Podcast Beta
Questions and Answers
Resonance structures represent the actual electronic structure of a molecule, which is often a hybrid of the contributing ______
structures
Sigma bonds are the strongest type of bond that represents the 'glue' that holds the atoms together. They are the most ______ type of bond
strongest
Pi bonds in double bonds or triple bonds can move without destroying the connectivity and are denoted as ______ bonds
pi
Unshared electron pairs or lone pairs represent the most mobile type of ______
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Electrons move towards areas of lower electron density and away from ______ charges
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Bond energy calculates how strong the bond is, representing the energy required to break a covalent bond. It is measured in joules or kilocalories per ______
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Metallic bonds have a ______ distance typically SHORTER THAN IONIC BONDS
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Electronegativity is the atom's ability to attract other shared electrons in a ______
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Non-polar Covalent bonds occur between ______
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Polar Covalent Bonds occur between ______ atoms
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Ionic Bonds occur between ______ and non-metal ions
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In Ionic bonds, it results in ______
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Study Notes
Resonance
- Represents the actual electronic structure of a molecule, often a hybrid of contributing resonance structures.
Sigma Bonds
- The strongest type of bond, holding atoms together.
- Represent the "glue" that holds atoms together.
Pi Bonds
- Found in double bonds or triple bonds and can move without destroying connectivity.
Unshared Electron Pairs (Lone Pairs)
- Represent the most mobile type of electrons.
Electron Mobility
- Order of electron mobility: Unshared electron pairs (lone pairs) > pi-bonds > sigma bonds.
- Electrons move towards areas of lower electron density and away from negative charges.
Chemical Bonding
- Bond distance (bond length) refers to the spatial arrangement of atoms and is measured in picometers.
Bond Energy
- Calculates the strength of a bond, representing the energy required to break a covalent bond.
- Measured in joules or kilocalories per mole.
- Tends to increase from single to double to triple bonds.
- Higher bond energy indicates a stronger bond.
Bond Relationships
- Shorter bond distance = higher bond energy.
- Longer bond distance = lower bond energy (with exceptions due to variations in atomic properties and bond types).
Covalent Bonds
- Strongest and used as a basis in all organic molecules.
- Bond distance is usually short, indicating a close interaction between atoms.
Ionic Bonds
- Atoms gain and lose electrons later on.
- Bond distance is usually large, indicating a greater distance between atoms.
Metallic Bonds
- Bond distance varies, but is typically shorter than ionic bonds.
Electronegativity
- Ability of an atom to attract shared electrons in a bond.
- Used to predict the polarity of a bond.
Non-polar Covalent Bonds
- Occurs between non-metals.
- Electronegativity difference between atoms is very small (< 0.5).
- Equal or almost equal sharing of electrons between bonding atoms.
- Example: Cl-Br bond.
Polar Covalent Bonds
- Occurs between non-metal atoms.
- Electronegativity difference between atoms is moderate (> 0.5).
- Unequal sharing of electrons between bonding atoms.
- Example: Cl-C bond.
Dipole and Bond Polarity
- Dipole is the separation of charges in a polar bond.
Ionic Bonds
- Occurs between metal and non-metal ions.
- Results in electron transfer.
- Electronegativity difference between atoms is high (> 1.8).
- Example: N-Na bond.
Electron Bonding
- Non-polar Covalent: Electrons are equally shared.
- Polar Covalent: Electrons are shared unequally.
- Ionic: Electrons are transferred.
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Description
Learn about how resonance structures are used to represent the electronic structure of molecules and understand the concept of electron mobility in different types of bonds. Explore sigma bonds, pi bonds, and unshared electron pairs in this quiz.
