Which of the elements highlighted in Figure P 7.3 forms monatomic ions by a. losing an s electro

Which of the elements highlighted in Figure P 7.3 forms...

Which of the elements highlighted in Figure $\mathrm{P} 7.3$ forms monatomic ions by
a. losing an s electron?
b. losing two s electrons?
c. losing two s electrons and a $d$ electron?
d. adding an electron to a $p$ orbital?
e. adding electrons to two $p$ orbitals?

Key Concepts

Electron Configuration

This concept involves the distribution of electrons among the atomic orbitals (s, p, d, etc.) in an atom. It determines not only the chemical properties of an element but also how it forms ions by losing or gaining electrons from specific orbitals.

Ion Formation

Ion formation describes the process through which an atom becomes charged by either losing or gaining electrons. This key concept examines which electrons (such as those in the s, p, or d orbitals) are removed or added, thereby influencing the resulting monatomic ion's charge.

Valence Electrons and Orbital Types

Understanding the roles of different orbitals—s, p, and d—is crucial as they contain the valence electrons that participate in chemical reactions. The behavior of electrons in these orbitals determines if an atom is likely to lose or gain electrons to achieve stability.

Periodic Table Trends

The trends observed in the periodic table, such as variations in ionization energy and electron affinity, are central to predicting which electrons in different orbitals are more easily removed or added. These trends help explain the systematic behavior of elements when forming different types of ions.

Transcript

00:01 Okay, so i'm looking at the figure in your textbook that goes with this, and i'm going to make a quick mock -up just so that we can be on the same page here.

00:10 So we had a blue square in the periodic table way here in group 1a, and a green square, so this is representing one row in the periodic table.

00:25 And these colorful boxes are your options as answers, right? and then there's a bunch of squares in between, and then way at the end they had a red square that represents that element there, a black square, and then this is the end of the row, right? so this is going to be the noble gas for this row.

00:47 So this is representing a single row in the periodic table from start to finish over here.

00:54 And so the first question is, which of these elements is going to form a monoatomic ion? first question is by losing an s electron.

01:13 So we need to think first, which of these is going to be more likely to gain electrons, and which is going to be more likely to lose.

01:22 So in general, over here are going to be the ones that are more likely to gain electrons, right? because they're very close to this noble gas configuration right here in the same row, and all they need to do is gain some electrons to get there.

01:37 In contrast, these are going to be losing electrons, and their goal actually is going to be to have the same electron configuration of the noble gas of the prior row, which would be actually up here, this box, okay? so they would be trying to go here, and the other ones are trying to gain electrons to get to this electron configuration.

02:03 So losing just one s electron, well, that is going to be the blue element, or the element represented by the blue square, because this only needs to lose one electron to form an ion, and the electron that is being formed is from the s, or lost, is from the s orbital...

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