SF6
Yes. Both O-F bonds are single covalent, so all three atoms can claim 8 electrons.
Lewis defined an acid as an electron pair acceptor. BF3 is a compound where boron does not have an octet of electrons in the outer energy level, so it can readily accept electrons.
The octet rule.
8 electrons and yes, the Octet rule states this
Sulfur (S) would be the central atom, and it will have 6 Cl bonded to it by single bonds. Each Cl will have 3 lone pairs of electrons around them. S will have 12 electrons but it can have an expanded octet, and doesn't have to have 8 electrons.
Yes. Both O-F bonds are single covalent, so all three atoms can claim 8 electrons.
An octet of electrons is when the outermost electron shell of an atom contains eight electrons.
No, metals tend to lose electrons to achieve a full octet.
Phosphorus need 3 electrons to complete its octet.
Elements which have d-orbitals (i. e. n=3 or higher) can form compounds with an expanded octet. Some examples are;Phosphorous Pentachloride PCl5Sulfur Hexafluoride SF6Dichloro Heptoxide Cl2O7
8: that's the meaning of "octet".
The element whose atomic, and therefore proton number, of 6 is Carbon (C) and of 17 is Chlorine (Cl). Carbon has a valence of 4 electrons meaning it needs to 'take in' four more electrons to fill its octet (and thus follow the octet rule). The chlorine has a valence of 7 electrons and therefore it only needs 1 electron to fill its octet. Through a covalent bond, where the electrons are 'shared' between the molecules, 4 Cl and 1 C can bond to form the compound CCl4. All of the elements have a full octet and form a tetrahedrally shaped molecule.
Lewis defined an acid as an electron pair acceptor. BF3 is a compound where boron does not have an octet of electrons in the outer energy level, so it can readily accept electrons.
The octet rule.
Well according to the octet rule the a compound must have 8 valance electrons to be stable.
i think 4 is the valency of tetrachloride
8 electrons and yes, the Octet rule states this