[Kr]
When an atom of potassium bonds with an atom of iodine, they undergo an ionic bonding process. Potassium, a metal, loses one electron to achieve a stable electron configuration, becoming a positively charged ion (K⁺). Iodine, a non-metal, gains that electron to become a negatively charged ion (I⁻). The electrostatic attraction between these oppositely charged ions results in the formation of potassium iodide (KI), a stable ionic compound.
Iodine gains one electron to achieve a noble gas electron configuration. Its electron configuration is [Kr]5s²4d¹⁰5p⁵, and by gaining one electron, it attains the stable configuration of [Kr]5s²4d¹⁰5p⁶, which is similar to the noble gas xenon.
The element that gains 1 electron to attain the noble gas configuration of Xenon (Xe) is iodine (I). When iodine gains an electron, it achieves a stable electron configuration with a filled outer shell, similar to that of Xenon.
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.
[Kr]
When potassium forms a compound with iodine, one electron is transferred from the potassium atom to the iodine atom. This transfer results in the formation of potassium iodide, which is an ionic compound with a one-to-one ratio of potassium to iodine ions. Potassium becomes a positively charged ion (K+) while iodine becomes a negatively charged ion (I-).
The element with the electron configuration Kr 5s2 4d10 5p5 is iodine, which has 53 electrons in total. The electron configuration indicates that iodine has 7 valence electrons in its outermost shell, which is in the 5p subshell.
When an atom of potassium bonds with an atom of iodine, they undergo an ionic bonding process. Potassium, a metal, loses one electron to achieve a stable electron configuration, becoming a positively charged ion (K⁺). Iodine, a non-metal, gains that electron to become a negatively charged ion (I⁻). The electrostatic attraction between these oppositely charged ions results in the formation of potassium iodide (KI), a stable ionic compound.
Iodine gains one electron to achieve a noble gas electron configuration. Its electron configuration is [Kr]5s²4d¹⁰5p⁵, and by gaining one electron, it attains the stable configuration of [Kr]5s²4d¹⁰5p⁶, which is similar to the noble gas xenon.
The unabbreviated electron configuration for iodine is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p5.
The unabbreviated electron configuration of iodine is 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p5.
The element that gains 1 electron to attain the noble gas configuration of Xenon (Xe) is iodine (I). When iodine gains an electron, it achieves a stable electron configuration with a filled outer shell, similar to that of Xenon.
No, iodine has four electron shells, marked as "K", "L", "M", and "N". The number of electron shells is determined by the electron configuration of an element.
The ion formed from iodine would have a charge of -1, since iodine typically gains one electron to achieve a stable electron configuration.
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.
The ground state electron configuration for Iodine is [Kr] 5s^2 4d^10 5p^5.