Name: how ionic charge changes ion size
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 3 min 10 s
Channel: JoVE

K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.2.2

Ionic Radii

İyonik yarıçap, bir iyonik bileşikteki iyonlar arasındaki mesafe ile tanımlanan bir katyon veya bir anyonun yarıçapıdır. Katyonlar ana atomdan daha küçüktür, oysa anyonlar daha büyüktür. Atom yarıçaplarına benzer şekilde, iyonik yarıçaplar elektronların sayısı, değerlik elektronlarını tutan orbitaller ve nükleer yük ile belirlenir.Bir helyum çekirdeğinin elektron konfigürasyonuna ve en dıştaki 2s elektronuna sahip lityumu ele alalım. 2s elektronu çekirdek yükünden iki 1s elektron ile perdelenir ve 152 pikometrelik atom yarıçapını oluşturur. En dıştaki 2s elektronunun kaybı, daha az elektrona sahip ancak ana atomla aynı sayıda protona sahip bir lityum katyonu oluşturur.İki 1s elektronu çekirdeğe daha yakın tutulur çünkü 2s elektronundan daha büyük bir etkili çekirdek yüküne sahiptir. Dolayısıyla, lityum katyonunun iyonik yarıçapı, ana atomdan çok daha küçük olan 60 pikometredir. Bu eğilim genellikle tüm metal katyonlarında ve bunların ana atomlarında görülür.Buna karşılık, anyonlar ana atomlarından daha büyüktür. Bir flor atomu bir elektron aldığında, bu yeni elektron en dışa eklenir, ancak proton sayısı ve dolayısıyla çekirdek yükü aynı kalır. Artan elektron-elektron itmesi, elektronların uzayda daha fazla yayılmasına neden olur.Bu nedenle, florür anyonu, ana atomdan çok daha büyük olan 136 pikometrelik bir yarıçapa sahip olur. Genel olarak, s ve p-blok elementlerinin iyonik yarıçapı, ana enerji seviyelerinin sayısı ve dolayısıyla orbitallerin sayısı arttıkça, sütunda aşağı doğru artar. Peki ya aynı sayıda elektrona sahip bir grup atom ve iyon çapları nasıl değişir?Bunlar izoelektronik seri olarak adlandırılırlar ve atom numarası artırılarak düzenlenebilirler. Gösterilen izoelektronik serinin her bir üyesi 18 elektrona sahiptir. Bununla birlikte, proton sayısında farklılık gösterirler.Sülfür iyonunun 18 elektron çeken 16 protonu varken, kalsiyum iyonunun aynı sayıda elektronu çeken 20 protonu vardır. Böylece, daha fazla protonla kalsiyum elektronları çekirdeğe sülfittekinden çok daha yakına çekebilir ve bu da kalsiyum iyonunun sülfid iyonundan daha küçük olmasına neden olur. Çekirdek yükü ne kadar büyükse, yarıçap o kadar küçüktür, ancak bir elektron kabuğunun eklenmesi bu eğilimi bozar.Yine de, sülfür bu serideki en büyük iyon kalsiyum ise en küçük iyondur.

İyonik yarıçap

İyonik yarıçap, bir iyonun boyutunu tanımlamak için kullanılan ölçüdür. Bir katyon her zaman daha az elektrona ve nötr atomla aynı sayıda protona sahiptir; türetildiği atomdan daha küçüktür. Örneğin, bir alüminyum atomunun (1s22s22p63s23p1) kovalent yarıçapı 118 pm iken, bir Al+3'ün (1s22s22p6) iyonik yarıçapı 68 pm'dir. Elektronlar dış değerlik kabuğundan çıkarıldıkça, daha küçük kabukları işgal eden çekirdek elektronları daha büyük etkili nükleer yük Zeff etkisinde kalır ve çekirdeğe daha da yaklaşır.
 
 Daha büyük yüklü katyonlar, daha küçük yüklü katyonlardan daha küçüktür (örneğin, V+2 79 pm'lik bir iyonik yarıçapa sahipken, V+3'nınki 64 pm'dir). Periyodik tabloda gruplarda aşağı doğru ilerlerken, aynı yüke sahip ardışık elementlerin katyonları genellikle daha büyük yarıçaplara sahiptir ve bu, baş kuantum sayısındaki, n artışına karşılık gelir.
 
 Bir anyon (negatif iyon), bir atomun değerlik kabuğuna bir veya daha fazla elektronun eklenmesiyle oluşur. Bu, elektronlar arasında daha büyük bir itme ve elektron başına Zeff'te bir azalma ile sonuçlanır. Her iki etki de (artan elektron sayısı ve azalmış Zeff) bir anyonun yarıçapının nötr atomunkinden daha büyük olmasına neden olur. Örneğin, bir sülfür atomu ([Ne]3s23p4) 104 pm'lik bir kovalent yarıçapa sahipken, sülfid anyonunun iyonik yarıçapı ([Ne]3s23p6) 170 pm'dir. Herhangi bir grupta ilerleyen ardışık elementler için, anyonlar daha büyük baş kuantum numaralarına ve dolayısıyla daha büyük yarıçaplara sahiptir.
 
 Aynı elektron konfigürasyonuna sahip atom ve iyonların izoelektronik olduğu söylenir. İzoelektronik türlere örnek olarak N–3, O–2, F–, Ne, Na+, Mg+2 ve Al+3 (1s22s22p6) verilebilir. Diğer bir izoelektronik seri P–3, S–2, Cl–, Ar, K+, Ca+2 ve Sc+3 ([Ne]3s23p6)'dır. İzoelektronik olan atomlar veya iyonlar için proton sayısı boyutu belirler. Nükleer yük ne kadar büyükse, bir dizi izoelektronik iyon ve atomdaki yarıçap o kadar küçük olur.
 
 Bu metin bu kaynaktan uyarlanmıştır: <a href="https://openstax.org/books/chemistry-2e/pages/6-5-periodic-variations-in-element-properties">OpenStax Chemistry 2e, Section 6.5: Periodic Variations in Element Properties.</a>

İyonik Yarıçap

İyonik yarıçap, bir iyonun boyutunu tanımlamak için kullanılan ölçüdür. Bir katyon her zaman daha az elektrona ve ana atomla aynı sayıda protona sahiptir; o...

Education

JoVE Core

Kimya

Periodic Properties of the Elements

Elementlerin Periyodik Özellikleri

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

how ionic charge changes ion size

Ionic radius describes the size of an ion. It changes when an atom gains or loses electrons. Cations are positive ions with fewer electrons than the parent atom, and they are smaller than the atoms they come from.

Aluminum shows this pattern clearly. A neutral aluminum atom has a covalent radius of 118 pm, while Al3+ has an ionic radius of 68 pm. When electrons are removed from the outer valence shell, the remaining core electrons feel a stronger effective nuclear charge, or Zeff. That pull draws them closer to the nucleus.

Cations with larger charges are usually smaller than cations with smaller charges. For example, V2+ has an ionic radius of 79 pm, while V3+ is smaller at 64 pm. Moving down a group in the periodic table, cations with the same charge generally get larger. This happens because the principal quantum number, n, increases.

Anions are negative ions formed when one or more electrons are added to the valence shell. Extra electrons increase electron repulsion and reduce Zeff per electron. Both effects make an anion larger than its parent atom. Sulfur is an example: a sulfur atom has a covalent radius of 104 pm, while the sulfide anion has an ionic radius of 170 pm. Anions also tend to have larger radii down a group because n increases.

Atoms and ions with the same electron configuration are called isoelectronic. One example set is N3−, O2−, F−, Ne, Na+, Mg2+, and Al3+, which all have the same electron arrangement. Another is P3−, S2−, Cl−, Ar, K+, Ca2+, and Sc3+. In an isoelectronic series, the number of protons controls size. The greater the nuclear charge, the smaller the radius.

How Ionic Charge Changes Ion Size

periodic classification of the elements

How Valence Electrons Shape the Periodic Table

The periodic table organizes elements by increasing atomic number, and it also shows why elements in the same group behave alike. As the electron configurations are placed into the table, a repeating pattern appears in the outer shells of atoms. These outer electrons are called valence electrons, and they play the biggest role in chemical reactions. They are the highest-energy electrons in an atom, so they are easier to lose or share than core electrons. Valence electrons also help determine...

ionization energy

Ionization Energy Trends in the Periodic Table

Ionization energy is the energy needed to remove an electron from a gaseous atom or ion in its ground state. The first ionization energy, or IE1, removes the most loosely bound electron and forms a 1+ cation. The second ionization energy, IE2, removes the next electron, and each later ionization energy removes another electron from the atom or ion. Ionization always requires energy, so these processes are endothermic. That means ionization energy values are always positive. In general, larger...

atomic radii and effective nuclear charge

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Periodic Trends in Atomic Size

Periodic trends in atomic size help explain why atoms get larger or smaller across the periodic table. Elements in the same group show similar chemical behavior because they have the same number and arrangement of valence electrons. Across a period, each new element adds one proton to the nucleus and one electron to the valence shell. Down a group, the number of valence electrons stays the same, but the principal quantum number increases by one. Atomic radius is not easy to define with perfect...

ionic radii

Ionic radius describes the size of an ion. It changes when an atom gains or loses electrons. Cations are positive ions with fewer electrons than the parent atom, and they are smaller than the atoms they come from. Aluminum shows this pattern clearly. A neutral aluminum atom has a covalent radius of 118 pm, while Al3+ has an ionic radius of 68 pm. When electrons are removed from the outer valence shell, the remaining core electrons feel a stronger effective nuclear charge, or Zeff. That pull...

electron affinity

Electron Affinity Trends on the Periodic Table

Electron affinity is the energy change that happens when a gaseous atom gains an electron and becomes a negative ion, or anion. For many elements, this process releases energy, so the electron affinity value is negative. For some elements, energy must be added instead, so the value is positive. Electron affinity also applies when more than one electron is added. The second electron affinity is the energy change for adding an electron to an anion to make a 2− ion. Later electron affinities...

alkali metals

Alkali Metals: Reactivity Trends

Alkali metals are Group 1 elements with one valence electron. They are soft, shiny metallic solids that are malleable, ductile, and good conductors of heat and electricity. Their melting points are unusually low for metals and drop as you move down the group. Density generally increases down the group, except for potassium. The trend in atomic size helps explain their behavior. Moving from lithium to cesium, each element has a higher principal quantum number, so the outer electron is farther...

halogens

Halogens: Trends and Reactions

Halogens are Group 17 nonmetals that show clear trends in structure and reactivity. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid. Astatine is highly unstable and radioactive, so most of its properties are still unknown because it has a very short half-life. Tennessine is a synthetic element that is also predicted to belong to this group. These elements do not usually exist as single atoms. Instead, they form diatomic molecules, which means...

noble gases

Noble Gases: Sources, Uses, and Reactions

Noble gases are the group 18 elements helium, neon, argon, krypton, xenon, and radon. They were called “noble” because they were once thought to be nonreactive. That idea changed in 1962, when Dr. Neil Bartlett at the University of British Columbia showed that this assumption was not fully correct. These gases occur in very small amounts in the atmosphere. Some natural gas contains 1–2% helium by mass. Helium is separated from natural gas by removing the condensable components, which leaves...

key terms and concepts

Learn how cations and anions change size, why ionic radius varies with charge, and how isoelectronic species compare across the periodic table.

How Ionic Charge Changes Ion Size | JoVE K12

chemistry

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Physical Science

PS.PSc.1.6

Pennsylvania State Academic Standards

Chemical Reactions

3.2.9-12.C

Structure and Properties of Matter

3.2.9-12.A

Louisiana Student Standards for Science

High School

Matter And Its Interactions

HS-PS1-1

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Ohio’s Learning Standards and Model Curriculum

Study Of Matter

Periodic trends of the elements

Structure And Properties Of Matter

Periodic Table

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Matter and Its Interactions

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Arizona Science Standards

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Texas Essential Knowledge and Skills

CHEM.5

CHEM.5.A

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9-12.C.1.1

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Motion and Stability: Forces and Interactions

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New York State Science Learning Standards

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Georgia Standards of Excellence

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Periodic Table Trends

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Periodic Table Trends: Atomic Radii, Ionization, and Electronegativity

Scientific Laws and Theories

Scientific Laws

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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

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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

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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

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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 ...

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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

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 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.

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

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Ionic Bonding and Electron Transfer

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The Born-Haber Cycle

Lattice Energy&#xA0;

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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

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Electronegativity

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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 ...

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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 ...

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

PS.Chm.3.1

Analyze the structure of atoms and isotopes.

How Ionic Charge Changes Ion Size

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