds

15. Section 2.8
Naming Simple Compounds
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• Binary Compounds
 Composed of two elements
• Binary Ionic Compounds
 Metal—nonmetal
• Binary Covalent Compounds
 Nonmetal—nonmetal

16. Section 2.8
Naming Simple Compounds
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• Binary ionic compounds
contain positive cations
and negative anions.
 Type I compounds
• Metal present forms
only one cation.
 Type II compounds
• Metal present can
form 2 or more
cations with
different charges.

17. Section 2.8
Naming Simple Compounds
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17
1. Contain 2 different elements
2. The cation is always named first and the
anion second.
2. A cation has same name as element.
Examples: Ca2+ calcium
Al3+ aluminum
Na + sodium
3. A anion has the same name as the element
name with adding –ide to the end.
Examples: Cl - chloride
S2- sulfide
P3- phosphide
Binary Ionic Compounds (Type I monatomic cations & anions)

18. Section 2.8
Naming Simple Compounds
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Common Simple Cations and Anions

19. Section 2.8
Naming Simple Compounds
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1. The cation is always named first and the anion
second.
2. A simple cation takes its name from the name
of the element.
3. A simple anion is named by taking the first part
of the element name (the root) and adding –ide.
Rules for Naming Type I Ionic Compounds

20. Section 2.8
Naming Simple Compounds
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• Examples:
KCl Potassium chloride
MgBr2 Magnesium bromide
CaO Calcium oxide
Binary Ionic Compounds (Type I)

21. Section 2.8
Naming Simple Compounds
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Ionic Compounds
Now let us put it all together:
Na3N
Cation: sodium
Anion: nitride
Compound: Sodium nitride
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22. Section 2.8
Naming Simple Compounds
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Ionic Compounds
BaO
Cation: barium
Anion: oxide
Compound: barium oxide
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23. Section 2.8
Naming Simple Compounds
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Naming Binary Ionic Compounds (Type I)
SUMMARY - Name the metal first, then the
nonmetal with ending changed to -ide.
Examples:
NaCl sodium chloride
ZnI2 zinc iodide
Al2O3 aluminum oxide
KCl Potassium chloride
MgBr2 Magnesium bromide
CaO Calcium oxide
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24. Section 2.8
Naming Simple Compounds
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24
Exercise
What is the name of the compound SrBr2?
a) strontium bromine
b) sulfur bromide
c) strontium dibromide
d) strontium bromide

25. Section 2.8
Naming Simple Compounds
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Learning Check
Complete the names of the following type I
binary compounds:
Na3N sodium ________________
KBr potassium________________
Al2O3 aluminum ________________
MgS _________________________
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26. Section 2.8
Naming Simple Compounds
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Solution
Complete the names of the following binary
compounds:
Na3N sodium nitride
KBr potassium bromide
Al2O3 aluminum oxide
MgS magnesium sulfide
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27. Section 2.8
Naming Simple Compounds
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Binary Ionic Compounds (Type II)
• Metals in these
compounds can form
more than one type of
positive charge.
• Charge on the metal ion
must be specified.
• Roman numeral
indicates the charge of
the metal cation.
• Transition metal cations
usually require a Roman
numeral.

28. Section 2.8
Naming Simple Compounds
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• Metals in these compounds form more than one
type of positive charge.
• Charge on the metal ion must be specified.
• Roman numeral indicates the charge of the metal
cation.
• Transition metal cations that form 2 or more
positive ions require a Roman numeral.
Binary Ionic Compounds (Type II)
1+ or 2+ ____________________ 2+ or 3+
Cu+, Cu2+ Fe2+, Fe3+
copper(I) ion iron(II) ion
copper (II) ion iron(III) ion

29. Section 2.8
Naming Simple Compounds
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Common Type II Cations

30. Section 2.8
Naming Simple Compounds
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1. The cation is always named first and the anion
second.
2. Because the cation can assume more than one
charge, the charge is specified by a Roman
numeral in parentheses.
Rules for Naming Type II Ionic Compounds

31. Section 2.8
Naming Simple Compounds
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• Examples:
CuBr Copper(I) bromide
FeS Iron(II) sulfide
PbO2 Lead(IV) oxide
Binary Ionic Compounds (Type II)

32. Section 2.8
Naming Simple Compounds
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Binary Ionic Compounds (Type II)
Use a roman number after the name of a metal that forms
two or more ions (note compound is neutral)
Example:
FeCl3 (Fe3+) iron (III) chloride
CuCl (Cu+ ) copper (I) chloride
SnF4 (Sn4+) tin (IV) fluoride
PbCl2 (Pb2+) lead (II) chloride
Fe2S3 (Fe3+) iron (III) sulfide
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33. Section 2.8
Naming Simple Compounds
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33
Exercise
What is the name of the compound CrO2?
a) chromium oxide
b) chromium(II) oxide
c) chromium(IV) oxide
d) chromium dioxide

34. Section 2.8
Naming Simple Compounds
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34
Exercise
What is the correct name of the compound that
results from the most stable ion for sulfur and
the metal ion that contains 24 electrons?
a) iron(III) sulfide
b) chromium(II) sulfide
c) nickel(III) sulfate
d) iron(II) sulfide

35. Section 2.8
Naming Simple Compounds
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Learning Check
Complete the names of the following binary
compounds with variable metal ions:
FeBr2 iron (_____) bromide
Cu2O copper (_____) oxide
SnCl4 ___(_____ ) ______________
Fe2O3 ________________________
CuS ________________________
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36. Section 2.8
Naming Simple Compounds
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Solution
Complete the names of the following binary
compounds with variable metal ions:
FeBr2 iron ( II ) bromide
Cu2O copper ( I ) oxide
SnCl4 tin (IV) chloride
Fe2O3 iron (III) oxide
CuS copper (II) sulfide
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37. Section 2.8
Naming Simple Compounds
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Learning Check
Name the following compounds:
A. CaO
B. SnCl4
C. Co2O3
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38. Section 2.8
Naming Simple Compounds
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Solution
Name the following compounds:
A. CaO calcium oxide
B. SnCl4 tin(IV) chloride
C. Co2O3 cobalt (III) oxide
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39. Section 2.8
Naming Simple Compounds
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• Polyatomic ions are charged entities composed
of several atoms bound together.
• They have special names and must be
memorized. (see Table 2.5 on pg. 62 in text).
• Examples of compounds containing polyatomic ions:
NaOH Sodium hydroxide
Mg(NO
3
)
2
Magnesium nitrate
(NH
4
)
2
SO
4
Ammonium sulfate

40. Section 2.8
Naming Simple Compounds
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Names of Common Polyatomic Ions

41. Section 2.8
Naming Simple Compounds
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• Naming ionic compounds containing
polyatomic ions follows rules similar to those
for binary compounds.
 Ammonium acetate

42. Section 2.8
Naming Simple Compounds
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NaOH Sodium hydroxide
Mg(NO3)2 Magnesium nitrate
(NH4)2SO4 Ammonium sulfate
FePO4 Iron(III) phosphate
Examples

43. Section 2.8
Naming Simple Compounds
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Exercise
What is the name of the compound KClO3?
a) potassium chlorite
b) potassium chlorate
c) potassium perchlorate
d) potassium carbonate