Polyatomic ions
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This document lists common polyatomic ions and their charges, along with some monatomic ions for comparison. It includes ions like ammonium (NH4+), hydronium (H3O+), hydroxide (OH-), phosphate (PO43-), sulfate (SO42-), nitrate (NO3-), and others that are important for students to memorize from chemistry. A note at the bottom indicates that the colored polyatomic ions should be committed to memory from Table 7.9 of the referenced chemistry book.
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this is a ppt made bby Hima Mohammed
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hope you ll like it
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2. Carbonates and bicarbonates react with acids to produce carbon dioxide gas. Sulphur-containing anions such as sulphides, sulphites, thiosulphates and sulphates are identified through reactions that produce precipitates, gases, or color changes with reagents like barium chloride, silver nitrate, and iron (III) chloride.
3. Common tests involve observing properties like solubility, as
Precipitates
This document discusses precipitation reactions and salt families. It provides the following key points:
1. Salts are produced from chemical reactions between acids and other substances. Each acid produces a characteristic family of salts, such as sulfates from sulfuric acid and nitrates from nitric acid.
2. Precipitation occurs when two solutions are mixed and an insoluble compound forms, coming out of solution as a solid precipitate. Solubility rules can be used to predict whether a precipitation reaction will occur.
3. Practical experiments are described to mix solutions of substances like lead nitrate and barium chloride and observe any precipitates that form based on the solubility rules. Word equations are also written for precipitation
Atoms and molecules
The document provides information about common elements, atoms, molecules, and ions. It includes tables that list element symbols and atomic masses, common ions and their symbols, examples of ionic compounds and their ratios, and the valencies of different ions. The tables provide essential data about common elements, ions, and how they combine to form ionic compounds.
New chm 151 unit 8 power points su13
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. It explains that the name of the cation (metal) comes first, followed by the anion (nonmetal) with the "-ide" suffix. Examples of naming compounds of common metals like calcium, magnesium, and sodium are provided. The document then discusses polyatomic ions and compounds containing them. It also covers compounds where the metal forms more than one ion. Finally, it discusses acids and naming compounds containing oxoanions. In summary, the document outlines the system for systematically naming inorganic compounds based on their formulas as well as writing formulas from IUPAC names.
Formula list form 4
Chemical formulae, equations, calculations, and reactions are summarized. Molar mass, moles, volume, and molarity calculations are explained for gases, solids, liquids, and solutions. Common cationic and anionic symbols are listed. Formulae for common compounds are provided. Group 1 and 17 elements and their reactions are summarized. Electrochemistry concepts like electrolytes, ionization, and the discharge of ions are condensed. Acid-base reactions and properties are highlighted at a high level. Solubility, preparation, color, and the effect of heating on salts are briefly touched upon.
Spm chemistry formula list form 4
Chemical formulae, equations, calculations, and reactions are summarized. Molar mass, moles, volume, and molarity calculations are explained for gases, solids, liquids, and solutions. Common cationic and anionic symbols are listed. Formulae for molecules and ions are provided. Periodic trends and reactions of Groups 1 and 17 are summarized. Electrochemistry principles of electrolytes, discharge reactions, and test observations are condensed. Characteristics of acids, bases, and ionization are highlighted. Solubility, preparation, color, and effects of heating for various salts are summarized concisely.
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Polyatomic ions
- 1. +1 CHARGE -1 CHARGE -2 CHARGE -3 CHARGE -4 CHARGE ion name ion name ion name ion name ion name NH4+ ammonium H2PO3- dihydrogen HPO32- hydrogen PO33- phosphite P2O74- pyrophosphate phosphite phosphite H3O+ hydronium H2PO4- dihydrogen HPO42- hydrogen PO43- phosphate phosphate phosphate Hg22+ mercury(I) HCO3- hydrogen CO32- carbonate PO23- hypophosphite carbonate - HSO3 hydrogen SO32- sulfite AsO33- arsenite sulfite - HSO4 hydrogen SO42- sulfate AsO43- arsenate sulfate - NO2 nitrite S2O32- thiosulfate NO3- nitrate SiO32- silicate - OH hydroxide C22- carbide - C2H3O2 acetate C2O42- oxalate CrO2- chromite CrO42- chromate - CN cyanide Cr2O72- dichromate - CNO cyanate C4H4O62- tartrate CNS- thiocyanate MoO42- molybdate - O2 superoxide O22- peroxide - MnO4 permanganate S22- disulfide ClO- hypochlorite - ClO2 chlorite ClO3- chlorate - ClO4 perchlorate - BrO hypobromite BrO2- bromite - BrO3 bromate - BrO4 perbromate IO- hypoiodite - IO2 iodite - IO3 iodate IO4- periodate - AlO2 aluminate N3 - azide *** The coloured Polyatomic Ions are from table 7.9 in Chemistry book. (MUST be memorized)***