Hydrolysis reactions (Inorganic reactions):

Hydrolysis is  a chemical process in which  a certain molecule is split into two parts by the addition of a molecule of water. One fragment of the parent molecule gains a hydrogen ion (H+) from the addition of water. The other group collects the remaining hydroxyl group(OH-) for examples :

(1) During  hydrolysis of a covalent compound having non metal central atom, if water molecule attack at central atom and hydrolysis occurs at room temperature then oxy acid of the non metal will be formed, if the central atom is in it one of the common oxidation state.  Oxidation state of  central atom of the oxy acid  will be same as its in the given substrate, However this rule is not applicable to XeF₂, XeF₄ and XeF₃.

(2) hydrolysis reactions occur in non redox reaction except XeF₂ and XeF₄ and  mixed anhydride i.e. central atoms has its uncommon oxidation state for examples;

(3) During  hydrolysis, hybridization of central atom in transition state and may  or may not change.

(4) BF₃, SiF₄, CCl₄, SbCl₃, and BiCl₃ undergo partial hydrolysis even in excess of water while PCl₅, SF₄, SeF₆,IF₇, XeF₆ H₄P₂O₈, H₂S₂O₈,P₄O₁₀ can undergo partial as well as complete hydrolysis by adjusting the amount water.

(5) Rate of hydrolysis is directly proportional to the positive (+) charge density at least electronegative atoms of  substrate provided. And  the least electronegative  atom must contain vacant  orbital and have no crowding.The order of  rate of hydrolysis of some compounds are given as;

PCl₅(V) > SiCl₄(IV) > AlCl₃(III) > MgCl₂(II) > CCl₄ (NO vacant orbital) > SF₆ (Crowding)

Related Questions:

Question (1): Why aqueous solution of AlCl₃ is acidic in nature?

Question (2): What happen when aq AlCl₃ react with Acid or Base?

Question (3): Although anhydrous aluminium chloride is covalent but its aqueous solution is ionic in nature. Why?

Question (4): Arrange in increasing order of extent of hydrolysis [ CCI₄, MgCI₂, AICI₃, PCl₅, SiCI₄].

Question (5): Although Sulphur contain vacant d-orbital but SF6 does not undergo hydrolysis. Why?

Question (6): CCl₄ can not be hydrolysed but SiCl4 can be. Why?

Question (7): What are the hydrolysis products of urea?

Question (8): Why SF₆ is inert where as SF₄ is highly reactive towards H₂0?.

Question (9): Why SF₆ behaves inert towards hydrolysis?

Question (10): Why PCl₃ hydrolysed while NCl₃ can not be hydrolysed?

Question (11): Why hydrolysis of NCl3 gives NH4OH and HOCl, while PCl3 on hydrolysis gives H3PO3 and HCl?

Question (12) NCl3 and PCl3 on hydrolysis give different kinds of products. These is because of

Which of the correct sequence of increasing order of pi bonds in the structure of the following {(I) H2S2O6 (II) H2SO3 (III) H2S2O5} molecules?

 

Related Questions:

What are the oxy-acids?

What are "pyro" oxy acids?

Oxy acids of Phosphorous:

What are "Ortho" or "Meta" oxyacids?

Why "meta" phosphoric acid always exit in a polymeric form?

What is structure of (HPO3) metaphosphoric acid?

Oxy acids of Chlorine:

What is structure and also explain the bridge bonding of I2Cl6 ?

I₂Cl₆ is  the dimer of ICl₃ which is dimerised  through (3C-4e-) bridge bonds. And it shape is rectangular planer and all the iodine as well as chlorine atoms lies in same plane. And (I-Cl-I) bridge bond have sp³d²-sp³-sp³d² hybridization.

Related Questions:

(1) What is the difference between the structure of AlCl3 and diborane?

(2) What is structural feature of monomeric and polymeric Beryllium halides ?

(3) What is bridge bond ? explaine 3C-4e bridge bond with suitable examples .

(4) What is structure of Beryllium chloride ?

(5) What is the structure of Aluminium tetrahydridoborate (Al(BH4)3) ?

(6) What is structure of Al(CH3)3 and also explain the bridge bonding in Al(CH3)3?

(7) The type of overlap in the bridge bond exist in Al2(CH3)6 is

(8) What is structure of diborane?

(9) What is structure of BeH2 in solid state ?

(10) Consider the structure of Al(CH3)3 given below and select the correct option?

(11) Consider Al2(OH)6 compound and calculate the value of (X+Y)/Z Where X= total number of two centre-two electrons (2C-2e) bond, Y= total number of three centre-two electron(3C-2e)bonds, and Z=total number of three centre-four electron (3C-4e) bond;

Wave mechanical concept of chemical bonding:

There are two important  theories which help the nature  of covalent bond on the basis of quantum mechanics:

(1) Valence bond theory (VBT)       (2) Molecular orbital theory (MOT)

(1) Valence bond theory (VBT):

(1) The valence bond theory given by Heitler and London to explain how to covalent bond form. And it is  extented by Pauling and Slater. 

(2) the main point of valence bond theory are given as:

(A) The covalent bond formed by overlapping of half filled orbitals of valence shell.

(B)The covalent bond requires a pair of electrons with opposite spins.

(C) The Atomic orbitals come closer to each other from the direction in which there is maximum overlapping, hence covalent has directional in nature.

(D)  The strength of covalent bond is directly proportional to extent of overlapping.

(E) The extent of overlapping depends on two factors like nature of orbitals and nature of overlapping

(1) S-orbital is non directional- less overlapping extent while p,d,f are directional orbitals hence more overlapping extent.

(2) Co-axial overlapping – extent of overlapping is more while in collateral overlapping – extent of overlapping  is less. The order of strength of co-axial overlapping is : P-P > S-P > S-S

(3) As the value of principle  quantum number(n) increases the strength decreases: 1-1 > 1-2 > 2-2 > 2-3 > 3-3

(4) If the value of value of principle  quantum number(n) is same then bond strength order follow as:

                         2p-2p > 2s-2p >2s-2s

                         1s-2p > 2s-2p > 3s-3p

(5) The electron which is already paired in valency shell can enter into bond formation, it they can be unpaired  first and shift to vacant orbitals of slightly higher energy of same energy shell, this point can explain the trivalency of boron, tetravalency of carbon, penta-valency of phosphorous etc.

(6) There are  two type of covalent bonds on basis of way of overlapping.

(A) Sigma bond  (B)   Pi bond

What is Sigma Bond ?

What is Pi-(π)Bond ?

Why the extent of overlap is more in 2p-3d than 2p-3p?

 Related Questions: 

(1) Why aqueous solution of AlCl3 is acidic in nature ?

(2) What happen when aq AlCl3 react with Acid or Base?

(3) Although anhydrous aluminium chloride is covalent but its aqueous solution is ionic in nature. Why?

(4) Why BF3 do not exist as dimer?. Explain.

(5) Why B-F bond length in BF3 is shorter (130 pm) than B-F bond Iength in BF4- (143 pm)?. Explain.

(6) B-F bond length in BF3 is shorter than B-F bond length in (BF4)- why?

(7) When B2H6 is allowed to react with following Lewis bases, then how may given Lewis base form adduct through symmetrical Cleavage of B2H6.

(8) What is product of reaction between diborane (B2H6) and ammmonia (NH3)?

(9) Why methylation of Diborane (B2H6) replace four hydrogen only ?

(10) What is Use of Boric Acid?

(11) What is use of Orthoboric acids?

(12) What is basicity of "Boric acid" ?

(13) Why Boric acid exist in solid state ?

(14) What is structure of solid Ortho Boric acid ?

(15) What is effect of heat on Borax?

(16) What is the structure of trimetaboric acid and trimetaborate ion?

(17) What is the Sodium per borate ,give the structure and its uses?

(18) Why aqueous solution of borax reacts with two moles of acids ?

(19) What is the molecular formula of Borax ?

(20) Why Boric acid become strong acid in the presence of cis 1,2-diol or 1,3-diol ?

(21) Why Borazine is more reactive than benzene towards Electrophic Aromatic substitution reactions ?

(22) Why Borazine (B3N3H6) is also known as inorganic benzene ?.

The type of overlap in the bridge bond exist in Al2(CH3)6 is

(A) sp3-sp3d-sp3

(B) sp3-sp2-sp3

(C) sp3-s-sp3

(D) sp3-sp3-sp3

Solution: Structure of Al2(CH3)6:

 Answer Key (D)

Related Questions:

(1) What is structure of diborane?

(2) What is structure of Al(CH3)3 and also explain the bridge bonding in Al(CH3)3?

(3) What is bridge bond ? explaine 3C-4e bridge bond with suitable examples .

(4) What is structural feature of monomeric and polymeric Beryllium halides ?

(5) What is the difference between the structure of AlCl3 and diborane?

(6) What is structure of Beryllium chloride ?

(7) What is structure of BeH2 in solid state ?

Which of the molecule have strongest P=O bond present the given molecules are POF3, POCl3, POBr3 and PO(CH3)3 ?

All the given molecules have same hybridization (sp3) and same central atom (P) the we can apply Bent's rule of hybridization. And according to Bent’s rule more electronegative atoms attach in those hybrid orbital’s which have less s-character or more electronegative atoms decreases s-character and increases p-character.

In case of POF₃  fluorine is more electronegative hence s-character  is increase more and more in P=O bond  as compare to other given molecules so P=O bond is shortest in POF₃  than others and also increase with decreasing electronegativity.  Hence P=O bond length order is x₁ < x₂ < x₃ < x₄  and Bond strength order is reverse of bond length.

Related Questions:

What is Bent’s rule of hybridization?

Which of the following compound have longest (S=O)bond length , O=SF2, O=SCl2, O=SBr2.

Why Bond length of O-O is greater in H2O2 than O2F2?

How to arrange increasing (C-H) bond length in increasing order and H-C-F bond angle in the given compounds, CH4, CH3F, CH2F2 and CHF3 ?

Dipole moment of PCl3F2 molecule is zero while dipole moment of PCl2F3 molecule is non zero why?

Dipole moment of P(CH3)2(CF3)2 molecule is zero while dipole moment of P(CH3)2(CF)3 molecule is non zero why?

How to compare equatorial bond angle (F-S-F) and S-F bond length of SOF4 and SF4 molecules ?

How to compare P=O bond length of POF3, POCl3, POBr3 and PO(CH3)3 molecules?

How to compare P=O bond length of POF3, POCl3, POBr3 and PO(CH3)3 molecules?

All the given molecules have same hybridization (sp3) and same central atom (P) the we can apply Bent’s rule of hybridization. And according to Bent’s rule more electronegative atoms attach in those hybrid orbital’s which have less s-character or more electronegative atoms decreases s-character and increases p-character.

In case of POF₃  fluorine is more electronegative hence s-character  is increase more and more in P=O bond  as compare to other given molecules so P=O bond is shortest in POF₃  than others and also increase with decreasing electronegativity.  Hence P=O bond length order is x₁ < x₂ < x₃ < x₄

Related Questions:

What is Bent’s rule of hybridization?

Which of the following compound have longest (S=O)bond length , O=SF2, O=SCl2, O=SBr2.

Why Bond length of O-O is greater in H2O2 than O2F2?

How to arrange increasing (C-H) bond length in increasing order and H-C-F bond angle in the given compounds, CH4, CH3F, CH2F2 and CHF3 ?

Dipole moment of PCl3F2 molecule is zero while dipole moment of PCl2F3 molecule is non zero why?

Dipole moment of P(CH3)2(CF3)2 molecule is zero while dipole moment of P(CH3)2(CF)3 molecule is non zero why?

How to compare equatorial bond angle (F-S-F) and S-F bond length of SOF4 and SF4 molecules ?

How to compare equatorial bond angle (F-S-F) and S-F bond length of SOF4 and SF4 molecules ?

According to Bent's rule lone pair containing hybrid orbital have more s-character than double bond. 

In case of SF4 molecule has sp3d hybridization and one of the equatorial hybrid orbital containing lone pair it means it has more s-character and less p-character while  other remaining  equatorial hybrid orbitals have less s-character and more p-character hence its bond angle decreases and bond length increases.

Related Questions:

What is Bent’s rule of hybridization?

Which of the following compound have longest (S=O)bond length , O=SF2, O=SCl2, O=SBr2.

Why Bond length of O-O is greater in H2O2 than O2F2?

How to arrange increasing (C-H) bond length in increasing order and H-C-F bond angle in the given compounds, CH4, CH3F, CH2F2 and CHF3 ?

Dipole moment of PCl3F2 molecule is zero while dipole moment of PCl2F3 molecule is non zero why?

Dipole moment of P(CH3)2(CF3)2 molecule is zero while dipole moment of P(CH3)2(CF)3 molecule is non zero why?

 

Dipole moment of P(CH3)2(CF3)2 molecule is zero while dipole moment of P(CH3)2(CF)3 molecule is non zero why?

 According to bent’s rule more electronegative atom or group attached those hybrids orbital have minimum s-character.

There is sp3d (Sp2+pd) hybridization trigonal bipiramidal(TBP) geometry in P(CH₃)₂(CF₃)₂ molecule. we known that axial orbital (pd) have no s-character so –CF₃  groups are attached with axial positions while –CH₃ groups attach with equatorial (Sp2) position. Hence net dipole moment becomes zero. While in case of P(CH₃)₂(CF)₃ molecule one of the –CF₃ group is also present at equatorial position hence there is net dipole moment.

Related Questions:

What is Bent’s rule of hybridization?

Which of the following compound have longest (S=O)bond length , O=SF2, O=SCl2, O=SBr2.

Why Bond length of O-O is greater in H2O2 than O2F2?

How to arrange increasing (C-H) bond length in increasing order and H-C-F bond angle in the given compounds, CH4, CH3F, CH2F2 and CHF3 ?

Dipole moment of PCl3F2 molecule is zero while dipole moment of PCl2F3 molecule is non zero why?

According to bent’s rule more electronegative atom or group attached those hybrids orbital have minimum s-character.

There is sp3d (Sp2+pd) hybridization trigonal bipiramidal(TBP) geometry in PCl₃F₂ molecule. we known that axial orbital (pd) have no s-character so F  atoms are attached with axial positions while chlorine atoms attach with equatorial (Sp2) position. Hence net dipole moment becomes zero. While in case of PCl₂F₃ one of the fluorine atom is also present at equatorial position hence there is net dipole moment.

Related Questions:

What is Bent’s rule of hybridization?

Which of the following compound have longest (S=O)bond length , O=SF2, O=SCl2, O=SBr2.

Why Bond length of O-O is greater in H2O2 than O2F2?

How to arrange increasing (C-H) bond length in increasing order and H-C-F bond angle in the given compounds, CH4, CH3F, CH2F2 and CHF3 ?

Consider Al2(OH)6 compound and calculate the value of (X+Y)/Z Where X= total number of two centre-two electrons (2C-2e) bond, Y= total number of three centre-two electron(3C-2e)bonds, and Z=total number of three centre-four electron (3C-4e) bond;

 

Total number of two centre-two electrons (2C-2e) bonds(X)=6

Total number of three centre-two electron(3C-2e) bonds(Y)=4

Total number of three centre-four electron (3C-4e) bond(Z)=2

Hence (X+Y)/Z=(6+4)/2=5

Related Questions:

(1) What is the difference between the structure of AlCl3 and diborane?

(2) What is structural feature of monomeric and polymeric Beryllium halides ?

(3) What is bridge bond ? explaine 3C-4e bridge bond with suitable examples .

(4) What is structure of Beryllium chloride ?

(5) What is the structure of Aluminium tetrahydridoborate (Al(BH4)3) ?

(6) What is structure of Al(CH3)3 and also explain the bridge bonding in Al(CH3)3?

(7) The type of overlap in the bridge bond exist in Al2(CH3)6 is

(8) What is structure of diborane?

(9) What is structure of BeH2 in solid state ?

(10) Consider the structure of Al(CH3)3 given below and select the correct option?

(11) Consider Al2(OH)6 compound and calculate the value of (X+Y)/Z Where X= total number of two centre-two electrons (2C-2e) bond, Y= total number of three centre-two electron(3C-2e)bonds, and Z=total number of three centre-four electron (3C-4e) bond;