yes
No, it is possible to satisfy the octet rule for XeF2. Xenon has eight electrons in its outer shell (octet) by sharing two electrons with each of the two fluorine atoms in the molecule, resulting in a stable electron configuration.
Molecular formulae that must contain a double bond in order to satisfy the octet rule are those of compounds like O2, HCN, and CO2.
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.
Each sodium atom will lose one electron to achieve a complete octet in its outer shell, as the octet rule dictates atoms will gain or lose electrons to achieve a stable electron configuration with 8 electrons in the outer shell.
The 2 outermost orbitals that must be filled to satisfy the octet rule are the s and p orbitals. These orbitals can hold a maximum of 8 electrons in total, which is needed to achieve a stable, full octet configuration for many elements.
There are three resonance structures for the nitrate ion that satisfy the octet rule. In each of these structures, each oxygen atom has a full octet by sharing electrons through double bonds with the nitrogen atom.
Oxygen typically forms two covalent bonds to satisfy the octet rule.
Fluorine needs one additional electron to satisfy the octet rule, giving it a total of 8 valence electrons and achieving a stable electron configuration.
Xenon difluoride, XeF2. Xenon is a noble gas, and as such has a full outer shell of eight electrons; as per the octet rule, it doesn't usually form chemical bonds. However, highly reactive nonmetals such as fluorine can induce it to do so.
Strontium is part of Group IIA, which means it loses 2 valence electrons to satisfy the rule. Sr2+.
Molecular formulae that must contain a double bond in order to satisfy the octet rule are those of compounds like O2, HCN, and CO2.
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.
Each sodium atom will lose one electron to achieve a complete octet in its outer shell, as the octet rule dictates atoms will gain or lose electrons to achieve a stable electron configuration with 8 electrons in the outer shell.
Ionic Bonds are when electrons are exchanged to satisfy the octet of each element reacting. Covalent Bonds are when two atoms SHARE their electrons to satisfy the octet rule.
The 2 outermost orbitals that must be filled to satisfy the octet rule are the s and p orbitals. These orbitals can hold a maximum of 8 electrons in total, which is needed to achieve a stable, full octet configuration for many elements.
There are three resonance structures for the nitrate ion that satisfy the octet rule. In each of these structures, each oxygen atom has a full octet by sharing electrons through double bonds with the nitrogen atom.
Four
A potassium atom has 1 electron in its outer shell. In order to satisfy the octet rule, it needs to donate 7 electrons to another atom to reach a stable configuration with a full outer shell.