Chemistry291

Iron(III) ion Explanation: The systematic name(IUPAC) of Fe^3+ cation is iron(III) ion.               Step-1: First,write the name of the element Fe. Fe is called iron.               Step-2: Now put the oxidation number of Fe within parentheses, ( ). Iron(III) Now you have got the systematic nomenclature of Fe^3+. Now I going to give the old name of Fe^3+. The Latin name for iron element is ferrum.The  charged iron ion with the highest oxidation number (3+) is  named as ferric ion and the lower charged iron ion (2+) was is named as ferrous ion.

  There are nine orbitals in the third energy level or shell of electrons(n=3). Explanation: Here the value of principal quantum number is 3(n=3). For n=3 ,we get the value of angular momentum quantum number l= 0,1,2 [l=0 to n-1] •For l=0,  we get s sublevel. •For  l=1,  we get p sublevel. •For l=2 ,we get d sublevel  We will get three sublevels for n=3. These sublevels are 3s,3p and 3d. •The numbers of orbitals in sublevels is specified by the value of magnetic quantum number ,m l.   •In s sublevel, we get one orbital. •In p sublevel , we get three orbitals. •In d sublevel, we get five orbitals.  •The third energy level has three sublevels which are 3s, 3p and 3d. So, for n=3, we get 1+3+5=9 orbitals. 

  In Fe^3+,we get 23 electrons.  Explanation: The atomic number of iron is 26.This means that it has 26 protons and 26 electrons. If you deduct 3 electrons from netral iron atom , you get the iron(III) ion, Fe^3+.So, in Fe^3+ ion you get 23 electrons. Remember that one proton neutralize one electron.The charge of proton is positive(+1) and the charge of electron is negative(-1). 

The sublevel s can hold two electrons as it has one orbital. In addition, the sublevel p can hold 6 electrons as it has three orbitals. Moreover, the sublevel d can hold 10 electrons as it has five orbitals. At last, f sublevel can hold fourteen electrons as it has seven electrons.  In a sublevel, we get one or more than one orbitals.One orbital can hold maximum two electrons. 

In the 4d sublevel, totally ten electrons can be contained.  Explanation: Any d sublevel has five orbitals and we know that each orbital can hold maximum two electrons with opposite spin.As d sublevel has five orbitals, 4d sublevel can hold maximum 10 electrons. 

The p sublevel can hold maximum six electrons. Explanation: The p sublevel has three orbitals and we know that each orbital can hold maximum two electrons with opposite spin.As p sublevel has three orbitals, it can hold maximum  six electrons. 

The f sublevel can hold maximum fourteen electrons. Explanation: The f sublevel has seven orbitals and we know that each orbital can hold maximum two electrons with opposite spin.As f sublevel has seven orbitals, it can hold maximum 14 electrons. 

  The d sublevel can hold maximum ten electrons. Explanation: The d sublevel has five orbitals and we know that each orbital can hold maximum two electrons with opposite spin.As d sublevel has five orbitals, it can hold maximum 10 electrons. 

The s sub-level can hold maximum two electrons. Explanation: The s sub level has one orbital and we know that each orbital can hold maximum two electrons with opposite spin.As s sub level has one orbital, it can hold maximum 2 electrons. 

 The maximum number of unpaired electrons in Fe^3+ is 5. Explanation: Click here 

The ground state  electron configuration of Fe^3+ is given below: 1s²2s²2p⁶3s² 3p⁶ 4sº 3d⁵ =[Ar]3d⁵

   You need to write the  electron configuration  of Fe3+ using noble gas  notation. Remember that the atomic number of iron is 26. Here is the  electron configuration of Fe^3+ using noble gas notation: [Ar]3d⁵ The noble gas argon is used here.The atomic number of argon is 18. Remember that the d subshell has five orbitals.Each orbit can take maximum two electrons. In case of filling degenerate orbits ,each orbital will take one electron  before pairing by the second electron  according to Hunds' rule. The Fe^3+ ion has five unpaired electrons.That is why it is paramagnetic. The Fe^3+ has 26 protons but 23 electrons.

    In the ground-state electron configuration of oxygen, O, two  unpaired electrons are present. Explanation: To find out the number of unpaired electrons in oxygen, you need to write the electron configuration of O(Oxygen atom). Remember that the atomic number of oxygen is 8. Here is the ground state electron configuration of O: 1s²2s²2p⁴ =[He] 2s²2p ⁴ Remember that the p subshell has three orbitals.Each orbit can take maximum two electrons. In case of filling degenerate orbits ,each orbital will take one electron  before pairing by the second electron  according to Hunds' rule. Next

    In the ground-state electron configuration of iron, Fe, four  unpaired electrons are present. Explanation: To find out the number  of unpaired electrons in Fe, you need to write the electron configuration of Fe. Remember that the atomic number of iron is 26. Here is the ground state electron configuration of Fe: [Ar]3d⁶4s² Remember that the d subshell has five orbitals.Each orbit can take maximum two electrons. In case of filling degenerate orbits ,each orbital will take one electron  before pairing by the second electron  according to Hunds' rule. Next   In the ground-state electron configuration of Fe2+, four  unpaired electrons are present. Explanation: To find out the number of unpaired electrons in Fe^2+ ion, you need to write the electron configuration of Fe^2+. Remember that the atomic number of iron is 26. Here is the electron configuration of Fe^2+: [Ar]3d⁶ Remember that the d subshell has five orbitals.Each orbit can take maximum two electrons. In case of filling dege

   In the ground-state electron configuration of iron, Fe, four  unpaired electrons are present. Explanation: To find out the number of unpaired electrons in Fe, you need to write the electron configuration of Fe. Remember that the atomic number of iron is 26. Here is the electron configuration of Fe: [Ar]3d⁶4s² Remember that the d subshell has five orbitals.Each orbit can take maximum two electrons. In case of filling degenerate orbits ,each orbital will take one electron  before pairing by the second electron  according to Hunds' rule. Next

  In the ground-state electron configuration of Fe2+, four  unpaired electrons are present. Explanation: To find out the number of unpaired electrons in Fe^2+ ion, you need to write the electron configuration of Fe^2+. Remember that the atomic number of iron is 26. Here is the electron configuration of Fe^2+: [Ar]3d⁶ Remember that the d subshell has five orbitals.Each orbit can take maximum two electrons. In case of filling degenerate orbits ,each orbital will take one electron  before pairing by the second electron  according to Hunds' rule. Next

In the ground-state electron configuration of Fe3+, five  unpaired electrons are present. Explanation: To find out the number of unpaired electrons in Fe^3+ ion, you need to write the electron configuration of Fe3+.Remember that the atomic number of iron is 26. Here is the  ground state  electron configuration of Fe^3+: [Ar]3d⁵ Remember that the d subshell has five orbitals.Each orbit can take maximum two electrons. In case of filling degenerate orbits ,each orbital will take one electron before pairing by the second electron according to Hunds' rule. Next

A)MgCl₂ B)MgBr₂ C)Mg₂Br₂ D)MgH₂ Answer: The option is (B)  MgBr₂. For explanation: Click this Link