review of ions objective: when atoms give away electrons
TRANSCRIPT
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REVIEW of IONS
OBJECTIVE: When atoms give away electrons
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IONS
ION
What is it?An atom that
LOST/GAINEDelectron(s)
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IONS
Goal is to get to the NEAREST Noble Gas
RULES
1. If you go LEFT, you become POSITIVE.
2. If you go RIGHT, you become NEGATIVE
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IONS
Ions that LOSE electrons have a
POSTIVE charge
called
cations
pronounced “cat – ions”
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IONS
All metals become
CATIONS
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IONS
USE HALF SHEET FOR TRANSITION METALS
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IONS
Ions that GAINS electrons have a NEGATIVE
charge
called
anions
pronounced “an – ions”
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IONS
Ex: CN-
NH4+
CO32-
Because these ions are made from two or more atoms, they are called
polyatomic ions
Some ions are made from two or more atoms
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IONS
-ite has less oxygenthan –ate
Memorize? Kind of
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IONSSummary & Review1. What is an ion?
2. What are the two types of ions?
3. Which ions gains electrons: cations or anions?
4. Predict the charge of each atom if it were to become an ion:
Ca, Cl, Cu, F, Fe, Li, Na, N, O
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Ionic Compounds
OBJECTIVE: Joining Cations + Anions to make compounds
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Ionic Compounds
Na+ + Cl- NaCl cation anion ionic compound
forumula
NaCl joined byIONIC BOND
IONIC BOND = giving away/gaining electrons
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Ionic Compounds
Li+ + Cl-
K+ + Cl-
Ca2+ + Cl-
Li+ + O2-
Ca2+ + O2-
LiCl
KCl
CaCl2
Li2O
CaOCharges must cancel and = 0
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Ionic Compounds
Cu+ + CH3COO-
NH4+ + Cr2O7
-
Mg2+ + OH-
CuCH3COO
NH4Cr2O7
Mg(OH)2
Parenthesis for POLYATOMIC
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Ionic CompoundsWrite formula for ionic compounds
1. Al3+ + O2- 2. Fe2+ + Cl-
3. Na+ + HCO3-
4. Na+ + NO2-
5. Ca2+ + PO43-
6. H+ + SO42-
7. Mg2+ + OH- 8. Fe3+ + Cl-
9. NH4+ + PO4
3-
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1. Naming Ionic Compounds
Write from 1 to 5 in Roman Numerals
III
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1. Naming Ionic Compounds
OBJECTIVE: Learn how to name compounds like NaHCO3
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1. Naming Ionic Compounds
First Name + Last Name = Full Name
only TRANSITION METALS
have roman numerals
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Cations with Roman Numerals in BOLD
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1. Naming Ionic Compounds
1.Start with CATION, always
2.Name the anion using the suffix “IDE”. If anion is polyatomic…
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1. Naming Ionic Compounds
“uncross”numbers to figure our
roman numeral forcation
FeCl3 Cr2O3
Cu2O Mn3N2
Mn(NO2)3
Mn(NO3)3
Mn(NO3)2
If no numbers then
1. Figure out charge of anion
FeO CrOMnO CoN
CrPO4 ZnCrO7
CuSO4 CuNO3
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1. Naming Ionic Compounds
1.Start with CATION, always2.If cation is Transition Metal check
table for roman numerals3.Name the anion using the suffix
“IDE”. If anion is polyatomic…4.That’s it!
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1. Naming Ionic Compounds
Writing formulas from names of ionic compounds
1.Write anion and charge.
2. Write cation and charge. 3. Cross charges and write formula.
-ATE -ITEhalf sheet
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Naming Ionic Compounds
1. Sodium Chloride2. Lithium Fluoride3. Iron(II) Chloride4. Sodium Nitrate5. Magnesium
Hydroxide6. Sodium Acetate7. Ammonium Chloride8. Hydrogen Peroxide9. Sodium Carbonate10.Ammonium Phosphate
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1. Naming Ionic CompoundsSUMMARY & REVIEW
Formula to Name1. Start with cation
2. When to use roman numerals?3. Then add…to anion
4. What about polyatomic ions?
Name to Formula5. Start with anion – LAST NAME
6. What if anion ends in ATE or ITE?7. Write symbol for cation – FIRST NAME
8. Roman numerals?
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4. Lewis Dot Structures
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7. Lewis Structures
1.Write elements 2. Count total number of valence
e3. LEAST electronegative is in
the center (usually CARBON)4.Draw bond5.Then draw dots until you run
out6.Make double/triple bonds if
necessary
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7. Lewis Dot Structures
Exceptions to the Octet Rule
1. Less than 82. More than 8
3. Polyatomic Ions
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7. Lewis Dot Structures
Exceptions to the Octet Rule
1. Less than 8
Group 1 &Beryllium and Boron
BeCl2 BCl3
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4. Lewis Dot Structures
Exceptions to the Octet Rule
2. More than 8 Phosphorus ,Sulfur and
XenonPCl5 SF6 XeF4
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4. Lewis Dot Structures
Exceptions to the Octet Rule
3. Polyatomic IonsCations AnionsSUBTRACT electrons
ADD electrons
add brackets [ ]