Hydrogen, helium and the transition metals
Yes, sulfur can break the octet rule by expanding its valence shell to accommodate more than eight electrons. This is known as an expanded octet.
Yes, sulfur can break the octet rule by expanding its valence shell to accommodate more than eight electrons. This is known as an expanded octet.
Yes, certain elements in the periodic table, such as elements in the third row and beyond, can have an expanded octet, meaning they can have more than eight valence electrons in their outer shell.
Xenon can achieve a stable octet by forming compounds with elements that can share their electrons with xenon. For example, xenon can form compounds with fluorine, chlorine, or oxygen where xenon acts as the central atom and bonds with these more electronegative elements to complete its octet.
The elements in period 3 and above have d orbitals available for bonding which makes the "expansion" of the octet more likely. period 2 elements do not, the 2d shell has only s and p orbitals. P is in period 3, an example is PCl5 with 5 electron pairs. Se in period 4 can also expand its octet, an example is SeF6, with 6 electron pairs.
An Octave (occasionally an Octet)
Yes, sulfur can break the octet rule by expanding its valence shell to accommodate more than eight electrons. This is known as an expanded octet.
Yes, sulfur can break the octet rule by expanding its valence shell to accommodate more than eight electrons. This is known as an expanded octet.
The elements can be described by dot structure. Metals combine with other elements to make its octet complete.
eight. it is important to obtain octet so that elements become stable.
The octet rule is the tendency of many chemical elements to have eight electrons in the valence shell.
Yes, certain elements in the periodic table, such as elements in the third row and beyond, can have an expanded octet, meaning they can have more than eight valence electrons in their outer shell.
it has a full octet
Xenon can achieve a stable octet by forming compounds with elements that can share their electrons with xenon. For example, xenon can form compounds with fluorine, chlorine, or oxygen where xenon acts as the central atom and bonds with these more electronegative elements to complete its octet.
To complete their octet
The octet rule cannot be satisfied in molecules whose total number of valence electrons is an odd number.There are also molecules in which an atom has fewer, or more, than an octet of valence electrons.
Uranium typically forms compounds where it does not have an octet due to its ability to expand its valence shell beyond eight electrons. Uranium can often exceed the octet rule in its bonding arrangements.