Susanta Maity

Hi....I am Susanta Maity. I have completed my Masters from Vidyasagar university with a specialization in organic chemistry. I love to write complicated Chemistry concepts in understandable and simple words. Let's connect through LinkedIn:

O2 Bond Order: 7 Facts Beginners Should Know !

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In this article we find out O2 bond order and 7 facts regarding this.

The O2 molecule composed of 2 O atom. O atom has electronic configuration 1s22s22p4.Each O atom contains a total number of 8 electrons i.e. the whole O2 molecule contain a total number of 16 electrons. When atomic orbitals of O atom are mixed to form O2 molecule the energies of atomic orbitals changes i.e. some goes to higher energy level and some goes to lower energy level.

O2 bond order diagram

When 2 O atoms are engaged in forming O2 molecule, the atomic orbitals of O atom is also involved in the formation of O2 molecule. The total number of atomic orbital of O atom involved in forming O2 molecular diagram is 10 i.e. 5 atomic orbitals from each O atom.

These atomic orbitals are 1s,2s and 2p orbitals. 1s and 2s has only 1 orbit but 2p has 3 orbits. We see that there are a total of 10 atomic orbitals involved in O2 bond order diagram, hence molecular orbital also formed in the same number i.e. 10.

o2 bond order
O2 bond order diagram

Molecular orbital diagram O2 bond order

At first, 1s orbital of both O atom are mixed to form 1 bonding MO i.e. σ1s and 1 antibonding MO i.e. σ1s* .Both molecular orbitals contains 2 electrons. σ1s bonding MO is lower in energy and σ1s* MO is higher in energy. Then 2s orbitals of each O atoms are coupled to form 1 σ2s bonding MO and 1 σ2s* antibonding MO. Similarly σ2s which is always lower in energy and σ2s* is always higher in energy. 

.When 2p orbitals of each O atom are combined total 6 MO’s are formed, each 2p subshell contain 3 atomic orbitals i.e. 2px , 2py , 2pz . one 2px orbital of each O atom combined to form 1 σ2px , and 1 σ2px* MO. σ2px is bonding in nature and σ2px* MO is antibonding in nature. Out of these 2 MO only bonding σ2px MO is filled with 2 electrons but antibonding σ2px* MO remains vacant.

Then 2py and 2pz atomic orbitals of each O atom mixed together to form 4 MO’s. out of which 2 are ∏2py and ∏2pz and their corresponding antibonding MO’s i.e. ∏2py* and ∏2pz* . ∏2py and ∏2pz MO’s each contain 2 electrons making a total of 4 electrons in ∏ MO’s. ∏2py* and ∏2pz* each contain 1 electron making a total of 2 electrons in ∏*Mo’s.

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Molecular orbital diagram of O2

Mot O2 bond order

The formula through which bond order is calculated is given below:

Bond Order= (Total no of electrons in bonding Mo-Total no of electrons in antibonding MO)/2 .

Total no of electrons in bonding MO of O2 molecule= 10.

Total no of electrons in antibonding MO of O2 molecule= 6.

Bond order of O2 molecule= 10-6/2= 2.

Hence one σ bond and 1 ∏ bond is formed between 2 O atom.

Bond order of O22-

When 2 electrons are added in O2 molecule O22- ion is formed. This is known as peroxide ion. These 2 electrons are added 1 electron each in higher energy ∏2py* and ∏2pz* MO’s. By the addition of these 2 electrons O22- ion contains a total of 18 electrons. These 18 electrons are filled similar way as in O2 with extra 2 electrons in ∏2py* and ∏2pz* MO’s.

The bond order of O22- ion is calculated by the above mentioned formula.

Total no of electrons in bonding MO of O22- ion=10.

Total no of electrons in antibonding MO of O22- ion=8.

Bond order of O22- ion= 10-8/2=1.

Hence there is only 1 bond which is σ bond is formed in O22- ion.

Covalent bond in O2 molecule

From O2 bond order diagram we see that there 2 covalent bonds between 2 O atoms. Hence 1 σ bond and 1 ∏ bond is formed between 2 O atoms. These 2 covalent bonds contains a total of 4 electrons.

The σ bond is formed by overlap of 2px  orbital of each O atom and the ∏ bond is formed by the overlap of either 2py and 2pz orbitals of each O atom. The ∏ bond is higher in energy as well as weakly bonded than σ bond.

How to find O2 bond order?

To find out O2 bond order we can use the following formula,

Bond Order= (Total no of electrons in bonding MO-Total no of electrons in antibonding MO)/2 .

Total no of electrons in bonding MO of O2 molecule= 10.

Total no of electrons in antibonding MO of O2 molecule= 6.

Bond order of O2 molecule= 10-6/2= 2.

How many orbitals are singly occupied in O2?

When atomic orbitals of O atom are mixed to form O2 molecule the energies of atomic orbitals changes i.e. some goes to higher energy level and some goes to lower energy level. Higher energy orbitals are unstable in nature where as lower energy orbitals are stable. When we see the O2 bond order diagram, all the MO’s are fulfilled expect ∏2py* and ∏2pz* MO’s which are singly occupied.

Conclusion

From O2 bond order diagram we see that the bond order in O2 molecule is 2 i.e. 1 sigma bond and 1 pi bond is formed and in O22- ion the bond order is 1. Hence from bond order we see that O2 molecule is more stable than O22- ion.

5 Cis Trans Isomers Example:With Deatiled Facts

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Cis-trans isomers are those isomers which have same molecular formula but have different orientation of functional groups in 3D space. In Cis isomer functional group are on the same side of the double bond while in trans isomer they are on the opposite side of the double bond. Cis trans isomers example are a part of structural isomer.

But-2-ene

But-2-ene shows cis-trans isomerism. It’s cis trans isomers example are cis-2-butene and the other is trans-2-butene. In cis-2-butene 2 methyl group is situated on the same side of the double bond while in trans isomer 2 Me group is on opposite position with respect to double bond. But in both isomer 2 methyl groups are attached to sp2 hybridized C atom but not in same C atom.

As cis-2-butene is polar in nature (because,µ≠0) its boiling point is higher than trans-2-butene which is non-polar in nature (µ=0). Also trans isomer has more symmetrical structure than cis isomer, trans-2-butene has higher melting point than cis-2-butene. In terms of stability trans-2-butene is more stable than cis-2-butene due to the fact that in cis isomer there occurs steric crowding between 2 bulky Me groups.

cis trans isomers example
Cis-trans isomers of But-2-ene

Pent-2-ene

Pent-2-ene shows cis-trans isomerism. It’s cis trans isomers example are cis-2-pentene and the other is trans-2-pentene. In cis isomer Me and Et group is situated on the same side of the double bond while in trans isomer these 2 groups is on opposite position of the double bond. In cis isomer as sp2 hybridized carbon is more electronegative than sp3 hybridized C atom, sp2C-sp3Me bond moment lies towards sp2C and also sp2C-SP3Et bond moment lies towards sp2C.

But in case of trans-2-pentene Me and Et groups is on opposite side of the double bond and these 2 bond moment lies in same direction and cancel each other. Hence its dipole moment is 0. As cis-2-pentene is polar in nature, its boiling point is higher than trans-2-pentene which is non-polar in nature(µ=0). Also trans isomer has more symmetrical structure than cis isomer, trans-2-pentene has higher melting point than cis-2-pentene.

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Cis-trans isomers of Pent-2-ene

Diazene

Diazene also shows cis-trans isomerism. In cis-diazene 2 lone pair and 2 H atoms are on the same side of the double bond while in trans isomer these are on the opposite direction to each other with respect to double bond. These 2 isomer can be differentiate from each other by their reactivity.

. Cis-diazene is much more reactive than trans diazene due to repulsion between 2 lone pair in cis-diazene increases the lone pair availability towards an alkene. For the same reason cis isomer is less stable than trans isomer. Cis-diazene is more polar than trans-diazene as because 2N-H bond moment lies in the same direction which is in opposite direction in case of trans-diazene making it a non-polar compound.

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Cis-trans isomers of Diazene

Hex-3-ene

Hex-2-ene shows cis-trans isomerism. It’s cis trans isomers example are cis-Hex-3-ene and the other is trans-Hex-3-ene. In cis-isomer 2 ethyl group is situated on the same side of the double bond while in trans isomer 2 Et group is on opposite side Of double bond. In cis isomer as sp2 C is more electronegative than sp3 hybridized Me group, 2 sp2C-sp3C bond moment lies towards sp2C i.e. its overall dipole moment is high. But in trans isomer 2 Et group is on opposite side 2 sp2C-sp3C bond moment lies in same direction and cancel each other. Hence its dipole moment is 0.

As cis-Hex-3-ene polar in nature(because,µ≠0) its boiling point is higher than trans-Hex-3-ene which is non-polar in nature(µ=0). Also trans isomer has more symmetrical structure than cis isomer, trans-Hex-3-ene has higher melting point than cis-Hex-3-ene. In terms of stability trans-Hex-3-ene is more stable than cis-Hex-3-ene due to the fact that in cis isomer there occurs steric crowding between 2 bulky Et groups.

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Cis-trans isomers of Hex-3-ene

1,2-dibromoethene

1,2-dibromoethene shows cis-trans isomerism. It’s cis trans isomers example are cis-1,2-dibromoethene and the other is trans-1,2-dibromoethene. In cis isomer 2 Br group is situated on the same side of the double bond while in trans isomer 2 Br group is on opposite position with respect to double bond. In terms of stability trans isomer is more stable than cis isomer due to the fact that in cis isomer there occurs steric crowding between 2 bulky Br  groups.

.In cis isomer as 2 Br group is on the same side of the double bond, 2 C-Br bond moment lies towards Br group i.e. its dipole moment is high. But in trans isomer 2 C-Br bond moment lies in same direction and cancel each other. Hence its dipole moment is 0. As cis isomer is polar in nature, its boiling point is higher than trans isomer which is non-polar in nature. Also trans isomer has more symmetrical structure than cis isomer, trans isomer has higher melting point than cis isomer.

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Cis-trans isomers of 1,2-Dibromoethene

7 Functional Isomers Example:With Deatiled Facts

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In this article we want to discuss things related functional isomers example with detailed facts as well.

Isomers are a type of compounds which possess same molecular formula but distribution of atoms are different in space. . Functional isomer is those organic as well as inorganic compound which possess same formula but have different functional group in them. Functional isomer is a part of structural isomer.

Functional isomers example are given below:

C2H6O

C2H6O has two functional isomers example. One is di-methyl ether (CH3OCH3) and other is ethanol (CH3CH2OH). In di-methyl ether the functional group is ether i.e. -C-O-C- linkage. Di-methyl ether also known as methoxymethane. In ethanol the functional group is hydroxyl group i.e. –OH group.

As two isomer differ in their boiling point these 2 isomer can be distinguished easily. Due to presence of OH group in ethanol there occurs intermolecular H bonding between the molecules of ethanol. To separate them large amount of energy is required for this it has high boiling point.

But in case of dimethyl ether due to absence of OH group no H bonding takes place between them so that it has lower boiling point. As ethanol is more polar than dimethyl ether, these 2 isomer are identified by their polarity. Also ethanol is capable of forming intermolecular H bonding with H2O molecule it is soluble in water but dimethyl ether can’t form H bonding with water. It is less soluble in water.

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Functional isomer of C2H6O

C3H6O

C3H6O has two functional isomers example. One is propanal (CH3CH2CHO) and the other is propanone (CH3COCH3). In propanal the functional group is –CHO i.e. aldehyde and in propanone the functional group is –CO i.e. ketone. Propanal and propanone can be differentiate from each other by a chemical reaction named haloform reaction.

when both the compound are reacted with NaOH and I2 due to presence of α-H atom in propanone it gives the yellow precipitate of CHI3 but propanal does not give this test due to the absence of α- H atom. Nucleophilic addition reaction is fast with propanal than propanone due to steric as well electronic factor.

Carbonyl carbon is less sterically hindered and more electrophilic in propanal than propanone. Propanone has higher boiling point than propanone because in propanone the carbonyl group is more polarized than that of propanal. For this dipole-dipole force of attraction is higher in propanone than propanal and boiling point is higher in propanone than propanal.

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Functional isomer of C3H6O

C2H4O2

C2H4O2 has two functional isomers example. One is acetic acid (CH3COOH) and the other is methyl formate (HCOOCH3). In acetic acid the functional group is acid i.e. –COOH group. In methyl formate the functional isomer is ester i.e. –COOR group.

Both isomer have same molecular formula but different functional group and have different physical and chemical properties. By their boiling point these 2 isomer can be separated from each other . Acetic acid has higher boiling point than methyl formate because in acetic acid there occurs intramolecular H bonding which does not occur in methyl formate due to absence of –OH group.

For that reason to separate acetic acid molecule from each other large amount of energy is required. If both the isomer are reacted with NaHCO3 in presence of small amount of heat the isomer in which we see the effervescence of CO2 gas is acetic acid. By this chemical method we can distinguish between an acid and an ester.

They can also be differentiating by their dipole moment values. Acetic acid has higher dipole moment value than methyl formate. For this higher polarity of acetic acid it is more soluble in water than methyl formate.

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Functional isomer of C2H4O2

C3H9N

C3H9N exist in 3 functional isomers example. These are propan-1-amine (CH3CH2CH2NH2), N-methyl ethanamine (CH3CH2NHCH3), N,N- dimethyl methanamine [(CH3)3N]. Propane-1-amine is 10 amine, N-methyl ethanamine is 20 amine, N,N-dimethyl methanamine is 30 amine. All these have same molecular formula but have different functional groups.

These three amines are differentiating from each other by Hinsberg’s reagent. When reacts with hinsberg’s reagent propan-1-amine give a sulphonamide which is readily soluble in alkali. N-methyl ethanamine also give a sulphonamide which is insoluble in nature. But N,N-dimethyl methanamine does not give this test due to absence of H atom on N atom, it can’t be neutralized further.

They can also be distinguished by their boiling point. The boiling point order is: propan-1-amine>N-methyl ethanamine>N,N –dimethyl methanamine. Also their solubility is different in water. Propan-1-amine is highly soluble in nature and N,N-dimethyl Methanamine is least soluble in water and 20 amine lies between them.

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Functional isomer of C3H9N

C4H10O

C4H10O exist in two functional isomers example. One is butan-1-ol (CH3CH2CH2CH2OH)and the other is ethoxyethane (CH3CH2OCH2CH3). In butan-1-ol the functional group is –OH group and in ethoxyethane the functional group is ether i.e. –C-O-C- linkage.

These two isomer can be isolated from each other by the difference in their boiling point. Due to presence of –OH group there occurs intermolecular H bonding between the molecules of butan-1-ol. As to separate them from each other large amount of energy is required.

For this reason it has higher boilling point than ethoxyethane where no H bonding occurs due to absence of –OH group. By reacted the two isomer with PCl5 butan-1-ol gives the precipitate of alkyl chloride whereas ether does not give the same. By this chemical method we also differentiate these 2 isomer.

Also butan-1-ol is soluble in water where as  ethoxyethane is insoluble in water. As because butan-1-ol forms H bonding with water but ethoxyethane does not.

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Functional isomer of C4H10O

C4H8O2

C4H8O2 has 2 functional isomers example. One is butanoic acid (CH3CH2CH2COOH) and the other is methyl propionate (CH3CH2COOCH3). In butanoic acid the functional group is acid i.e. –COOH group and methyl propionate has functional group ester i.e. –COOR group.

As their boiling point is different 2 isomers can be distinguished separately. Butanoic acid has higher boiling point than methyl propionate. This is due to the presence of intramolecular H bonding in former compound which does not arises in case of latter compound due to absence of –OH group.

That is why to separate the molecules of butanoic acid large amount of energy is required so that it has higher boiling point than methyl propionate. when 2 isomers are reacted with NaHCO3 in heat butanoic acid gives the effervescence of CO2 gas but methyl propionate does not give this test.

By this chemical method we can distinguish an acid and an ester. Butanoic acid has higher boiling point than methyl propionate due to the higher polarity of acid than ester.

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Functional isomer of C4H8O2

C4H8O

C4H8O has 2 functional isomers example. One is butanal (CH3CH2CH2CHO)and the other is butanone (CH3COCH2CH3). In butanal the functional group is –CHO i.e. aldehyde and butanone has ketonic functional group i.e. –CO.

These 2 functional isomers can be differentiate from each other by a chemical reaction named haloform reaction. When both the isomers are reacted with NaOH and I2 due to presence of α-H atom butanone gives yellow precipitate of CHI3 but butanal does not give this test due to absence of α-H atom.

Nucleophilic addition reaction occurs at a faster rate in butanal due to steric as well as electronic factor. Carbonyl carbon is less sterically hindered and more electrophilic in butanal than butanone. Butanone has higher boiling point than butanal because in butanone the carbonyl group is more polarized than that of butanal.

For this dipole-dipole force of attraction is higher in butanone than butanal and boiling point is higher in butanone than butanal.

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Functional isomer of C4H8O

5 Chain Isomers Example:With Deatiled Facts

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In this article we want to discuss things related chain isomer example with detailed facts as well.

Isomers are those compounds which have same molecular formula but arrangement of atoms is different in space. There are various types of isomer exist in chemistry out of those chain isomer is an important one. There are some compounds which have same molecular formula but arrangement of carbon atoms are different in chains defined as chain isomers.

Chain isomers example are given below:

n-butane

n-butane has molecular formula C4H10. It’s 2 chain isomers examples are one is n-butane which is a straight chain compound and the other one is 2-Methyl Propane which is branched chain compound. In n-butane there are 4 C atoms which are arranged in a straight chain and each C atom is sp3 hybridized.

In 2-Methyl Propane there are also 4 C atoms out of which 3 are in single straight chain and 1 is in branched form. Here also all the C atoms are sp3 hybridized. In n-butane there are 2 -Ch2 groups which are 20 i.e. attached with 2 C atom and 2 -Ch3 groups which are 10 i.e. attached with 1 C atom.

Both chain isomers have same molecular formula but arrangement of C atoms are different in 2 structure. But these two isomers have different physical and chemical property. As for example n-butane has more van der waals force of attraction than 2- Methyl Propane. For this reason n-butane has more boiling point than 2-Methyl Propane.

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Chain isomer of n-butane

n-pentane

n-pentane has molecular formula C5H12. It exist in 3 chain isomers. It’s chain isomers example are n-pentane, 2-Methylbutane, 2,2-Dimethylpropane. Out of these 3 only n-pentane is straight chain isomer and the remaining 2 are branched chain compound. in n-pentane there are 5 C atoms which are arranged in straight chain and each C atom is sp3 hybridized.

In these compound there are 3 –Ch2 groups out of these 2(attached with 2 C atoms) are 20 and 1 is primary(attached with 1 C atom). There are also 2 methyl groups which are 10( attached with only 1 C atom). All the 3 chain isomers have same molecular formula but C atom’s distribution is different.

But these 3 chain isomers examples have different chemical and physical property. Boiling point order of these 3 isomers is given below: n-pentane>2-methylbutane>2,2-dimethyl propane. This is because n-pentane has highest and 2,2-dimethylpropane has least van der waals force of attraction.

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Chain isomer of n-pentane

n-hexane

n-hexane has molecular formula C6H14. It has 5 chain isomers example. These are n-hexane, 2-methyl pentane, 3-methyl pentane, 2,3-dimethyl butane, 2,2- dimethyl butane. Out of these only n-hexane is straight chain isomer and the remaining ones are branched chain isomer.

In n-hexane there are 6 C atoms which are arranged in straight chain and each C atom is sp3 hybridized. In this compound there are 5 Ch2 groups and 2 Ch3 groups. In 2-methyl pentane there are 2 Ch2 group and 2 Ch3 group and also 1 Ch group with which 1 Ch3 group (at 2 position) is attached.

In 3-methyl pentane arrangement of groups i.e. (Ch,Ch2,Ch3) are same but in this compound Ch3 group attached with Ch group at 3 position. In 2,3-dimethyl butane there are total 4 Ch3 groups attached with 2 Ch group symmetrically.

In 2,2-dimethyl butane 3 Ch3 groups attached with 1 C and 1 Ch3 group is attached with Ch2 group. All 5 chain isomer have same molecular formula but distribution of atoms is different.

Boiling point order of these isomer are given below: n-hexane>3-methyl pentane>2-methyl pentane>2,3-dimethyl butane>2,2- dimethyl butane. This is due to the fact that n-hexane has highest VDW and 2,2-dimethyl butane has least Van Der waals force of  attraction.

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Chain isomer of n-hexane

n-heptane

n-heptane has molecular formula C7H16. It has 7 chain isomers example. These are n-heptane, 2,3-dimethyl pentane, 3,3-dimethyl pentane, 2-methyl hexane, 2,4-dimethyl butane, 3-ethyl pentane, 3-methyl hexane, 2,2-dimethyl pentane, 2,2,3-trimethyl butane.

Out of these only n-heptane is straight chain isomer but the remaining ones are branched chain isomers. In n-heptane there are 5 Ch2 groups and 2 Ch3 groups. In 2,3-dimethyl pentane there are 1 Ch2 group, 2 Ch3 group and2 Ch group with which 2 Ch3 group is attached. In 3,3-dimethyl pentane there are 2 Ch2 group , 2 Ch3 group and 1 C atom with which 2 Ch3 group is attached.

In 2-methyl hexane there are 3 Ch2 group, 2 Ch3 group and 1 Ch group with which 1 Ch3 group is attached. In 2,4-dimethyl pentane there are 1 Ch2 group, 2 Ch3 group and 2 Ch group with which 2 Ch3 group is attached. In 3-ethyl pentane there are 2 Ch2 group, 2 Ch3 group  and 1 Ch group with which 1 Ethyl group is attached.

In 3-methyl hexane there are 3 Ch2 group, 2 Ch3 group and 1 Ch group with which 1 Ch3 group is attached. In 2,2-dimethyl pentane there are 2 Ch2 group,2 Ch3 group and 1 C atom with which 2 Ch3 groups are attached. In 2,2,3-trimethyl butane there are 2 Ch3 group, 1 Ch group with which 1 Ch3 is attached and 1 C atom with which 2 Methyl group is attached.

All these 9 isomer have same molecular formula but distribution of C and H atoms are different in chains in these isomers. Out of the 9 chain isomer n-heptane has highest boiling point and 2,2,3-trimethyl butane has least boiling point. This is due to the fact that n- heptane has highest VDW and 2,2,3-trimethyl butane has least Van der waals force of attraction.

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Chain isomer of n-heptane

n-butyl amine

n-butyl amine has molecular formula C4H11N. It has 4 chain isomers example. These are n-butyl amine, 1-methyl propyl amine, isobutyl amine, tert-butyl amine. Out of these only n-butyl amine has chain structure and the remaining 3 have branched structure.

In n-butyl amine there are 3 Ch2 group,1 methyl group and 1 Nh2 group which is 10 is nature. In 1-methyl propyl amine there are 1 Ch2 group,1 methyl group and 1 Ch group with which 1 Ch3 as well as 1 Nh2 is attached. In isobutyl amine there are 1 Ch2 group with which 1 Nh2 group is attached .

There also 1 Ch group with which 2 methyl group is attached. In tert butyl amine there is 1 C atom with which 3 Ch3 group and 1 Nh2 group is attached. Out of these 4 chain isomer of amine n-butyl amine (highest VWD forces) has highest boiling point and tert-butyl amine has least boiling point(least van der waals forces).

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Chain Isomer of n-butyl amine

n-propyl amine

It is the simplest chain isomer of monomeric amines. It has the formula C3H9N. It has 2 chain isomers example. These are n-propyl amine and 2-methyl Ethan amine. N-propyl amine has straight chain structure while 2-methyl amine has branched chain structure.

In the 1st one there are 2 Ch2 group,1 Ch3 group and 1 Nh2 group. In the 2nd one there are 1 Ch group with which 2 methyl group and 1 Nh2 group is attached.

As expected straight chain isomer i.e. n-propyl amine has highest boiling point and 2-methyl amine has least boiling point. This is because n-propyl amine has higher van der waals force of attraction than 2-methyl ethan amine.

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Chain Isomer of n-propyl amine

IO3- lewis structure: Drawings, Hybridization, Shape, Charges, Pairs

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In this article we are discussing about io3- lewis structure including its drawing, hybridization, shape, pairs and some FAQS.

Iodate is an oxoanion of iodine. It is formed when Iodic acid losses one proton. It has the molecular weight of 174.903. Usually iodates occur in nature as salts which are generally colorless.

IO3- Lewis Structure Drawing

As iodine is bigger in size and has less electronegativity than O atom I act as the central atom in this compound.

Iodine has 7 valance electrons out of which 3 electrons take part in sigma bonding with 3 O atoms and forms 2 pi bond with 2 O atoms. One electron pair still present on I atom which remains as lone electron pair on central I atom. O atom has 6 valance electrons out of which 1 is used in making sigma bond and 1 is used in making pi bond and remaining 4 electrons present as lone pair of electrons on O atom.

io3- lewis structure
IO3- LEWIS STRUCTURE

IO3- Lewis Structure Resonance

Resonance means movement of electrons from one atom to another atom and the structure obtained by this process is called canonical structure.

Io3- has 3 canonical structures. In all the structures I-O bond has partial double bond character due to delocalization of electron pair that present on O atom with empty antibonding orbital of I=O double bond.

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IO3- LEWIS STRUCTURE RESONANCE

IO3- Lewis Structure Shape

According to VSEPR theory the shape of io3- is pyramidal in which iodine is tetrahedrally surround by 2 O atoms and 1 O- ion. Due to the presence of 1 lone pair on central I atom ideal tetrahedral geometry does not occur. As lone pair is absent on I atom the geometry of this compound is tetrahedral. But as because lone pair is present the structure becomes is distorted and the correct geometry is pyramidal.

IO3- Lewis Structure Formal Charge

The formal charge on any atom or ion can be calculated by the formula given below:

Formal Charge (f) =V-B/2-N

Where,

V= No of valance electrons, B= No of bonding electrons, N= No of nonbonding electrons.

Hence formal charge on I atom in io3- = 7-10/2-2=0.

Formal charge on each double bonded O atom in io3- =6-4/2-4=0.

Formal charge on single bond O atom in io3- =6-2/2-6=-1.

Hence iodine atom has 0 formal charge on it. Each double bond O atom has 0 and single bond O atom has -1 formal charge making the whole compound is negatively charged.

IO3- Lewis Structure Angle

Io3- has distorted tetrahedral geometry hence normal tetrahedral bond angle 109028’ does not arises here. This is because of lone pair present on I atom.

In this compound both lp-lp and bp-bp repulsion occurs. But lp-lp repulsion is stronger in nature than bond pair-bond pair electronic repulsion. To minimize this bond pair-lone pair repulsion O-I-O bond angle is reduced to 1000 from 109028’.

IO3- Lewis structure Octet Rule

In the lewis structure of io3- we found that each O atom has 8 electrons in its outermost shell and fulfill their octet. In io3- ion I forms 2 I=O double bonds and 1 I-O single bond, also there exist 1 lone pair of electron that present on central I atom creating a total of 12 electrons around I atom. As I is a member of 3rd period element. It can increase their octet more than 8 electrons. Hence according to octet rule iodate is a stable compound.

IO3- Lewis Structure Lone Pair

The valance shell electron that don’t take part in sigma as well as pi bonding is called lone pair of electron or nonbonding electrons pair.

The basic formula with the help of which we can find the lone pair of electron on the given atom is given below:

No of lone pairs= Total no of valance electron of the atom-no of bonds formed by that atom.

In io3- lone pair present on I atom= 7-5=2 i.e. 1 lone pair

Lone pair present on each double bonded O atom=6-2=4 i.e. 2 lone pair.

Lone pair present on single bonded O- ion= 8-2=6 i.e.3 lone pair.

These lone pair of electrons is found In the lewis structure of io3- on the given atoms as electron dots.

IO3- Valance Electrons

Firstly to find out the total valance electron in io3- ion, it is important  to know the electronic configuration of I and O atom.

The electronic configuration of I is [Kr36]4d105s25p5 and as we see from electronic configuration that there are 7 electrons in valance shell of I atom. The electronic configuration of O atom is [He2]2s22p4. There is 6 electrons in the valance shell of O atom. Also one negative charge is present on O atom.

The total valance electrons that present on io3- ion will be equal to the (sum of the valance electron of I and O atom+1 negative charge) i.e. equals to (7*1)+(6*3)+1=26. There are 26 valance electrons in io3- ion.

IO3- Lewis Structure Hybridization

Hybridization is the process in which hybrid orbitals are formed by mixing of same energy atomic orbitals.

The ground state outermost shell electronic configuration of I is 5s25p5. As we see from electronic configuration of I atom that there is only 1 unpaired electron and to form io3- ion 3 unpaired electron is required. In the excited state, I transfer 2 p electrons in 5d orbital and now a total of 5 unpaired electron is present.

In the next step 3 O atom gave 3 unpaired electron to form 3 electron pair by which 3 I-O single bond is formed. There still 1 unpaired electron present on O atom which forms 2 I=O pi bonds.

In this compound I uses sp3 hybrid orbital to make I-O bonds. Due to sp3 hybridization iodate should have tetrahedral geometry but as because of presence of lone pair of electron the shape of io3- ion is pyramidal.

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IO3- LEWIS STRUCTURE HYBRIDIZATION

Io3- Uses

Iodates are used in treatment of thyroid gland disorder.

It used in iodometry for the manufacture of medicine.

It is used in the analysis for testing arsenic and zinc salts.

Sometimes it is used for iodination of table salt to remove iodine deficiency.

Some FAQS About IO3-

Is IO3- Ionic or Covalent?

Io3- is a covalent compound. Iodate is formed by covalent sigma bond formation. When a ionic compound is formed, one or more electron is moved towards electronegative atom from less electronegative atom. Here in the formation of this compound nothing happens. Io3- ion is formed by sharing of electron pair between I and O atom. Hence it is a covalent compound.

Is IO3- Stable?

Io3- is a stable compound. As lone pair of electron is present on I atom lp-bp repulsion is occurred. For this reason its stability is decreased. But due to resonance each I-O bond gets a partial double bond character which overcomes lone pair-bond pair repulsion and makes the compound stable.

Is io3- polar in nature?

Io3- is polar in nature. A molecule is found to be polar if its dipole moment(µ) is not equal to 0. In this compound 3 I-O bonds are polar this is due to electronegativity difference between I and O atom. As I is more electronegative than O atom the 3 I-O bond moments lies towards I atom.

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IF2- lewis structure: Drawings, Hybridization, Shape, Charges, Pairs

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In this article we want to discuss about the if2- lewis structure including its drawing, hybridization, shape, charges, pairs and some FAQS.

IF2– is a poly halide in which iodine act as a central atom and 2 fluorine atoms act as terminal atom.

IF2– Lewis Structure Drawing

if2- lewis structure
IF2– Lewis Structure

In the if2- lewis structure we see that as iodine becomes larger in size and less electronegative than F it goes in the center of the Lewis structure.

Iodine has 7 valance electrons out of which 2 electrons take part in bonding with F atom and form 2 covalent sigma bond and still 3 electron pair there on I atom which does not take part in bonding F atom and exist as lone pair of electron. F has also 7 electron in their valance shell out of which only 1 electron make covalent bond with central I atom and remaining 6 electrons present as lone pair on I atom.

IF2– Lewis Structure Resonance

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if2- lewis structure resonance

Resonance means shifting of electron pair from one atom to another atom and the structure obtained by this process is called resonating structure.

IF2– has 3 resonating structure in which each I-F bond gets partial double bond character by the process in which F atom donate its lone pair of electron into vacant d orbital of I atom to form p(pi)-d(pi) back bonding.

IF2– Lewis Structure Shape

According to VSEPR theory the shape of IF2–is linear in which iodine is the central atom around which 2 F atoms surround it. As 3 lone pair present in the central I atom the ideal TBP geometry becomes distorted. If 3 lone pair is not present in IF2–  the shape becomes TBP but as 3 lone pair present on central I atom the shape becomes distorted and the actual shape is linear.

IF2– Lewis Structure Formal Charge

The formal charge on any atom can be calculated by the formula given below:

Formal Charge (f) =V-B/2-N

Where,

V= No of valance electrons, B= No of bonding electrons, N= No of nonbonding electrons.

Hence formal charge on I atom in IF2–=7-4/2-6= -1

Formal charge on each F atom in IF2– =7 -2/2-6= 0

Hence formal charge on I atom is -1 and on each F atom is 0 making the whole compound is negatively charged.

IF2– Lewis Structure Angle

if2- lewis structure has distorted TBP geometry hence normal TBP bond angle 1200 and 900 does not arises here. Here in this compound lone pair will occupy the equatorial position and F atoms will occupy the axial position.

This is because according to Bent’s rule more electronegative atom will occupy the hybrid orbital having less s character and less electronegative atom will occupy the hybrid orbital having more s character.

Hence we know that lone pair has 0 electronegativity for that it will occupy equatorial position where % of s character is 33.3 and more electronegative F atom will occupy the axial position where % of s character is 0 making the F-I-F bond angle is 1800.

IF2– Lewis Structure Octet Rule

In if2- lewis structure we see that each F atom has 8 valance electrons and completes their octet. In I forms 2 I-F bonds and each bond contain 2 electrons. There is also 3 lone pairs that present on I atom making a total of 10 electrons around I atom. As I is a member of 3rd period and we also know that 3rd period element can increase their octet more than 8 electrons. Hence according to octet rule IF2– is a stable compound.

IF2– Lewis Structure Lone Pairs

The valance electron that does not take place in bonding is defined as lone pair of electron or nonbonding electrons.

The formula through which we can calculate the lone pair of electron is given below:

For central atom,

No of lone pairs=Total no of valance electron of the atom-no of bonding electron formed by that atom

In if2- lewis structure , lone pair present on I atom=7-4=3

For terminal atom,

No of lone pairs=Total no of valance electron-no of bonds formed by that atom

 Lone pair present on each F atom=7-1=6 i.e. 3 lone pair

These lone pairs are shown In the Lewis structure of IF2– on the given atoms as dots.

IF2– Valance Electrons

At first, to calculate the total valance electron in IF2–, it is essential to know the electronic configuration of I and F atom.

The electronic of I is [Kr36]4d105s25p5 and from electronic configuration we see that there are 7 electrons in the outermost shell of I atom. The electronic configuration of F atom is [He2]2s22p5 and has 7 electrons. As both I and F both belong to same group i.e. 17, there are 7 valance electrons in both I and F atom. There is also 1 negative charge.

The total valance electron in the compound will be equal to the sum of the valance electron of I and F atom + 1 negative charge i.e. (7*1) + (7*2) + 1=22. There are 22 valance electrons in this species.

IF2– Hybridization

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IF2– Hybridization

Hybridization is the process of mixing of same energy atomic orbitals to form an equal number of hybrid orbitals.

The ground state valance shell electronic configuration of I is 5s25p5. In the ground state of I we see that there is only 1 unpaired electron and to make IF2– 2 unpaired electron is required. In the excited state I send its 1 p electron into d orbital making a total of 3 unpaired electrons. In the next step 2 F atoms give their 1 unpaired electron to form 2 I-F sigma bonds and sp3d hybridization takes place according to VSEPR theory.

In this compound I uses sp3d hybrid orbital to make I-F bonds. According to sp3d hybridization the geometry should be TBP but the actual structure is linear due to the presence of 3 lone pair of electron in the equatorial position of if2- lewis structure.

IF2– Uses

if2- mainly used in making eye drops. It is used as a fluorinating agent. It is used in explosive material.

FAQS about IF2–

Is IF2– Ionic or Covalent?

IF2– is a covalent compound. This is because it is formed by covalent sigma bonds. In the formation of ionic compound there occurs shifting of electron from electropositive atom to electronegative atom. In if2- lewis structure it is not possible because there occurs mutual sharing of electron between I and F atom to form sigma bonds so that no ions is formed. Hence it is a covalent compound.

Is IF2– Stable?

IF2– is an unstable compound. This is due to the presence of 3 lone pair electron around I atom and there occurs severe LP-LP repulsion. Also I-F bonds are not too strong due to large electronegativity difference and poor orbital overlap between I and F atoms. Due to these two reason this compound is not stable.

Is IF2– polar in nature?

IF2– is a nonpolar compound. A compound is said to be polar when its dipole moment is not equal to 0. The electronegativity of I and F is 2.66 and 3.98 respectively that’s why I-F bond moment lies towards F atom. But as the shape is linear, 2 I-F bond moments lie in opposite direction and cancel each other making the molecule nonpolar.

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ICL5 lewis structure: Drawings, Hybridization, Shape, Charges, Pairs

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In this article we discuss about the Lewis Structure of ICL5.

ICL5 is prepared by the reaction of chlorine (Cl2) and iodine (I2) at a particular stoichiometric ration. It is an inter halogen compound. Inter halogen compound are those which are composed of more than one halogen atom. Basically Icl5 belongs to the category of poly halides.

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ICL5 Lewis Structure

In the Lewis structure of Icl5 we see that as iodine becomes larger in size and less electronegative than cl it goes In the center of the Lewis structure.

Iodine has seven valance electrons out of which five electrons take part In covalent bonding with cl atom and forms five covalent chemical bonds and still one electron pair there on iodine atom which does not take part in bonding with cl atom and exist as lone pair of electron. Chlorine atom has also 7 electrons in their valance shell out of which only 1 electron make covalent bond with central iodine atom and remaining 6 electrons present as lone pair of electron on cl atom.

ICl5 Lewis Structure Resonance

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ICL5 Lewis Structure Resonance

Resonance means shifting of electron pair from one atom to another atom and the structure obtained by this process is called resonating structure.

ICl5 has 6 resonating structure in which each I-CL bond gets partial double bond character by the process in which CL atom donate its lone pair of electron into vacant d orbital of iodine atom to form p(pi)-d(pi) back bonding.

ICl5 Lewis Structure Shape

According To VSEPR theory the shape of Icl5 is square pyramidal in which iodine is the central atom around which five chlorine atoms surround it. As lone pair present in the central I atom the ideal octahedral geometry becomes distorted. If lone pair is not present in ICL5 the shape becomes octahedral but as lone pair is present the shape becomes distorted and the actual shape is square pyramidal.

ICl5 Lewis structure Formal Charge

The formal charge on any atom can be calculated by the formula given below:

Formal Charge (f) = V- B/2 -N

Where,

V= No of valance electrons

B= No of bonding electrons

N= No of nonbonding electrons

Hence formal charge on I atom in Icl5 = 7-10/2 -2=0

Formal charge on each CL atom in Icl5= 7-2/2-6=0

Hence formal charge on both I and CL atom in ICL5 are zero which means that the compound is neutral.

ICL5 Lewis Structure Angle

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ICL5 Lewis Structure Angle

ICL5 has distorted octahedral geometry hence normal octahedral bond angle 900 does not attained here. Due to repulsion between lone pair of electron on central I atom and bonding electron pair on I-CL bond, CL-I-CL  bonds angle slightly decreased from 900 to 81.90 to minimize the lone pair- bond pair repulsion.

ICL5 Lewis Structure Octet Rule

In the Lewis structure of ICL5 we see that each CL atom has 8 valance electrons and complete its octet. In ICL5 Iodine atom forms 5 I-CL bonds and each bond contains 2 electrons. There is also a lone pair that present on central I atom making a total of 12 electrons around I atom. As iodine is a member of third period we know that third period element can increase their octet more 8 electrons. Hence according to octet rule ICL5 is a stable compound.

ICL5 Lewis Structure Lone Pair

The valance electron that does not take part in bonding is defined as lone pair of electron or nonbonding electrons.

The formula through which we can calculate the lone pair of electron is given below:

No of lone pairs= Total no of valance electron of the atom-no of bonds formed by that atom

In ICL5, Lone pair present on I atom=7-5=2 i.e. 1 lone pair

Lone pair present on each CL atom=7-1=6 i.e. 3 lone pair

These lone pairs are shown in the Lewis structure of ICL5 on the given atoms as dots.

ICL5 Hybridization

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ICL5 Hybridization

Hybridization is the process of mixing of same energy atomic orbitals to form an equal number of mixed orbitals/hybrid orbitals.

The ground state valance shell electronic configuration of is 5s25p5. In the ground state of I we see that there is only one unpaired electron and to make the formation of ICL5 feasible 5 unpaired electron is needed. In the excited state I send its 2 p electron into d orbital making a total of 5 unpaired electrons. In the next step 5 CL atoms give their one unpaired electron to form 5 I-CL covalent sigma bonds and sp3d2 hybridization takes place according to VSEPR theory.

ICL5 Uses

ICL5 mainly used in making water and oil repellent emulsions which is used for the treatment of textiles and leathers. It is also used in making water repellent paper. Due to its insulating properties it is used in electric motors.

Is ICL5 Ionic or Covalent?

ICL5 is a covalent compound. This is because this compound is formed by covalent sigma bonds. In the formation of ionic compound there occurs shifting of electron from electropositive atom to electronegative atom.

In ICL5 it is not possible due to less electronegative difference between I and CL atom. Here in this compound mutual sharing of electrons take place between I and CL atom to form sigma bonds so that no ions is formed. Hence it is a covalent compound.

Is ICL5 stable?

ICL5 is an unstable compound. This is because large cl atoms surrounds central Iodine atom so that severe steric crowding takes place in this compound and dissociates. Also I-CL bonds are not too strong to make the compound stable due to poor orbital overlap between I and CL atom.

Due to these two reasons this compound is not too stable

FAQS about ICL5

Is ICL5  polar in nature ?

A compound is polar when its dipole moment becomes not equal to zero. The electronegativity of I and CL is 2.66 and 3.16 respectively that why I-CL bond moment lies towards CL atom. Hence electronegativity difference occurs between I and CL. In the square pyramidal structure of ICL5 4 CL atoms lying in the same square plane and hence 4 I-CL bond moments cancel each other. But one I-CL bond moment still exist for which dipole moment of ICL5 does not equal to zero. Hence it is polar in nature.

Which type of crystal Structure ICL5 have?

ICL5 Has monoclinic crystal structure.

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SRO Lewis Structure: Drawings, Hybridization, Shape, Charges, Pair And Detailed Facts

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 In this article we are going to analyze the SRO Lewis structure and various facts about it.

Strontium oxide is produced when strontium reacts with oxygen. When strontium is burned in presence of air results in a mixture of strontium oxide and strontium nitride.

SRO Lewis Structure

SRO is formed by two elements i.e. one is strontium and other is oxygen. Strontium has atomic number 38. Its electronic configuration is [Kr]5s2. When it losses two electron from 5s orbital it gets the nearest noble gas configuration i.e. Kr(Z=36) which is a stable electronic configuration because in the valence shell of Kr octet is fulfilled.

When Strontium loss 2 electrons by the above process Sr+2 is formed. In case of oxygen, it has atomic number 8. Its electronic configuration is [He]2s22p4. When it gains 2 electrons which is rejected by Strontium it gets nearest noble gas configuration i.e. Ne(Z=10) which is a stable electronic configuration. O2- ion has octet fulfilled valance shell electronic configuration.

Lewis Structure Diagram of SRO

Lewis Structure of SRO 
Lewis Structure of SRO 

SRO Lewis Structure Formal Charges

In Strontium Oxide overall formal charge on the compound Is Zero(0).When SRO ionizes Sr+2 and O2- ion is formed. Strontium +2 charge is neutralized by Oxygen -2 charge. In the crystal lattice structure of strontium oxide equal number of Sr+2 and O-2 is present so that overall formal charge is Zero.

SRO Lewis Structure Lone Pair

In the Lewis structure of Strontium Oxide zero lone pair present on strontium and two lone pair present on oxygen atom. This is due to the fact that Strontium has lost its two electron i.e. one lone pair and converted to Sr+2 which has no lone pair on it. But in case of Oxygen atom it accepts two electrons from strontium and converted into O2- which has two lone pair on it.

SRO Hybridization

In strontium Oxide Sr+2 and O2- ion is present. Strontium oxide exists in a cubic crystal lattice structure. Both strontium and oxygen have d2sp3 hybridization i.e. octahedral co-ordination geometry. In the lattice structure of strontium oxide each Sr+2 ion is surrounded by six oxygen atoms and each O2- ion is surrounded by six Sr+2 ion. Hence both strontium ion and oxide ion have co-ordination number equals to 6.

SRO Lewis structure Resonance

Strontium Oxide is overall a neutral molecule with zero formal charge on it. But during resonance takes place strontium oxide breaks into Sr+2 ion and O2- ion. After resonance both strontium and oxide ion are stabilized because both stable nearest noble gas configuration i.e. Strontium ion acquires krypton(Kr) noble electronic configuration and Oxide ion acquires Neon(Ne) noble gas configuration.

SRO Lewis Structure Octet Rule

In strontium Oxide both Strontium and Oxygen have their octet fulfilled. During the formation of Strontium oxide Strontium losses two electron to get nearest noble gas configuration i.e. (Kr) which have 8 electrons in its valance shell (4s24p6) and Oxygen accepts two electrons from strontium to get nearest noble gas configuration i.e. (Ne) which also have 8 electrons in their valance shell (2s22p6). Hence both atoms get their octet fulfilled.

SRO Polar Or Nonpolar

Strontium Oxide is a polar compound. This is because in strontium oxide both strontium and oxygen have different electronegativity and hence opposite dipole creates on strontium and oxygen. Due to less electronegativity of strontium it acquires positive dipole on it and due to more electronegativity of Oxygen atom it gets negative dipole. Due to this opposite dipole that exists in strontium Oxide, it is an ionic compound as well as polar compound.

SRO Uses

Strontium Oxide has various useful applications. It is largely used in cathode ray tubes where strontium is present by 8% of its weight. Now a days Strontium oxide used for making television picture tube glasses. It is also used in glass, optic, and ceramic industry. In recent times for the preparation of strontium SRO is used as a starting material which is being heated with aluminum under vacuum. It is the best method for the production of pure strontium. It also has application in medical industry.

Detailed Fact about SRO

Strontium Oxide is an ionic compound. In the Lewis structure both strontium and oxygen have fulfilled their octet by the process of resonance in which strontium losses two electron and oxygen accepts two electrons. This is because due to less electronegativity strontium gains positive charge and oxygen gains two electrons due to higher electronegativity.

SRO exists in cubic crystal lattice structure in which both Strontium and Oxygen have octahedral arrangement around each other. SRO is a polar molecule due to electronegativity difference between Strontium and Oxygen atom.

Frequently Asked Question about SRO(FAQ)

What happens when Strontium Oxide Reacts with Water?

Strontium Oxide reacts with Water vigorously to form strontium hydroxideas white precipitate with the evolution of heat.

               SRO + H20 = SR(OH)2

Why SRO is soluble in Water?

As strontium Oxide is a polar compound, it dissolves in polar solvent as for example water.

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