Key Terms week 2-adv chem.docx - Key Terms Arrhenius Acids Amphoteric Strong Acid Monoprotic Diprotic pH Strong base Conjugate acid Lewis acid Lewis

Key Terms week 2-adv chem.docx - Key Terms Arrhenius Acids...

This preview shows page 1 - 2 out of 2 pages.

Key Terms Definition Arrhenius Acids acid-base reactions are characterized by acids, which dissociate in aqueous solution to form hydrogen ions (H+) and bases, which form hydroxide (OH−) ions. Acids are defined as a compound or element that releases hydrogen (H+) ions into the solution. Amphoteric (of a compound, especially a metal oxide or hydroxide) able to react both as a base and as an acid. Strong Acid one that completely ionizes (dissociates) in a solution (provided there is sufficient solvent). In water, one mole of a strong acid HA dissolves yielding one mole of H+ (as hydronium ion H3O+) and one mole of the conjugate base, A−. Essentially, none of the non-ionized acid HA remains. Monoprotic an acid that donates only one proton or hydrogen atom per molecule to an aqueous solution. This contrasts with acids capable of donating more than one proton or hydrogen, which are called polyprotic acids. Diprotic a class of Arrhenius acids which can donate two protons or hydrogen cations per molecule when dissociating in aqueous solutions.
Image of page 1
Image of page 2

You've reached the end of your free preview.

Want to read both pages?

  • Summer '17

  • Left Quote Icon

    Student Picture

  • Left Quote Icon

    Student Picture

  • Left Quote Icon

    Student Picture

Stuck? We have tutors online 24/7 who can help you get unstuck.
A+ icon
Ask Expert Tutors You can ask You can ask You can ask (will expire )
Answers in as fast as 15 minutes