ib dp1 chemistry hl bonding n.
Download
Skip this Video
Loading SlideShow in 5 Seconds..
IB DP1 Chemistry HL Bonding PowerPoint Presentation
Download Presentation
IB DP1 Chemistry HL Bonding

Loading in 2 Seconds...

play fullscreen
1 / 21

IB DP1 Chemistry HL Bonding - PowerPoint PPT Presentation


  • 427 Views
  • Uploaded on

IB DP1 Chemistry HL Bonding. What makes atoms join together to make compounds?. Topic 14 : Bonding. 14.1 Shapes of molecules and ions 1 hour 14.1.1 Predict the shape and bond angles for species with five and six negative charge centres using the VSEPR theory. 14.2 Hybridization

loader
I am the owner, or an agent authorized to act on behalf of the owner, of the copyrighted work described.
capcha
Download Presentation

PowerPoint Slideshow about 'IB DP1 Chemistry HL Bonding' - kaiya


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.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.


- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript
ib dp1 chemistry hl bonding

IB DP1 ChemistryHL Bonding

What makes atoms join together to make compounds?

topic 14 bonding
Topic 14: Bonding

14.1 Shapes of molecules and ions

1 hour

14.1.1 Predict the shape and bond angles for species with five and six negative charge centres using the VSEPR theory.

14.2 Hybridization

2 hours

14.2.1 Describe σ and π bonds.

14.2.1 Describe σ and π bonds.

14.2.2 Explain hybridization in terms of the mixing of atomic orbitals to form new orbitals for bonding.

14.2.3 Identify and explain the relationships between Lewis structures, molecular shapes and types of hybridization (sp, sp2 and sp3).

14.3 Delocalization of electrons

2 hours

14.3.1 Describe the delocalization of π electrons and explain how this can account for the structures of some species.

which energy level is an electron in
Whichenergylevel is an electron in?

2p1

2nd quantum number

1st quantum number

3rd quantum number

electron orbital shapes 2nd quantum number
Electronorbitalshapes (2nd quantum number)

http://chemwiki.ucdavis.edu/Physical_Chemistry/Quantum_Mechanics/Atomic_Theory/Electrons_in_Atoms/Electronic_Orbitals

hybridization
Hybridization

atoms  circular electron shells 2,8,8,…orbitals s,p,d,f,…

  • s, p, d, f orbitals only for single atoms in gaseous state

 hybridization

  • electron orbitals change shape (and energy) during bonding
slide8
σ-bond
  • strongest form of covalent bond
  • orbitals overlap on line between nuclei
  • commonly s+s, pz+pz, s+pz

Image: http://en.wikipedia.org/wiki/Pi_bond

slide9
π-bond
  • orbital overlap not on line between nuclei
  • usually weaker than sigma bonds
  • stop rotation

Image: http://en.wikipedia.org/wiki/Pi_bond

orbital shapes of spdf orbitals and hybrid ized orbitals
Orbital shapes of spdf orbitals and hybrid ized orbitals

Image: http://en.wikipedia.org/wiki/Pi_bond

methane sp3 hybridization
Methane sp3 hybridization
  • 2s and 2p3 orbitals hybridize
carbon carbon bonds
Carbon-carbon bonds
  • Describe and explain the change in bond energy
  • Describe and explain the change in bond length
single bond ethane
Single bond (ethane)
  • one axial C-C s -Bond
  • Hybridisation: ones-orbital and three p-orbitals  four sp3-orbitals
  • The sp3-orbitals have a tetrahedral shape (109.5o).
double bond ethene
Double bond(ethene)
  • one axials -bond and one offset p-bond
  • Hybridisation: one s-orbital and two p-orbitals threesp2-orbitals
  • The sp2-orbitals have a trigonal planar shape, 120o
triple bond
Triple bond
  • One axial s -bond and two offset p -bonds
  • Hybridisation: One s-orbital and one p-orbital Two sp-orbitals
  • The sp-orbitals give a linear shape
the shape of the hybrids corresponds to the structure given by vsepr lewis structure
The shape of the hybrids corresponds to the structure given by VSEPR / Lewis structure.
  • Ethane : Ethene : Ethyne

sp3: sp2: sp

Ammonia: sp3

Water: sp3

benzene c 6 h 6 ring
Benzene, C6H6 ring

B

A

  • The p-bond in the double bond can switch place Electrons are delocalized.
  • A and B: resonance structures.
  • C: resonance hybrid. Molecule gains resonance energy by delocalizing electrons.

C

Image: http://commons.wikimedia.org/wiki/File:Benzene_resonance_structures.png

resonance bond
Resonance bond
  • Resonance describes delocalized electrons within some molecules or polyatomic ions where the bonding cannot be expressed by one single Lewis formula.
  • A molecule or ion with such delocalized electrons is represented by several resonance structures.

Draw the structures of NO3-, CO32-, O3