chemical bonding shape lab. 1)one structural isomer only
TRANSCRIPT
![Page 1: Chemical Bonding Shape Lab. 1)One structural isomer only](https://reader035.vdocuments.mx/reader035/viewer/2022081602/551acab0550346b2288b58c9/html5/thumbnails/1.jpg)
Chemical Bonding
Shape Lab
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1) One structural isomer only
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i) water, H2O
• shape: angular
O
H
H
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• END = O – H = 3.5 – 2.1 = 1.4• polar covalent bond
– bond dipoles exist, – molecule is asymmetrical– dipoles do not cancel– molecule is polar
O H
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ii) methane, CH4
C
H
H
H
H
C
H
H
H
H
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• Shape: Tetrahedral
• END = C – H = 2.5 – 2.1 = 0.4
• polar covalent bond
– bond dipoles exist, – molecule is symmetrical – the forces cancel– molecule is non-polar
C H
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iii) methanol, CH3OH
C
HO
H
H
HC
H
O
H
H
H
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• Shape: Tetrahedral about C Angular about O
• END = C – H = 2.5 – 2.1 = 0.4• END = C – O = 2.5 – 3.5 = 1.0• END = O – H = 3.5 – 2.1 = 1.4• all bonds are polar covalent
– bond dipoles exist– molecule is not symmetrical because different atoms
are bonded to the C and the O is angular– the forces do not cancel– molecule is polar
C H
O H
C O
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iv) carbon tetrachloride, CCl4
C
Cl
Cl Cl
Cl
C
Cl
Cl Cl
Cl
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• Shape: Tetrahedral
• END = C – Cl = 2.5 – 3.0 = 0.5
• polar covalent bond– bond dipoles exist– molecule is symmetrical– the forces cancel– molecule is non-polar
C Cl
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v) ammonia, NH3
NH
H
H
N
H H
H
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• Shape: Trigonal pyramidal
• END = N - H = 3.0 – 2.1 = 0.9
• polar covalent bond
– bond dipoles exist, – molecule is asymmetrical– dipoles do not cancel– molecule is polar
N H
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vi) hydrazine, N2H4
N
H
H
N H
H
N
H
H
N H
H
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• Shape: Trigonal pyramidal about each N• END = N - H = 3.0 – 2.1 = 0.9• END = N – N = 3.0 – 3.0 = 0.0• N – H is polar covalent bond• N – N is covalent bond
– bond dipoles exist, – molecule is asymmetrical– dipoles do not cancel– molecule is polar
N H
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vii) hydrogen sulfide, H2S
SH
H
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• Shape: Angular
• END = S – H = 2.5 – 2.1 = 0.4
• polar covalent bond
– bond dipoles exist, – molecule is asymmetrical– dipoles do not cancel– molecule is polar
S H
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viii) nitrogen triiodide, NI3
N
I
I
I
N
I
I
I
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• Shape: Trigonal pyramidal
• END = N - I = 3.0 – 2.5 = 0.4
• polar covalent bond
– bond dipoles exist, – molecule is asymmetrical– dipoles do not cancel– molecule is polar
N I
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ix) hydrogen peroxide, H2O2
O
OH H
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• Shape: Angular about each O
• END = O – H = 3.5 – 2.1 = 1.4
• polar covalent bond
– bond dipoles exist, – molecule is asymmetrical– dipoles do not cancel– molecule is polar
O H
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x) chlorine, Cl2
Cl
Cl
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• Shape: only 2 atoms (linear)• END: Cl – Cl = 3.0 – 3.0 = 0.0• covalent bond• no bond dipoles exist, so molecule is
non-polar
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2) Double and triple bonds
(use the springs)
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i) carbon dioxide, CO2
C
O
O
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• Shape: Linear (bonded to 2 atoms with no lone pairs)
• END = C – O = 2.5 – 3.5 = 1.0• END = C – C = 2.5 – 2.5 = 0.0• C – O is polar covalent bond
– bond dipoles exist– molecule is symmetrical– the forces cancel– molecule is non-polar
C O
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ii) nitrogen, N2
N
N
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• Shape: only 2 atoms (linear)• END: N – N = 3.0 – 3.0 = 0.0• covalent bond
– no bond dipoles exist– molecule is non-polar
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iii) oxygen, O2
O O
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• Shape: only 2 atoms• END: O – O = 3.5 – 3.5 = 0.0• covalent bond
– no bond dipoles exist– molecule is non-polar
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iv) ethyne, C2H2
C CH H
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• Shape: Linear (each C bonded to 2 atoms with no lone pairs)
• END = C – H = 2.5 – 2.1 = 0.4• END = C – C = 2.5 – 2.5 = 0.0• C – H is polar covalent bond, • C - C is covalent
– bond dipoles exist– molecule is symmetrical– the forces cancel– molecule is non-polar
C H
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v) hydrogen cyanide, HCN
C NH
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• Shape: Linear (C bonded to 2 atoms with no lone pairs)
• END = C – H = 2.5 – 2.1 = 0.4• END = C – N = 2.5 – 3.0 = 0.5• both are polar covalent bonds
– bond dipoles exist– molecule is symmetrical but the C is bonded to
2 different atoms– the forces do not cancel– molecule is polar
C H
C N
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vi) carbon disulfide, CS2
C SS
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• Shape: Linear (bonded to 2 atoms with no lone pairs)
• END = C – S = 2.5 – 2.5 = 0.0
• END = C – C = 2.5 – 2.5 = 0.0
• both are covalent bonds– no bond dipoles exist– molecule is non-polar
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vii) methanal, CH2O
CO
H
H
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• Shape: Trigonal planar (bonded to 3 atoms with no lone pairs)
• END = C – O = 2.5 – 3.5 = 1.0• END = C – H = 2.5 – 2.1 = 0.4• both are polar covalent bonds
– bond dipoles exist– molecule is symmetrical but the C is bonded to 2
different atoms– the forces do not cancel– molecule is polar
C H
C O
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viii) ethene, C2H4
C C
H
HH
H
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• Shape: Planar trigonal (each C bonded to 3 atoms with no lone pairs)
• END = C – H = 2.5 – 2.1 = 0.4• END = C – C = 2.5 – 2.5 = 0.0• C – H is polar covalent bond
– bond dipoles exist– molecule is symmetrical– the forces cancel– molecule is non-polar
C H
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3) Special Compounds
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i) beryllium hydride, BeH2
Be
H
H
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• Shape: Linear• END: Be – H = 1.5 – 2.1 = 0.6• polar covalent bond
– bond dipoles exist– molecule is symmetrical– the forces cancel– molecule is non-polar
Be H
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ii) boron trichloride, BCl3
B
Cl
Cl
Cl
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• Shape: Planar trigonal
• END: B – Cl = 2.0 – 3.0 = 1.0
• polar covalent bond– bond dipoles exist– molecule is symmetrical– the forces cancel– molecule is non-polar
B Cl
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iii) phosphorus pentabromide, PBr5
P
Br
Br
Br
Br
Br
P
Br
Br
Br
Br
Br
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• Shape: Trigonal bipyramidal
• END: P – Br = 2.1 – 2.8 = 0.7
• polar covalent bond– bond dipoles exist– molecule is symmetrical– the forces cancel– molecule is non-polar
P Br
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iv) sulfur hexachloride, SCl6
S
Cl
Cl
Cl
Cl
Cl
Cl
S
Cl
Cl
Cl
Cl
Cl
Cl
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• Shape: Octahedral
• END: S – Cl = 2.5 – 3.0 = 0.5
• polar covalent bond– bond dipoles exist– molecule is symmetrical– the forces cancel– molecule is non-polar
S Cl
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v) cyclohexane, C6H12
CC
C
CC
C
H
H
H
H
H
H
H
H
H
H
H
H
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• Shape: Tetrahedral about each C• END: C – H = 2.5 – 2.1 = 0.4• END: C – C = 2.5 – 2.5 = 0.0• C – H is polar covalent bond; C – C is
covalent– bond dipoles exist– molecule is symmetrical– the forces cancel– molecule is non-polar
C H
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vi) benzene, C6H6
CC
C
CC
C
H
H
H
H
H
H
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• Shape: Planar trigonal about each C (bonded to 3 atoms with no lone pairs)
• END: C – H = 2.5 – 2.1 = 0.4• END: C – C = 2.5 – 2.5 = 0.0• C – H is polar covalent bond; • C – C is covalent
– bond dipoles exist– molecule is symmetrical– the forces cancel– molecule is non-polar
C H