Ch.10 - Molecular Shapes & Valence Bond TheoryWorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Describe the orbitals used to form the pi-bond between the C* and N*.
  1. 2p – 2p
  2. sp2 – sp3
  3. sp3 – sp3
  4. sp2 – sp2
  5. sp2 – sp 

Solution: Describe the orbitals used to form the pi-bond between the C* and N*.2p – 2psp2 – sp3sp3 – sp3sp2 – sp2sp2 – sp 

Problem

Describe the orbitals used to form the pi-bond between the C* and N*.

  1. 2p – 2p
  2. sp2 – sp3
  3. sp3 – sp3
  4. sp2 – sp2
  5. sp2 – sp 
Solution

We’re being asked to determine the orbitals that overlap to form the indicated pi bond between C* and N* in the given molecule:



Recall that π (pi) bonds are the double and triple bonds in a molecule. They are formed from the side-on overlap of p atomic orbitals.



We first need to look at the valence electron configuration of carbon and nitrogen.


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