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Elements which have d-orbitals (i. e. n=3 or higher) can form compounds with an expanded octet. Some examples are;

  1. Phosphorous Pentachloride PCl5
  2. Sulfur Hexafluoride SF6
  3. Dichloro Heptoxide Cl2O7
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12y ago

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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.

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AnswerBot

10mo ago
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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.

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10y ago
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I think it is the Noble gases or the inert gases (they have full shells). Check it up on Google and you will get a full explanation :)

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16y ago
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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.

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11y ago
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Noble gases

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15y ago
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Q: What elements can form compomds with an expanded octet?
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Continue Learning about Earth Science

How does neon obey the octet rule when reacting to form ionic compounds?

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.


What is a element that will not form a compound?

Helium is an element that typically does not form compounds due to its stable electronic configuration with a full outer shell of electrons.


How does sodium obey the octet rule when reacting to form compounds?

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.


Ions of the elements oxygen (O) sulfur (S) and selenium (Se) usually have charges of -2. Ions of the elements fluorine (F) chlorine (Cl) and bromine (Br) usually have charges of -1.?

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.


Which obeys the octet rule PF5 Cs2 BBr3 CO3 2?

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.