Full form: 1s1.
it doesn't have noble gas configuration as there is no noble gas before hydrogen
The electron configuration of cesium in noble gas form would be [Xe] 6s^1. This indicates that cesium has the same electron configuration as the noble gas xenon in addition to one extra electron in the 6s orbital.
Transition metals such as copper, silver, and gold can form ions with a noble gas electron configuration. This occurs when they lose electrons to achieve a stable electron configuration similar to the nearest noble gas.
[Kr] 5s24d105p4
The long form electron configuration for carbon is simply 1s2 2s2 2p2. The noble gas shortcut electron configuration for C is [He] 2s2 2p2.
Iodine accepts one electron to achieve noble gas configuration. Strontium loses two electrons to achieve noble gas configuration. Nitrogen accepts three electrons to achieve noble gas configuration. Krypton already has a noble gas configuration.
They achieve the electron configuration of a noble gas.
[Kr] 5s24d105p4
The electron configuration of cesium in noble gas form would be [Xe] 6s^1. This indicates that cesium has the same electron configuration as the noble gas xenon in addition to one extra electron in the 6s orbital.
The long form electron configuration for carbon is simply 1s2 2s2 2p2. The noble gas shortcut electron configuration for C is [He] 2s2 2p2.
Iodine accepts one electron to achieve noble gas configuration. Strontium loses two electrons to achieve noble gas configuration. Nitrogen accepts three electrons to achieve noble gas configuration. Krypton already has a noble gas configuration.
Transition metals such as copper, silver, and gold can form ions with a noble gas electron configuration. This occurs when they lose electrons to achieve a stable electron configuration similar to the nearest noble gas.
Hydrogen and helium have different valence electron configurations. Hydrogen has one valence electron, and helium has two valence electrons. However, hydrogen does typically form covalent bonds in which it shares an electron, and thereby gains an effective electron configuration of two, like helium. Hydrogen also can form the H+ ion which has no electrons.
Group IA atoms need to lose 1 electron to achieve a noble gas configuration. This will result in a full outer shell, similar to the nearest noble gas in the periodic table.
The noble gas configuration for potassium is [Ar] 4s^1. To form a cation, potassium would lose its one valence electron, resulting in a 1+ ion. Therefore, the ion formed when potassium achieves a noble gas electron configuration is K^+.
In forming the molecule HF, the fluorine (F) atom attains the electron configuration of a stable octet by sharing one electron with hydrogen (H) to form a single covalent bond. This results in fluorine having a full outer shell with a total of eight electrons, achieving a stable electron configuration.
The electron configuration for argon is 1s2 2s2 2p6 3s2 3p6. Argon has 18 electrons and is found in the noble gas group, which means it has a stable configuration.
[He] 2s1