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Welcome to Chemistry I-2!

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. Predicting Charges on Monatomic Ions KNOW THESE !!!!.

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Welcome to Chemistry I-2!

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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

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

  3. Nomenclature Summary Flowchart

  4. Practice Round 1! N2O K2S Cu(NO2)2 H2S (aq) Cr2(SO4)3 Fe2(SO3)3 CaO BaCO3 ICl H3PO4 • 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! Barium iodide Hydrochloric acid Calcium hydroxide Iron (III) carbonate Sodium dichromate Diiodine pentoxide Copper (II) perchlorate Carbon disulfide Nitrous Acid Chromic Acid • 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 2 3 2

  8. Balancing Equations ____C3H8(g) + _____ O2(g) ----> _____CO2(g) + _____ H2O(g) 5 3 4 2 11 ____B4H10(g) + _____ O2(g) ----> ___ B2O3(g) + _____ H2O(g) 4 2 10 5

  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? 78.4 g K 1 mol K 6.02 X 1023 atoms K 39.1 g K 1 mol K = 1.20 X 1024 atoms K

  13. Learning Check! What is the mass (in grams) of 1.20 X 1024 molecules of glucose (C6H12O6)? 1.20 X 1024moleculesC6H12O61 mol C6H12O6 180. g C6H12O6 6.02 X 1023molec. C6H12O6 1 mol C6H12O6 = 358.8g C6H12O6

  14. Learning Check! How many atoms of O are present in 78.1 g of oxygen? 78.1 g O2 1 mol O2 6.02 X 1023molecules O2 2 atoms O 32.0 g O2 1 mol O2 1 molecule O2 = 2.94 X 1024 atoms O

  15. Quiz Thursday! Be prepared!

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