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Answered 2009-03-17 03:15:44

It would form an ionic bond. The atom with 7 electrons is cation and the atom with 1 is an anion.

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The electrons in the outermost level are known as the valence electrons.


Outer energy level electrons, or valence electron.


They have 7 outermost electron


there is only one electron in the outermost shell of Na.


francium only has one valence electron (one electron in the outermost shell).


2 electrons are found in the outermost electron shell of Helium. 8 electrons are found in the outermost electron shell of all other noble/inert gases.


The electrons in the outermost shell is called as valence electron. These electrons are free and they are involved in bonding reactions.


Neon (atomic number 10) and Argon (atomic number 18) mostly do not react with other elements because their outermost electron shells have a full complement of electrons. When two elements combine into a molecule they share electrons from their outermost electron shell. This happens when one element has a minimal number of electrons in its outer shell and the other element has an almost full complement of electrons in its outer shell. When they share electrons, they both have the equivalent of full outer electron shells. Since both Neon and Argon have full outermost shells by themselves they do not have a tendency to share electrons.


The electron structure of mercury is: 1s2 2s2p6 3s2p6d10 4s2p6d10f14 5s2p6d10 6s2 So the 6s orbital is outermost. This outermost shell can (and does) hold 2 electrons.


Calcium atoms have two electrons in the s orbital of their outermost energy level. Their electron configuration is [Ar]4s2.



Valence electrons are located in the outermost shell in an atom. Chromium has only one valence electron.



Electrons in the outermost shell are valence electrons!


If an atom has three electrons, it will have one valence electron (valance = outer shell). It will be more likely to lose an electron than gain one, since it has only one to lose, but seven to gain.


an electron is a wavelength of energy that orbits a nucleus at the speed of light in an orbital where only one other electron can exist with an opposite spin, the electons in the orbitals in the outermost energy levels are valence electrons. ex: C= 1s^2 2s^2 2p^2 (the second energy level ((the outermost in this example)) contains a total of 4 electrons or its valence electrons)


The number of electron shells and the number of electrons in the outer most shell are what determines what the atom is.


Chlorine has one more electron then sulfur, so it has 1 more electron in the outer shell, 1 more valence electron. Chlorine has 5 electrons in the outermost shell and sulfur has 4.


Nonreactive elements like noble gases have 8 electrons in the outermost shell. An element is the most stable when its outermost shell has 8 electron that's is it is completely filled. 8 is the maximum number of electrons which can be accommodated in the outer most shell. Helium is an exception as it has only 2 electrons in its only shell. Yet it is nonreactive.


The outer ring is either n=the number of ring it is, or just plain say "the outer shell." The proper term is VALENCE, the outermost shell = valence shell, outermost electrons = valence electrons


Aluminum's electron configuration is 13. It has three outermost electrons. It tends to donate three electrons to form the stable Aluminum(III) ion.


The outer most shell is the 3s orbital and it holds 2. The others fill first giving it a total of 12 electrons for the element.


The outer-most electrons are the only ones included in the orbital filling diagram and the electron dot diagram because the outer-most electrons are the only ones that need to be used in chemical reactions and bonding, so the other electrons are insignificant in these diagrams.


A bromine atom has seven electrons in its outermost shell.


The noble gasses all have a filled outer electron shell of eight electrons, except helium which has two electrons. Since their outer electron shells are filled, they are less likely to react with other atoms.



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