Name: ionization energy trends in the periodic table
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 3 min 12 s
Channel: JoVE

K12 Standards

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

NC K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.2.2

Ionization Energy

Het chemische gedrag van atomen en ionen wordt sterk beïnvloed door hoe gemakkelijk of moeilijk het is om hun elektronen te verwijderen, vooral de buitenste elektronen die deelnemen aan chemische bindingsformaties. De energie die nodig is om een elektron uit een gasvormig atoom in zijn grondtoestand te verwijderen, wordt de eerste ionisatie-energie genoemd en wordt gegeven in kilojoules per mol. De energie die nodig is om het volgende elektron te verwijderen, wordt de tweede ionisatie-energie genoemd, enzovoort.Als we een kolom naar beneden gaan, nemen de ionisatie-energieën af. Bedenk dat het hoogste hoofdkwantumaantal valentie-elektronen naar beneden in de kolom toeneemt, wat leidt tot grotere atomaire afmetingen. Dus hoe verder de buitenste elektronen zijn, hoe gemakkelijker ze te verwijderen zijn.Voor elementen uit de hoofdgroep neemt de ionisatie-energie toe gedurende de periode. De reden ligt in het toenemende atoomnummer, waarbij valentie-elektronen een hogere effectieve nucleaire lading ervaren, waardoor het verwijderen van de buitenste elektronen moeilijker wordt. Dit verklaart waarom chloor een hogere ionisatie-energie heeft dan bijvoorbeeld natrium.Over het algemeen is ionisatie-energie een minimum voor een alkalimetaal en stijgt tot een piek bij elk edelgas. Overgangsmetalen vertonen een kleine toename van de ionisatie-energie gedurende de periode, en de f-blokelementen vertonen een nog kleinere verandering. Maar er zijn enkele uitzonderingen om te overwegen.Borium heeft een kleinere ionisatie-energie dan beryllium, ook al staat het verder naar rechts op het periodiek systeem. Beryllium heeft 2s-elektronen met een lagere energie, terwijl boor een 2p-elektron met hogere energie heeft, waardoor de verwijdering ervan energetisch gunstiger is. Een andere uitzondering is zuurstof, dat een lagere eerste ionisatie-energie heeft dan stikstof.In vergelijking met stikstof heeft zuurstof vier p-elektronen, en het verwijderen van één elektron elimineert de elektronen-elektronen-afstoting. Er is dus minder energie nodig voor de ionisatie. Deze uitzonderingen worden ook in volgende periodes in acht genomen.Het verwijderen van elektronen uit kationen is moeilijker dan uit neutrale atomen. Over het algemeen nemen de opeenvolgende ionisatie-energieën toe voor elementen. Denk aan kalium.De tweede ionisatie-energie is aanzienlijk hoger, omdat het de verwijdering van een kernelektron uit een ion met een edelgasconfiguratie inhoudt. Evenzo is er voor calcium een sterke toename van de tweede naar de derde ionisatie-energie als een kernelektron wordt verwijderd uit een kation met een edelgasconfiguratie.

ionisatie-energie

De hoeveelheid energie die nodig is om het meest losjes gebonden elektron uit een gasvormig atoom in zijn grondtoestand te verwijderen, wordt de eerste ionisatie-energie (IE1) genoemd. De eerste ionisatie-energie voor een element, X, is de energie die nodig is om een kation met 1+ lading te vormen: <img alt="Eq1" src="https://www.jove.com/files/core/CDNSource/lessons/1049/1049_Equations-01.png" style="height: 40px;"> De energie die nodig is om het op één na meest losjes gebonden elektron te verwijderen, wordt de tweede ionisatie-energie (IE2) genoemd. <img alt="Eq2" src="https://www.jove.com/files/core/CDNSource/lessons/1049/1049_Equations-02.png" style="height: 40px;"> De energie die nodig is om het derde elektron te verwijderen is de derde ionisatie-energie, enzovoort. Er is altijd energie nodig om elektronen uit atomen of ionen te verwijderen, dus ionisatieprocessen zijn endotherm en IE-waarden zijn altijd positief. Bij grotere atomen bevindt het meest losjes gebonden elektron zich verder van de atoomkern en is dus gemakkelijker te verwijderen. Dus naarmate de grootte (atoomstraal) toeneemt, zou de ionisatie-energie moeten afnemen.  Binnen een bepaalde periode neemt de IE1 over het algemeen toe met toenemende Z. In een groep lager neemt de IE1-waarde over het algemeen af met toenemende Z. Er zijn echter enkele systematische afwijkingen van deze trend. Merk op dat de ionisatie-energie van boor (atoomnummer 5) kleiner is dan die van beryllium (atoomnummer 4), ook al is de nucleaire lading van boor één proton groter. Dit kan worden verklaard omdat de energie van de subshells toeneemt naarmate l toeneemt, als gevolg van penetratie en afscherming. Binnen elke schil hebben de s-elektronen een lagere energie dan de p-elektronen. Dit betekent dat een s-elektron moeilijker uit een atoom te verwijderen is dan een p-elektron in dezelfde schil. Het elektron dat wordt verwijderd tijdens de ionisatie van beryllium ([He]2s2) is een s-elektron, terwijl het elektron dat wordt verwijderd tijdens de ionisatie van boor ([He]2s22p1) een p-elektron is; dit resulteert in een lagere eerste ionisatie-energie voor boor, ook al is de nucleaire lading één proton groter. We zien dus dat er telkens wanneer een nieuwe subshell begint een kleine afwijking van de voorspelde trend optreedt. Een andere afwijking treedt op als orbitalen voor meer dan de helft gevuld raken. De eerste ionisatie-energie voor zuurstof is iets minder dan die voor stikstof, ondanks de trend van stijgende IE1-waarden over een bepaalde periode. Voor zuurstof zal het verwijderen van één elektron de elektron-elektronenafstoting elimineren die wordt veroorzaakt door het paren van de elektronen in de 2p-orbitaal en resulteren in een halfgevulde orbitaal (wat energetisch gunstig is). Analoge veranderingen vinden plaats in opeenvolgende perioden. Het verwijderen van een elektron uit een kation is moeilijker dan het verwijderen van een elektron uit een neutraal atoom vanwege de grotere elektrostatische aantrekkingskracht op het kation. Op dezelfde manier is het verwijderen van een elektron uit een kation met een hogere positieve lading moeilijker dan het verwijderen van een elektron uit een ion met een lagere lading. Opeenvolgende ionisatie-energieën voor één element nemen dus altijd toe. Zoals te zien is in Tabel 1 is er een grote toename in de ionisatie-energieën voor elk element. Deze sprong komt overeen met het verwijderen van de kernelektronen, die moeilijker te verwijderen zijn dan de valentie-elektronen. Sc en Ga hebben bijvoorbeeld allebei drie valentie-elektronen, dus de snelle toename van de ionisatie-energie vindt plaats na de derde ionisatie. Tabel 1: Opeenvolgende ionisatie-energieën voor geselecteerde elementen (kJ/mol) <table style="margin-left: auto; margin-right: auto;"> <tbody style="border: 1px solid black;"> <tr> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">Element</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">IE1</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">IE2</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">IE3</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">IE4</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">IE5</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">IE6</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">IE7</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">K</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">418.8</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">3051.8</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">4419.6</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">5876.9</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">7975.5</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">9590.6</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">11343</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">Ca</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">589.8</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">1145.4</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">4912.4</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">6490.6</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">8153.0</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">10495.7</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">12272.9</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">Sc</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">633.1</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">1235.0</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">2388.7</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">7090.6</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">8842.9</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">10679.0</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">13315.0</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">Ga</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">578.8</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">1979.4</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">2964.6</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">6180</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">8298.7</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">10873.9</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">13594.8</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">Ge</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">762.2</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">1537.5</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">3302.1</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">4410.6</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">9021.4</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">Not available</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">Not available</td> </tr> <tr> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">As</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">944.5</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">1793.6</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">2735.5</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">4836.8</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">6042.9</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">12311.5</td> <td style="color: black; border: 1px solid black; text-align: center; padding: 10px; ">Not available</td> </tr> </tbody> </table> Dit tekst is aangepast van <a href="https://openstax.org/books/chemistry-2e/pages/6-5-periodic-variations-in-element-properties">OpenStax Chemistry 2e, Sectie 6.5: Periodieke variaties in elementeigenschappen.</a>

Ionisatie-energie

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 ...

Education

JoVE Core

Scheikunde

Eén

Periodic Properties of the Elements

Periodieke eigenschappen van de elementen

KEY TERMS AND CONCEPTS

BELANGRIJKE TERMEN EN CONCEPTEN

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 atoms have lower ionization energy because their outermost electrons are farther from the nucleus and easier to remove.

Across a period, first ionization energy generally increases as atomic number increases. Down a group, first ionization energy generally decreases as atomic number increases. The trend is useful, but there are some clear exceptions.

One exception appears when a new subshell begins. Boron has a lower first ionization energy than beryllium, even though boron has one more proton. This happens because s electrons are lower in energy than p electrons in the same shell, so the s electron in beryllium is harder to remove than the p electron in boron. The effect comes from penetration and shielding.

Another exception appears when a p subshell becomes more than half filled. Oxygen has a slightly lower first ionization energy than nitrogen. Removing one electron from oxygen reduces electron-electron repulsion in the 2p orbital and gives a more stable half-filled orbital.

Successive ionization energies always increase. It is harder to remove an electron from a cation than from a neutral atom because the positive charge pulls more strongly on the remaining electrons. It is even harder to remove an electron from a cation with a higher positive charge.

The large jump in successive ionization energies shows when core electrons begin to be removed. Core electrons are harder to remove than valence electrons. For example, scandium and gallium both have three valence electrons, so the sharp rise in ionization energy comes after the third ionization. The table of values for K, Ca, Sc, Ga, Ge, and As shows this pattern clearly.

Ionization Energy Trends in the Periodic Table

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 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

atomic-radii-and-effective-nuclear-charge

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

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...

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

Explore first and successive ionization energy, periodic trends, and key exceptions such as boron, oxygen, and the jump to core electrons.

Ionization Energy Trends in the Periodic Table | JoVE K12

chemistry

JoVE Core Chemistry brings general chemistry concepts to life using concise and easy-to-understand animated video lessons. Plus, in the scientist-in-action videos, we demonstrate classical and original research experiments performed in today's laboratories worldwide.

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

HS-PS1-2

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

Study Of Matter

Periodic trends of the elements

Structure And Properties Of Matter

Periodic Table

Tennessee Academic Standards

Matter and Its Interactions

CHEM1.PS1.12

Virginia  Standards of Learning

HIgh School

CH.2

CH.2.c

PS.2

PS.2.b

PS.4

PS.4.a

PS.4.b

Arizona Science Standards

HS.P1

HS.P1U1.1

HS+C.P1

HS+C.P1U1.1

new-jersey-student-learning-standards-for-science

New Jersey Student Learning Standards for Science

Texas Essential Knowledge and Skills

CHEM.5

CHEM.5.A

CHEM.5.C

CHEM.7

CHEM.7.A

Alabama Course of Study Science

9-12.C.1.1

9-12.C.1.1.e

motion-and-stability-forces-and-interactions

Motion and Stability: Forces and Interactions

9-12.C.2.2.f

9-12.PS.3.4.b

Next Generation Science Standards

Chemistry and Physics

IPC.7

IPC.7.B

new-york-state-science-learning-standards

New York State Science Learning Standards

HS. Structure and Properties of Matter

HS-PS1-1.

HS. Chemical Reactions

HS-PS1-2.

Georgia Standards of Excellence

SPS1.

Periodic Table Trends

SC1.

periodic-table-trends-atomic-radii-ionization-and-electronegativity

Periodic Table Trends: Atomic Radii, Ionization, and Electronegativity

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

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 ...

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

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

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, 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 ...

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.

Ionization Energy Trends in the Periodic Table

Description

Transcript

Tags

More videos by Standards