Name ____________________ Period ____ CRHS Academic Chemistry Unit 6 - Nomenclature Notes & Practice Problems Date Assignment On-Time Late ____ 6.1 _____ _____ ____ 6.2 _____ _____ ____ 6.3 _____ _____ ____ 6.4 _____ _____ ____ Warm Up _____ ____ Total (500) _____ Key Dates Quiz Date Exam Date Lab Dates Notes, Homework, Exam Reviews and Their KEYS located on CRHS Academic Chemistry Website: https://cincochem.pbworks.com
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Name ____________________ Period ____
CRHS Academic Chemistry
Unit 6 - Nomenclature
Notes & Practice Problems
Date Assignment On-Time Late
____ 6.1 _____ _____
____ 6.2 _____ _____
____ 6.3 _____ _____
____ 6.4 _____ _____
____ Warm Up _____
____ Total (500) _____
Key Dates Quiz Date Exam Date
Lab Dates
Notes, Homework, Exam Reviews and Their KEYS located on CRHS Academic Chemistry Website: https://cincochem.pbworks.com
6.1 NAMING AND WRITING FORMULAS OF IONIC COMPOUNDS - GROUP 1-3 METALS
1. Chemical nomenclature is a set of ____________________ used to generate systematic _______________
for chemical compounds.
2. Fill in the missing information in each of the cells of the table.
Element Group Number? Metal or
Nonmetal?
Group Name? Oxidation
Number?
Gain or Lose
Electrons?
How Many
Electrons Gained
or Lost?
Rb 1 Metal Alkali Metal +1 Lose 1
Al
O
I
Sr
Be
S
N
Br
F
Ne
Xe
Ra
P
Ar
Na
Ca
Ba
Unit 6 Notes Page 5 of 24
Name the Ionic compound
1. SrCl2
2. MgI2
3. Li2O
4. CaBr2
5. MgS
6. Al2O3
7. BCl3
8. CaO
9. Al2S3
Fill in the table
Chemical Name Elements Charge of Ions Formula
Barium nitride Ba & N Ba+2 N–3 Ba3N2
Magnesium sulfide
Aluminum oxide
Sodium iodide
Lithium sulfide
Radium chloride
Calcium oxide
Potassium nitride
Page 6 of 24 Unit 6 Notes
HW 6.2 NAMING AND WRITING FORMULAS OF IONIC COMPOUNDS - POLYATOMIC IONS Indicate the type of compound then name the compound! Ionic (I) or Polyatomic Ion(IP) or Ionic Transition Metal Polyatomic (IPT)
1. Na2SO4
2. Ca3(PO4)2
3. KMnO4
4. K2S
5. NaI
6. Rb2N3
7. K2CO3
8. Cs2SO4
9. Ba(NO3)2
10. LiC2H3O2
11. Ca3P2
12. Li2CrO4
13. KCN
Unit 6 Notes Page 7 of 24
Indicate the type of compound then write the formula! Ionic (I) or Polyatomic Ion(IP) or Ionic Transition Metal Polyatomic (IPT)
1. potassium permanganate
2. calcium hydroxide
3. sodium fluoride
4. sodium perchlorate
5. ammonium hydroxide
6. calcium carbonate
7. lithium nitride
8. calcium chlorate
9. barium sulfide
10. ammonium sulfate
11. sodium sulfite
12. ammonium chromate
13. potassium chromate
Page 8 of 24 Unit 6 Notes
HW 6.3 NAMING AND WRITING FORMULAS OF IONIC COMPOUNDS – TRANSITION METALS Indicate the type of compound then name the compound! Ionic (I) or Polyatomic Ion(IP) or Ionic Transition Metal Polyatomic (IPT)
1. NiF2
2. Cu2O
3. FeI2
4. CuBr2
5. FeSO4
6. SnS2
7. Na2S
8. CrSe
9. MgBr2
10. MnO
11. Mn2Se3
12. Na2SO3
13. AuI
14. PbO
15. KC2H3O2
16. CoCl3
Unit 6 Notes Page 9 of 24
17. Fill in the table
Indicate the type of compound then write the formula! Ionic (I) or Polyatomic Ion(IP) or Ionic Transition Metal Polyatomic (IPT)
18. copper (II) fluoride
19. sulfurous acid
20. dinitrogen pentoxide
21. barium chloride
22. hydronitric acid
23. lithium perchlorate
24. phosphorus trihydride
25. chromium (III) oxide
26. sodium peroxide
Compound Name Ions Formed Formula
iron (III) chloride Fe+3 & Cl–1 FeCl3
tin (IV) fluoride
chromium (III) oxide
manganese (II) sulfide
copper (II) nitride
lead (II) oxide
lead (IV) oxide
titanium (III) chloride
tin (II) sulfide
iron (III) selenide
Page 10 of 24 Unit 6 Notes
HW 6.4 NAMING AND WRITING FORMULAS OF COVALENT COMPOUNDS Fill in the table of numerical prefixes
=1 =2 =3 =4 =5
=6 =7 =8 =9 =10
Name the following covalent compounds using the appropriate prefixes.
1. SO2
2. S3F7
3. N2O5
4. SiCl4
5. AsH3
6. H2O
7. SO3
Write the formula of the given covalent compound.
8. nitrogen triiodide
9. silicon tetrafluoride
10. arsenic pentafluoride
11. xenon hexafluoride
12. triiodine nonafluoride
13. sulfur trioxide
14. diiodine pentoxide
15. dinitrogen tetroxide
Unit 6 Notes Page 11 of 24
Indicate the type of compound then write the name Ionic (I) or Polyatomic Ion(IP) or Ionic Transition Metal Polyatomic (IPT) or Covalent (C)
1. Li2O
2. N2O5
3. HBr
4. Co2SO3
5. Ba(NO2)2
6. HClO4
7. H2C2O7
8. NiO2
Indicate the type of compound then write the formula Ionic (I) or Polyatomic Ion(P) or Ionic Transition Metal Polyatomic (IPT) or Covalent (C)
9. trinitrogen pentasulfide
10. hydrochloric acid
11. zirconium(III)bromide
12. strontium chromate
13. cesium nitride
14. chloric acid
15. nitrous acid
Page 12 of 24 Unit 6 Notes
6.1 NAMING AND WRITING FORMULAS OF IONIC COMPOUNDS - GROUP 1-3 METAL
CATIONS There are millions of known chemical substances. Without a universal, international system, naming them reliably would
be impossible. The system used in naming substances is called chemical nomenclature.
Chemical nomenclature is a set of rules used to generate systematic names for chemical compounds.
The governing body responsible for chemical nomenclature is the International Union of Pure and Applied Chemistry
(IUPAC). There are two major divisions to the IUPAC system:
1. Organic nomenclature – contain carbon, usually bonded with hydrogen, oxygen, nitrogen, and sulfur. Organic
chemistry and naming organic compounds is a topic for a college chemistry course.
2. Inorganic nomenclature – everything else is inorganic and is divided into three categories…
Covalent (a.k.a. molecular) compounds
Ionic compounds
Acids
This unit covers inorganic nomenclature for covalent compounds and ionic compounds. Nomenclature of acids
will be done in the acid and base unit.
Review Practice: Fill in the missing information
Group Number Group Name Oxidation Number Gain or Lose
Mixed Practice: indicate I, or IP, or IT (transition metal) or IPT (polyatomic & transition metal). Write the formula.
tin (IV) iodide IT SnI4
mercury (II) sulfide IT HgS
lithium chloride I LiCl
iron (III) oxide IT Fe2O3
manganese (II) chloride IT MnCl2
chromium (VI) phosphate IPT Cr3(PO4)4
copper (III) permanganate IPT Cu(KMnO4)3
Page 20 of 24 Unit 6 Notes Extra Mixed Practice: indicate I, or IP, or IT (transition metal) or IPT (polyatomic & transition metal). Write the formula.
barium fluoride I BaF
aluminum phosphate IP Al2(PO4)3
sodium acetate IP NaOC2H3O2
lead (II) oxide IT PbO
sodium hydroxide IP NaOH
calcium bromide I Ca(OH)2
potassium dichromate IP K2Cr2O7
manganese (III) oxide IT Mn2O3
sodium nitride I Na3N
tin (II) oxide IT SnO
Unit 6 Notes Page 21 of 24
6.4 NAMING AND WRITING FORMULAS OF COVALENT COMPOUND
Binary ___covalent_________ compounds are made of TWO___nonmetals_______(Ex. P2O5) bound together. Nonmetals
are ___right____ of the zig-zag line (except _hydrogen___).
Covalent Compound Naming Rules
1) Confirm the compound is __covalent________.
2) Check the number of atoms of each element by the ___subscript___. If there is no subscript, there is one atom.
Ex. P2O5 – __2__ phosphorus, _5___oxygen
3) Name the _first_____ element using the prefix (page bottom) with the element name. (Ex. P2O5 –
diphosphorus…)
NEVER use “_mono___” on the first element.
4) Name the ___second________ element. Choose the prefix, write the root of the element, and change the
ending to “___ide_________”. (Ex. P2O5 – diphosphorus pentoxide…)
Practice:
1) SF6 sulfur hexaflouride
2) CS carbon monosulfide
3) S3N2 trisulfur dinitride
STEPS for Writing Formulas for Covalent Compounds
STEPS
1. Check the elements in the compound. Confirm they are both ____nonmetals___________________________.
2. Use the ______prefixes________________________ to determine how many _______________ of each
element are in the compound.
3. Use _____subscripts_____________________ to indicate how many atoms of each element are in the formula
4. Example: carbon dioxide has __1__ carbon(s) and __2_ oxygen(s) = C1O2 = CO2 (1 subscripts are understood)
Mono = 1 Di = 2 Tri = 3 Tetra = 4 Penta = 5
Hexa = 6 Hepta = 7 Octa = 8 Nona = 9 Deca = 10
Page 22 of 24 Unit 6 Notes 5. Example: nitrogen trifluoride NF3