2.1.2 Chemical bonding

• What is the main purpose of chemical bonding?

  To form stable compounds
• Covalent bonds involve the sharing of electrons between atoms.


  True
• An example of a compound formed by ionic bonding is NaCl
• What does chemical bonding achieve for atoms?

  Stability
• Ionic bonds create positive and negative ions that are electrostatically attracted
• Metallic bonds provide strong electrical conductivity due to a sea of delocalized electrons.


  True
• What type of bond is formed by a sea of delocalized electrons surrounding positive metal ions?

  Metallic bond
• Why do metallic bonds allow for electrical conductivity?

  Sea of delocalized electrons
• What are the oppositely charged ions in ionic bonding electrostatically attracted to?

  Each other
• What is the structure of a metallic bond described as?

  Sea of delocalized electrons
• Metallic bonding provides strong electrical conductivity in metallic substances.


  True
• What kind of ions are created in ionic bonding?

  Positive and negative
• Covalent bonds allow atoms to achieve a stable electron configuration.


  True
• Ionic bonding creates positive and negative ions that are electrostatically attracted to each other.
• Why do ionic compounds have high melting and boiling points?

  Strong electrostatic forces
• Arrange the types of covalent bonds by the number of electron pairs shared:

  1️⃣ Single bond (1 pair)

  2️⃣ Double bond (2 pairs)

  3️⃣ Triple bond (3 pairs)
• What is an example of a molecule with four single covalent bonds?

  Methane (CH₄)
• What is the structure formed by positive metal ions in metallic bonding called?

  Metallic lattice
• Chemical bonding is the attraction between atoms that enables them to form stable compounds and molecules.
• What are the three main types of chemical bonds?

  Ionic, covalent, metallic
• What is the key difference between covalent and ionic bonding?

  Electron sharing vs. transfer
• Covalent bonding occurs when atoms share electrons to achieve a stable electron configuration.
• A single covalent bond involves the sharing of one pair of electrons.
• How many single covalent bonds are in methane (CH₄)?

  Four
• Covalent compounds are excellent conductors of electricity.

  False
• Metallic bonding involves a sea of delocalized electrons surrounding positive metal ions.
• Metals are ductile because their electron cloud is flexible.


  True
• Ionic bonds have high melting and boiling points due to strong electrostatic forces.
• Arrange the bond types in order of decreasing electrical conductivity.

  1️⃣ Metallic

  2️⃣ Ionic (when dissolved)

  3️⃣ Covalent
• Copper (Cu) has a high melting point and excellent electrical conductivity due to metallic bonding.

  True
• Ionic bonds form when electrons are transferred
• What surrounds positive metal ions in metallic bonds?

  Sea of electrons
• Arrange the bond types in order of increasing electrical conductivity:

  1️⃣ Covalent

  2️⃣ Ionic

  3️⃣ Metallic
• Why do atoms share electrons in covalent bonds?

  To achieve stable configuration
• In covalent bonds, atoms share electrons to achieve a stable electron configuration
• Metallic bonds provide strong electrical conductivity in metallic substances.


  True
• Match the bond type with its example:

  Ionic ↔️ NaCl

  Covalent ↔️ CH₄

  Metallic ↔️ Cu
• Ionic bonding results in high melting and boiling points due to strong electrostatic forces.


  True
• Ionic bonds are formed by the transfer of electrons from one atom to another.
• How are covalent bonds formed?

  Sharing of electrons