e) All of the above are paramagnetic. Build your reputation. What is lanthanoid contraction? Vapour pressure of water at 298 K is 23 mm. The lesser number of oxidation states at extreme ends arise from either too few electrons to loose or share (e.g. are trapped inside the crystal lattices of metals. A group of fourteen elements following lanthanum i.e. Fe2+ to Zn2+ it changes from d6 to d10). Assuming 2s-2p mixing is NOT operative, the paramagnetic species among the following is : (A) Be2 (B) B2 (C) C2 (D) N2 Sir, plz explain why (C) is the answer of the above question. They are generally non-stoichiometric and neither typically ionic nor covalent.Most of transition metals form interstitial compounds with small non-metal atoms such as hydrogen, boron, carbon and nitrogen. from 58Ce to 71Lu placed in 6th period of long form of periodic table is known as lanthanoids (or lanthanide series). (viii) These metals form interstitial compounds with C, N, B and H.The presence of partially filled d-orbitaIs in the electronic configuration of atomic and ionic species of these elements is responsible for the characteristic properties of transition elements. Sc and Ti) or too many d electrons (hence fewer orbitals available in which to share electrons with others) for higher elements at upper end of first transition series (i.e., Cu and Zn). No, N2O5 has to be diamagnetic as the molecule has even number of electrons (54) that are fully paired. Open App Continue with Mobile Browser. (ii) These metals exhibit variable oxidation states. Paramagnetic: Mercury: Diamagnetic: Up to date, curated data provided by Mathematica's ElementData function from Wolfram Research, Inc. Click here to buy a book, photographic periodic table poster, card deck, or 3D print based on the images you see here! Cl^(o): [He]2s^(2)2p_x^2p_y^2p_z^1 + e^- => Cl^(-): [He]2s^(2)2p_x^2p_y^2p_z^2 (All orbitals are filled (i.e., … Have you registered for the PRE-JEE MAIN PRE-AIPMT 2016? Assuming 2s-2p mixing is NOT operative, the paramagnetic species among the following is : (A) Be2 (B) B2 (C) C2 (D) N2 Sir, plz explain why (C) is the answer of the above question. So, Mg+2 is also diamagnetic because all its electrons are paired up. (ii) They are very hard. In transition elements, there are greater horizontal similarities in the properties in contrast to the main group elements because of similar ns2 common configuration of the outermost shell.An examination of common oxidation states reveals that excepts scandium, the most common oxidation state of first row transition elements is +2 which arises from the loss of two 4s electrons. Some borides of transition elements approach diamond in hardness. [Inner orbital or low spin complex] (6NH 3 molecules) (d) Electronic configuration of Zn 2+ in [Zn(NH 3) 6] 2+. © (vii) These metals form various alloys with other metals of the series. O-2 is paramagnetic due to the presence of one unpaired electron. C2 2+ has the same number of electrons as B2, and since B2 is paramagnetic, so is C2 2+. Identify the species that has the smallest radius. The bond length in the oxygen species can be explained by the positions of the electrons in molecular orbital theory. More than one answer may apply. Which of the following species is paramagnetic? C. C 2. Our videos prepare you to succeed in your college classes. The species which is not paramagnetic among the following is. This means that after scandium, d-orbitals become more stable than the s-orbital.Further, +2 state becomes more and more stable in the first half of first row transition elements with increasing atomic number because 3d orbitals acquire only one electron in each of five 3d orbitals (i.e. Identify the number of valence electrons in Cl^-1. 9 - Consider the following list of small molecules and... Ch. Therefore, [Zn(NH 3) 6] 2+ is an outer orbital complex and is diamagnetic. Which of the following statements is TRUE? a) O b) Ar c) Ti4+ d) None of the above is paramagnetic. (iii) Transition metal atoms or ions generally form the complexes with neutral, negative and positive ligands. a) 5 b) 7 c) 6 d) 1 e) 2. b) 7. Other examples are : VH0.56, TiH1.7 Some main characteristics of these compounds are:(i) They have high melting and boiling points, higher than those of pure metals. La3+ and Ce4+ have 4f0 configuration whereas Yb2+ and Lu3+ have 4f14configuration, which makes all these four deficient of unpaired electrons and thus they all are diamagnetic whereas all rest of the lanthanoids have atleast one or more unpaired electron which makes them paramagnetic. However, the electronic configuration of all the tripositive ions (the most stable oxidation state of all lanthanoids) are of the form 4f n(n = 1 to 14 with increasing atomic number). If an electron is paired (i.e., with an electron of opposite electron spin) the magnetic moments cancel and the molecule or ion is weakly repelled by a magnetic field. paramagnetic: has unpaired e-s that generate a magnetic moment that attracts the cmpd with the unp e-s into a magnetic field; diamagnetic all e- paired: weakly repelled by a magnetic field. Assuming 2s-2p mixing is not operative, the paramagnetic species among the following is (A) Be2 (B) B2 (C) C2 (D) N2 . So, Na+ is diamagnetic because all its electrons are paired up. Improve concepts using videos, connect with students and teachers globally. The paramagnetic species among the following is - Na^+, Zn^2+, Cu^+, Fe^3+, Paramagnetic species have at least one unpaired electron. Among the following, the paramagnetic compound is a. Na2O2 b. O3 c. N2O d. KO2Sol. Books. What are interstitial compounds? The shielding effect of f-orbitals in very poor due to their diffused shape. Name an ore of one of the. Select the correct statem ent about and and O 2. (iv) Compounds of transition metals are usually coloured. (v) The compounds of these metals are usually paramagnetic in nature. A) O 2 B) N 2 C) F 2 D) CO E) NO + Q2. 2. Electronic configuration of Scandium; Sc = 21 = 1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹ Sc³⁺ = 1s², 2s², 2p⁶, 3s², 3p⁶ Hence in Sc³⁺ there is no unpaired electron. To obtain the molecular orbital energy-level diagram for \(\ce{O2}\), we need to place 12 valence electrons (6 from each O atom) in the energy-level diagram shown in Figure \(\PageIndex{1}\). Ltd. Download books and chapters from book store. It results in the stronger force of nuclear attraction of the 4f electrons and the outer electrons causing decrease in size.Consequences of lanthanoid contraction:(i) Similarly in the properties of elements of second and third transition series e.g. Posted 5 years ago For example, Mn exhibits all oxidation states from +2 to +7 as it has 4s23d5 configuration. 9 - These questions are not designated as to type or... Ch. 1. The regular small decrease in atomic radii and ionic radii of lanthanides with increasing atomic number along the series is called lanthanoid contraction.Cause of lanthanoid contraction: When one moves from 58Ce to 71Lu along the lanthanide series nuclear charge goes on increasing by one unit every time. If you are having trouble with Chemistry, Organic, Physics, Calculus, or Statistics, we got your back! remains half filled) and electronic repulsion is the least and nuclear charge increases. I believe C2 2+ is the only paramagnetic species. Thus electronic configuration, to large extent, the existence and stability of oxidation states.The other factors which determine stability of oxidation state are:(i) Enthalpy of atomisation (ii) Ionisation energy (iii) Enthalpy of solvation (iv) E.N. Welcome to Sarthaks eConnect: A unique platform where students can interact with teachers/experts/students to get solutions to their queries. Paiye sabhi sawalon ka Video solution sirf photo khinch kar. La. 9 - Among the following, which has the shortest bond... Ch. Paramagnetism is due to the presence of one or more unpaired electrons in a species. 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