In the resonance form of ozone shown below, the formal charge on the central oxy
ID: 1067655 • Letter: I
Question
In the resonance form of ozone shown below, the formal charge on the central oxygen atom is _. Provide answers as indicated for each of the following questions Write the ground state electron configuration of 34_Sc in orbital notation. How many electrons in the ground stale configuration of Sc arc unpaired? Write the ground state condensed electron configuration of the Mn^2+ cation. How many electrons in the ground state configuration of Mn^2+ are unpaired? Write the ground state condensed electron configuration of the Te^2- anion. List all possible quantum numbers as indicated below: a) When n = 3, I can have value (s) of: _ b) When l = 2. m_l can have value(s) of __ c) If an electron has a principal quantum number (n) of 5 and an angular momentum quantum number (l) of 2. the sub shell designation is _. d) If an electron in an atom has the quantum numbers n=4, 1=1. m_1= 0. m, +1/2, how many other atoms in this atom could have the values of this set of quantum numbers? _. e) Sketch the shape and orientation of the p_y orbital. 5a) How many valence electrons docs an atom with the electron configuration (1s^2s^2 2p^6 3s^2 3p^1 have? _Explanation / Answer
13. Formula to calculate formal charge shown below:
Formal charge = No. of valence electron - No. of non-bonding valence electron - No. of bonding electron / 2
Number of valence electron in O is 6 and central O atom in ozone have one pair of non-bonding electron or loe pair.
Formal charge on central O = 6 - 2 - 6/2 = +1
Hence the correct option is (B)
Part II
1. Electronic configuration of Se in orbital notation = 1s22s22p63s23p63d104s24p4
There is 2 unpaired electron in 4p4 orbital (px2 py1 4pz1)
2. Electronic configuration of Mn = 1s22s22p63s23p64s23d5
Electronic configuration of Mn2+ = 1s22s22p63s23p64s23d3
There are 3 unpaired electrons in 3d3 orbital.
3. Electronic configuration of Te = [Kr] 4d10 5s2 5p4
Te2- = [Kr] 4d10 5s2 5p6