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- Hydrogen is an unusual element because it behaves in someways like the alkali metal elements and in other ways likenonmetals. Its properties can be explained in part by its electronconfiguration and by the values for its ionization energyand electron affinity. (a) Explain why the electron affinity ofhydrogen is much closer to the values for the alkali elementsthan for the halogens. (b) Is the following statement true?“Hydrogen has the smallest bonding atomic radius of anyelement that forms chemical compounds.” If not, correct it.If it is, explain in terms of electron configurations. (c) Explainwhy the ionization energy of hydrogen is closer to the valuesfor the halogens than for the alkali metals. (d) The hydrideion is H-. Write out the process corresponding to the firstionization energy of the hydride ion. (e) How does the processin part (d) compare to the process for the electron affinityof a neutral hydrogen atom?For each of the following pairs of atoms, state which youexpect to have the higher electron affinity: (a) Rb or Sr;(b) I or Rn; (c) Ba or Te; (d) Bi or CConsider the isoelectronic series Zr4+, Nb5+, Mo6+, Tc7+. Arrange these species as follows. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) in order of increasing atomic or ionic radius b) in order of increasing ionization energy
- Use the periodic table to arrange the following elements in order of increasing firstionisation energy: P, S, O. Give a brief explanation why you chose this arrangement.How many valence electrons in Groups 1,2,3,5,6,7,8A?The gadolinium +3 ion (Gd3+) has advantageous magnetic properties for Magnetic Resonance Imaging (MRI) applications, specifically a high number of unpaired electrons. In fact, both neutral Gd and Gd3+ have a set of degenerate orbitals with seven unpaired electrons. a) Write the electron configuration for Gd and Gd3+ using the condensed noble gas notation. Identify which orbitals lose electrons to yield the +3 cation based on the above information. Explain your reasoning (2-3 sentences). b) Curium (Cm) is an actinide element named for Marie Curie. Cm is in the same group as Gd and also forms a +3 cation. Write the electron configuration for Cm and Cm3+. c) While +3 is the most common oxidation state for lanthanide elements, some can form +2 ions. Identify an isoelectronic ion to Gd3+ that has a +2 oxidation state and indicate which orbitals lose electrons to form that ion.
- Write electron configurations of • C, N, O, F, Ne • Be, Mg, Ca • F, Cl, Br • He, Ne, Ar, KrWhy fluorin has low electron affinity as compared to chlorine?Rank the following in increasing order of ionization energy by numbering them in order from 1 through 6, with 1 having the lowest ionization energy and 6 having the highest ionization energy. Se Cr K Br Са Kr
- 2. Explain the following phenomena on the basis of electron configuration. i) Fluorine forms an ion having a charge of -1. Support your answer by providing the electron configuration of both atom and ion. ii) Which is the more likely the configuration for Mn2+: [Ar]4s23d3 or [Ar]3d5. Give reason for your answer.Arrange the following material according to the increasing tendency to lose an electron. (I.) glass, (II.) copper, (III.) fur, (IV.) SilkIn group 15 elements, there is considerable increase in covalent radius from N to P but small increase from As to Bi. Why?
