I think this question should be read (and written) like:
"What is the electron configuration ending in 4s2 4p5 " because 4p2 4p5 is an unusual and even impossible ending of any electronconfiguration.
Answer:
Bromium, number 35, ends with ... (3d10) 4s2 4p5 (period 4, group 17)
This electron configuration represents the element Selenium, with 34 electrons. It is located in the fourth period of the periodic table, in Group 16. The configuration includes filled sublevels up to the 4p orbital.
The correct electron configuration for arsenic is [Ar] 4s2 3d10 4p3.
The electron configuration of arsenic is [Ar] 3d10 4s2 4p3. This means that arsenic has 2 electrons in its outermost shell (4s2 4p3) and belongs to the p-block of the periodic table.
The electron configuration for arsenic is [Ar] 4s2 3d10 4p3, where [Ar] represents the electron configuration of argon before it. This corresponds to the placement of 33 electrons within the various orbitals of an arsenic atom.
Krypton. In order to find this you have to look at the periodic table. Imagine the periodic table is divided into three sections, the first two columns, 1A and 2A, the middle section, the transition metals, and the right side, 3A to 7A. The first two columns are the s electrons, the middle section is the d electrons, and the right side is the p electrons (oversimplification). 4s2 4p6 means go to the 4th period (row). two s's and 6 p's. Just count it. the 4th element in the p electrons in the 4th period is Krypton.
The electron configuration of neutral arsenic (As) is [Ar] 4s2 3d10 4p3. Since As3- has gained three extra electrons, the electron configuration becomes [Ar] 4s2 3d10 4p6, as the additional electrons fill the 4p subshell.
That is Arsenic.
This electron configuration represents the element Selenium, with 34 electrons. It is located in the fourth period of the periodic table, in Group 16. The configuration includes filled sublevels up to the 4p orbital.
[Ar] 4s2 3d10 4p3
The correct electron configuration for arsenic is [Ar] 4s2 3d10 4p3.
The electron configuration of arsenic is [Ar] 3d10 4s2 4p3. This means that arsenic has 2 electrons in its outermost shell (4s2 4p3) and belongs to the p-block of the periodic table.
1s2 2s2 2p6 3s2 3d10 4s2 4p3
[Ar] 4s2 3d10 4p3
The mistake in this electron configuration is in the 5p subshell, where it shows 5p5 instead of 5p6. The correct element for this configuration is Xenon (Xe). The correct electron configuration for Xenon is [Kr] 5s2 4d10 5p6.
The noble gas configuration for arsenic (As) is [Ar] 3d10 4s2 4p3. This means that it has the same electron configuration as argon (Ar) up to its previous noble gas, with additional electrons filling the 3d, 4s, and 4p sublevels.
[Ar] 4s2 3d10 4p3 or 2, 8, 18, 5
The electron configuration for arsenic is [Ar] 4s2 3d10 4p3, where [Ar] represents the electron configuration of argon before it. This corresponds to the placement of 33 electrons within the various orbitals of an arsenic atom.