a) For the following molecule and ion AlCl3 and NH2
i. Draw the shape (showing the lone pair(s) and bond pair(s) of electrons)
ii. State bond angle(s)
iii. Give the overall polarity
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We have : Aluminium Chloride (AlCl3) and Amide ion (NH2) (-).
1) Aluminum Chloride :
Molecular geometry : Trigonal Planar.
Structure : Three Bonds each Al-Cl.
No lone pairs on Al. (central atom)
Amide ion : (NH2 )(-1)
Molecular Geometry : Bent / Angular.
2)
In AlCl3,
Bond Angle between each bonds is 120° .
In Amide, (NH2) (-))
Bond angle between two bond pairs is 104.5°.
3) Polarity will be such that partial negative charge is more stable on more electrinegative atom and vice -versa.
=>Cl has partial negative charge as its mire electronegative than Al.
=>H has partial positive charge as its more electropositive.
1) Aluminum Chloride :
Molecular geometry : Trigonal Planar.
Structure : Three Bonds each Al-Cl.
No lone pairs on Al. (central atom)
Amide ion : (NH2 )(-1)
Molecular Geometry : Bent / Angular.
2)
In AlCl3,
Bond Angle between each bonds is 120° .
In Amide, (NH2) (-))
Bond angle between two bond pairs is 104.5°.
3) Polarity will be such that partial negative charge is more stable on more electrinegative atom and vice -versa.
=>Cl has partial negative charge as its mire electronegative than Al.
=>H has partial positive charge as its more electropositive.
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Given molecule Here :- AlCl₃ & (NH₂)⁻
Now We have to find the shape,bond angle and polarity . So
The structure of AlCl₃ is Trigonal Planer & Hybridisation is SP₂.
The structure of NH₂⁻ is Bent , Also It has two Bond pair & two lone pair.
⇒(i) Here.Refer to the attachment for the diagrammatic structure for showing the lone pair & Bond pair of the electron.
(a) AlCl₃ . :- It doesn't have lone pair of electron & it is stable.
(b) NH₃⁻ :- It has two lone pair & also unstable.
⇒(ii) For Bond Angle :-
(a) AlCl₃ (Aluminium Trichloride) :- As we know , the structure of AlCl₃ is Trigonal Planer, The Bond angle bonded with 3 Chlorine atoms is 120°. Each chlorine atoms are sharing 1 pair of electron with Al for completing the valence shell.
(b) NH₂⁻ :- As the structure of NH₂⁻ is bent , Then the bond angle between two atoms is 104.5° .
⇒ (iii) Overall Polarity :-
(a) AlCl₃ :- We know the electronegativity of Aluminium is 1.61 and that of Chlorine is 3.16 . Thus electronegativity difference is 1.55 , This means that the shared pair of electron are tilted towards the chlorine atoms(Hence it Polar Compound). Thus a Dipole is created in which chlorine has the negative charge and Al has the positive .
(b) NH₂⁻ :- The NH₂⁻ is a polar compound because it Tends to attract the electron towards itself . This creates a negative charge on the compound.
Hope it Helps. :-)
Now We have to find the shape,bond angle and polarity . So
The structure of AlCl₃ is Trigonal Planer & Hybridisation is SP₂.
The structure of NH₂⁻ is Bent , Also It has two Bond pair & two lone pair.
⇒(i) Here.Refer to the attachment for the diagrammatic structure for showing the lone pair & Bond pair of the electron.
(a) AlCl₃ . :- It doesn't have lone pair of electron & it is stable.
(b) NH₃⁻ :- It has two lone pair & also unstable.
⇒(ii) For Bond Angle :-
(a) AlCl₃ (Aluminium Trichloride) :- As we know , the structure of AlCl₃ is Trigonal Planer, The Bond angle bonded with 3 Chlorine atoms is 120°. Each chlorine atoms are sharing 1 pair of electron with Al for completing the valence shell.
(b) NH₂⁻ :- As the structure of NH₂⁻ is bent , Then the bond angle between two atoms is 104.5° .
⇒ (iii) Overall Polarity :-
(a) AlCl₃ :- We know the electronegativity of Aluminium is 1.61 and that of Chlorine is 3.16 . Thus electronegativity difference is 1.55 , This means that the shared pair of electron are tilted towards the chlorine atoms(Hence it Polar Compound). Thus a Dipole is created in which chlorine has the negative charge and Al has the positive .
(b) NH₂⁻ :- The NH₂⁻ is a polar compound because it Tends to attract the electron towards itself . This creates a negative charge on the compound.
Hope it Helps. :-)
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