Atomic Hook-Ups - Types of Chemical Bonds: Crash Course Chemistry #22

CrashCourse
16 Jul 201309:45
EducationalLearning
32 Likes 10 Comments

TLDRThis video explores the different types of chemical bonds that form between atoms and ions. It explains that atoms bond to achieve a lower energy state. Covalent bonds involve the sharing of electrons, either equally in nonpolar bonds or unequally in polar bonds. Ionic bonds form through the complete transfer of electrons from metal atoms to nonmetal atoms, resulting in charged ions that strongly attract. The summary describes how bond length, electronegativity, and polarity relate to bond type. It notes key differences in properties between ionic and covalent compounds based on their polarity.

Takeaways
  • 😀 Chemical bonds form between atoms to minimize the overall energy and achieve a balance between attractive and repulsive forces.
  • 👥 The distance between two bonded atoms at which the energy is lowest is called the bond length.
  • 💑 A covalent bond involves sharing electrons between two atoms.
  • ❤️ Nonpolar covalent bonds form between identical atoms that share electrons equally.
  • 💔 Polar covalent bonds form between different atoms that share electrons unequally.
  • 🔌 Ionic bonds form between a metal and nonmetal by complete transfer of electrons.
  • ⚗️ Coulomb's law calculates the energy in ionic bonds using the charges and distance between ions.
  • 🌡 Ionic compounds tend to form crystals while covalent compounds are often softer substances.
  • 💧 Ionic compounds dissolve in water but covalent compounds often don't.
  • ⚡ Dissolved ionic compounds conduct electricity but covalent compounds usually don't.
Q & A

  • Why do atoms bond with each other?

    -Atoms bond with each other in order to reach their lowest energy state by achieving a balance between attractive and repulsive forces.

  • What is a covalent bond?

    -A covalent bond is a chemical bond formed by the sharing of one or more electron pairs between two atoms. The atoms are held together because the electron pair is attracted by the nuclei of both atoms.

  • What is the difference between a polar and non-polar covalent bond?

    -In a non-polar covalent bond, the electrons are shared equally between the atoms. In a polar covalent bond, the electrons are shared unequally, resulting in slightly positive and negative charged areas on the atoms.

  • What is an ionic bond?

    -An ionic bond is a chemical bond formed between two ions with opposite charges. One atom transfers one or more outer shell electrons to another atom, resulting in positive and negative ions which attract.

  • How can you calculate the energy in an ionic bond?

    -The energy in an ionic bond can be calculated using Coulomb's law. The formula calculates the product of the charges on the ions divided by the distance between them.

  • Why are properties of ionic and covalent compounds different?

    -Ionic compounds form crystalline solids that are often water soluble. Covalent compounds form softer solids, liquids or gases that are often not water soluble. This stems from differences in their molecular polarity.

  • What is bond length?

    -Bond length is the ideal distance between two bonded nuclei where the attractive and repulsive forces between them are balanced resulting in minimum energy.

  • Why is water such an important molecule?

    -Water is such an important molecule because it has polar covalent bonds. The uneven sharing of electrons makes one end of the molecule slightly positive and the other slightly negative.

  • What causes the separation of charges in a polar bond?

    -The separation of charges in a polar bond is caused by the difference in electronegativity between the two atoms. The more electronegative atom pulls the shared electrons closer.

  • How are chemical bonds similar to human relationships?

    -The video uses an analogy between human relationships and chemical bonds in terms of factors like distance, attraction, stresses and energy levels. Both seek to minimize energy/stress and find an optimal balance.

Outlines
00:00
👨‍🔬 The Basics of Chemical Bonds

This paragraph introduces chemical bonds, explaining how atoms form bonds to reduce their overall energy and achieve stability. It discusses how atoms balance attractive and repulsive forces to settle at an ideal distance called the bond length. This introductory section also covers how shared electrons in covalent bonds occupy the space between two nuclei.

05:00
🧲 The Three Main Types of Chemical Bonds

This paragraph differentiates between the three main types of chemical bonds: non-polar covalent, polar covalent, and ionic. It explains how electronegativity differences determine bond polarity in covalent bonds. The paragraph also notes how metals readily form cations that bond ionically with anions from non-metals.

Mindmap
Keywords
💡chemical bond
A chemical bond is a lasting attraction between atoms, ions or molecules that enables the formation of chemical compounds. Chemical bonds are discussed extensively in the video as they determine why atoms form relationships with each other. For example, the video states that 'atoms do whatever they can to reduce their overall energy, and they reach their lowest energy by achieving a balance between attractive and repulsive forces, being neither too clingy nor too aloof.' This balance of forces leads to chemical bonding.
💡covalent bond
A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms. Covalent bonding occurs between two non-metal atoms. As explained in the video, 'when one atom is attracted to another, just like Edward Cullen and Bella in chemistry class..., it gets stressed out by the attractive force and tries to relieve the stress by getting closer.' This mutual sharing of electrons is called a covalent bond.
💡ionic bond
An ionic bond is a chemical bond formed through an electrostatic attraction between two oppositely charged ions. As stated in the video, 'when positive ions come across negative ions...they are attracted to each other, which means energy is required to keep them apart, which means that they're gonna bond if they can, creating that oh-so-wonderful point of minimum energy.' Ionic bonds form between a metal and a nonmetal.
💡polarity
Polarity refers to the separation of electric charge leading to a molecule having an electric dipole. Polar molecules have a net separation of charge. As explained in the video, 'when the electrons hang out closer to one side of the bond, it creates a slight negative charge in that area and a slight positive charge around the other atom. This separation of charges is called polarity.'
💡electronegativity
Electronegativity refers to the tendency of an atom to attract shared electrons in a covalent bond. The video explains that 'The strength with which an atom holds shared electrons is called its electronegativity.' Atoms with high electronegativities form more polar bonds.
💡bond length
Bond length refers to the distance between the nuclei of two bonded atoms at their minimum energy. As stated in the video, 'This ideal, wonderful distance is the bond length. It's the distance between two nuclei at the point of minimum energy.' The bond length represents the optimal distance between two bonded atoms.
💡Coulomb's law
Coulomb's law is used to calculate the electrostatic force between two charged particles. As explained in the video, 'we can calculate the amount of energy that exists in a bond between ions at a given distance using a formula called Coulomb's law.' Coulomb's law mathematically describes the interaction between ions.
💡crystalline solid
A crystalline solid is a type of solid material whose constituents (atoms, molecules, or ions) are arranged in an orderly repeating pattern. As stated in the video, ionic compounds 'are often crystalline in their solid form because of the way the ions pack together.' The structure of crystalline solids is an important chemical property.
💡solubility
Solubility refers to the ability of a given substance to dissolve in a solvent to form a solution. The video compares the solubility of ionic and covalent compounds, stating that ionic compounds 'are generally soluble in water' while 'covalent compounds...often are not soluble in water.'
💡electrical conductivity
Electrical conductivity is the ability of a material to conduct electric current. The video explains that 'ionic solutions allow the solution to conduct electricity' while covalent solutions generally do not conduct electricity. A material's conductivity depends on its molecular structure.
Highlights

First significant research finding

Introduction of new theoretical model

Description of innovative methodology

Key conclusions and practical applications

Transcripts

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