Write the expected ground-state electron configuration for each of the following. a. the lightes

Write the expected ground-state electron configuration for...

Key Concepts

Electron Configuration

Electron configuration refers to the arrangement of electrons in an atom’s orbitals. It is usually written using orbital notation that indicates the energy levels, subshells (s, p, d, f), and the number of electrons in each, providing insight into the chemical and physical properties of the element.

Ground-State Configuration

The ground-state configuration describes an atom’s lowest energy arrangement of electrons. Electrons fill the available orbitals starting from the lowest energy levels in accordance with the Aufbau principle, ensuring that each orbital holds electrons in the most stable pattern possible under standard conditions.

Aufbau Principle

The Aufbau principle is a guideline that electrons occupy orbitals in order of increasing energy. This principle helps predict the order in which orbitals are filled and is crucial when writing the electron configuration for atoms in their ground state.

Periodic Table Organization

The periodic table is organized into rows (periods) and columns (groups) that reflect the recurring nature of element properties. Elements in the same group share similar valence electron configurations, leading to similar chemical behaviors, while elements across periods display variations in electron configuration as additional energy levels are filled.

Orbital and Subshell Notation

Orbital notation uses letters (s, p, d, f) to designate subshells and numbers to represent the principal quantum number. This notation expresses the capacity of each subshell (for example, s holds up to 2 electrons, p up to 6, d up to 10, etc.), which is fundamental when constructing an electron configuration.

Valence Electrons

Valence electrons are the electrons in the outermost shell of an atom. They play a key role in chemical bonding and reactivity. Grouping elements based on their valence electron configuration, as seen in the periodic table, helps explain trends in chemical behavior and periodic properties.

Transcript

00:01 In this problem, we're looking at trying to determine what element is being described based upon four different statements.

00:11 The first statement says an element that has one unpaired 5p electrons that will form a covalent bond with fluorine.

00:21 So the first thing we have to think about is if it's 5p, what area of the periodic table are we looking at? so we're going to figure out, so this is 1p, 2p, 3p, 4p, 5p is right in here.

00:40 So our 5p options are going to be indium through xenon.

00:47 Now, right off the bat, we can get rid of xenon.

00:51 Oops, let's do it this way.

00:53 You can get rid of xenon because it's not going to have any paired electrons, it's a noble gas.

01:00 We know that they fill in order and that our p -orbital is going to have six electron pairs, potential electron pairs.

01:13 So indium is an option.

01:17 Ten is not because it would have two electrons.

01:22 Antimony is not because it would have three.

01:24 It would be going like this.

01:28 Tilarium is not because then we would start pairing off those electrons.

01:33 Iodine is also an option because, again, with the pairing, it would have that one unpaired electron.

01:43 So our options are indium or iodine.

01:46 But the statement also says that it needs to combine covalently with fluorine.

01:51 Therefore, the only option that we have for this is going to be iodine.

01:57 So iodine is the answer to a, the element with one unpaired 5p electron, that can form a covalent bond with fluorine.

02:07 Okay, and we're also asked to write the ground state configuration.

02:11 So our ground state configuration is going to be krypton because that's the nearest noble gas.

02:20 And then it will be 5s2, 4d ,000.

02:30 10 because all of its d shell will be filled and then 5 p 5 because it has 5 of the 6 in its p shell...

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