QQuestionChemistry
QuestionChemistry
For each atom in the table below, write down the subshell from which an electron would have to be removed to make a + 1 cation, and the subshell to which an 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 | 1s | 1s |
| Hg | | |
| Ne | | |
| K | | |
| × | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | | |
12 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
Step 1:: To make a + 1 cation, we need to remove an electron from the outermost shell.
"Hg (+1) cation" \Rightarrow "remove 1 electron from 6s subshell"
For Hg, the outermost shell is the 6s subshell.
Step 2:: To make a - 1 anion, we need to add an electron to the outermost shell.
"Hg (-1) anion" \Rightarrow "add 1 electron to 6s subshell"
For Hg, the outermost shell is the 6s subshell.
Step 3:: For Ne, the outermost shell is the 2s and 2p subshells.
"Ne (-1) anion" \Rightarrow "add 1 electron to 2s subshell"
However, the 2p subshell is completely filled with 6 electrons, so we cannot add an electron to it. Therefore, the 2s subshell will be the one to which an electron is added to form a - 1 anion.
Step 4:: For Ne, the outermost shell is the 2s and 2p subshells.
"Ne (+1) cation" \Rightarrow "remove 1 electron from 2p subshell"
However, the 2s subshell is completely filled with 2 electrons, so we cannot remove an electron from it. Therefore, we need to remove an electron from the 2p subshell to form a + 1 cation.
Step 5:: For K, the outermost shell is the 4s and 3d subshells.
"K (-1) anion" \Rightarrow "add 1 electron to 4s subshell"
However, the 3d subshell is completely filled with 10 electrons, so we cannot add an electron to it. Therefore, the 4s subshell will be the one to which an electron is added to form a - 1 anion.
Step 6:: For K, the outermost shell is the 4s and 3d subshells.
"K (+1) cation" \Rightarrow "remove 1 electron from 4s subshell"
The 4s subshell contains only 1 electron, so we can remove it to form a + 1 cation.
Final Answer
| atom | subshell from which electron removed to form + 1 cation | subshell to which electron added to form - 1 anion | | --- | --- | --- | | H | 1s | 1s | | Hg | 6s | 6s | | Ne | 2p | 2s | | K | 4s | 4s | Note: The subshells for forming cations and anions are based on the electron configuration of the neutral atoms. The actual electron configuration of the ions may differ due to the rearrangement of electrons to achieve stability.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students