Write the actual electronic configuration of Chromium and Europium. Why are they different from the expected configuration (trend)?
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Some elements do not follow the Aufbau principle, there are some alternate ways that electrons can arrange themselves that give these elements better stability.
Explanation:
Using the Aufbau principle, you would write the following electron configurations
Cr = [Ar] 4s2 3d4
Cu = [Ar] 4s2 3d9
The actual electron configurations are:
Cr = [Ar] 4s1 3d5
Cu = [Ar] 4s1 3d10
To understand why this occurs, it is important to realize that...
1. Completely filled sublevels are more stable than partially filled sublevels.
2. A sublevel which is exactly half filled is more stable than a partially filled sublevel which is not half full.
Explanation:
Using the Aufbau principle, you would write the following electron configurations
Cr = [Ar] 4s2 3d4
Cu = [Ar] 4s2 3d9
The actual electron configurations are:
Cr = [Ar] 4s1 3d5
Cu = [Ar] 4s1 3d10
To understand why this occurs, it is important to realize that...
1. Completely filled sublevels are more stable than partially filled sublevels.
2. A sublevel which is exactly half filled is more stable than a partially filled sublevel which is not half full.
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Answer:
In writing the electron configuration for Chromium the first two electrons will go in the 1s orbital. ... After the 4s is full we put the remaining four electrons in the 3d orbital and end with 3d4. Therefore the expected electron configuration for Chromium will be 1s22s22p63s23p44s23d9.
Explanation:
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