For elements of atomic number (a) 15, (b) 26 , and (c) 32 in their ground states, answer the fol

For elements of atomic number (a) 15, (b) 26 , and (c) 32 in...

Key Concepts

Electron Configuration

This concept describes the distribution of electrons in an atom's orbitals according to energy levels and subshells. It provides the framework to determine how many electrons reside in specific orbitals such as d orbitals, and is fundamental in predicting an element's chemical properties and behavior.

Quantum Numbers

Quantum numbers are parameters that describe the properties of electrons within an atom, including their energy level, orbital shape, orientation, and spin. In particular, the azimuthal quantum number (l) defines the subshell type (s, p, d, f); for example, l=1 corresponds to the p orbitals, which is significant when counting electrons with specific orbital characteristics.

d Orbitals

d orbitals are part of the electron configuration in atoms and pertain to the subshell where the azimuthal quantum number l is equal to 2. They are critical for understanding the electron occupation in atoms, especially for transition elements, and are instrumental in determining properties like bonding, magnetism, and overall chemical reactivity.

Electron Pairing and Unpaired Electrons

Electron pairing involves the arrangement of electrons within orbitals where each orbital can hold up to two electrons with opposite spins. Unpaired electrons, which occur when electrons occupy separate orbitals in accordance with Hund's rule, play a significant role in determining the magnetic properties and reactivity of an atom.

Transcript

00:01 In this question we've been given atomic numbers or proton numbers and we've been asked to answer a few questions based on each of those.

00:10 So for the first one we've been given z being equal to 15.

00:15 So looking at this, if we at least just write the electronic configuration, 1s2, 2 s2 2p6, 3 s2 3p3.

00:25 What is important to note that this set is a proton number.

00:29 But since we are looking at a neutral atom it means this is also equal to the number of electrons we did not just write this electronic configuration from the proton number but it was coming from the guideline to say if this is a neutral atom in its ground state the number of protons are also going to be equal to the number of electrons hence this electronic configuration the electronic configuration should always we should try to always write it from the number of electrons because these are actually electrons in shells and sub orbitals.

01:06 So looking at this electronic configuration, if we are to look at it is at ground state and there are not d electrons in this element or in this atom, they are not d subshells or d shells.

01:20 And then moving on to the next one, if l is equal to 1, it means we are looking for the p orbitals.

01:28 And if we are to look for the p orbitals here, we are going to have a total of 9 p electrons.

01:37 We have these 2p orbital and the 3p orbital each contributing 6 plus 3 to make a total of 9 electrons in the p orbitals.

01:47 So if we now want to look into the number of unpaid electrons, we might just decide to draw this like a pictorial where we have 1.

02:00 2 s 2 s 2 p 6 3 s 2 and finally 3 p 3 3 here we are going to be having 2 electrons 2 3 4 and 6 here we have our 2 remember a p orbital can take up to 6 electrons and s orbital can take up to 2 electrons looking at this we always have to remember that in in terms of the orbital, we first of all fill in all the orbitals before we actually start pairing the electrons.

02:44 So for these 3p orbital, these are our 3 electrons.

02:47 They are not yet paid because we still have to must first of all fill all of these orbitals before suborbital before we actually start pairing.

02:56 And we've already run out of the electrons that are in the 3p orbitals.

03:01 So looking at this pictorial view, we have a total of the three unpaired electron.

03:09 And then moving on to the next one, we have our z being equal to 26...

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