1 / 19

Formula Writing Formulas show both: Quantitative – how much, how many atoms

Formula Writing Formulas show both: Quantitative – how much, how many atoms Qualitative – what types of elements present 3 C 6 H 12 O 6 3 – coefficient, how many glucose (3 moles) This tells you: Quantitative(subscripts) – 6 Carbon, 12 Hydrogen

jack
Download Presentation

Formula Writing Formulas show both: Quantitative – how much, how many atoms

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Formula Writing Formulas show both: Quantitative – how much, how many atoms Qualitative – what types of elements present 3 C6H12O6 3 – coefficient, how many glucose (3 moles) This tells you: Quantitative(subscripts) – 6 Carbon, 12 Hydrogen and 6 Oxygen are present Qualitative – Made up of Carbon, Hydrogen and Oxygen

  2. Types of Formulas • Empirical – simplest whole number ratio • CH2O • Molecular (true formula) • C6H12O6 • Structural • Hydrates • CuSO4 5 H2O .

  3. Formula Writing 1. Sum of all oxidation numbers of any formula must = 0 2. work only with the metals, non-metals and polyatomic ions (table E) CrissCross Method K+Cl- Mg+2 S-2 Al+3 Cl-1 Mg +2 Br - K Cl Mg S AlCl3 MgBr2

  4. Formula Writing 1. Sum of all oxidation numbers of any formula must = 0 2. work only with the metals, non-metals and polyatomic ions (table E) CrissCross Method K+ ClO4- Mg+2 PO4-3 Al+3 NO2-1 Mg +2 Mn04- KClO4 Mg3(PO4)2 Al(NO2)3 Mg(MnO4)2

  5. Zone 1 Zone 3 Zone 2

  6. Binary Compounds - ide Zone 1-3 Zone 3-3 Zone 2-3 • Grp 1,2 M – NM Trans M – NM Molecular compds (Covalent NM – NM) “Call it like you see it” “Call it like you see it” Use Prefix on 2nd NM Roman Numerals to indicate Use on first if more than 1NM NaCl FeCl2 FeCl3 1- mono, 2- di, 3-tri, 4 tetra Name Metal – Sodium Name Metal with ox # 5- penta, 6 hexa Name the Non Metal Iron II Chloride Iron III Chloride (Chlorine) drop end add - ide CO Carbon Monoxide Sodium Chloride CO2 Carbon Dioxide N2O5DinitrogenPentoxide

  7. Zone 1 Zone 4 Zone 2 Zone 3

  8. Ternary Compounds Zone 1-3 Zone 2-3 Zone 3-4 Zone 3-3 Transition M –PI- nm (Roman Numerals) Cu2SO4 Copper (I) Sulfate CuSO4 Copper (II) sulfate PI + - PI - m nm (call it like you say it) (NH4)2SO4 Ammonium Sulfate NH4NO3 Ammonium Nitrate Group 1,2 M –PI- nm Na2SO4 Sodium Sulfate Al2(SO4)3 Aluminum Sulfate PI+ - NM m (name it like a binary –ide) NH4Cl Ammonium chloride

  9. Naming AcidsBinary vs Ternary (formula always begin with H) H – polyatomic ion (end in ate or ite) H – ate H- ite Remember, you ate it and it was icky! (ate-ic) (ite-ous) H2SO4 HNO2 Sulfuric Acid Nitrous Acid • HCl • Always start with “Hydro” • Name the non-metal • Chlorine • Change ending to • - ic acid • Name = Hydrochloric Acid

  10. Types of Equations Synthesis ( 2 to 1) A + B AB Decomposition (1 to 2) AB  A + B • Fermentation • Always produces Alcohol and CO2 • (C2H5OH + CO2) • C6H12O6  C2H5OH + CO2 Combustion (Always produces CO2 and H2O Burn reaction – need O2 C3H8 + O2 CO2 + H2O

  11. Types of Equations Single Replacement ( element-compound element compound) Red is the Metal A + BC  AC + B ***Remember Table J Activity Series Who is the Bully? Ca + HCl  CaCl2 + H2 (g) works. Cu + HCl  N.R. Why? AG + MgCl2  Reaction….yes or no?

  12. Types of Equations Double Replacement ( compound-compound compound - compound) Red is the Metal A B + C D  AD + CB HCl + NaOH  NaCl + HOH NaCl + HOH  NaOH + HCl MgCl2 + (NH4)2SO4 

  13. A Reaction will go to completion when: • A gas (g) is produced • Water is a product • One of the products is insoluble (does not dissolve) Table F solubility Guidelines

  14. Table F Solubility Guidelines for Aqueous solutions

  15. Try these out! What type of reactions do we see? • Zn + HCl ZnCl2 + H2 • NaClO3  NaCl + O2 • P4 + Cl2  PCl3 • HCl + Mg(OH)2  MgCl2 + H(OH) • BaO + SO3  BaSO4 • Pb + AgNO3  Ag + Pb(NO3)2 • AgNO3 + Na2CrO4  Ag2CrO4 + NaNO3

  16. Balancing Equations **An equation must show conservation of both Mass and Charge 2Ca0 + O20 2Ca+2O-2 Steps to follow: 1. Write the correct formula first, if needed 2. Pick a start point and let it take you to the next…… 3. If you see water, change the formula from H2O to H(OH) 4. Always work the polyatomic ions (SO4, NO3etc.) as a whole 5. Try not to deal with any odd # coefficients. a. if present, double their value to make it even

  17. PRACTICE ___HgO  ___Hg + ___O2 ___ Li + ___Br2 ___ LiBr ___Al + ___Cl3  ___AlCl3 ___Al2O3 ___Al + ___O2 ___Ca3(PO4)2 + ___H2SO4  ___Ca(SO4) + ___ H3PO4 (Combustion Reactions: Always do in this order- C,H,O) ____C3H8 + ___O2  ___CO2 + ____H2O

More Related