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

what are the óptions. pléase list them

8

explanation:

each principal energy level above the first contains one s orbital and three p orbitals. a set of three p orbitals, called the p sublevel, can hold a maximum of six electrons. therefore, the second level can contain a maximum of eight electrons - that is, two in the s orbital and 6 in the three p orbitals.

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