1.3 Chemical Bonding

• What is chemical bonding defined as?

  Electrostatic attraction between atoms
• Why do ionic compounds have high melting and boiling points?

  Strong electrostatic forces
• Metallic bonding allows metals to be ductile and malleable
• There are three main types of chemical bonds that hold atoms together
• Ionic bonds form when electrons are shared between atoms.

  False
• Ionic compounds have low melting and boiling points due to strong electrostatic forces.

  False
• Match the type of covalent bond with the number of electron pairs shared.

  Single ↔️ 1

  Double ↔️ 2

  Triple ↔️ 3
• What is the key feature of metallic bonding?

  Free movement of electrons
• Covalent bonds form molecules with strong bonds by sharing electrons.


  True
• What type of bond involves the sharing of electrons to achieve a stable electron configuration?

  Covalent
• Steps involved in ionic bonding:

  1️⃣ Metal atom loses electrons to become a cation

  2️⃣ Nonmetal atom gains electrons to become an anion

  3️⃣ Electrostatic attraction forms between ions

  4️⃣ An ionic compound is formed
• What is the "sea" of electrons in metallic bonding called?

  Delocalized electrons
• What is chemical bonding defined as?

  Electrostatic attraction between atoms
• What is the key characteristic of metallic bonds?

  Delocalization of electrons
• What is a positively charged ion called?

  Cation
• Covalent bonds allow atoms to achieve a full outer shell of electrons.

  True
• Metallic bonding results in high electrical and thermal conductivity.

  True
• Ionic bonds involve electrostatic attraction between oppositely charged ions.
• Match the bond type with its solubility in water.

  Ionic ↔️ Often soluble

  Covalent ↔️ Depends on polarity

  Metallic ↔️ Insoluble
• There are three main types of chemical bonds: ionic, covalent, and metallic
• Metallic bonds involve delocalized electrons that are free to move throughout the metal lattice
• Covalent bonding occurs when atoms share electrons to achieve a stable electron configuration
• What is the fundamental force responsible for chemical bonding?

  Electrostatic attraction
• What is the key feature of ionic bonds?

  Electrostatic attraction between ions
• Metallic bonds allow for high electrical conductivity due to delocalized electrons.


  True
• Ionic compounds conduct electricity in their molten or aqueous state.
• In water (H₂O), each oxygen atom shares electrons with two hydrogen atoms.
• What property of metallic bonds makes metals ductile and malleable?

  Delocalized electrons
• Ionic bonds form when atoms share electrons.

  False
• Match the bond type with its key feature:

  Ionic ↔️ Electrostatic attraction between ions

  Covalent ↔️ Stable electron configuration

  Metallic ↔️ Free movement of electrons
• A double covalent bond involves the sharing of two electron pairs.


  True
• Match the bond type with its formation and key feature:

  Ionic ↔️ Electron transfer, electrostatic attraction

  Covalent ↔️ Sharing of electrons, stable configuration

  Metallic ↔️ Delocalization of electrons, free movement
• Covalent bonds involve the sharing of electrons
• Ionic bonding creates positive and negative ions held together by strong electrostatic attraction.
• What type of bonding involves the sharing of electrons between two nonmetal atoms?

  Covalent bonding
• What is the "sea" of electrons in metallic bonding called?

  Electron sea
• Match the bond type with its formation mechanism.

  Metallic ↔️ Delocalization of electrons

  Ionic ↔️ Electron transfer

  Covalent ↔️ Sharing of electrons
• Ionic bonds have high melting and boiling points due to strong electrostatic forces.