Name: drawing lewis structures with valence electron counts
Uploaded: 2020-09-03T13:38:28.000Z
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Lewis Structures of Molecular Compounds and Polyatomic Ions

路易斯结构是原子间 化学键的简化表示。写出中性化合物如乙烯或氨，或多原子离子如水合氢离子 或磷酸盐的路易斯结构涉及以下顺序的步骤。首先，计算分子中价电子的 总数。以乙烯为例。每个碳原子有 4 个价电子，每个氢原子有 1 个价电子；乙烯有 2 个碳原子和 4 个氢原子，因此共有 12 个价电子。接下来，画出分子的骨架结构。一般来说，化学式中的第一个原子 或电负性较小的原子放在中心。这个原子也被称为中心原子 并且必须能够形成至少两个键。氢原子或电负性更强的原子 位于中心原子的末端。在这里，碳原子占据了中心位置，氢原子围绕着它们。下一步是八电子结构的完成。首先，在每两个原子之间放置一对电子 来表示成键对。剩下的电子以孤对的形式分布到 末端原子和中心原子以满足二电子或八电子的 稳定结构。在这种情况下，由于氢已经达到二电子结构，剩下的电子被转移 到碳原子上。现在，用孤对电子在缺少八电子结构的原子之间 形成多个键。在乙烯中，碳原子还没有达到八电子稳定结构。因此，一个孤对被移到键合区 以形成双键，使所有原子 都能达到稳定的电子构型。为了写出带电多原子离子，如水合氢离子 或磷酸盐的路易斯结构，也采用了 同样的方法，只是加了一个修改来 调节离子电荷。要绘制水合氢离子的路易斯结构，首先，计算离子上价电子的数目。因为氢离子带正电荷，所以从总的价电子中去掉一个电子，使其数目减少到 8 个。接下来，用它的骨架结构来说明这个分子。现在在每个原子之间放置一对电子，然后 在中心原子上放置一对孤对电子。这样的话，氢原子和氧原子 就分别满足二电子结构和八电子结构。最后，把路易斯结构 写在括号里，然后在它的右上角 加上一个正电荷。

分子化合物和多原子离子的路易斯结构

要绘制复杂分子和分子离子的路易斯结构，遵循以下概述的分步操作会有所帮助：
 
 <ol>
 <li>确定价电子（外壳）的总数。对于阳离子，每个正电荷减去一个电子。对于阴离子，每个负电荷加一个电子。</ li>
 <li>绘制分子或离子的骨架结构，将原子排列在中心原子周围。 （通常，最小负电性的元素应放在中心。）将每个原子与中心原子通过单键（一个电子对）连接。</ li>
 <li>将剩余的电子以孤对形式分布在末端原子上（氢除外），从而在每个原子周围形成一个八偶体。</ li>
 <li>将所有剩余的电子放在中心原子上。</ li>
 <li>重新排列外部原子的电子，使其与中心原子形成多个键，以便尽可能获得八偶体。</ li>
 </ ol>
 
 例如，考虑SiH 4 ，CHO 2 ＆ndash; ，NO + 和OF 2 作为示例，可以应用此一般准则来确定其路易斯结构。
 
 <ol>
 <li>确定分子或离子中的价电子（外壳）总数。</ li>
 </ ol>
 
 对于像SiH 4 这样的分子，该分子中每个原子上的价电子数相加：
 
 = [4价e ＆minus; / Si原子＆times; 1 Si原子] + [1价e ＆minus; / H原子＆times; 4 H原子] = 8价e ＆minus; 
 
 <h4> CHO 2 ＆ndash; </ h4>
 
 对于负离子，例如CHO 2 ＆ndash; ，原子上的价电子数与离子上的负电荷数相加（每个负电荷会获得一个电子）：
 
 = [4价e ＆minus; / C原子＆times; 1 C原子] + [1价e ＆minus; / H原子＆times; 1 H原子] + [6价e ＆minus; / O原子＆times; 2个O原子] + [另外1个e ＆minus; ] = 18价e ＆minus; 
 
 <h4>否 + </ h4>
 
 对于正离子（如NO +），将离子中原子上的价电子数量相加，然后减去价电子总数：
 
 = [5价e ＆minus; / N原子＆times; 1 N原子] + [6价e ＆minus; / O原子＆times; 1 O原子] + [＆minus; 1 e ＆minus; ] = 10价e ＆minus; 
 
 <h4> OF 2 ＆nbsp; </ h4>
 
 OF 2 是中性分子，只需添加价电子数：
 
 = [6价e ＆minus; / O原子＆times; 1 O原子] + [7价e ＆minus; / F原子＆times; 2个F原子] = 20价e ＆minus; 
 
 <ol start =“ 2”>
 <li>绘制分子或离子的骨架结构，将原子排列在中心原子周围，并通过单键（一个电子对）将每个原子连接到中心原子。 （请注意，离子在结构周围用方括号表示，离子电荷在方括号之外：） 
 <img alt="Figure1" src="https://www.jove.com/files/core/CDNSource/lessons/1063/1063Image_1.svg" style="height: 80px;" /> 
 对于CHO 2 ＆minus; 可能存在几种原子排列的情况，将使用实验证据来选择正确的原子。通常，负电性较低的元素更有可能是中心原子。在CHO 2 ＆minus 中，负电性较低的碳原子的中心位置是氧和氢原子。其他示例包括POCl 3 中的P，SO 2 中的S和＆Clb 4 ＆minus; 中的Cl 。 ＆nbsp;一个例外是氢几乎从来不是中心原子。作为最具负电性的元素，氟也不能成为中心原子。</ li>
 <li>将剩余的电子以孤对形式分布在末端原子上（氢除外），以一个八偶体电子完成它们的化合价壳。 （SiH 4 上没有剩余电子，其结构不变。） 
 <img alt="Figure2" src="https://www.jove.com/files/core/CDNSource/lessons/1063/1063image_2.svg" style="height: 80px;" /></li>
 <li>将所有剩余的电子放在中心原子上。
 <ul>
 <li>对于SiH 4 ，＆nbsp; CHO 2 ＆minus; ，＆nbsp;和NO + ，有没有剩余的电子。对于OF 2 ，剩余的16个电子中有12个被放置，从而使4个电子被放置在中心原子上： 
 <img alt="Figure3" src="https://www.jove.com/files/core/CDNSource/lessons/1063/1063Image_3.svg" style="height: 40px;" /></li>
 </ ul>
 </ li>
 重新排列外部原子的电子，使其与中心原子形成多个键，并尽可能获得八偶体。
 <ul>
 <li> SiH 4 ：Si已经有一个八偶体，因此无需执行任何操作。 
 <img alt="Figure4" src="https://www.jove.com/files/core/CDNSource/lessons/1063/1063Image_4.svg" style="height: 70px;" /></li>
 <li> CHO 2 ＆minus; ：价电子以孤对形式分布在氧原子上，而碳原子缺少一个八偶体。 >
 <img alt="Figure5" src="https://www.jove.com/files/core/CDNSource/lessons/1063/1063Image_5.svg" style="height: 80px;" /></li>
 因此，一对孤立的电子从一个氧原子提供给碳原子，形成一个双键。根据提供给电子的氧原子的不同，可以有两种可能的结构，也称为共振结构。</ li>
 <li> NO + ：对于此离子，添加了八个价电子，但两个原子都没有八偶体。由于总电子已用完，因此无法添加其他电子。在这种情况下，必须移动电子以形成多个键。氮原子有两个孤对电子，氧原子有一个对电子。 
 <img alt="Figure6" src="https://www.jove.com/files/core/CDNSource/lessons/1063/1063Image_6.svg" style="height: 55px;" /></li>
 <li>这仍然不会产生八偶体，因此必须移动另一对以形成三重键。 
  <img alt="Figure7" src="https://www.jove.com/files/core/CDNSource/lessons/1063/1063Image_7.svg" style="height: 50px;" /></li>
 <li>在OF 2 中，由于每个原子已经具有一个八偶体，因此没有任何变化。 
 <img alt="Figure8" src="https://www.jove.com/files/core/CDNSource/lessons/1063/1063Image_8.svg" style="height: 40px;" /></li>
 </ ul>
 </ li>
 </ ol>
 
 本文改编自<a href="https://openstax.org/books/chemistry-2e/pages/7-3-lewis-symbols-and-structures">Openstax, 化学2e, 第7.3节：路易斯符号和结构。</a>
 
 ＆nbsp;

要绘制复杂分子和分子离子的 Lewis 结构，遵循概述的分步程序会很有帮助:

确定 ...

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drawing lewis structures with valence electron counts

Drawing Lewis structures starts with counting valence electrons and building the atom arrangement step by step. Valence electrons are the outer-shell electrons that help show how atoms bond. For ions, a positive charge means one electron is removed for each plus sign, and a negative charge means one electron is added for each minus sign.

The next step is to sketch the skeleton structure. The least electronegative atom usually goes in the center, while hydrogen is almost never central. Fluorine also cannot be a central atom because it is the most electronegative element. Ions are written in brackets, with the charge shown outside the brackets.

After the skeleton is drawn, connect the atoms to the central atom with single bonds. Each single bond represents one electron pair. Then place the remaining electrons as lone pairs on the terminal atoms, except hydrogen, until those atoms have octets when possible. Any electrons still left go on the central atom.

If the central atom still does not have an octet, move lone pairs to make double or triple bonds. This can create resonance structures, which are different valid arrangements of electrons. For the formate ion, CHO2−, one oxygen can donate a lone pair to make a double bond with carbon. That gives two possible resonance forms.

The examples in the model show how the procedure works in real cases. SiH4 has 8 valence electrons total, so its structure does not need more changes once the single bonds are drawn. CHO2− has 18 valence electrons. NO+ has 10 valence electrons, and its atoms must be rearranged into a triple bond to satisfy octets as much as possible. OF2 has 20 valence electrons, and after the lone pairs are placed, its structure stays unchanged because each atom already has an octet.

Drawing Lewis Structures with Valence Electron Counts

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Drawing Lewis structures starts with counting valence electrons and building the atom arrangement step by step. Valence electrons are the outer-shell electrons that help show how atoms bond. For ions, a positive charge means one electron is removed for each plus sign, and a negative charge means one electron is added for each minus sign. The next step is to sketch the skeleton structure. The least electronegative atom usually goes in the center, while hydrogen is almost never central. Fluorine...

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Learn the step-by-step method for drawing Lewis structures, counting valence electrons, placing lone pairs, and handling ions, resonance, and multiple bonds.

Drawing Lewis Structures with Valence Electron Counts | JoVE K12

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Drawing Lewis Structures with Valence Electron Counts

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