The elements with the electron configurations that end in ns 2 and np 5 are halogens, group VII A elements.
The elements with electron configurations that end in ns 2 and np 5 are found in Group 17 of the periodic table, known as the halogens. This group includes elements such as fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At).
The general electron configuration for atoms in Group 5A is ns^2 np^3, where "n" represents the principal energy level. This group includes elements like nitrogen, phosphorus, arsenic, antimony, and bismuth.
Electron configuration of neptunium: [Rn]7s26d15f4
This description fits elements in the lanthanide and actinide series of the periodic table. These elements have their highest occupied s sublevel and a nearby f sublevel containing electrons due to the electron configurations in their atoms.
The valence electron configuration for Group 6A elements is ns^2 np^4. This means that Group 6A elements have 6 valence electrons in their outermost shell.
The elements with electron configurations that end in ns 2 and np 5 are found in Group 17 of the periodic table, known as the halogens. This group includes elements such as fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At).
Similarities: - Np and Pu are radioactive, unstable chemical elements - Np and Pu are man made - Np and Pu are dangerous - Np and Pu are fissionable with thermal neutrons
The general electron configuration for atoms in Group 5A is ns^2 np^3, where "n" represents the principal energy level. This group includes elements like nitrogen, phosphorus, arsenic, antimony, and bismuth.
Electron configuration of neptunium: [Rn]7s26d15f4
This description fits elements in the lanthanide and actinide series of the periodic table. These elements have their highest occupied s sublevel and a nearby f sublevel containing electrons due to the electron configurations in their atoms.
The halogens are is group VII (17), and thus they all have 7 valence electrons. These will be located in different energy levels for the different halogens, but since they are all also p-block elements, they will all have ns^2 np^5 electron configurations, where n is the period number. Examples: Cl will be [Ne] 3s^2 3p^5 and Br will be [Ar] [Ar] 4s2 3d10 4p5 (note the inclusion of the d-block electrons for Br).
The valence electron configuration for Group 6A elements is ns^2 np^4. This means that Group 6A elements have 6 valence electrons in their outermost shell.
House codes:/np @931629/np @709003Bootcamp like codes:/np @172976/np @608368/np @191205/np @842019/np @159932/np @593204/np @145219/np @1450120/np @449496/np @618999/np @801683/np @1014313/np @1444036/np @633644/np @808800/np @1444041Thats all I got sorry if some don't work I didn't check them allIf you want to find me on TFM my user is Butterbe
House codes: /np @931629 /np @709003 Bootcamp like codes: /np @172976 /np @608368 /np @191205 /np @842019 /np @159932 /np @593204 /np @145219 /np @1450120 /np @449496 /np @618999 /np @801683 /np @1014313 /np @1444036 /np @633644 /np @808800 /np @1444041 That's all I know, but I hope it'll be to help ^^
It is the reverse: Np-235 decay to U-235 by electron capture.
The halogens are is group VII (17), and thus they all have 7 valence electrons. These will be located in different energy levels for the different halogens, but since they are all also p-block elements, they will all have ns^2 np^5 electron configurations, where n is the period number. Examples: Cl will be [Ne] 3s^2 3p^5 and Br will be [Ar] [Ar] 4s2 3d10 4p5 (note the inclusion of the d-block electrons for Br).
All are radioactive, artificial elements (but note that Np and Pu can exist also naturally in extremely low concentrations).