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Building Atoms

Building Atoms. OBJECTIVES. REVIEW ATOMIC CONCEPTS BUILD MODELS OF ATOMS AS A REVIEW BUILD MODELS OF IONIC BONDING BUILD MODELS OF COVALENT BONDING BUILD MODELS OF HYDROGEN BONDS COMPARE & CONTRAST IONIC, COVALENT AND HYDROGEN BONDING. BUILD A HELIUM ATOM.

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Building Atoms

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  1. Building Atoms

  2. OBJECTIVES REVIEW ATOMIC CONCEPTS BUILD MODELS OF ATOMS AS A REVIEW BUILD MODELS OF IONIC BONDING BUILD MODELS OF COVALENT BONDING BUILD MODELS OF HYDROGEN BONDS COMPARE & CONTRAST IONIC, COVALENT AND HYDROGEN BONDING

  3. BUILD A HELIUM ATOM • Draw the helium atom & label its parts

  4. Jot down the following • What would happen if the number of protons changed? • What would happen if the number of electrons changed? • What would happen if the number of neutrons changed?

  5. BUILD A HYDROGEN ATOM • Draw the hydrogen atom & label its parts • What happens if you change the number of: • Protons? • Electrons? • Neutrons?

  6. ORBITALS

  7. BUILD ATOMS • C • N • O • F

  8. ELECTRONEGATIVITY • "Electronegativity is the power of an atom when in a molecule to attract electrons to itself." • Increases left to right • Decreases top to bottom

  9. QUESTIONS • How many electrons fit on each orbital? • How does the proton number compare to the electron number? • How does the number of electrons in the outer orbital relate to the stability of the element? • Which elements are the most stable? Why? • Which elements are the most reactive? Why?

  10. QUESTIONS • How many electrons fit on each orbital? • 2 on the inner s orbital • Eight on the next two

  11. QUESTIONS • How does the proton number compare to the electron number? • They are the same if the element is unchanged/unaltered

  12. QUESTIONS • How does the number of electrons in the outer orbital relate to the stability of the element? • Elements with full orbitals or valence shells are more stable & less reactive • Elements with partially complete valence shells are more reactive • The closer an element is to having a completely full or completely empty valence shell is more reactive

  13. QUESTIONS • Which elements are the most stable? Why? • Nobel gases (Column VIII) • Their outer orbitals are filled

  14. QUESTIONS • Which elements are the most reactive? Why? • The halogens (VII) • Their outer shell is almost complete • Metals (I) • Their outer shell is almost empty (need to lose one electron)

  15. BUILD A FLUORINE ATOM &A HYDROGEN ATOM • HOW WILL THE GAIN/LOSS OF AN ELECTRON CHANGE THE STABILITY OF EACH? • WHAT HAPPENS WHEN AN ELECTRON IS MOVED FROM HYDROGEN TO FLUORINE? • MOVE THE ELECTRONS • DRAW A BEFORE AND AFTER DIAGRAM OF THE HF MOLECULE

  16. BUILD IONIC COMPOUNDS • LiCl • MgO • BeS • NaF

  17. IONIC BONDING • Ionic bonding is the complete transfer of valence electron(s) between atoms. • It is a type of chemical bond that generates two oppositely charged ions. • In ionic bonds, the metal loses electrons to become a positively charged cation, whereas the non-metal accepts those electrons to become a negatively charged anion. • Ionic bonds require an electron donor, metal, and an electron acceptor, nonmetal.

  18. QUESTIONS • In the models you built, which atoms are the cations? Which are the anions? • Which elements of the periodic table tend to become negative ions/anions (have the greatest potential for gaining electrons)? Why? • Which elements of the periodic table tend to become positive ions/cations (have the weakest ability to retain their electrons)? Why? • Which columns would combine well in order for both to be more stable?

  19. QUESTIONS • Which elements of the periodic table tend to make ionic bonds? • How does electronegativity correlate with ionic bonding? • Why don’t all the elements of the periodic table form ionic bonds? • What do atoms that cannot form ionic bonds do to become more stable?

  20. QUESTIONS • In the models you built, which atoms are the cations? Which are the anions? • Cations – Li, Mg, Be, Na • Anions – Cl, O, S, F

  21. QUESTIONS • Which elements of the periodic table tend to become negative ions/anions (have the greatest potential for gaining electrons)? Why? • Column VII (halogens) • Only missing one electron & have high electronegativity

  22. QUESTIONS • Which elements of the periodic table tend to become positive ions/cations (have the weakest ability to retain their electrons)? Why? • Far left, column I • They have only one electron in their outer orbital & have low electronegativity

  23. QUESTIONS • Which columns would combine well in order for both to be more stable? • Columns I & VII • Columns 2 & VI

  24. QUESTIONS • Which elements of the periodic table tend to make ionic bonds? • Columns I & VII • Columns II & VI

  25. QUESTIONS • How does electronegativity correlate with ionic bonding? • Atoms with high electronegativity steal electrons • Atoms with low electronegativity have their electrons stolen

  26. QUESTIONS • Why don’t all the elements of the periodic table form ionic bonds? • Elements are unable to steal or give enough electrons • Electronegativity too low to steal enough electrons • Electronegativity too high to release enough electrons

  27. QUESTIONS • What do atoms that cannot form ionic bonds do to become more stable? • They share

  28. BUILDING COVALENT MOLECULES • Make two hydrogen atoms • Are these atoms likely to form ionic bonds? • NO – have equal electronegativity & cannot give or take • What can these atoms do to become stable? • Form covalent bonds

  29. BUILD COVALENT MOLECULES • H2

  30. BUILD COVALENT MOLECULES • CH4 • NH3

  31. BUILD COVALENT MOLECULES • O2 • CO2

  32. COVALENT BONDING • Electrons are shared – valence shells then complete

  33. BUILD COVALENT MOLECULES • C2H6 • C3H8

  34. BUILD COVALENT MOLECULES • C2H6 • C3H8

  35. BUILD COVALENT MOLECULES • C2H6 (ethane) • C3H8 (propane)

  36. QUESTIONS • How do the valence electrons influence molecular bonding? • How does electronegativity influence molecular bonding?

  37. QUESTIONS • How do the valence electrons influence molecular bonding? • The number of open places on the valence shell determine the number of bonds the atom can form

  38. QUESTIONS • How does electronegativity influence molecular bonding? • If the difference in electronegativity between the 2 atoms is great, then ionic bonds form (one atom steals the atoms from another) • If the electronegativity is equal (or close), then covalent bonds form

  39. HYDROGEN BONDING - DRAW • CH4 • C2H6 • C3H8

  40. HYDROGEN BONDING - DRAW • O2 • CO2

  41. HYDROGEN BONDS • How many bonds can the following atoms make: • H? • O? • C?

  42. HYDROGEN BONDING - DRAW • H2O • H2 • O2 • CH2F • CH4

  43. QUESTIONS • Which molecules are symmetrical? • Which are polar and which are non-polar? • How does symmetry correlate with polarity? • How does electronegativity correlate with polarity?

  44. QUESTIONS • Which molecules are symmetrical? • H2, O2, CH4

  45. QUESTIONS • Which are polar and which are non-polar? • Polar - H2O & CH2F • Non-polar - H2, O2, CH4

  46. QUESTIONS • How does symmetry correlate with polarity? • Symmetrical molecules are non-polar • Asymmetrical molecules are polar

  47. QUESTIONS • How does electronegativity correlate with polarity? • The atom in the molecule with the higher electronegativity will pull the electrons to it unequally • This creates an unequal distribution of charge (without becoming a charged ion)

  48. HYDROGEN BONDING • Bonds that forms between the positive and negative ends of a water molecule (hydrogen to oxygen)

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