Elements which have d-orbitals (i. e. n=3 or higher) can form compounds with an expanded octet. Some examples are;
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Elements in period 3 and beyond, such as sulfur, phosphorus, chlorine, and bromine, can form compounds with an expanded octet. These elements have empty d orbitals available for bonding, allowing them to exceed the octet rule and form compounds with more than eight electrons around the central atom.
An octet of electrons means the last shell of the atom has 8 electrons. The last column in the Periodic Table (also called noble gases) has all the elements that contain an octet of electrons such as Helium, Neon, and Argon, to name a few.
The noble gases have a complete octet. If you go across the groups (1a to 8a), left to right. They have 1 to 8 of the octet in order. This gives them remarkable stability.
Neon does not typically form ionic compounds because it already has a full valence shell with 8 electrons, satisfying the octet rule. Its electron configuration (1s^2 2s^2 2p^6) makes it very stable and unreactive with other elements.
Helium is an element that typically does not form compounds due to its stable electronic configuration with a full outer shell of electrons.
Sodium typically loses its one valence electron to achieve a stable electron configuration, resembling the nearest noble gas (Neon), thereby obeying the octet rule. This electron loss allows sodium to form a stable ionic bond with other elements by attaining a complete outer shell with 8 electrons.
That's correct. Oxygen, sulfur, and selenium typically form ions with a charge of -2 by gaining two electrons to achieve a stable octet. Fluorine, chlorine, and bromine usually form ions with a charge of -1 by gaining one electron to achieve a stable octet.
PF5 obeys the octet rule as it has 5 bonding pairs of electrons around the central phosphorus atom, satisfying the octet. Cs2 does not follow the octet rule as Cs is in Group 1 and can only form ionic bonds. BBr3 is an exception to the octet rule as boron has only 6 electrons around it due to the empty d orbital. CO3 2- also obeys the octet rule as each oxygen atom has a complete octet.