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Chemical Nomenclature

This guide covers the essentials of naming Type I binary ionic compounds, which are composed of a metal cation and a non-metal anion. Key rules include naming the cation first, using the element's name, and naming the anion by taking the root of the element name and adding "-ide." Examples of cations and anions are provided, as well as an overview of Type II compounds with transition metals and Type III compounds consisting solely of nonmetals. Understanding these rules is crucial for correct chemical communication and formula writing.

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Chemical Nomenclature

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  1. Chemical Nomenclature Unit 4

  2. Naming Type I Binary Compounds • Binary compound • Made up of 2 elements consisting of a cation and an anion to make a Binary Ionic Compound • Made of a metal and non-metal element

  3. Rules for Naming Type I Ionic Compounds • 1. The cation is always named first and the anion second • 2. A simple cation (obtained from a single atom) takes its name from the name of the element. For example: Na+ is called sodium in the name of compounds containing this ion • 3. A simple anion (obtained from a single atom) is named by taking the first part of the element name (the root) and adding –ide. Thus the Cl- ion is called Chloride • 4. Write the name for the compound by combining the names of the ions

  4. Table 1: Common Simple Cations and Anions

  5. Examples

  6. Type II – Naming Binary Ionic Compounds that contain metals that form more than one type of cations • This type of compound contains a metal that can form more than one type of cation (Transition metals) • Differs from the Type I in that you place the Roman Numeral in the name • The Roman numeral tells the charge on the ion, not the number of ions present in the compound

  7. Examples • CuCl • Cu(I) chloride • HgO • Mercury (II) oxide

  8. Type III – Naming binary compounds that contain only nonmetals • 1. The first element in the formula is named first, and the full element name is used • 2. The element is named as though it were an anion • 3. Prefixes are used to denote the numbers of atoms present. These prefixes are given in the following table • 4. The prefix mono- is never used for naming the first element. • For example: CO is called carbon monoxide, not monocarbon monoxide

  9. Prefixes Used to Indicate Numbers in Chemical Names

  10. Examples • NO • Nitrogen monoxide • N2O5 • Di nitrogen pentaoxide • SF6 • Sulfur hexafluoride • SO2 • Sulfur dioxide • P4O6 • Tetra phosphorus hexaoxide

  11. Review • Type I • Ionic compounds with metals that always form a cation with the same charge • Type II • Ionic compounds with metals (usually transition metals) that form cations with various charges • Type III • Compounds that contain only nonmetals

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