Oxidation reaction is a type of reaction wherein there is a loss of electrons. An oxidation reaction may also be a reducing agent. Example is the reaction Zn + 2H+ = Zn2+ + H2. When you separate them by their half cell reaction, you have 2H+ 1e- = H2. H here is the reducing agent and has lost 1 electron in the process.
protons
neutrons
electrons
A Brønsted-Lowry base is a species that accepts a proton (hydrogen ion) from another species. NH3, OH-, and even water itself are examples of Brønsted-Lowry bases, denoting they accept protons.
A Brønsted-Lowry base is a species that can accept a proton (a hydrogen ion) from another species. For instance, in a reaction between water and ammonia, NH3 is the Brønsted-Lowry base because it accepts a proton from water. This means that any species capable of accepting a proton, such as hydroxide ion (OH-), ammonia (NH3), or water itself can be considered a Brønsted-Lowry base.
For example, think about the dissociation of water:
H2O + H2O ⇌ H3O+ + OH-
In this reaction, water is acting as both a Brønsted-Lowry acid and a Brønsted-Lowry base. One water molecule donates a proton and becomes a hydroxide ion (the conjugate base), while the other accepts a proton to become hydronium (the conjugate acid).
Another example would be the ionization of ammonia in water:
NH3 + H2O ⇌ NH4+ + OH-
Here, ammonia (NH3) is the Brønsted-Lowry base as it accepts a proton from water to become ammonium (NH4+).
#SPJ12
2) KHSO3+ and O2– ions
3) K+ and HS– ions
4) K+ and HSO4– ions.
In the compound KHSO4, there is an ionic bond between the K+ and HSO4– ions.
Ionic bond is a type of bond that is formed between metals and non metals. During the reaction, metals usually donate electron[s] to non metals. The metals thus become positively charged while the non metals become negatively charged. Therefore, ionic compound are usually composed of charged particles. For the ionic compound given above, the charged particles in the compound are K+ and HSO4- ions.