5- A Brønsted–Lowry acid is a chemical species
being able to lose or donate a hydrogen cation,
H+H+. Obviously, it needs other substance (base) being able to gain
or accept the transferred hydrogen cation.
Examples: Hydrochloric acid (HClHCl), Acetic acid
(CH3−COOHCH3−COOH), and NH4+(ammonium cation)
are examples of B-L acids. Water is a Bronsted lowry base in these
reactions because it accepts the H+H+ donated by the acid to become
the hydronium or oxonium cation.
bA Lewis acid is a
chemical species being able to accept an
electron-pair and therefore able to react with a Lewis
base to form a Lewis adduct, by sharing the electron pair furnished
by the Lewis base.
Thus, a Lewis acid is an atomic or molecular species with a
localized empty atomic or molecular orbital of low
energy. This lowest energy molecular orbital (LUMO; Lowest
Unoccupied Molecular Orbital) can accommodate a pair of electrons.
Lewis bases are lone-electron-pair-containing species, such as
H2O, NH3, OH-,H-,
F- H2O, amines.
Examples:
A strong acid is an acid that ionizes completely in solutions.
The common strong acids include:
Problem 5: Define the following: Bronsted-Lowry acid - Lewis acid- Strong acid - (5 points) Problem...
Draw the bond- line (not Lewis) structure of the conjugate acid for the Bronsted- Lowry acid- base reaction that ocurs when the fllowing base reacts with water. Show all unshared electron pairs and formal charges. Please explain how to get answer!
Identify the Bronsted- Lowry acid, Bronsted- Lowry base, conjugate acid, and conjugate base in the reaction below. HNO3 (aq) + H2 O(1) H3O+ (aq) + NO-3 (aq)
Classify each of the listed catalysts as a lewis or Bronsted-Lowry acid or base
4. Explain things in the following question(s) In each reaction, identify the Brønsted-Lowry acid, the Brønsted-Lowry base, the conjugate acid, and the conjugate base. (a) H2SO4(aq) + H2O(l) —— HSO4 (aq) + H30+(aq) (b) HCO3(aq) + H20(1) = H,CO3(aq) + OH(aq) 5. Using examples, distinguish between a Nucleophile vs Electrophile. Give at least 2 differences between the 2 concepts 6. What are curved arrows or "curly arrows" in Organic Chemistry? What do they represent? Give an example (b) Using Ammonia...
(4 pts) 6. For each of the following conjugate-acid, and the conjugate-base pairs. Bronsted-Lowry acid caving reactions, dentity the Bronsted-Lowry acid,Bronsted-Lowry base, and the NH(aq)F(aq) b) CN(ag)+H
Base 3. Describe the difference between Lewis and Brønsted-Lowry acids. and Bronsted Lowry Acid is a proton donor Bronsted Lowry Base is a proton acceptor Lewis Acid is an electron acceptor Lewis Base is an electron donator hinn af hnth an imaraua calihility of a metal (I want different answers for
3(b). Define an Arrhenius Acid vs An Arrhenius Base? Give examples in cach case? (c) Define a Brownstead -Lorry Acid vs A base. Give Examples 4. Explain things in the following question(s) In each reaction, identify the Brønsted-Lowry acid, the Brønsted-Lowry base, the conjugate acid, and the conjugate base. (a) H2SO4(aq) + H2O(1) - HSO4 (aq) + H30+(aq) (b) HCO3(aq) + H20(I) = H,CO3(aq) + OH(aq) 5. Using examples, distinguish between a Nucleophile vs Electrophile. Give at least 2 differences...
Identify whether each species functions as a Bronsted-Lowry acid or a Bronsted-Lowry base in this net ionic equation. + H3PO4 (aq) Brønsted-Lowry - + CIO Brønsted-Lowry H2P04 Brønsted-Lowry HCIO Brønsted-Lowry ' In this reaction: The formula for the conjugate of H3PO4 is The formula for the conjugate | of CIO is
16 EXPERIMENT 16 Pre-Lab Questions 1. What is a Bronsted-Lowry acid? : What is a Bronsted-Lowry base? 2. Provide the formula of the conjugate base for each of the following acids: a. HCI ΟΟΟΟΟΟΟΟΟυυυυυυυυυυυυυ b. HCO, c. H3PO4 3. The pH of blood is 7.4 and that for saliva is 6.4. Which of the two is more basic? PYRIGHT 2013 Cangage Learning
Complete the following acid/base reaction with curved arrows. Label Bronsted Acid (BA), Bronsted Base (BB), Conjugate Acid (CA), Conjugate Base (CB) or Lewis Acid (LA), Lewis Base (LB), when applicable. (5 Pts) + H-Br