I saw this on a classmate's past test. O-2 and CL-1 are isoelectronic. I don't understand. Can you please run me through all the steps to determining how this pair of atoms IS electronic!!??! Thanks in advance!

S4-, C4-, P4- and B5- are all isoelectronic with the noble gas neon i.e. they have the same electronic configurations. why, therefore do they not have a stable existence? Please help me to answer this question and provide an explanation because I...

What does it mean that permanganate and tungstate ions are isoelectronic?

and Write the symbol for a cation and anion that are isoelectronic with krypton. can you help me on these questions? thanks!

The question states: What would be the charge and electron configuration of an ion formed from calcium that is isoelectronic with the following ions? Then it goes on to say find the charge of Ar+. Any help would be appreciated!

A) Isoelectronic molecules are molecules that have the same number of valence electrons. B) Isoelectronic molecules are molecules that have the same shape. C) Isoelectronic molecules are molecules that have the same number of valence ...

Describe why a mono-atomic cation would have a smaller atomic radius than an element with which it is isoelectronic. Use the examples of Na+ being smaller than Ne. Also, why are elemental anions always larger than the elements for which they ...

is it possible for a cation to be isoelectronic with an anion from the same period? explain. i just don't get it.

Not really understanding how to answer this one. Please help me understand. Thank you. Name 5 chemical species that are isoelectronic with magnesium ion.

Which of these cations are isoelectronic with eachother? calcium nitrate, strontium nitrate, potassium nitrate, sodium nitrate, sodium nitrate, barium nitrate, copper nitrate, lithium. And, how do you know that it was the cation not the anion ...

Is it possible for a cation to be isoelectronic with an anion from the same period?

All the following species are isoelectronic with Ne except A.HF B.Na+. C.NH3. D.O2-. E.Be2+.

Atoms and ions are described as isoelectronics if they have the same number of electrons. Name the noble gas that is isoelectronic with each of the following: a) Li+ b) F- c) Ca^2+ - I don't know how to do this, so please state how ...

Help!!!!! how do i write the symbol for a cation and an anion that are isoelectronic with krypton?

The Ti2+ ion is isoelectronic with the Ca atom. 1) Are there any differences in their electron configurations? 2) Will they have the same number of unpaired electrons? Offer an explanation for both parts 1 and 2

I have a question which asks, "Which of the following molecules or ions are isoelectronic?" Then it lists four different compounds. Could somebody just explain how to determine when/if a compound is isoelectronic? Thanks so much in ...

what is the relationship between ions and atoms that are isoelectronic?

a) the cation possessing a positive one charge that is isoelectronic with krypton. b) the anion possessing a negative two charge that is isoelectronic with neon.

Which lists species with the same electron configuration, that is, species that are isoelectronic? A) Mg, Ca, Sr B) Mg^2+, Ca^2+, Sr^2+ C) S^2-, Cl^-, K^+ D) Fe, Co, Ni E) F^-, S^2-, As^3- (if u didnt know the ^ means to that power)

Explain what it means to be isoelectronic and give an example of it

In which of the following pairs are the two species isoelectronic? (A) S − , F − (B) N, S (C) O, S (D) Si − , P (E) Aℓ 3+ , P 2−

In which of the following pairs are the two species isoelectronic? (A) S − , F − (B) N, S (C) O, S (D) Si − , P (E) Aℓ 3+ , P 2−

When a phosphorus atom is converted into an ion, it becomes isoelectronic with argon. What is the name of the ion?

Which of the following species is NOT isoelectronic with Ca2+ a. P2- b. S2- c. Ar d. K+ Please help! I think the answer is A) does anyone agree?

(If the ion is isoelectronic with a noble gas, simply give that noble gas in square brackets.) Pb2+ An explanation would be great. Thanks for any help!

Explain this problem to me: The atom and ions Na, Mg+, Al2+, and Si+3 are isoelectronic. For which of these would the effective nuclear charge be the smallest?

For example, Chlorine needs to gain one electron to become isoelectronic with the next noble gas, Argon; so, the ion is Cl(-1). Is there any way to do the same thing with elements in the d-block? How else do you remember the ions?

Arrange the following isoelectronic series in order of decreasing radius: Na+, O2-, F-, Al3+, Mg2+ and an explanation would be helpful!

I have the ions N^-3, Mg^+2, F^-2, and O^-2 which are all isoelectronic. I simply do not understand how to place them in order of increasing size. Can someone please explain this to me? Thanks in advance.

Br−, Se2−, Kr, Rb+, Sr2+ 1. They are listed in order of decreasing electronegativity. 2. They are isoelectronic. 3. They are listed in order of increasing number of electrons. 4. They are listed in order of increasing electronegativity...