Formation of Ions
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Transcript of Formation of Ions
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Formation of Ions
• Atoms lose or gain electrons only from their outermost energy level (valence shell)
• The number of electrons lost or gained determines the “ion charge”. An ion is a “charged” atom (+) or (-).
• One electron lost leaves an atom with one extra proton which gives it a 1+ charge.
• One electron gained gives an atom a 1- charge
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How Ions Form
• Atoms try to have the same number of outer electrons as the Noble Gas atom closest to it (which is usually 8 outer electrons).
• Nonmetals tend to gain 1, 2, or 3 electrons to have 8 outer electrons (form – charged ions).
• Metals tend to lose their 1, 2 or 3 outer electrons to go down to the next energy level with 8 outer electrons (form + charged ions).
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Warm ups Atom Group Period Number of
outer electrons
Ion charge Lewis dot diagram
Cl
F
Ba
C
Ne
S
O
Remember in the Lewis Dot diagram, you only put the electrons in the outer most shell.
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Warm ups Atom Group Period Number of
outer electrons
Ion charge Lewis dot diagram
Cl VII A 3 7 1-
F VII A 2 7 1-
Ba II A 6 2 2+
C IV A 2 4 4+ or 4-
Ne VIII A 2 8 none
S VI A 3 6 2-
O VI A 2 6 2-
Remember in the Lewis Dot diagram, you only put the electrons in the outer most shell.
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• Reminders: • 1. In a neutral atom the number of protons
equals the number of electrons. • 2. An atom can NEVER gain or lose protons • 3. The number of protons equals the atomic
number
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Write the ion for each of the following elements based on their locations on the
periodic table
1. Fluorine F-1
2. Magnesium 3. Aluminum4. Sodium5. Nitrogen 6. Hydrogen 7. Argon 8. Barium 9. Sulfur
Check with your seat mate when you are done.
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Write the ion for each of the following elements based on their locations on the
periodic table
1. Fluorine F1-
2. Magnesium Mg2+
3. Aluminum Al3+
4. Sodium Na1+
5. Nitrogen N3-
6. Hydrogen H1+
7. Argon Ar (no charge)8. Barium Ba2+
9. Sulfur S2-
Check with your seat mate when you are done.
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Write the ion for each of the following elements based on their locations on the
periodic table Answers:1. Fluorine F1-
2. Magnesium Mg2+
3. Aluminum Al3+
4. Sodium Na1+
5. Nitrogen N3-
6. Hydrogen H1+
7. Argon Ar (no charge)8. Barium Ba2+
9. Sulfur S2-
Check with your seat mate when you are done.
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Now we are writing compounds
Hydrogen + Fluorine H+1 + F-1 HFHydrogen Fluoride
Magnesium + Sulfur Mg+2 + S-2 MgS+2 + -2 0 Magnesium sulfide
Aluminum + Nitrogen Al+3 + N-3 AlN+3 + -3 0 Aluminum Nitride
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WHAT IF CHARGES DON’T EQUAL 0
• Hydrogen + Sulfur H+1 + S-2
No match
H S
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What can we do
• GET ANOTHER HYDROGEN
H
H S
NOW HAVE 2 HYDROGEN &1 SULFUR
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Writing and Naming
H2S1 don’t write the 1
Like in math – you don’t write 1x just x
So it is H2S
name is hydrogen sulfide
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Use the matching kits
Where I had the arrows they have lines – every line needs a partner
Remember – drop final syllable of
second element then add ide
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Predicting Ionic ChargesGroups 3 - 12:
Many transition elements have more than one possible oxidation state.Iron(II) = Fe2+ Iron(III) = Fe3+
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Predicting Ionic ChargesGroups 3 - 12:
Many transition elements have more than one possible oxidation state.Copper (II) = Cu2+Copper(I) = Cu1+
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Practice: Use your Periodic Table to write balanced chemical formulas for:
• Magnesim Bromide• Sodium sulfide• Copper (I) oxide• Potassium nitride• Zinc iodide• Aluminum oxide• Nickel (III) sulfide
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Practice: Use your Periodic Table to write balanced chemical formulas for:
• Magnesium Bromide Mg2+ Br1- = MgBr2
• Sodium sulfide Na1+ S2- = Na2S
• Copper (I) oxide Cu1+ O2- = Cu2O
• Potassium nitride K1+ N3- = K3N
• Zinc iodide Zn2+ I1- = ZnI2
• Aluminum oxide Al3+ O2- = Al2O3
• Nickel (III) sulfide Ni3+ S2- = Ni2S3
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Group Ions• “Group Ion” – an ion that is made of a group
of atoms and more than one element that acts like a single ion
• Group ions can NOT be found on the Periodic Table, but you will be given a list of them.
• Group ions each have their own name and charge.
• Most Group ions have a negative charge and contain the element oxygen
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Examples of Group Ions
• Nitrate = NO31-
• Sulfate = SO42-
• Hydroxide = OH1-
• Phosphate = PO43-
• Carbonate = CO32-
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Writing Formulas with Group Ions
• Treat the ENTIRE GROUP as having that charge• If more than one of Group Ion is needed then
put the group into parenthesis ( NO31-)
• Put the subscripts for more than one group below and to the right of the parenthesis (NO3
1-)2 • Example of a formula Calcium nitrate Ca2+
NO31- balanced is Ca(NO3)2
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Practice – Write these formulas of compounds with Group Ions
• Aluminum hydroxide• Sodium phosphate• Iron (III) sulfate• Barium carbonate• Copper (II) nitrate
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Answers
• Aluminum hydroxide Al3+ OH1- = Al(OH)3
• Sodium phosphate Na1+ PO43- = Na3PO4
• Iron (III) sulfate Fe3+ SO42- = Fe2(SO4)3
• Barium carbonate Ba2+ CO32- = BaCO3
• Copper (II) nitrate Cu2+ NO31- = Cu(NO3)2
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Writing Names of Chemical Formulas
• The name of the positive metal ion never changes• If the metal ion has more than one possible
charge then use parenthesis ( ) and put the ion charge as a Roman numeral in the ( )
• If the nonmetal is a single element then change the ending to “ide” Example: chlorine becomes “chloride”, oxygen becomes “oxide”
• Group Ions have their own name like NO31- is
nitrate, SO42- is sulfate
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Practice: Name these ionic formulas
• AlCl3
• CaS• Cu(OH)2
• Na3N
• MgSO4
• PbO2
• AgCO3
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Practice: Name these ionic formulas
• AlCl3 Aluminum chloride• CaS Calcium sulfide• Cu(OH)2 Copper (II) hydroxide
• Na3N Sodium nitride
• MgSO4 Magnesium sulfate
• PbO2 Lead (IV) oxide
• AgCO3 Silver carbonate