The document discusses ions and ionic bonding. It defines ions as atoms that have gained or lost electrons to become positively or negatively charged. Cations are positively charged ions that form when metals lose electrons, while anions are negatively charged ions that form when nonmetals gain electrons. The octet rule states that atoms seek to attain eight electrons in their valence shell. Ionic compounds form when cations and anions bond via electrostatic attraction to yield an electrically neutral compound. Transition metals can form ions with multiple possible charges. Ionic compounds have properties like crystalline structures, high melting points, and conductivity when dissolved in water.

1. Ions and IonicIons and Ionic
BondingBonding
Chapter 7 (Sections 7.1 & 7.2)Chapter 7 (Sections 7.1 & 7.2)
Chapter 9 (Sections 9.1 & 9.2)Chapter 9 (Sections 9.1 & 9.2)

2. Representative ElementsRepresentative Elements
 All elements in “A”All elements in “A”
groups of P.T.groups of P.T.
 Wide range ofWide range of
physical/chemicalphysical/chemical
propertiesproperties
 All elements exceptAll elements except
transition metals andtransition metals and
inner transition metalsinner transition metals

3. Valence ElectronsValence Electrons
 Electrons on the highestElectrons on the highest
primary energy levelprimary energy level
(highest number)(highest number)
 Corresponds to groupCorresponds to group
number of representativenumber of representative
elementselements
 __??_ is the only exception_ is the only exception

4. Lewis StructureLewis Structure
 a.k.a. “Electron Dot Structure”a.k.a. “Electron Dot Structure”
 Shows valence electrons asShows valence electrons as
dots around andots around an
atom’s symbolatom’s symbol
 Valence electronsValence electrons
only electrons usedonly electrons used
in chemical bondingin chemical bonding

5.  The maximum number of electrons an elementThe maximum number of electrons an element
can have in its outer shell is…can have in its outer shell is…

6. The Octet RuleThe Octet Rule
 The maximum number of electrons an elementThe maximum number of electrons an element
can have in its valence energy level is…can have in its valence energy level is…
 EIGHT!EIGHT!

7. The Octet RuleThe Octet Rule
 Often, atoms tend to lose orOften, atoms tend to lose or
gain electrons in order togain electrons in order to
form a complete octet, whichform a complete octet, which
makes the atom most stablemakes the atom most stable
 Metals (few valence electrons)Metals (few valence electrons)
lose electronslose electrons
 Nonmetals (many valenceNonmetals (many valence
electrons)electrons) gain electronsgain electrons

8. The Octet RuleThe Octet Rule
 When atoms lose/gainWhen atoms lose/gain
electrons, they take onelectrons, they take on
the electronthe electron
configuration of a nobleconfiguration of a noble
gasgas

9. IonsIons
 Ion – atom with a positive or negative charge (lost orIon – atom with a positive or negative charge (lost or
gained an electron)gained an electron)

10. IonsIons
 Ions that lose an electron, or multiple electrons,Ions that lose an electron, or multiple electrons,
become positively charged (and are calledbecome positively charged (and are called
CATIONSCATIONS).).  Metals!Metals!
 Ions that gain an electron, or multiple electrons,Ions that gain an electron, or multiple electrons,
become negatively charged (and are calledbecome negatively charged (and are called
ANIONSANIONS).).  Nonmetals!Nonmetals!

11. Answer these questions:Answer these questions:
 How many TOTAL electrons does oxygen have?How many TOTAL electrons does oxygen have?
 How many valence electrons does oxygen have?How many valence electrons does oxygen have?
 How many electrons must oxygen gain/lose to form aHow many electrons must oxygen gain/lose to form a
complete octet?complete octet?
 Does this make oxygen positively- or negatively-charged?Does this make oxygen positively- or negatively-charged?
 What is theWhat is the exactexact charge on the oxygen ion?charge on the oxygen ion?
 Is the oxygen ion a cation or an anion?Is the oxygen ion a cation or an anion?

12. Example 1Example 1
 Fluorine has 9 electrons. (7 in valence level)Fluorine has 9 electrons. (7 in valence level)
 As it ionizes (becomes an ion), what shouldAs it ionizes (becomes an ion), what should
happen?happen?
 What is the charge on the ion?What is the charge on the ion?
 FIRST, DRAW THE LEWIS STRUCTURE!FIRST, DRAW THE LEWIS STRUCTURE!

13. Example 2Example 2
 Nitrogen has 7 electrons (5 in valence level)Nitrogen has 7 electrons (5 in valence level)
 As it ionizes, what should happen?As it ionizes, what should happen?
 What is the charge on the ion?What is the charge on the ion?

14. Example 3Example 3
 Indium (In) has 49 electrons.Indium (In) has 49 electrons.
 As it ionizes, what should happen?As it ionizes, what should happen?
 What is the charge on the ion?What is the charge on the ion?

15. Group
Number
Example
Elements
Name of
Group (if
any)
# of
Valence
Electrons
# of
Electrons
Gained or
Lost to
Form Ion
Ionic
Charge
Cation or
Anion?
1A
2A
3A
4A
5A
6A
7A
8A

16. Group
Number
Example
Elements
Name of
Group (if
any)
# of
Valence
Electrons
# of
Electrons
Gained or
Lost to
Form Ion
Ionic
Charge
Cation or
Anion?
1A Lithium,
Potassium
Alkali
Metals
1 Lose 1 +1 Cation
2A
3A
4A
5A
6A
7A
8A

17. Group
Number
Example
Elements
Name of
Group (if
any)
# of
Valence
Electrons
# of
Electrons
Gained or
Lost to
Form Ion
Ionic
Charge
Cation or
Anion?
1A Lithium,
Potassium
Alkali
Metals
1 Lose 1 +1 Cation
2A Magnesium,
Calcium
Alkali Earth
Metals
2 Lose 2 +2 Cation
3A
4A
5A
6A
7A
8A

18. Group
Number
Example
Elements
Name of
Group (if
any)
# of
Valence
Electrons
# of
Electrons
Gained or
Lost to
Form Ion
Ionic
Charge
Cation or
Anion?
1A Lithium,
Potassium
Alkali
Metals
1 Lose 1 +1 Cation
2A Magnesium,
Calcium
Alkali Earth
Metals
2 Lose 2 +2 Cation
3A Aluminum 3 Lose 3 +3 Cation
4A
5A
6A
7A
8A

19. Group
Number
Example
Elements
Name of
Group (if
any)
# of
Valence
Electrons
# of
Electrons
Gained or
Lost to
Form Ion
Ionic
Charge
Cation or
Anion?
1A Lithium,
Potassium
Alkali
Metals
1 Lose 1 +1 Cation
2A Magnesium,
Calcium
Alkali Earth
Metals
2 Lose 2 +2 Cation
3A Aluminum 3 Lose 3 +3 Cation
4A Carbon,
Lead, Tin
4 Lose 4 /
Gain 4
+4 / -4 Cation /
Anion
5A
6A
7A
8A

20. Group
Number
Example
Elements
Name of
Group (if
any)
# of
Valence
Electrons
# of
Electrons
Gained or
Lost to
Form Ion
Ionic
Charge
Cation or
Anion?
1A Lithium,
Potassium
Alkali
Metals
1 Lose 1 +1 Cation
2A Magnesium,
Calcium
Alkali Earth
Metals
2 Lose 2 +2 Cation
3A Aluminum 3 Lose 3 +3 Cation
4A Carbon,
Lead, Tin
4 Lose 4 /
Gain 4
+4 / -4 Cation /
Anion
5A Nitrogen,
Phosphorus
5 Gain 3 -3 Anion
6A
7A
8A

21. Group
Number
Example
Elements
Name of
Group (if
any)
# of
Valence
Electrons
# of
Electrons
Gained or
Lost to
Form Ion
Ionic
Charge
Cation or
Anion?
1A Lithium,
Potassium
Alkali
Metals
1 Lose 1 +1 Cation
2A Magnesium,
Calcium
Alkali Earth
Metals
2 Lose 2 +2 Cation
3A Aluminum 3 Lose 3 +3 Cation
4A Carbon,
Lead, Tin
4 Lose 4 /
Gain 4
+4 / -4 Cation /
Anion
5A Nitrogen,
Phosphorus
5 Gain 3 -3 Anion
6A Oxygen,
Sulfur
6 Gain 2 -2 Anion
7A
8A

22. Group
Number
Example
Elements
Name of
Group (if
any)
# of
Valence
Electrons
# of
Electrons
Gained or
Lost to
Form Ion
Ionic
Charge
Cation or
Anion?
1A Lithium,
Potassium
Alkali
Metals
1 Lose 1 +1 Cation
2A Magnesium,
Calcium
Alkali Earth
Metals
2 Lose 2 +2 Cation
3A Aluminum 3 Lose 3 +3 Cation
4A Carbon,
Lead, Tin
4 Lose 4 /
Gain 4
+4 / -4 Cation /
Anion
5A Nitrogen,
Phosphorus
5 Gain 3 -3 Anion
6A Oxygen,
Sulfur
6 Gain 2 -2 Anion
7A Chlorine,
Bromine
Halogens 7 Gain 1 -1 Anion
8A

23. Group
Number
Example
Elements
Name of
Group (if
any)
# of
Valence
Electrons
# of
Electrons
Gained or
Lost to
Form Ion
Ionic
Charge
Cation or
Anion?
1A Lithium,
Potassium
Alkali
Metals
1 Lose 1 +1 Cation
2A Magnesium,
Calcium
Alkali Earth
Metals
2 Lose 2 +2 Cation
3A Aluminum 3 Lose 3 +3 Cation
4A Carbon,
Lead, Tin
4 Lose 4 /
Gain 4
+4 / -4 Cation /
Anion
5A Nitrogen,
Phosphorus
5 Gain 3 -3 Anion
6A Oxygen,
Sulfur
6 Gain 2 -2 Anion
7A Chlorine,
Bromine
Halogens 7 Gain 1 -1 Anion
8A Neon,
Radon
Noble
Gases
8 0 No charge

24. Group
Number
Example
Elements
Name of
Group (if
any)
# of
Valence
Electrons
# of
Electrons
Gained or
Lost to
Form Ion
Ionic
Charge
Cation or
Anion?
1A Lithium,
Potassium
Alkali
Metals
1 Lose 1 +1 Cation
2A Magnesium,
Calcium
Alkali Earth
Metals
2 Lose 2 +2 Cation
3A Aluminum 3 Lose 3 +3 Cation
4A Carbon,
Lead, Tin
4 Lose 4 /
Gain 4
+4 / -4 Cation /
Anion
5A Nitrogen,
Phosphorus
5 Gain 3 -3 Anion
6A Oxygen,
Sulfur
6 Gain 2 -2 Anion
7A Chlorine,
Bromine
Halogens 7 Gain 1 -1 Anion
8A Neon,
Radon
Noble
Gases
8 0 No charge

25. Write Ions of These Elements:Write Ions of These Elements:
 BariumBarium
 ChlorineChlorine
 PhosphorusPhosphorus
 Lead cationLead cation
 AluminumAluminum
 Indium (In)Indium (In)
 Krypton (Kr)Krypton (Kr)
 HydrogenHydrogen

26. Answer all questions.Answer all questions.
 MagnesiumMagnesium
 BromineBromine
 SulfurSulfur
 PotassiumPotassium
 AluminumAluminum
 NitrogenNitrogen

27.  As Fluorine becomes an ion, what happens?As Fluorine becomes an ion, what happens?
 Gain 1 electronGain 1 electron
 Gain 2 electronsGain 2 electrons
 Gain 3 electronsGain 3 electrons
 Lose 1 electronLose 1 electron

28. Polyatomic IonsPolyatomic Ions
 Ions composed of moreIons composed of more
than one tightly-bondedthan one tightly-bonded
atomsatoms
 Usually have a negativeUsually have a negative
chargecharge
 Usually end in –ite or –Usually end in –ite or –
ate, meaning that there isate, meaning that there is
oxygen in the ionoxygen in the ion

29. -1 charge-1 charge
HydroxideHydroxide OHOH--
NitrateNitrate NONO33
--
Hydrogen CarbonateHydrogen Carbonate
HCOHCO33
--
-2 charge-2 charge
SulfateSulfate SOSO44
2-2-
CarbonateCarbonate COCO33
2-2-
-3 charge-3 charge
PhosphatePhosphate POPO44
3-3-
+1 charge+1 charge
AmmoniumAmmonium NHNH44
++

30. Ionic Bonding
Blue Book: Chapter 15
Red Book: Chapter 7

31. 2 Types of Compounds / Bonds
 Ionic – metal bonded with
nonmetal
 Electrons lost/gained
 Covalent – usually nonmetal
bonded with nonmetal
 Electrons shared

32. Ionic Compounds
 Usually contain a metal
and a nonmetal
 Why?

33. Ionic Compounds
 Although they contain
ions, ionic compounds
are electrically neutral
 Positive and negative
charges must balance!

34. Reminders
 Multiple cations can form an
ionic bond with multiple
anions!
 Electrons lost from cations
must equal electrons gained by
anions.

35. Examples
 Sodium and Iodine
 Aluminum and Bromine
 Magnesium and Nitrogen

36. Write the FormulaWrite the Formula
 Potassium and ChlorinePotassium and Chlorine
 Magnesium and OxygenMagnesium and Oxygen
 Sodium and PhosphorusSodium and Phosphorus
 Barium and PhosphorusBarium and Phosphorus

37. Vocabulary
 Ionic Bond – the
electrostatic forces that
hold ions together
 Chemical Formula –
shows the kinds and
numbers of ions;
represents ratio called a
“formula unit”

38. Transition MetalsTransition Metals
 Ions of manyIons of many
transition metals cantransition metals can
take on multipletake on multiple
chargescharges
 Ex: Chromium +2,Ex: Chromium +2,
+3, +6+3, +6

39. Transition MetalsTransition Metals
 Ionic charge designated by Roman NumeralIonic charge designated by Roman Numeral
 Copper (III) is CuCopper (III) is Cu 3+3+

40. More Examples
 Aluminum and Sulfur
 Lead (IV) and Bromine
 Mercury (II) and Iodine
 Strontium (Sr) and Oxygen
 Iron (III) and Oxygen

41. Properties of Ionic Compounds
 Crystalline solids at room
temperature
 Atoms arranged in
repeating, three-dimensional
patterns

42. Properties of Ionic Compounds
 Extremely high melting
points
 Conduct electric current
when dissolved in water

43. Names of IonsNames of Ions
 Anions (negative) areAnions (negative) are
named by adding “-ide” tonamed by adding “-ide” to
their elemental names.their elemental names.
 Cl = chlorineCl = chlorine
 ClCl--
= chloride ion= chloride ion

44. Ions of Transition Metals
 REMEMBER: Transition
metal ions are named for their
charge
 Fe2+
called iron (II) ion
 Fe3+
called iron (III) ion

45. Ions of Transition Metals
 Also must occur for some non-transition metals: Tin
and Lead

46. Write the Formula for These Compounds!
1. Mercury(II) Iodide
2. Sodium Carbonate
3. Copper(II) Oxide
4. Potassium Oxide
5. Barium Sulfate
6. Berrylium (Be) Nitride
7. Manganese(III) Iodide
8. Tin(IV) Phosphate
9. Ammonium Sulfide
10. Titanium(II) Hydroxide

47. A Brief ReviewA Brief Review

48. 1.1. Draw the LewisDraw the Lewis
structure for Nitrogen.structure for Nitrogen.
2.2. What is the octet rule?What is the octet rule?
3.3. How many electronsHow many electrons
would be lost/gained bywould be lost/gained by
a Calcium ion as ita Calcium ion as it
ionizes?ionizes?
4.4. Name two properties ofName two properties of
ionic compounds.ionic compounds.
5.5. Write the formula for:Write the formula for:
 Sodium and NitrogenSodium and Nitrogen
 Iron (III) and OxygenIron (III) and Oxygen
 Magnesium and NitrateMagnesium and Nitrate

49. Naming Ionic Compounds

50. Types of QuestionsTypes of Questions
 Write a formula givenWrite a formula given
the name of an ionicthe name of an ionic
compound.compound.
 Write the name of anWrite the name of an
ionic compoundionic compound
given the formula.given the formula.

51. Ionic Compound NamesIonic Compound Names
 Write cation first.Write cation first.
 Add Roman numeral for transitionAdd Roman numeral for transition
metals, tin, and lead.metals, tin, and lead.
 Write anion second, adding “-ide”Write anion second, adding “-ide”
to the element.to the element.
 Leave polyatomic ion names alone.Leave polyatomic ion names alone.

52. (Use Polyatomic Ion List…)(Use Polyatomic Ion List…)
 CaCa22COCO33
 AlAl22OO33
 CuFCuF22
 AgNOAgNO33

53. 1.1. Why are some elementsWhy are some elements
more stable as ions than asmore stable as ions than as
atoms?atoms?
2.2. Write the formulas andWrite the formulas and
describe the majordescribe the major
difference between copper(I)difference between copper(I)
nitride and copper(II) nitride.nitride and copper(II) nitride.
3.3. Criticize this statement: “TheCriticize this statement: “The
ionic charge of any metalionic charge of any metal
may be determined from themay be determined from the
position of the element inposition of the element in
the periodic table.”the periodic table.”
4.4. Explain what is wrong withExplain what is wrong with
each ionic formula:each ionic formula:
CsClCsCl22 BrOBrO22
LiNeLiNe BaBa22SS22
5.5. Lead (IV) PhosphateLead (IV) Phosphate
6.6. Barium IodideBarium Iodide
7.7. Mercury (I) OxideMercury (I) Oxide
8.8. Ammonium CarbonateAmmonium Carbonate
9. AlNO3
10. SnF4
11. Mn3N2
12. ZnS
Cation
Anion
A B C D
M MA2 (13) (14) MD
N (15) N4B (16) (17)
P PA3 (18) PC P2(D)3