QQuestionChemistry
QuestionChemistry
For each atom in the table below, write down the subshell from which an electron would have to electron would have to be added to make a - 1 anion.
The first row has been completed for you.
| atom | subshell from which electron removed to form + 1 cation | subshell to which electron added to form - 1 anion |
| --- | --- | --- |
| H | 1x | 1x |
| C | | |
| Ti | | |
| Ar | | |
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Answer
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Step 1:: To determine the subshell to which an electron must be added to form a - 1 anion, we need to find the outermost subshell in each atom.
This is the subshell that can accommodate one more electron to complete the octet and form a stable - 1 anion.
Step 2:: For Carbon (C), the atomic number is 6, and its electron configuration is 1s^2 2s^2 2p^2.
The outermost subshell is $$2p$$.
Therefore, an electron must be added to the 2p subshell to form a - 1 anion.
Step 3:: For Titanium (Ti), the atomic number is 22, and its electron configuration is 1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2 4p^6 4d^{2}.
The outermost subshell is $$4d$$.
Therefore, an electron must be added to the 4d subshell to form a - 1 anion.
Step 4:: For Argon (Ar), the atomic number is 18, and its electron configuration is 1s^2 2s^2 2p^6 3s^2 3p^6.
The outermost subshell is $$3p$$.
Therefore, an electron must be added to the 3p subshell to form a - 1 anion.
Final Answer
| atom | subshell from which electron removed to form + 1 cation | subshell to which electron added to form - 1 anion | | --- | --- | --- | | H | 1s | 1s | | C | 2s or 2p | 2p | | Ti | 4s or 3d or 4p | 4d | | Ar | 3p | 3p | Note: For Carbon, either the 2s or 2p subshell can be used to form a + 1 cation, depending on the specific chemical reaction. Similarly, for Titanium, either the 4s, 3d, or 4p subshell can be used to form a + 1 cation, depending on the specific chemical reaction.
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