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.
8 electrons and yes, the Octet rule states this
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