they enjoy making love to oxygen atoms
A boron atom would need 3 hydrogen atoms to form covalent bonds with it in order to achieve stability. This would allow boron to have a full octet of electrons in its outer shell, satisfying the octet rule.
In a boron atom, typically three covalent bonds are formed due to its electron configuration (1s² 2s² 2p¹). Boron has an incomplete outer electron shell with only three electrons, so it can share electrons with three other atoms to complete its 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.
No, MgCl2 does not follow the octet rule. Magnesium typically forms ionic bonds with a 2+ charge, so in MgCl2, magnesium has only 8 electrons in its outer shell (2 from Mg and 6 from 2 Cl atoms), not a full octet.
There are exactly three electron pairs attached to the Boron atom, each one of them bonded to a chlorine atom as well.
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.
octet rule
Boron trichloride does not follow the octet rule. Boron does not allow the eight required electrons in the outer shell.
Atoms in the third period or beyond (period 3 and below) can exceed the octet rule due to the availability of d orbitals for expanded valence shells. Examples include sulfur, phosphorus, chlorine, and others in the third row and beyond in the periodic table. Additionally, atoms with an odd number of valence electrons, such as nitrogen and radicals, may also not follow the octet rule.
An example of a molecule that follows the octet rule is methane (CH4). In methane, carbon forms four covalent bonds with hydrogen, allowing each atom to achieve a full outer shell of electrons (octet) and satisfy the octet rule.
Boron typically forms compounds with only 6 electrons in its outer shell. Phosphorus can exceed the octet rule and accommodate more than 8 electrons due to the availability of d orbitals. Sulfur can have more than 8 electrons around it in certain compounds, such as sulfite and sulfate ions.
BCl3 is the formula for Boron Chloride. As a matter of interest it does not obey the octet rule. It is also called a Lewis Acid.
A boron atom would need 3 hydrogen atoms to form covalent bonds with it in order to achieve stability. This would allow boron to have a full octet of electrons in its outer shell, satisfying the octet rule.
First, it helps to draw out the Lewis structure. Boron, being the least electronegative element is in the center, with the three Bromines singly bonded around it. Each Br has an octet of electrons (3 lone pairs plus the single bond) and there are no electrons left over to go onto the Boron. This leaves Boron without an octet, but Boron is an exception to the octet rule so that's okay. So, no BBr3 does not follow the octet rule.
No, AlCl3 does not follow the octet rule. Aluminum typically forms compounds where it only has 6 electrons in its outer shell, such as in AlCl3 where it forms 3 bonds with chlorine atoms.
Some elements that are known to violate the octet rule are: Hydrogen, Helium and Lithium (two electrons) Aluminum and Boron (less than octet but will form an octet if possible), Period 3 elements with p orbitals (more than an octet using empty d orbitals), noble gas compounds (more than an octet), and elements like nitrogen with an odd number of electrons (form free radicals when octets are not possible).
no it does not follow octet rule