Which property of the third-row nonmetallic elements might be the one depicted below:

a. first ionization energy,

b. atomic radius,

c. electronegativity,

d. melting point,

e. X―X single-bond enthalpy? [Find more in Sections 22.3, 22.4, 22.6, 22.8, and 22.10]

Video transcript

Hello everyone. Today, we have the following problem. Which property of the non metallic elements from the second period period of the periodic table could be illustrated in the diagram below a atomic radius. B first ionization energy C halogen halogen, single bond enthalpy D electron negativity or E melting point. So the set property is increasing as we see from a carbon to neon with a small discontinuity at the oxygen. So if we look at the atomic radius, we can recall that the atomic radius essentially it decreases from left to right across a periodic table period. And is it due to increasing nuclear charge? And so the bars would actually decrease in length from carbon to neon, which is the opposite of what we see here. So choice A is not the right answer. And with the answer, choice B the ionization energy specifically, the first ionization energy will increase across a period from left to right. And first ionization energy essentially can be summarized as the energy needed to abstract an electron. So if we look at our carbon nitrogen, oxygen form in neon, we see that it is increasing. And this makes sense because fluorine is actually the most electron negative element. And so it makes sense that it would have the highest first ionization energy. So Andras B is not wrong, but it is looking most likely the answer if we move on to enter IC, the halogen halogen single bond enthalpy that does not generally show a clear trend across the periods on a periodic table. Essentially, there is no neon neon single bond that exists. So no value for this property can be known. So 20 C is not correct for electron. This increases across a period from left to right, as does the first ionization energy and this is due to increasing nuclear charge and eventually the attraction of bond electrons. However, leon is a noble gas and as such, it has no electron negativity value. So we have to answer answer choice e this varies across a period with no consistent increase or decrease. So that answer choice is wrong. And thus, we are left with b first ionization energy as our final answer. Overall, I help is helped. And until next time.