Determine which ions have noble-gas configurations:
Cd2+
Ru3+
P3−
As3−
Ag+
Zr4+
Thanks for any help. (I tried As3- and Zr4+, but that was wrong, so maybe i'm just missing one.
For anyone looking for the answer for mastering chemistry, it’s As3- Zr4+ and P3-
Oh, it seems like even ions can be confused sometimes! Let me help you sort this out:
Cd2+ - Cadmium (Cd) has an electron configuration of [Kr] 4d10 5s2, so removing 2 electrons leaves it with the noble-gas configuration of [Kr].
Ru3+ - Ruthenium (Ru) has an electron configuration of [Kr] 4d7 5s1, so losing 3 electrons leads to the noble-gas configuration of [Kr].
P3- - Phosphorus (P) has an electron configuration of [Ne] 3s2 3p3. By gaining 3 electrons, it completes the noble-gas configuration of [Ne].
As3- - Arsenic (As) has an electron configuration of [Ar] 4s2 3d10 4p3. Unfortunately, by gaining 3 electrons, it does not obtain a noble-gas configuration.
Ag+ - Silver (Ag) has an electron configuration of [Kr] 4d10 5s1. Losing an electron still leaves it one electron short of achieving a noble-gas configuration.
Zr4+ - Zirconium (Zr) has an electron configuration of [Kr] 4d2 5s2. Eliminating 4 electrons brings it to the noble-gas configuration of [Kr].
So, the ions that have noble-gas configurations are Cd2+, Ru3+, P3−, and Zr4+.
To determine which ions have noble-gas configurations, we need to compare the electron configurations of the ions to the electron configurations of noble gases.
The noble gases have a full outer electron shell, meaning that they have achieved a stable electron configuration. Therefore, we can compare the electron configurations of the given ions to the electron configurations of the noble gases to see if any match.
Here are the electron configurations of the noble gases:
- Helium (He): 1s^2
- Neon (Ne): 1s^2 2s^2 2p^6
- Argon (Ar): 1s^2 2s^2 2p^6 3s^2 3p^6
- Krypton (Kr): 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6
- Xenon (Xe): 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6
Now, let's determine which ions have noble-gas configurations:
1. Cd2+: The electron configuration of Cd is [Kr] 4d^10 5s^2. When Cd loses two electrons to form Cd2+, it becomes [Kr] 4d^10, which is the electron configuration of Kr. Therefore, Cd2+ has a noble-gas configuration.
2. Ru3+: The electron configuration of Ru is [Kr] 4d^7 5s^1. When Ru loses three electrons to form Ru3+, it becomes [Kr] 4d^5, which is not the electron configuration of any noble gas. Therefore, Ru3+ does not have a noble-gas configuration.
3. P3-: The electron configuration of P is 1s^2 2s^2 2p^6 3s^2 3p^3. When P gains three electrons to form P3-, it becomes 1s^2 2s^2 2p^6 3s^2 3p^6, which is the electron configuration of Ne. Therefore, P3- has a noble-gas configuration.
4. As3-: The electron configuration of As is [Ar] 3d^10 4s^2 4p^3. When As gains three electrons to form As3-, it becomes [Ar] 3d^10 4s^2 4p^6, which is not the electron configuration of any noble gas. Therefore, As3- does not have a noble-gas configuration.
5. Ag+: The electron configuration of Ag is [Kr] 4d^10 5s^1. When Ag loses one electron to form Ag+, it becomes [Kr] 4d^10, which is the electron configuration of Kr. Therefore, Ag+ has a noble-gas configuration.
6. Zr4+: The electron configuration of Zr is [Kr] 4d^2 5s^2. When Zr loses four electrons to form Zr4+, it becomes [Kr], which is the electron configuration of Kr. Therefore, Zr4+ has a noble-gas configuration.
Based on the analysis, the ions with noble-gas configurations are: Cd2+, P3-, Ag+, and Zr4+.
Dial up each and take a look at adding or subtracting electrons to make the ion isoelectronic with a noble gas.
don't think Zr^4+ will do it.
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