Binary.Ionic.Compds
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This presentation is a brief introduction to the nomenclature topic of naming and writing of binary ionic chemical compounds.
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This document discusses the rules for naming ionic compounds, covalent compounds, and compounds containing transition metals. It provides examples of naming compounds from their formulas, such as sodium hydroxide (NaOH), lithium sulfide (Li2S), and iron(III) chloride (FeCl3). It also gives examples of writing formulas from compound names, like beryllium chloride (BeCl2), copper(I) oxide (Cu2O), and diphosphorus pentoxide (P2O5).
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This document provides notes on chemical nomenclature and bonding. It discusses the naming of ionic and molecular compounds using common names and IUPAC rules. Key topics covered include naming binary ionic compounds, transition metal ions, polyatomic ions, acids, and writing formulas from names and vice versa. The document emphasizes memorizing common monatomic ions and using subscripts, prefixes and Roman numerals correctly in naming various chemical species.
New chm-151-unit-8-power-points-su13-140227172225-phpapp01
This document provides information on naming and writing formulas for inorganic compounds. It begins by discussing binary ionic compounds formed from a metal and nonmetal, such as magnesium chloride (MgCl2). It then covers compounds containing polyatomic ions like hydroxide (OH-) or sulfate (SO42-). The document also discusses ternary compounds containing an oxoanion and a metal. Finally, it discusses acids, explaining how acid names are related to the anion names and providing examples like hydrochloric acid (HCl). Overall, the document outlines the systematic approach to naming inorganic compounds of different types based on their constituent elements and ions.
Chemical Formula
The document discusses chemical formulas and how they are derived. It explains that chemical formulas show the number and type of atoms in a molecule using element symbols. It then provides examples of how to determine formulas using valency, including transition metals that can have multiple valencies indicated by Roman numerals. Prefixes in compound names can also indicate the number of atoms present.
Nomenclature
The document provides information on naming and writing formulas for various types of chemical compounds including:
1. Ionic compounds formed from cations and anions are named by writing the metal first followed by the nonmetal with the appropriate ending (e.g. NaCl is sodium chloride).
2. Molecular compounds formed from nonmetals use prefixes to indicate the number of atoms and the second element takes the "-ide" ending (e.g. CO2 is carbon dioxide).
3. Acids are named by identifying if they contain one or two elements and whether they contain oxygen, and using appropriate endings like "-ic", "-ous", or specifying the anion (e.g. HCl is hydrochlor
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Binary.Ionic.Compds
- 1. Chemistry 101 NoMnClAtURe D. Hamilton, Instructor
- 2. Chemistry is Elementary What is the name of the chemical in the picture? Objective Naming ionic compounds from formulas Writing formulas from ionic compounds 2
- 4. Transition Metals Requiring Roman Numerals Transition Metals can form more than one kind of charged ion. Roman Numerals are used to indicate the charge when naming them: Fe2+ iron II ion or ferrous ion Fe3+ iron III ion or ferric ion 4
- 7. Naming Simple Ionic Compounds Name the compound whose formula is CaCl2 Name the two ions present: Metal cation Nonmetal anion Ca2+Cl1- Name: calcium chloride 7
- 8. To name the ions present: Remember that metals use the element name nonmetals change end of name to -ide. Name the compound KI. 8
- 9. Name these simple binary ionic compounds: Li2S Mg3N2 AlI3 CaSe KBr 9
- 10. Answers: Formula Li2S Mg3N2 AlI3 CaSe KBr Name lithium sulfide magnesium nitride aluminum iodide calcium selenide potassium bromide 10
- 11. Writing an Ionic Compound’s Formula Step 1: Write ions for elements in the name. Step 2: Balance charges by one of two methods. Step 3: Place subscripts behind each element if needed. Sodium chloride Na1+ Cl1- NaCl 11
- 12. Balancing Charges I Write the formula for tin (II) fluoride. Step 1: Write the ions Sn2+ and F1-. 12
- 13. Balancing Charges II Write the formula for tin (II) fluoride. Step 2: How many of each ion will it take to balance the charge electrically? + F1- + F1- 1Sn(2+) + 2F(-1) = 0 13 Sn
- 14. Balancing Charges III Write a formula for tin (II) fluoride. 1Sn(2+) + 2F(-1) = 0 Step 3: Place subscripts behind each element. SnF2 14
- 15. Crisscrossing Charges I Write the formula for magnesium nitride. Step 1: Write the ions: Mg2+ and N3- 15
- 16. Crisscrossing Charges II Write the formula for magnesium nitride. Step 2: Crisscross charges to become subscripts but delete the sign on the charge: Mg2+ N3- Mg3N2 16
- 17. Crisscrossing Charges III Write the formula for magnesium nitride. Step 3: Check the algebraic sum and complete the formula with subscripts: 3Mg(2+) + 2N(-3) = 0 Mg3N2 17
- 18. Write a formula for: Lithium oxide Copper (II)sulfide Aluminum selenide
- 19. Answers: Names Lithium oxide Copper(II) sulfide Aluminum selenide IonsFormula Li1+ O2- Li2O Cu2+ S2- CuS Al3+ Se2- Al2Se3
- 20. …and now a parting riddle… Two atoms are leaving Blackboard’s EyeOn Cafe. Atom A says to Atom B, “I think I left my electrons inside.” Atom B says, “Are you sure?” “Yes,” Atom A replies. “I’m positive!” Atom B says, “That’s OK, I picked them up!” Who are these two atoms now? 20
- 21. Credits Creative Commons/Flicker images found on slides 2, 6, 7, 10-12. Retrieved 3:00 PM June 22, 2009 from http://creativecommons.org/ and http://www.flickr.com Graphics on slides 3, 4 from Instructor Resource CD that accompanies Karen Timberlake’s General, Organic, and Biological Chemistry: Structures of Life, 2nd edition, (2007), Pearson Publishing, San Francisco. Slide 16 Cybart image from Microsoft Office 2007 clipart. Riddle adapted from a joke told on National Public Radio original author is unknown. 21