Chemistry291

 Each carbon atom has 4 valence electrons. Explanation: To find out valence electrons of carbon,you need to look at the periodic table.For main group element,the group number is equal to the number of  valence electrons. The element carbon is in group 4A,that is why it has four valence electrons(Just skip the letter A).If you say carbon is in group 14,then you need to consider unit place digit 4 for valence electrons. Now I will show you how to find valance electrons of carbon from electron configuration. The atomic number of carbon is six.So it has six protons and six electrons. If you write electron configuration of carbon,the you will get the following: C ---> 1s² 2s² 2p² We know that valence electrons are the electrons that are found in the valence shell.Valence shell is the outter most shell. We can easily found the outter most shell or valence shell considering the highest value of principal quantum number,n. From C electron configuration,we see that the highest value...

7 Explanation: Seven d electrons are found in cobalt.Here is the way to find the number of d electrons  in cobalt. The electrons that are found in d subshell or orbitals are called d electrons. The atomic number of cobalt is 27.This means that cobalt has 27 protons and 27 electrons. Now write the electron configuration of cobalt: ₂₇Co =1s²2s²2p⁶3s²3p⁶4s² 3d⁷ In  3d⁷ subshell,we are getting 7 electrons.So,in cobalt you get seven d electrons.

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...

   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 

In the element with the  electron configuration  1s2 2s2 2p6 3s2 3p4 has 6 valence electrons. Explanation: From 1s2 2s2 2p6 3s2 3p4 ,we see that the highest value of n is 3 ,for n=3 ,we get 3s2 3p4 .We know that the highest value of n indicates the valence shell and the electrons that are in valence shell are called valence electrons.So, the element with the  electron configuration 1s2 2s2 2p6 3s2 3p4 has (2+4=6) 6 valence electrons.

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

  The electronic configuration of an element is 1s2 2s2 2p6 3s2 3p5.This is the element chlorine. Explanation: 1s2 2s2 2p6 3s2 3p5 means that  ●s subshell of first orbit or energy level has two electrons, ●s subshell of second orbit or energy level has two electrons,   ●p subshell of second orbit or energy level has six electrons, ●s subshell of third orbit or energy level has two electrons,  ● and p subshell of third orbit or energy level has five electrons. Read:CO2 Lewis Structure From 1s2 2s2 2p6 3s2 3p5 electron configuration,we get 2+2+6+2 + 5 = 17 electrons. We know that electron's number is equal to proton number or atomic number for neutral atom.Since here there is no words about charge,we can say that 1s2 2s2 2p6 3s2 3p5 indicates the element whose atomic number is 17. Now if you look at the periodic table,Cl has atomic number 17. So 1s2 2s2 2p6 3s2 3p5 is electron configuration of Chlorine(Cl).

The electron dot symbol for this element is given below: Explanation: From    the electron configuration of 1s22s22p63s23p5,we can see that this atom has 17 electrons.We know that in a neutral atom the number of electrons is equal to the number of protons.So this atom has 17 protons which indicates that this atom is chlorine whose atomic number is 17. From   the electron configuration of the atom 1s22s22p63s23p5,we also see that its outermost shell is the third shell( 3s23p5) and it has 7 valence electrons. To draw the electron dot symbol or Lewis dot symbol of this atom,we need to only consider the valence electrons.

  The electronic configuration of an element is 1s2 2s2 2p6 3s2 3p5.This is the element chlorine. Explanation: 1s2 2s2 2p6 3s2 3p5 means that  ●s subshell of first orbit or energy level has two electrons, ●s subshell of second orbit or energy level has two electrons,   ●p subshell of second orbit or energy level has six electrons, ●s subshell of third orbit or energy level has two electrons,  ● and p subshell of third orbit or energy level has five electrons. Read:CO2 Lewis Structure From 1s2 2s2 2p6 3s2 3p5 electron configuration,we get 2+2+6+2 + 5 = 17 electrons. We know that electron's number is equal to proton number or atomic number for neutral atom.Since here there is no words about charge,we can say that 1s2 2s2 2p6 3s2 3p5 indicates the element whose atomic number is 17. Now if you look at the periodic table,Cl has atomic number 17. So 1s2 2s2 2p6 3s2 3p5 is electron configuration of Chlorine(Cl).

The atomic number of this element is 9. Explanation: From the electron configuration,1s22s22p5,we get (2+2+5=9) nine electrons. We know that ,in a neutral atom, the atomic number indicates the equal number of protons and electrons in a atom as the charge of protons is positive and the charge of electrons is negative.So,the above element's atomic number will be 9 and the element is F.

This atom has 9 electrons. Explanation: The given electron configuration is 1s22s22p5. Here ,we get four s electrons(2+2=4) and 5 p electrons.So,4+5 =9 electrons totally.That is it.

   The electron dot structure of carbon dioxide showing covalent bonding in a molecule of carbon dioxide,CO2, is given below: In CO2 electron dot structure of CO2,we have four bonds which are covalent bonds.Actually,we get two sigma bonds and two pi bonds. Explanation: CO2  Electron Dot Structure Setup Step-01:                  To draw the  CO2 electron dot structure  , we have to find out the  CO2 valence electrons  first.We express valence electrons as dots in  CO2 lewis dot structure . To get the valence electrons of carbon,we need to look at the electronic configuration of carbon. C(6)=1s²2s²2p² The highest value of principal quantum number here is n=2. The highest value of principal quantum number ,n , indicates the valence shell and we know the electrons in valence shell is called valence shell. The nunber of valence electrons in carbon is 4. Now,to draw the lewis dot structure of carbon,we need t...