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irina [24]
3 years ago
12

In the reaction between bromine and sodium, a bromine atom gains an electron. What ion is formed? Is the bromine oxidized, or is

it reduced?
Chemistry
2 answers:
Paraphin [41]3 years ago
4 0

Ion formed for bromine = Br-

And it's reduced in that case as it gained an electron

SVETLANKA909090 [29]3 years ago
3 0

Answer: The ion formed after the reduction of bromine is Br^-

Explanation:

The electronic configuration of Sodium (Na) = [Ne]3s^1

The electronic configuration of Bromine (Br) = [Ar]3d^{10}4s^24p^5

From the above configurations, Sodium ion will loose 1 electron in order to gain stable electronic configuration and that electron is accepted by the Bromine atom because it is 1 electron short of the stable electronic configuration.

Na\rightarrow Na^++e^-   (oxidation reaction)

Br+e^-\rightarrow Br^-   (Reduction reaction)

Bromine atom is reduced to form Br^-

Reduction reactions are the reactions in which the element gain electrons.

Oxidation reactions are the reactions in which the element looses its electrons.

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A white crystalline salt conducts electricity when it is melted and when it dissolves in water.
sergeinik [125]

Answer: Option (a) is the correct answer.

Explanation:

Ionic salts are defined as the salts which tend to contain ionic bonds as there occurs transfer of electrons between its combining atoms.

So, when an ionic salt melts or it is dissolved in water then it will dissociate into its respective ions and as electricity is the flow of electrons or ions. Hence, this salt is then able to conduct electricity.

As covalent compounds are insoluble in water so, they do no dissociate into ions. Hence, they do not conduct electricity.

Similarly, metallic and network solids do not dissociate into ions either when melted or dissolved in water. Therefore, they also do not conduct electricity.

Thus, we can conclude that when a white crystalline salt conducts electricity when it is melted and when it dissolves in water then this bond is of ionic type.

7 0
3 years ago
Calculate the standard cell potential given the following standard reduction potentials: Al3++3e−→Al;E∘=−1.66 V Cu2++2e−→Cu;E∘=0
Maru [420]

Answer:

Explanation:

To calculate the cell potential we use the relation:

Eº cell = Eº oxidation + Eº reduction

Now in order to determine which of the species is going to be oxidized, we have to remember that the more the value of the reduction potential is negative,  the greater its tendency to be oxidized is. In electrochemistry we use the values of the reductions potential in the tables for simplicity  because the only thing we need to do is change the sign of the reduction potential for the oxized species .

So the species that is going to be oxidized is the Aluminium, and therefore:

Eº cell = -( -1.66 V ) + 0.340 V =  5.06 V

Equally valid is to write the equation as:

Eº cell = Eº reduction for the reduced species - Eº reduction for the oxidized species

These two expressions are equivalent, choose the one you fell more comfortable but be careful with the signs.

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