Identify the atoms that correspond to each of the following...

Identify the atoms that correspond to each of the following electron configurations. Then, write the Lewis symbol for the common ion formed from each atom: (a) $1 s^{2} 2 s^{2} 2 p^{5}$ (b) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2}$ (c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10}$ (d) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{4}$ (e) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{1}$

Identify the atoms that correspond to each of the following electron configurations. Then, write the Lewis symbol for the common ion formed from each atom:
(a) $1 s^{2} 2 s^{2} 2 p^{5}$
(b) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2}$
(c) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10}$
(d) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{4}$
(e) $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{2} 3 d^{10} 4 p^{1}$

Key Concepts

Lewis Dot Symbols

Lewis dot symbols are a shorthand representation of an element’s valence electrons, depicted as dots around the element’s chemical symbol. This visualization aids in understanding the bonding behavior and ionic or covalent interactions, especially when illustrating the common ion formed by an atom.

Ion Formation

Ion formation involves the gain or loss of electrons by an atom to achieve a stable electron configuration, often resembling that of a noble gas. Understanding the number of valence electrons enables predicting whether an atom will form a cation (by losing electrons) or an anion (by gaining electrons), and what the resulting charge will be.

Electron Configuration

Electron configuration describes how electrons are distributed in an atom’s orbitals. It follows the Aufbau principle, Hund's rule, and the Pauli exclusion principle, laying out the order in which electrons fill energy levels. This concept is key for identifying elements based on their unique arrangements of electrons.

Periodic Table

The periodic table organizes elements by increasing atomic number and similar chemical properties. By comparing a given electron configuration to the standard order of orbital filling, one can identify the corresponding element and its position in the periodic table.

Valence Electrons

Valence electrons are the electrons in the outermost energy level of an atom and are primarily responsible for chemical reactivity. Counting these electrons from an electron configuration helps determine how atoms gain or lose electrons to form ions.

Transcript

00:01 Okay, so today we're going to be identifying some elements from their, sorry, i don't want to use blue yet, from their electron configuration, and then we're going to be writing the lewis symbol for their specific ions.

00:17 So firstly, we have 1s2, which takes up hydrogen and helium, and then next we have 2s2, so we know that it's not going to be these four.

00:31 And then we go to 2p5.

00:35 So you know, one, two, three, four, five.

00:40 So the element is going to be fluorine.

00:43 And so to start writing the common ion for this, we have to determine how many electrons who need to gain or lose to reach its full octet set, and we have to take into account what it would prefer to do and will be most likely for it.

00:58 So, fluorine is very electronegative.

01:04 It's actually the most electronegative.

01:05 So it's going to take the electrons to become here at neon.

01:11 So it's going to be gained the full eight electrons in its common ion of f minus.

01:22 I'll just draw a little arrow to that.

01:26 All right.

01:27 So next we have 1s2, 2s2.

01:35 2p6 and 3s2.

01:38 So starting off with where we left off here at 2p5, we know that it's not going to be that.

01:44 It's not going to be that.

01:46 And then that clears out the 2 energy level.

01:50 So now we move on to 3s.

01:53 So it's 3s2.

01:54 So we know it's not that, but there's nothing after this.

01:56 So it's actually going to be magnesium here.

02:00 So then we have to realize that magnesium's common ion is going to be mg, 2 plus and that's because it does not, it is very unlikely that magnesium has enough electronegativity to gain the six more electrons that it needs to get a full octet.

02:19 So it generally just surrenders those two electrons so that it can get to that full octet set, which means that its valence electron.

02:29 Lewis shell is just going to be its chemical symbol...

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