Name: drawing lewis structures with valence electron counts
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 2 min 54 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

lewis-structures-of-molecular-compounds-and-polyatomic-ions

Lewis Structures of Molecular Compounds and Polyatomic Ions

Lewis-Strukturen sind vereinfachte Darstellungen von chemischen Bindungen zwischen Atomen. Das Schreiben von Lewis-Strukturen für neutrale Verbindungen wie Ethen oder für mehratomige Ionen wie Hydronium oder Phosphat umfasst die folgende Abfolge von Schritten. Zuerst wird die Gesamtzahl der Valenzelektronen im Molekül berechnet.Nehmen wir zum Beispiel Ethen. Jedes Kohlenstoffatom hat 4 Valenzelektronen, und jedes Wasserstoffatom hat 1 Valenzelektron;mit 2 Kohlenstoff-und 4 Wasserstoffatomen, hat Ethen insgesamt 12 Valenzelektronen. Zeichnen Sie als nächstes die Skelettstruktur des Moleküls auf.Im Allgemeinen wird das erste Atom in der chemischen Formel oder das weniger elektronegative Atom zentral angeordnet. Dieses Atom wird auch als Zentralatom bezeichnet und muss in der Lage sein, mindestens zwei Bindungen zu bilden. Wasserstoffatome oder mehr elektronegative Atome sind außen um das Zentralatom angeordnet.Hier besetzen die Kohlenstoffatome die zentralen Positionen und sind mit Wasserstoffatomen umgebenden. Der nächste Schritt ist die Vervollständigung des Oktettes. Platzieren Sie zunächst ein Elektronenpaar zwischen jeweils zwei Atomen, um Bindungspaare darzustellen.Die restlichen Elektronen werden als Einzelpaare auf terminale und zentrale Atome verteilt, um die Duett-oder Oktett-Konfigurationen zu erfüllen. Da in diesem Fall Wasserstoff ein Duett erreicht hat, werden die restlichen Elektronen auf die Kohlenstoffatome übertragen. Verwenden Sie nun die einzelnen Paare, um Mehrfachbindungen zwischen Atomen zu bilden, denen ein Oktett fehlt.Bei Ethen haben die Kohlenstoffatome noch kein Oktett erreicht. Daher wird das einsame Paar in den Bindungsbereich bewegt, um eine Doppelbindung zu bilden, die es allen Atomen ermöglicht, eine stabile Elektronenkonfiguration zu erreichen. Um die Lewis-Struktur für geladene polyatomare Ionen wie Hydronium oder Phosphat zu schreiben, wird der gleiche Ansatz verfolgt, mit einer Modifikation um die Ionenladung mit einzubeziehen.Um die Lewis-Struktur des Hydroniums zu zeichnen, berechnen Sie zunächst die Anzahl der Valenzelektronen des Ions. Da das Hydroniumion eine positive Ladung hat, entfernen Sie ein Elektron von den Gesamtvalenzelektronen und reduzieren Sie die Anzahl auf 8. Als nächstes veranschaulichen Sie das Molekül anhand seiner Skelettstruktur.Platzieren Sie nun ein Elektronenpaar zwischen jedem Atom, gefolgt von dem einzelnen Elektronenpaar des Zentralatoms. Auf diese Weise erfüllen die Wasserstoff-und Sauerstoffatome das Duett bzw. das Oktett.Zum Schluss schreiben Sie die Lewis-Struktur in Klammern mit einer positiven Ladung in der rechten oberen Ecke.

lewis-strukturen molekularer verbindungen und mehratomiger ionen

Um Lewis-Strukturen für komplizierte Moleküle und Molekülionen zu zeichnen, ist es hilfreich, dem folgenden schrittweisen Verfahren zu folgen: <ol> <li>Bestimmen Sie die Gesamtzahl der Valenzelektronen (äußere Schale). Bei Kationen subtrahieren Sie ein Elektron für jede positive Ladung. Fügen Sie bei Anionen für jede negative Ladung ein Elektron hinzu.</li> <li>Zeichnen Sie eine Skelettstruktur des Moleküls oder Ions und ordnen Sie die Atome um ein Zentralatom an. (Im Allgemeinen sollte das am wenigsten elektronegative Element in der Mitte platziert werden.) Verbinden Sie jedes Atom mit dem Zentralatom über eine Einfachbindung (ein Elektronenpaar).</li> <li>Verteilen Sie die verbleibenden Elektronen als freie Elektronenpaare auf die terminalen Atome (außer Wasserstoff) und bilden Sie so ein Oktett um jedes Atom.</li> <li>Platzieren Sie alle verbleibenden Elektronen auf dem Zentralatom.</li> <li>Ordnen Sie die Elektronen der äußeren Atome neu an, um Mehrfachbindungen mit dem Zentralatom einzugehen und so, wo immer möglich, Oktette zu erhalten.</li> </ol> Betrachten Sie beispielsweise SiH4, CHO2–, NO+ und OF2 als Beispiele, für die diese allgemeine Richtlinie zur Bestimmung ihrer Lewis-Strukturen angewendet werden kann. <ol> <li>Bestimmen Sie die Gesamtzahl der Valenzelektronen (Außenhülle) im Molekül oder Ion. </li> </ol> Für ein Molekül wie SiH4 wird die Anzahl der Valenzelektronen an jedem Atom im Molekül addiert:  = [4 Valenz e−/Si-Atom × 1 Si-Atom] + [ 1 Valenz e−/H-Atom × 4 H-Atome] = 8 Valenz e− <h4>CHO2–</h4> Bei einem negativen Ion wie CHO2– wird die Anzahl der Valenzelektronen auf den Atomen zur Anzahl der negativen Ladungen auf dem Ion addiert (für jede einzelne negative Ladung wird ein Elektron gewonnen): = [4 Valenz e−/C-Atom × 1 C-Atom] + [1 Valenz e−/H-Atom × 1 H-Atom] + [6 Valenz e−/O-Atom × 2 O-Atome] + [1 zusätzliches e−] = 18 Valenz e− <h4>NO+</h4> Bei einem positiven Ion wie NO+ wird die Anzahl der Valenzelektronen der Atome im Ion addiert und anschließend die Anzahl der positiven Ladungen des Ions (für jede einzelne positive Ladung geht ein Elektron verloren) von der Gesamtzahl der Valenzelektronen subtrahiert: = [5 Valenz e−/N-Atom × 1 N-Atom] + [6 Valenz e−/O-Atom × 1 O-Atom] + [−1 e−] = 10 Valenz e− <h4>OF2 </h4> Da OF2 ein neutrales Molekül ist, wird die Anzahl der Valenzelektronen einfach addiert: = [6 Valenz e−/O-Atom × 1 O-Atom] + [7 Valenz e−/F-Atom × 2 F-Atome] = 20 Valenz e− <ol start="2"> <li>Zeichnen Sie eine Skelettstruktur des Moleküls oder Ions, ordnen Sie die Atome um ein Zentralatom an und verbinden Sie jedes Atom mit dem Zentralatom durch eine einzelne Bindung (ein Elektronenpaar). (Beachten Sie, dass Ionen durch Klammern um die Struktur gekennzeichnet sind und die Ionenladung außerhalb der Klammern steht:) <img alt="Figure1" src="https://www.jove.com/files/core/CDNSource/lessons/1063/1063Image_1.svg" style="height: 80px;"> In Fällen, in denen mehrere Anordnungen von Atomen möglich sind, wie bei CHO2−, werden experimentelle Beweise verwendet, um die richtige Form auszuwählen. Im Allgemeinen handelt es sich bei den weniger elektronegativen Elementen eher um Zentralatome. In CHO2− nimmt das weniger elektronegative Kohlenstoffatom die zentrale Position zwischen den es umgebenden Sauerstoff- und Wasserstoffatomen ein. Weitere Beispiele sind P in POCl3, S in SO2 und Cl in ClO4−. Eine Ausnahme ist, dass Wasserstoff fast nie ein Zentralatom ist. Als elektronegativstes Element kann auch Fluor kein Zentralatom sein.</li> <li>Verteilen Sie die verbleibenden Elektronen als freie Elektronenpaare auf die terminalen Atome (außer Wasserstoff), um deren Valenzschalen mit einem Elektronenoktett zu vervollständigen. (Da auf SiH4 keine Elektronen mehr vorhanden sind, bleibt seine Struktur unverändert.) <img alt="Figure2" src="https://www.jove.com/files/core/CDNSource/lessons/1063/1063image_2.svg" style="height: 80px;"></li> <li>Platzieren Sie alle verbleibenden Elektronen auf dem Zentralatom.  <ul> <li>Für SiH4, CHO2− und NO+ gibt es keine verbleibenden Elektronen. Für OF2 werden von den 16 verbleibenden Elektronen 12 platziert, sodass 4 Elektronen übrig bleiben, die auf dem Zentralatom platziert werden müssen: <img alt="Figure3" src="https://www.jove.com/files/core/CDNSource/lessons/1063/1063Image_3.svg" style="height: 40px;"></li> </ul> </li> <li>Ordnen Sie die Elektronen der äußeren Atome neu an, um Mehrfachbindungen mit dem Zentralatom einzugehen und wo immer möglich Oktette zu erhalten.  <ul> <li>SiH4: Si hat bereits ein Oktett, daher muss nichts getan werden.  <img alt="Figure4" src="https://www.jove.com/files/core/CDNSource/lessons/1063/1063Image_4.svg" style="height: 70px;"></li> <li>CHO2−: Die Valenzelektronen sind als freie Elektronenpaare auf den Sauerstoffatomen verteilt, dem Kohlenstoffatom fehlt jedoch ein Oktett.  <img alt="Figure5" src="https://www.jove.com/files/core/CDNSource/lessons/1063/1063Image_5.svg" style="height: 80px;"></li> <li>Daher wird ein einzelnes Elektronenpaar von einem der Sauerstoffatome an das Kohlenstoffatom abgegeben und bildet eine Doppelbindung. Abhängig davon, welches Sauerstoffatom die Elektronen gespendet hat, kann es zwei mögliche Strukturen geben, auch Resonanzstrukturen genannt. </li> <li>NO+: Für dieses Ion werden acht Valenzelektronen hinzugefügt, aber keines der Atome hat ein Oktett. Es können keine weiteren Elektronen hinzugefügt werden, da die gesamten Elektronen bereits aufgebraucht sind. In diesem Szenario müssen Elektronen bewegt werden, um Mehrfachbindungen zu bilden. Das Stickstoffatom hat zwei freie Elektronenpaare und das Sauerstoffatom eines.  <img alt="Figure6" src="https://www.jove.com/files/core/CDNSource/lessons/1063/1063Image_6.svg" style="height: 55px;"></li> <li>Dadurch entsteht immer noch kein Oktett, daher muss ein weiteres Paar verschoben werden, um eine Dreifachbindung zu bilden.  <img alt="Figure7" src="https://www.jove.com/files/core/CDNSource/lessons/1063/1063Image_7.svg" style="height: 50px;"></li> <li>In OF2 ändert sich nichts, da jedes Atom bereits ein Oktett hat. <img alt="Figure8" src="https://www.jove.com/files/core/CDNSource/lessons/1063/1063Image_8.svg" style="height: 40px;"></li> </ul> </li> </ol> Dieser Text wurde adaptiert von <a href="https://openstax.org/books/chemistry-2e/pages/7-3-lewis-symbols-and-structures">Openstax, Chemistry 2e, Section 7.3: Lewis Symbols and Structures.</a>

Lewis-Strukturen molekularer Verbindungen und mehratomiger Ionen

Um Lewis-Strukturen für komplizierte Moleküle und molekulare Ionen zu zeichnen, ist es hilfreich, ein Schritt-für-Schritt-Verfahren zu befolgen, wie beschrieben:

Bestimmen Sie die ...

Education

Lehre

JoVE Core

Chemie

Eins

Chemical Bonding: Basic Concepts

Chemische Bindungen: Grundkonzepte

KEY TERMS AND CONCEPTS

KERNBEGRIFFE UND KONZEPTE

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

drawing-lewis-structures-with-valence-electron-counts

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 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...

trends in lattice energy: ion size and charge

trends-in-lattice-energy-ion-size-and-charge

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

bond-polarity-dipole-moment-and-percent-ionic-character

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

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

Some covalent molecules do not follow the octet rule in their Lewis structures. Their central atoms can fall into three groups: odd-electron molecules, electron-deficient molecules, and hypervalent molecules. These cases show why a Lewis structure may not always give every atom eight valence electrons. Odd-electron molecules have an odd number of valence electrons, so one electron remains unpaired. Molecules with an odd number of electrons are called radicals. Nitric oxide, NO, is one example,...

bond energies and bond lengths

How Bond Energy Predicts Reaction Heat

Bond energy helps explain why molecules stay together and how much heat a reaction may release or absorb. A covalent bond is stronger when more energy is needed to separate the atoms. The energy needed to break one specific covalent bond in one mole of gaseous molecules is called bond energy, or bond dissociation energy. For a diatomic molecule, bond energy is the standard enthalpy change for an endothermic reaction that breaks that bond. The H-H bond is a common example. Its bond energy is...

bonding in metals

Electron Sea Model in Metals

Electron sea model explains how metallic bonding holds metals together. In this model, most metal atoms do not have enough valence electrons to form ionic or covalent bonds in the usual way. Their valence electrons are held loosely because metals have low electronegativity, and their ionization energy is low, so electrons are removed easily. When a metal atom loses these outer electrons, it becomes a positively charged metal ion. The freed electrons form a delocalized electron cloud around...

key terms and concepts

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

chemistry

JoVE Core Chemie erweckt allgemeine Konzepte der Chemie durch kompakte und leicht verständliche animierte Videolektionen zum Leben. Außerdem zeigen wir in den Videos Wissenschaftler in Aktion bei klassischen und neuartigen Forschungsexperimenten, wie sie heutzutage in Laboren weltweit durchgeführt wurden.

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

Physical Science

Study Of Matter

Bonding and compounds

Structure And Properties Of Matter

Chemical bonding

Representing compounds

Tennessee Academic Standards

High School

Matter and Its Interactions

CHEM1.PS1.12

CHEM1.PS1.14

Virginia  Standards of Learning

HIgh School

CH.3

CH.3.d

Physics

PH.9

PH.9.e

Arizona Science Standards

HS.P1

HS.P1U1.2

Texas Essential Knowledge and Skills

CHEM.6

CHEM.6.E

Alabama Course of Study Science

motion-and-stability-forces-and-interactions

Motion and Stability: Forces and Interactions

9-12.C.2.2.a

9-12.C.2.2.c

Chemistry and Physics

IPC.7

IPC.7.A

new-york-state-science-learning-standards

New York State Science Learning Standards

HS. Structure and Properties of Matter

HS-PS1-3.

HS. Chemical Reactions

HS-PS1-2.

HS-PS1-4.

HS-PS1-12.

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 ...

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 ...

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

Analyze the structure of atoms and isotopes.

Drawing Lewis Structures with Valence Electron Counts

Description

Transcript

Tags

More videos by Standards