Practice Writing Formulas of Type I Ionic Compounds

Similar documents
Naming Compounds Handout Key

Naming Compounds. There are three steps involved in naming ionic compounds- naming the cation, naming the anion, and naming the entire compound.

Naming Ionic Compounds

Monatomic Ions. A. Monatomic Ions In order to determine the charge of monatomic ions, you can use the periodic table as a guide:

Nomenclature Packet. 1. Name the following ionic compounds: a. Al 2 O 3 Aluminum oxide. b. Cs 2 O Cesium oxide. c. Rb 3 N Rubidium nitride

Decomposition. Composition

Nomenclature and Formulas of Ionic Compounds. Section I: Writing the Name from the Formula

Name: Block: Date: Test Review: Chapter 8 Ionic Bonding

Naming Ionic Compounds Answer Key

NAMING QUIZ 3 - Part A Name: 1. Zinc (II) Nitrate. 5. Silver (I) carbonate. 6. Aluminum acetate. 8. Iron (III) hydroxide

Nomenclature of Ionic Compounds

Polyatomic Ions Worksheet. 2. Name or write the formula for the following Type I polyatomic ionic compounds

CHAPTER 5: MOLECULES AND COMPOUNDS

Oxidation States of Nitrogen

David A. Katz Chemist, Educator, Science Communicator, and Consultant Department of Chemistry, Pima Community College

Calculating Molar Mass of a Compound

INORGANIC NOMENCLATURE ~ NAMING INORGANIC COMPOUNDS

Moles, Molecules, and Grams Worksheet Answer Key

CHEMICAL NAMES AND FORMULAS

CHAPTER Naming Ions. Chemical Names and Formulas. Naming Transition Metals. Ions of Transition Metals. Ions of Transition Metals

Solution. Practice Exercise. Concept Exercise

AP Chemistry Reaction Questions

HOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions

CHEM 1411 General Chemistry I Practice Problems, Chapters 1 3

Problem Solving. Mole Concept

Balancing Chemical Equations Worksheet

Chemistry Themed. Types of Reactions

= 11.0 g (assuming 100 washers is exact).

Chapter 4 Compounds and Their Bonds

Sample Exercise 2.1 Illustrating the Size of an Atom

47374_04_p25-32.qxd 2/9/07 7:50 AM Page Atoms and Elements

SOFIA UNIVERSITY ST. KLIMENT OHRIDSKI Faculty:...Chemistry and Pharmacy... Subject area: (code and name) C H L

Chapter 4: Nonionic Compounds and Their Nomenclature

Problem Solving. Percentage Composition

Tutorial 2 FORMULAS, PERCENTAGE COMPOSITION, AND THE MOLE

Name period Unit 3 worksheet

Molar Mass Worksheet Answer Key

SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001

Chapter 3 Chemical Compounds

Rules for Naming and Writing Compounds

Study Guide For Chapter 7

FORMULAS AND NOMENCLATURE OF IONIC AND COVALENT COMPOUNDS Adapted from McMurry/Fay, section 2.10, p and the 1411 Lab Manual, p

Monday 25 June 2012 Afternoon

Polyatomic ions can form ionic compounds just as monatomic ions.

MOLES AND MOLE CALCULATIONS

Stoichiometry Review

XIX. Chemistry, High School

FORMULA WRITING AND NOMENCLATURE OF INORGANIC COMPOUNDS 2011, 2006, 2004, 2002, 1990 by David A. Katz. All rights reserved.

Name: Class: Date: 2 4 (aq)

ICP - Mono Element ppm Standard Solutions (Plasma HIQU)

Writing and Balancing Chemical Equations

WRITING AP EQUATIONS

7) How many electrons are in the second energy level for an atom of N? A) 5 B) 6 C) 4 D) 8

CHEMICAL NOMENCLATURE

Chapter 12: Oxidation and Reduction.

PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points)

Unit 6. Chapter 10: The MOLE! Date In Class Homework. % Composition & Calculating Empirical Formulas

Elements and Compounds. Chemical Bonds compounds are made of atoms held together by chemical bonds bonds are forces of attraction between atoms

W1 WORKSHOP ON STOICHIOMETRY

Periodic Table, Valency and Formula

Names and Formulas in General Chemistry

2) How many significant figures are in the measurement, g? A) 4 B) 8 C) 6 D) 7 E) 5

Topic 4 National Chemistry Summary Notes. Formulae, Equations, Balancing Equations and The Mole

Problem Solving. Mole Concept

Tuesday 22 January 2013 Morning

Monday 25 June 2012 Afternoon

Naming and Writing Formulas for Ionic Compounds Using IUPAC Rules

SOLUBILITY PRODUCT CONSTANTS

Reactions in Aqueous Solution

Tuesday 22 January 2013 Morning

APPENDIX B: EXERCISES

b. N 2 H 4 c. aluminum oxalate d. acetic acid e. arsenic PART 2: MOLAR MASS 2. Determine the molar mass for each of the following. a. ZnI 2 b.

English already has many collective nouns for fixed, given numbers of objects. Some of the more common collective nouns are shown in Table 7.1.

Unit 9 Stoichiometry Notes (The Mole Continues)

Chapter 6 Notes Science 10 Name:

Chapter 3. Molecules, Compounds and Chemical Equations

Exercise Naming Binary Covalent Compounds:

Chapter 2 Compounds and Chemical Reactions. 6. The number of atoms in one formula unit of the substance, CO(NH 2 ) 2, is

Periodic Table Questions

Texas Commission on Environmental Quality

Start: 26e Used: 6e Step 4. Place the remaining valence electrons as lone pairs on the surrounding and central atoms.

Chemistry Reference Tables

Chemistry: Chemical Equations

WRITING CHEMICAL FORMULA

BASIC CONCEPTS of CHEMISTRY Please revise: names of element, Periodic Table (understanding the notation), acid, base and salt nomenclature

Atomic Structure. Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/ Orbit nucleus in outer shells

2. Write the electron configuration notation and the electron dot notation for each: (a) Ni atom (b) Ni 2+ ion (c) Ni 3+ ion

B) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal

Chemical Reactions. Section 9.1 Reactions and Equations pages SOLUTIONS MANUAL. Practice Problems pages

TOPIC 1. ELEMENTS, COMPOUNDS AND MIXTURES.

Unit 10A Stoichiometry Notes

4. Balanced chemical equations tell us in what molar ratios substances combine to form products, not in what mass proportions they combine.

1332 CHAPTER 18 Sample Questions

neutrons are present?

CHEMICAL NAMES AND FORMULAS

Candidate Number. Other Names

Exam 2 Chemistry 65 Summer Score:

Chapter 5. Chapter 5. Naming Ionic Compounds. Objectives. Chapter 5. Chapter 5

Principles and Modern Applications Petrucci Harwood Herring 8 th Edition. A combination of two or more different elements.

Success criteria You should be able to write the correct formula for any ionic compound

Transcription:

Practice Writing Formulas of Type I Ionic Compounds 1. Lithium and Fluorine LiF 2. Calcium and Chlorine CaCl2 3. Aluminum and Bromine AlBr3 4. Gallium and Sulfur Ga2S3 5. Cesium and Tellurium Cs2Te 6. Strontium and Oxygen SrO 7. Indium and Iodine InI3 8. Potassium and Bromine KBr 9. Magnesium and Selenium MgSe 10. Aluminum and Sulfur Al2S3 11. Beryllium and Fluorine BeF2 12. Barium and Selenium BaSe 13. Lithium and Oxygen Li2O 14. Francium and Astatine FrAt 15. Gallium and Iodine GaI3 16. Sodium and Phosphorus Na3P 17. Silver and Arsenic Ag3As 18. Zinc and Oxygen ZnO 19. Scandium and Bromine ScBr3 20. Rubidium and Sulfur Rb2S

Practice Writing Names of Type I Ionic Compounds 1. LiF lithium fluoride 2. GaI3 gallium iodide 3. FrAt francium astatide 4. Li2O lithium oxide 5. BaSe barium selenide 6. CaBr2 calcium bromide 7. NaI sodium iodide 8. BaO barium oxide 9. Na3As sodium arsenide 10. Al2O3 aluminum oxide 11. ZnS zinc sulfide 12. KBr potassium bromide 13. SrO strontium oxide 14. RaCl2 radium chloride 15. BeF2 beryllium fluoride 16. Cs2Te cesium telluride 17. RbI rubidium iodide 18. CaBr2 calcium bromide 19. MgO magnesium oxide 20. Be3P2 beryllium phosphide

Practice Writing Formulas of Type II Ionic Compounds 1. Cu 1+ and chlorine CuCl 2. Fe 3+ and oxygen Fe2O3 3. Co 2+ and bromine CoBr2 4. Pb 4+ and iodine PbI4 5. Cr 3+ and chlorine CrCl3 6. Au 3+ and bromine AuBr3 7. Mn 4+ and sulfur MnS2 8. Pt 2+ and oxygen PtO 9. Sb 3+ and fluorine SbF3 10. Co 3+ and oxygen Co2O3 11. Ti 4+ and chlorine TiCl4 12. Fe 2+ and oxygen FeO 13. Pb 2+ and bromine PbBr2 14. Hg 2+ and fluoride HgF2 15. Hg2 2+ and fluoride Hg2F2 16. Po 2+ and arsenic Po3As2 17. V 4+ and astatine VAt4 18. Cu 1+ and fluorine CuF 19. Ni 3+ and nitrogen NiN 20. Fe 2+ and sulfur FeS

Practice Writing Names of Type II Ionic Compounds 1. SnBr2 tin (II) bromide 2. CrO chromium (II) oxide 3. HgI2 mercury (II) iodide 4. SbCl3 antimony (III) chloride 5. CoCl3 cobalt (III) chloride 6. MnCl2 manganese (II) chloride 7. CuI2 copper (II) iodide 8. FeO iron (II) oxide 9. Cr2O3 chromium (III) oxide 10. Co2O3 cobalt (III) oxide 11. AuBr3 gold (III) bromide 12. RuO2 ruthenium (IV) oxide 13. TiP titanium (III) phosphide 14. Mn3N4 manganese (IV) nitride 15. PtS platinum (II) sulfide 16. CuAt2 copper (II) astatide 17. NiI3 Nickel (III) iodide 18. Au2O gold (I) oxide 19. SnCl4 tin (IV) chloride 20. Bi2Se3 bismuth (III) selenide

Practice Writing Formulas of Polyatomic Compounds 1. Sodium and sulfate Na2SO4 2. Calcium and hydroxide Ca(OH)2 3. Francium and phosphate Fr3PO4 4. Potassium and permanganate KMnO4 5. Cu 2+ and perchlorate Cu(ClO4)2 6. Ammonium and nitrate NH4NO3 7. Rubidium and hydrogen sulfate RbHSO4 8. Co 2+ and sulfate CoSO4 9. Cu 1+ and hydroxide CuOH 10. Sn 4+ and acetate Sn(C2H3O2)4 11. Fe 3+ and sulfite Fe2(SO3)3 12. Potassium and carbonate K2CO3 13. Cr 3+ and cyanide Cr(CN)3 14. Magnesium and hydrogen phosphate MgHPO4 15. Cesium and hydroxide CeOH 16. Zinc and iodite Zn(IO3)2 17. Cadmium and dichromate CdCr2O7 18. Sb 3+ and nitrogen SbN 19. Strontium and oxalate SrC2O4 20. V 4+ and nitrite V(NO2)4

Practice Naming Polyatomic Compounds 1. Fe(NO3)3 iron (III) nitrate 2. Co3(PO4)2 cobalt (II) phosphate 3. Cr(CN)3 chromium (III) cyanide 4. Al2(SO4)3 aluminum sulfate 5. Cr(C2H3O2)2 chromium (II) acetate 6. (NH4)2SO3 ammonium sulfite 7. Cu(NO3)2 copper (II) nitrate 8. CuOH copper (I) hydroxide 9. Sn(IO3)2 tin (II) iodate 10. Fe2(SO3)3 iron (III) sulfite 11. NH4NO3 ammonium nitrate 12. FeSO4 iron (II) sulfate 13. LiClO4 lithium perchlorate 14. CoSO4 cobalt (II) sulfate 15. Mg(SCN)2 magnesium thiocyanate 16. Fe(NO2)3 iron (III) nitrite 17. BaCO3 barium carbonate 18. Ag2CrO4 silver chromate 19. In(IO3)3 indium iodate 20. Ni2(HPO4)3 nickel (II) hydrogen phosphate

Practice Writing Formulas and Naming Acids 1. HF hydrofluoric acid 2. HNO3 nitric acid 3. HClO4 perchloric acid 4. HI hydroiodic acid 5. HCN hydrocyanic acid 6. HC2H3O2 acetic acid 7. H2Se hydroselenic acid 8. H2Te hydrotelluric acid 9. HIO hypoiodous acid 10. H2CrO4 chromic acid 11. Hydrophosphoric acid H3P 12. Sulfurous acid H2SO3 13. Iodic acid HIO3 14. Boric acid H3BO3 15. Chloric acid HClO3 16. Phosphoric acid H3PO4 17. Hydrobromic acid HBr 18. Nitrous acid HNO2 19. Sulfuric acid H2SO4 20. Hydrotelluric acid H2Te

Practice Writing Formulas and Naming Type III Compounds 1. CCl4 carbon tetrachloride 2. NO2 nitrogen dioxide 3. IF3 iodine trifluoride 4. AsCl3 arsenic trichloride 5. SeO selenium oxide 6. XeF4 xenon tetrafluoride 7. NI3 nitrogen triiodide 8. H2O water 9. N2O5 dinitrogen pentoxide 10. SO2 sulfur dioxide 11. Iodine heptafluoride IF7 12. Phosphorus pentachloride PCl5 13. Tetraphosphorus hexoxide P4O6 14. Diboron trioxide B2O3 15. Carbon dioxide CO2 16. Dinitrogen tetrachloride N2Cl4 17. Diphosphorus pentoxide P2O5 18. Carbon tetraiodide CCI4 19. Sulfur dioxide SO2 20. Dinitrogen tetroxide N2O4

2026 © DocPlayer.net Privacy Policy | Terms of Service | Feedback  | Do Not Sell My Personal Information