All of them. There is no problem with elements not having stable electron configurations. The only stability issue concerns the nucleus, not the electrons-- all elements except helium have isotopes with unstable nuclei, some have only unstable nuclei (radioactive elements), and some have only very short-lived unstable nuclei.
The elements with electron configurations ending in ns2np5 are the halogens in Group 17 of the periodic table. This includes fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). These elements have seven valence electrons and readily gain an electron to achieve a stable octet configuration.
Yes, noble gases are stable elements in the periodic table because they have a full outer electron shell, making them less likely to react with other elements.
The electron configurations of LiF will be the same as the electron configurations of atoms in Group 18 (noble gases) because Li will lose its single electron to attain a stable octet similar to the noble gases, while F will gain an electron to achieve a complete valence shell.
The elements in Group 7A (halogens) on the periodic table would need only 1 electron to achieve a stable electron configuration by filling their outermost shell with 8 electrons. For example, elements like fluorine, chlorine, and bromine each need only 1 more electron to reach stability.
The noble gases are found in the last column of the periodic table, known as Group 18 or Group 8A. This group includes elements such as helium, neon, argon, krypton, xenon, and radon. They are known for their low reactivity and stable electron configurations.
The elements with electron configurations ending in ns2np5 are the halogens in Group 17 of the periodic table. This includes fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). These elements have seven valence electrons and readily gain an electron to achieve a stable octet configuration.
protons
Noble gases actually have the most stable electronic configurations in the periodic table due to having a full outer shell of electrons. This full octet makes them less likely to react with other elements, earning them the name "noble gases."
no
Group 8A elements in the periodic table are the noble gases, which include helium, neon, argon, krypton, xenon, and radon. These elements are known for their stable electron configurations and lack of reactivity.
Yes, noble gases are stable elements in the periodic table because they have a full outer electron shell, making them less likely to react with other elements.
Group 18 as they have completely filled electronic configurations, are stable and hence do not ionize.
any time there are as many electrons and protons and they fill each orbital optimally.
The noble gases are found in column 18 (VIII Group) of the periodic table. This group includes elements such as helium, neon, argon, krypton, xenon, and radon. These elements are characterized by their stable electron configurations and lack of reactivity.
Strutt and Ramsey discovered the noble gases, which include helium, neon, argon, krypton, xenon, and radon. These elements are characterized by their low reactivity and stable electron configurations. Their discovery was a significant contribution to the periodic table of elements.
Element 118, Oganesson (Og), belongs to the noble gases family, also known as group 18 on the periodic table. These elements are characterized by their stable electron configurations and low reactivity.
The electron configurations of LiF will be the same as the electron configurations of atoms in Group 18 (noble gases) because Li will lose its single electron to attain a stable octet similar to the noble gases, while F will gain an electron to achieve a complete valence shell.