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Chemistry Review & Practice: Nomenclature, Equations, Molar Conversions

Welcome to Chemistry I-2! This review covers important topics from Chemistry I-1, including nomenclature, balancing equations, and gram/mole/atom/molecule conversions. Learn about predicting charges on monatomic ions, follow nomenclature flowcharts, and practice balancing equations. Gain a deeper understanding of the mole and molar mass concepts, with interactive learning checks and quizzes to reinforce your knowledge. To save paper and ink, print handouts instead of slides in PowerPoint and turn off backgrounds. Stay prepared for upcoming quizzes and tests in chemistry class!

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Chemistry Review & Practice: Nomenclature, Equations, Molar Conversions

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  1. Welcome to Chemistry I-2! • Review of Important Chemistry I-1 topics of science! • Nomenclature (writing formulas and names) • Balancing Equations • Gram / Mole / Atom / Molecule conversions SAVE PAPER AND INK!!! When you print out the notes on PowerPoint, print "Handouts" instead of "Slides" in the print setup. Also, turn off the backgrounds (Tools>Options>Print>UNcheck "Background Printing")!

  2. Predicting Charges on Monatomic Ions KNOW THESE !!!! +1 +2 -3 -2 -1 0 Cd+2

  3. Nomenclature Summary Flowchart

  4. Practice Round 1! • Dinitrogen monoxide • Potassium sulfide • Copper (II) nitrite • Hydrosulfuric acid • Chromium (III) sulfate • Iron (III) sulfite • Calcium oxide • Barium carbonate • Iodine monochloride • Phosphoric acid

  5. Practice Round 2! • BaI2 • HCl (aq) • Ca(OH)2 • Fe2(CO3)3 • Na2Cr2O7 • I2O5 • Cu(ClO4)2 • CS2 • HNO2 10. H2CrO4

  6. Balancing Equations • When balancing a chemical reaction you may add coefficients in front of the compounds to balance the reaction, but you may not change the subscripts. • Changing the subscripts changes the compound. Subscripts are determined by the valence electrons (charges for ionic or sharing for covalent)

  7. Balancing Equations Sodium phosphate + iron (III) oxide  sodium oxide + iron (III) phosphate Na3PO4 + Fe2O3 ----> Na2O + FePO4

  8. Balancing Equations ____C3H8(g) + _____ O2(g) ----> _____CO2(g) + _____ H2O(g) ____B4H10(g) + _____ O2(g) ----> ___ B2O3(g) + _____ H2O(g)

  9. The Mole • A counting unit • Similar to a dozen, except instead of 12, it’s 602,000,000,000,000,000,000,000 • 6.02 X 1023 (in scientific notation) • This number is named in honor of Amedeo Avogadro (1776 – 1856)

  10. Molar Mass • The Mass of 1 mole (in grams) • Equal to the numerical value of the average atomic mass (get from periodic table), or add the atoms together for a molecule 1 mole of C atoms = 12.0 g 1 mole of Mg atoms = 24.3 g 1 mole of Cu atoms = 63.5 g 1 mole of O2 molecules = 32.0 g

  11. Calculations molar mass Avogadro’s numberGrams Moles particles Everything must go through Moles!!!

  12. Learning Check! How many atoms of K are present in 78.4 g of K?

  13. Learning Check! What is the mass (in grams) of 1.20 X 1024 molecules of glucose (C6H12O6)?

  14. Learning Check! How many atoms of O are present in 78.1 g of oxygen?

  15. Quiz Wednesday! Be prepared!

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