Name: lewis structures with formal charge
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 2 min 42 s
Channel: JoVE

K12 Standards

north-carolina-k-12-science-standard-course-of-study

North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.3.1

Formal Charges

어떤 분자나 다원자 이온은 여러 개의 루이스 구조로 표현될 수 있는데 어떤 것이 주된 구조인지 어떻게 결정할까요? 원자의 형식 전하를 계산하면 분자의 실제 구조에 가장 가까운 루이스 구조를 결정할 수 있습니다. 각 원자에는 형식 전하라고 불리는 가상적인 전하가 할당되는데 이것은 분자 내의 모든 원자들이 동일한 전기음성도를 가지고 있는 경우 원자에 대한 전하가 될 것입니다.

이 때 각각의 결합 전자가 두 원자에 의해 동등하게 공유된다고 가정합니다. 염화수소를 생각해 봅시다. 각 원자의 형식 전하를 결정하려면 먼저 결합 전자 수의 절반에 비결합 전자 수를 더한 다음 원자가 전자 수에서 얻은 값을 뺍니다.

분자 또는 이온의 모든 형식 전하의 합계는 분자 또는 이온의 순 전하와 동일합니다. 예를 들어, 아산화질소는 3개의 가능한 루이스 구조로 표현될 수 있습니다. 하나는 질소 원자 사이의 두 개의 이중 결합, 하나는 질소 원자 사이의 삼중 결합, 그리고 하나는 질소와 산소 사이에 삼중 결합입니다.

이 모든 것이 옥텟을 만족시킵니다. 최선의 루이스 구조는 형식 전하 계산으로 확인됩니다. 질소는 5개의 원자가 전자를 가지고 있고, 산소는 6개의 원자가 전자를 가지고 있습니다.

비결합 전자 수와 결합 전자 수의 절반에 기반하여 계산하면 각 구조에 대한 형식 전하를 얻습니다. 아산화질소는 중성 분자이기 때문에 모든 형식 전하의 합은 0이어야 합니다. 일반적으로 주된 루이스 구조에서 개별 원자의 형식 전하는 0에 가장 가깝습니다.

따라서, 형식 전하량이 더 높은 세 번째 구조는 무시할 수 있습니다. 또한, 음의 형식 전하가 존재한다면, 가장 전기음성도가 높은 원자에 의해 운반되어야 합니다. 산소가 질소보다 전기적으로 더 음성이기 때문에 산소에 음의 형식 전하가 있는 두 번째 구조가 아산화질소의 주된 구조로 적합합니다.

형식 전하는 분자나 원자의 실제 전하가 아니라 문서상의 관례입니다. 분자의 실제 전하는 구성 원자들 사이의 전기 음성도의 차이를 포함한 몇 가지 요인에 의해 좌우됩니다.

형식 전하

어떤 경우에는 분자와 다원자 이온에 대해 하나 이상의 유효한 루이스 구조가 있는 것처럼 보입니다. 형식 전하의 개념은 둘 이상의 합리적인 구조가 존재할 때 가장 적절한 루이스 구조를 예측하는 데 도움이 될 수 있습니다.

형식 전하 계산

분자 내 원자의 형식 전하는 결합의 전자가 원자 사이에 고르게 분포되어 있는 경우 원자가 가질 수 있는 가상 전하입니다. 대안적으로, 형식 전하는 중성 원자의 원자가 전자 수에서 비결합 전자가 먼저 감소되고 루이스 구조에서 해당 원자에 연결된 결합 수를 뺄 때 발생합니다.

따라서 형식 전하는 다음과 같이 계산됩니다.

<img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/1065/1065_Equations-01.png" style="height: 60px;" />

형식 전하 계산은 전체 구조에 대한 형식 전하 합계를 결정하여 다시 확인할 수 있습니다. 분자 내 모든 원자의 형식 전하의 합은 0이어야 합니다. 이온의 형식 전하의 합은 이온의 전하와 같아야 합니다. 원자에 대해 계산된 형식 전하는 분자 내 원자의 실제 전하가 아니라는 점을 기억하세요. 형식 전하는 유용한 장부 절차일 뿐입니다. 이는 실제 전하가 있음을 나타내지는 않습니다.

루이스 구조에서 형식 전하 계산하기

인터할로겐 이온 ICl_4^−의 각 원자에 형식 전하를 할당하려면 다음 단계를 따릅니다.

Step 1. 모든 I-Cl 결합에 대해 결합 전자쌍을 동일하게 나눕니다.

<img alt="Figure1" src="https://www.jove.com/files/core/CDNSource/lessons/1065/1065image_1.svg" style="height: 120px;" />

Step 2. 비공유 전자쌍을 원자에 할당합니다. 이제 각 염소 원자에는 7개의 전자가 할당되고, 요오드 원자에는 8개의 전자가 할당됩니다.



Step 3. 중성 원자의 원자가 전자 수에서 이 숫자를 뺍니다.



요오드: 7 – 8 = –1

염소: 7 – 7 = 0

모든 원자의 형식 전하의 합은 -1이며, 이는 이온의 전하(-1)와 동일합니다.

형식 전하를 사용하여 분자 구조 예측

분자나 이온의 원자 배열을 분자 구조라고 합니다. 많은 경우 루이스 구조를 작성하는 단계를 따르면 여러 개의 서로 다른 결합과 고립전자쌍 배치 또는 서로 다른 원자 배열 등 하나 이상의 가능한 분자 구조가 생성될 수 있습니다. 형식 전하와 관련된 몇 가지 지침은 가능한 구조 중 특정 분자 또는 이온에 대해 가장 가능성이 높은 구조를 결정하는 데 도움이 될 수 있습니다.

<ol>
	<li>모든 형식 전하가 0인 분자 구조는 일부 형식 전하가 0이 아닌 분자 구조보다 바람직합니다.</li>
	<li>루이스 구조가 0이 아닌 형식 전하를 가져야 한다면 가장 작은 0이 아닌 형식 전하를 갖는 배열이 바람직합니다.</li>
	<li>루이스 구조는 인접한 형식 전하가 0이거나 반대 부호일 때 선호됩니다.</li>
	<li>유사한 형식 전하 분포를 갖는 여러 루이스 구조 중에서 선택할 때 전기 음성도가 더 높은 원자에 음의 형식 전하를 갖는 구조가 바람직합니다.</li>
</ol>

이러한 지침이 어떻게 적용되는지 보려면 이산화탄소, CO_2의 몇 가지 가능한 구조를 생각해보세요. 일반적으로 전기음성도가 낮은 원자가 중심 위치를 차지하는 것으로 알려져 있지만 형식 전하는 이것이 왜 발생하는지 이해하는 데 도움이 됩니다. 구조에 대한 세 가지 가능성이 그려질 수 있습니다. 중앙에 두 개의 이중 결합이 있는 탄소, 중앙에 단일 및 삼중 결합이 있는 탄소, 중앙에 이중 결합이 있는 산소가 있습니다.

<img alt="Figure2" src="https://www.jove.com/files/core/CDNSource/lessons/1065/1065image_2.svg" style="height: 80px;" />

세 가지 형식 전하를 비교할 때 왼쪽의 구조는 형식 전하가 0이므로 바람직한 것으로 식별할 수 있습니다.

또 다른 예로서, 탄소 원자, 질소 원자 및 황 원자로 형성된 이온인 티오시아네이트 이온은 NCS-, CNS- 또는 CSN-의 세 가지 다른 분자 구조를 가질 수 있습니다. 이러한 각 분자 구조에 존재하는 형식 전하는 가장 가능성이 높은 원자 배열을 선택하는 데 도움이 될 수 있습니다. 가능한 루이스 구조와 티오시안산염 이온의 세 가지 가능한 구조 각각에 대한 형식 전하는 이중 결합이 있는 중앙의 탄소, 이중 결합이 있는 중앙의 질소, 이중 결합이 있는 중앙의 황입니다.

<img alt="Figure3" src="https://www.jove.com/files/core/CDNSource/lessons/1065/1065Image_3.svg" style="height: 95px;" />

각 경우의 형식 전하의 합은 이온의 전하(-1)와 같습니다. 그러나 중앙에 탄소가 있는 원자의 첫 번째 배열은 0이 아닌 형식 전하를 갖는 원자 수가 가장 적기 때문에 선호됩니다. 또한, 전기 음성도가 가장 낮은 원자를 중앙에 배치하고 전기 음성도가 더 높은 원소에 음전하를 배치합니다.

이 문서는 에서 발췌되었습니다 <a href="https://openstax.org/books/chemistry-2e/pages/7-4-formal-charges-and-resonance">Openstax, Chemistry 2e, Chapter 7.4 Formal Charges and Resonance.</a>

어떤 경우에는 분자와 다원자 이온에 대해 하나 이상의 유효한 루이스 구조가 있는 것처럼 보입니다. 공식 요금의 개념은 다음과 같이 사용될 수 있습니다.

Education

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화학

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Chemical Bonding: Basic Concepts

화학 결합: 기본 개념

KEY TERMS AND CONCEPTS

주요 용어 및 개념

lewis structures with formal charge

Lewis structures can sometimes show more than one reasonable arrangement for a molecule or polyatomic ion. Formal charge helps chemists choose the best Lewis structure when that happens. It is a useful way to compare possible structures in chemistry.

Formal charge is the hypothetical charge an atom would have if bonding electrons were shared evenly between the atoms. It can also be found by starting with the valence electrons of the neutral atom, subtracting the nonbonding electrons, and then subtracting the number of bonds on that atom in the Lewis structure. This is a bookkeeping tool, not the actual charge on the atom.

The formal charge of a full structure should also be checked as a whole. For a neutral molecule, the sum of all formal charges must be zero. For an ion, the sum of all formal charges should match the ion’s overall charge.

A common example is the interhalogen ion ICl4−. To assign formal charges, the bonding electron pairs are divided equally among the I–Cl bonds. Then lone pairs are assigned to their atoms. In this structure, each chlorine has seven electrons assigned to it, and iodine has eight. That gives iodine a formal charge of −1 and each chlorine a formal charge of 0, which adds up to the −1 charge of the ion.

Formal charge also helps predict molecular structure when several Lewis structures are possible. A structure with all formal charges equal to zero is preferred over one with nonzero charges. If nonzero charges are needed, the best choice has the smallest charges possible. Structures are also preferred when adjacent formal charges are zero or opposite in sign. When several choices are still possible, the negative charge should be on the more electronegative atom.

Carbon dioxide shows why these rules matter. One possible structure has carbon in the center with two double bonds. Other possibilities place carbon between a single and a triple bond, or place oxygen in the center with double bonds. The structure with carbon in the center and two double bonds is preferred because all of its formal charges are zero.

The thiocyanate ion, NCS−, gives another clear example. It can be written with carbon, nitrogen, or sulfur in the center. The formal charges in each possible Lewis structure help identify the most likely arrangement of atoms. The carbon-centered structure is preferred because it has the fewest atoms with nonzero formal charges. It also places the least electronegative atom in the center and the negative charge on the more electronegative element.

Lewis Structures with Formal Charge

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Learn how formal charge helps compare Lewis structures, check total charge, and choose the best arrangement for molecules and ions like CO2 and NCS−.

Lewis Structures with Formal Charge | JoVE K12

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The process of converting very light nuclei into heavier nuclei is also accompanied by the conversion of mass into large amounts of energy, a process ...

Nuclear Transmutation

Nuclear transmutation is the conversion of one nuclide into another. It can occur by the radioactive decay of a nucleus, or the reaction of a nucleus with ...

Use models to compare nuclear reactions including alpha decay, beta decay and gamma decay; nuclear fusion and nuclear fission.

PS.Chm.1.2

Atomic Orbitals

An atomic orbital represents the three-dimensional regions in an atom where an electron has the highest probability to reside. The radial distribution ...

The Pauli Exclusion Principle

The arrangement of electrons in the orbitals of an atom is called its electron configuration. We describe an electron configuration with a symbol that ...

The Energies of Atomic Orbitals

In an atom, the negatively charged electrons are attracted to the positively charged nucleus. In a multielectron atom, electron-electron repulsions are ...

The Aufbau Principle and Hund's Rule

To determine the electron configuration for any particular atom, we can build the structures in the order of atomic numbers. Beginning with hydrogen, and ...

electron-configuration-of-multielectron-atoms

Electron Configuration of Multielectron Atoms

The alkali metal sodium (atomic number 11) has one more electron than the neon atom. This electron must go into the lowest-energy subshell available, the ...

Use models to explain how electrons are distributed in atoms.

PS.Chm.1.3

Periodic Classification of the Elements

The periodic table arranges atoms based on increasing atomic number so that elements with the same chemical properties recur periodically. When their ...

The Periodic Table

As early chemists discovered more elements, they realized that various elements could be grouped by their similar chemical behaviors. One such grouping ...

Atomic Mass

Atoms &mdash; and the protons, neutrons, and electrons that compose them &mdash; are extremely small. For example, a carbon atom weighs less than 2 ...

Molar Mass

The identity of a substance is defined not only by the types of atoms or ions it contains but by the quantity of each type of atom or ion. For example, ...

Use the Periodic Table as a model to predict the relative properties of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.Chm.2.1

atomic-radii-and-effective-nuclear-charge

Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number ...

Ionic Radii

Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it ...

Ionization Energy

The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy ...

Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).



This process can be either ...

Construct an explanation to infer the atomic size, reactivity, electronegativity, and ionization energy of an element based on its position in the Periodic Table.

PS.Chm.2.2

Types of Chemical Bonds

Chemical bonding theories were pioneered by American chemist Gilbert&#xA0;N. Lewis. He developed a model called the Lewis model to explain the type and ...

Lewis Symbols and the Octet Rule

Chemical bonds are complex interactions between two or more atoms or ions, which reduce the potential energy of the molecule. Gilbert N. Lewis developed a ...

Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence ...

The Born-Haber Cycle

Lattice Energy&#xA0;

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a ...

Trends in Lattice Energy: Ion Size and Charge

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a compound is a measure ...

Covalent Bonding and Lewis Structures

Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual ...

Electronegativity

Whether a bond is nonpolar or polar covalent is determined by a property of the bonding atoms called electronegativity.&#xA0;

Electronegativity values of ...

Bond Polarity, Dipole Moment, and Percent Ionic Character

Bond Polarity

The absolute value of the difference in electronegativity (&Delta;EN) of two bonded atoms provides a rough measure of the polarity to be ...

Lewis Structures of Molecular Compounds and Polyatomic Ions

To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined:


	Determine the ...

Resonance

The Lewis structure of a nitrite anion (NO2&minus;) may actually be drawn in two different ways, distinguished by the locations of the N-O and N=O ...

In some cases, there are seemingly more than one valid Lewis structures for molecules and polyatomic ions. The concept of formal charges can be used to ...

Exceptions to the Octet Rule

Many covalent molecules have central atoms that do not have eight electrons in their Lewis structures. These molecules fall into three categories:


	...

Bond Energies and Bond Lengths

Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, ...

Analyze and interpret data to explain the mechanisms and properties of the two main types of intramolecular (ionic and covalent) bonds.

molecular-comparison-of-gases-liquids-and-solids

Molecular Comparison of Gases, Liquids, and Solids

Particles in a solid are tightly packed together (fixed shape) and often arranged in a regular pattern; in a liquid, they are close together with no ...

Intermolecular vs Intramolecular Forces

Intermolecular forces (IMF) are electrostatic attractions arising from charge-charge interactions between molecules. The strength of the intermolecular ...

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions ...

comparing-intermolecular-forces-melting-point-boiling-point

Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, ...

Construct an explanation to summarize the influences intermolecular forces have on the properties of chemical compounds.

PS.Chm.3.2

Analyze the structure of atoms and isotopes.

Lewis Structures with Formal Charge

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