Explanations 
Textbooks 
Flashcards 
91影视 AI 
Notes 
Study Plans 
Study Sets 
Find a degree 
Magazine Chapter 4: Problem 11
Write the Lewis electron-dot formula for \(\mathrm{Ar} \quad \mathrm{S}\) \(\mathrm{S}^{2-}\) \(\mathrm{Al}^{4}\) Cl-
Short Answer
Expert verified
Ar: :Ar:, S: :S:, \(S^{2-}\): [:S:], Al: Error, use \(Al^{3+}\), Cl鈦�: [:Cl:].
Step by step solution
01
Identify Valence Electrons
To draw the Lewis electron-dot formula, first identify the number of valence electrons for each element or ion: - For \(\text{Ar}\), an argon atom, it is a noble gas with 8 valence electrons.- For \(\text{S}\), a sulfur atom, it has 6 valence electrons.- For \(\text{S}^{2-}\), a sulfide ion, it has 8 valence electrons because it gains 2 additional electrons.- For \(\text{Al}^4\), an aluminum 4+ ion is not possible in this context, but if we consider \(\text{Al}^{3+}\), it would have 0 valence electrons due to losing 3 electrons.- For \(\text{Cl}^-\), a chloride ion, it has 8 valence electrons because it gains 1 electron.
02
Determine Lewis Dot Structure for Ar
Argon \((\text{Ar})\) is a noble gas with 8 valence electrons. Therefore, represent Ar with eight dots around it, indicating a full valence shell::Ar: Each pair represents an electron pair, and four pairs completely fill the valence shell.
03
Determine Lewis Dot Structure for S
Sulfur \((\text{S})\) has 6 valence electrons. Place the dots around the \(\text{S}\) symbol. Start by placing single dots on each side and then pair them::S:Of the six dots, two are paired, and four are unpaired.
04
Determine Lewis Dot Structure for S虏鈦�
Sulfur ion \((\text{S}^{2-})\) has gained 2 electrons, leading to 8 valence electrons. The Lewis structure resembles that of a noble gas with all pairs:[:S:]Each side of the \(\text{S}\) symbol is now paired, totaling to four pairs (8 electrons).
05
Discuss Aluminum Ion (Error with 4+)
There is an error with \((\text{Al}^{4}\)), as normally \(\text{Al}\) can form the 3+ ion \((\text{Al}^{3+})\). Let's consider \(\text{Al}^{3+}\): An aluminum ion with three positive charges \((\text{Al}^{3+})\) has no remaining valence electrons since all are lost, leaving no dots around it.
06
Determine Lewis Dot Structure for Cl鈦�
A chloride ion \((\text{Cl}^- )\) has 8 valence electrons as it gains one extra electron over the neutral Cl. The Lewis structure mirrors that of a noble gas:[:Cl:]Each pair represents an electron pair, and this configuration fills the valence electron shell.
Unlock Step-by-Step Solutions & Ace Your Exams!
-
Full Textbook Solutions
Get detailed explanations and key concepts
-
Unlimited Al creation
Al flashcards, explanations, exams and more...
-
Ads-free access
To over 500 millions flashcards
-
Money-back guarantee
We refund you if you fail your exam.
Over 30 million students worldwide already upgrade their learning with 91影视!
Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Valence Electrons
Valence electrons are the outermost electrons of an atom. They play a crucial role in chemical bonding and determining an atom's behavior in reactions. These electrons are found in the highest energy level and can be easily shared or transferred during reactions.
- For instance, argon (Ar) in its elemental state has 8 valence electrons. This makes it very stable.
- Sulfur (S) has 6 valence electrons. While it is not as stable as argon, it can gain or share electrons to reach a stable state.
- For ions like \( ext{S}^{2-} \), the addition of 2 electrons increases sulfur's valence electrons to 8, resembling a noble gas configuration.
Noble Gases
Noble gases are elements that are characterized by having a full valence shell. This full outer shell means they are generally non-reactive and stable.
Noble gases like helium, neon, and argon do not usually form compounds because they already have a complete set of valence electrons.
Noble gases like helium, neon, and argon do not usually form compounds because they already have a complete set of valence electrons.
- Argon (Ar) is an example, having 8 electrons that completely fill its outer electron shell.
- In Lewis structures, noble gases are represented with 8 dots around them, indicating these full valence shells.
Ions
Ions form when atoms gain or lose electrons. This results in a charge imbalance, creating either positive or negative ions.
- Positive ions, or cations, occur when an atom loses electrons. For example, aluminum can form \( ext{Al}^{3+} \), having lost 3 electrons, resulting in no remaining valence electrons.
- Negative ions, or anions, occur when an atom gains electrons. A chloride ion (Cl鈦�) gains one electron to fill its valence shell.
Electron Pairs
Electron pairs are sets of two electrons occupying the same orbital in an atom's outer shell. In Lewis structures, electron pairs are shown as pairs of dots.
- A complete electron pair contributes to the stability of an atom, as seen in noble gases.
- Lone pairs are used in Lewis dot diagrams to indicate unshared electrons. For sulfur (S), its Lewis structure shows 2 paired electrons and 4 single dots.
