Consider the isoelectronic series Ca2+, Sc3+, Ti4+, V5+. 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
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Consider the isoelectronic series Ca2+, Sc3+, Ti4+, V5+. 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
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- Consider 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 energyGive the group number and the general valence electron configuration of an element with the following electron-dot symbol. (For example, type ns2 np6 for ns²np°, which is the valence configuration of all group 8A elements.) (a) group number electron configuration (b) group number electron configuration11)Explain the given ionization energy for each pair using electron configurations. (12(Be)l1(B), I1(N)>l1(O) ).
- Based on their positions in the periodic table, predict whichatom of the following pairs will have the smaller first ionizationenergy: (a) Cl, Ar; (b) Be, Ca; (c) K, Co; (d) S, Ge; (e) Sn, Te.2. Which one of each of the following pairs has the higher ionization energy? Explain in detail for each case. (a) Na or K (b) Ве or B (с) В or C (d) N or O F or Ne (f) Mg or Mg* Ne or Na5. Which of the following alkali metal halides has the larger lattice energy, and which has the smaller lattice energy? Explain. (a) (b)
- 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?Which of the following is isoelectronic pair? (i) ICl2, ClO2 (ii) BrO2– , BrF2+ (iii) ClO2, BrF (iv) CN–, O3Consider the first ionization energy of neon and the electronaffinity of fluorine. (a) Write equations, including electronconfigurations, for each process. (b) These two quantities haveopposite signs. Which will be positive, and which will be negative?(c) Would you expect the magnitudes of these two quantitiesto be equal? If not, which one would you expect to be larger?
- Consider an ionic compound, MX,, composed of generic metal M and generic gaseous halogen X. • The enthalpy of formation of MX, is AH; = -723 kJ/mol. • The enthalpy of sublimation of M is AH sub 123 kJ/mol. • The first, second, and third ionization energies of M are IE1 609 kJ/mol, IE, = 1653 kJ/mol, and IE3 2585 kJ/mol. • The electron affinity of X is AHEA = -347 kJ/mol. (Refer to the hint). • The bond energy of X, is BE = 215 kJ/mol. Determine the lattice energy of MX,. AHjattice kJ/molGiven the following elements: Si, Sr, Cu, Ti, S (a) which of those elements would have the larget atomic radius? (b) which of those elements would have the highest ionization energy? (c) which of those elements would have the lowest electronegativity?1.) a.) True or false: Elements with high ionization energies tend to have lave electron affinities as well. Explain why in terms of nuclear chargeb.) The size of the transition metals decreases slightly in going from left to right across the period. Explain in terms of nuclear charge.c.) Carbon monoxide has a larger bond dissociation energy (1072 Kj/mol) than molecular nitrogen (N2, 945 Kj/mol). Suggest an explanationd.) Given that both the electronic configuration of Ca ([Ar] 4s2 and Zn ([Ar] 3d10 4s2 end with 4s2, explain the difference between the first ionization energy of Ca (IE1 = 590Kj/mol) and Zn (IE1 =906 kJ/mol) e.) In general, ionization energies increase across a period from left to right. Explain why the second ionization energy of Cr is higher, not lower, than that of Mn f.) Which of each of the following pairs of molecules has the larger bond angle? Explain your reasoning. i.) PH3 and NH3