For all the complexes, the valence electron counting is done using neutral atom method.
[Rh(PMe3)4]+
The oxidation state of the metal atom is +1. Hence it is a d8 ion.
Now, valence electron counting around the metal
Rh………..9e-
4PMe3……….2x4 = 8e-
1+ charge……………= -1e-
Total valence electron = 16e-
The electron counting is done for all other complexes similarly.
[(n6-C6H6)Cr(CO)3]
The chromium atom is in zero oxidation state. Hence, it is a d6 ion.
Cr……………6e-
(n6-C6H6)……….6e-
3CO………….6e-
Total valence electron = 18e-
[Rh(bipy)2Cl]+
The oxidation state of the Rh is +2 and hence it is a d7 ion.
Rh……………9e-
2bipy……….8e-
Cl……………1e-
2+ charge……….-2e-
Total valence electron = 16e-
[(n5-C5H5)Fe(CO)2]-
The oxidation state of Fe is zero, hence it is a d8 ion.
(n5-C5H5)…………..5e-
Fe……………………8e-
2CO………………..4e-
1- charge…………..1e-
Total valence electron = 18e-
[Rh2(CO)4Cl2]
The oxidation state of Rh is +1, hence it is a d8 ion.
2Rh……………..18e-
4CO……………….8e-
2Cl(bridging)……..6e-
Total valence electon 32e-, i.e. 16e- for each metal atom.
[Ir(CO)Cl(PPh3)2]
The oxidation state of Ir is +1, hence it is a d8 ion.
Ir…………….9e-
CO……………2e-
Cl……………..1e-
2PPh3…………..4e-
Total valence electrons 16e-
1. Write the metal d" configuration and identify the number of valence electrons around the metal...
6 Identify the coordination number (C.N.), metal oxidation state(O.S.) and the number of metal d electrons for each of the following complexes. (a) [Ni(CN):) C.N. = _ ; O.S. = __, d-electrons = d-electrons = (b) [Pd(Cl)]2 C.N. = _ ; O.S. = ___, d-electrons = (c) [Cr(CN)]C.N. =__; O.S. = —, (d) [Fe(CO).]? C.N. = __; O.S. = ___, d-electrons =- (e) [Cr(CI):]& C.N. = ___; O.S. = __, d-electrons = (1) [Ag(CN)2] C.N. = ___; O.S. = ___,...
Q1) For each of the following compounds, determine the formal oxidation state of the transition metal and the corresponding number of d electrons. State whether each one is likely to be stable enough to be characterized. (1) [Re(CO)5] (2) [HFe(CO)4]- (3) ((ŋ6-C5H5)2Fe) (4) ((ŋ6-C6H6)2Cr) (5) ((ŋ5-C5H5)ZrCl(OCH3) (6) (IrCl(PPh3)3) (7) (Mo(CO)3(PPh3)3) (8) (Fe(CO)4(C2H4)) (9) (W(CO)5Cl)- (10) Ni(CO)4)Q2) Use the 18-electron rule to predict the number of carbonyl ligands, n, in each of the following complexes: (1) [Cr(CO)n] (2) [Fe(CO)n(PPh3)2)] (3) [Mo(CO)n(PMe3)3] ...
6 Identify the coordination number (C.N.), metal oxidation state(O.S.) and the number of metal d electrons for each of the following complexes. (a) [Ni(CN)s] C.N. = __;0.S. = ___, d-electrons = (b) (Pd(C1).]C.N. = ____; O.S. - ___, d-electrons = (c) (Cr(CN)] C.N. - ___.O.S. = ___, d-electrons = (d) [Fe(CO).)? C.N. = ___; O.S. = ___, d-electrons = (e) (Cr(Cl)s) C.N. = ____ ; O.S. = ____ d-electrons =_ (1) (Ag(CN)2] C.N. = _ ; O.S. = _ ,...
1. Write the electron configurations and identify the number of valence electrons for each of the following elements. oxygen sulfur nitrogen hydrogen fluorine phosphorus 2. Write name of the molecular geometry for each of the following molecules. a. A molecule with the central atom surrounded by three atoms and one lone pair. b. A molecule with a central atom surrounded by two doubly-bonded atoms. c. A molecule with a central atom surrounded by two singly-bonded atoms and two lone pairs....
1)Determine the number of valence electrons for each of the atoms. Enter each answer as a numeral. For example, if an atom has two valence electrons, enter the number 2. (Li, CI, Al, Ne) 2) Identify the number of core and valence electrons for each atom. Ra: Core electrons and Valence Electrons
1) Give the full electron configuration for lawrencium (LR #103). Identify all core and valence electrons. 2) Explain, using bond theory, why ionic crystals crack when hit while metallic lumps do not . 3) What is penetration and how does it influence orbital stability? Give an example. 4) How are odor and molecular shape connected? 5) Arrange these elements in order of increasing degree of magnetism: Fe, Cr, Au, Hg Explain why you ordered them that way.
gands arge Ka[Fe(C2O4)a] (hint: bidentate oxalate ligands) valence electrons on Metal Charge on the ligands: Charge on the Metal: Revised Count on the Metal (accounting for charge Number of electrons donated from the ligands: Total electrons in this complex: INi(en)2(CI)2] Valence electrons on Metal; Charge on the ligands: Charge on the Metal: Revised Count on the Metal (accounting for charge Number of electrons donated from the ligands Total electrons in this complex: Re(CO)s(PF3)]Cl Valence electrons on Metal: Charge on the...
1. a) Write the electronic configuration for the atom of Co b) Draw the box diagram for the valence electrons of Co c) From the complete set of the 4 n° quantum ns to one of the highest energy electrons for the d) Write the electronic configuration for the ion Co +3
The following Lewis diagram represents the valence electron configuration of a main-group element. The element in period 2 that has this valence electron congfiguration is SA 4A 5A6A7A He CI Mg 3B 48 5B 6B7B8B1B 29 Al Si P S SC V Cr Mn Fe Co Ni Cu Zn Ga Ge As IZE NG Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te W Re Os Pt Au Hg Tl Pb Bi Po At Rn REH e Pr...
Which element has the ground-state electron configuration [Xe]6s25d14f7? Eu Tb Pt Gd How many valence electrons does a neutral polonium atom have? 4 6 2 84 Of the following, which atom has the largest atomic radius? Cr Sc Co Br Of the following, which atom has the smallest atomic radius? Po Ba Te Sr Of the following, which atom has the smallest atomic radius? Br K Co Ni