Repeat Exercise 114 for (a) 1 s^2 2 s^2 2 p^6 3 s^2 3 p^6 3 d^10 4 s^1 (b) [Kr] 4 d^10 4 f^14 5

step 1 Hello. This will be problem number 115. In this problem, they give us some electron configuratio

Repeat Exercise 114 for (a) 1 s^2 2 s^2 2 p^6 3 s^2 3 p^6 3...

Repeat Exercise 114 for (a) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{1}$ (b) $[\mathrm{Kr}] 4 d^{10} 4 f^{14} 5 s^{2} 5 p^{6} 5 d^{10} 6 s^{2} 6 p^{4}$ (c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5}$ (d) $[\mathrm{Kr}] 4 d^{10} 4 f^{14} 5 s^{2} 5 p^{6} 5 d^{10} 6 s^{2} 6 p^{6} 7 s^{2}$

Repeat Exercise 114 for
(a) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{1}$
(b) $[\mathrm{Kr}] 4 d^{10} 4 f^{14} 5 s^{2} 5 p^{6} 5 d^{10} 6 s^{2} 6 p^{4}$
(c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5}$
(d) $[\mathrm{Kr}] 4 d^{10} 4 f^{14} 5 s^{2} 5 p^{6} 5 d^{10} 6 s^{2} 6 p^{6} 7 s^{2}$

Key Concepts

Electron Configuration

This concept refers to the arrangement of electrons in an atom’s orbitals, indicating how electrons are distributed among different energy levels and sublevels. It is fundamental in understanding an element’s chemical properties, reactivity, and its position in the periodic table.

Aufbau Principle

The Aufbau principle dictates that electrons fill atomic orbitals in order of increasing energy, starting from the lowest energy level before moving to higher ones. This principle helps explain the order in which electrons populate the subshells as seen in various electron configurations.

Noble Gas Notation

Noble gas shorthand is a compact way to represent electron configurations by using the electron configuration of a noble gas to summarize inner, core electrons. This notation simplifies the presentation of configurations, especially for larger atoms, by highlighting the valence electrons that determine chemical properties.

Electron Subshell Notation

Electron subshell notation, using symbols such as s, p, d, and f combined with superscripts denoting the number of electrons, provides a concise method to depict the distribution of electrons among orbitals. It is crucial in analyzing and comparing the electronic structure of atoms.

Valence Electrons

Valence electrons are the electrons located in the outermost shell of an atom and are primarily responsible for the chemical bonding and reactivity of the element. Identifying the number and arrangement of valence electrons from an electron configuration is key to predicting an element’s chemical behavior.

Transcript

00:01 Hello.

00:02 This will be problem number 115.

00:07 In this problem, they give us some electron configurations, four of them, to be exact, e, b, c, and d.

00:13 And they ask us to identify which element these configurations represent.

00:20 There are a couple ways to do this.

00:22 One way is to look at those superscripts in the configurations, because those superscripts represent electrons.

00:32 So if we add those superscripts together, we will get the number of electrons.

00:36 And we know that if it's a neutral atom, the number of electrons also equals the number of protons, and therefore the atomic number.

00:50 So whatever number we get for the number of electrons, by adding those superscripts together, will tell us the atomic number.

00:58 So let's get started.

00:59 So with letter a, we have two plus two.

01:03 So i'm just writing down the superscripts that are there, plus six, plus two, plus six, plus ten, plus one.

01:15 Adding these together, i get 29.

01:18 So 29 electrons means 29 protons, which means an atomic number of 29, and this element would be copper.

01:27 So correct answer is copper.

01:31 Right, and letter b, letter b is written in shorthand form with krypton in brackets.

01:36 That means that that represents the first 36 electrons.

01:42 So we're starting with 36, and we're adding 10, 14, 2, 6, 10, 2, and 4...

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