Protons are good for cars, bad for breathing which we need electrons and well neutrons even though neutrons are pretty much neutral with no charge.
The electrons (negative) is what we need to support which everywhere you go to a city, town etc, you end up seeing pollution everywhere. The pollution is causing to eliminate the negative ions which we need the most.
The solution, get yourself an ionizer, I was told that it works like wonders!
Protons have a positive charge and electrons have a negative charge so they will attract each other, making a proton a good electron acceptor :)
No, in fact they are proton donours.
Acids are Proton donors Bases are Proton acceptors
Acids and bases have many definitions, but for your question, these will do: Bases are proton (H+) acceptors. Acids are proton (H+) releasers.
have a bitter taste, feel slippery, and are proton acceptors.
Bases are proton acceptors, so they will be positively charged - but only in presence of proton donators like acids or water (which dissociates into H+ and OH-). -- 100% pure bases aren't charged.
Fluorine is highly electronegative, but does not easily release a proton into aqueous solution. Because of this, it is not as strong an acid as HCl, HBr, HI, etc., which more easily release a proton into solution. For Bronsted-Lowry acids, the more easily a substance dissociates into a proton (or multiple protons) and an electronegative moiety, the stronger an acid it is. For Lewis acids, stronger acids are substances that are stronger electron acceptors.
Acids are Proton donors Bases are Proton acceptors
1) Bronsted-Lowry acids are proton donors. Bronsted-Lowry bases are proton acceptors. 2) Lewis acids are electron acceptors. Lewis bases are electron donors.
Acids and bases have many definitions, but for your question, these will do: Bases are proton (H+) acceptors. Acids are proton (H+) releasers.
1) Bronsted-Lowry acids are proton donors. Bronsted-Lowry bases are proton acceptors. 2) Lewis acids are electron acceptors. Lewis bases are electron donors.
No, in fact they are proton donours.
have a bitter taste, feel slippery, and are proton acceptors.
No. Proton acceptors.
1) Bronsted-Lowry acids are proton donors. Bronsted-Lowry bases are proton acceptors. 2) Lewis acids are electron acceptors. Lewis bases are electron donors.
Bases are proton acceptors, so they will be positively charged - but only in presence of proton donators like acids or water (which dissociates into H+ and OH-). -- 100% pure bases aren't charged.
Fluorine is highly electronegative, but does not easily release a proton into aqueous solution. Because of this, it is not as strong an acid as HCl, HBr, HI, etc., which more easily release a proton into solution. For Bronsted-Lowry acids, the more easily a substance dissociates into a proton (or multiple protons) and an electronegative moiety, the stronger an acid it is. For Lewis acids, stronger acids are substances that are stronger electron acceptors.
Acids: 1) Taste Sour 2) PH less than 7 3) Proton Donnors 4) Lewis Acids 5) React with Metals to give hydrogen 6) Electrolytes Bases: 1) Taste Bitter 2) PH greater than 7 3) Proton Acceptors 4) Electrolytes
Acids, bases and salts are chemical compounds. Examples are: Acids: sulfuric acid, nitric acid, stearic acid, phosphoric acid, hydrofluoric acid etc. Bases: sodium hydroxide, magnesium hydroxide, calcium hydroxide, lithium hydroxide etc. Salts: sodium chloride, gallium arsenide, potassium bromide, uranyl nitrate etc.