1 / 21

Atomic Trends and Bonding in Chemistry

This interactive session delves into atomic trends like radius and ionization energy, alongside bonding concepts in chemistry. Explore the intricacies of valence electrons, ionization energy increases, and covalent versus ionic bonding.

chaires
Download Presentation

Atomic Trends and Bonding in Chemistry

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. 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?

More Related