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In this article we want to discuss about cr2o3 lewis structure, characteristics and 21 most important characteristics regarding this topic.
Cr2o3 is mainly used in color industry which acts as a pigment. It is generally insoluble in water and it is an amphoteric oxide. Naturally it occurs as a dark green and hexagonal crystalline solid. For the preparation of chromium metal, for polishing of stainless steel cr2o3 is largely used.
Cr2o3 Lewis Structure Drawing
In cr2o3, out of 3 o atoms 1 o atom is shared both by cr atoms by covalent sigma bonds. 2 cr atoms forms 1 sigma and 1 pi bonds with o atoms.
The whole molecule is arrangd in a tetrahedral manner in which central o atom forms 2 bond with 2 cr atoms and it contains 2 lone pair and in all aspect all these bonds are purely covalent and formed by sharing of electrons. In cr2o3, terminal o atoms contain 2 lone pairs each.
Cr2o3 Lewis Structure Shape
In cr2o3 lewis structure, the central o atom is sp3 hybridized. This is because of the fact that it contains 2 sigma bonds with two cr atoms and remaining hybrid orbital contain 2 pairs. According to sp3 hybridization the structure should be tetrahedral but the actual shape is bent / V-shaped.
Cr2o3 Lewis Structure Formal Charges
The formal charge on the central o atom in cr2o3=6-4/2-4=0.
Formal charge on terminal oxygen atom in cr2o3=6-4/2-4=0.
Formal charge on 2 cr atoms in cr2o3=6-6/2-3=0.
Hence formal charge on central o atom in cr2o3 is 0 and also two o terminal atoms, two cr atoms also contain o formal charge. Hence this compound is overall electrically neutral.
Cr2o3 lewis Structure Lone Pairs
The lone pairs mean how many no of unshared electrons present in cr2o3 that does not take part in bonding. This can be calculated by the following way-
Lone pair present on central o atom in cr2o3=6-4=2 lone pairs.
Lone pair present on terminal cr atom in cr2o3=6-6=0 i.e. 0 lone pair of electron.
Lone pair present on terminal o atoms in cr2o3=6-4=2 lone pairs.
In cr2o3 compound these nonbonding electron pair are shown on the above mentioned atoms as electron dots.
Cr2O3 Hybridization
During hybridization means during bond formation central o atom uses sp3 hybrid orbital to form cr2o3 compound. Central o atom has 6 valance electron out of which 2 unpaired electrons is used for the formation of 2 sigma bonds with two cr atoms. Two cr atoms has 6 valance electron out of which 2 are used in bonding with 2 terminal o atoms.
2 terminal o atoms forms 1 sigma and 1 pi bonds with cr atoms by using its 2 unpaired electrons and remaining 4 electrons which does not take part in bonding with cr atoms present as lone pair of electron. Hence in cr2o3, central o atom uses sp3 hybrid orbital to form cr2o3 compound. according to sp3 hybridization its structure is pyramidal not tetrahedral due to presence of 2 lone pairs.
Cr2o3 is insoluble in water, ethanol and even in acetone and also acids. By considering the fact mentioned above it is concluded that cr2o3 is a nonpolar compound. As it is nonpolar in nature, it is soluble in nonpolar solvents like carbon tetrachloride, carbon disulphide etc.
Cr2O3 valance electrons
The total no of valance elctron in cr2o3 is equal to the valance electron present in cr and o atoms. Cr contains 6 and O also contains 6 valance electron. The total no of valance electron present in cr2o3 is (6*2)+(6*3)=12+18=30.
Cr2O3 lewis structure angle
In cr2o3 lewis structure, central o atom is bonded with 2 cr atoms with which 2 o atoms are double bonded with cr atoms in a tetrahedral manner. The central O atom is sp3 hybridized in cr2o3 and also contain 2 lone pairs. As the structure is pyramidal, the angle should be 104.50.
Cr2o3 lewis Structure Resonance
In cr2o3 lewis structure when electron pair movement i.e resonance takes place, 3 resonating structure is obtained. In cr2o3, lone pair of electron present on central o atom is delocalized with the cr=o bonds i.e. with vacant ∏* orbital of cr=o bonds.
Cr2o3 lewis structure Octet Rule
The lewis structure of cr2o3 shows that all the atoms in cr2o3 fulfill their octet. In cr2o3, the central o atom forms 2 sigma bonds with 2 cr atoms and also contains 2 lone pairs. That is why, central o atom satisfy its octet. Two terminal o atom forms double bond with cr atom and also contain 2 lone pairs.
By this terminal o atoms fulfill their octet. 2 cr atoms forms 2 sigma bond and 1 pi bond with central and terminal o atoms. It also contains 1 lone pair. Hence it contains total of 8 electrons and fulfill its octet. Hence by applying octet rule the compound cr2o3 is a stable compound.
Cr2o3 Polar Or Nonpolar?
Cr2O3 is nonpolar compound. As we seen that it is a nonpolar compound it is insoluble in polar solvents like water. Its lattice energy is higher than hydration energy. To break it into Cr3+ and O2- ions higher energy is required. For this reason, it usually does not break into cr3+ and O2- ions.
Is cr2o3 ionic?
Cr2O3 is ionic compound. When cr2o3 ionizes, 2cr3+ ions and 3o2- ions are produced. As therefore, Cr2O3 is overall a neutral compound because total 6 positive charges is neutralized by total 6 negative charges. As because cr is metallic in nature, it acquires positive charge and o is nonmetallic in nature it acquires negative charge.
Is cr2o3 acidic or basic?
Cr2O3 is amphoteric in nature i.e. it both reacts with acid as well as base. When it reacts with acid it behaves like base and when it reacts with base it behaves like acid. When it reacts with acid, it produces hydrated Cr species which is capable of reacting with bases to produce complex salts.
Is cr2o3 tetrahedral?
In Cr2O3, central O atom is tetrahedral arranged around 2 lone pairs and 2 Cr=O fragments. Hence central O atom in cr2o3 is sp3 hybridized. That is why cr2o3 is tetrahedral in nature.
Is cr2o3 linear?
Cr2O3 is not linear because from structure of cr2o3 we see that 2 Cr atoms and 3 O atoms are arranged in angular manner i.e. in bent manner. Hence Question of linear structure does not arise.
Is cr2o3 symmetrical or asymmetrical?
Cr2O3 is symmetrical in nature. When a sigma or mirror plane passes through the compound it divided the compound into 2 symmetric halves. Actually, the mirror plane passes through the O atom in cr2o3 compound, 2 symmetric halves are obtained i.e. Cr=O part.
Cr2O3 Molar Mass
As cr2o3 contains 2 cr atoms and 3 o atoms in it. The molar mass of cr2o3 is equal to the sum of molar mass of 2 cr atoms and 3 atoms. Hence the molar mass of cr2o3 is 151.9904 gm/mol.
Cr2O3 Oxidation Number
O atom has -2 oxidation states. Hence 3 o atoms provide -6 oxidation states. Cr2o3 is overall a neutral compound. For this reason, -6 charge is neutralized by +6 charge. Hence each cr atom provides +3 oxidation state.
Cr2O3 Charge
Cr2O3 is overall a neutral compound. This is because of the fact that -6 charge of o atom is neutralized by +6 charge of cr atoms. Cr2o3 has overall a neutral compound.
Is Cr2O3 Paramagnetic?
Cr2O3 contains a total of 6 unpaired electrons i.e. each cr atoms provide 3 unpaired electron. Hence this compound is paramagnetic due to presence of unpaired of electrons. In cr2O3, each cr atom provides 3BM spin only magnetic moment.
Is Cr2O3 a Strong Electrolyte?
Cr2O3 contains 6 unpaired electrons. This unpaired free electron is responsible for the creation of electricity by cr2o3. For this reason, cr3o3 behaves as a strong electrolyte.
Conclusion
Keeping the above facts in mind about cr2o3 it is stated that cr2o3 is a neutral nonpolar tetrahedral compound. It reacts with both acid and bases to behave as an amphoteric oxide. In cr2o3 the two cr atoms contain +3 oxidation state and 3 o atoms contain -2 oxidation state each.
In this article we going to discuss about cobr2 lewis structure including its characteristics and structure and 13 most important facts regarding this.
Cobr2 which is commonly known as bromophosgene in analogy with phosgene. It is produced in fire extinguishers, when halon compounds are decomposed. It is a colourless liquid with a molar mass of 187.818 gm/mol. It starts boiling at 64.50c, when it decomposes. Even at low temperature, it slowly decomposes to poisonous co and elemental br.
Cobr2 Lewis Structure Drawing
In cobr2 the central atom is C atom in which O and 2 Br atoms are attached. In cobr2, central c atom uses sp2 hybrid orbital. In the ground state, C atom has 4 valance electron but only 2 remains unpaired. To form cobr2, 4 unpaired electrons is required.
When some energy is applied, one 2s electron of c atom becomes unpaired and total 4 unpaired electron is present now. Hence 2 br atoms form 2 sigma bonds and o atom forms 1 sigma as well as 1 pi bond with central c atom. All these are covalent bonds. This is because all these are formed by sharing of electrons between 2 atoms.
From VSEPR theory we can assume that the shape of cobr2 is trigonal planner. In this structure central carbon atom is surrounded by 2 br atoms and 1 o atom in trigonal planner manner.
The structure of cobr2 does not contain any lone pair of electron on central c atom; hence distortion of ideal trigonal planner structure does not occur. In cobr2, central C atom uses sp2 hybrid orbital to form 2 c-br bonds and 1 c=o bond. As cobr2 has planner structure all the atoms in cobr2 lie in the same plane.
Cobr2 Lewis Structure Formal Charges
The formula we used to calculate the formal charge is -Formal Charge (f.c) on each atom= (Total No of valance electrons of the atom)-(Total no of bonding electron formed by that atom)/2- (total no of nonbonding electrons on that atom).
Hence formal charge on the central c atom in bromophosgene =4-8/2-0=0.
Formal charge on oxygen atom in cobr2=6-4/2-4=0.
Formal charge on 2 terminal br atoms in cobr2=7-2/2-6=0.
Hence formal charge on central C atom in cobr2 is 0 and each bromine atoms and also O atom has formal charge of 0, making the overall compound is electrically neutral.
Cobr2 lewis Structure Lone Pairs
Total No of unshared pair of electron exist on any atom= the valance electrons present on the atom-total no of bonds formed by that particular atom.
In cobr2 lone pair present on central c atom= 4-4=0 i.e. No lone pair of electron on c atom.
Lone pair present on oxygen atom in cobr2=6-2=4 i.e. 2 lone pair of electron.
Lone pair present on br atoms in cobr2= 7-1=6 i.e.3 unshared pair of electron.
These unshared pair of electrons on o and terminal br atoms is shown in the cobr2 lewis structure as electron dots.
Cobr2 Hybridization
Hybridization is a process in which central c atom in cobr2 mixes its atomic orbital to form hybrid orbitals because higher energy atomic orbitals does not take part in bonding. In the ground phase, C has 4 valance electrons out of which only 2 electrons are unpaired. But this is not enough electrons to form cobr2.
Hence when C absorbs hybridization energy, its 2s electron becomes unpaired and requirement of 4 unpaired electron becomes fulfilled. By using this electron C atom forms Cobr2 with the help of 3 sigma bonds and 1 pi bond. In cobr2, c uses sp2 hybrid orbital to make c-br and c=o bonds. According to sp2 hybridization, the structure of cobr2 is trigonal planner.
Cobr2 Hybridization
Cobr2 solubility
Cobr2 is soluble in polar solvents because of the fact that as cobr2 is polar in nature, it like to dissolve in polar solvents like water, ethanol, methanol etc. In 100 ml of water, approx 66.7 gm cobr2 dissolved at about 590c.
Cobr2 valance electrons
To calculate the total no of valance electron in cobr2, it is required to know the valance electron of c,o and br atoms. The valance electron present in c atom is 4. The valance electron present in O and Br atom is 6 and 7 respectively. The total no of valance electron present in cobr2 is sum of valance electron of c,o and br atoms i.e. (4*1+6*1+7*2)=24.
Cobr2 lewis structure angle
In cobr2, central c atom is sp2 hybridized and the structure of cobr2 is trigonal planner. According to VSEPR theory, the angle prsent in trigonal planner shape is 1200. Hence the angle between br-C-br and br-C-O is exactly 1200.
Cobr2 lewis Structure Resonance
In Cobr2 resonance occurs and in resonance process nonbonding electron pair shifts from one atom into another atom through conjugation. The structure we get through delocalization is called resonating structure.
When resonance takes place in cobr2, we get 3 equivalent resonating structure and delocalization occurs through conjugation of nonbonding electron pair with carbonyl group in its ∏* orbital.
Cobr2 Resonance
Cobr2 lewis structure Octet Rule
When we see the lewis structure of cobr2 we find that each bromine atom has 8 electrons in the outermost shell and satisfy octet rule. In cobr2 compound central carbon atom forms 2 C-Br bonds and 1 C=O bond making a total of 4 electron pair i.e. 8 electrons around central C atom.
O atom forms 2 bond with central C atom and also contain 2 lone pairs making a total of 8 electrons around O atom. 2 Br atoms form 1 sigma bond each with C atom and both contains 3 lone pair of electron i.e. octet rule is also satisfied for Br atom.
Cobr2 Polar Or Nonpolar?
SOCl2 is a non-polar compound. In cobr2, c=o bond moment lies towards more electronegative o atom. 2 c-br bond moments lie towards Br atom, as br is more electronegative than c atom. All these bond moments cancel each other and hence making the dipole moment of this compound is 0 Debye.
Is cobr2 ionic?
Cobr2 is an ionic compound. This is due to the fact that the electronegativity difference between the C-Br bonds and C=O bond. Cobr2 is soluble in water like ionic compounds do. It has also high melting as well as boiling point similar to that of ionic compound. It also conducts electricity in molten as well as in solution state.
Is cobr2 acidic or basic?
Cobr2 is amphoteric in nature i.e. it is act as an acid or as a base. When cobr2 reacts with acid, it accepts H+ ion through the donation of O atom and act like a like base. When it reacts with base, OH- donates its lone pair of electron and cobr2 accepts this electron and act as a lewis base.
Is cobr2 tetrahedral?
Cobr2 attains trigonal planner geometry in which c atom act as the central atom. It has no tetrahedral geometry, because central c atom is not sp3 hybridized.
Is cobr2 linear?
Cobr2 is not linear because central c atom is not sp hybridized. As the central c atom in cobr2 acquires sp2 and does not attain 1800 hence, question of cobr2 has linear geometry does not arises.
Is cobr2 symmetrical or asymmetrical?
Cobr2 is symmetrical in nature. This is because of the fact that a mirror plane i.e. sigma plane cut the cobr2 compound into 2 symmetrical halves. The sigma plane passes through the carbonyl group. It also contains c2 axis which passes through C=O group, after this operation br is superimposable with another br group.
Conclusion
Cobr2 is a stable compound in which central C atom is sp2 hybridized and due to absence of lone pair of electron the structure is real trigonal planner. In this compound all the atoms satisfied their octet.
In this article we are going to discuss about clcn lewis structure, characteristics and 13 essential facts regarding cyanogen chloride.
Clcn is a colorless easily condensed toxic gas. It has acrid odor. It belongs to the category of pseudohalogen. It is produced when sodium cyanide is oxidized with chlorine gas. The reaction involves an intermediate which is cyanogen. In presence of acid it trimerizes to produce cyanuric chloride.
Clcn Lewis Structure Drawing
In the lewis structure of Clcn, central C atom uses sp hybrid orbital to form Clcn compound. When C atom is exicted, there occurs 4 valance electron. Out of these 4 electrons, 1 is used in making sigma bond with Cl atom. Hence 1 electron of Cl atom is take part in bonding with central C atom, remaining 6 electron exist as 3 lone pair of electron.
Remaining 3 velence electrons of C atom form 1 sigma and 2 pi bonds with N atom. Hence no lone pair exist on C atom. N has 5 valance electrons, only 2 is remain unused, this exist as 1 lone pair of electron. But 3 electrons take part in bonding with central C atom.
Resonance or mesmerism is a process of describing movement of nonbonding and pi electrons between atoms in various types of polyatomic molecules through delocalization and resonance hybrid is a combination all the resonation structure. In Clcn 2 equivalent resonating structure are found. In these structures C-Cl bond acquires partial double bond character.
The fact behind this anomalous characteristics is that filled 2p electron i.e. nonbonding electron pair on Cl atom is delocalized with the vacant ∏* antibonding molecular orbital of –CN group and partial double bond character is developed between C and Cl atom. By this resonance process triple bond between C and N atom is reduced to double bond.
According to VSEPR theory the shape of Clcn is linear in which central carbon atom is attached with Cl atom by single bond and with N atom by triple bond. Each atom in Clcn is lie in a line. The linear shape of Clcn occurs because of the fact that central C atom is sp hybridized. As Clcn has linear shape so that the bond angle found in Clcn is 1800.
Clcn Lewis Structure Formal Charge
In Clcn, the formal charge on the given atoms is calculated by the following formula given below:
Formal Charge (F.C) on any atom= valance electrons of the atom-(total bonding electrons)/2- No of nonbonding electron pair.
Hence formal charge on central C atom in Clcn =4-8/2-0= 0.
Formal charge on N atom of –CN group in Clcn =5-6/2-2=0.
Formal charge on Cl atom in Clcn compound =7-2/2-6=0.
Hence formal charge on central C atom in Clcn is equal to 0. All of the atoms in Clcn has zero formal charge making the whole compound is electrically neutral.
Clcn Lewis Structure Angle
In Clcn , central carbon atom uses sp hybrid orbital to form bonds with chloride group and N atom i.e. the angle between Cl-C-N is 1800. The N atom in –CN group is also sp hybridized.
When Cl atom is in conjugation with –CN group, Cl atom becomes sp2 hybridized. As central C atom in Clcn is sp hybridized and the angle is 1800, the compound Clcn is linear in nature.
In the clcn lewis structure, all the atoms i.e. Cl, C, N fulfilled their octet. The central C atom in Clcn forms 1 sigma bond with Cl atom and another with N atom. At the same time it forms 2 pi bonds with N atom by overlap of 2 p orbitals of C and N atom. Hence central C atom forms 4 bonds which contains total of 8 electrons.
Cl atom forms 1 single bond with central C atom and contains 3 lone pair of electron i.e. a total of 8 electrons present in Cl. The N atom forms 1 sigma and 2 pi bonds with central C atom and also contain 1 lone pair i.e. again total 8 electrons present in N. According to octet rule Clcn is a stable compound.
Clcn Lewis Structure Lone Pairs
The lone pair of electrons is those valance electrons which are not shared when 2 atoms are connected by a covalent bond. It is also defined as unshared pair of electrons.
The formula through which we can calculate the lone pair of electron on the given atoms in Clcn is given below:
Lone electron pairs present on an atom= electrons which is present on the valance shell of the atom – how many chemical bonds formed by that particular atom.
Lone pair of electron present on central C atom in Clcn= 4-4=0 i.e. 0 lone pair of electron.
Lone electron pair present on N atom of –CN group in Clcn=5-3=2 i.e. 1 unshared electron pair.
Lone pair of electrons present on Cl atom in Clcn compound= 7-1=6 i.e.3 nonbonding pairs of electron.
These nonbonding electron pairs are depicted in the lewis structure of Clcn on C, N, Cl atoms as electron dots.
Clcn Valance Electrons
As to find out total no of valance electron in Clcn it is essential to know how many valance electrons present in C, N and cl atoms. In C the total valance electron present is 4 (2s2 2p2). Nitrogen atom has ground state electronic configuration of 1s2 2s2 2p3 hence, total 5 valance electrons present in N atom and from electronic configuration of Cl atom we see that there exist 7 valance electrons.
Thus the total valance electron of Clcn is equal to sum of valance electron of C, Cl, N atoms.
The total valance electron present in Clcn is (4*1)+(1*5)+(7*1)=16.
Clcn Hybridization
We know that pure atomic orbitals don’t participate in bonding because they have different energies. For this reason atomic orbitals of different energy mixes to form hybrid orbitals of similar energy. This process is denied as hybridization.
C atom has the electronic configuration of 2s2 2p2 in ground energy and we see that there only 2 unpaired electrons present in the valance shell of C atom and to produce Clcn, 4 unpaired electrons required. When some energy is applied, 1 2s electrons enters into empty 2p orbital creating a total of 4 unpaired electrons in the valance shell of C atom.
In the next step, 1 Cl atom give its 1 unpaired electron to form C-Cl bond. At first N atom forms 1 sigma bond with central C atom by using its 1 unpaired electron, then the remaining 2 unpaired electrons of 2p orbital of N atom forms pi bonds with central C atom. As central C atom forms 2 sigma and 2 pi bonds, it is sp hybridized.
Clcn hybridization
Clcn solubility
Clcn is polar compound. As it is polar in anture, it is soluble in polar solvent e.g. water, methanol, ethanol etc. When it reacts with water, it is undergoes slow hydrolysis to form cyanate (NCO-) and chloride ions (cl-) and H+ ion is also produced. This reaction happens in neutral pH medium.
Reaction of Clcn with water
Is Clcn Ionic?
Clcn is an ionic compound. This is due to the fact that It disintrigates into ions when it is in molten state or in aqueous state. When Clcn is added in water medium, isocyante, chloride and H+ ions are formed. As it forms ions in aqueous solution, it is an ionic compound.
The aqueous solution of Clcn also conducts electricity, like other ionic compound does when they dissolve in aqueous solution.
Is Clcn acidic or basic?
Clcn is basic in nature. It is a bronsted as well as lewis base. When it reacts with lewis acid it donates its lone pair of electron through N atom and forms coordination compound.
When it reacts with acid which gives H+ ions, it accept H+ ions by donating its lone pair of electron through N atom. Lone pair donation occurs through N atom because N is less electronegative than Cl atom i.e. +ve charge favorable on N atom that Cl atom.
Is Clcn polar or nonpolar?
Clcn is polar in nature. A compound is found to be polar if all the bond moments in the compound are not cancelled out. In this compound due to presence of sp hybridized –CN group, C-Cl bond moment lies towards –CN group.
In Clcn compound, lone pair on Cl atom is delocalized with the empty ∏* antibonding orbital of -CN group and for this reason, –ve pole creates on N atom and +ve pole creates on chlorine atom. Hence there occurs larger distribution of charge. That is why Clcn in polar in nature and its dipole moment not equal to zero.
Is Clcn linear or Tetrahedral?
Clcn has linear shape with sp hybridization of the central C atom. So, probability of tetrahedral shape does not arise.
Conclusion
By the above facts we discussed it is concluded that Clcn is a polar, ionic, covalent compound in which central C atom uses sp hybrid orbital. It is miscible with water because it is a polar compound. It is a stable compound according to octet as well as resonance.
In this article we are going to explore ch3cooh lewis structure, characteristics and 13 essential facts regarding acetic acid.
Ch3cooh is a colorless liquid which has vinegar like odor. It is miscible in water. Its conjugate base is acetate ion. Ch3cooh is largely used for the manufacture of vinyl acetate monomer. The molecular weight of acetic acid is 60.052 g/mol.
Ch3cooh Lewis Structure Drawing
In the Ch3cooh lewis structure, central C atom uses sp2 hybrid orbital to form ch3cooh compound. In the exicted state C have 4 valance electron out of which 1 is used for bonding with C atom –Ch3 group, 1 is used in making σ bonding with O atom of –OH group and 1 is used to form σ bond with O atom.
The reamining 1 valance electron is used to form C=O (pi) bond. The carbonyl O atom form 1σ and 1∏ bond with C atom and remaining 4 electrons exist as 2 lone pairs. The O atom of –OH group form 2 σ bonds with –Ch3 group and H atom. Remaining 4 electron as ususal exist as 2 lone pairs on – OH group.
The empirical process through which electron pair movement occurs from one to another atom i.e. electron pair distribution takes place by delocalization is termed as resonance and by this process the species which are obtained is defined as resonating structure.
In Ch3cooh 2 equivalent resonating structure are obtained. In these structure partial double bond occurs between C-O bond. The reason behind it is that unshared electron pair on O atom of –OH group is in conjugation with the empty ∏* antibonding orbital of carbonyl group.
According to VSEPR theory the shape of Ch3cooh is trigonal planner in which central carbonyl carbon is surround by carbonyl O atom, -Ch3 group and -OH group.
But C of –Ch3 group is tetrahedrally surrounded by 3 H and –C=O group and also O atom of –OH group is tetrahedrally surrounded by –C=O group, H atom and 2 lone pairs. Ch3cooh exist in planner shape so that the bond angle found in acetic acid is 1200.
Ch3cooh Lewis Structure Formal Charge
The formal charge on the atoms in Ch3cooh can be obtained by the formula which is given below:
Formal Charge (F.C) = No of valance electrons-(bonding electrons)/2- No of unshared pair of electron
Hence formal charge on carbonyl C atom in Ch3cooh=4-8/2-0= 0.
Formal charge on carbonyl O atom in Ch3cooh=6-4/2-4=0.
Formal charge on O atom of –OH group=6-4/2-4=0.
Formal charge on C atom of –ch3 group=4-8/2-0=0.
Hence formal charge on central C atom is 0.Each atoms in Ch3cooh has 0 formal charge making the whole compound is electrically neutral.
Ch3cooh Lewis Structure Angle
In Ch3cooh lewis structure, carbonyl carbon uses sp2 hybrid orbital to form bonds with –ch3 group and –OH group i.e. the angle C-C-O is 1200. The carbon atom in –Ch3 group is sp3 hybridized i.e. angle H-C-H should be 109.280.
The carbonyl O is same as that of carbonyl carbon which is sp2 hybridized (i.e. 1200) and also O atom of –OH group is sp3 hybridized (i.e. 109.280). As the central atom in Ch3cooh is titled at 1200 angle, the overall compound is planner.
In the Ch3cooh lewis structure we see that all the atoms fulfilled their octet. The C of ch3 group forms 3 bonds with H atom and 1 bond with C=O group.
The carbonyl carbon form 1σ and 1∏ bond with O atom and also forms 2 σ bonds with -ch3 and –OH group. The carbonyl O forms double bond with C atom and also contain 2 lone pairs. The O atom of –OH group forms 2 σ bonds with C=O group and 1 H atom. From this we see that all the atoms satisfy octet rule expect H which satisfy doublet rule.
Ch3cooh Lewis Structure Lone Pairs
The lone electron pairs are that valance electrons which are not shared between 2 atoms when they are connected through a covalent bond. It is also known as nonbonding electron pair.
The formula with the help of which we can calculate the lone pair of electron on the given atom of Ch3cooh is depicted below:
Lone electron pairs of an atom= electrons that present on the valance shell of the atom – how many are bonds formed by that atom.
lone electron pair present on O atom of C=O group in acetic acid=6-2=4 i.e. 2 unshared electron pair.
Lone electron pair present on O atom of –OH group in Ch3cooh=6-2=4 i.e. 2 unshared electron pair.
Lone pair of electrons present on C atom of –C=O group= 4-4=0 i.e.no nonbonding electron pairs.
These unshared electron pairs are shown in the lewis structure of Ch3cooh on C, H, O atoms as electron dots.
Ch3cooh Valance Electrons
To find out total valance electron in Ch3cooh it is must to know how many valance electrons present in C, H and oxygen atoms. C has the electronic configuration of 1s2 2s2 2p2 and electronic configuration of C atom shows that there exist 4 electrons.
Oxygen atom has the electronic configuration of 1s2 2s2 2p4 i.e. there exist 6 valance electrons in O atom and H has only 1 valance electron.Ch3cooh contains total valance electron which will be equal to the summation of all the valance electron of C, O and H atoms. Hence in Ch3cooh (4*2)+(2*6)+(4*1)=24 valance electron present.
Ch3cooh Hybridization
Hybridization means where central atom mixes its atomic orbitals such as s, p, d which are in different energy state to produce similar energy hybrid orbitals e.g. sp2, sp3, sp3d etc. Electronic configuration of C atom is 2s2 2p2 in ground energy state. In the valance shell of C atom we found that only 2 unpaired electrons present and to produce Ch3cooh, 4 unpaired electrons needed.
When energy is applied, 1 2s electrons goes into vacant 2p orbital making a total of 4 unpaired electrons in the valance shell of C atom. In the next step 1 O atom of –OH group, C atom of –Ch3 group and another O atom give their 1 unpaired electrons to form C-Ch3, C-OH and C-O bonds. O atom give their remaining unpaired electron to form C=O (pi) bonds.
In this compound central C uses sp2 hybrid orbital to make these bonds. According to sp2 hybridization, the geometry of Ch3cooh will be planner.
Ch3cooh Hybridization
Ch3cooh solubility
As Ch3cooh is polar in a nature, it is soluble in polar solvents like water, ethanol, methanol etc. It is highly soluble in polar solvents. As Ch3cooh is acidic in nature, it reacts with aqueous alkali’s, neutralization reaction takes place and water, and acetate salts are formed. When it dissolved in water, Ch3cooh dissociates in water to give Ch3coo- and H+ ions.
Ch3cooh ionization
Is Ch3cooh Ionic?
Ch3cooh is an ionic compound. This is for the reason that when ch3cooh disintrigates acetate and H+ ion are produced. When acetic acid is added water, it readily dissolves and aq. solution of Ch3cooh conducts electricity as there exists ions which is similar to an ionic compound.
Acetic acid has high boiling point like other ionic compounds. 2 Ch3cooh molecules dimerises through intramolecular H bonding, to separate them large amount of energy is required. This clearly mentioned that Ch3cooh is ionic in nature.
Is Ch3cooh acidic or basic?
Ch3cooh is an acidic compound. This is due to the presence of cooh group. In aqueous solution it gives H+ ion and ch3coo- ion. Like acidic compound it reacts with bases to give water and salt. Acetic acid reacts with base like NaoH, it gives water and sodium acetate (ch3ccoNa).
Is Ch3cooh polar or nonpolar?
Ch3cooh is polar in nature. A compound is said to be polar if its dipole moment is not equal to zero. In this compound due to presence of carbonyl group, C=O bond moment lie towards oxygen atom.
In ch3cooh, lone pair on O atom of -OH group is delocalized with ∏* antibonding orbital of C=O group and for this –ve pole creates on carbonyl O atom and +ve pole creates on oxygen atom of OH group. Hence there occurs separation of charge. That is why ch3ccoh in polar in nature.
Is Ch3cooh linear or Tetrahedral?
Ch3cooh has planner shape with sp2 hybridization of the central C atom. It is not linear or tetrahedral in nature.
Conclusion
By keeping in mind the above discussed facts, we conclude that acetic acid is a polar ionic compound in which carbonyl C uses sp2 hybrid orbital which makes the compound planner. Its pka is low so that it is a weak acid and also has a tendency to form water and salts whenever reacts with bases. Ch3cooh is a stable compound due to resonance.
In this article we are going to discuss about socl2 lewis structure including its drawing, hybridization, shape, formal charges, electron pairs and some important facts regarding socl2.
SOCl2 is commonly known as thionyl chloride. It is toxic in nature. Socl2 has no color which is volatile as well pungent in nature. It is generally used as a chlorinating agent which converts alcohols into chlorides. SOCl2 reacts with water to produce sulphur dioxide and hcl. It has the molecular weight of 118.94 gm/mol.
SOCl2 Lewis Structure Drawing
In socl2 lewis structure we see that as S has larger size and also less electronegative than other atoms it works as central atom in socl2.
Sulphur has 6 electrons in the outermost shell out of which 4 electrons participate in sigma bonding with 2 cl atoms and 1 O atom. With O atom S forms 1 sigma and 1 Pi bond. There is 1 electron pair that still present on central S atom which present as a electron pair on sulphur atom.
O has 6 electrons in the valance shell out of those only 2 are used for the formation of sigma and pi bonding and that 4 existing electrons present as lone pair of electrons on O. In cl 7 valance electron present out of which only 1 electron is take part in sigma bonding formation and those existing 6 electrons present as 3 nonbonding electron pairs.
From VSEPR theory we see that the geometry of socl2 is trigonal pyramidal. In this structure central sulphur atom is surround by 2 cl atoms and 1 lone pair in tetrahedral manner. As one lone pair present in the central S atom the true tetrahedral shape becomes distorted.
If we consider, the lone pair of electron is absent in socl2 the geometry is actual tetrahedral but as we seen 1 lone pair of electron is present on central sulphur atom, the real td structure does not occur and the actual shape becomes pyramidal.
The formal charge on particular atoms in socl2 compound can be estimated by using the formula given below:
Formal Charge (f) =NV.E-NB.E/2-NN.E
Where,
NV.E =Total No of valance electrons, NB.E = Total No of bonding electrons,
NN.E= Total No of nonbonding electrons.
Hence formal charge on central S atom in socl2=6-8/2-2=0.
Formal charge on double bonded O atom in socl2=6-4/2-4=0.
Formal charge on cl atoms in socl2=7-2/2-6=0.
Hence formal charge on central S atom is 0 and each cl atom and also O atom has 0 formal charges, making the whole compound is electrically neutral.
SOCl2 lewis Structure Lone Pairs
The electrons that present in the valance shell of an atom that don’t participate in bonding with similar or another atom is called as lone pair of electron or nonbonding electrons.
The lone pairs on particular atoms in socl2 compound can be estimated by using the formula given below:
No of lone pair of electron on any atom= maximum no of valance electron of the atom-no of bonds that formed by that particular atom.
In socl2 lone pair present on central S atom= 6-4=2 i.e. 1 lone pair of electron.
Lone pair present on double bonded O atom in socl2=6-2=4 i.e. 2 lone pairs.
Lone pair present on Cl atoms in socl2= 7-1=6 i.e.3 lone pair of electron.
These lone pairs on s,cl,o atoms are given in the socl2 lewis structure as electron dots.
SOCl2 Hybridization
Hybridization is a method in which different energy atomic orbitals are mixed to produce an equal number of hybrid orbitals having same energy.
The electronic configuration of S atom in the valance shell is 3s2 3p4. In the ground state of S atom we see that there are only 2 unpaired electrons and to form socl2, 3 unpaired electrons are needed. In the excited state S send its 1 3p electron into 3d orbital making a total of 4 unpaired electrons.
2 Cl give 1 unpaired electron to form 2 S-Cl bonds and 1 O give 1 unpaired electron to form S-O sigma bond and remaining unpaired electron of O form S=O (pi) bond. In socl2, S uses sp3 hybrid orbital to make S-Cl and S=O bonds. According to sp3 hybridization the geometry should be Tetrahedral but the actual shape is pyramidal.
Socl2 hybridization
SOCl2 lewis Structure Resonance
Resonance is an empirical method in which electron pair shifting occurs from one atom to another atom by delocalization of electron and the structure we get by this process is defined as resonating or canonical structure.
Socl2 have 3 resonating structure in which each s-cl bond gets partial double bond character by the process in which nonbonding electrons on Cl atom is in conjugation with the vacant ∏* antibonding orbital of S=O bond.
When we see the lewis structure of socl2 we find that each chlorine atom has 8 electrons in the valance shell and satisfy their octet. In socl2 compound S forms 2 S-Cl bonds and 1 S=O bond, also there is 1 lone pair of electron that present on central S atom making a total of 10 electrons around central S atom.
As S is a part of 3rd period in the periodic table, sulphur atom can expand their octet which contains more than 8 electrons. Hence socl2 is a stable compound in terms of octet rule.
SOCl2 Polar Or Nonpolar?
SOCl2 is a polar compound. In SOCl2 S=O bond moment lies towards O atom, because O is more electronegative than S atom. 2 S-Cl bond moments lies towards more electronegative Cl atom.
All these bond moments lies in the same direction which makes the compound polar. The overall dipole moment od of socl2 is 1.44 Debye.
SOCl2 Uses
It is an important reagent for converting alkyl alcohols to alkyl halide through SN1 mechanism.
It is used for the preparation of acyl chloride from carboxylic acid.
As socl2 is a polar aprotic solvent which stabilises cations only. It is used as a solvent in SN2 reaction.
SOCl2 is used in lithium-thionyl chloride batteries. In these batteries it is used as positive electrodes.
SOCl2 is used as a reducing agent for the EPR detection of Tc(6) compounds.
By considering the above facts we see that socl2 is a polar covalent compound which has pyramidal shape in which central S uses sp3 hybrid orbital.
In this article we are discussing about bro4- lewis structure, characteristics and 13 important facts regarding this.
Perbromate (bro4-) is an oxoanion of bromine. Like clo4-, io4- it is difficult to prepare. The molar mass of bro4- ion is 143.901 g/mol. When bro3- ion reacts with fluorine in alkaline medium, bro4- ion is produced. When perbromic acid losses one proton bro4- ion is produced.
Bro4- Lewis Structure Drawing
In the bro4- lewis structure we see that as bromine becomes bigger in size and less electronegative than O, br act as the central atom in the lewis structure of bro4- ion. Bromine has 7 valance electrons out of which 4 electrons take part in sigma bonding with 4 O atoms and forms 3 pi bonds with 3 O atoms.
There is no remaining electrons on br atom which act as lone pair of electron. O atom has 6 electrons in the valance shell out of which 1 is used in making sigma bond and another is used in making pi bond with br atom and remaining 4 electrons present as nonbonding electron pair on O atom.
Resonance is an empirical process in which movement of electron pair takes place from one atom to another atom and the structure obtained by this process is called resonating or canonical structure.
According to VSEPR theory the shape of Bro4- is tetrahedral in which central Br atom is tetrahedrally surround by 3 O atoms and 1 O- ion. As lone pair absent in the central Br atom, Bro4- ion possesses true tetrahedral structure. As the shape is tetrahedral, the bond angle occurs in this compound is exactly 109.280.
The formal charge on any atom or ion can be obtained by the formula which is given below:
Formal Charge (f.c) =V.E- B.E/2- N.E
Where,
V.E= Total No of valance electrons, B= Total bonding electrons, N= Total No of nonbonding electrons.
Hence formal charge on br atom in bro4- ion = 7-14/2-0=0.
Formal charge on each double bonded O atom in bro4- ion =6-4/2-4=0.
Formal charge on single bonded O atom in bro4- ion =6-2/2-6=-1.
Hence formal charge on central br atom is 0.Each double bonded O atom has 0 and single bonded O atom has -1 formal charge making the overall compound is negatively charged.
Bro4- Lewis Structure Angle
In bro4- br uses sp3 hybrid orbitals to form bro4- ion. The structure of bro4- is tetrahedral. As lone pair of electron is not present in bro4- ion the angle is exactly same as that of in real tetrahedral structure. The angle in bro4- ion is 109.280 i.e. the o-br-o bond angle is 109.280.
In the bro4- lewis structure we see that each O atom has 8 valance electrons and fulfill their octet. In bro4- ion br forms 3 br=O bonds and 1 br-O bond making a total of 14 electrons around central br atom.
As br is a congener of 4th period element br atom can increase their octet more than 8 electrons due to presence of vacant d orbital. Hence according to octet rule bro4- is a stable compound.
Bro4- Lewis Structure Lone Pair
The valance electron which does not take part in bonding is defined as lone pair of electrons or nonbonding electrons.
The formula which is used to calculate the lone pair of electron on the given atom is given below:
No of lone pair of electrons = no of valance electrons present on the atom-no of covalent bonds formed by that atom.
In bro4- ion lone pair present on br atom= 7-7=0 i.e. zero lone pair of electrons.
Lone pair of electrons present on each double bonded O atom=6-2=4 i.e. 2 lone pair of electrons.
Lone pair of electrons present on single bonded O- ion= 8-2=6 i.e.3 nonbonding electron pairs.
These lone pairs are shown in the lewis structure of bro4- ion on the given atoms as electron dots.
Bro4- Valance Electrons
At first, to calculate the total valance electron in bro4-, it is important to know the electronic configuration of br atom and O atom. The electronic configuration of br atom is [Ar18] 4s2 3d10 4p5 and from electronic configuration we see that there are 7 electrons in the valance shell of br atom.
The electronic configuration of O atom is [He2] 2s2 2p4 i.e. 6 valance electrons present in O atom.1 negative charge is also present. The total valance electrons in bro4- ion will be equal to the sum of the valance electron of br atom and O atom+1 negative charge i.e. (7*1)+(6*4)+1=32. There are 32 valance electrons in bro4- ion.
Bro4- Hybridization
Hybridization is the process of mixing of similar energy atomic orbitals to produce an equal number of hybrid orbitals.
The ground state valance shell electronic configuration of br atom is 4s2 4p5. In the ground state of br atom only 1 unpaired electron is present and to make bro4-, 4 unpaired electron is required. In the excited state br send its 1 4s electrons and 2 4p electrons into vacant d orbital making a total of 7 unpaired electrons.
In the next step 4 o atoms give their 1 unpaired electron to form 4 br-o sigma bonds and 4 O atoms give their remaining unpaired electron to form 3 br=O (pi) bonds. In this compound br uses sp3 hybrid orbital to make br-O bonds. According to sp3 hybridization, the geometry of bro4- ion will be tetrahedral.
Bro4- hybridization
Bro4- solubility
Bro4- ion is soluble in polar solvents like water, ethanol, methanol etc. When Hbro4 losses 1 proton bro4- ion is formed i.e. bro4- ion is a conjugate base of Hbro4.
Hence, bro4- ion behaves as a base and has a strong tendency to accept proton. When it reacts with water, bro4- ion accepts 1 proton from water to form Hbro4 and Oh- ions making the aqueous medium alkaline.
Is BrO4- Ionic?
Bro4- is an ionic compound. This is because of the fact that it is formed when Hbro4 losses 1 proton. It is an anionic species.
Like ionic species, it has a strong tendency to react with water and also aq. solution of bro4- ion conducts electricity like other ionic compounds does. Like other ionic compounds it has high melting point. These facts suggest that bro4- ion is an ionic compound.
Is Bro4- acidic or basic?
Bro4- ion is a basic compound. It is the conjugate base of Hbro4 acid. Like other bases, it has a strong tendency to accept protons to form acid.
It also has high electron density on it like other bases and donates its electron density towards a proton or a lewis acid. Hence it act as a lewis base and forms adduct with lewis acid.
Is Bro4- polar or nonpolar?
Bro4- is nonpolar in nature. A compound is said to be nonpolar if its dipole moment is equal to zero. In this compound 4 br-O bonds are polar this is due to electronegativity difference between br and O atom.
As O is more electronegative than br atom, br-o bond moment lies towards o atom. As bro4- has real tetrahedral shape 4 br-o bond moments cancel each other and hence dipole moment becomes equals to 0.
By considering the above mentioned facts, bro4- ion is an ionic, covalent compound which has tetrahedral geometry. It is basic in nature and has a tendency to accept proton from any protonic solvent. Bro4- ion is not much stable due large size difference between Br and O atom.
In this article we are going to discuss the ba(oh)2 lewis structure and 13 important facts regarding its lewis structure and characteristics.
Barium hydroxide is produced when barium oxide is dissolved in water. It exists in white granular form. It is used as a dehydrating agent and used for the removal of sulphur from various compounds.
Ba(oh)2 Lewis Structure Drawing
Ba(oh)2 is formed by two elements i.e. one is barium atom and the other is hydroxide group. Ba is a congener of alkaline earth metal i.e. group (II) and oxygen is a congener of group 16 family. Barium has atomic number of 56. Its outermost shell electronic configuration is [Xe] 6s2. When it losses two electrons it gains the nearest noble gas configuration of Xe.
When Ba atom lost its 2 electrons Ba+2 ion is produced. In case of hydroxide radical, O atom is singly bonded with H atom i.e. it contains a total of 7 electrons. When 2 Oh radicals gains 1 electron each which are rejected by Ba it gets stable nearest noble gas configuration of Ne. Then Ba+2 and 2 Oh- ions are attached by columbic force of attraction and ba(oh)2 is formed.
Resonance is an empirical method in which electrons moving from one atom to another by losing and gaining of electrons. Barium hydroxide is a neutral compound with zero formal charge (f.c) on it. As resonance takes place Ba(oh)2 breaks into Ba+2ion and 2 OH- ions.
Both barium and hydroxide ions are stabilized because both gains stable nearest noble gas configuration after resonance i.e. Ba2+ ion possess Xenon (Xe) noble electronic configuration and hydroxide ion acquires Neon (Ne) noble gas configuration, both the ions fulfilled their octet after resonance.
Ba(oh)2 Lewis structure shape
According to VSEPR theory ba(oh)2 has octahedral co-ordination geometry. In the crystal structure of ba(oh)2 6 Ba2+ ions are surrounding by 6 Oh- ions and 6 Oh- ions are surround by 6 Ba2+ ions.
For this reason both Ba2+ and Oh- ions have co-ordination number equals to 6. Because of this fact that ba(oh)2 has octahedral shape and acquires d2sp3 hybridization.
Ba(oh)2 Lewis Structure Formal Charges
In barium hydroxide overall formal charge on the compound is Zero. Ba(oh)2 ionizes to form Ba2+ and 2 Oh- ions. Barium has +2 formal charges which are cancelled out by 2 hydroxide -1 formal charge.
In the cubic crystal lattice structure of barium hydroxide 6 Ba2+ ions are surround by 6 Oh- ions and 6 Oh- ions are surrounded by 6 Ba2+ ions making the whole compound is electrically neutral.
Ba(oh)2 Lewis structure angle
As we seen from ba(oh)2 lewis structure, ba(oh)2 has octahedral geometry with d2sp3 hybridization and according to octahedral geometry the angle must be 900. Ba(oh)2 also possess the same bond angle which is equal to 900.
Ba(oh)2 Lewis Structure Octet Rule
In the lewis structure of barium hydroxide both barium and hydroxide ions fulfilled their octet. When ba(oh)2 is produced ba lost its two electrons from valance shell to acquire the nearest noble gas configuration of Xe which have 8 electrons in its valance shell (5s25p6) i.e. octet is fulfilled.
Hydroxide radical gains two electrons which is rejected by ba atom to acquires the nearest noble gas configuration of neon which also possessed 8 valance electrons (2s2 2p6). Hence both barium and oh radical fulfilled their octet.
Ba(oh)2 Lewis Structure Lone Pairs
When we see the ba(oh)2 lewis structure zero lone pair present on Ba atom and 1 lone pair of electrons present on hydroxide ion.
This is due to the fact that barium losses its two electron to form Ba2+ion which does not contain any lone pair of electron in it. But 2 Oh radical gains 1 electron each which is rejected by Ba atom and is converted into 2 Oh- ions in which 1 lone pair of electrons present on each Oh- ion.
Ba(oh)2 Valance Electrons
Firstly to find out the total no of valance electron in Ba(oh)2, it is important to find out the electronic configuration of Ba atom. The electronic configuration of Ba atom is [Xe] 6s2 and we see from electronic configuration of ba that there are 2 electrons in the valance shell of Ba atom.
There is 7 electrons in the Oh radical. The total valance electrons that exist on ba(oh)2 will be equal to the (sum of the valance electron of Ba atom and oh radical) i.e. equals to (1*2)+(7*2)=16. There are 16 valance electrons in ba(oh)2.
In the crystal lattice structure of barium hydroxide each Ba+2 ion is surrounded by six Oh- ions and each Oh-ion is surrounded by 6 Ba+2ions. Hence both barium ion and htdroxide ion have same co-ordination number which is equal to 6.
Ba(oh)2 Solubility
In ba(oh)2 due to greater electronegativity of oh group and lesse electronegativity of barium atom it exists in Ba2+ and 2 oh- ions i.e. opposite dipoles are produced. As different dipoles created on Ba2+ and oh- ions it is a polar compound.
It is soluble in polar solvents e.g. ethanol (C2H5OH), dilute mineral acids like HCl, HBr, HF etc and also soluble in water. But it is not soluble in nonpolar solvents like acetone, ether etc. When barium hydroxide reacts with water it produces Ba2+ ions and hydroxide ions. This medium is basic in nature.
Solubility of Ba(oh)2 in water
Is Ba(oh)2 Ionic?
Ba(oh)2 is an ionic compound. This is due to the fact that ba(oh)2 disintrigates to give Ba2+ and Oh- ions when it dissolves in aqueous solution or in molten state. This is an essential characteristic of ionic compound.
It conducts electricity in aqueous or in molten state. This is because of the presence of Ba2+ and Oh- ions in both the states and we also know that ions carry current. Like ionic compounds ba(oh)2 is soluble in polar solvents for example water, methanol etc.
Is Ba(oh)2 Polar Or Nonpolar?
Barium hydroxide is a polar compound. This is because of the fact that in barium hydroxide both barium atom and hydroxide radical have difference in electronegativity and hence opposite dipole creates on barium and hydroxide radical.
Due to lower electronegativity of barium it acquires positive dipole on it and due to higher electronegativity of O atom Oh radical possesses negative dipole. As because opposite dipoles creates on barium hydroxide, it is an ionic compound with high dipole moment. Hence ba(oh)2 is a polar compound.
Is Ba(oh)2 acidic or basic?
Ba has greater tendency to loss electrons i.e. it has metallic characteristics. Ba(oh)2 is basic in nature. This is due to the fact that it is a hydroxide of a metal which usually basic in nature.
When we dissolve barium hydroxide in water, it dissociates in water to form Ba2+ and Oh- ions. We know from Arrhenius theory that the compound which gives Oh- ions in solution are alkaline or basic in nature.
By considering the above mentioned facts we can conclude that ba(oh)2 is a stable ionic compound. As it is an ionic compound it is polar in nature as well as soluble in polar hydrophilic solvents and ba(oh)2 is an alkaline hydroxide because it gives Oh- ions in aqueous solution.
In this article we are going to discuss the bao lewis structure and 13 important facts regarding its structure and characteristics.
Barium oxide is formed when barium is burned in presence of Oxygen. It is white crystal cubic structure solid which is non-flammable as well as hygroscopic in nature. The cathode ray tube is composed of bao. It is also used in making crown glasses and as a catalyst.
Bao Lewis Structure Drawing
Bao is formed by two elements i.e. one is barium (Ba) and other is oxygen (O). Ba is a member of alkaline earth metal i.e. group (II) and oxygen is a member of group 16. Barium has atomic number 56. Its electronic configuration is [Xe] 6s2. When it losses two electron from 6s orbital it acquires the nearest noble gas configuration i.e. Xe (Z=54).
When Ba atom losses 2 electrons Ba+2 ion is formed. In case of oxygen, it has atomic number 8. Its electronic configuration is [He]2s22p4. When it gains 2 electrons it gets nearest noble gas configuration of Ne in which octet is fulfilled. Then Ba+2 and O2- ions are attached by electrostatic force of attraction which is a strong force and bao is formed.
Resonance is an empirical process in which electrons moves from one atom to another by losing and gaining of electrons. Barium Oxide is a neutral molecule having zero formal charge (f.c) on it. When resonance takes place BaO breaks into Ba+2 ion and O2- ion.
Both barium and oxide ion are stabilized because both possess stable nearest noble gas configuration after resonance i.e. barium ion acquires Xenon (Xe) noble electronic configuration and Oxide ion acquires Neon (Ne) noble gas configuration, both the ions fulfill their octet after resonance.
Bao Lewis structure shape
According to VSEPR theory bao has octahedral co-ordination geometry. In the crystal structure of bao 6 Ba2+ ions are surrounding by 6 O2- ions and 6 O2- ions are surround by 6 Ba2+ ions.
For this reason both Ba2+ and O2- ions have co-ordination number equals to 6. As because bao has octahedral shape it possess d2sp3 hybridization.
Bao Lewis Structure Formal Charges
In barium oxide overall formal charge on the compound is Zero. Bao ionizes to form Ba2+ and O2- ions. Barium has +2 formal charges which are neutralized by Oxygen 2- formal charge.
In the cubic crystal lattice structure of barium oxide 6 Ba2+ ions are surround by 6 O2- ions and 6 O2- ions are surrounded by 6 Ba2+ ions making the whole compound is neutral.
Bao Lewis structure angle
As we seen form bao lewis structure, bao has octahedral shape with d2sp3 hybridization and according to octahedral geometry the angle should be 900. Bao also possess the same bond angle which is equal to 900.
Bao Lewis Structure Octet Rule
In the bao lewis structure both barium and Oxygen atom fulfilled their octet. When bao is formed barium lost its two electrons to acquire the nearest noble gas configuration of Xe which have 8 electrons in its valance shell (5s25p6).i.e. octet is fulfilled.
Oxygen atom gains two electrons which is rejected by barium atom to possess the nearest noble gas configuration of neon which also possessed 8 valance electrons (2s22p6). Hence both barium and oxygen atom fulfilled their octet.
Bao Lewis Structure Lone Pairs
When we see the bao lewis structure zero lone pair present on Ba and 2 lone pair of electrons present on oxide ion.
This is because of the fact that barium losses its two electron to form Ba2+ion which does not have any lone pair of electron on it. But Oxygen atom gains two electrons which is rejected by Ba atom and is converted into O2- ion in which two lone pair of electrons present.
Bao Valance Electrons
Firstly to find out the total valance electron in Bao, it is essential to know the electronic configuration of Ba and O atom. The electronic configuration of Ba is [Xe] 6s2 and we see from electronic configuration that there are 2 electrons in valance shell of Ba atom.
The electronic configuration of O atom is [He]2s2 2p4. There is 6 electrons in the valance shell of O atom. The total valance electrons that exist on bao will be equal to the (sum of the valance electron of Ba and O atom) i.e. equals to (1*2)+(6*1)=8. There are 8 valance electrons in bao.
In the crystal lattice structure of barium oxide each Ba+2 ion is surrounded by six O2- ions and each O2-ion is surrounded by six Ba+2ions. Hence both barium ion and oxide ion have same co-ordination number which is equal to 6.
Bao Solubility
In bao due to higher electronegativity of O and lower electronegativity of Ba atom it exists in Ba2+ and O2- ions i.e. opposite dipoles are produced. As different dipoles created on Ba2+ and O2- ions it is polar in nature and it is soluble in polar solvents.
It is soluble in ethanol (C2H5OH), dilute mineral acids like HCl, HBr, HI etc and also soluble in alkalies like NaOH, KOH etc. But it is insoluble in nonpolar solvents like acetone, ether, liquid ammonia. When barium oxide reacts with water it forms barium hydroxide [Ba(OH)2] which is alkaline in nature.
Reaction of BaO with Water
Is BaO Ionic?
Bao is an ionic compound. This is due to the fact that bao dissociates to give Ba2+ and O2- ions when it dissolves in aqueous solution or in molten state. This is an important characteristic of ionic compound.
It also conducts electricity in aqueous or in molten state. This is due to the presence of Ba2+ and O2- ions in both the states and we know that ions carry current. Like ionic compounds bao is soluble in polar solvents e.g. water, ethanol etc.
Is Bao Polar Or Nonpolar?
Barium Oxide is a polar compound. This is because in barium oxide both barium and oxygen have different electronegativity and hence opposite dipole creates on barium and oxygen.
Due to less electronegativity of barium it accommodates positive dipole on it and due to higher electronegativity of O atom it possesses negative dipole. As because opposite dipole formed in barium Oxide, it is an ionic compound with high dipole moment. Hence bao is a polar compound.
Is BaO acidic or basic?
Ba has a tendency to loss electrons i.e. it is metallic in nature. This is because of the fact that Ba has lower electronegativity and also it acquires stable noble gas electronic configuration of Xe by losing 2 electrons.
We know that the oxide of a metal is basic in nature i.e. when basic oxide reacts with water it forms alkalies. In the similar way when bao reacts with water, it forms basic hydroxide i.e. barium hydroxide which is alkaline in nature. This is because it gives OH- ions in solution.
Conclusion
By considering the above mentioned facts we can conclude that bao is a stable ionic compound. As it is an ionic compound it is polar in nature as well as soluble in polar solvents and bao is a basic oxide because it is an oxide of a metal i.e. Ba.
Iron (Fe) is a chemical element that belongs to the transition metals group in the periodic table. It is widely known for its importance in various industries, including construction, manufacturing, and medicine. The electron configuration of iron, specifically Fe2+ and Fe3+ ions, plays a crucial role in understanding its chemical properties and reactivity. In this article, we will delve into the electron configuration of Fe, Fe2+, and Fe3+, exploring their significance and implications in different contexts. So, let’s dive in and unravel the mysteries of iron’s electron configuration.
Key Takeaways
The electron configuration of Fe, Fe2+, and Fe3+ can be determined by following the Aufbau principle, Hund’s rule, and the Pauli exclusion principle.
Fe has the electron configuration [Ar] 3d^6 4s^2, Fe2+ has the electron configuration [Ar] 3d^6, and Fe3+ has the electron configuration [Ar] 3d^5.
The electron configuration of Fe2+ and Fe3+ ions is obtained by removing electrons from the 4s orbital first before removing from the 3d orbital.
The electron configuration of Fe, Fe2+, and Fe3+ influences their chemical properties and reactivity.
on in the periodic table. By studying electron configuration, we can unravel the fascinating world of atoms and their interactions.
Iron (Fe) Electron Configuration
Iron (Fe) is a fascinating element that plays a crucial role in our everyday lives. From construction materials to the transportation industry, iron is widely used due to its strength and versatility. Understanding the electron configuration of iron is essential in comprehending its chemical properties and behavior. In this section, we will explore the standard electron configuration, subshell electron configuration, and condensed and abbreviated electron configuration of iron.
A. The Standard Electron Configuration of Iron (Fe)
The standard electron configuration of an atom describes the distribution of electrons in its various energy levels and orbitals. For iron (Fe), which has an atomic number of 26, the standard electron configuration is as follows:
1s2 2s2 2p6 3s2 3p6 4s2 3d6
Let’s break this down. The first number represents the principal energy level (n), followed by the letter indicating the type of subshell (s, p, d, or f), and finally, the superscript denotes the number of electrons in that subshell. In the case of iron, the electron configuration starts with the 1s subshell and gradually fills up the subsequent subshells until it reaches the 3d subshell.
Ground state electronic configuration of Fe
B. Subshell Electron Configuration of Iron (Fe)
To delve deeper into the electron configuration of iron, let’s focus on the subshells. The subshells in iron’s electron configuration are:
1s
2s
2p
3s
3p
3d
Each subshell can hold a specific number of electrons. The s subshell can hold a maximum of 2 electrons, the p subshell can hold a maximum of 6 electrons, and the d subshell can hold a maximum of 10 electrons. In the case of iron, the 3d subshell can hold up to 10 electrons, but in its ground state, it only has 6 electrons.
C. Condensed and Abbreviated Electron Configuration of Iron (Fe)
While the standard electron configuration provides a detailed account of the electron distribution in iron, it can be quite lengthy. To simplify the representation, we can use condensed and abbreviated electron configurations.
The condensed electron configuration of iron is written as:
[Ar] 4s2 3d6
The [Ar] represents the electron configuration of the noble gas argon (Ar), which has the same electron configuration as the filled inner shells of iron. By using the noble gas notation, we can condense the electron configuration and focus on the outermost energy levels.
Additionally, we can further abbreviate the electron configuration by only indicating the valence electrons. The valence electrons are the electrons in the outermost energy level, which are responsible for the chemical properties and reactivity of an element. In the case of iron, the abbreviated electron configuration is:
4s2 3d6
This notation emphasizes the valence electrons and their involvement in chemical reactions.
Understanding the electron configuration of iron is crucial in comprehending its chemical behavior and its ability to form different oxidation states. By knowing the electron arrangement, scientists can predict the element’s reactivity and its interactions with other elements.
In conclusion, the electron configuration of iron provides valuable insights into its atomic structure and chemical properties. The standard electron configuration, subshell electron configuration, and condensed and abbreviated electron configuration all contribute to our understanding of iron’s behavior. By delving into the world of iron’s electron configuration, we gain a deeper appreciation for this essential element and its role in our daily lives.
Fe3+ Ground State Electron Configuration
When 3 electrons are removed from neutral fe atom fe3+ ion is formed. The ground state fe3+electron configuration is 1s2 2s2 2p6 3s2 3p6 3d5. First 2 electrons are removed from 4s orbital as because it has higher energy than 3d orbital and then 1 electron removed from 3d orbital making the valance shell electronic configuration of fe3+ is 3d5.
When 3 electrons are removed from fe atom it contains 5 electrons in the outermost shell i.e. 3d orbital has 5 electrons which is half-filled. As fe3+ ion has stable half-filled 3d orbital and also 1s,2s, 3s orbitals have fulfilled 2 electrons and 3p orbital have stable fulfilled 6 electrons in them it is more stable than fe atom where fe atom has 6 electrons in 3d orbital.
Ground state electronic configuration of Fe3+
Fe3+ Abbreviated Electron Configuration
To know the abbreviated fe3+electron configuration first of all we must know the abbreviated electronic configuration of fe atom. The abbreviated fe electron configuration is [Ar] 3d6 4s2. By counting the electrons from 1s to 3p orbital we find that there is a total number of 18 electrons and we replace it by writing in the form of [Ar].
When 3 electrons are realized from fe atom, fe3+ ion is formed and the electronic configuration of fe3+ ion in abbreviated form is [Ar] 3d5 i.e. 2 electrons are removed from 4s orbital as it is higher in energy than 3d orbital and then 1 electron is removed from remaining 3d orbital making it stable half-filled electronic configuration of fe3+ ion.
Fe3+ Condensed Electron Configuration
To know the condensed fe3+electron configuration first of all we must know the condensed electronic configuration of fe atom. The condensed electronic configuration of fe is [Ar] 3d6 4s2. By counting the electrons from 1s to 3p orbital we find that there is a total number of 18 electrons.
When 3 electrons are realized from fe atom, fe3+ ion is formed and the electronic configuration of fe3+ ion in condensed form is [Ar] 3d5 i.e. 2 electrons are removed from 4s orbital and 1 electron is removed from remaining 3d orbital making it stable half-filled electronic configuration of fe3+ ion.
Fe3+ Noble gas Electron Configuration
When 3 electrons are removed from neutral fe atom fe3+ ion is formed. The noble gas fe3+electron configuration is 1s2 2s2 2p6 3s2 3p6 3d5. 1st 2 electrons are removed from 4s orbital as because it has higher energy than 3d orbital and then 1 electron removed from 3d orbital making the valance shell electronic configuration of fe3+ is 3d5.
When 3 electrons are removed from fe atom it contains 5 electrons in the outermost shell i.e. 3d orbital has 5 electrons which is half-filled. By counting the electrons from 1s to 3p there are a total of 18 electrons i.e. fe3+ acquire nearest noble gas configuration of [18Ar] 3d5.
Fe2+ Ground State Electron Configuration
When 2 electrons are removed from neutral fe atom fe2+ ion is formed. The ground state fe2+electron configuration of fe2+ is 1s2 2s2 2p6 3s2 3p6 3d6. 2 electrons are removed from 4s orbital as it has higher energy than 3d orbital making the valance shell electronic configuration of fe2+ is 3d6.
When 2 electrons are removed from fe atom it contains 6 electrons in the outermost shell i.e. 3d orbital has 6 electrons. fe2+ is less stable than fe3+ as fe2+ has 6 electrons in d shell which is just 1 electron excess to the stable half-filled d5 configuration of fe2+ ion. Also it is less stable than fe atom due to the fact every charged species is less stable than neutral atom.
we know elemental Fe is neutral in nature it also contain same no of electrons in it i.e. it has 26 electrons as well. We distribute the 26 electrons in various subshell which is done according to aufbau principle. The subshell fe electron configuration is 1s2 2s2 2p6 3s2 3p6 4s2 3d6
When 2 electrons are removed from 4s subshell fe2+ ion is formed. The subshell electronic configuration of fe2+ is 1s2 2s2 2p6 3s2 3p6 3d6. From the subshell electronic configuration of fe2+ ion we see that there are 2 electrons in 1s subshell,2 each in 2s and 3s subshell, 6 electrons in both 2p and 3p subshell and 6 electrons in the last 3d subshell.
Fe2+ Condensed Electron Configuration
To know the condensed electronic configuration of fe2+ first of all we must know the condensed electronic configuration of fe atom. The condensed electronic configuration of fe is [Ar] 3d6 4s2. By counting the electrons from 1s to 3p orbital we find that there is a total number of 18 electrons.
We also know that 18 electrons are present in noble gas Ar and we replace it in the electronic configuration of fe by writing it in the form of [Ar]. When 2 electrons are realized from fe atom, fe2+ ion is formed and the electronic configuration of fe2+ ion in condensed form is [Ar] 3d6 i.e. 2 electrons are removed from 4s orbital.
Fe2+ Noble gas Electron Configuration
When 2 electrons are removed from neutral fe atom fe2+ ion is formed. The noble gas fe2+electron configuration of fe2+ is 1s2 2s2 2p6 3s2 3p6 3d6. These 2 electrons are removed from 4s orbital as because it has higher energy than 3d orbital.
When 2 electrons are removed from fe atom it contains 6 electrons in the outermost shell i.e. 3d orbital has 6 electrons. By counting the electrons from 1s to 3p there are a total of 18 electrons i.e. fe2+ acquires nearest noble gas configuration of [18Ar] 3d6.
Predicting the Electron Configuration for Fe+4 Ion
When it comes to understanding the electron configuration of ions, it’s important to know that ions are formed when atoms gain or lose electrons. In the case of the Fe+4 ion, we are dealing with an iron ion that has a charge of +4. To predict the electron configuration of Fe+4, we need to consider the electron configuration of the neutral iron atom (Fe) and the number of electrons it has gained or lost.
The electron configuration of a neutral iron atom (Fe) is 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^6. This configuration tells us that iron has 26 electrons distributed across its electron shells and subshells. However, since the Fe+4 ion has a charge of +4, it means that it has lost 4 electrons.
Electronic configuration of Fe4+
To determine the electron configuration of Fe+4, we start by removing the 4 electrons from the neutral iron atom‘s highest energy level, which is the 4s subshell. This leaves us with the electron configuration of Fe+4 as 1s^2 2s^2 2p^6 3s^2 3p^6 3d^6.
The Role of Electron Configuration in Stability of Ions
The electron configuration of an ion plays a crucial role in determining its stability. In the case of Fe+4, the electron configuration 1s^2 2s^2 2p^6 3s^2 3p^6 3d^6 is significant because it fulfills the stability requirements for the Fe+4 ion.
To understand why this electron configuration is stable, we need to consider the concept of the noble gas configuration. Noble gases, such as argon (Ar), have completely filled electron shells and are known for their stability. By looking at the electron configuration of Fe+4, we can see that it is abbreviated as [Ar] 3d^6. This notation indicates that Fe+4 has the same electron configuration as argon, except for the 3d subshell.
By achieving a configuration similar to a noble gas, Fe+4 attains a more stable electron arrangement. This stability is due to the fact that the 3d subshell is half-filled, which is a relatively stable configuration. The half-filled 3d subshell provides a balance between the repulsion and attraction of electrons, resulting in increased stability for the Fe+4 ion.
In summary, the electron configuration of Fe+4, 1s^2 2s^2 2p^6 3s^2 3p^6 3d^6, is predicted by removing 4 electrons from the neutral iron atom‘s 4s subshell. This configuration fulfills the stability requirements for the Fe+4 ion by achieving a configuration similar to a noble gas, with a half-filled 3d subshell. Understanding the electron configuration of ions is crucial in comprehending their stability and chemical properties.
How many electrons are in Fe3+?
The ground state fe3+electron configuration is 1s2 2s2 2p6 3s2 3p6 3d5. We see from electronic configuration that there are a total of 23 electrons out of which 6 electrons in s-orbital, 12 electrons in p-orbital, and 5 electrons in d orbital.
Does Fe3+ have a noble gas electronic configuration?
No, fe3+ does not have a noble gas electronic configuration. fe3+ contains a total of 23 electrons which does not match with any noble gases.
Application of Electron Configuration in Predicting Chemical Behavior
The electron configuration of an atom plays a crucial role in determining its chemical behavior. By understanding the arrangement of electrons within an atom, scientists can predict how it will interact with other atoms and molecules. Let’s explore some of the applications of electron configuration in predicting chemical behavior.
Chemical Reactivity: The electron configuration of an atom influences its reactivity. Atoms with incomplete outer electron shells tend to be more reactive as they seek to achieve a stable electron configuration. For example, iron (Fe) has an electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2 3d6. The presence of two unpaired electrons in the 4s and 3d orbitals makes iron prone to forming compounds and participating in chemical reactions.
Formation of Ions: Electron configuration also helps in understanding the formation of ions. When an atom gains or loses electrons, it forms an ion. For instance, iron can form two common ions: Fe2+ and Fe3+. Fe2+ is formed by removing two electrons from the 4s orbital, resulting in an electron configuration of 1s2 2s2 2p6 3s2 3p6 3d6. On the other hand, Fe3+ is formed by removing three electrons, leading to an electron configuration of 1s2 2s2 2p6 3s2 3p6 3d5. The electron configuration of these ions affects their chemical properties and reactivity.
Stability of Compounds: The electron configuration of an atom also influences the stability of compounds it forms. Atoms tend to form compounds that allow them to achieve a stable electron configuration, often resembling that of a noble gas. For example, iron can form compounds with oxygen to create iron oxides, such as Fe2O3. In this compound, iron loses three electrons to achieve a stable electron configuration similar to argon (Ar).
Role of Electron Configuration in Understanding Periodic Trends
The periodic table is organized based on the electron configuration of elements, and understanding electron configuration helps in deciphering various periodic trends. Let’s explore the role of electron configuration in understanding these trends.
Atomic Size: The electron configuration influences the size of an atom. As you move across a period from left to right, the atomic size generally decreases. This is because the number of protons in the nucleus increases, resulting in a stronger attraction for the electrons in the same energy level. However, when moving down a group, the atomic size increases due to the addition of new energy levels. For example, iron (Fe) is larger than oxygen (O) because it has additional energy levels.
Ionization Energy:Ionization energy is the energy required to remove an electron from an atom. The electron configuration affects the ionization energy of an element. Elements with a stable electron configuration, such as noble gases, have high ionization energies because it is difficult to remove an electron from a stable configuration. In contrast, elements with incomplete outer electron shells have lower ionization energies as they are more willing to lose or gain electrons to achieve stability.
Electronegativity: Electronegativity is a measure of an atom’s ability to attract electrons in a chemical bond. The electron configuration influences an atom’s electronegativity. Elements with a high electronegativity tend to have nearly filled or completely filled outer electron shells, such as the halogens. Iron, with its electron configuration of 1s2 2s2 2p6 3s2 3p6 4s2 3d6, has a moderate electronegativity compared to elements like oxygen or fluorine.
In conclusion, electron configuration plays a crucial role in predicting the chemical behavior of atoms and understanding periodic trends. By analyzing the arrangement of electrons within an atom, scientists can make informed predictions about an element’s reactivity, ion formation, stability of compounds, and its position in the periodic table. This knowledge is essential in various fields, including chemistry, materials science, and engineering.
Conclusion
In conclusion, the electron configuration of iron (Fe) and its ions Fe2+ and Fe3+ play a crucial role in understanding their chemical properties and reactivity. By examining the electron configuration, we can determine the distribution of electrons in different energy levels and orbitals. Iron, with an atomic number of 26, has an electron configuration of [Ar] 3d6 4s2. This configuration indicates that iron has two electrons in its outermost energy level, making it a transition metal. When iron loses two electrons to form Fe2+, its electron configuration becomes [Ar] 3d6. On the other hand, when iron loses three electrons to form Fe3+, its electron configuration becomes [Ar] 3d5. These changes in electron configuration result in different chemical properties and reactivity for each ion. Overall, understanding the electron configuration of iron and its ions is crucial in comprehending their behavior in chemical reactions and their role in various biological processes.
Frequently Asked Questions
What is the electron configuration of Fe (Iron)?
The electron configuration of Fe (Iron) is [Ar] 4s2 3d6. This means that Iron has 2 electrons in its 4s orbital and 6 electrons in its 3d orbital, following the Argon (Ar) core.
How does the electron configuration change for Fe2+ and Fe3+ ions?
The electron configuration for Fe2+ is [Ar] 3d6 4s0 and for Fe3+ is [Ar] 3d5 4s0. This change occurs because the Fe2+ ion has lost 2 electrons and the Fe3+ ion has lost 3 electrons from the neutral Iron atom.
What is the subshell electron configuration?
Subshell electron configuration refers to the distribution of electrons in the subshells of an atom. For instance, in the case of Iron (Fe), the subshell electron configuration is 4s2 3d6.
What is the condensed electron configuration?
The condensed electron configuration is a simplified version of the electron configuration where the core electrons are represented by the symbol of the previous noble gas in the periodic table. For Iron (Fe), the condensed electron configuration is [Ar] 4s2 3d6.
How many electrons does Fe+4 have and what is its electron configuration?
Fe+4, or Iron (IV), has lost 4 electrons, so it has 22 electrons. Its electron configuration is [Ar] 3d4.
What is the electron configuration for the Fe3+ ion?
The electron configuration for the Fe3+ ion is [Ar] 3d5 4s0. This is because the Fe3+ ion has lost 3 electrons, 2 from the 4s orbital and 1 from the 3d orbital.
What is the difference between Fe2 and Fe3 in terms of electron configuration?
The difference between Fe2 and Fe3 lies in the number of electrons each has lost from the neutral Iron atom. Fe2+ has lost 2 electrons, resulting in the electron configuration [Ar] 3d6 4s0, while Fe3+ has lost 3 electrons, resulting in the electron configuration [Ar] 3d5 4s0.
What is the state electron configuration?
The state electron configuration refers to the electron configuration of an atom in a specific state. For example, the state electron configuration of Iron (Fe) in its ground state is [Ar] 4s2 3d6.
What is the abbreviated electron configuration?
The abbreviated electron configuration is another term for the condensed electron configuration. It provides a shortened version of the electron configuration by representing the core electrons with the symbol of the previous noble gas in the periodic table.
What is the gas electron configuration?
The gas electron configuration refers to the electron configuration of an atom in its gaseous state. For Iron (Fe), the gas electron configuration is the same as its ground state configuration, which is [Ar] 4s2 3d6.
In this article we are discussing about Albr3 lewis structure and geometry and 9 facts regarding this.
Albr3 is composed of central Al and 3 Br atoms. It has the molecular weight of 266.694. It is colorless and hygroscopic in nature. It is a pungent smell pale yellow solid.
Albr3 lewis structure drawing
As Al is bigger in size and has less electronegativity than Br atom, Al act as the central atom in this compound. Al has 3 valance electrons by the use of which it can form 3 sigma bonds with 3 Br atoms.
There is total of 7 electrons in valance shell of Br atom and out of this 7 electrons only 1 is used to form covalent bond with Al atom and 6 remaining electrons present as lone electrons.
Resonance is a process in which movement of electrons occurs from atom to atom by delocalization of electrons. Albr3 possess 3 resonance structures.
In all the structures Al-Br bond has partial double bond character due to delocalization of electron pair that present on Br atom with the vacant p orbital of Al atom to form p∏-p∏ back bonding.
According to VSEPR theory the shape of Albr3 is trigonal planer in which central Al is surrounding by 3 Br atoms. As lone pair is absent on Al atom the geometry of this compound is ideal trigonal planer.
This is because all the valance shell electrons of Al atom take part in covalent bonding with Br atom, hence there exist on lone pair of electron on central Al atom.
Albr3 lewis structure formal charge
The formal charge of an atom in a compound can be determined by the following formula:
Formal Charge (f) = Total No of valance electrons- (No of bonding electrons)/2- Total No of nonbonding electrons.
Hence formal charge on Al atom in Albr3=3-6/2-0=0
Formal charge on each Br atom in Albr3=7-2/2-6=0.
We see that formal charge on central Al atom and each Br atom is 0 making the whole compound is neutral.
Albr3 lewis structure angle
In Albr3 Al uses sp2 hybrid orbitals to form Albr3. The structure of Albr3 is trigonal planner. As it is not a distorted structure the bond angle found in Albr3 is exactly 1200.
The distortion is bond angle does not occur due to absence of lone pair of electron in the central Al atom. The bond angle in Albr3 suggested that all the atoms in Albr3 are present in same plane.
Albr3 lewis structure octet rule
In the lewis structure of Albr3 we found that each Br atom has 8 electrons in its valance shell and fulfill their octet. In Albr3 Al forms 3 covalent sigma bonds with Br atom and each bond contains 2 electrons.
There are a total 6 electrons in the valance shell of Al atom, hence it can’t fulfill their octet. Hence according to octet rule Albr3 is a unstable compound.
Albr3 lewis Structure lone pairs
The 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 Albr3 lone pair present on Al atom= 3-3=0 i.e. 0 lone pair.
Lone pair present on each Br atom=7-1=6 i.e. 3 lone pair.
Firstly to find out the total valance electron in Albr3, it is important to know the electronic configuration of Al and Br atom. The electronic configuration of Al is [Ne] 3s2 3p1 and we see from electronic configuration that there are 3 electrons in valance shell of Al atom.
The electronic configuration of Br atom is [Ar] 4s2 3d10 4p5. There is 7 electrons in the valance shell of Br atom.. The total valance electrons that present on Albr3 will be equal to the (sum of the valance electron of Al and Br atom) i.e. equals to (3*1)+(7*3)=24. There are 24 valance electrons in Albr3.
Albr3 Hybridization
Hybridization is the process in which lower energy hybrid orbitals are formed by mixing of higher energy atomic orbitals. Al has valance shell electronic configuration 3s2 3p1. From electronic configuration of Al atom it can stated that only 1 unpaired electron present in p orbital and we must have 3 unpaired electrons to make Albr3.
In the excited state, Al transfer 2 electrons from 3s orbital to 3p orbital and now a total of 3 unpaired electron is present in central Al atom. After that 3 Br atom gave 3 unpaired electrons to form 3 electron pairs by which 3 Al-Br single covalent bond is formed and remaining 6 electrons on Br atom present as 3 lone pair of electrons. In this compound Br uses sp2 hybrid orbital to form Al-Br bonds.
Albr3 Hybridisation
Albr3 solubility
In Albr3 due to high electronegativity of Br atom Al-Br bond moments lies towards Br atom. The net dipole moment of Albr3 is 0, because Albr3 has planner structure in which 3 Al-Br bond moments cancel each other.
That is why Albr3 is nonpolar in nature. As it is nonpolar in nature it is soluble in nonpolar solvents e.g. diethyl ether, acetone. Although Albr3 is also soluble in methanol, as it is a polar solvent with low dielectric constant.
Conclusion
Due to large size of Br atom, p∏-p∏ back bonding found in Al-Br bond is not to too strong to make the compound octet fulfilled. That is why this compound is electron deficient and acts as a lewis acid. For this same reason Albr3 is an unstable compound. To release electron deficiency some times Albr3 dimerises to form Al2Br6 molecule.
