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Chemistry Basics for Exams: Polyatomic Ions, Chemical Formulas, and Calculations

Learn how to memorize polyatomic ions, name acids, understand chemical formulas, hydrated compounds, molar mass, and more! Prepare for exams with essential tips and examples.

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Chemistry Basics for Exams: Polyatomic Ions, Chemical Formulas, and Calculations

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  1. MORE OF CHAPTER 3

  2. THE POLYATOMIC IONS • YOU MUST MEMORIZE, BY THE EXAM, ALL OF THE POLY ATOMIC IONS AND THEIR CHARGES. • TIPS ON NAMES AND CHARGES – IF IT ENDS IN ‘ATE’ IT WILL HAVE ___OXYGENS IF___________________ _________________________________ OTHERWISE IT WILL HAVE _____ OXYGENS. IF IT HAS ‘PER’ IN FRONT OF THE NAME, IT WILL HAVE ONE MORE OXYGEN THAN ITS ‘____’. EXAMPLES FOLLOW:

  3. NAMING ACIDS – Binary and ternary (oxy) acids BINARY – COMPOSED OF _______________________, ______________________________________________ NAME AS ____________ NON METAL_________ACID. OXY ACIDS – COMPOSED OF ____________________ ______________________________________________ OR A ________________________________________ _____________________________________________. NAME AS ________________ ‘IC’ ACID OR AS POLYATOMIC ION ‘IC’ ACID. EXAMPLES:

  4. TYPES OF CHEMICAL FORMULAS • MOLECULAR-______________________ __________________________________ • CONDENSED-______________________ __________________________________ • STRUCTURAL-_____________________ __________________________________ EXAMPLES:

  5. WHAT ARE HYDRATED COMPOUNDS? • HYDRATED COMPOUNDS ___________ __________________________________ EXAMPLES: AFTER HEATING THEY BECOME ANHYDROUS- THE ________________ _________________________________ EXAMPLE:

  6. MOLAR MASS OF COMPOUNDS • MOLECULAR WEIGHT -_____________ _________________________________ EXAMPLE: • FORMULA WEIGHT-_________________ _________________________________ EXAMPLE:

  7. MOLE TO MASS • CONVERT 3.25 MOLES OF PROPANE (C3H8) TO GRAMS • CONVERT 5.50 GRAMS OF CALCIUM SULFATE TO MOLES.

  8. MOLES TO ATOMS • CONVERT 6.21 MOLES OF WATER TO MOLECULES OF WATER AND THEN TO ATOMS OF HYDROGEN • CONVERT 2.15 X 1035 MOLECULES OF SULFURIC ACID TO MOLES OF SULFURIC ACID

  9. CALCULATING % COMPOSITION • WHAT IS THE % OF NITROGEN IN HCN • WHAT IS THE % COMPOSITION OF HCN • WHAT IS THE % OF H IN WATER • WHAT IS THE % COMPOSITION OF WATER DIRECTIONS: ADD UP _______________, ADD UP MASS OF PARTICLE OF INTEREST, ________________________ _____________ AND MULTIPLY BY ____

  10. CALCULATING THE EMPIRICAL FORMULA • THE EMPIRICAL FORMULA IS THE ____ ____________. EXAMPLE: C6H14 IS NOT AN EMPIRICAL FORMULA. IT IS A ______________ FORMULA. WHY? __________________ C—H–- IS AN EMPIRICAL FORMULA. TO CALCULATE – EXAMPLES FOLLOW:

  11. CALCULATE THE EMPIRICAL FORMULA OF A COMPOUND THAT IS 1.25%Ga AND 0.43% O. ANSWER = Ga2O3 STEPS: 1. ASSUME % OF ______g SAMPLE SO % = ______ 2. CONVERT TO _______________ OF EACH 3. DIVIDE BY _________ _________ 4. IF DECIMAL IS .1 OR .9 IT CAN BE ROUNDED, OTHERWISE YOU MUST MULTIPLY BY _______________________________________.

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