Podcast
Questions and Answers
Ionic bonds are formed between two atoms that share one or more pairs of electrons.
Ionic bonds are formed between two atoms that share one or more pairs of electrons.
False
Covalent bonds are typically polar.
Covalent bonds are typically polar.
True
Hydrogen bonds are a type of intermolecular force.
Hydrogen bonds are a type of intermolecular force.
True
VSEPR theory predicts the shape of molecules based on the arrangement of electron pairs around the central atom.
VSEPR theory predicts the shape of molecules based on the arrangement of electron pairs around the central atom.
Signup and view all the answers
Bond length is the energy required to break a bond.
Bond length is the energy required to break a bond.
Signup and view all the answers
Pi bonds occur when orbitals overlap end-to-end.
Pi bonds occur when orbitals overlap end-to-end.
Signup and view all the answers
Study Notes
Types of Chemical Bonds
-
Ionic Bond: formed between two atoms that have a large difference in electronegativity, resulting in the transfer of electrons
- One atom loses an electron (becomes a cation) and the other atom gains an electron (becomes an anion)
- Electrostatic attraction between oppositely charged ions holds them together
-
Covalent Bond: formed between two atoms that share one or more pairs of electrons
- Atoms share electrons to achieve a full outer energy level
- Can be polar or nonpolar depending on the difference in electronegativity between atoms
-
Hydrogen Bond: a type of intermolecular force that arises between molecules with a hydrogen atom bonded to a highly electronegative atom (e.g. oxygen, nitrogen, or fluorine)
- Weak electrostatic attraction between the hydrogen atom and another electronegative atom
Bonding Theories
- Electrostatic Theory: explains the formation of ionic bonds based on the electrostatic attraction between oppositely charged ions
- Valence Shell Electron Pair Repulsion (VSEPR) Theory: predicts the shape of molecules based on the arrangement of electron pairs around the central atom
- Molecular Orbital (MO) Theory: explains the formation of covalent bonds in terms of the overlap of atomic orbitals to form molecular orbitals
Bond Characteristics
- Bond Length: the average distance between the nuclei of two bonded atoms
- Bond Angle: the angle between two bonded atoms and the central atom
- Bond Strength: the energy required to break a bond
- Polarity: the distribution of electrons within a bond, resulting in a partial positive and partial negative charge
Bonding in Molecules
- Sigma (σ) Bond: a type of covalent bond that occurs when orbitals overlap end-to-end
- Pi (π) Bond: a type of covalent bond that occurs when orbitals overlap side-by-side
- Multiple Bonds: bonds that involve more than one pair of electrons between two atoms, resulting in a stronger bond
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
Description
Learn about the different types of chemical bonds, bonding theories, and characteristics of bonds in molecules. Understand the formation of ionic, covalent, and hydrogen bonds, and how they affect molecular structure.
