The electron configuration of arsenic (At) is 4s2 3d10 4p3.
The electron configuration of arsenic allows it to combine in several different valances, including -3, 0, +3 and +5. It combines with other elements, including hydrogen, oxygen, the halogens and sulfur.
Many of these compounds are extremely poisonous. Arsenic (III) oxide, white arsenic is one of the most well-known. In dilute concentrations, too weak to be poisonous, arsenic is a carcinogen, according to Reference.com.
To come up with the electron configuration for Arsenic, you first need to count up how many electrons it has (it will be the same as the atomic number since the charge is neutral)... 18. Then you need to follow the aufbui order and work your way up the orbitals filling them in. 1s takes 2electrons, 2s takes 2 electrons, 2p takes 6 electrons, 3s takes 2 electrons, and lastly 3p takes 6 electrons (total of 18). The order of the orbitals and how many electrons each can take you will just need to memorize or learn some tricks to remember.
You can also just take a short cut and ignore all the orbitals before the row Arsenic is on to show ONLY the valence electrons, ie:
[Ne] 3s2 3p6
If you are still having trouble, http://mymcat.com/wiki/Electron_Configuration, has a lot of examples, including your question.
Arsenic is in period 4, so valence electrons will be in 4th shell. It is a p block element, so filling orbitals will be p (4p), and it comes after transition elements, so it will have the 3d orbitals already filled. Thus, it will be [Ar]4s2 3d10 4p3
I believe there are many excited states...and only one ground state. (wrong) 1s22s22p63s23p64s23d104p25s1. just take the last electron in the ground state and bump it up one level....
electron configuration: [Ar] 4s2 3d10 4p3
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3
4s2 3d10 4p3
1s22s22p63s2sp6
The electron configuration of 1s22s22p3s1 is not the ground state electron configuration of any element. This configuration contains 8 electrons, which in the ground state would be oxygen. The ground state configuration of oxygen is 1s22s22p4.
Ground state electron configuration of zinc (Zn): [Ar]3d104s2.
The expected ground-state electron configuration of copper is ; however, the actual configuration is because a full dsubshell is particularly stable. There are 18 other anomalous elements for which the actual electron configuration is not what would be expected.
The ground-state electron configuration for a neutral atom of manganese is: 1s22s22p63s23p63d54s2 or [Ar]3d54s2
[Xe]6s24f1
The electron configuration of 1s22s22p3s1 is not the ground state electron configuration of any element. This configuration contains 8 electrons, which in the ground state would be oxygen. The ground state configuration of oxygen is 1s22s22p4.
Ground state electron configuration of zinc (Zn): [Ar]3d104s2.
The ground state electron configuration for nitrogen is [He]2s2.2p3.
The expected ground-state electron configuration of copper is ; however, the actual configuration is because a full dsubshell is particularly stable. There are 18 other anomalous elements for which the actual electron configuration is not what would be expected.
The ground state electron configuration of the hydrogen atom is 1s1, and for helium it is 1s2.
ground state
The symbol for sulfur is S. Its electron configuration is 1s22s22p63s23p4
The most likely electron configuration for a sodium ion in its ground state is 1s22s22p63s1.
The ground-state electron configuration for a neutral atom of manganese is: 1s22s22p63s23p63d54s2 or [Ar]3d54s2
Arsenic is paramagnetic because the electron configuration is {Ar}4s^2,3d^10,4p^3. Due to the unpaired electron at the end (4p^*3*) the atom in ground state is paramagnetic. **OR Arsenic would be paramagnetic since the 4 p orbitals each contain one electron with parallel spin. These three unpaired electrons give arsenic its paramagnetic property.
Hydrogen electron configuration will be 1s1.
The electron configuration of gallium is: [Ar]3d104s24p1.