Which best describes the reducing agent in the reaction below? Cl2(aq) + 2Br(aq) 2Cl(aq) + Br2(aq) Bromine (Br) loses an electron, so it is the reducing agent. Bromine (Br) gains an electron, so it is the reducing agent. Chlorine (Cl) loses an electron, so it is the reducing agent. Chlorine (Cl) gains an electron, so it is the reducing agent.

Bromine (Br) loses an electron, so it is the reducing agent.

Explanation:

A reducing agent also called a reducer, is known to be an electron donor. A reducing agent is oxidized, because it loses electrons in the redox reaction.

A oxidising agent also called a oxidant or oxidiser, is known to be an electron acceptor. A oxidising agent is reduced, because it gains electrons in the redox reaction.

Cl2(aq) + 2Br-(aq) --> 2Cl-(aq) + Br2(aq)

Half ionic equations,

Cl2(aq) + 2e- --> 2Cl-(aq)

2Br-(aq) --> Br2(aq) + 2e-

Reducing agent = Br-

Oxidizing agent = Cl2

A

Explanation:

Bromine (Br) loses an electron, so it is the reducing

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.