Chlorine forms a number of oxides with the following oxidation numbers: 1, 3, 4, 6, and 7. These compounds are stable and neutra
1 answer:
Answer:
,
,
,
,
Explanation:
Empirical formula of the compound is the simplest ratio of elements present in the compound.
Empirical formula of compounds of chlorine with oxygen is as follows:
Compounds in which oxidation state of Cl is +1
Compounds in which oxidation state of Cl is +3
Compounds in which oxidation state of Cl is +4
Compounds in which oxidation state of Cl is +6
Compounds in which oxidation state of Cl is +7
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<u>Answer:</u> The complete molecular, ionic, and net ionic equations are given below. The spectator ions are sodium and nitrate ions.
<u>Explanation:</u>
The ionic equation is defined as the equation in which all the substances that are strong electrolytes present in an aqueous state and are represented in the form of ions.
The net ionic equation is defined as the equations in which spectator ions are not included.
Spectator ions are the ones that are present equally on the reactant and product sides. They do not participate in the reaction.
The balanced molecular equation for the reaction of lead (II) nitrate and sodium sulfide follows:
The ionic equation follows:
As sodium and nitrate ions are present on both sides of the reaction. Thus, they are considered spectator ions.
The net ionic equation follows: