Consider the electron configuration of the species below and choose the diamagnetic species: A) P B) Sn2⁺ C) Cr D) Br
(A) Phosphorus (15) electronic configuration is (Ne)3S23P3
it contains 3 un paired electrons so it is para magnetic nature.
(B) Sn+2 Electronic configuration is (Kr) 4d105S25P0
it does not contains unpaired electrons so it is Dia magnetic nature.
(C) Cr electronic configuration is (Ar)3d54S1
it contains unpaired electrons so it is para magnetic nature.
(D) Br electronic configuration is (Ar)3d104S24P5
It contains unpaired electrons so it is para magnetic nature.
Consider the electron configuration of the species below and choose the diamagnetic species: A) P B)...
Choose the diamagnetic species from below. А Fe B. P Pb2+ D F E None of the above is diamagnetic.
20. Choose the diamagnetie species from below. a. Sn? b. As c. Br d. Cr e. None of the above is diamagnetic 21. How many valence electrons do the noble gases possess? a. 8 b. 1 d. 6 e 2 Identify the isoelectronic elements. a. Cl, F, Br, 1, At b. P3-, S-, Cl-, K, Ca²+ C. Ne, Ar, Kr, Xe, He d. N3, S2-, Br, Cst, Sr2+ e. Zn2+, Co2+, CuCr, Cd? 23. Choose the best Lewis structure for...
Complete the following table using the subshell electron configuration method. A. Species Electron Configuration Number of Valence electrons Ca, Calcium As, Arsenic Mn, Manganese B) Species Electron Configuration Cd, Cadmium Te, Tellurium Br, Bromide ion
14. The electron configuration 1s22s22p63s23p6 applies to all of the following species except: A) Br B) 92- C) 02- D) CI E) Ca2+
For each of the following species, write the electron configuration (assuming no s-p hybridization) and compute the bond order. Then tell: (a) Which should have the longer bond, O2 or O22? (b) Which should have the stronger bond, B2 or B22-? (c) Which should have the weaker bond, C2 or C22? (d) Which should have the shorter bond, 0 or ?
Classify each of the species given below as para-magnetic or diamagnetic Classify each of the species given below as paramagnetic or diamagnetic.
3. The electron configuration of a chemical species is 1s 2s 2p 38* sp a. State the element with the configuration. b. State an element with similar properties to the element in part a. c. Under what circumstances could this electron configuration belong to an element in group 6? d. Under what circumstances could this electron configuration belong to an element in group 2? e. Is it possible for this electron configuration to belong to an element in period 2?
The ground state electron configuration of a mn^2+ is 1s^22s^22p^63s^23p^63d^5 me^2+ is paramagnetic with five unpaired electron. diamagnetic. paramagnetic with one unpaired electron paramagnetic with three unpaired electron paramagnetic with two unpaired electron which ground-state electron configuration is incorrect? br:[ar]3d^104s^24p^5 k: [ar] 4s^1 fe: [ar]3d^5 zn: [ar]3d^104s^2 What 2+ ion has the following ground state electron configuration? The procedure by which electrons are assigned to (or buih up into) orbitals is known as the principle. a. Aufbau b. Bohr c....
Consider the electron configuration of the ion to determine which ion shown below has an incorrect ionic charge? A) Se B) Rb C)C) Ba? D) A- E) none of the above
A species has the following MO configuration: (σ1s)2(σ1s*)2(σ2s)2(σ2s*)2(σ2p)2(π2p)2 The substance is: A. Paramagnetic with one unpaired electron B. Two unpaired electrons C. Three unpaired electrons D. Four unpaired electrons E. Diamagnetic