(b) Properties of the chemical elements often show regular variation with respect to their positions in the periodic table. (i) Describe the general trend in acid-base character of the oxides for the elements in the third period. (ii) Using one example for each acidic oxide and basic oxide in third period, show the equation of the reaction between the oxides with water.

(b) Properties of the chemical elements often show regular variation with respect to their positions in the periodic table. (i) Describe the general trend in acid-base character of the oxides for the elements in the third period. (ii) Using one example for each acidic oxide and basic oxide in third period, show the equation of the reaction between the oxides with water.

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter18: Representative Metals, Metalloids, And Nonmetals

Section: Chapter Questions

Problem 10E: The elements sodium, aluminum, and chlorine are in the same period.. (a) Which has the greatest...

See similar textbooks

Similar questions

Group 15 elements react with hydrogen to form hydrides with a general formula of EH3 (where E = N, P, As, Sb or Bi) and they are Lewis base. (i) Briefly discuss why Group 15 hydrides are Lewis base. (ii) Arrange the strength of Lewis basicity of EH3 in decreasing trend. Explain your answer.
(a) Write a balanced equation representing the reaction of the acid, H2PO4- with the base, water. (b) Write the expression for Ka of H2PO4- in terms of concentrations of relevant species.
(b) The K₂ of HClO₂ is 0.010. Determine the pH of a 0.1 M HClO₂ aqueous solution at equilibrium.
(a) Wr ite an equat ion for the react ion in whichH2C6H7O5-(aq) acts as a base in H2O(l). (b) Write an equationfor the reaction in which H2C6H7O5-(aq) acts as an acidin H2O(l). (c) What is the conjugate acid of H2C6H7O5-(aq)?What is its conjugate base?
(a) Give the conjugate base of the following Brønsted–Lowry acids: (i) HIO3, (ii) NH4+. (b) Give the conjugate acidof the following Brønsted–Lowry bases: (i) O2-, (ii) H2PO4-.
Why is (CH3)3Cl considered to be a Lewis Acid?
The substance HIO, is expected to be a stronger acid than the substance HIO.
(a) Draw the Lewis structures for at least four species thathave the general formula where X and Y may be the same or different, and n mayhave a value from +1 to -2. (b) Which of the compoundsis likely to be the strongest Brønsted base?
Provide your view on the below statement ? Across a row of the periodic table, the acidity of HA increases as theelectronegativity of A increases
Hypothesize what your observations will be for the reactions of hydrogen carbonate withthe acids in Part D. Include your rationale. Part D: Part D: Reactions with NaHCO3 and Na2C2O413. Place a small quantity (about the size of an almond or a bean) of sodium hydrogen carbonate (i.e., sodiumbicarbonate) into an evaporating dish. Place the same amount of sodium oxalate into a separate dish.14. Add one dropper’s worth* of 1.0 M H2SO4 to one of the dishes. Note any visible changes (bubbling, smokeformation, color changes, etc.) that occur to the dish’s contents. When the reaction has finished, add adropper of 1.0 M H2SO4 to the other dish and again observe.15. *The dropper does not have to be full, just what one fully squeezed bulb picks up16. Clean the dishes out and set them up as you did before with solid NaHCO3 and Na2C2O4. Add acid to thesalts as you did before, but use 1.0 M HCl instead of H2SO4.
What is the basis for referring to the hydrogen ion as a proton? (a) The Arrhenius definition of an acid. (b) The Brønsted-Lowry definition of an acid x (c) The Lewis definition of an acid. (d) H* exists as a bare proton. (e) None of these.
Phosphorous acid (H3PO3) has the Lewis structure shown at right.(a) Explain why H3PO3 is diprotic and not triprotic. (b) A 25.0-mL sample of an H3PO3 solution titrated with 0.102 M NaOH requires 23.3 mL of NaOH to neutralize both acidic protons. What is the molarityof the H3PO3 solution? (c) The original solution from part (b) has a pH of 1.59. Calculate the percentionization and Ka1 for H3PO3, assuming that Ka1 >> Ka2. (d) How does the osmotic pressure of a 0.050 M solution of HCl compare qualitatively with that of a 0.050 M solution of H3PO3? Explain.