CHM 233 SI Session Acid+Base Terminology

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Fun way to practice these concepts and this information!

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Kaveh Miller

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CHM 233 SI Session Acid+Base Terminology


CHM 233 SI Session Acid+Base TerminologyVersion en ligne Fun way to practice these concepts and this information! par Kaveh Miller 1 Lewis Acid a Electron Donor b Electron Acceptor c Proton Donor d Proton Acceptor 2 Lewis Base a Electron Donor b Electron Acceptor c Proton Donor d Proton Acceptor 3 Brønsted-Lowry Acid a Proton Donor b Proton Acceptor c Electron Donor d Electron Acceptor 4 Brønsted-Lowry Base a Proton Donor b Proton Acceptor c Electron Donor d Electron Acceptor 5 Strong Acids can be described as Choose one or more answers a Having a highly stable conjugate base (which is nonreactive) b Having a highly unstable conjugate base (which is reactive) c Being highly reactive themselves (and therefore less stable than their conjugate base alternative) d Being highly nonreactive themselves(and therefore more stable than their conjugate base alternative) e Being favored in the equilibrium 6 Weak Acids can be described as Choose one or more answers a Having a highly stable conjugate base (which is nonreactive) b Having a highly unstable conjugate base (which is reactive) c Being highly reactive themselves (and therefore less stable than their conjugate base alternative) d Being highly nonreactive themselves(and therefore more stable than their conjugate base alternative) e Being favored in the equilibrium Feedback 1 Lewis Acids and Bases are mainly concerned with electrons. Lewis acids are electrophile and lewis bases are nucleophiles. 2 Lewis Acids and Bases are mainly concerned with electrons. Lewis acids are electrophile and lewis bases are nucleophiles. 3 All Brønsted-Lowry acids/bases are concerned with protons and their movement. Generally speaking, bases will be negatively charged or neutral. 4 All Brønsted-Lowry acids/bases are concerned with protons and their movement. Generally speaking bases will be negatively charged or neutral. 5 Strong acids will want to deprotonate in order to become their more stable conjugate base form. Due to this, they will be highly reactive when in the presence of a base to reach that more stable form. The equilibrium will not favor the strong acid species as it is less stable. 6 A weak acid will not want to react as much when combined with a base. Usually this is due to the instability of its conjugate base, or its deprotonated form, which means the reaction will favor the weak acid species as it is "happier" being here.

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CHM 233 SI Session Acid+Base Terminology

Test

À propos de cette activité

Créé par

Téléchargez la version pour jouer sur papier

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CHM 233 SI Session Acid+Base TerminologyVersion en ligne

par Kaveh Miller

Lewis Acid

Lewis Base

Brønsted-Lowry Acid

Brønsted-Lowry Base

Strong Acids can be described as

Choose one or more answers

Weak Acids can be described as

Choose one or more answers

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