What element is isoelectronic with phosphorus?
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What element is isoelectronic with phosphorus?
Sulfur form a S2− ion…. i.e. 18 electrons, and this is isoelectronic with neutral argon, i.e. Ar …. And phosphorus forms a P3− ion…. i.e. 18 electrons, and this is isoelectronic with neutral argon, i.e. Ar ….
What is isoelectronic P+?
The K+ ion is isoelectronic with the Ca2+ ion. The carbon monoxide molecule (CO) is isoelectronic to nitrogen gas (N2) and NO+. CH2=C=O is isoelectronic to CH2=N=N….More Examples of Isoelectronic Ions and Elements.
| Isoelectronic Ions/Elements | Electron Configuration |
|---|---|
| K, Ca2+ | [Ne]4s1 |
| Ar, S2- | 1s2 2s2 2p6 3s2 3p6 |
Is isoelectronic with which of the following ions?
Be^(2+) is isoelectronic with which of the following ions? Be2+=(4-2)=2 is isoelectronic with Li+(3-1=2) Since both have the same number of electron in their outermost shell.
How many valence electrons are there in an phosphide anion?
8 valence electrons
For the phosphide anion there are 8 valence electrons….. Truong-Son N.
What ion is isoelectronic with K+?
And we can see that the potassium ion, K+, has the same electronic configuration as the chloride ion, Cl-, and the same electronic configuration as an atom of argon, Ar. Therefore, Ar, Cl-, and K+ are said to be isoelectronic species.
What are the isoelectronic elements?
Atoms and ions that have the same electron configuration are said to be isoelectronic. Examples of isoelectronic species are N3–, O2–, F–, Ne, Na+, Mg2+, and Al3+ (1s22s22p6). Another isoelectronic series is P3–, S2–, Cl–, Ar, K+, Ca2+, and Sc3+ ([Ne]3s23p6).
What is isoelectronic Sr2+?
Because every species contains an equal number of electrons, therefore, Sr2+ , Se2− , and Br− ions are isoelectronic.
What is isoelectronic with N3?
The trick here is to realize that the nitride anion, N3− , is isoelectronic with neon, Ne , the noble gas that shares a period with nitrogen, N . In other words, the nitride anion has the same number of electrons as neon.
Are Be2+ and Mg2+ isoelectronic?
No, Be2+ and Li+ would actually be isoelectronic to He since Be would be losing 2 and Li would be losing 1 electron. In order to be isoelectronic, Be2+, Li+, and Ne would have to have the same number of electrons. For example, Na+ and Mg2+ would be isoelectronic to Ne.