Question 1 : An atom has electronic configuration 1s$^{2}$ 2s$^{2}$ 2p$^{6}$3s$^{2}$ 3p$^{6}$ 3d$^{3}$ 4s$^{2}$, you will place it in which group:

Question 6 : How many valence electrons are there in the following electronic configuration?&#160;<div>$1s^{2}\ 2s^{2}\ 2p^{6}\ 3s^{2}\ 3p^{2}$</div>

Question 7 : The number of unpaired electron in chromium (Atomic number = 24) is?<br/>

Question 9 : Which of the following represents the electronic configuration of d-block elements?

Question 11 : An atom has electronic configuration of $2,8,18,7,$<br/>What is the atomic number the of atom?<br/>

Question 12 : The element which readily forms an ionic bond has the electronic configuration is:

Question 15 : The valence electronic configuration of an element is $[Ne]&#160; 3s^1$. The element is :

Question 16 : If a dipositive ion has an electronic configuration of 2, 8, then the number of electrons in that ion is:

Question 18 : The electronic configuration of dipositive ion is [Kr] $4d^{10} 5 s^2 5p^2$. Then atomic number of the element is .........

Question 21 : The electronic configuration of an element having atomic number $17$ is:

Question 23 : If an element has an atomic number of $11$, it will combine most readily with an element that has an electron configuration of<span>&#160;:</span>

Question 24 : Which one among the following contains the valence electrons in the ground state of the magnesium atom?

Question 26 : Among the following which one contains valence electrons in the ground state of the magnesium $Mg$ atom?

Question 29 : Which one among the following is exactly one-half filled in the ground-state electron configuration of the phosphorous atom?

Question 31 : Which of the following does not have valence electron in $3&#160;d$ - subshell?

Question 33 : By using the above informations define the electronic configuration of $S$ atom.

Question 35 : The number of electrons having $(n\times l\times m)=0$ in $Na^{+}$ is :<span><br/></span>

Question 37 : The&#160;$\displaystyle 39^{th}$ electron will go into which one of the following sub-levels?

Question 38 : The atomic number of the element having maximum number of unpaired 3p electrons is (in ground state) :

Question 40 : The quantum number of 20th electron of Fe (Z = 26) ion would be :

Question 41 : $\displaystyle 4s^{2}$ is the configuration of the outermost orbit of an element. Its atomic number would be<span>:</span>

Question 42 : Sum of the paired electrons present in the orbital with&#160;$\displaystyle l =2$ in all the species&#160;$\displaystyle Fe^{2+},Co^{2+}\, \, and\, &#160;Ni^{+2}$ are<span>:</span>

Question 43 : An atom has 2 electrons in K shell, 8 electrons in L shell and 8 electrons in M shell. The number of s electrons present in the element is&#160;:

Question 44 : In which of these options do both constituents of the pair have the same magnetic moment?

Question 45 : Elements upto atomic no. 112 have been discovered till now. What will be the electronic configuration of the element possessing atomic no. 108.

Question 46 : Which of the following is electronic configuration of Cu$^{2+}$(Z = 29)?

Question 47 : What is the total number of electrons with quantum number $l=0$ for Be?

Question 48 : Which of the following ions has the maximum number of unpaired d-electrons?

Question 49 : Given: K &#160;L M &#160;N<br/>&#160; &#160; &#160; &#160; &#160; &#160; 2 &#160;8&#160; 11&#160; 2.The number of electrons present in l = 2 is :

Question 50 : The value $l$ and m for the&#160;last electron in the Cl$^-$ ion are :

Question 53 : Magnetic moment of V(Z = 23), Cr( Z = 24), and Mn(Z = 25) are x, y, z, respectively, hence:

Question 54 : Amongst the following elements (whose electronic configurations are given below), the one having the highest ionization energy is:

Question 57 : Assertion: The magnetic moment of $Mg$-atom is more than $K$-atom as the former has two electrons in outermost shell. Reason: The magnetic moment of $N$-atom is more than magnetic moment of $O$-atom and former has more number of unpaired electrons.

Question 58 : Assertion: Electronic configuration $_{23}\textrm{V}^{3+}$ ion is $[Ar]^{18}3d^2$ and not $[Ar]^{18}3d^04s^2$. Reason: $V^{3+}$ ion is dia-magnetic in nature.<div><br/></div><div>Read the above assertion and reason and choose the correct option regarding it.</div>

Question 59 : <div><span>State True or False.</span><br/></div>Depositive zinc exhibits para-magnetism due to loss of two electrons from $3d$-orbital of neutral atom.

Question 60 : The number of electrons in an atom with atomic number $105$ having $(n+l)=8$ are:

Question 61 : <div><div>State True or False.</div><span></span></div>The chemical properties are determined by its nuclear charge.<br/>

Question 62 : A neutral atom of certain elements has 15 electrons. How many unpaired electrons does it have? <br/>

Question 63 : Write down the four quantum number for $8th$ electron of oxygen atom?<br/>

Question 64 : <div><span>Write down all the four quantum number for :</span><br/></div><div><span><br/></span></div>$19th$ electron of $_{24}\textrm{Cr}$

Question 65 : <span>What is the atomic no. and symbol of elements whose outermost electrons are represented as -&#160;</span>$2p^2$?

Question 68 : Correct set of four quantum numbers for the valence (outermost) electron of rubidium $(Z=37)$ is:

Question 69 : An elements has electronic configuration $2, 8, 18, 1$. If its atomic weight is $63$, then how many neutrons will be present in its nucleus?

Question 71 : Which of the following has the maximum number of unpaired electrons?

Question 72 : If an ion of $_{25}$Mn has a magnetic moment of 3.873 B.M. Then which state $Mn$ is?<br/>

Question 75 : In the pinwheel galaxy, atomic number of all elements are the same as that on earth and paulis principle is obeyed. However the shell closest to the nucleus is saturated with electrons before the next shell starts to fill and the process continues this way, also each orbital can accommodate only one electron having&#160;$\displaystyle +\frac{1}{2}$ spin. If noble gases are defined as the elements with completely filled outermost shell, which elements would be the nobel gas &#160;in their periodic table ?

Question 78 : Which of the following is paramagnetic if it is a single regardless of its electron configuration?

Question 79 : How many electrons in an atom with atomic number $105$ that can have $(n + 1) = 8$?

Question 80 : The correct set of four quantum numbers for the outermost electrons of rubidium (z$=$37) is:

Question 81 : Find the correct electronic configuration, which represents an excited state of Scandium.

Question 82 : Which among the following sets of atomic numbers is/are associated with the increasing order of the number of unpaired electrons?<div><br/>(a) Z = 29; Z = 20; Z = 25; Z = 27; Z = 24</div><div><br/>(b)&#160;Z = 20; Z = 29; Z = 22; Z = 27; Z = 25</div><div><br/>(c)&#160;Z = 19; Z = 22; Z = 24; Z = 26; Z = 25</div><div><br/>(d)&#160;Z = 19; Z = 22; Z = 26; Z = 25; Z = 24</div>

Question 83 : An atom has 2K,8L,5M electrons. Which of the following is its correct electronic configuration?

Question 84 : Which of the following is the CORRECT electron configuration for the potassium ion $(K^{+1})$?

Question 85 : This time all you are told is $5s^{2}4d^{2}$.<br>What element contains this valence level configuration?

Question 86 : The electron configuration for $Cu$ is $1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{1} 3d^{10}$.<br/>How many valence electrons does copper contain?

Question 88 : <span>The excepted ground state configuration for $Cu$ is:</span><br/><span>$1s^{2} 2s^{2} 2p^{ 6} 3s^{2} 3p^{6} 4s^{2} 3d^{9}$</span><br/><span>The actual configuration is:</span><br/><span>$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{1} 3d^{10}$</span><br/><span>Why is the true electron configuration different?</span>

Question 89 : $\displaystyle 1{ s }^{ 2 }2{ s }^{ 2 }2{ p }^{ 6 }3{ s }^{ 2 }3{ p }^{ 6 }3{ d }^{ 2 }$<br/>The above electronic configuration is represented for which atoms among the following? <br/>