Boron And Berylium
No, AsH3 does not follow the octet rule. Arsenic, the central atom in AsH3, can expand its valence shell to hold more than eight electrons in bonding.
No, BCl3 does not follow the octet rule as boron only has 6 valence electrons in this molecule. Boron can form stable compounds with less than an octet due to its electron deficiency.
Yes, sulfur can exceed the octet rule in chemical bonding by expanding its valence shell to accommodate more than eight electrons.
Boron trichloride does not follow the octet rule. Boron does not allow the eight required electrons in the outer shell.
BCl3 and BEH2 obey the octet rule because Boron and Beryllium are exceptions to the octet rule and can have stable electron configurations with less than 8 electrons. Cl3CF, NO, and SbF5 do not obey the octet rule because they have incomplete or expanded valence shells.
no it does not follow octet rule
No, AsH3 does not follow the octet rule. Arsenic, the central atom in AsH3, can expand its valence shell to hold more than eight electrons in bonding.
No, BCl3 does not follow the octet rule as boron only has 6 valence electrons in this molecule. Boron can form stable compounds with less than an octet due to its electron deficiency.
Yes, sulfur can exceed the octet rule in chemical bonding by expanding its valence shell to accommodate more than eight electrons.
octet rule
No, H2CO2 is not a stable molecule. It does not exist in a stable form because it violates the octet rule for stability in chemical bonding, as it would require carbon to have 10 valence electrons to accommodate all the atoms.
Yes, oxygen is an exception to the octet rule. Molecular oxygen can have two unpaired electrons making it a biradical molecule.
1. the incomplete octet of a central atom 2. odd electron molecule 3. compound with expanded octet 4. acc. to rule atoms complete their octet to complete their octet to become stable like inert gas, but it is seen that inert gases like xenon are not stabkle they combine with fluorine and oxygen to form no. of compounds. 5. shape of molecule cant be explained 6. stability of molecule cant be explained
See the Related Questions to the left for how to solve this problem.First draw the Lewis Dot structures of each molecule, then count the valence electrons of each atom in the structures. Find the one that doesn't have eight!In this case, there is actually a little trick. To follow the octet rule, each atom must have 8 valence electrons in the structure, right? Therefore, the molecule must have an even number of total electrons for that to work. So which molecule does not have an even number of total electrons?
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.
You probably mean the octet rule, which states that atoms undergo chemical bonding in order to achieve an octet (8) of electrons in their valence shell. This makes them stable. All of the main group elements follow this rule, except for hydrogen. It is stable with two valence electrons. The main group elements are Groups 1, 2, and 13-18.
Boron trichloride does not follow the octet rule. Boron does not allow the eight required electrons in the outer shell.