The interhalogen compound BrF3 is a volatile, straw-colored liquid. The compound exhibits appreciable electrical conductivity because of autoionization (“solv” refers to BrF3 as the solvent): 2 BrF31l2 ∆ BrF2 +1solv2 + BrF4- 1solv2 One chemical characteristic of BrF3 is that it acts as a Lewis acid toward fluoride ions. What do we expect will happen when KBr is dissolved in BrF3?

The interhalogen compound BrF3 is a volatile, straw-colored liquid. The compound exhibits appreciable electrical conductivity because of autoionization (“solv” refers to BrF3 as the solvent): 2 BrF31l2 ∆ BrF2 +1solv2 + BrF4- 1solv2 One chemical characteristic of BrF3 is that it acts as a Lewis acid toward fluoride ions. What do we expect will happen when KBr is dissolved in BrF3?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section19.6: A Periodic Perspective: The Main-group Elements

Problem 19.6PSP

See similar textbooks

Similar questions

I was instructed to balence the equation of HCl(aq) + NaHCO3(aq) which yields to H20(l) + CO2(g) +NaCl(aq). However, I am pretty sure this equation is already balenced, but I am confused.
Boric acid, B(OH)3 (or H3BO3), does not lose a proton in water, but rather bonds to the O atom of an H2O molecule, which then releases an H+ ion to form the B(OH)4- ion. Use VESPR theory to draw structures, with ideal bond angles, for boric acid and the anion it forms when it reacts with water.
H2PO4 can act as either an acid or a base. Species with this property are called... O Amorphic O Ambiprotic O Amphoteric O Allotropes O Amorphous
Arrange the Lewis acids GaCl3, BCl3 en AlCl3 in order of increasing acidity.
Why do nonmetals oxides tend to form acids and metal oxides tend to form bases? Metal oxides tend to form bases because the metal does not pull electron density towards itself, and this makes the oxygen electron rich, and the oxygen can then more readily bind a hydrogen atom. Metal oxides tend to form bases because the metal pulls electron density towards itself, and this makes the oxygen electron rich, and the oxygen can then more readily bind a hydrogen atom. Nonmetal oxides tend to form acids because the central atom is electronegative and pull electron density towards itself. Thus, the bond between the oxygen and the hydrogen becomes stronger, and the hydrogen can be released. Nonmetal oxides tend to form acids because the central atom is electronegative and pull electron density towards itself. Thus, the bond between the oxygen and the hydrogen weakens, and the hydrogen can be released.
Oxides can react with water to form acids or bases. Identify each of the following oxides as acidic or basic. Write the chemical formula of and give the name of the acid (include 'acid') or base formed upon reaction with water. Acid/Base Acid/Base Oxide Туре Formula Name (a) As,0g (b) Cao (c) Cl,0,
What is the enthalpy change, Delta Hrxn, for the following reaction? 2 NaOH (s) + CO2 (g) → Na2CO3 (s) + H2O (l) a. – 597.5 kJ b. – 991.0 kJ c. + 171.9 kJ d. none of these e. +2661.4 kJ f. – 2661.4 kJ g. – 171.9 kJ h. + 991.0 kJ
What is the Enthlapy of the equation? What is the Bond Energy? NaOH(s) ─HCl→ Na+(aq) + Cl-(aq) + H2O(l)
A baker uses sodium hydrogen carbonate (baking soda) asthe leavening agent in a banana-nut quickbread. The baking sodadecomposes according to two possible reactions: 2NaHCO₃(s)→Na₂CO₃(s)+CO₂(g)+H₂O(l) , NaHCO₃(s)+H⁺(aq)→Na⁺(aq)+CO₂(g)+H₂O(l) Calculate the volume (in mL) of CO₂ that forms at 200°C and0.975 atm per gram of NaHCO₃ by each of the reaction processes.
Define conduction
Explain which is the stronger acid, H3PO4 or H2SO3; CCl3CH2COOH or CCl2FCH2COOH. [Draw possible Lewis structure models]
How can we describe the acid-base interaction in terms of boundary orbitals?