1. Chapter 7 Chapter 7 Table of Contents
Chemical Formulas and Chemical Compounds
Chapter 7
Chapter 7
Table of Contents
Section 1 Chemical Names and Formulas
Section 2 Oxidation Numbers
Section 3 Using Chemical Formulas
Section 4 Determining Chemical Formulas
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2. Opener #9 - Thursday, October 18, 2012
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Opener #9 - Thursday, October 18, 2012
CCl MgCl2
1. Guess the name of each of the above compounds based on the formulas written.
2. What kind of information can you discern from the formulas?
3. Guess which of the compounds represented is molecular and which is ionic.
Chemical formulas form the basis of the language of chemistry and reveal much information about the substances they represent.
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3. Chapter 7 Chapter 7 Objectives
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Objectives
Explain the significance of a chemical formula.
Determine the formula of an ionic compound formed between two given ions.
Name an ionic compound given its formula.
Using prefixes, name a binary molecular compound from its formula.
Write the formula of a binary molecular compound given its name.
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4. Reading Chemical Formulas
Visual Concepts
Chapter 7
Reading Chemical Formulas
NOT NEEDED
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Visual Concept
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5. Naming Ions
7.1
A rose is rosa in Spanish, warda in Arabic, and julab in Hindi. To truly understand another culture, you must first learn the language used in that culture. Similarly, to understand chemistry, you must learn its language. For this you need to know how to name ions.
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6. Significance of a Chemical Formula
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Significance of a Chemical Formula
A chemical formula indicates the relative number of atoms of each kind in a chemical compound.
For a molecular compound, the chemical formula reveals the number of atoms of each element contained in a single molecule of the compound.
example: octane — C8H18
The subscript after the C indicates that there are 8 carbon atoms in the molecule.
The subscript after the H indicates that there are 18 hydrogen atoms in the molecule.
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7. Chapter 7
Hydrocarbons are molecular compounds composed only of carbon and hydrogen.
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8. Significance of a Chemical Formula, continued
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Significance of a Chemical Formula, continued
An ionic compound consists of a lattice of positive and negative ions held together by mutual attraction.
The chemical formula for an ionic compound represents one formula unit—the simplest ratio of the compound’s positive ions (cations) and its negative ions (anions).
example: aluminum sulfate — Al2(SO4)3
Parentheses surround the polyatomic ion to identify it as a unit. The subscript 3 refers to the unit.
Note also that there is no subscript for sulfur: when there is no subscript next to an atom, the subscript is understood to be 1.
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9. 7.1
Naming Ions
>
Monatomic Ions
Monatomic Ions
How are the charges of Group A metal and nonmetal ions related to their positions in the periodic table?
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10. 7.1
Naming Ions
>
Monatomic Ions
Monatomic ions consist of a single atom with a positive or negative charge resulting from the loss or gain of one or more valence electrons, respectively.
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11. Chapter 7 Chapter 7 Monatomic Ions
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Monatomic Ions
Many main-group elements can lose or gain electrons to form ions.
Ions formed form a single atom are known as monatomic ions.
example: To gain a noble-gas electron configuration, nitrogen gains three electrons to form N3– ions.
Some main-group elements tend to form covalent bonds instead of forming ions.
examples: carbon and silicon
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12. Group 1 has 1+ charge (loses 1 electron)
7.1
Naming Ions
>
Monatomic Ions
Cations
When the metals in Groups 1, 2, & 13 (1A, 2A, and 3A) lose electrons, they form cations with positive charges equal to their group number. (13 also known as 3A.)
Group 1 has 1+ charge (loses 1 electron)
Group 2 has 2+ charge (loses 2 electrons)
Aluminum in Group 13 (3A) has 3+ charge (loses 3 electrons).
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13. 7.1
Naming Ions
>
Monatomic Ions
The names of the cations of the Group 1, 2, and 13 (1A, Group 2A, and Group 3A) metals are the same as the name of the metal, followed by the word ion or cation.
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14. Monatomic Ions, continued
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Monatomic Ions, continued
Naming Monatomic Ions
Monatomic cations are identified simply by the element’s name.
examples:
K+ is called the potassium cation
Mg2+ is called the magnesium cation
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15. 7.1
Naming Ions
>
Monatomic Ions
These elements have ionic charges that can be obtained from their group numbers.
The representative elements shown form positive ions with charges equal to their group numbers. Applying Concepts Are the ions anions or cations?
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16. Group 15, 16, & 17 (5A, 6A, 7A) elements form anions.
7.1
Naming Ions
>
Monatomic Ions
Group 15, 16, & 17 (5A, 6A, 7A) elements form anions.
Note the positions of the nonmetals and the metalloid, arsenic. These elements form anions. Common transition elements that form more than one ion are also shown. Applying Concepts Do the transition metals form anions or cations?
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17. Anion names start with the stem of the element name and end in -ide.
7.1
Naming Ions
>
Monatomic Ions
Anions
The charge of any ion of a nonmetal Group is determined by subtracting 8 from the valence electron number. (example Group 15 would have 5 valence electrons, so 5-8 = -3, so charge is -3 for Group Similarly charge for Group 16 is -2 and Group 17 is -1.
Anion names start with the stem of the element name and end in -ide.
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18. Monatomic Ions, continued
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Monatomic Ions, continued
Naming Monatomic Ions
For monatomic anions, the ending of the element’s name is dropped, and the ending -ide is added to the root name.
examples:
F– is called the fluoride anion
N3– is called the nitride anion
Group 14 share electrons in covalent bonds.
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19. 7.1 > Naming Ions Monatomic Ions 19 End Show Slide of 33
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20. Chapter 7 Chapter 7 Common Monatomic Ions
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Common Monatomic Ions
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21. Chapter 7 Naming Monatomic Ions
Visual Concepts
Chapter 7
Naming Monatomic Ions
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Visual Concept
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22. Ions of Transition Metals
7.1
Naming Ions
>
Monatomic Ions
Ions of Transition Metals
How are the charges of some transition metal ions determined?
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23. 7.1
Naming Ions
>
Monatomic Ions
The charges of the cations of many transition metal ions must be determined from the number of electrons lost.
The d-block (transition metals) form 2 or more cations with different charges.
Example Copper, Cu may be 1+ or 2+ depending upon if it loses 1 or 2 electrons.
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24. 7.1
Naming Ions
>
Monatomic Ions
These colorful solutions contain the transition metal ions Co3+, Cr3+, Fe3+, Ni2+, and Mn2+.
The ions of these transition metals produce an array of colors when dissolved in water. From left to right, the ions are Co3+, Cr3+, Fe3+, Ni2+, and Mn2+.
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25. 7.1
Naming Ions
>
Monatomic Ions
Many transition metal compounds are colored and can be used as pigments.
Many transition metals form brightly colored compounds that are used in making artists’ paints.
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26. Two methods are used to name the ions of transition metals.
7.1
Naming Ions
>
Monatomic Ions
Two methods are used to name the ions of transition metals.
The Stock system
The classical method
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27. 7.1
Naming Ions
>
Monatomic Ions
In the Stock system, a Roman numeral in parentheses is placed after the name of the element to indicate the numerical value of the charge.
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28. 7.1
Naming Ions
>
Monatomic Ions
In an older less, useful method, the classical name of the element is used to form the root name for the element.
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29. 7.1 > Naming Ions Monatomic Ions 29 End Show Slide of 33
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30. Chapter 7 Chapter 7 Common Monatomic Ions
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Common Monatomic Ions
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31. Conceptual Problem 9.1 Conceptual problem 1.1 1.1 End Show Slide of 33
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32. Conceptual Problem 9.1 1.1 End Show Slide of 33
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33. Conceptual Problem 9.1 1.1 End Show Slide of 33
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34. Practice Problems For Conceptual Problem 9.1
CLICK HERE FOR ACTIVITY
CLICK HERE FOR ACTIVITY
Problem-Solving 9.1 Solve Problem 1 with the help of an interactive guided tutorial.
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35. Naming and Writing Formulas for Ionic Compounds
7.1
A recipe is a formula for the sauce—a complete list of ingredients and their proportions. Chemistry also uses formulas. Once you know the rules, you can write the formula for any chemical compound.
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36. Binary Ionic Compounds
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Binary Ionic Compounds
Compounds composed of two elements are known as binary compounds.
In a binary ionic compound, the total numbers of positive charges and negative charges must be equal.
To name any binary ionic compound, place the cation name first, followed by the anion name.
The formula for a binary ionic compound can be written given the identities of the compound’s ions.
example: magnesium bromide
Ions combined: Mg2+, Br–, Br–
Chemical formula: MgBr2
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37. Binary Ionic Compounds, continued
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Binary Ionic Compounds, continued
A general rule to use when determining the formula for a binary ionic compound is “crossing over” to balance charges between ions.
example: aluminum oxide
1) Write the symbols for the ions.
Al3+ O2–
2) Cross over the charges by using the absolute value of each ion’s charge as the subscript for the other ion.
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38. Binary Ionic Compounds, continued
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Binary Ionic Compounds, continued
example: aluminum oxide, continued
3) Check the combined positive and negative charges to see if they are equal.
(2 × 3+) + (3 × 2−) = 0
The correct formula is Al2O3
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39. Writing the Formula of an Ionic Compound
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Writing the Formula of an Ionic Compound
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40. Naming Binary Ionic Compounds, continued
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Ionic Compounds, continued
Sample Problem A
Write the formulas for the binary ionic compounds formed between the following elements:
a. zinc and iodine
b. zinc and sulfur
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41. Naming Binary Ionic Compounds, continued
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Ionic Compounds, continued
Sample Problem A Solution
Write the symbols for the ions side by side. Write the cation first.
a. Zn2+ I–
b. Zn2+ S2–
Cross over the charges to give subscripts. a. b.
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42. Naming Binary Ionic Compounds, continued
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Ionic Compounds, continued
Sample Problem A Solution, continued
Check the subscripts and divide them by their largest common factor to give the smallest possible whole- number ratio of ions.
a. The subscripts give equal total charges of 1 × 2+ = 2+ and 2 × 1– = 2–.
The largest common factor of the subscripts is 1.
The smallest possible whole-number ratio of ions in the compound is 1:2.
The formula is
ZnI2.
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43. Naming Binary Ionic Compounds, continued
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Ionic Compounds, continued
Sample Problem A Solution, continued
b. The subscripts give equal total charges of 2 × 2+ = 4+ and 2 × 2− = 4−.
The largest common factor of the subscripts is 2.
The smallest whole-number ratio of ions in the compound is 1:1.
The formula is
ZnS.
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44. Naming Binary Ionic Compounds
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Ionic Compounds
The nomenclature, or naming system, or binary ionic compounds involves combining the names of the compound’s positive and negative ions.
The name of the cation is given first, followed by the name of the anion:
example: Al2O3 — aluminum oxide
For most simple ionic compounds, the ratio of the ions is not given in the compound’s name, because it is understood based on the relative charges of the compound’s ions.
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45. Naming Ionic Compounds
Visual Concepts
Chapter 7
Naming Ionic Compounds
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Visual Concept
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46. Naming Binary Ionic Compounds, continued
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Ionic Compounds, continued
The Stock System of Nomenclature
Some elements such as iron, form two or more cations with different charges.
To distinguish the ions formed by such elements, scientists use the Stock system of nomenclature.
The system uses a Roman numeral to indicate an ion’s charge.
examples: Fe2+ iron(II)
Fe3+ iron(III)
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47. Naming Compounds Using the Stock System
Visual Concepts
Chapter 7
Naming Compounds Using the Stock System
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Visual Concept
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48. Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Ionic Compounds, continued The Stock System of Nomenclature, continued
Sample Problem B
Write the formula and give the name for the compound formed by the ions Cr3+ and F–.
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49. Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Ionic Compounds, continued The Stock System of Nomenclature, continued
Sample Problem B Solution
Write the symbols for the ions side by side. Write the cation first.
Cr3+ F–
Cross over the charges to give subscripts.
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50. Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Ionic Compounds, continued The Stock System of Nomenclature, continued
Sample Problem B Solution, continued
The subscripts give charges of 1 × 3+ = 3+ and 3 × 1− = 3−.
The largest common factor of the subscripts is 1, so the smallest whole number ratio of the ions is 1:3.
The formula is
CrF3.
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51. chromium(III) fluoride.
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Ionic Compounds, continued The Stock System of Nomenclature, continued
Sample Problem B Solution, continued
Chromium forms more than one ion, so the name of the 3+ chromium ion must be followed by a Roman numeral indicating its charge.
The compound’s name is
chromium(III) fluoride.
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52. CLICK HERE FOR ACTIVITY
Naming and Writing Formulas
for Ionic Compounds
>
Simulation 9.11
CLICK HERE FOR ACTIVITY
ACTIVITY INCLUDES THE FOLLOWING:
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53. Practice Problems pg. 223 Chapter 7
Complete the above problems before going to next page. Ask questions if you do not understand or miss the problems!!!
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54. ANSWERS to pg. 223 Chapter 7 Ask me if you do not understand.
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55. Practice Problems pg. 225 Chapter 7
Complete all problems above before going to the next page. ASK QUESTIONS if you do not understand!
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56. ANSWERS pg. 225 Chapter 7 Chapter menu Resources
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57. 7.1
Naming Ions
>
Polyatomic Ions
Polyatomic Ions
What are the two endings of the names of most polyatomic ions?
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58. Some ions, called polyatomic ions, are composed of more than one atom.
7.1
Naming Ions
>
Polyatomic Ions
Some ions, called polyatomic ions, are composed of more than one atom.
The names of most polyatomic anions end in -ite or -ate.
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59. Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Ionic Compounds, continued Compounds Containing Polyatomic Ions
Many common polyatomic ions are oxyanions—polyatomic ions that contain oxygen.
Some elements can combine with oxygen to form more than one type of oxyanion.
example: nitrogen can form or
The name of the ion with the greater number of oxygen atoms ends in -ate. The name of the ion with the smaller number of oxygen atoms ends in -ite.
nitrate nitrite
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60. Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Ionic Compounds, continued Compounds Containing Polyatomic Ions, continued
Some elements can form more than two types of oxyanions.
example: chlorine can form , , or
In this case, an anion that has one fewer oxygen atom than the -ite anion has is given the prefix hypo-.
An anion that has one more oxygen atom than the -ate anion has is given the prefix per-.
hypochlorite chlorite chlorate perchlorate
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61. These models show the structures of four common polyatomic ions.
7.1
Naming Ions
>
Polyatomic Ions
These models show the structures of four common polyatomic ions.
These molecular models show the arrangement of atoms in four common polyatomic ions. Interpreting Diagrams How does the ammonium ion differ from the other three?
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62. Sodium hydrogen carbonate can relieve an upset stomach.
7.1
Naming Ions
>
Polyatomic Ions
Sodium hydrogen carbonate can relieve an upset stomach.
Hydrogen-containing polyatomic ions are part of many compounds that affect your daily life. a) Sodium hydrogen carbonate, which contains the HCO3- ion, can relieve an upset stomach. b) The presence of dissolved HCO3-, HPO42-, and H2PO4- ions in your blood is critical for your health. c) Crop dusters spread fertilizers containing HPO42- and H2PO4- ions.
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63. 7.1
Naming Ions
>
Polyatomic Ions
HCO3–, HPO42–, and H2PO4– ions in your blood are critical for your health.
Hydrogen-containing polyatomic ions are part of many compounds that affect your daily life. a) Sodium hydrogen carbonate, which contains the HCO3- ion, can relieve an upset stomach. b) The presence of dissolved HCO3-, HPO42-, and H2PO4- ions in your blood is critical for your health. c) Crop dusters spread fertilizers containing HPO42- and H2PO4- ions.
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64. Fertilizers contain HPO42– and H2PO4– ions.
7.1
Naming Ions
>
Polyatomic Ions
Fertilizers contain HPO42– and H2PO4– ions.
Hydrogen-containing polyatomic ions are part of many compounds that affect your daily life. a) Sodium hydrogen carbonate, which contains the HCO3- ion, can relieve an upset stomach. b) The presence of dissolved HCO3-, HPO42-, and H2PO4- ions in your blood is critical for your health. c) Crop dusters spread fertilizers containing HPO42- and H2PO4- ions.
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65. Names and Formulas of Some Common Polyatomic Ions
7.1
Naming Ions
>
Polyatomic Ions
Names and Formulas of Some Common Polyatomic Ions
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66. Chapter 7 Chapter 7 Polyatomic Ions
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Polyatomic Ions
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67. Naming Compounds with Polyatomic Ions
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Compounds with Polyatomic Ions
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68. Compounds With Polyatomic Ions
7.1
Naming and Writing Formulas
for Ionic Compounds
>
Compounds With Polyatomic Ions
Naming Compounds with Polyatomic Ions
To name a compound containing a polyatomic ion, state the cation first and then the anion, just as you did in naming binary ionic compounds.
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69. Compounds With Polyatomic Ions
7.1
Naming and Writing Formulas
for Ionic Compounds
>
Compounds With Polyatomic Ions
Sodium hypochlorite (NaClO) is used as a disinfectant for swimming pools. The metallic cation in this compound is sodium (Na+) so the polyatomic ion must be ClO–.
Sodium hypochlorite (NaClO) is often added to the water in swimming pools to prevent bacteria from exceeding safe levels.
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70. CLICK HERE FOR ACTIVITY ACTIVITY INCLUDES THE FOLLOWING:
Naming and Writing Formulas
for Ionic Compounds
>
Simulation 9
CLICK HERE FOR ACTIVITY
ACTIVITY INCLUDES THE FOLLOWING:
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71. Understanding Formulas for Polyatomic Ionic Compounds
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Understanding Formulas for Polyatomic Ionic Compounds
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72. Naming Compounds Containing Polyatomic Ions
Visual Concepts
Chapter 7
Naming Compounds Containing Polyatomic Ions
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Visual Concept
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73. Compounds With Polyatomic Ions
7.1
Naming and Writing Formulas
for Ionic Compounds
>
Compounds With Polyatomic Ions
Compounds with Polyatomic Ions
How do you write the formulas and names of compounds containing polyatomic ions?
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74. Compounds With Polyatomic Ions
7.1
Naming and Writing Formulas
for Ionic Compounds
>
Compounds With Polyatomic Ions
Write the symbol for the cation followed by the formula for the polyatomic ion and balance the charges.
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75. Compounds With Polyatomic Ions
7.1
Naming and Writing Formulas
for Ionic Compounds
>
Compounds With Polyatomic Ions
For example, calcium nitrate is composed of a calcium cation (Ca2+) and a polyatomic nitrate anion (NO3–).
In calcium nitrate, two nitrate anions, each with a 1– charge, are needed to balance the 2+ charge of each calcium cation. The formula for calcium nitrate is Ca(NO3)2.
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76. Practice Problems For Conceptual Problem 9.3
CLICK HERE FOR ACTIVITY
Problem-Solving 9.12 Solve Problem 12 with the help of an interactive guided tutorial.
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77. CLICK BELOW TO SEE SIMULATION ACTIVITY.
Naming and Writing Formulas
for Ionic Compounds
>
Simulation 9
Simulation 9 Simulate combining ions and deriving the chemical formulas for several ionic compounds.
CLICK BELOW TO SEE SIMULATION ACTIVITY.
ACTIVITY - CLICK HERE
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78. Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Ionic Compounds, continued Compounds Containing Polyatomic Ions, continued
Sample Problem C
Write the formula for tin(IV) sulfate.
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79. Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Ionic Compounds, continued Compounds Containing Polyatomic Ions, continued
Sample Problem C Solution
Write the symbols for the ions side by side. Write the cation first.
Cross over the charges to give subscripts. Add parentheses around the polyatomic ion if necessary.
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80. Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Ionic Compounds, continued Compounds Containing Polyatomic Ions, continued
Sample Problem C Solution, continued
The total positive charge is 2 × 4+ = 8+.
The total negative charge is 4 × 2− = 8−.
The largest common factor of the subscripts is 2, so the smallest whole-number ratio of ions in the compound is 1:2.
The correct formula is therefore
Sn(SO4)2.
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81. Conceptual Problem 9.2 TRY THESE WITHOUT WRITING DOWN Note if ratio
can be
simplified to
lower terms,
it will be reduced.
Example - a ratio
of 2:2 will reduce to
1:1.
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82. Sample Problems For Conceptual Problem 9.2
Practice Problems
for Conceptual Problem 9.2
Sample Problems For Conceptual Problem 9.2
SEE IF YOU CAN GET THESE CORRECT BEFORE DOING THE ADDITIONAL PRACTICE PROBLEMS - NOTE THE CLICK BELOW.
CLICK HERE FOR ACTIVITY
Problem Solving 9.11 Solve Problem 11 with the help of an interactive guided tutorial.
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83. Practice Problems pg. 227 Chapter 7
Complete all of these before going to next slide!
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84. ANSWERS pg. 227 Chapter 7 Chapter menu Resources
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85. Naming Binary Molecular Compounds
7.1
Naming and Writing Formulas for Molecular Compounds
Naming Binary Molecular Compounds
>
Naming Binary Molecular Compounds
What does a prefix in the name of a binary molecular compound tell you about the compound’s composition?
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86. Naming Binary Molecular Compounds
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Molecular Compounds
Unlike ionic compounds, molecular compounds are composed of individual covalently bonded units, or molecules.
As with ionic compounds, there is also a Stock system for naming molecular compounds.
The old system of naming molecular compounds is based on the use of prefixes.
examples: CCl4 — carbon tetrachloride (tetra- = 4) CO — carbon monoxide (mon- = 1) CO2 — carbon dioxide (di- = 2)
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87. Naming Binary Molecular Compounds
7.1
Naming and Writing Formulas for Molecular Compounds
Naming Binary Molecular Compounds
>
A prefix in the name of a binary molecular compound tells how many atoms of an element are present in each molecule of the compound.
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88. Prefixes for Naming Covalent Compounds
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Prefixes for Naming Covalent Compounds
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89. Naming Covalently-Bonded Compounds
Visual Concepts
Chapter 7
Naming Covalently-Bonded Compounds
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Visual Concept
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90. Naming Compounds Using Numerical Prefixes
Visual Concepts
Chapter 7
Naming Compounds Using Numerical Prefixes
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91. Prefix Method for COVALENT
Chapter 7
Prefix method:
The element that has the smaller group number is usually given first. If both are in same group, then the element whose period number is greater goes first. The element is given a prefix only if greater than one. Do not use mono- on the first element.
The 2nd element is named by combining a prefix and the root name of the element
ending in –ide.
The o or a at the end of a prefix is usually dropped when the word following the prefix begins with another vowel.
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92. Naming Binary Molecular Compounds, continued
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Molecular Compounds, continued
Sample Problem D
a. Give the name for As2O5.
b. Write the formula for oxygen difluoride.
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93. Naming Binary Molecular Compounds, continued
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Molecular Compounds, continued
Sample Problem D Solution
a. A molecule of the compound contains two arsenic atoms, so the first word in the name is diarsenic.
The five oxygen atoms are indicated by adding the prefix pent- to the word oxide.
The complete name is
diarsenic pentoxide.
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94. Naming Binary Molecular Compounds, continued
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Naming Binary Molecular Compounds, continued
Sample Problem D Solution, continued
b. Oxygen is first in the name because it is less electronegative than fluorine.
Because there is no prefix, there must be only one oxygen atom.
The prefix di- in difluoride shows that there are two fluorine atoms in the molecule.
The formula is
OF2.
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95. ›
Chapter 7
DO NOT GO TO THE NEXT PAGE UNTIL YOU ARE DONE WITH THE PROBLEMS. ASK FOR HELP IF NEEDED.
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96. ANSWERS pg. 229 Chapter 7 ANSWERS pg. 229 Chapter menu Resources
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97. Covalent-Network Compounds
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Covalent-Network Compounds
Some covalent compounds do not consist of individual molecules.
Instead, each atom is joined to all its neighbors in a covalently bonded, three-dimensional network.
Subscripts in a formula for covalent-network compound indicate smallest whole-number ratios of the atoms in the compound.
examples: SiC, silicon carbide SiO2, silicon dioxide Si3N4, trisilicon tetranitride.
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98. Chapter 7
7.1 QUESTION - use points later as needed to incorporate into other ppt
not using the next slides right now - may incorporate some of them at later date for 7.1
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99. Assess students’ understanding of the concepts in Section 7.1.
7.1 Section Quiz.
Assess students’ understanding of the concepts in Section 7.1.
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100. 1. Which of the following compounds is named INCORRECTLY?
7.1 Section Quiz.
1. Which of the following compounds is named INCORRECTLY?
CS2, carbon disulfide
BCl3, boron trichloride
IF7, iodine heptafluoride
PCl5, phosphorus hexachloride
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101. 2. Which of the following molecular compounds is named INCORRECTLY?
7.1 Section Quiz.
2. Which of the following molecular compounds is named INCORRECTLY?
SbCl3, antimony trichloride
C2O5, dicarbon pentoxide
CF4, carbon tetrafluoride
H3As, hydrogen arsenide
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102. 3. The correct formula for tetraphosphorus trisulfide is P3S4 S3P4
7.1 Section Quiz.
3. The correct formula for tetraphosphorus trisulfide is
P3S4
S3P4
P4S3
S4P3
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103. 4. Which of the following are positively charged polyatomic ions?
7.1 Section Quiz
4. Which of the following are positively charged polyatomic ions?
(I) ammonium ion
(II) perchlorate ion
(III) ferric ion
I only
II only
III only
I and III
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104. 5. If the name of an ion ends in -ite or -ate, the ion is a
7.1 Section Quiz
5. If the name of an ion ends in -ite or -ate, the ion is a
polyatomic cation.
polyatomic anion.
transition metal cation.
monatomic anion.
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105. 6. The correct name for CrCl3 is chromium chlorine.
7.1 Section Quiz
6. The correct name for CrCl3 is
chromium chlorine.
chromium(III) chloride.
monochromium trichloride.
chromium(III) trichloride.
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106. 7. What is the correct formula for strontium nitride? Sr3N2 SrN2 Sr2N3
7.1 Section Quiz
7. What is the correct formula for strontium nitride?
Sr3N2
SrN2
Sr2N3
Sr3N
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107. 8. Which one of the following compounds is named correctly?
7.1 Section Quiz
8. Which one of the following compounds is named correctly?
sodium chlorite, NaClO
potassium nitrate, KNO2
sodium acetate, NaC2H3O2
lithium sulfate, Li2SO3
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108. Naming and Writing Formulas for Acids and Bases
7.1
Some ants can give painful stings when threatened or disturbed. Certain ant species called formicines have poison glands that produce venom containing formic acid. You will learn the names and formulas of some important acids such as formic acid.
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109. 7.1
Naming and Writing Formulas for Acids and Bases
>
Naming Acids
An acid is a compound that contains one or more hydrogen atoms and produces hydrogen ions (H+) when dissolved in water. Acids have various uses.
To create designs such as this on glass, the glass is first coated with wax and the design is drawn through the wax. When the glass is dipped into hydrofluoric acid (HF), the acid etches (eats away) the glass wherever the wax has been removed.
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110. Chapter 7 Chapter 7 Acids and Salts
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Acids and Salts
Most acids used in the laboratory are either binary acids or oxyacids.
Binary acids are acids that consist of two elements, usually hydrogen and a halogen.
Oxyacids are acids that contain hydrogen, oxygen, and a third element (usually a nonmetal).
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111. Naming Acids What are the three rules for naming acids? 7.1 >
Naming and Writing Formulas for Acids and Bases
>
Naming Acids
Naming Acids
What are the three rules for naming acids?
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112. Three rules can help you name an acid with the general formula HnX.
7.1
Naming and Writing Formulas for Acids and Bases
>
Naming Acids
Three rules can help you name an acid with the general formula HnX.
When the name of the anion (X) ends in - ide, the acid name begins with the prefix hydro-. The stem of the anion has the suffix -ic and is followed by the word acid.
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113. 7.1
Naming and Writing Formulas for Acids and Bases
>
Naming Acids
When the anion name ends in -ite, the acid name is the stem of the anion with the suffix -ous, followed by the word acid.
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114. 7.1
Naming and Writing Formulas for Acids and Bases
>
Naming Acids
When the anion name ends in -ate, the acid name is the stem of the anion with the suffix -ic followed by the word acid.
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115. A Summary of the Three Rules for Naming Acids.
7.1
Naming and Writing Formulas for Acids and Bases
>
Naming Acids
A Summary of the Three Rules for Naming Acids.
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116. Prefixes and Suffixes for Oxyanions and Related Acids
Visual Concepts
Chapter 7
Prefixes and Suffixes for Oxyanions and Related Acids
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Visual Concept
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117. Naming and Writing Formulas for Molecular Compounds
9.3
One milligram of gold is worth only about one cent, but one kilogram of gold is worth approximately $12,500. The correct prefix ( milli- or kilo-) makes quite a difference! Prefixes are important in chemistry, too. The prefixes in the name of a binary molecular compound tell you its composition.
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118. Naming Binary Molecular Compounds
9.3
Naming and Writing Formulas for Molecular Compounds
Naming Binary Molecular Compounds
>
Carbon and oxygen combine to form carbon monoxide (CO) and carbon dioxide (CO2), but these two invisible gases are very different.
Carbon monoxide is an invisible, gaseous compound of carbon and oxygen. It is a toxic product of incomplete burning, such as occurs in automobile engines and faulty furnaces.
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119. Naming Binary Molecular Compounds
9.3
Naming and Writing Formulas for Molecular Compounds
Naming Binary Molecular Compounds
>
Sitting in a room with small amounts of CO2 in the air would not present any problems. If the same amount of CO were in the room, you could die of asphyxiation. A naming system that distinguishes between these two compounds is needed.
Carbon monoxide is an invisible, gaseous compound of carbon and oxygen. It is a toxic product of incomplete burning, such as occurs in automobile engines and faulty furnaces.
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120. Naming Binary Molecular Compounds
9.3
Naming and Writing Formulas for Molecular Compounds
Naming Binary Molecular Compounds
>
A prefix in the name of a binary molecular compound tells how many atoms of an element are present in each molecule of the compound.
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121. Naming Binary Molecular Compounds
9.3
Naming and Writing Formulas for Molecular Compounds
Naming Binary Molecular Compounds
>
Some guidelines for naming binary molecular compounds:
Name the elements in the order listed in the formula.
Use prefixes to indicate the number of each kind of atom.
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122. Naming Binary Molecular Compounds
9.3
Naming and Writing Formulas for Molecular Compounds
Naming Binary Molecular Compounds
>
Omit the prefix mono- when the formula contains only one atom of the first element in the name.
The suffix of the name of the second element is -ide.
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123. Writing Formulas for Binary Molecular Compounds
9.3
Naming and Writing Formulas for Molecular Compounds
Writing Formulas for Binary Molecular Compounds
>
Writing Formulas for Binary Molecular Compounds
How do you write the formula for a binary molecular compound?
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124. Writing Formulas for Binary Molecular Compounds
9.3
Naming and Writing Formulas for Molecular Compounds
Writing Formulas for Binary Molecular Compounds
>
Use the prefixes in the name to tell you the subscript of each element in the formula. Then write the correct symbols for the two elements with the appropriate subscripts.
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125. Writing Formulas for Binary Molecular Compounds
9.3
Naming and Writing Formulas for Molecular Compounds
Writing Formulas for Binary Molecular Compounds
>
Silicon carbide is a hard material like diamond. The name silicon carbide has no prefixes, so the subscripts of silicon and carbon must be one. Thus, the formula for silicon carbide is SiC.
A grinding wheel made of silicon carbide (SiC) can shape even the toughest materials. Inferring What causes the sparks?
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126. 9.1 Section Quiz.
Assess students’ understanding of the concepts in Section
9.1.
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127. 9.1 Section Quiz.
1. When metals from groups 1A, 2A, and 3A form cations, the charge on the ion is equal to
8 minus the group number.
the group number minus 8.
the period number.
the group number.
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128. Assess students’ understanding of the concepts in Section 9.2.
9.2 section Quiz.
Assess students’ understanding of the concepts in Section 9.2.
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129. Acids and Salts, continued
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Acids and Salts, continued
In the laboratory, the term acid usually refers to a solution in water of an acid compound rather than the acid itself.
example: hydrochloric acid refers to a water solution of the molecular compound hydrogen chloride, HCl
Many polyatomic ions are produced by the loss of hydrogen ions from oxyacids.
examples:
sulfuric acid H2SO4 sulfate
nitric acid HNO3 nitrate
phosphoric acid H3PO4 phosphate
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130. Chapter 7 Naming Binary Acids
Visual Concepts
Chapter 7
Naming Binary Acids
Click below to watch the Visual Concept.
Visual Concept
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131. Chapter 7 Naming Oxyacids
Visual Concepts
Chapter 7
Naming Oxyacids
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132. OTHER EXAMPLES - add roots
Chapter 7
OTHER EXAMPLES - add roots
H2SO3 - sulfurous acid (coming from sulfite)
HClO3 - chloric acid
HClO2 - chlorous acid
HClO - hypochlorous acid
H2S hydrosulfuric acid
HClO4 - perchloric acid
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133. Writing Formulas for Acids
7.1
Naming and Writing Formulas for Acids and Bases
>
Writing Formulas for Acids
Writing Formulas for Acids
How are the formulas of acids determined?
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134. Writing Formulas for Acids
7.1
Naming and Writing Formulas for Acids and Bases
>
Writing Formulas for Acids
Use the rules for writing the names of acids in reverse to write the formulas for acids.
What is the formula for hydrobromic acid? Following Rule 1, hydrobromic acid (hydro- prefix and -ic suffix) must be a combination of hydrogen ion (H+) and bromide ion (Br–). The formula of hydrobromic acid is HBr.
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135. Writing Formulas for Acids
7.1
Naming and Writing Formulas for Acids and Bases
>
Writing Formulas for Acids
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136. Acids and Salts, continued
Section 1 Chemical Names and Formulas
Chapter 7
Chapter 7
Acids and Salts, continued
An ionic compound composed of a cation and the anion from an acid is often referred to as a salt.
examples:
Table salt, NaCl, contains the anion from hydrochloric acid, HCl.
Calcium sulfate, CaSO4, is a salt containing the anion from sulfuric acid, H2SO4.
The bicarbonate ion, , comes from carbonic acid, H2CO3.
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137. Visual Concepts
Chapter 7
Salt
Click below to watch the Visual Concept.
Visual Concept
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138. Section Review pg. 231 Chapter 7
Answer questions #2, 3, and 4 in your notes before going to next page..
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139. Chapter 7
Answers pg. 231
Be sure you answered these on your own first.
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140. Names and Formulas for Bases
7.1
Naming and Writing Formulas for Acids and Bases
>
Names and Formulas for Bases
Names and Formulas for Bases
How are bases named?
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141. Names and Formulas for Bases
7.1
Naming and Writing Formulas for Acids and Bases
>
Names and Formulas for Bases
Bases are named in the same way as other ionic compounds—the name of the cation is followed by the name of the anion.
For example, aluminum hydroxide consists of the aluminum cation (Al3+) and the hydroxide anion (OH–). The formula for aluminum hydroxide is Al(OH)3.
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142. Test yourself on the concepts in Section 7.1.
Section Assessment
Test yourself on the concepts in Section 7.1.
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143. 7.1 Section Quiz 1. The name for H2S(aq) is sulfuric acid.
hydrosulfuric acid.
sulfurous acid.
hydrosulfurous acid.
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144. 2. The chemical formula for chlorous acid is HClO2. HClO3. HClO4. HCl.
7.1 Section Quiz
2. The chemical formula for chlorous acid is
HClO2.
HClO3.
HClO4.
HCl.
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145. 3. The correct chemical name for NH4OH is
7.1 Section Quiz
3. The correct chemical name for NH4OH is
nitrogen tetrahydrogen hydroxide.
nitrogen pentahydrogen oxide.
ammonium oxyhydride.
ammonium hydroxide.
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146. Online Self-Check Quiz
Complete the online Quiz and record answers. Ask if you have any questions about your answers.
click here for online Quiz 7.1
(10 questions)
You must be in the “Play mode” for the slideshow for hyperlink to work.
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147. VIDEOS FOR ADDITIONAL INSTRUCTION
Additional Videos for Section 7.1: Chemical Names and Formulas
Elements and Compounds
Acid and Base Properties
Salts
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148. End of 7.1 Notes and Practice Problems
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