What is the electron configuration for As. [Ar]
When I looked on the periodic table, it didn't make sense because [Ar] comes before As.
3.) Predict ground-state electron configuration. Write in abbreviated form using noble gas in brackets.
a.) Cr^2+
b.) Cu^2+
c.) Co63+
What is your problem in doing this? What do you not understand?
The electron configuration for arsenic (As) is actually not simply [Ar]. The [Ar] represents the electron configuration of the noble gas argon (Ar), which is the nearest noble gas before arsenic in the periodic table. The electron configuration of an atom describes how its electrons are distributed within its orbitals.
To determine the electron configuration of arsenic (As), you need to consider the distribution of electrons in each energy level (shell) and within each sublevel (s, p, d, f). Arsenic has an atomic number of 33, which means it has 33 electrons.
The electron configuration of arsenic is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p³.
Let's break down how we arrived at this electron configuration:
1s²: This represents the first energy level (n=1) and the 1s sublevel, with 2 electrons.
2s²: This represents the second energy level (n=2) and the 2s sublevel, with 2 electrons.
2p⁶: This represents the second energy level (n=2) and the 2p sublevel, with 6 electrons.
3s²: This represents the third energy level (n=3) and the 3s sublevel, with 2 electrons.
3p⁶: This represents the third energy level (n=3) and the 3p sublevel, with 6 electrons.
4s²: This represents the fourth energy level (n=4) and the 4s sublevel, with 2 electrons.
3d¹⁰: This represents the third energy level (n=3) and the 3d sublevel, with 10 electrons.
4p³: This represents the fourth energy level (n=4) and the 4p sublevel, with 3 electrons.
So, the electron configuration for arsenic is [Ar] 3d¹⁰ 4s² 4p³. The [Ar] represents the filled inner energy levels up to the noble gas argon.
Remember, the electron configuration follows the pattern of filling up the orbitals according to the Aufbau principle, the Pauli exclusion principle, and Hund's rule.