Let Su, Tn, and VI be imaginary elements in the same column in the periodic table. Their relative electronegativities are Su > Tn > VI and their relative atomic radii are VI > Tn > Su. Which of the following anions would have the highest K₁? HSuO3 HVIO3 HTnO3 All of these would be expected to have the same K₁.

Let Su, Tn, and VI be imaginary elements in the same column in the periodic table. Their relative electronegativities are Su > Tn > VI and their relative atomic radii are VI > Tn > Su. Which of the following anions would have the highest K₁? HSuO3 HVIO3 HTnO3 All of these would be expected to have the same K₁.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter3: Atomic Shells And Classical Models Of Chemical Bonding

Section: Chapter Questions

Problem 1P: Before the element scandium was discovered in 1879, it was known as “eka-boron.” Predict the...

See similar textbooks

Similar questions

Before the element scandium was discovered in 1879, it was known as “eka-boron.” Predict the properties of scandium from averages of the corresponding properties of its neighboring elements in the periodic table. Compare your predictions with the observed values in Appendix F.
What is the valence electron configu.ration for Group SA (lS) elements?Metallic character increases when going down a group. Give some examples illustrating how Bi and Sbhave metallic characteristics not associated with N, P,and As. Elemental nitrogen exists as N2 whereas in the gas phase the elements phosphorus, arsenic, and antimony consist of P4' As4, and Sb4 molecules, respectively.Give a possible reason for" this difference between N2 and the other Group SA (lS) elements. White phosphorus is much more reactive than black or red phosphorus. Explain.
Consider the Mg2+, Cl-, K+, and Se2- ions. The four spheresbelow represent these four ions, scaled according to ionic size.(a) Without referring to Figure 7.8, match each ion to its appropriatesphere. (b) In terms of size, between which of the sphereswould you find the (i) Ca2+ and (ii) S2- ions?
Use the electron affinity (EA) data for ClCl , BrBr , and II , along with your knowledge of periodic trends, to estimate the electron affinity of astatine to two significant figures.
18 - for Cl, Cl + and Cl- ions;Cl- is the largest number of electronsII. Stripping electrons from the Cl + ion is most difficultIII. Neutral Cl atom and Cl- ions have equal radiiWhich of his judgments are correct? A) Only IIIB) I, IIC) I, IIID) I onlyE) I, II, III
(a) Account for formation of the following series of oxidesin terms of the electron configurations of the elementsand the discussion of ionic K2O, CaO, Sc2O3, TiO2, V2O5, CrO3. (b) Name these oxides.(c) Consider the metal oxides whose enthalpies of formation(in kJ mol -1) are listed here. Calculate the enthalpy changes in the following general reactionfor each case:MnOm(s) + H2(g)----->nM(s) + mH2O(g)(You will need to write the balanced equation for each caseand then compute ΔH°.) (d) Based on the data given, estimatea value of ΔHf° for Sc2O3(s).
Sulfur, B, element 16, tends to form a 2- ion. Write the electron configuration of neutral S and ofthis ion.S: S^2- Explain why the 2- ion is the one that tends typically to form? In what group of the periodie table is S located? What ions would the other elements in thisgroup tend to form? Why?
Predict the trend in values of Slater's constant of the every first element of each group of p block elements
Which group in the periodic table has elements with high (en-dothermic) IE₁ and very negative (exothermic) first electronaffinities (EA₁)? Give the charge on the ions these atoms form
Rank the following in order of increasingradius:(a) O²⁻, F⁻, Na⁺(b) S²⁻, P³⁻, Cl⁻
In group 15 elements, there is considerable increase in covalent radius from N to P but small increase from As to Bi. Give reason.
Explain the horizontal irregularity in size of the most com-mon ions of Period 3 elements.