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Summary Chapter 14, Chemical Bonding & Structure (IB Chemistry) 2,99 €
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Summary Chapter 14, Chemical Bonding & Structure (IB Chemistry)
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  • Grado
  • Scheikunde
  • Nivel
  • VWO / Gymnasium
  • Book
  • IB Chemistry Course Book

This page mainly encompasses orbitals including pi & sigma bonds including how to identify then and their definitions. These notes also discuss formal charges, how to determine hybridisation (sp…), the shapes of molecules (mainly HL shapes), and reasons as structures.

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Información del documento

  • Desconocido
  • 14 de junio de 2024
  • 1
  • 2023/2024
  • Resumen

Temas

  • stochiometry
  • atomic structure
  • periodicity
  • chemical bonding
  • energetics
  • kinetics
  • acids bases
  • redox reactions
  • organic chemistry
  • medicinal chemistry
  • mass spectromet
  • equilibrium
  • measurement data processing

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Formals charge
Orbitals
• FC = valence electrons - 1/2 (number of bonding electrons) - (number of non bonding electrons)
• s= s orbital is closer to nucleus =



·
greater bond compared to p orbital • —> FC = V - 1/2 x B = N
• p= & • most preferred structure when formal charge is 0
• d=
• f =& Hybridization H
Cl Hy I
It - -s
294 sp3
↑ P




st
• 4 single bonds = sp^3 c = H C
J
H
C
• each atom that combine has an atomic orbital
-



p
- -
i


• 3 single bonds = sp^2
↓I I -
S
-
↳
-
P
> Oxygen has 2 lone pairs of
containing a single unpaired electron
• 2 single bonds = sp CI
C d Hip H3
electrons. This is also counted.

• when a covalent bond is formed, form a combined
CI Sp
orbital containing 2 electrons
• Consider double single bonds with hybridisation cause it is about s and p orbitals
• the greater the atomic over lap, the stronger the bonds
Shapes of Molecules 4

-bond Resonance structures Trigonal bipyramid
jop
.. 180
- CI
120
• bonding pairs = 5
• are formed from head to head (end to end) overlap to atomic orbitals F di
• lone pairs = 0
-




II
• a single covalent bond formed when 2 non-metals combine Species Resonance structure Hybrid


D&
• molecular geo = Trigonal bipyramid
&
-




• the electron density is concentrated between 2 nuclei Carbonate ions gi·
:
[o]"
Sp
Die
• s + s orbital & s + p-orbitals = sigma ortbial
di-
E > C


&
S
-




I+ &D
4) H CO is - - · • bonding pairs = 4 Fe
...... 2179
O
a-
.. :
-



S

-
Sp

• lone pairs = 1
&
-




• the electron density in a sigma bond is symmetrical about a line Benzene


•
joining in the nuclei of the atoms forming the bond
The electrostatic attraction between the electrons and nuclei bond
& • molecular geo = See saw

F
• bonding pairs = 3
the atom to each other Ozone
r I
...
↑
7
& F
• lone pairs = 2
-




D3 "
0..
.



F
-


• molecular geo = T- shape
Carbonylate ion
T -bonds
E m-
:




[
-




(RCOO )
&



c • bonding pairs = 2
R- -
m
• are formed from the sideways overlaps of adjacent orbitals -



r
o




• lone pairs = 3
r -

-




• the 2 lobes that make up the pi-bond lie above and below the plane
• molecular geo = linear
-




of a sigma bond
• this maximise overlap of p-orbitals
Octahedral
• a single pi-bond is drawn as 2 electron clouds, one arising from F


• bonding pairs = 6
F F

each lobe of p-orbitals
...........
S




·
• lone pairs = 0 #
#F
&
• p-orbital + p-orbital = pi bond if ‘lateral overlap’, from double bonds F
• molecular geo = Octahedral

O - ..... i ..... F
Ef • bonding pairs = 5
F
- c c
- plane
-
>
-

T
& • lone pairs = 1
I F>F S
S
-
-
e-cloud


• molecular geo = Square based planar

180
F
• bonding pairs = 4 ...-
F
Xe---
XX




• lone pairs = 2 F
/ 1 XX
-




• molecular geo = Square planar

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