Which choice(s) contain(s) an isoelectronic pair in the ground...

Question

Which choice(s) contain(s) an isoelectronic pair in the ground state?

Accepted Answer

hey everyone in this example, we need to identify the set that has all species with the same number of electrons. And we need to explain what this relationship with having the same number of electrons is called. So looking at example a we have rubidium plus carryin krypton as a neutral atom and strontium two plus as a Catalan So to find the number of electrons in rubidium, we want to focus on a neutral atom of rubidium, Recognizing that a neutral atom of rubidium corresponds to the atomic number 37. And we want to recall that the atomic number Is always written in the left hand sub subscript of our chemical symbol and is described by our number of protons, which in a neutral atom is also equal to our number of electrons. And so a neutral atom of rubidium we would say has 37 protons and 37 electrons. But in this case we are given our B plus as a caddy on. And so we would say that those 37 electrons, we recall that acadian charge means we lose one electron. So we would subtract one electron from those 37 leaving us with electrons for R B plus. Now moving on to Krypton. When we find Krypton on our periodic tables, we see Krypton corresponds to atomic number 36. It's found in Group Eight a on our periodic tables because it's a noble gas. And so that means we would have 36 protons and 36 electrons in our given neutral atom of Krypton. And so so far that's consistent moving on to strontium two plus, we want to find strontium two plus on our periodic tables or strong tea. I'm sorry. We would find strontium in group two A. On our periodic tables corresponding to atomic number 38. Which means that in a neutral atom of strontium we would have 38 protons and 38 electrons however, were given strontium as a caddy on with a two plus charge, meaning those 38 electrons would lose Two electrons from that based on that Catalan charge. And that would leave us with 36 electrons for our catalog of strontium. And so all of our electrons stayed consistent amongst these three species. And so we would say that these three species have an isil electronic relationship. And so we would consider a as an isil electronic choice where all of the number of electrons are equal between the different species. So the relationship is called electronic. Moving onto choice B. We have carbon night nitride with the three minus charge and fluoride with the f minus charge. So focusing first on the carbon, it's a neutral atom of carbon. We would find carbon in group four A. On our periodic tables corresponding to atomic number six, meaning that in a neutral atom of carbon, we have six protons and six electrons. So we can fill that in above. Now for our nitride, we want to focus on a neutral atom of nitrogen. First, we would find nitrogen in group five A. On the periodic table corresponding to atomic number seven. And so in a neutral atom of nitrogen we have seven protons and seven electrons. However in this case we have an an ion of nitrogen with a three minus charge. Recall that an an ion means that are seven original electrons in the neutral atom will gain three electrons because it's an an ion. And so that would leave us with 10 electrons for our nitride and ion. And so we can already rule out into choice B. Because this does not equal six electrons as in our first given species carbon. And so we would not consider B as containing an electronic set with all equal electrons amongst the different species. Moving onto choice C. Let's see if we can rule that out. So we're given the N. I. Plus carry on. We find sodium in group two A. Or sorry, we would find sodium in group one A. On the periodic table. And so we see that sodium corresponds to atomic number 11, which is filled in the left hand subscript of our chemical symbol for sodium. And so in a neutral atom of sodium we would have 11 protons and electrons corresponding to our atomic number. And so because we aren't given a neutral atom, were given a charged cad ions of sodium are 11 original electrons in the neutral atom would lose one more electron leaving us with 10 electrons for the custodian of a one plus. Moving on to the second given adam, we have strontium two plus. So we focus on the neutral atom of strontium. We find strontium in group two A. On our periodic tables corresponding to atomic number 38. Which is written in the left hand subscript of our chemical symbol, meaning a neutral atom of strontium will have an atomic number of corresponding to 38 protons and 38 electrons. And so because we are not given a neutral atom of strontium were given a two plus cat ion of strontium R. 38 electrons would correspond to losing two electrons based on that two plus catatonic charge. Leaving us with 36 electrons for our charged atoms of strontium two plus. And this does not equal the 10 electrons in the first given species and a plus. So we would also rule out choice C leaving choice a as the only correct answer choice with all of the differing species having the same number of electrons. And that relationship is called being ISil Electronic. So I hope that everything we reviewed was clear. If you have any questions, please leave them down below. And I will see everyone in the next practice video

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Which choice(s) contain(s) an isoelectronic pair in the ground state?

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