Chapter 5: Ions and Ionic Compounds
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Transcript of Chapter 5: Ions and Ionic Compounds
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Ion: an atom or group of atoms that has a charge as a result of losing or gaining one or more electrons
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Ca+ion: positively charged ion
Formed from a metal atom losing electrons
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Anion: negatively charged ion
Formed from a nonmetal atom gaining electrons
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+1 0-1-2
-3+/- 4
+2
+3
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Metals can have various charges, so you MUST specify which one you have!
The charge of a metal is indicated by a Roman Numeral.
Exceptions: Groups 1 & 2, Silver (Ag), and Zinc (Zn) have only one charge, so they do not get Roman numerals in their names!
Examples:1.) Copper (II) = Cu+2
2.) Iron (III) = Fe+2
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Name the following transition metal ions:1.) Cr+2
2.) Cr+3
3.) Mn+2
4.) Mn+3
5.) Pt+2
6.) Pt+4
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Name the following transition metal ions:1.) Cr+2 Chromium (II)2.) Cr+3 Chromium (III)3.) Mn+2 Manganese (II)4.) Mn+3 Manganese (III)5.) Pt+2 Platinum (II)6.) Pt+4 Platinum (IV)
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Determine if the following ions are cations (metal) or anions (nonmetal):
1.) Calcium ion2.) Nitrogen ion3.) Potassium ion4.) Bromine ion5.) Oxygen ion6.) Lead (IV) ion
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Determine if the following ions are cations or anions:
1.) Calcium ion: cation2.) Nitrogen ion: anion3.) Potassium ion: cation4.) Bromine ion: anion5.) Oxygen ion: anion6.) Lead (IV) ion: cation
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Element Symbol and Charg
e
Metal or Nonmeta
l?
Anion or
Cation?
Sodium Na+1 Metal CationFluorine
Magnesium
Copper (II)
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Element Symbol and Charg
e
Metal or Nonmeta
l?
Anion or
Cation?
Sodium Na+1 Metal CationFluorine F-1 Nonmetal Anion
Magnesium
Mg+2 Metal Cation
Copper (II) Cu+2 Metal Cation
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Ion # of protons
# of electrons
S-2
Al+3
Fe+2
N-3
Ca+2
C-4
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Ion # of protons
# of electrons
S-2 16 18Al+3 13 10Fe+2 26 24N-3 7 10
Ca+2 20 18C-4 6 10
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Ion # of protons
# of electrons
Na+1
O-2
Zn+2
F-1
Mg+2
P-3
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Ion # of protons
# of electrons
Na+1 11 10O-2 8 10
Zn+2 30 28F-1 9 10
Mg+2 12 10P-3 15 18
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Octet Rule: Atoms lose or gain electrons to match the valence electron configuration of a noble gas.
Atoms gain or lose electrons because they want to be more stable.
Full valence shells = stable atoms
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1.) Determine number of electrons2.) Write electron configuration
Example: Fluorine ion = F-1
Fluorine ion has 10 electronsElectron configuration is 1s22s22p6
Neon also has 10 electrons and has the same electron configuration, so F-1 and neon are isoelectronic.
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Determine the electron configuration of the following ions and write which noble gas they are isoelectronic with.
1.) Lithium ion2.) Magnesium ion3.) Calcium ion
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Determine the electron configuration of the following ions and write which noble gas they are isoelectronic with.
1.) Lithium ion (2 electrons): 1s2
isoelectronic with helium2.) Magnesium ion (10 electrons): 1s22s22p6
isoelectronic with neon3.) Calcium ion (18 electrons): 1s22s22p63s23p6
isoelectronic with argon
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Transfer of electrons Metal + Nonmetal Ions come together due to electrostatic
attraction (opposites attract)
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Determine if the following compounds are ionic:
NaCl : metal and nonmetal = ionic CO2 : metal and nonmetal = not ionic
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Determine if the following compounds are ionic:
1.) CO2.) MgCl23.) CaBr2
4.) H2O5.) LiF
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Determine if the following compounds are ionic:
1.) CO = nonmetal + nonmetal = not ionic2.) MgCl2 = metal + nonmetal = ionic3.) CaBr2 = metal + nonmetal = ionic4.) H2O = metal + metal = not ionic5.) LiF = metal + nonmental = ionic
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http://www.visionlearning.com/library/module_viewer.php?mid=55
Na (1 valence e-) + Cl ( 7 valence e-) Na+ ion (8 valence e-) + Cl- ion (8 valence e-):
The result is a positively charged sodium ion (left) and a negatively chorline atom (right). Both have full outer shells!
Soidum (on the left) loses its one valence electron to chlorine (on the right)
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Ionic compounds organize in characteristic crystal lattice of alternating positive and negative ions.
Unit Cell: The smallest portion of a crystal lattice that shows the three-dimensional pattern of the entire lattice.
Image from: http://www.docbrown.info/page04/4_72bond2.htm
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When ionic bonds are formed, the energy that is released is called the lattice energy.
Alternatively, you can think of it as the amount of energy required to break the ionic bonds of a compound.
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Sodium chloride (NaCl) dissolves in water: low lattice energy
Magnesium oxide (MgO) does not dissolve in water: high lattice energy
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Solid at room temperature High boiling/melting points Dissolve in water Conduct electricity Hard (the crystal is able to resist a large
force applied to it) Brittle (applied force results in fracture, not
dents)
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1.) Identify the state of matter-should be a solid at room temperature
2.) Tap it-will not break (hard) OR-will fracture if it breaks (brittle)
3.) Heat it-will only melt at high temperatures
4.) Shock it-will conduct electricity
5.) Dissolve it in water-will dissolve in water
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You tap the crystal and they shatter but still retain their sharp edges.
You heat the substance and after 2-3 minutes of heating it does not melt.
It dissolves in water and conducts electricity.
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You tap the crystal and they shatter but still retain their sharp edges.
Yes You heat the substance and after 2-3
minutes of heating it does not melt.
It dissolves in water and conducts electricity.
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You tap the crystal and they shatter but still retain their sharp edges.
Yes You heat the substance and after 2-3
minutes of heating it does not melt.Yes
It dissolves in water and conducts electricity.
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You tap the crystal and they shatter but still retain their sharp edges.
Yes You heat the substance and after 2-3
minutes of heating it does not melt.Yes
It dissolves in water and conducts electricity.
Yes
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Binary Ionic Compounds
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Metal + Nonmetal
Cation = positive charge
Anion = negative charge
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1. Write the symbol of the cation.
2. Write the charge of the cation.
3. Write the symbol of the anion.
4. Write the charge of the anion.
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5. Criss-cross the charges and write as subscripts without the signs.
6. Rewrite the formula.
7. Reduce the subscripts.
8. Check your answer (the compound should be neutral).
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1. Sodium oxide
2. Aluminum sulfide
3. Barium chloride
4. Magnesium oxide
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1. Sodium oxide = Na2O
2. Aluminum sulfide = Al2S3
3. Barium chloride = BaCl2
4. Magnesium oxide = MgO
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The metal will have its charge listed behind its name as a roman numeral in parentheses.
Example:Iron(III) bromide = FeBr3
Exceptions: Groups 1&2, Ag, and Zn don’t have Roman numerals because they have only one charge!
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Copper(II) chloride
Tin(IV) iodide
Chromium(III) oxide
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Copper(II) chloride = CuCl2
Tin(IV) iodide = SnI4
Chromium(III) oxide = Cr2O3
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Polyatomic Ionic Compounds
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An ion made up of one atom.
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A charged group of 2 or more covalently bonded atoms.
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When writing the polyatomic ion, put parentheses around the formula.
When criss-crossing the charges, drop the subscript behind the parentheses.
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NEVER change any subscripts inside the parenthesis.
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1. Sodium Phosphate2. Calcium Nitrate3. Magnesium Hydroxide4. Potassium Sulfate5. Calcium Acetate6. Chromium (III) Nitrite7. Magnesium Hydrogen Carbonate
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1. Sodium Phosphate: Na3PO4
2. Calcium Nitrate: Ca(NO3)2
3. Magnesium Hydroxide: Mg(OH) 2
4. Potassium Sulfate: K2SO4
5. Calcium Acetate: Ca(C2H3O2) 2
6. Chromium (III) Nitrite: Cr(NO2) 3
7. Magnesium Hydrogen Carbonate: Mg(HCO3)2
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Binary Ionic Compounds
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1. Write the name of the cation.
2. Write the name of the anion, change the ending to –ide.
Examples: RbCl = rubidium chloride K2S = potassium sulfide
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1. CaBr2
2. MgS
3. NaBr
4. AlP
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1. CaBr2 = calcium bromide
2. MgS = magnesium sulfide
3. NaBr = sodium bromide
4. AlP = aluminum phosphide
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1. Write the name of the cation.
2. Write the charge of the cation using a roman numeral inside of parentheses.
3. Write the anion, change the ending to –ide.
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Metals in Groups 1 and 2, Zinc and Silver are the only metals that will not follow the stock system because they only ever have one charge.
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1. CuCl2 = copper(II) chloride
2. FeCl2
3. CuBr
4. Cu2O
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1. CuCl2 = copper(II) chloride
2. FeCl2 = iron(II) chloride
3. CuBr = copper(I) bromide
4. Cu2O = copper(I) oxide
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Polyatomic Ionic Compounds
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1. Name the cation.
2. Name the anion.
3. If the anion is monatomic, change the ending to –ide.
4. Note: Only one polyatomic ion is a cation.
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1. Ca3(PO4) 2
2. NaOH3. Ba(C2H3O2)2
4. MgSO4
5. (NH4)2S
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1. Ca3(PO4) 2 : Calcium Phosphate2. NaOH : Sodium Hydroxide3. Ba(C2H3O2)2 : Barium Acetate4. MgSO4 : Magnesium Sulfate5. (NH4)2S : Ammonium Sulfide