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Clicker #1

Clicker #1. How many unpaired electrons and valence electrons does Se have? A) 0; 14 B) 2; 6 C) 2; 14 D) 0; 6 E) 2; 4. Atomic Trends. Atomic Radius: size of the orbital. decreasing. H. F. increasing. Fr. Atomic Trends. Atomic Radius: size of the orbital. decreasing. H. F.

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Clicker #1

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  1. Clicker #1 How many unpaired electrons and valence electrons does Se have? A) 0; 14 B) 2; 6 C) 2; 14 D) 0; 6 E) 2; 4

  2. Atomic Trends • Atomic Radius: size of the orbital decreasing H F increasing Fr

  3. Atomic Trends • Atomic Radius: size of the orbital decreasing H F More protons = more attraction and smaller radius Orbitals are getting bigger and further from nucleus increasing Fr

  4. Clicker #2 Which of the following elements has the largest atomic radius? A) Ca B) Al C) N D) Sr E) F

  5. Atomic Trends • Ionization Energy increasing H F decreasing Fr

  6. Atomic Trends • Ionization Energy increasing H F Electron is at its lowest energy state when closest to the nucleus takes more energy to take an electron away when closer to the nucleus decreasing Fr

  7. Clicker #3 Which of the following elements has the largest ionization energy? A) P B) Al C) Cl D) Ba E) K

  8. Isoelectronic Series • Same number of electrons Example: Which is larger Na+ or Ne?

  9. Isoelectronic Series • Same number of electrons Example: Which is larger Na+ or Ne? Same number of electrons but Na+ has 11 protons and Ne has 10 protons.

  10. Example Which is larger Cl- or Ar? Which has a higher ionization energy Cl- or Ar?

  11. Example Which is larger Cl- or Ar? Which has a higher ionization energy Cl- or Ar?

  12. BONDING • “Forces” • What is meant by a “chemical bond”? • Why do atoms bond to form molecules? • How do atoms bond to form molecules?

  13. BONDING • Two Types of Bonding • Intramolecular (within a molecule) • Intermolecular (between molecules)

  14. Ionic Compounds • Between a metal and a nonmetal Example: NaCl Na: [Ne]3s1 Cl: [Ne]3s23p5

  15. Ionic Compounds • Between a metal and a nonmetal Example: NaCl Na: [Ne]3s1 Na+: [Ne] Cl: [Ne]3s23p5 Cl-: [Ne] 3s23p6

  16. Mg -> Mg+ -> Mg2+ • Ionization energies of atoms are highly endothermic • HOWEVER… • Takes more energy to remove 2nd electron • Once you get Mg2+ (noble gas configuration) gives off energy OVERALL = EXOTHERMIC PROCESS

  17. Bonding in H2 • Is this ionic?

  18. Bonding in H2 • Covalent Bonding • Sharing electrons • Hydrogens share the electrons and have noble gas configuration • Why isn’t He diatomic?

  19. Bonding in H2 • Covalent Bonding • Sharing electrons • Hydrogens share the electrons and have noble gas configuration • Why isn’t He diatomic? • Already has a noble gas configuration

  20. Therefore… • Covalent bonding has same idea as ionic bonding… But Neither atom is “strong” enough to remove electron from the other atom

  21. What about CO?

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