Covalent Compounds
This guide outlines the essential rules for naming covalent compounds, including the use of prefixes to indicate the number of atoms of each element present. Key points include writing the second element with an "-ide" ending and dropping vowels in prefixes when encountered with the same vowel at the beginning of an element name. It also clarifies when to omit "mono-" in the case of a single atom. Additionally, it lists common diatomic molecules and provides example formulas, aiding in understanding the nomenclature of binary covalent compounds.
Covalent Compounds
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Presentation Transcript
Rules for Naming Covalent Compounds 1. Prefixes are used to show how many atoms of each element are present in the compound Prefixes used for Naming Binary Covalent Compounds
2. Second element is written with an –ide ending. ***All binary compounds, both ionic and covalent end in –ide. 3. The vowel at the end of the prefix is dropped when the name of the element begins with the same vowel. Example: monoxide, not monooxide Rules for Naming Covalent Compounds
4. Mono is omitted if there is just a single atom on the first element in the name. Example: carbon dioxide not monocarbon dioxide Rules for Naming Covalent Compounds
Diatomic Molecules “BrINCl HOF” There are 7 nonmetals that exist in nature as diatomic molecules. Di-Atomic Formula: Br2 I2 N2 Cl2 H2 O2 F2 (means 2) atoms How to Remember-
Writing Formulas From Names Write the formulas for the following compounds. 1. carbon monoxide CO 2. nonacarbon tetrachloride C9Cl4 3. hexabromine dioxide Br6O2 4. phosphorus trichloride PCl3 5. octanitrogenpentafloride N8Fl5
Naming Binary Compounds (Covalent) Carbon monoxide Sulfur dioxide Dinitrogen monoxide Carbon tetrachloride Dinitrogenpentaoxide N2O4 OF2 Dinitrogentetraoxide Oxygen difluoride 1. CO 2. SO2 3. N2O 4. CCl4 5. N2O5
