2.2 Intramolecular Force and Potential Energy

• What are intramolecular forces?

  Attractive forces within molecules
• Order the following types of intramolecular forces by strength (from strongest to weakest):

  1️⃣ Covalent bond

  2️⃣ Ionic bond

  3️⃣ Metallic bond
• Ionic bonds are directional.

  False
• What is the relationship between intramolecular forces and potential energy?

  Stronger forces lower potential energy
• Ionic bonds involve the transfer of electrons
• Stronger intramolecular forces result in lower potential energy.
• Covalent bonds occur when atoms share electrons.
• Ionic bonds create oppositely charged ions that attract each other.
• The potential energy of a compound depends on the strength and arrangement of its intramolecular forces
• Covalent bonds occur when atoms share electrons
• Order the following factors based on their effect on intramolecular force strength:

  1️⃣ Electronegativity Difference

  2️⃣ Bond Polarity

  3️⃣ Bond Length

  4️⃣ Bond Angle
• Potential energy is the energy stored within a compound due to intramolecular forces and the position of its atoms.


  True
• In which type of bond are electrons delocalized across a lattice of metal ions?

  Metallic bond
• Greater electronegativity differences lead to more ionic character
• What is potential energy stored within a compound influenced by?

  Intramolecular forces
• Intramolecular forces are the attractive forces that hold atoms together within a molecule
• The strength of intramolecular forces is influenced by electronegativity difference, bond polarity, bond length, and bond angle
• Van der Waals forces involve minimal attraction and repulsion at close range
• Compounds with stronger intramolecular forces have lower potential energy
• Covalent bonds occur when atoms share electrons
• Metallic bonds feature delocalized electrons
• Match the type of intramolecular force with its example:

  Covalent bond ↔️ H₂O, CH₄

  Ionic bond ↔️ NaCl, MgO

  Metallic bond ↔️ Cu, Fe
• What is the key characteristic of metallic bonds?

  Delocalized electrons
• What is an example of a compound with ionic bonds?

  NaCl
• Covalent bonds are formed by the transfer of electrons.

  False
• What are metallic bonds characterized by in metals?

  Delocalized electrons
• Which type of bond is found in copper (Cu)?

  Metallic bond
• Ionic bonds are non-directional because the electrostatic attraction is uniform in all directions.

  True
• What happens to the strength of covalent bonds when bond length decreases?

  Increases
• What is the primary characteristic of covalent bonds?

  Sharing of electrons
• Polar bonds with unequal electron sharing result in stronger dipole-dipole interactions
• Match the factor with its effect on intramolecular force strength:

  Electronegativity Difference ↔️ Increased ionic character

  Bond Polarity ↔️ Stronger dipole-dipole interactions

  Bond Length ↔️ Stronger covalent and metallic bonds

  Bond Angle ↔️ Stronger covalent bonds at optimal angles
• Covalent bonds have higher potential energy compared to ionic bonds.


  True
• What type of intramolecular force is present in sodium chloride (NaCl)?

  Ionic bonds
• What is the equilibrium bond length in a potential energy diagram?

  Lowest potential energy
• What type of intramolecular forces are present in water (H₂O)?

  Covalent bonds
• Covalent bonds are directional.


  True
• Ionic bonds are stronger than covalent bonds.

  False
• Why are ionic bonds considered non-directional?

  Electrons are transferred
• Metallic bonds are directional.

  False