The elements with the electron configurations that end in ns 2 and np 5 are halogens, group VII A elements.
The elements with the electron configurations that end in ns 2 and np 5 are halogens, group VII A elements.
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 the electron configurations that end in ns 2 and np 5 are halogens, group VII A elements.
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).