Name: ionic compounds and crystal lattices
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 2 min 48 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

Ionic Bonding and Electron Transfer

イオン結合金属から非金属への 電子の移動によって 形成されます 電子を共有する 共有結合と比較して イオン結合では 傾向として 金属は電子を失い 非金属は電子を受け入れます しかし なぜでしょうか？原子の電子配置が 最も安定しているのは 完全なオクテットの状態です ポテンシャルエネルギーを 下げることと併せて この状態を達成することが 結合形成の大きな 原動力となります しかし どのようにして 電子が移動し 共有されない状態になるかを 予測するのでしょうか？そのためには 原子のイオン化エネルギーと 電子親和性を調べてみましょう 周期表では sブロック金属は イオン化エネルギーが 低くなっています そのため 陽イオンを 形成しながら オクテットに到達するための 電子を失いやすくなっています 一方 希ガスを除く pブロックの非金属は 電子親和性が高く 電子を受け入れて 陰イオンを形成します 反対に帯電した 陽イオンと陰イオンは 強い静電相互作用を起こし 互いに引き合って イオン結合を形成します イオン性化合物は イオン間の強力な静電引力により 高融点の硬く 明確な結晶構造を 形成することがよくあります リチウムとフッ素からなる イオン性化合物である フッ化リチウムを 考えてみましょう リチウムが電子を失って デュエットを持つ リチウムカチオンになるとき その電子はフッ素に取り込まれて オクテットを持つ アニオンになります クーロンの法則によれば これら2つの荷電粒子は 互いに引き合って中性化合物の フッ化リチウムを形成します ルイスモデルは イオン性化合物の化学式を記述し 予測するために 使用することができます ルイス記号は右上に電荷を示し カッコの中に 陰イオンと陽イオンを 記号で表しています 花火の真っ赤な色を出すために　よく使われる塩である 塩化ストロンチウムを 考えてみましょう ルイス記号でストロンチウムは 2個の不対電子を 塩素は1個の 不対電子を持っています ストロンチウムは電子を 2個失う必要があるのに対し 塩素は電子を1個増やさなければ オクテットになりません ゆえに1つのストロンチウム カチオンは2つの塩素アニオンに 1:2の割合で結合します

イオン結合と電子移動

イオンとは、電荷を持つ原子や分子のことです。カチオン（陽イオン）は、中性原子がその原子価殻から電子を1つ以上失うことで形成され、アニオン（陰イオン）は、中性原子がその原子価殻から電子を1つ以上得ることで形成されます。イオンからなる化合物はイオン性化合物（または塩）と呼ばれ、構成するイオンはイオン結合（逆に帯電した陽イオンと陰イオンの間の静電力による引力）によって結合しています。
 
 <h4>イオン化合物の特性 </h4>
 
 イオン性化合物の性質から、イオン結合の性質を知ることができます。 
 
 <ul>
 <li>イオン性固体は結晶構造を持ち、硬くて脆い傾向があります。また、融点や沸点が高い傾向があり、イオン結合が非常に強いことを示唆しています。</li>
 <li>イオン性固体が電気を通さないのも同じ理由で、イオン結合の強さのためにイオンが固体内を自由に移動できないからです。</li>
 <li>しかし、ほとんどのイオン性固体は、水に容易に溶解します。イオン性化合物は、いったん溶解したり溶けたりすると、イオンが自由に動き回るため、電気や熱の伝導性に優れています。 </li>
 </ul>
 
 <h4>イオン化合物の形成 </h4>
 
 金属元素の多くはイオン化ポテンシャルが比較的低く、電子を失いやすいです。これらの元素は、周期表では周期の左側、またはグループの下側に位置します。非金属原子は比較的電子親和力が高いため、金属原子が失った電子を容易に獲得し、価電子殻を満たすことができます。非金属元素は、周期表の右上にあります。 
 
 すべての物質は電気的に中性でなければならないので、イオン化合物の陽イオンの正電荷の合計数と陰イオンの負電荷の合計数は等しくなければなりません。イオン性化合物の式は、同じ数の正負の電荷を与えるために必要なイオンの数の最も単純な比率を表しています。
 
 <h4>イオン化合物は規則的な3次元構造を形成する </h4>
 
 ただし、イオン性化合物の式は、そのイオンの物理的な配置を表すものではないことに注意する必要があります。ナトリウムイオンと塩化物イオンの間には、イオン結合が1つもないため、塩化ナトリウム（NaCl）分子と呼ぶのは誤りです。イオン間の引力は等方的で、すべての方向に同じです。つまり、特定のイオンは、近くにある反対の電荷を持つすべてのイオンに等しく引き付けられます。つまり、あるイオンは、近くにある反対の電荷を持つすべてのイオンに同じように引き付けられ、その結果、イオンは3次元の格子構造を形成して緊密に結合します。例えば、塩化ナトリウムは、同数のNa+イオンとCl–イオンが規則的に配列されています。Na+イオンとCl–イオンの間には強い静電引力が働いており、固体のNaClではそれらが強固に結合しています。1モルの固体NaClをガス状のNa+とCl–イオンに分解するには769kJのエネルギーが必要です。
 
 <h4>陽イオンの電子構造 </h4>
 
 陽イオンを形成すると、主群元素の原子はすべての価電子を失う傾向があり、その結果、周期表でその前に位置する希ガスの電子構造をとります。
 
 <ul>
 <li>1族（アルカリ金属）と2族（アルカリ土類金属）では、族番号は原子価殻電子の数に等しく、その結果、これらの元素の原子からすべての原子価殻電子を取り除いたときに形成される陽イオンの電荷にも等しいです。</li>
 <li>たとえば、カルシウムは、中立原子が 20 電子を持ち、基底状態の電子構成が1s22s22p63s23p64s2の2族元素です。 Ca 原子が両方の価電子を失うと、その結果、 18 電子の陽イオン、 2+ 電荷、および1s22s22p63s23p6の電子構成が得られます。 したがって、 Ca2+ イオンは希ガス Ar と等電子になります。 </li>
 <li> 13～17族では、族番号が価電子の数を10上回っています（第4周期以上の元素の原子では完全なd小軌道が存在する可能性を考慮している）。したがって、すべての価電子を失って形成された陽イオンの電荷は、群番号から10を引いた値になります。例えば、アルミニウム（13族）は3+イオン（Al3+）を形成します。 </li>
 </ul>
 
 <h4>例外 </h4>
 
 <ul>
 <li>想定される動作の例外として、族の下部に位置する元素があります。</li>
 <li>Tl3+、Sn4+、Pb4+、Bi5+の予想されるイオンに加えて、これらの原子の価電子が部分的に失われると、 Tl+、Sn2+、Pb2+、Bi3+イオンが形成される可能性があります。 これらの 1+ 、 2+ 、および 3+ 陽イオンの形成は不活性電子対効果の原因とされ、それは13 、 14 、および 15族の重元素の原子に対する原子価電子対の比較的低いエネルギーを反映しています。</li>
 <li>水銀（第12族）も予想外の挙動を示し、予想される1原子イオンHg2+（1つの水銀原子から形成されるイオン）に加えて、2原子イオンHg2+（2つの水銀原子から形成されるイオンで、Hg-Hg結合を持つ）を形成します。 </li>
 <li>遷移金属元素と内部遷移金属元素は、主族元素とは異なる挙動を示します。ほとんどの遷移金属の陽イオンは、最初に最外殻のs電子を失い、時には次の最外殻のd電子を1つまたは2つ失った結果、2+または3+の電荷を持ちます。 </li>
 <li>遷移元素のd軌道は、アウフバウの原理により、電子配置を構築する際に最後に充填されるが、原子がイオン化する際には一番外側のs電子が最初に失われることになります。内側の遷移金属がイオンを形成すると、最外周のs電子とd電子またはf電子が失われて、通常は3+の電荷を持ちます。 </li>
 </ul>
 
 <h4>陰イオンの電子構造 </h4>
 
 ほとんどの単原子陰イオンは、中性の非金属原子がその外側のsおよびp軌道を完全に満たすのに十分な電子を獲得して、次の希ガスの電子配置に達すると形成されます。したがって、このような負イオンの電荷を決定するのは簡単です。電荷は、親原子のs軌道とp軌道を満たすために獲得しなければならない電子の数に等しいです。例えば、酸素は1s22s22p4という電子配置を持っていますが、酸素イオンは希ガスであるネオン（Ne）の電子配置である1s22s22p6を持っています。価電子軌道を埋めるのに必要な2つの電子が追加されることで、酸化物イオンの電荷は2-（O2-）となります。 
 
 このテキストは <a href="https://openstax.org/books/chemistry-2e/pages/7-1-ionic-bonding">、 Openstax, Chemistry 2e, Section 7.3: Ionic Bonding から引用したものです。</a>

イオンは、電荷を帯びた原子または分子です。陽イオン(陽イオン)は、中性原子がその価電子から1つ以上の電子を失ったときに形成されます...

Education

JoVE Core

化学

Chemical Bonding: Basic Concepts

化学結合：基本概念

KEY TERMS AND CONCEPTS

主要用語と概念

ionic compounds and crystal lattices

Ionic compounds form when positive and negative ions attract each other. A cation is a positive ion, and it forms when an atom loses one or more valence electrons. An anion is a negative ion, and it forms when an atom gains one or more valence electrons. Compounds made of these ions are called ionic compounds, or salts, and the force between them is an ionic bond.

The properties of ionic solids help show how strong this attraction is. They usually form rigid, brittle crystals and have high melting and boiling points. They are also poor conductors of electricity in the solid state because the ions cannot move freely. Most ionic solids dissolve readily in water. When an ionic compound is melted or dissolved, it conducts electricity and heat well because the ions can move about freely.

Ionic compounds form most easily when metals lose electrons and nonmetals gain them. Many metals have low ionization potentials, so they lose electrons easily. These elements are found on the left side of the periodic table or near the bottom of a group. Nonmetals have high electron affinities, so they readily gain the electrons lost by metals. They are found in the upper-right corner of the periodic table.

Ionic compounds must remain electrically neutral. That means the total positive charge from the cations must equal the total negative charge from the anions. The formula of an ionic compound gives the simplest ratio of ions needed to balance charge. The formula does not show the physical layout of the ions. In solid sodium chloride, for example, the ions form a tightly bound three-dimensional lattice. The attraction between Na+ and Cl- ions is strong, and it takes 769 kJ of energy to separate one mole of solid NaCl into gaseous ions.

Main-group cations often form by losing all valence electrons and taking on the electron structure of the noble gas before them. For groups 1 and 2, the group number matches the number of valence electrons and also the charge of the ion formed. Calcium is a group 2 element. A neutral calcium atom has 20 electrons, and Ca2+ has 18 electrons with the same electron configuration as argon. For groups 13 through 17, the cation charge equals the group number minus 10. Aluminum, in group 13, forms Al3+.

Some heavy main-group elements do not follow the expected pattern exactly. Thallium, tin, lead, and bismuth can also form lower-charge ions such as Tl+, Sn2+, Pb2+, and Bi3+. This is explained by the inert pair effect, which reflects the relatively low energy of the valence s-electron pair in these heavy atoms. Mercury is another exception. It can form the diatomic ion Hg2^2+, which contains a Hg-Hg bond, as well as the monatomic ion Hg2+.

Transition metals and inner transition metals form ions in a different way. Most transition metal cations have 2+ or 3+ charges. These usually come from losing the outermost s electron or electrons first, and sometimes one or two d electrons after that. Even though d orbitals fill later according to the Aufbau principle, the outermost s electrons are lost first when transition metals ionize. Inner transition metals usually form 3+ ions by losing their outermost s electrons and one d or f electron.

Most monatomic anions form when a nonmetal atom gains enough electrons to fill its outer s and p orbitals. The charge on the ion equals the number of electrons needed to reach the next noble-gas electron configuration. Oxygen is a clear example. A neutral oxygen atom has the configuration 1s2 2s2 2p4. The oxide ion, O2-, has the neon configuration, 1s2 2s2 2p6, after gaining two electrons.

Ionic Compounds and Crystal Lattices

types of chemical bonds

Chemical Bonding and Bond Properties

Chemical bonding explains how atoms and ions join to form molecules and compounds. American chemist Gilbert N. Lewis pioneered chemical bonding theory with the Lewis model. This model helps explain why bonds form, why some are stronger than others, and why compounds have fixed formulas like H2O instead of H4O. Ionic bonding involves ions, which are atoms or molecules with an electrical charge. A cation is a positive ion formed when a neutral atom loses one or more electrons from its valence...

the born-haber cycle

Predicting Ionic Stability with Lattice Energy

Lattice energy helps explain why ionic compounds are stable. It measures the strength of attraction between positive and negative ions in a crystal. In one common definition, lattice energy is the energy required to separate one mole of an ionic solid into gaseous ions, so it has a positive value. Another definition uses the opposite sign and describes the energy released when gaseous ions form a lattice. When checking data, it is important to confirm which convention is being used. In either...

lewis symbols and the octet rule

Valence Electrons, Lewis Symbols, and Bonding

Chemical bonds form when atoms or ions interact in ways that lower the potential energy of a molecule. Gilbert N. Lewis created a simple model to show bond formation using valence electrons, the electrons in the outer shell. In this model, electrons are shared or transferred to help atoms reach a stable electron configuration. The Lewis model helps describe two common bond types. An ionic bond forms when electrons move from a metal to a nonmetal. A covalent bond forms when two nonmetals share...

electronegativity

Electronegativity and Polar Bonds

Electronegativity helps explain why some covalent bonds are nonpolar and others are polar covalent. It is a measure of how strongly an atom attracts shared electrons toward itself. That pull controls how electron density is distributed in a bond. Linus Pauling proposed the first electronegativity values by studying bond energies in heteronuclear molecules such as hydrogen fluoride. He expected the bond energy of HF to be about the average of the bond energies of H2 and F2, or 296 kJ/mol. The...

ionic bonding and electron transfer

Ionic compounds form when positive and negative ions attract each other. A cation is a positive ion, and it forms when an atom loses one or more valence electrons. An anion is a negative ion, and it forms when an atom gains one or more valence electrons. Compounds made of these ions are called ionic compounds, or salts, and the force between them is an ionic bond. The properties of ionic solids help show how strong this attraction is. They usually form rigid, brittle crystals and have high...

trends in lattice energy: ion size and charge

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Lattice Energy Patterns in Ionic Solids

Lattice energy shows how strongly ions hold an ionic solid together. It is the energy required to separate one mole of a solid into its gaseous ions. For sodium chloride, this process requires 769 kJ per mole. The opposite convention may also be used, where lattice energy is the energy released when gaseous ions form the solid. In either case, a larger magnitude means a more stable ionic compound. For ionic crystals, lattice energy follows a pattern based on charge and ion size. The...

covalent bonding and lewis structures

Shared Electrons in Covalent Molecules

Covalent molecules form when atoms share electrons instead of transferring them. This bonding usually happens between nonmetal atoms with similar tendencies to attract electrons. Because the atoms pull on the electrons in a shared way, the bond is held together by mutual attraction. Covalent compounds often have physical properties that differ from ionic compounds. The attraction between neutral molecules is weaker than the attraction between charged ions. As a result, many covalent compounds...

bond polarity, dipole moment, and percent ionic character

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How Bond Polarity Shapes Molecular Dipoles

Bond polarity depends on electronegativity, the ability of an atom to attract shared electrons. The absolute value of the electronegativity difference, or ΔEN, gives a rough guide to bond type. When the difference is very small or zero, the bond is covalent and nonpolar. When it is larger, the bond may be polar covalent or ionic. Examples show how this works in real compounds. H–H has a ΔEN of 0, so it is nonpolar. H–Cl has a ΔEN of 0.9, so it is polar covalent. Na–Cl has a ΔEN of 2.1, so it...

lewis structures of molecular compounds and polyatomic ions

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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...

resonance

Resonance Forms in Lewis Structures

Resonance forms in Lewis structures help explain molecules and ions that cannot be shown correctly with just one drawing. In nitrite ion, NO2−, the Lewis structure can be drawn in two ways. The N-O and N=O bonds switch positions in the two drawings, but the atoms stay in the same arrangement. If nitrite really had one single bond and one double bond, the two bond lengths should be different. A double bond is shorter and stronger than a single bond between the same atoms. Experiments show that...

formal charges

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...

exceptions to the octet rule

Octet Rule Exceptions in Lewis Structures

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bond energies and bond lengths

How Bond Energy Predicts Reaction Heat

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Electron Sea Model in Metals

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key terms and concepts

Explore how ions form, why ionic compounds make crystal lattices, and how charge, conductivity, and electron configurations shape ionic behavior in chemistry.

Ionic Compounds and Crystal Lattices | JoVE K12

chemistry

JoVE Core 化学は、簡潔で理解しやすいアニメーションビデオレッスンを使用して、一般的な化学の概念を生き生きとしたものにします。さらに、活動する科学者のビデオでは、現在世界中の実験室で行われている古典的そして独創的な研究・実験をお見せします。

Physical Science

PS.PSc.2.1

Pennsylvania State Academic Standards

Structure and Properties of Matter

3.2.9-12.B

3.2.9-12.N

Louisiana Student Standards for Science

High School

Matter And Its Interactions

HS-PS1-3

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Ohio’s Learning Standards and Model Curriculum

Study Of Matter

Bonding and compounds

Structure And Properties Of Matter

Chemical bonding

Physical Geology

Minerals

Chemical bonding (ionic, covalent, metallic)

Tennessee Academic Standards

Matter and Its Interactions

CHEM1.PS1.13

CHEM1.PS1.14

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Motion and Stability: Forces and Interactions

CHEM1.PS2.1

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CH.3.d

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PS.3.c

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1.2.1 9L.4.2.2.1

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HS.P1U1.2

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New Jersey Student Learning Standards for Science

HS-PS1-2

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9-12.C.2.2.b

Florida Department of Education

SC.912.P.8

SC.912.P.8.6

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Chemistry and Physics

IPC.7

IPC.7.A

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New York State Science Learning Standards

HS. Structure and Properties of Matter

HS-PS1-3.

HS. Chemical Reactions

HS-PS1-2.

Georgia Standards of Excellence

SPS2.

Chemical Bonds

SC2.

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Bonding Types: From Nonpolar Covalent to Ionic

Scientific Laws and Theories

Scientific Laws

In science, a law is defined as a concise, verbal or mathematical, statement that summarizes a vast number of experimental observations. ...

The Scientific Method

Chemistry is an empirical science. Scientists often pose questions to understand the chemistry in everyday life and seek answers to these questions. To ...

Classifying Matter by State

Chemistry is the study of matter and the changes it undergoes. Matter is anything that has mass and occupies space. Matter is all around us; the air, ...

Classifying Matter by Composition

Matter: Pure Substances and Mixtures
According to its composition, the matter can be classified into two broad categories &mdash; pure substances and ...

The Atomic Theory of Matter

The earliest recorded discussion of the basic structure of matter comes from ancient Greek philosophers. Leucippus and Democritus argued that all matter ...

Subatomic Particles

Dalton was only partially correct about the particles that make up matter. All matter is composed of atoms, and atoms are composed of three smaller ...

Elements: Chemical Symbols and Isotopes

A chemical symbol is an abbreviation used to indicate an element or an atom of an element. For example, the symbol for mercury is Hg. The same symbol is ...

Use models to explain how the scientific understanding of atomic structure has evolved.

PS.Chm.1.1

Radioactivity and Nuclear Equations

Nuclear chemistry is the study of reactions that involve changes in nuclear structure. The nucleus of an atom is composed of protons and, except for ...

Types of Radioactivity

The most common types of radioactivity are &#945; decay, &#946; decay, &#947; decay, neutron emission, and electron capture.
Alpha (&#945;) decay is the ...

Nuclear Stability

Protons and neutrons, collectively called nucleons, are packed together tightly in a nucleus. With a radius of about 10&#8722;15 meters, a nucleus is ...

Nuclear Binding Energy

The difference between the calculated and experimentally measured masses is known as the mass defect of the atom. In the case of helium-4, the mass defect ...

Radioactive Decay and Radiometric Dating

Radioactivity is a spontaneous disintegration of an unstable nuclide and is a random process, as all the nuclei in the sample do not decay simultaneously. ...

Nuclear Fission

Many heavier elements with smaller binding energies per nucleon can decompose into more stable elements that have intermediate mass numbers and larger ...

Nuclear Power

Controlled nuclear fission reactions are used to generate electricity. Any nuclear reactor that produces power via the fission of uranium or plutonium by ...

Nuclear Fusion

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 ...

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

Analyze the structure of atoms and isotopes.

Ionic Compounds and Crystal Lattices

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