Summary
Highlights
The video starts by defining an acid as a compound where one or more H+ ions are bonded to a negative ion. It demonstrates how to break down common acid formulas into their H+ and negative ion components, emphasizing that the charges must balance. The key takeaway is that an acid's name is based on the name of its negative ion.
For acids that do not contain oxygen, the naming rule is introduced. If the negative ion ends in -ide (e.g., chloride, bromide), you remove -ide and place the stem of the name between 'hydro-' and '-ic acid'. Examples like HCl (hydrochloric acid) and HBr (hydrobromic acid) are used to illustrate this rule.
For acids containing oxygen, the negative ions are polyatomic ions. If the polyatomic ion ends in -ate (e.g., nitrate, carbonate), you remove -ate and replace it with '-ic acid'. Examples include HNO3 (nitric acid) and H2CO3 (carbonic acid).
If the polyatomic ion ends in -ite (e.g., nitrite, chromite), you remove -ite and replace it with '-ous acid'. Examples provided are HNO2 (nitrous acid) and HCrO2 (chromous acid).
A mnemonic is provided to easily remember the naming rules: 'My ride has hydraulics' (for -ide to hydro-ic acid), 'I ate something icky' (for -ate to -ic acid), and 'Sprite, it is delicious-o us' (for -ite to -ous acid).
The video highlights exceptions for acids containing phosphate, phosphite, sulfate, and sulfite. For phosphate and phosphite, an 'o' is added before the '-ic' or '-ous' (e.g., phosphoric acid, phosphorous acid). For sulfate and sulfite, 'ur' is added (e.g., sulfuric acid, sulfurous acid).
When dealing with polyatomic ions that start with 'hypo' or 'per', the video clarifies that only the ending (-ate or -ite) is relevant for naming the acid. Examples like permanganate becoming permanganic acid and hypochlorite becoming hypochlorous acid are used to demonstrate this.