Ionic Compounds
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Transcript of Ionic Compounds
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Ionic Compounds
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Lewis Dot DiagramsChemical Interactions Occur between
the Valence Electrons
Dots: represent valence electrons
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When atoms combine to make molecules, they form chemical bonds.
Valence electron interaction
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Forming Chemical Bonds
• Octet Rule Atoms will form bonds by: – Sharing– Giving or – Takingelectrons to complete their octet
Higher energy farther away from nucleus
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Atoms form ions to have stable electron configurations (similar
to noble gases)
hh
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Ionic Bonds
• Ionic Bonds form when one atom (nonmetal) gains electrons and the other atom (metal) loses electrons in order to gain stability.
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• Ionic Bonds form between a metal (cation) and a nonmetal (anion).
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To form an ion, lithium will most likely:
1 2 3 4
5% 5%
91%
0%
1. Gain 1 electron2. Gain 2 electrons3. Lose 1 electron4. Lose 2 electrons
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Forming Chemical Bonds• Lithium
–Better to lose 1 electron or to gain 7
electrons?
X
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Therefore, as an ion lithium will have what charge?
1 2 3 4
73%
0%
27%
0%
1. 1+2. 2+3. 1-4. 2-
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Ionic Bonds • Atoms gain or lose its electrons
+
NaCl - salt
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Chemical Interactions Occur between the Valence Electrons
Lewis structures are simpler to do & see
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Formation of MgCl2
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Formation of Na2S
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• Write down the chemical formula for Aluminum Flouride
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Formation of AlF3
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Today is a practice Day!
• We need to be able to name ions given chemical formula
• We need to be able to determine the chemical formula given the name
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Valence Electrons Noble Gas Structure = Octet
1,2 3,4,5,6,7,8
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IONIC BONDS / Cations and Anions
Cation – positive ionsTransition Metals use
Roman Numerals to tell you the ox # Anion – negative ions
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Oxidation Numbers
• Oxidation Numbers- indicated # of e’ lost, gained or shared.
Ex. Oxidation number of chlorine is -1
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Halogens will have an oxidation number of:
1 2 -1 -2
0% 0%0%0%
1. +12. +23. -14. -2
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Alkaline earth metals will have an oxidation number of:
1 2 -1 -2
0% 0%0%0%
1. +12. +23. -14. -2
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We will name binary compounds together
• Using pages 156- 158• Describe how to name cations
and anions when they are by themselves
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Naming Binary Ionic Compounds
• Write the name of the ionic compound, Ca2N3.
• Write the name of the ionic compound, K2O.
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What is the name of BeBr2?
Boron bro
mine
Beryllium bro
m...
Bromide beryll...
Beryllium bro
m...
Beryllide brom...
0% 0% 0%0%0%
1. Boron bromine2. Beryllium bromine3. Bromide beryllide4. Beryllium bromide5. Beryllide bromide
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Metals with Variable Charges
• Many transition metals can form more than one type of cation.
• For this reason, you must show the oxidation number in the name using Roman Numerals
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Naming Binary Ionic Compounds with Transition
Metal Cations• Write the name of
the ionic compound, Cu2O..
• Write the name of the ionic compound, NiS.
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What is the name for SnBr2?
Bromide Tin
Tin Bromide
Tin (I) Bromid...
Tin (II) B
romi...
Tin (III) B
rom...
Tin (IV) B
romi...
0% 0% 0%0%0%0%
1. Bromide Tin2. Tin Bromide3. Tin (I) Bromide4. Tin (II) Bromide5. Tin (III) Bromide6. Tin (IV) Bromide
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What is the name for FeI3?
Iron io
dide
Iron (I)
iodid...
Iron (II
) iodi...
Iron (II
I) iod...
0% 0%0%0%
1. Iron iodide2. Iron (I) iodide3. Iron (II) iodide4. Iron (III) iodide
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What is the name for MnS?
Manganese
sulf..
.
Manganese
(I) ...
Manganese
(II)...
Manganese
(III...
0% 0%0%0%
1. Manganese sulfide2. Manganese (I) sulfide3. Manganese (II) sulfide4. Manganese (III) sulfide
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Exceptions:• 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+)
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Writing Formulas for Binary Ionic Compounds
• Write the formula for barium iodide.
• Write the formula for sodium oxide.
• Write the formula for aluminum nitride.
• Write the formula for copper (I) sulfide.
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Criss-Cross Method for Writing Formulas
- You can write the oxidationnumber and criss-cross them as subscripts.
- Note – if not in lowest termsyou must reduce the subscripts(ex. Magnesium oxide)
Al3+ S2-2 3
= Al2S3
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What is the formula for aluminum bromide?
AlBr AlBr2
Al3Br Br3Al
AlBr3
0% 0% 0%0%0%
1. AlBr2. AlBr2
3. Al3Br4. Br3Al5. AlBr3
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What is the formula for magnesium oxide?
MgO
Mg2
O2
MgO
2 M
g2O
OMg
0% 0% 0%0%0%
1. MgO2. Mg2O2
3. MgO2
4. Mg2O5. OMg
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Write the formula for titanium (II) chloride.
TiCl Ti2Cl
TiCl2 Ti2Cl2
0% 0%0%0%
1. TiCl2. Ti2Cl3. TiCl24. Ti2Cl2
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Write the formula for tin (IV) oxide.
SnO
SnO4
SnO2
Sn4O
Sn2O
0% 0% 0%0%0%
1. SnO2. SnO4
3. SnO2
4. Sn4O5. Sn2O
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POLYATOMIC IONS• Not all compounds are made of only 2
types of atoms• poly – “many”
Memorize the polyatomic ions from p. 170.
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Tricks for Polyatomic Naming
Perchlorate per+root+ate ClO4-1
chlorate root+ate ClO3-1
chlorite root+ite ClO2-1
Hypochlorite hypo+root+ite ClO-1
Prefixes and suffixes designate number of oxygens
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Naming Polyatomic Ionic Compounds
• Polyatomic ionic compounds are named just like binary ionic compounds.
• Exception: be sure to enclose the polyatomic ion in parentheses before writing the subscript (only necessary if subscript is not 1).
• Ex. Barium hydroxide = Ba(OH)2
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Write the formula for Calcium Nitrate.
CaNO2
Ca(NO2)2
Ca2NO3
Ca2NO2
Ca(NO3)2
0% 0% 0%0%0%
1. CaNO2
2. Ca(NO2)2
3. Ca2NO3
4. Ca2NO2
5. Ca(NO3)2
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Write the formula for Magnesium Phosphate.
MgP
O4
Mg3
(PO4)2
Mg4
(PO3)2
MgP
O3
Mg(P
O4)2
0% 0% 0%0%0%
1. MgPO4
2. Mg3(PO4)2
3. Mg4(PO3)2
4. MgPO3
5. Mg(PO4)2
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Naming Ionic Compounds