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Atomic Theory Practice

Atomic Theory Practice. Name the element: Na 23 11 ? 32 16 ? 14 6 ? 39 19 + Group IIA, Period 3 1s 2 2s 2 2p 5. Sodium. Sulfur. Carbon-14. Potassium ion. Magnesium. Fluorine. MOLECULAR MADNESS. Bonding, Shape, Polarity & Reactions. ATOMIC THEORY.

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Atomic Theory Practice

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  1. Atomic Theory Practice Name the element: • Na2311 • ?3216 • ?146 • ?3919+ • Group IIA, Period 3 • 1s22s22p5 Sodium Sulfur Carbon-14 Potassium ion Magnesium Fluorine

  2. MOLECULAR MADNESS Bonding, Shape, Polarity & Reactions

  3. ATOMIC THEORY • Atoms composed of subatomic particles

  4. Exothermic (heat emitting, i.e. chem warm up :) Exercise #1 A. Draw the Lewis structure for Carbon. B. Why do atoms bond with one another? C. What are the 2 main types of intramolecular bonds? To fill their valence shell (Octet Rule) Ionic – transfer electrons Covalent – share electrons

  5. BONDING Ionic Bonds Transferred electrons Formed between metals & nonmetals Metals = + cations w/full valence Nonmetals = - anions w/full valence Opposing charges attract STRONGLY Ionic Compounds High melting pts Good electrical conductors in solution

  6. Ionic Bonding - Lewis Dot structures http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/bond.html

  7. BONDING Non-polar Covalent e- shared equally atoms w/similar electronegativities Polar Covalent e- shared Unequally atoms w/different electronegativities Covalent Bonds – shared electrons http://iws.collin.edu/biopage/faculty/mcculloch/1406/outlines/chapter%202/chap02.html

  8. Covalent Bonding - Lewis Dot structures Polar or Nonpolar? Nonpolar Polar or Nonpolar? Nonpolar Polar or Nonpolar? Polar http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/bond.html

  9. Polarity in Molecules Nonpolar Molecules • Very little attraction between them • Generally gases @ room temp • Ex: CO2 Polar Molecules • Have dipoles (ends with opposite charges) • Electrons pulled toward more electronegative atom • Attraction between dipoles of adjacent molecules • Ex: H2O CO2 http://www.exo.net/~pauld/workshops/Greenhouse%20Effect/greenhouse.html http://www.chem1.com/acad/webtext/states/interact.html http://www.chem.umass.edu/genchem/whelan/class_images/Structure_of_Water.jpg

  10. VSEPR Theory • Valence Shell Electron Pair Repulsion • Outer shell e- pair up • Arrange themselves as far apart from other pairs as possible since they repel other neg. charges • Responsible for molecular shape Sample Shapes chemistry.gcsu.edu Bent

  11. http://www.chem.latech.edu/~upali/chem101/101MSJc8.htm Bond Length Periodic Trend • as you move down group and right to left within a period, bond length increases • Same as atomic radius • Double & triple bonds are shorter than single Radius & bond length increase http://chemwiki.ucdavis.edu/Theoretical_Chemistry/Chemical_Bonding/Bond_Order_and_Lengths

  12. Intermolecular Forces Hydrogen Bonds • Formed between molecules whose atoms have extremely different electronegativities • Most electronegative atoms: F, O, N bonded to • Least electronegative atom: H • Strong intermolecular force, causing high boiling points • Not nearly as strong as INTRAmolecular bonds like covalent

  13. Bonding Review

  14. Endergonic(chem energy INTO your brain :)Exercise #1 • In textbook, • Read p.275 • Answer the following questions from p.276-77: • MC 1,2,6,10 • T/F 13,18 • CM 22,24,26

  15. Chemical Reactions • Substances converted into NEW substances w/NEW properties Reactants – What goes in Products – What comes out ReactantsProducts Glucose + Oxygen  Carbon Dioxide + Water C6H12O6 + O2  CO2 + H2O C6H12O6 + 6O2  6CO2 + 6H2O C6H12O6(s) + O2(g)  CO2(g) + H2O(l) Words Formulas Balanced Equation Complete Equation

  16. Writing & Balancing Chemical Equations • Going from word formula to balanced… • Remember your naming rules! • Ionic compounds – cation (+) first then anion (-) • # of + charges must equal # of - charges • Ex: Sodium + Chlorine  Sodium Chloride Na+ + Cl- NaCl • Ex: Aluminum nitrate + Iron chloride  Iron Nitrate + Aluminum Chloride Al(NO3)3 + FeCl2 Fe(NO3)2 + AlCl3 • Covalent compounds – use the number prefixes to indicate numbers of atoms • Carbon + Chlorine  Carbon Tetrachloride C + 2Cl2  CCl4

  17. Cations +1 Group 1 atoms Ammonium NH4+1 +2 Group 2 atoms Anions -1 Group 7 atoms Chlorate = ClO3-1 Nitrate = NO3-1 Hydroxide = OH-1 -2 Group 6 atoms Sulfate = SO4-2 Carbonate = CO3-2 -3 Group 5 atoms Phosphate = PO4-3 Ions & Charges

  18. Naming & Writing Gases & Acids Gases • The name of the element followed by the word gas is always a diatomic molecule • Ex: Oxygen gas = O2 • Ex: Chlorine gas = Cl2 • Ex: Hydrogen gas = H2 Acids • The name of an ion followed by the word acid means you add the appropriate # of H’s in front of the ion • The # of H’s equals the - charge of the anion • Ex: Hydrochloric acid = HCl • Ex: Sulfuric acid = H2SO4 • Ex: Phosphoric acid = H3PO4

  19. Types of Chemical Reactions • Synthesis Reaction • aka direct combination reaction • 2 or more reactants come together to form a single product • A + B  AB • 2Na + Cl2  2NaCl • Decomposition Reaction • Single compound broken down into 2 or more smaller products • AB  A + B • 2H2O  2H2 + O2

  20. Types of Chemical Reactions • Single Replacement Reaction • Uncombined element takes the place of another element within a compound • A + BX  AX + B • Mg + CuSO4  MgSO4 + Cu • More active elements replace less active ones • Activity level shown in activity series • If uncombined element NOT more active, then no reaction takes place

  21. Types of Chemical Reactions • Double Replacement Reaction • Atoms or ions from 2 different compounds replace each other • AX + BY  AY + BX • CaCO3 + 2HCl  CaCl2+ H2CO3

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