Name: chemical bonds: types and strength
Uploaded: 2023-04-30T18:28:31.000Z
Duration: 2 min 40 s
Channel: JoVE

K12 Standards

Louisiana Student Standards for Science

High School

Chemistry

Matter And Its Interactions

HS-PS1-1

Chemical Bonds

כאשר אטומים מתקרבים זה לזה, גרעיניהם דוחים זה את זה, וכך גם האלקטרונים. במקביל, האלקטרונים מכל אטום נמשכים זה לגרעין של זה ומסודרים כך שימקסם את הכוחות המושכים בין האטומים תוך מזעור כוחות הדחייה.
אם התוצאה היא כוח אטרקטיבי נטו, האנרגיה הפוטנציאלית של המערכת יורדת. אינטראקציה זו נקראת קשר כימי.
עם זאת, לא כל שילוב של אטומים יכול ליצור קשרים כימיים יציבים. ההתנהגות הכימית של אטום נקבעת בעיקר על ידי מה יוצר קשרים ואיזה סוג של קשרים הם. הבנת הקשר בין אטומים שיוצרים תרכובת מסייעת להבין ולחזות את ההתנהגות המולקולרית שלהם.
אנרגיית בונד היא האנרגיה הדרושה לשבירת קשר בשומה אחת של תרכובת גזית. זה תלוי בסוג האטומים הקשורים ובמספר האלקטרונים המעורבים. חוזק הקשר עולה עם אנרגיית האג"ח.
סוג האטומים הקשורים ומספר האלקטרונים המעורבים משפיעים גם הם על אורך הקשר, שהוא המרחק הממוצע בין גרעינים של שני אטומים קשורים והוא ביחס הפוך לריבוי הקשר וחוזק הקשר.
אינטראקציות הקשר הנפוצות ביותר משתרעות על ספקטרום הנע בין קשרים יוניים, הכוללים משיכה אלקטרוסטטית בין יונים טעונים מנוגדים, לקשרים קוולנטים, החולקים אלקטרונים ערכיים בין אטומים.
קשר יוני הוא האינטראקציה העיקרית המצויה בתרכובות יוניות. הקטיונים והאניונים המרכיבים מוחזקים יחד על ידי כוחות משיכה אלקטרוסטטיים. לעתים קרובות, היווצרות היונים קודמת להעברת אלקטרונים ערכיים בין האטומים המשתתפים.
האטום שמאבד אלקטרונים הופך לקטיון, ואילו האטום שמקבל אלקטרונים הופך לאניון. העברת אלקטרונים בדרך כלל נותנת לכל יון את תצורת הגז האציל הקרובה ביותר, שהיא התצורה שאליה מגיעים עם השינוי הקטן ביותר במספר האלקטרונים, מה שהופך את היונים ליציבים יותר מבחינה אנרגטית.
בקשר קוולנטי, האלקטרונים המשותפים מתקשרים עם גרעיני אטומי הקשר ומפחיתים את האנרגיה הפוטנציאלית. קשרים כפולים ומשולשים חולקים שניים ושלושה זוגות אלקטרונים בין אטומים, בהתאמה. ככל שזה מגדיל את מספר האלקטרונים הנתונים לכוחות משיכה נוספים מהגרעין השני, חוזק הקשר גדל עם ריבוי הקשרים.

קשרים כימיים

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 אטומים משתתפים ביצירת קשר כימי כדי לרכוש קונפיגורציית אלקטרונים ערכיות-קליפה דומה לזו של הגז האציל הקרוב אליו במספר האטומי. קשרים יוניים, קוולנטיים ומתכתיים הם חלק מהסוגים החשובים של קשרים כימיים. אנרגיית הקשר ואורך הקשר קובעים את חוזק הקשר הכימי.
 
 
 סוגי קשרים כימיים
 
 
 קשר יוני נוצר עקב משיכה אלקטרוסטטית בין קטיונים לאניונים. לעתים קרובות, היונים נוצרים על ידי העברת אלקטרונים מאטום משתתף אחד לשני. עם זאת, לקשרים אלה אין כיווניות מוגדרת מכיוון שכוח המשיכה האלקטרוסטטי מופץ באופן אחיד בכל המרחב התלת ממדי.
 
 
 קשר קוולנטי הוא קשר כימי שנוצר על ידי שיתוף של זוגות אלקטרונים בין אטומים סמוכים. זוג האלקטרונים המשותף נקרא זוג אלקטרונים קושרים. קשרים קוולנטיים הם בעלי אופי כיווני.
 
 
 קשר מתכתי נוצר בין שני אטומי מתכת. קשר מתכתי מתואר על ידי "מודל ים האלקטרונים". בהתבסס על אנרגיות היינון הנמוכות של מתכות, המודל קובע כי אטומי מתכת מאבדים בקלות את אלקטרוני הערכיות שלהם והופכים לקטיונים. אלקטרוני ערכיות אלה יוצרים מאגר של אלקטרונים delocalized המקיפים את הקטיונים על פני המתכת כולה.
 
 
 אנרגיות קשר ואורך קשר
 
 
 חוזקו של קשר קוולנטי נמדד באנרגיה הנדרשת כדי לשבור אותו - כלומר, האנרגיה הדרושה להפרדת האטומים המחוברים. הפרדת כל זוג של אטומים קשורים דורשת אנרגיה. ככל שהקשר חזק יותר, האנרגיה הדרושה כדי לשבור אותו גדולה יותר.
 
 
 האנרגיה הנדרשת כדי לשבור קשר קוולנטי ספציפי מול אחת של מולקולות גזיות נקראת אנרגיית הקשר או אנרגיית פירוק הקשר. אנרגיית הקשר של מולקולה דו-אטומית מוגדרת כשינוי האנתלפיה הסטנדרטי עבור התגובה האנדותרמית. למולקולות עם שלושה אטומים או יותר יש שני קשרים או יותר. סכום כל אנרגיות הקשר במולקולה כזו שווה לשינוי האנתלפיה הסטנדרטי לתגובה האנדותרמית שמפרקת את כל הקשרים במולקולה.
 
 
 חוזק הקשר בין שני אטומים גדל ככל שמספר זוגות האלקטרונים בקשר גדל. ככלל, ככל שמספר הקשרים בין שני אטומים גדול יותר, כך אורך הקשר קצר יותר וחוזק הקשר גדול יותר. לפיכך, קשרים משולשים חזקים וקצרים יותר מקשרים כפולים בין אותם שני אטומים; כמו כן, קשרים כפולים חזקים וקצרים יותר מקשרים בודדים בין אותם שני אטומים. כאשר אטום אחד נקשר לאטומים שונים בקבוצה, חוזק הקשר יורד בדרך כלל ככל שאנו נעים למטה בקבוצה.
 
 
 הטקסט הזה מותאם מ <a href="https://openstax.org/books/chemistry-2e/pages/7-1-ionic-bonding">Openstax, Chemistry 2e, Section 7.1: Ionic Bonding</a>, <a href="https://openstax.org/books/chemistry-2e/pages/7-2-covalent-bonding">Openstax, Section 7.2: Covalent Bonding</a>, <a href="https://openstax.org/books/chemistry-2e/pages/10-5-the-solid-state-of-matter">Section 10.5: The Solid State of Matter</a>, and Section<a href="https://openstax.org/books/chemistry-2e/pages/7-5-strengths-of-ionic-and-covalent-bonds"> 7.5. Bond Strength: Covalent Bonds</a>.
 
 
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אטומים משתתפים בהיווצרות קשר כימי כדי לרכוש תצורת אלקטרונים מעטפת ערכיות מלאה הדומה לזו של הגז האציל הקרוב ביותר ...

Education

JoVE Core

Organic Chemistry

כימיה אורגנית

Unit 1

יחידה 1

Covalent Bonding and Structure

קשרים קוולנטיים ומבנה

KEY TERMS AND CONCEPTS

מונחים ומושגים מרכזיים

chemical bonds: types and strength

Chemical bonds help atoms reach a full valence shell like the nearest noble gas. The main bond types are ionic, covalent, and metallic. Bond energy and bond length also help explain how strong a bond is.

An ionic bond forms from electrostatic attraction between cations and anions. In many cases, one atom transfers electrons to another atom, and the ions form from that transfer. Ionic bonds have no defined direction because the attraction spreads evenly through three-dimensional space.

A covalent bond forms when adjacent atoms share electron pairs. The shared pair is called the bonding pair. Covalent bonds are directional, so the atoms are linked in a specific orientation.

A metallic bond forms between two metal atoms. The electron sea model describes this type of bonding. In this model, metal atoms lose valence electrons easily and become cations, while the delocalized electrons form a pool around the cations across the metal.

The strength of a covalent bond is measured by the energy needed to break it and separate the bonded atoms. Stronger bonds require more energy. For one mole of gaseous molecules, this value is called bond energy, or bond dissociation energy. For a diatomic molecule, it is the standard enthalpy change for the endothermic reaction that breaks the bond.

Molecules with three or more atoms have more than one bond. In those cases, the total bond energy is the sum of all bond energies needed to break every bond in the molecule. Bond strength also increases as the number of electron pairs in the bond increases. Triple bonds are stronger and shorter than double bonds between the same atoms, and double bonds are stronger and shorter than single bonds. When one atom bonds to different atoms in a group, bond strength usually decreases as you move down the group.

Chemical Bonds: Types and Strength

what is organic chemistry?

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Organic chemistry focuses on carbon compounds called organic compounds. These compounds may come from living things or be made by chemists. Carbon is the main element in them, and it bonds with other carbon atoms as well as hydrogen, oxygen, nitrogen, and sulfur. Carbon can form up to four strong bonds. That ability lets carbon atoms build chains and rings of many sizes, shapes, and levels of complexity. Not every carbon-containing substance is classified as organic. Carbonates, cyanides, and...

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Atomic Orbitals and Quantum Numbers

Atomic orbitals and quantum numbers describe how electrons are arranged around the nucleus. An atom has a small, positively charged nucleus with electrons surrounding it. The nucleus contains protons and neutrons, and the quantum mechanical model gives a better picture of this structure than older models. Protons carry a +1 charge and have a mass of 1.0073 amu. Neutrons have no charge and have a mass of 1.0087 amu. Electrons carry a −1 charge and have a mass of 0.00055 amu. The number of...

electron configurations

How Electrons Fill Atomic Orbitals

Electron filling in atoms follows a set order based on orbital energy. The Aufbau principle says each new electron enters the lowest-energy subshell available. The Pauli exclusion principle says no two electrons can share the same set of four quantum numbers. Hund’s rule of maximum multiplicity says electrons stay unpaired in equal-energy orbitals when possible. The order of filling follows the relative energies of the subshells. A common sequence is 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, and so on.

chemical bonds

Chemical bonds help atoms reach a full valence shell like the nearest noble gas. The main bond types are ionic, covalent, and metallic. Bond energy and bond length also help explain how strong a bond is. An ionic bond forms from electrostatic attraction between cations and anions. In many cases, one atom transfers electrons to another atom, and the ions form from that transfer. Ionic bonds have no defined direction because the attraction spreads evenly through three-dimensional space. A...

polar covalent bonds

Electronegativity in Polar Covalent Bonds

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Lewis Structures, Bonds, and Formal Charge

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vsepr theory

Molecular Shapes from Electron Pairs

Molecular shape can be predicted from the way electron pairs arrange around a central atom. Valence shell electron-pair repulsion theory, or VSEPR theory, uses a Lewis structure to count bonding pairs and lone electron pairs. The main idea is simple: electron pairs spread out as far as possible to reduce repulsion. In a molecule, the valence electrons around the central atom can be bonding pairs or lone pairs. Bonding pairs are found mainly between bonded atoms. Lone pairs stay on one atom and...

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Predicting Shape and Molecular Polarity

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resonance and hybrid structures

Resonance in Nitrite and Carbonate Ions

Resonance explains why some Lewis structures do not match the measured properties of a molecule or ion. When two or more Lewis structures have the same atom arrangement, the real electron distribution is an average of the structures shown. The nitrite anion, NO2−, is one example. It can be drawn in two ways, with the N–O and N=O bonds in different places. If nitrite had one single bond and one double bond, the two bond lengths should be different, because a double bond is shorter and stronger...

valence bond theory and hybridized orbitals

valence-bond-theory-and-hybridized-orbitals

Covalent Bond Overlap and Orbital Hybridization

Covalent bonds form when orbitals on two atoms overlap and their single electrons pair up. The bond is stronger when the overlap is greater. Maximum overlap happens when the orbitals meet along a direct line between the two nuclei. A sigma bond, or σ bond, is the kind of covalent bond found in a single bond in a Lewis structure. In a σ bond, electron density is concentrated along the internuclear axis. A pi bond, or π bond, forms when two p orbitals overlap side by side. In a π bond, the...

mo theory and covalent bonding

Bond Order and Molecular Orbitals

Molecular orbital theory explains how electrons are arranged in molecules. It treats electron regions in a molecule much like atomic orbitals in an atom. A molecular orbital is the region of space where a valence electron is most likely to be found. Molecular orbitals form through the linear combination of atomic orbitals, or LCAO. When atomic wave functions combine in phase, they create regions with high electron density. When they combine out of phase, they create nodes, or regions with no...

intermolecular forces and physical properties

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How Intermolecular Forces Affect Matter

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solubility

Why Some Substances Dissolve in Water

Solution formation depends on how solutes and solvents interact. A solution is a homogeneous mixture made of a solvent, which is the larger part, and a solute, which is the smaller part. The physical state of a solution is usually the same as the solvent. Concentration is often described as dilute for a low amount of solute or concentrated for a high amount of solute. When a solute dissolves, its particles are surrounded by solvent species. This process is called solvation. If water is the...

introduction to functional groups

Functional Groups and Organic Molecules

Functional groups are groups of atoms with specific chemical properties that appear within organic molecules. They are sometimes shown as "R." These groups sit along the carbon backbone of macromolecules, which can form chains or rings of carbon atoms. Functional groups help functionalize a compound. That means they can give the molecule different physical and chemical properties. In organic chemistry, this change in group structure can strongly affect how a compound behaves. Common...

overview of advanced functional groups

Advanced Functional Groups in Organic Chemistry

Advanced functional groups are atom clusters in organic molecules that give those molecules specific chemical properties. They are sometimes shown as "R" in formulas. By changing the atoms attached to a carbon skeleton, a functional group can make a compound behave differently in physical and chemical reactions. This topic covers several major classes of organic compounds with advanced functional groups. Aromatic hydrocarbons include benzene. Phenol is another example and is also called...

key terms and concepts

Explore ionic, covalent, and metallic bonds, plus bond energy and bond length. Learn how bond type affects strength in high school chemistry.

Chemical Bonds: Types and Strength | JoVE K12

organic chemistry

JoVE Core Organic Chemistry explains basic concepts of stereochemistry, reactions, and mechanisms using concise and easy-to-understand animated video lessons. Additionally, the scientist-in-action videos demonstrate the application of related concepts in classical and original research experiments performed in today's laboratories worldwide.

HS-PS1-3

motion-and-stability-forces-and-interactions

Motion And Stability: Forces And Interactions

HS-PS2-6

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

9-12

Physical Geology

Minerals

Chemical bonding (ionic, covalent, metallic)

Tennessee Academic Standards

Motion and Stability: Forces and Interactions

CHEM1.PS2.1

Virginia  Standards of Learning

HIgh School

Physics

PH.9

PH.9.e

Minnesota Academic Standards in Science

1.1.1 9L.4.2.1.1

3.1.1 9C.2.2.1.2

south-carolina-college-and-career-ready-science-standards

South Carolina College and Career Ready Science Standards

Matter and Its Interactions

C-PS1-3.

C-PS2-6.

The Periodic Table

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Periodic Classification of the Elements

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the-periodic-table-and-organismal-elements

The Periodic Table And Organismal Elements

Atomic Structure

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Electron Configurations

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Electronic Structure of Atoms


An atom comprises protons and neutrons, which are contained inside the dense, central&#160;core called the nucleus, with electrons present around the ...

electron-configuration-of-multielectron-atoms

Electron Configuration of Multielectron Atoms

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Atomic Radii and Effective Nuclear Charge

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The Aufbau Principle and Hund's Rule

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Coulomb's Law

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Electric Charges

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Sources and Properties of Electric Charge

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Types of Forces

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Electric Fields

Source: Yong P. Chen, PhD, Department of Physics &#38; Astronomy, College of Science, Purdue University, West Lafayette, IN
An electric field is generated ...

Intermolecular Forces

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

Van der Waals Interactions

Atoms and molecules interact with each other through intermolecular forces. These electrostatic forces arise from attractive or repulsive interactions ...


Atoms participate in a chemical bond formation&#160;to acquire a completed valence-shell electron configuration similar to that of the noble gas nearest ...

Electron Behavior

Electrons are negatively charged subatomic particles attracted to and orbit around the positively-charged nucleus of an atom. They reside in spaces ...

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 ...

Ions and Ionic Charges

In ordinary chemical reactions, the nucleus &mdash; which contains the protons and neutrons of each atom and thus identifies the element &mdash; remains ...

Use the periodic table as a model to predict the relative properties of elements based on the patterns of electrons in the outermost energy level and the composition of the nucleus of atoms.  Clarification Statement: Chemistry: Examples of properties that could be predicted from patterns could include reactivity of metals, types of bonds formed, numbers of bonds formed, atomic radius, atomic mass, or reactions with oxygen. Emphasis is on main group elements and qualitative understanding of the relative trends of ionization energy and electronegativity.

Properties of Transition Metals

Transition metals are defined as those elements that have partially filled d orbitals. As shown in Figure 1, the d-block elements in groups 3&#8211;12 are ...

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 ...

Chemical Reactions

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Chemical Equations

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Introduction to Chemical Reactions

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Temperature Dependence on Reaction Rate

The Collision Theory
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stoichiometry-product-yield-and-limiting-reactants

Stoichiometry, Product Yield, and Limiting Reactants

Source: Smaa Koraym at Johns Hopkins University, MD, USA

	Preparation of 25% v/v Ethylenediamine in Deionized WaterExpand
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physical-and-chemical-properties-of-matter

Physical and Chemical Properties of Matter

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Physical Properties of Matter

A physical property is ...

Dynamic Equilibrium

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Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties.  Clarification Statement: Chemistry: Examples of chemical reactions could include the reaction of sodium and chlorine, carbon and oxygen, or carbon and hydrogen. Reaction classification aids in the prediction of products (e.g. synthesis, decomposition, single displacement, double displacement, and acid-base).

HS-PS1-2

Intermolecular vs Intramolecular Forces

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comparison-between-electrical-and-gravitational-forces

Comparison Between Electrical And Gravitational Forces

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Intermolecular Forces and Physical Properties



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

electric-field-of-two-equal-and-opposite-charges

Electric Field of Two Equal and Opposite Charges

Atoms generally contain the same number of positively and negatively charged particles, protons, and electrons. Hence, they are electrically neutral. ...

Electric Field

Consider two point charges, each exerting Coulomb force on the other. It is possible to describe the Coulomb interaction via an intermediate step by ...

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 ...

Electric Dipoles and Dipole Moment

Consider two charges of equal magnitude but opposite signs. If they cannot be separated by an external electric field, the system is called a permanent ...

Plan and conduct an investigation to gather evidence to compare the structure of substances at the macroscale to infer the strength of electrical forces between particles.  Clarification Statement: Emphasis is on understanding the strengths of forces between particles, not on naming specific intermolecular forces (such as dipole-dipole). Examples of particles could include ions, atoms, molecules, and network solids (such as graphite). Examples of macro-properties of substances could include the melting point and boiling point, vapor pressure, and surface tension.

bond-dissociation-energy-and-activation-energy

Bond Dissociation Energy and Activation Energy

Bond energy is the energy required to break a bond homolytically. These values are usually expressed in units of kcal/mol or kJ/mol and are referred to as ...

Bond Energies and Bond Lengths

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

Coupled Reactions

Cellular processes such as building and breaking down complex molecules occur through stepwise chemical reactions. Some of these chemical reactions are ...

energy-diagrams-transition-states-and-intermediates

Energy Diagrams, Transition States, and Intermediates

Free-energy diagrams, or reaction coordinate diagrams, are graphs showing the energy changes that occur during a chemical reaction. The reaction ...

What is Metabolism?

Overview

Metabolism represents all of the chemical activity in a cell, including reactions that build molecules (anabolism) and those that break ...

types-of-chemical-reactions-anabolic-and-catabolic

Types of Chemical Reactions: Anabolic and Catabolic

The first law of thermodynamics holds that energy can neither be created nor destroyed&#8212;it can only change form. An organism&#39;s essential function ...

Non-equilibrium in the Cell

An important concept in studying metabolism and energy is that of chemical equilibrium. Most chemical reactions are reversible. They can proceed in both ...

Develop a model to illustrate that the release or absorption of energy from a chemical reaction system depends upon the changes in total bond energy.  Clarification Statement: Emphasis is on the idea that a chemical reaction is a system that affects the energy change.  Examples of models could include molecular-level drawings and diagrams of reactions, graphs showing the relative energies of reactants and products, and representations showing energy is conserved.

HS-PS1-4

Chemical Bonds: Types and Strength

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