Hello, I am doing GCSE chemistry and would just lik to know the answer to this question.
When writing an ionic equation, why do you not split up the cation and anion when it is a solid or covalent compound, even though they are charged (e.g. for water, the oxygen used to have 6 electrons in its outer shell, but after reacting and forming a covalent bond, it gained 2 electrons and became oxygen 2- ion) And also why do you not split the solid up, despite them having a charge too?
Thanks for your help :)
When writing an ionic equation, why do you not split up the cation and anion when it is a solid or covalent compound, even though they are charged (e.g. for water, the oxygen used to have 6 electrons in its outer shell, but after reacting and forming a covalent bond, it gained 2 electrons and became oxygen 2- ion) And also why do you not split the solid up, despite them having a charge too?
Thanks for your help :)
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You don't split them up because you have to balance the charges.
Example: Na(+1) Cl(-1)
NaCl is balanced. That is always your aim is to make the charges balance.
Example: Each column of the periodic table is assigned an oxidation number with the exception of the transition metals.
So O(-2) H(+1)
H2O is balanced.
If you need more explaination just tell me
Example: Na(+1) Cl(-1)
NaCl is balanced. That is always your aim is to make the charges balance.
Example: Each column of the periodic table is assigned an oxidation number with the exception of the transition metals.
So O(-2) H(+1)
H2O is balanced.
If you need more explaination just tell me