What are the hybridixation and shape of I3- and I3+ PolyIodide ions!

I3- ion has sp3d hybridization and linear shape containing two bond pair and three lone pair while I3+ ion has sp3 hybridization and bent shape containing two bond pair and two lone pair.

Related Questions: 

Why aqueous solution of AlCl3 is acidic in nature ?

What happen when aq AlCl3 react with Acid or Base?

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

Why BF3 do not exist as dimer?. Explain.

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

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

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

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

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

What is Use of Boric Acid?

What is use of Orthoboric acids?

What is basicity of "Boric acid" ?

Why Boric acid exist in solid state ?

What is structure of solid Ortho Boric acid ?

What is effect of heat on Borax?

What is the structure of trimetaboric acid and trimetaborate ion?

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

Why aqueous solution of borax reacts with two moles of acids ?

What is the molecular formula of Borax ?

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

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

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

Both CO2 and N2O are linear but dipole moment of CO2 is zero but for N2O it is non-zero, why?

The answer lies in the structure of these molecules, CO₂ is symmetrical molecule while N₂O is unsymmetrical, thus for N₂O, dipoles do not cancel each other, leaving the molecule with a resultant dipole, while the bond moment of CO₂ cancel each other, so CO₂ has no net dipole moment.

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 behave 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

What is hydrolysis product of BeCl2 with excess water at room temperature?

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;

What is structure of Al2Cl6 and also explain bridge bond in Al2Cl6?

AlCl₃ dimmerised to Al₂Cl₆ by 3C-4e bond bridge bond and Al₂Cl₆ is neither hypovalent nor hypovalent rather its octet is complete. Al₂Cl₆ contains six bond having two bridge bond(3c-4e) and four bond is (2C-2e).

We will used  MOT here  it cannot act as Lewis acid  due to crowding in spite having vacant d orbital’s however AlCl₃ act as Lewis acid.

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 ?.

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;

Consider the structure of Al2(CH3)3 given below and select the correct option?

(A) x < y

(B) alpha < Beta

(C) Bridge bond is formed by sp3-sp3-sp3 overlap.

(D) All of the correct.

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 ?

What is structure of BeH2 in solid state ?

BeH₂ is covalent hydride and having polymeric structure in solid state in which beryllium atoms are bonded together by three centre-two electrons(3c-2e) bridge bond which also know as banana bond and all the H-Be-H bond angle are below 109.28’

But in gaseous BeH₂ exist in dimeric form in which Be atoms are sp2 hybridised, planer  and non polar(dipole moment zero).

Related Questions:

What is structure of diborane?

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

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

What is structural feature of monomeric and polymeric Beryllium halides ?

What is the difference between the structure of AlCl3 and diborane?

What is structure of Beryllium chloride ?

What is structure of diborane?

(1)  B₂H₆ contains 4-Terminal H are bonded by Sigma bond and  remaining 2-H are bridging hydrogen's and of these are broken then dimer become monomer.

(2) Boron undergoes sp3 hybridisation 3 of its sp³ hybridised orbitals contain one( e¯) each and fourth sp³ hybrid orbital is vacant.

(3) 3-(Three) of these sp³ hybrid orbitals get overlapped by s orbitals of 3-hydrogen atoms.

(4) One of the sp3 hybrid orbitals which have been overlapped by s orbital of hydrogen gets overlapped by vacant sp³ hybrid orbital. Of 2^nd Boron atom. And it's vice versa.

(5) By this two types of overlapping take place 4 (sp3– s) overlap bonds and 2(sp² – s – sp³) overlap bonds.

(6) H is held in this bond by forces of attraction from B and This bond is called 3 centred two electron bonds (3C-2e bond) . Also called Banana bonds. Due to repulsion between the two hydrogen nuclei, the delocalised orbitals of bridges are bent away from each other on the middle giving the shape of banana.

(7) The two bridging hydrogens are in a plane and perpendicular to the rest four hydrogen atoms.

ILLUSTRATED EXAMPLE (1): In Diborane

(A) 4 bridged hydrogens and two terminal hydrogen are present

(B) 2 bridged hydrogens and four terminal hydrogen are present

(C) 3 bridged and three terminal hydrogen are present

(D)None of the above

 

ILLUSTRATED EXAMPLE (2): Which one of the following statements is not true regarding diborane?

(A) It has two bridging hydrogens and four perpendicular to the rest.

(B) When methylated, the product is Me₄B₂H₂.

(C) The bridging hydrogens are in a plane and perpendicular to the rest.

(D ) All the B–H bond distances are equal

 

ILLUSTRATED EXAMPLE (3): The structure of diborane (B₂H₆) contains

(A) Four (2C–2e–) bonds and two (2C–3e–) bonds

(B) Two (2C–2e–) bonds and two (3C–2e–) bonds

(C) Four (2C–2e–) bonds and four (3C– 2e–) bonds

(D ) None of these

ILLUSTRATED EXAMPLE (4): The molecular shapes  of diborane is shown:

Consider the following statements for diborane:

1. Boron is approximately sp3 hybridised

2. B–H–Bangle is 180°

3. There are two terminal B–H bonds for each boron atom

4. There are only 12 bonding electrons available

Of these statements:

(A ) 1, 3 and 4 are correct                  (B) 1, 2 and 3 are correct

(C) 2, 3 and 4 are correct                    (D) 1, 2 and 4 are correct