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Transcript of 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note...
![Page 1: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/1.jpg)
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Chemistry 102Section 6.4 Ionic Compounds
& Section 6.5 Molecular
Compounds and Acids
Unit II Note pack, pages 9-13
![Page 2: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/2.jpg)
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Ionic Compounds
A. Writing Formulas for Binary Ionic Compounds1. What are Binary Ionic Compounds?
Binary compounds have just 2 elements.Binary ionic compounds have 2 elements
that are from opposite sides of the table, a cation and an anion.
(metal) (nonmetal)
![Page 3: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/3.jpg)
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Ionic Compounds
A. Writing Formulas for Binary Ionic Compounds
2. What are the “rules” for writing Binary Ionic Compounds?
a. Write the metal (positive) ion first
b. Write the nonmetal (negative) ion last
c. The net charge for the compound must add up to zero (total positive + total negative = 0)
d. Use subscripts to indicate how many of each ion you need to “balance” the charge.
e. CrissCross Method
![Page 4: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/4.jpg)
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Ionic Compounds
• Practice Writing Formulas for Binary Ionic Compounds
Write the formula for the binary ionic compound formed between magnesium and chlorine. Then NAME IT.
![Page 5: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/5.jpg)
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Ionic Compounds
• Practice Writing Formulas for Binary Ionic Compounds
Write the formula for the binary ionic compound formed between magnesium and chlorine. Then NAME IT.
Mg +2 + Cl- MgCl2 Magnesium Chloride
![Page 6: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/6.jpg)
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Ionic Compounds
• Practice Writing Formulas for Binary Ionic Compounds
Write the formula for the binary ionic compound formed between magnesium and chlorine. Then NAME IT.
Mg +2 + Cl- MgCl2 Magnesium Chloride
Write the formula for the binary ionic compound formed between sodium and oxygen. Then NAME IT.
![Page 7: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/7.jpg)
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Ionic Compounds
• Practice Writing Formulas for Binary Ionic Compounds
Write the formula for the binary ionic compound formed between magnesium and chlorine. Then NAME IT.
Mg +2 + Cl- MgCl2 Magnesium Chloride
Write the formula for the binary ionic compound formed between sodium and oxygen. Then NAME IT.
Na+ + O-2 Na2O Sodium Oxide
![Page 8: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/8.jpg)
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Ionic Compounds
• Practice Writing Formulas for Binary Ionic Compounds
(pg. 10)Write the formula for the binary ionic compound between aluminum and sulfur, and
NAME IT.
![Page 9: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/9.jpg)
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Ionic Compounds
• Practice Writing Formulas for Binary Ionic Compounds
(pg. 10)Write the formula for the binary ionic compound between aluminum and sulfur, and
NAME IT.
Al+3 + S-2 Al2S3 Aluminum sulfide
![Page 10: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/10.jpg)
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Ionic Compounds
• Practice Writing Formulas for Binary Ionic Compounds
(pg. 10)Write the formula for the binary ionic compound between aluminum and sulfur, and
NAME IT.
Al+3 + S-2 Al2S3 Aluminum sulfide
Write the formula for the binary ionic compound between iron (III) and oxygen, and NAME IT.
![Page 11: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/11.jpg)
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Ionic Compounds
• Practice Writing Formulas for Binary Ionic Compounds
(pg. 10)Write the formula for the binary ionic compound between aluminum and sulfur, and
NAME IT.
Al+3 + S-2 Al2S3 Aluminum sulfide
Write the formula for the binary ionic compound between iron (III) and oxygen, and NAME IT.
Fe+3 + O-2 Fe2O3 Iron (III) oxide
![Page 12: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/12.jpg)
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Ionic Compounds
• Practice Writing Formulas for Binary Ionic Compounds
(pg. 10)Write the formula for the binary ionic compound between aluminum and sulfur, and
NAME IT.
Al+3 + S-2 Al2S3 Aluminum sulfide
Write the formula for the binary ionic compound between iron (III) and oxygen, and NAME IT.
Fe+3 + O-2 Fe2O3 Iron (III) oxide
Write the formula for the binary ionic compound between calcium and sulfur, and NAME IT.
![Page 13: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/13.jpg)
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Ionic Compounds
• Practice Writing Formulas for Binary Ionic Compounds
(pg. 10)Write the formula for the binary ionic compound between aluminum and sulfur, and
NAME IT.
Al+3 + S-2 Al2S3 Aluminum sulfide
Write the formula for the binary ionic compound between iron (III) and oxygen, and NAME IT.
Fe+3 + O-2 Fe2O3 Iron (III) oxide
Write the formula for the binary ionic compound between calcium and sulfur, and NAME IT.
Ca+2 + S-2 CaS Calcium sulfide
![Page 14: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/14.jpg)
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Polyatomic Ions (pg 10)
A. What is a polyatomic ion?
a tightly bound group of atoms that behaves as a unit and carries a charge
B. What endings to polyatomic ions receive when naming them?
most polyatomic ions receive endings of either –ite or –ate.
![Page 15: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/15.jpg)
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Polyatomic ions
C. There are 3 important exceptions (to the end of their names), they are:
Ammonium cation (NH4+)
Two polyatomic ions end in –ide;
cyanide (CN-) and
hydroxide (OH-)
![Page 16: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/16.jpg)
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Polyatomic Ions
• For “D”, see Chart 6.4
• Example:
• Ammonium NH4+
![Page 17: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/17.jpg)
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Ternary Ionic Compounds
A. Define ternary ionic compounds:
A compound that contains atoms of three, or more, different elements
Remember, they are still just two ions, and all rules from before still apply.
B. Write the formula for lithium nitrate, a ternary compound.
Li + + NO3- LiNO3
![Page 18: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/18.jpg)
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Ternary Ionic CompoundsC. Sometimes, we need to take more than one polyatomic
ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis.
D. Write the formula for aluminum carbonate:
Al+3 + CO3-2
E. Write the formula for ammonium sulfate:
F. Write the formula for calcium phosphate:
![Page 19: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/19.jpg)
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Ternary Ionic CompoundsC. Sometimes, we need to take more than one polyatomic
ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis.
D. Write the formula for aluminum carbonate:
Al+3 + CO3-2 Al2(CO3)3
E. Write the formula for ammonium sulfate:
F. Write the formula for calcium phosphate:
![Page 20: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/20.jpg)
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Ternary Ionic CompoundsC. Sometimes, we need to take more than one polyatomic
ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis.
D. Write the formula for aluminum carbonate:
Al+3 + CO3-2 Al2(CO3)3
E. Write the formula for ammonium sulfate:
NH4+ + SO4
-2
F. Write the formula for calcium phosphate:
![Page 21: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/21.jpg)
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Ternary Ionic CompoundsC. Sometimes, we need to take more than one polyatomic
ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis.
D. Write the formula for aluminum carbonate:
Al+3 + CO3-2 Al2(CO3)3
E. Write the formula for ammonium sulfate:
NH4+ + SO4
-2 (NH4)2SO4
F. Write the formula for calcium phosphate:
![Page 22: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/22.jpg)
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Ternary Ionic CompoundsC. Sometimes, we need to take more than one polyatomic
ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis.
D. Write the formula for aluminum carbonate:
Al+3 + CO3-2 Al2(CO3)3
E. Write the formula for ammonium sulfate:
NH4+ + SO4
-2 (NH4)2SO4
F. Write the formula for calcium phosphate:
Ca+2 + PO4-3
![Page 23: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/23.jpg)
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Ternary Ionic CompoundsC. Sometimes, we need to take more than one polyatomic
ion to balance the charge to 0. If this is happens, place the polyatomic ion in parenthesis and the subscript outside of the parenthesis.
D. Write the formula for aluminum carbonate:
Al+3 + CO3-2 Al2(CO3)3
E. Write the formula for ammonium sulfate:
NH4+ + SO4
-2 (NH4)2SO4
F. Write the formula for calcium phosphate:
Ca+2 + PO4-3 Ca3(PO4)2
![Page 24: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/24.jpg)
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Ternary Ionic Compounds
G. Do this one on your own, and compare with a partner.
Write the formula for beryllium carbonate.
![Page 25: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/25.jpg)
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Ternary Ionic Compounds
G. Do this one on your own, and compare with a partner.
Write the formula for beryllium carbonate.
Be+2 + CO3-2 BeCO3
Beryllium ion + carbonate beryllium carbonate
![Page 26: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/26.jpg)
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Practice Problems, pg. 11
1. Write the formulas for compounds formed AND name the compound from these pairs of ions:
a. NH4+1, SO3
2-
b. Calcium ion, phosphate ion
![Page 27: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/27.jpg)
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Practice Problems, pg. 11
1. Write the formulas for compounds formed AND name the compound from these pairs of ions:
a. NH4+1, SO3
2-
(NH4)2SO3 Ammonium Sulfite
b. Calcium ion, phosphate ion
![Page 28: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/28.jpg)
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Practice Problems, pg. 11
1. Write the formulas for compounds formed AND name the compound from these pairs of ions:
a. NH4+1, SO3
2-
(NH4)2SO3 Ammonium Sulfite
b. Calcium ion, phosphate ion
Ca+2 + PO4-3 Ca3(PO4)2
Calcium phosphate
![Page 29: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/29.jpg)
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Practice Problems, pg. 11
1. Write the formulas for compounds formed AND name the compound from these pairs of ions:
c. Al3+, NO3-1
d. Potassium ion, chromate ion
![Page 30: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/30.jpg)
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Practice Problems, pg. 11
1. Write the formulas for compounds formed AND name the compound from these pairs of ions:
c. Al3+, NO3-1
Al(NO3)3 Aluminum Nitrate
d. Potassium ion, chromate ion
![Page 31: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/31.jpg)
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Practice Problems, pg. 11
1. Write the formulas for compounds formed AND name the compound from these pairs of ions:
c. Al3+, NO3-1
Al(NO3)3 Aluminum Nitrate
d. Potassium ion, chromate ion
K+ + CrO4-2 K2CrO4
Potassium chromate
![Page 32: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/32.jpg)
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Practice Problems, pg. 11
2. Write formulas for these compounds
a. Lithium hydrogen sulfate __________
b. Chromium (III) nitrite ______________
c. Mercury (II) bromide ______________
d. Ammonium dichromate ___________
![Page 33: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/33.jpg)
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Practice Problems, pg. 11
2. Write formulas for these compounds
a. Lithium hydrogen sulfate _LiHSO4__
b. Chromium (III) nitrite _____________
c. Mercury (II) bromide ______________
d. Ammonium dichromate ___________
![Page 34: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/34.jpg)
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Practice Problems, pg. 11
2. Write formulas for these compounds
a. Lithium hydrogen sulfate _LiHSO4___
b. Chromium (III) nitrite __Cr(NO2)3_____
c. Mercury (II) bromide _______________
d. Ammonium dichromate ____________
![Page 35: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/35.jpg)
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Practice Problems, pg. 11
2. Write formulas for these compounds
a. Lithium hydrogen sulfate _LiHSO4__
b. Chromium (III) nitrite __Cr(NO2)3__
c. Mercury (II) bromide __HgBr2___
d. Ammonium dichromate _(NH4)2Cr2O7_
![Page 36: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/36.jpg)
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Section 6.5 Molecular Compounds and Acids (pg. 12)
A. Binary Molecular Compounds
1. What is a binary molecular compound?
A compound composed of 2 nonmetallic elements.
![Page 37: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/37.jpg)
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Section 6.5 Molecular Compounds and Acids
A. Binary Molecular Compounds2. We use prefixes when naming binary molecular
compounds: Refer to Table 6.5 and fill in the following:
Number Prefix Number Prefix
1 6
2 7
3 8
4 9
5 10
![Page 38: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/38.jpg)
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Section 6.5 Molecular Compounds and Acids
A. Binary Molecular Compounds2. We use prefixes when naming binary molecular
compounds: Refer to Table 6.5 and fill in the following:
Number Prefix Number Prefix
1 mono- 6 hexa-
2 di- 7 hepta-
3 tri- 8 octa-
4 tetra- 9 nona-
5 penta- 10 deca-
![Page 39: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/39.jpg)
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Section 6.5 Molecular Compounds and Acids
A. Binary Molecular CompoundsHow do we name binary molecular compounds? Say the name of the first element, say the name of the
second element, ending in ‘-ide’, and put the appropriate prefix in to indicate how many of each element there are in the formula:
If the prefix for the first element in a binary molecular compound is mono-, it may be dropped. However, it must be said if it is for the second element.
Don’t reduce the subscripts (like you did for binary ionic compounds)
![Page 40: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/40.jpg)
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Name these binary molecular compounds.
A. N2O -- ___________________
B. PCl3 -- ___________________
C. SF6 -- _____________________
D. OF2 -- _____________________
E. Cl2O8 -- ___________________
F. SO3 -- ____________________
![Page 41: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/41.jpg)
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Name these binary molecular compounds.
A. N2O -- _dinitrogen monoxide__
B. PCl3 -- ______________________
C. SF6 -- ________________________
D. OF2 -- _______________________
E. Cl2O8 -- _____________________
F. SO3 -- ______________________
![Page 42: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/42.jpg)
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Name these binary molecular compounds.
A. N2O -- _dinitrogen monoxide__
B. PCl3 -- _phosphorus trichloride_
C. SF6 -- ______________________
D. OF2 -- _____________________
E. Cl2O8 -- ____________________
F. SO3 -- ____________________
![Page 43: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/43.jpg)
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Name these binary molecular compounds.
A. N2O -- _dinitrogen monoxide__
B. PCl3 -- _phosphorus trichloride_
C. SF6 -- _sulfur hexafluoride___
D. OF2 -- _____________________
E. Cl2O8 -- _____________________
F. SO3 -- ____________________
![Page 44: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/44.jpg)
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Name these binary molecular compounds.
A. N2O -- _dinitrogen monoxide__
B. PCl3 -- _phosphorus trichloride_
C. SF6 -- _sulfur hexafluoride___
D. OF2 -- _oxygen difluoride___
E. Cl2O8 -- _dichlorine octoxide__
F. SO3 -- _sulfur trioxide___
![Page 45: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/45.jpg)
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Write the formulas for the following binary molecular compounds.
a. Nitrogen trifluoride ________________
b. Disulfur dichloride ________________
c. Dinitrogen tetraoxide _______________
d. Octoxygen dichloride _______________
e. Trinitrogen pentoxide _______________
![Page 46: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/46.jpg)
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Write the formulas for the following binary molecular compounds.
a. Nitrogen trifluoride ___NF3__________
b. Disulfur dichloride ________________
c. Dinitrogen tetraoxide ______________
d. Octoxygen dichloride _______________
e. Trinitrogen pentoxide _______________
![Page 47: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/47.jpg)
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Write the formulas for the following binary molecular compounds.
a. Nitrogen trifluoride ___NF3__________
b. Disulfur dichloride ___S2Cl2________
c. Dinitrogen tetraoxide ______________
d. Octoxygen dichloride ______________
e. Trinitrogen pentoxide ______________
![Page 48: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/48.jpg)
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Write the formulas for the following binary molecular compounds.
a. Nitrogen trifluoride ___NF3__________
b. Disulfur dichloride ___S2Cl2________
c. Dinitrogen tetraoxide __N2O4________
d. Octoxygen dichloride _______________
e. Trinitrogen pentoxide ______________
![Page 49: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/49.jpg)
49
Write the formulas for the following binary molecular compounds.
a. Nitrogen trifluoride ___NF3__________
b. Disulfur dichloride ___S2Cl2________
c. Dinitrogen tetraoxide __N2O4________
d. Octoxygen dichloride __O8Cl2_______
e. Trinitrogen pentoxide __N3O5_______
![Page 50: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/50.jpg)
50
Naming Acids (pg. 12, bottom)
A. What are acids?
Acids are compounds that produce H ions (H+) when dissolved in water
B. Write the chart that explains how to name acids: (next)
![Page 51: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/51.jpg)
51
Naming acids
![Page 52: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/52.jpg)
52
Name the following acids
Begin by finding the name of the anion (not the H) from the periodic Table or Table 6.4, then follow the naming flow chart.
- HClO =___________________________ ________________________________
- HClO4 = _________________________ ________________________________
![Page 53: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/53.jpg)
53
Name the following acids
Begin by finding the name of the anion (not the H) from the periodic Table or Table 6.4, then follow the naming flow chart.
- HClO = ClO is hypochlorite _so the name for this acid is… ______________
- HClO4 =_________________________ _______________________________
![Page 54: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/54.jpg)
54
Name the following acids
Begin by finding the name of the anion (not the H) from the periodic Table or Table 6.4, then follow the naming flow chart.
- HClO = ClO is hypochlorite _so the name for this acid is hypochlorous acid
- HClO4 = _________________________ ________________________________
![Page 55: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/55.jpg)
55
Name the following acids
Begin by finding the name of the anion (not the H) from the periodic Table or Table 6.4, then follow the naming flow chart.
- HClO = ClO is hypochlorite _so the name for this acid is hypochlorous acid
- HClO4 = ClO4 is perchlorate, so the name for this acid is…______________
![Page 56: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/56.jpg)
56
Name the following acids
Begin by finding the name of the anion (not the H) from the periodic Table or Table 6.4, then follow the naming flow chart.
- HClO = ClO is hypochlorite _so the name for this acid is hypochlorous acid
- HClO4 = ClO4 is perchlorate, so the name for this acid is perchloric acid
![Page 57: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/57.jpg)
57
Practice naming the following acids:
1. HCl = _________________________
2. HClO3 = _______________________
3. HClO2 = _______________________4. HClO = ________________________
5. HClO4 = _______________________
6. H2S = ____________________
7. H2SO3 = ___________________
8. H2SO4 = ___________________
9. HC2H3O2 = ____________________
![Page 58: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/58.jpg)
58
Practice naming the following acids:
1. HCl = ____Hydrochloric acid__________
2. HClO3 = ___________________________
3. HClO2 = ___________________________4. HClO = ____________________________
5. HClO4 = ___________________________
6. H2S = _____________________________
7. H2SO3 = ___________________________
8. H2SO4 = ___________________________
9. HC2H3O2 = _________________________
![Page 59: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/59.jpg)
59
Practice naming the following acids:
1. HCl = ____Hydrochloric acid__________
2. HClO3 = ____Chloric acid_____________
3. HClO2 = ___________________________4. HClO = ____________________________
5. HClO4 = ___________________________
6. H2S = _____________________________
7. H2SO3 = ___________________________
8. H2SO4 = ___________________________
9. HC2H3O2 = _________________________
![Page 60: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/60.jpg)
60
Practice naming the following acids:
1. HCl = ____Hydrochloric acid__________
2. HClO3 = ____Chloric acid_____________
3. HClO2 = ____Chlorous Acid ___________4. HClO = ____________________________
5. HClO4 = ____________________________
6. H2S = ______________________________
7. H2SO3 = ____________________________
8. H2SO4 = ____________________________
9. HC2H3O2 = __________________________
![Page 61: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/61.jpg)
61
Practice naming the following acids:
1. HCl = ____Hydrochloric acid__________
2. HClO3 = ____Chloric acid_____________
3. HClO2 = ____Chlorous Acid ___________4. HClO = ____Hypochlorous acid _______
5. HClO4 = ___________________________
6. H2S = _____________________________
7. H2SO3 = ___________________________
8. H2SO4 = ___________________________
9. HC2H3O2 = _________________________
![Page 62: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/62.jpg)
62
Practice naming the following acids:
1. HCl = ____Hydrochloric acid__________
2. HClO3 = __Chloric acid_____________
3. HClO2 = __Chlorous Acid __________4. HClO = ___Hypochlorous acid _______
5. HClO4 = __Perchloric acid __________
6. H2S = _____________________________
7. H2SO3 = ___________________________
8. H2SO4 = ___________________________
9. HC2H3O2 = _________________________
![Page 63: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/63.jpg)
63
Practice naming the following acids:
1. HCl = ____Hydrochloric acid__________
2. HClO3 = ____Chloric acid_____________
3. HClO2 = ____Chlorous Acid ___________4. HClO = ____Hypochlorous acid ________
5. HClO4 = ___Perchloric acid __________
6. H2S = _____Hydrosulfuric acid _________
7. H2SO3 = ____________________________
8. H2SO4 = ____________________________
9. HC2H3O2 = __________________________
![Page 64: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/64.jpg)
64
Practice naming the following acids:
1. HCl = ____Hydrochloric acid__________
2. HClO3 = ____Chloric acid_____________
3. HClO2 = ____Chlorous Acid ______________4. HClO = ____Hypochlorous acid ________
5. HClO4 = ___Perchloric acid __________
6. H2S = _____Hydrosulfuric acid _________
7. H2SO3 = ___Sulfurous acid __________
8. H2SO4 = ____Sulfuric acid_____
9. HC2H3O2 = ___Acetic acid_________
![Page 65: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/65.jpg)
65
Write the formula for the following acids:
1. Nitric acid ______________________2. Hydronitric acid _________________3. Nitrous acid ____________________4. Hydrocyanic acid ________________5. Phosphoric acid _________________6. Hydrobromic acid ________________7. Acetic acid _____________________8. Nitric acid ______________________
![Page 66: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/66.jpg)
66
Write the formula for the following acids:
1. Nitric acid _____HNO3_____________2. Hydronitric acid __________________3. Nitrous acid _____________________4. Hydrocyanic acid _________________5. Phosphoric acid __________________6. Hydrobromic acid _________________7. Acetic acid ______________________8. Nitric acid _______________________
![Page 67: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/67.jpg)
67
Write the formula for the following acids:
1. Nitric acid _____HNO3______________
2. Hydronitric acid _H3N______________3. Nitrous acid ______________________4. Hydrocyanic acid __________________5. Phosphoric acid ___________________6. Hydrobromic acid __________________7. Acetic acid _______________________8. Nitric acid ________________________
![Page 68: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/68.jpg)
68
Write the formula for the following acids:
1. Nitric acid _____HNO3_____________
2. Hydronitric acid _H3N______________
3. Nitrous acid __HNO2_______________4. Hydrocyanic acid _________________5. Phosphoric acid ___________________6. Hydrobromic acid __________________7. Acetic acid _______________________8. Nitric acid _______________________
![Page 69: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/69.jpg)
69
Write the formula for the following acids:
1. Nitric acid _____HNO3______________
2. Hydronitric acid _H3N_______________
3. Nitrous acid __HNO2_______________4. Hydrocyanic acid ___HCN___________5. Phosphoric acid ___________________6. Hydrobromic acid __________________7. Acetic acid _______________________8. Nitric acid ________________________
![Page 70: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/70.jpg)
70
Write the formula for the following acids:
1. Nitric acid _____HNO3______________
2. Hydronitric acid _H3N_______________
3. Nitrous acid __HNO2________________4. Hydrocyanic acid ___HCN___________
5. Phosphoric acid __H3PO4____________6. Hydrobromic acid __________________7. Acetic acid _______________________8. Nitric acid ________________________
![Page 71: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/71.jpg)
71
Write the formula for the following acids:
1. Nitric acid _____HNO3______________
2. Hydronitric acid _HN3_______________
3. Nitrous acid __HNO2______________
4. Hydrocyanic acid ___HCN___________
5. Phosphoric acid __H3PO4____________
6. Hydrobromic acid _HBr______________
7. Acetic acid _______________________
8. Nitric acid ________________________
![Page 72: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/72.jpg)
72
Write the formula for the following acids:
1. Nitric acid _____HNO3______________
2. Hydronitric acid _HN3_______________
3. Nitrous acid __HNO2________________4. Hydrocyanic acid ___HCN___________
5. Phosphoric acid __H3PO4____________6. Hydrobromic acid _HBr______________
7. Acetic acid __HC2H3O2____________8. Nitric acid ______________________
![Page 73: 1 Chemistry 102 Section 6.4 Ionic Compounds & Section 6.5 Molecular Compounds and Acids Unit II Note pack, pages 9-13.](https://reader031.fdocuments.in/reader031/viewer/2022032802/56649de55503460f94addb73/html5/thumbnails/73.jpg)
73
Write the formula for the following acids:
1. Nitric acid _____HNO3______________
2. Hydronitric acid _HN3_______________
3. Nitrous acid __HNO2________________
4. Hydrocyanic acid ___HCN___________
5. Phosphoric acid __H3PO4____________
6. Hydrobromic acid _HBr______________
7. Acetic acid __HC2H3O2____________
8. Nitric acid ___HNO3_______________