1. Unit 4: Nomenclature
VHS Chemistry

2. Monday, November 27
OBJECTIVE
I will identify ionic compounds and name and write formulas for binary ionic compounds.
WARM UP
Gather the papers from the front.
Then discuss the following:
What happens when ions form? What is a cation? What is an anion? Be prepared to share your answers with the class.

3. Cations & Anions

4. Metals & non-metals

6. Questions for Model One
Identify three elements that form only one cation
Identify three elements that form only one anion
Identify three elements that form more than one cation
In what region of the periodic table are these “multiple ion” elements typically located?

7. Using the model
Consider the ions of Potassium and Sulfur. Write chemical formulas for all possible ionic compound using these ions – using the SIMPLEST ratio of potassium to sulfur.
Keep in mind: the sum of the charges in an ionic compound must equal ZERO

8. Using the model
Consider the ions of iron and sulfur. Write chemical formulas for all possible ionic compounds involving these ions, using the simplest ratios of iron to sulfur.
Keep in mind: the sum of the charges in an ionic compound MUST equal zero

10. Circle the symbol for the metal in each of the compounds in Model 2
Model two questions
Circle the symbol for the metal in each of the compounds in Model 2
Which element comes first in the name AND formula for the compounds in metal two – the metal or the nonmetal?

11. Why is a ratio of 3 to 2 necessary for the zinc phosphide compound?
Using both models
In the compound zinc phosphide, what is the charge on the zinc ion? How do you know?
In the compound zinc phosphide, what is the charge on the phosphide ion? How do you know?
Why is a ratio of 3 to 2 necessary for the zinc phosphide compound?

12. Key question
Explain why you don’t need to specify the number of ions in the compound when you are naming ionic substances like those in Model 2.
For instance, why don’t I have to say “Zinc three Phosphide two”?

13. What’s up with the names?
How do we change the non- metal names to show that they have ionized?

14. Name the following ionic compounds using what you have learned so far:
Check in
Name the following ionic compounds using what you have learned so far:
Li2O
MgF2
Al2S3
K3N

15. Provide the chemical formulas for the following ionic compounds:
Tuesday, November 29th
OBJECTIVE
I will identify ionic compounds and name and write formulas for binary ionic compounds.
WARM UP
Provide the chemical formulas for the following ionic compounds:
Barium chloride
Magnesium oxide

16. Let’s make this more complicated!
When the metal in an ionic compound always forms an ion with the same charge, you don’t need to indicate the charge when you are naming the compound.
HOWEVER, some atoms have the ability to form more than one type of ion which can make things confusing.
I can’t refer to a compound of copper and oxygen as “copper oxide” because you wouldn’t know if I meant CuO or Cu2O

18. Questions for model 3
What is the most obvious difference between the names in model 3 and the names in model 2?
Using model three, and keeping in mind that the charges of the compound MUST sum to zero, use the chemical formulas to:
identify the charge on the copper cation in copper (I) oxide
Identify the charge on the copper cation in copper (II) oxide
Identify the charge on the iron cation in iron (II) chloride
Identify the charge on the iron cation in iron (III) chloride

19. Identify the charge on the copper cation in copper (I) oxide
Using model three, and keeping in mind that the charges of the compound MUST sum to zero, use the chemical formulas to:
Identify the charge on the copper cation in copper (I) oxide
Identify the charge on the copper cation in copper (II) oxide
Identify the charge on the iron cation in iron (II) chloride
Identify the charge on the iron cation in iron (III) chloride

20. So what do the roman numerals mean?
Discuss with your partner what the roman numerals mean, use an example (other than the ones we just went over) to support your claim

25. 1. Which of the following is the correct name for PbO2?
Lead oxide
Lead (I) oxide
Lead (II) oxide
Lead (IV) oxide
2. Which of the following is the correct chemical formula for iron (III) sulfide?
Fe2S
FeS3
FeS
Fe2S3
3. In a complete sentence, explain why the name “magnesium chloride” for MgCl2 does not include a Roman Numeral

26. Tuesday, November 28th - Continued
OBJECTIVE I will name and write formulas for Polyatomic Ions Pick up the Polyatomic Ions Model Sheet

30. Polyatomic ions
Polyatomic ions are a group of elements that are bonded together and who share a common charge. They act as one collective ion.

31. Questions using model 1 and your polyatomic ion list
Identify the polyatomic ion in each of these ion compounds. Write the name and formula of the ions including their charges:

32. Wednesday, November 29th Sodium Oxide Iron (II) Fluoride PbS2 Cu3N2
OBJECTIVE
I will name and write formulas for ionic compounds involving Polyatomic Ions
WARM UP
Independent Practice #1 is due tomorrow (Thursday)! Finish it up in class today when you are done, or for homework tonight.
On your white board, name or write formulas for the following compounds:
Sodium Oxide
Iron (II) Fluoride
PbS2
Cu3N2

33. Questions using model 1 and your polyatomic ion list
Identify the polyatomic ion in each of these ion compounds. Write the name and formula of the ions including their charges:
Example: in NaNO3 the polyatomic ion is NO31-
CaCO3
Mg(OH)2
NH4Cl

34. Consider the compound Iron (III) Hydroxide in model 2.
Using model 2
Consider the compound Iron (III) Hydroxide in model 2.
How many hydroxide ions are combined with an iron (III) ion?
Why?

35. Consider the compound barium nitrite
Using Model two
Consider the compound barium nitrite
What does the subscript “2” OUTSIDE the parentheses of the chemical formula tell you?
How many of each element are in the compound?
How many of each ION are in the compound?

36. Using model two
A student writes the chemical formula for the ionic compound calcium hydroxide as CaOH2
Write the chemical formula for each ion in the compound:
Calcium:
Hydroxide:
Why is the student’s answer wrong?

37. What is the rule for using parentheses in polyatomic ionic compounds?
Using Model two
What is the rule for using parentheses in polyatomic ionic compounds?

38. Rule for parentheses
Parentheses are used only around polyatomic ions used more than once in an ionic compound

40. Extra Cookie opportunity
Reward: Cookies
To earn: Memorize the first 72 elements of the periodic table, either symbols & full names. You will be given a blank periodic table and to earn your cookies you can fill in the first 72 spaces with their appropriate name or atomic symbol.
When: before or after school starting 12/6
End date: must be complete prior to 12/15

41. Check in- write chemical formulas for each of the compounds
Calcium sulfate
Copper (II) nitrate
Copper (II) nitride
Lithium phosphate
Potassium permanganate
Aluminum sulfite
Magnesium bicarbonate
Magnesium phosphide
Lithium Chloride
Per 1 ended on lithium phosphate

42. FeF3 (NH4)2SO4 MgS FeCO3 CuBr2 Na3PO4 CaCl2 Sn3(PO4)4 Formulas to name
CoCO3

43. Name the following compounds:
Check in
Name the following compounds:

44. Today’s agenda Finish Polyatomic Ions Work on Independent Practice
Group Check In Later in Class

45. Independent Practice #1 is Due
Thursday, November 30th
OBJECTIVE
I will name and write formulas for Ionic Compounds – including binary, transition, and those with Polyatomic Ions
WARM UP
Independent Practice #1 is Due
Quiz #1 is tomorrow (Friday) –there will be at least one question from a prior unit on each quiz. Continue to study content from prior units!

46. Check in- write chemical formulas for each of the compounds
Calcium sulfate
Copper (II) nitrate
Copper (II) nitride
Lithium phosphate
Potassium permanganate
Aluminum sulfite
Magnesium bicarbonate
Magnesium phosphide
Lithium Chloride
Per 1 ended on lithium phosphate

47. Name the following compounds:
Check in
Name the following compounds:

54. Lab- Ionic formula writing
Record all observations on the lab handout
If given a formula, supply the compound name
If given a compound name, supply the formula
Using your lab observations and the provided article, answer the follow up questions on the lab handout

55. Friday, December 1st
OBJECTIVE I will identify all types of ionic compounds by writing names and formulas WARM UP Have your notes out, we will be reviewing quickly before the quiz
Today: reviewed identification of ionic types, checked in on white boards, took quiz

56. QUIZ REVIEW
Prepare for Quiz You will need your notes, your periodic table, your common ion sheet (on the back of the learning targets), a white board and a white board marker for your table

57. Binary ionic compounds (non transition)
From the formula
Two different elements
The metal is from 1A, 2A, or 3A
From the name
Non metal ends in – ide
No roman numerals used

58. Transition binary ionic compounds
From the formula
Two different elements
The metal is not from 1A, 2A, or 3A
From the name
Non-metal ends in – ide
Roman numerals for the charge of the metal are used

59. MORE THAN TWO DIFFERENT ELEMENTS
Polyatomic ionic
From the formula
MORE THAN TWO DIFFERENT ELEMENTS
From the name
Usually will not end in –ide
One of the ions will be on your polyatomic ion list. (typically the anion)

60. Polyatomic ionic with a transition metal
From the formula
MORE THAN TWO ELEMENTS
The metal will not be in 1A, 2A, or 3A
From the name
Usually will not end in –ide
The anion will be on your polyatomic ion list.
The metal will have a roman numeral to show its charge

61. FeF3 (NH4)2SO4 MgS FeCO3 CuBr2 Na3PO4 CaCl2 Sn3(PO4)4 CoCO3
Review – identify these compounds as binary, transition, polyatomic ionic, or transition polyatomic ionic
CuBr2
Na3PO4
CaCl2
Sn3(PO4)4
CoCO3
FeF3
(NH4)2SO4
MgS
FeCO3

62. Magnesium bicarbonate Magnesium phosphide Lithium Chloride
Review – identify these compounds as binary, transition, polyatomic ionic, or transition polyatomic ionic
Aluminum sulfite
Magnesium bicarbonate
Magnesium phosphide
Lithium Chloride
Calcium sulfate
Copper (II) nitrate
Copper (II) nitride
Lithium phosphate
Potassium permanganate

63. Quiz!
You will need your periodic table, your common ion sheet (on the back of the learning targets), and something to write with
Collect Independent Practice #2 when you are done. Independent Practice #2 is due on your block day at the end of class.
Quiz #2 is Thursday 12/07

64. Group Practice Switch
Write a compound for another group to identify – you may write it as a formula or as the compound name

65. Consider this compound: Fe(HCO3)2
Monday, December 4
OBJECTIVE
I will name and identify covalent/molecular compounds
WARM UP
Consider this compound: Fe(HCO3)2
What type of compound is it? How can you tell?
What is the correct name for the compound?

67. Model one – molecular compounds
Fill in the table on Model One to indicate the number of atoms of each type in the molecular formula
Using your filled in table:
How many different elements are present in each compound?
Do the compounds combine metals with metals, metals with nonmetals, or nonmetals with nonmetals?

68. Model one
Find all the compounds in Model 1 that have chlorine and fluorine in them
Explain why the name “chlorine fluoride” is not sufficient to identify a specific compound

70. Model two
Fill in the numerical values in model two that correspond with the prefixes.
What suffix (ending) do all of the compound names have in common?
What prefix is NOT used in front of the name of an element and WHEN is it not used?

71. Consider the compound NO
Check in -
Consider the compound NO
Which element, nitrogen or oxygen, would require a prefix in the name? Explain why

72. Be ready to share out your rules
Collaborate with your group members to write a list of rules for recognizing and naming binary molecular compounds from their chemical formula.
Be ready to share out your rules

73. rules
Binary molecular compounds can be regonized because they contain only two elements that are both non-metals
In front of the name of the first element, write the prefix that corresponds with the subscript for that element. EXCEPT we never use mono on the first element
In front of the name of the second element, write the prefix that corresponds with the subscript for that element and then the element name.
Remove the ending from the second element and replace it with the suffix –ide
Sometimes we drop the vowel of the prefix so the vowels do not double up.

74. Check in
For each of the following compounds, indicate whether or not your naming rules apply:
FeI3
ICl5
HBrO4

79. Also, identify two similarities
Ionic and molecular
Using what you have learned about ionic and molecular compounds, identify two differences between the names or formulas for ionic compounds versus binary molecular compounds.
Also, identify two similarities

80. Check in
Use complete sentences to explain why AlCl3 is called aluminum chloride (no prefix required), but BCl3 is called boron trichloride

81. Group Practice Switch
Write a compound for another group to identify – you may write it as a formula or as the compound name

82. Tuesday, December 5th & Wednesday, December 6th
OBJECTIVE
I will name and identify covalent/molecular compounds
WARM UP
Consider this compound: CCl4
What type of compound is it? How can you tell?
What is the correct name for the compound?

83. Check in on identifying Ionic Compounds vs. Molecular Compounds
Plan for today
Review Quiz #1
Check in on identifying Ionic Compounds vs. Molecular Compounds
Practice Naming Compounds
Review Independent Practice #2
Board Switch

84. V+4 NO3-1 V+5 NO2-1 Ionic compound review
As a group, discuss and solve the following problem:
Given the following ions, how many different ionic compounds are possible? List them with their names and formulas.
V+4
NO3-1
V+5
NO2-1

85. Practice Problem
Explain why it is possible to write more than one correct chemical formula for a compound between iron and oxygen. In your answer be sure to discuss why it is possible, write the correct names and formulas of two possible compounds formed between these two elements.

88. Ionic or molecular?
CaCO3
AgCl
SO3
SF3
5. CuSO4
6. NO2
7. NaCl
8. P2O4

89. Ionic vs. molecular
Ionic = positive ion + negative ion (metal and a non-metal) Molecular/Covalent = non-metal + non-metal

90. Write an example of a NAME and FORMULA for a binary ionic compound on one white board.
Write and example of a NAME and FORMULA for a molecular compound on another white board.

91. On your other board write the compound type & the name
Board switch
On one whiteboard write any compound formula (either ionic or molecular)
On your other board write the compound type & the name
Pass the whiteboard with the formula to another table

92. Sodium Hydroxide Iron (II) Sulfide Disulfur Pentaoxide
Name to formula
Sodium Hydroxide
Iron (II) Sulfide
Disulfur Pentaoxide
Ammonium Chlorate

93. Formula to name
Ba(OH)2
PbO2
S2F3
NaOH

94. Iron (III) Selenide
Pb(SO4)2
P3Cl6
Sn3(PO4)4

95. Manganese (IV) Oxide

96. Wednesday, December 7th
OBJECTIVE I will name and identify covalent/molecular compounds & name and identify ionic compounds. I will be able to tell the difference between molecular and ionic compounds by name and formula WARM UP Consider the following compound: N2O4 What type of compound is it? How do you know? What is the correct compound formula name? Remember: Independent Practice #2 is due at end of class today. Quiz #2 is tomorrow (Thursday)

97. Use this time to complete the group review sheet.
When you are done, check your answers with the key
When you have the correct answers, you may complete your independent practice and study for tomorrow’s quiz on target B
For the last 10 minutes of class we will review the independent practice together so you are ready for the quiz

98. Molecular compounds

99. Rules for molecular compounds

100. Naming compounds flow chart

101. We will review before the quiz
Thursday- December 7th
Target: Ionic & Molecular Compounds
Warm-up:
Clear your table and get ready for the quiz! You need a periodic table, a calculator, and something to write with.
We will review before the quiz
Remember:
you need to be able to tell the difference between an ionic compound and a molecular compound and what that means for how they are named!

102. Quiz # 2 – Ionic and molecular compound nomenclature
When you’re done with the quiz turn it in up front and pick up:
Independent Practice #3 – due Monday 12/11
and
Naming Acids sheet

103. Warm-up (on a white board)
Friday - December 8th
Learning Target C: I can name and write formulas for binary and polyatomic acids.
Warm-up (on a white board)
Write an example of a binary ionic formula
Write an example of a polyatomic ionic formula
Write an example of a molecular/covalent formula
Upcoming: Independent Practice #3 is due Monday, Quiz 3 is Tuesday. EXAM is Thursday!

104. Positive ion and negative ion
Ionic Compounds
Positive ion and negative ion
Add up to zero
Molecular Compounds
Binary Ionic Compounds
2 types of elements
Metal + non-metal –ide
Ex: NaCl, FeO2
Use prefixes in the name
No mono on the first element
Second element ends in –ide
Do not have to add up to zero
NO METALS.
ALL NON METALS
Transition Metals
Need parenthesis and roman numerals in the name to show the charge of the metal
Polyatomic
Do not change the end of your polyatomic.
Use parenthesis in the formula when you have more than one

105. Model 1-Naming Acids: Binary acids
Name of Acid
Cation (+)
Anion (-)
HCl
Hydrochloric acid H+
Cl1-
HBr
Hydrobromic acid
H2S
Hydrosulfuric acid
2H+
S2- HF
Hydrofluoric acid

106. Naming acids: binary acids
What prefix is used to name all binary acids?
How do you change the ending of the anion name when naming binary acids?
What word do you add to the end of the name when naming binary acids?

107. Model 2-Naminc acids: oxyacids
Name of acid
Cation
Anion
Polyatomic anion name
HClO3
Chloric Acid H+
H2SO3
Sulfurous acid
H2SO4
Sulfuric acid
Sulfate
H3PO3
Phosphorous acid
3H+
Phosphite
H3PO4
Phosphoric acid
HNO3
Nitric acid
HNO2
Nitrous acid
Nitrite
H2CO3
Carbonic acid

108. Naming oxyacids
What do all oxyacids have in common (hint: what is the anion)?
Do you add the prefix hydro to oxyacids?
What ending do you use if the polyatomic ion ends in ate?
What ending do you use if the polyatomic ions ends in ite?

109. 12. Circle the acids that would be named beginning with the prefix “–hydro”
H2SO3 HF
H2S
H2CO3
HNO3

110. 12. Mixed review Hydroiodic Acid Chlorous Acid Phosphoric acid
Acid Name
Anion
Anion name
Acid formula
Hydroiodic Acid
Chlorous Acid
Phosphoric acid
Sulfurous acid

111. Monday December 11th
OBJECTIVE I will name and write formulas for ionic, covalent, and acidic compounds. WARM UP Remember: Independent Practice #3 is due today Quiz 3 tomorrow! Unit Exam Thursday 12/14.

112. Review rules for naming acids Go over independent practice #3
Plan for today
Review Quiz #2
Review rules for naming acids
Go over independent practice #3
Prepare for quiz #3 tomorrow

113. Recap on our naming acid rules!
Binary Acids (with 2 elements)
Hydro_______ic Acid
The negative ion (anion) changes from –ide ending to –ic ending
Example HCl (H+ + Cloride) becomes hydrochloric acid
Oxyacids (Ternary / Polyatomic Acids)
NO HYDRO IN NAME EVER
The negative polyatomic ion (polyatomic anion) changes from – ate ending to –ic ending OR –ite ending to –ous ending
Example H3PO4 (3 H+’s + Phosphate ion) becomes phosphic acid (or phosphoric acid) and H3PO3 (3 H+’s + Phosphite ion) becomes phosphous acid (or phosphorous acid)

114. Review Quiz #2 (from last Thursday)
Plan for today
Review Quiz #2 (from last Thursday)
Review Independent Practice #3 (due today)
Prepare for Quiz #3 by working on Mixed Covalent & Acidic Practice (quiz tomorrow)
Check key at front table
With remaining time: work on study guide

115. Tuesday December 12th
OBJECTIVE I will name and write formulas for ionic, covalent, and acidic compounds. WARM UP Quiz 3 today! Clear your table except for your periodic table, your polyatomic ion sheet, something to write with, and maybe a calculator We will review before the quiz

116. What naming rules apply only to molecular compounds?
Wednesday, December 13
Learning Target
I will name and write formulas for ionic, covalent, and acidic compounds.
WARM UP
What naming rules apply only to molecular compounds?

117. Positive ion and negative ion
Ionic Compounds
Positive ion and negative ion
Add up to zero
Molecular Compounds
Acidic Compounds
Start with H
Binary Ionic Compounds
2 types of elements
Metal + non-metal –ide
Ex: NaCl, FeO2
Use prefixes in the name
No mono on the first element
Second element ends in –ide
Do not have to add up to zero
NO METALS.
ALL NON METALS
Binary Acids
Hydro________ ic acid
Transition Metals
Need parenthesis and roman numerals in the name to show the charge of the metal
Non-Binary Acids (Oxyacids)
Change polyatomic ending
-ite becomes –ous acid
-ate becomes –ic acid
NEVER HYDRO
Polyatomic
Do not change the end of your polyatomic.
Use parenthesis in the formula when you have more than one

118. TOMORROW (THURSDAY) IS THE unit 4 NOMENCLATURE EXAM
You will be given a periodic table with the common ions on the back
You will need a calculator
You will need something to write with
You will need to show up on time because the test is a little long and you need ALL THE TIME available
I will be in the building tomorrow, but will not be in the class – so you need to ask me your questions TODAY.

119. Trinitrogen Pentachloride HCl Pb(NO2)2 CaCl2
H2CO3
Magnesium Hydroxide
Copper (II) Phosphate
NCl3
Hydroiodic acid
Chlorous Acid
Trinitrogen Pentachloride
HCl
Pb(NO2)2
CaCl2

120. Create a flow chart 1 for naming 1 for formula writing
You should ask a series of questions that will lead you to using the correct rules for naming or formula writing for the compound
15 minutes

121. You need a calculator and something to write with
Thursday December 14th
You need a calculator and something to write with
You do not need anything else on your table
When you are finished turn your exam in to your class folder.