1. Naming ions

2. (you do not have to copy notes in green)
OBJECTIVES:
Identify the charges on monatomic ions by using the periodic table, and name the ions.

3. OBJECTIVES:
Define a polyatomic ion and write the names and formulas of the most common polyatomic ions.

4. Identify the two common endings for the names of most polyatomic ions.
OBJECTIVES:
Identify the two common endings for the names of most polyatomic ions.

5. Atoms and Ions Atoms are electrically neutral.
Because there is the same number of protons (+) and electrons (-).
Ions are atoms, or groups of atoms, with a charge (positive or negative)
They have different numbers of protons and electrons.
Only electrons can move, and ions are made by gaining or losing electrons.

6. F1- O2- An Anion is… Has gained electrons.
Nonmetals can gain electrons.
Charge is written as a superscript on the right.
A negative ion.
Has gained one electron
F1-
O2-
Gained two electrons

7. K1+ Ca2+ A Cation is… A positive ion. Formed by losing electrons.
More protons than electrons.
Metals can lose electrons
K1+
Has lost one electron
Ca2+
Has lost two electrons

8. Predicting Ionic Charges
Group 1A:
Lose 1 electron to form 1+ ions
H1+
Li1+
Na1+
K1+
Rb1+

9. Predicting Ionic Charges
Group 2A:
Loses 2 electrons to form 2+ ions
Be2+
Mg2+
Ca2+
Sr2+
Ba2+

10. Predicting Ionic Charges
Group 13 Boron Family
B3+
Al3+
Ga3+
Lose 3 electrons

11. Predicting Ionic Charges
Neither! Group 14 Carbon Family rarely form ions (they tend to share)
Group 14

12. Predicting Ionic Charges
Nitride
Group15 Nitrogen Family:
P3-
Phosphide
Gains 3 electrons to form 3- ions
As3-
Arsenide

13. Predicting Ionic Charges
Oxide
Group 16 Oxygen Family
S2-
Sulfide
Gains 2 electrons to form 2- ions
Se2-
Selenide

14. Predicting Ionic Charges
Group 17 Fluoride Family:
F1-
Fluoride
Br1-
Bromide
Gains 1 electron to form1- ions
Cl1-
Chloride
I1-
Iodide

15. Predicting Ionic Charges
Group 8A:
Stable noble gases do not form ions!

16. Predicting Ionic Charges
Transition elements: Some have more than one ionic state – Roman numerals are used
Iron (II) = Fe2+
Iron (III) = Fe3+

17. Predicting Ionic Charges
Some of the post-transition elements also
have more than one possible cation
Tin (II) = Sn2+
Lead (II) = Pb2+
Tin (IV) = Sn4+
Lead (IV) = Pb 4+

18. Naming cations
Most of the metals simply take the name of the element itself.
Ca2+ Calcium
Na+ Sodium
Mg2+ Magnesium
Cd2+ Cadmium
K+ Potassium

19. Predicting Ionic Charges
Some transition elements have only one possible oxidation state, such as these three:
Silver = Ag1+
Zinc = Zn2+
Cadmium = Cd2+

20. Do not need to use roman numerals for these:
Some of the transition metals have only one ionic charge:
Do not need to use roman numerals for these:
Silver is always 1+ (Ag1+)
Cadmium and Zinc are always 2+ (Cd2+ and Zn2+)

21. Practice by naming these:
Ca2+
Al3+
Fe3+
Fe2+
Pb2+
Li1+

22. Write symbols for these:
Potassium ion
Magnesium ion
Copper (II) ion
Chromium (VI) ion
Barium ion
Mercury (II) ion

23. Naming MONOATOMIC Anions (1 atom)
The non-metallic elements form negative ions (anions).
Monatomic anions all end with the -ide suffix:

24. MONOATOMIC NON-METAL IONS
Cl–
chloride
S2–
sulfide
O2–
oxide
C4–
carbide I–
iodide H–
hydride

25. Practice by naming these:
Cl1-
N3-
Br1-
O2-
Ga3+

26. Write symbols for these:
Sulfide ion
Iodide ion
Phosphide ion
Strontium ion

27. Polyatiomic anions (more than one atom)
A few follow the pattern for the monatomic anions:
OH– hydroxide
CN– cyanide
O2– peroxide

28. Oxyanions (contain oxygen)
Names usually end in –ate

29. Examples CO32– carbonate NO3– nitrate NO2– nitrite SO42– sulfate
SO32– sulfite
PO43– phosphate

30. Exception Polyatomic – Oxygen and Chlorine, Bromine and Iodine
Have a unique naming system:
ClO– Hypochlorite
ClO2– Chlorite
ClO3– Chlorate
ClO4– Perchlorate

31. Practice
Name the following polyatomic anions:
BrO–
BrO2–
IO3–
BrO4–