Category: Chemical Bonds: Covalent Bonding and Shape of Molecules

• sp Hybridization: Covalent Bonds Course (20)

  

  Feeling lost with sp hybridization? We break down sp hybridization in an easy-to-understand way. Get ready to learn: The basics of sp hybridization. How to identify sp hybridized atoms in molecules. Plus, links at the end to the sp3 and sp2 hybridizations. Don’t forget to like and subscribe for more chemistry adventures!

• sp2 Hybridization: Covalent Bonds Course (19)

  

  sp2 hybridization occurs between one s orbital and two p orbitals. We say “2” indicating the number of involved p orbitals.

• sp3 Hybridization: Covalent Bonds (18)

  

  Sp3 hybridization involves the mixing of one s orbital and three p orbitals to form four equivalent hybrid orbitals.

• Molecular Orbital (MO) Theory: Covalent Bonds (17)

  

  Molecular orbitals describe the distribution of electrons in molecules according to quantum mechanics. They are formed by the overlap of atomic orbitals. These orbitals, such as sigma and pi orbitals, determine a molecule’s stability, reactivity, and overall chemical behavior in various chemical reactions.

• Wave Function and Shape of Atomic Orbitals: Covalent Bonds (16)

  

  The probability of finding electrons is equal to the square of the wave function (ψ²). Where wave function (Ψ) defines the energy of an electron in an atom and the region of space it may occupy (orbitals)

• Exercises on Bond Dipole Moment (µ): Chemical Bonds (15)

  

  Exploring Exercises on Bond Dipole Moment (µ) provides a deeper understanding of molecular polarity.

• Bond Dipole Moment (µ): Chemical Bonds (14)

  

  The dipole moment is a measure of molecular polarity which happens due to uneven electron distributions in covalent bonds. It helps predict molecular behavior, solubility, and reactivity during different chemical interaction

• The Effect of the Presence of Lone Pairs on Bond Angle (Chemical Bonds: 13)

  

  The presence of lone pairs in a molecule can significantly influence its shape compared to bonding pairs. The lone pairs push other atoms further apart. This makes bond angles bigger or smaller than normal. Molecules with lone pairs may bend more or less than we expect. Their shapes are different than if there were just…

• Bond Angles and Shapes of Molecules (Chemical Bonds: 12)

  

  We can predict bond angles and the shape of a molecule based on valence bonds and lone pairs. Lone pairs, exerting maximum repulsion, contrast bonding pairs with minimum repulsion.

• Exception to Octet Rule (Chemical Bonds: 11)

  

  The octet rule states that atoms tend to form bonds in such a way that they have eight electrons in their outer shell. However, there are some exceptions to this rule. For example, molecules can have an odd number of electrons, or central atoms can have more than eight electrons if they have d orbitals…

• How to Calculate Formal Charge (Covalent bonding: 10)

  

  Formal charge is a concept used in chemistry to assess the distribution of electrons within a molecule or ion.

• The Lewis Structures For Molecules And Polyatomic Ions (Chemical Bonds: 9)

  

  The Lewis structure for molecules and polatomic ions.

• The Types of Chemical Bonds (Chemical Bonds: 8)

  

  Ionic and polar and non-polar covalent bonds are formed based on the differences in electronegativity between atoms. Ionic bonds occur when the electronegativity difference exceeds 1.9, resulting in electron transfer. Polar covalent bonds form when the difference is between 0.5 and 1.9, while non-polar covalent bonds occur when the difference is below 0.5.

• Exploring Electronegativity and Electron Affinity (Chemical bonds: 7)

  

  Electronegativity measures an element’s ability to attract electrons. It increases as we move from left to right and up in the periodic table due to the decreasing of atomic radius. Electron affinity, which is the energy released when an electron is added to an atom, increases as the atomic radius decreases.

• The Octet Rule and Chemical Bonds (6)

  

  The octet rule is a basic rule of chemistry that explains how valence electrons behave in chemical reactions.

• Lewis Structure (Chemical Bonds 5)

  

  In chemistry, our primary focus is on valence electrons, those electrons residing in the outermost shells of atoms. Those electrons are the ones that interact during a chemical reaction; they are gained, lost, or shared during a chemical reaction.

• Writing Electron Configurations (Chemical Bonds 4)

  

  Electron configurations, a fundamental aspect of atomic structure, reveal how electrons are distributed within atoms. This knowledge serves as the cornerstone of elements chemistry and atomic interactions ⚛️📊🧪

• Quantum Numbers: Describing Electrons (Chemical Bonds 3)

  

  Quantum numbers are a set of four mathematical values that describe the unique characteristics and properties of electrons within an atom. We use quantum numbers to learn about the arrangement, energy, position, and spin of electrons in the atom.

• Atomic Structure and Atomic Shells (Chemical Bonds 2)

  

  Join me as we navigate the electron maze and gain insight into the fundamental organization of matter at the atomic level.

• Chemical Bonds: Covalent Bonding and Shape of Molecules (Course Overview)

  The course discusses the concept of covalent bonding and the shape of molecules. It begins by explaining the basic principles of covalent bonding, such as the sharing of electrons and the formation of electron pairs. The course then discusses the VSEPR theory, which can be used to predict the shape of molecules. Finally, the course…