1.3 Chemical Bonding

• What are the three primary types of chemical bonds?

  Ionic, covalent, metallic
• Describe the sequence of electron behavior in covalent and ionic bonds.

  1️⃣ Atoms share electrons in covalent bonds

  2️⃣ Atoms transfer electrons in ionic bonds

  3️⃣ Ions with opposite charges are formed

  4️⃣ Electrostatic attraction holds ions together
• Ionic compounds have high melting points due to strong electrostatic forces.


  True
• Covalent compounds have low melting and boiling points due to weaker intermolecular forces
• Metallic bonding occurs between metal atoms, where the outer electrons are delocalized
• Chemical bonding refers to the attractive forces that hold atoms together to form molecules or compounds
• Chemical bonds result in a more stable arrangement of atoms because they achieve a lower energy state
• Atoms bond to achieve a stable electron configuration.

  True
• Metals typically lose electrons to form positively charged ions
• What happens to electrons in covalent bonding?

  They are shared
• Match the bonding type with its description:

  Ionic bonding ↔️ Electrostatic attraction between ions

  Covalent bonding ↔️ Sharing of electrons

  Metallic bonding ↔️ Sea of delocalized electrons
• Metallic compounds have high melting points.


  True
• The electrons in an atom's outer shell determine how atoms form chemical bonds
• Why do ionic compounds have high melting points?

  Strong electrostatic forces
• What allows metallic compounds to conduct electricity?

  Delocalized electrons
• Are covalent bonds stronger or weaker compared to ionic bonds?

  Weaker
• Order the following properties based on their relative strength in covalent vs. ionic bonding:

  1️⃣ Bond Strength: Ionic > Covalent

  2️⃣ Melting Point: Ionic > Covalent

  3️⃣ Electrical Conductivity: Ionic > Covalent
• Covalent bonds form when atoms share electrons
• What is the melting point of ionic compounds compared to covalent compounds?

  High
• In metallic bonding, valence electrons form a sea of electrons.
• Order the types of bonding based on their stability, from highest to lowest:

  1️⃣ Ionic

  2️⃣ Covalent

  3️⃣ Metallic
• What type of attraction holds ions together in ionic bonding?

  Electrostatic
• Polar covalent compounds dissolve in water, while nonpolar covalent compounds do not
• Covalent compounds are poor conductors of electricity because they lack free-moving ions.


  True
• Match the bonding type with its bond formation process:

  Covalent Bonding ↔️ Electron sharing

  Ionic Bonding ↔️ Electron transfer
• In metallic bonding, outer electrons form a sea of electrons that allows excellent electrical and thermal conductivity
• Why do metallic compounds exhibit high electrical conductivity?

  Sea of electrons
• Why do ionic compounds have high melting and boiling points?

  Strong electrostatic forces
• Polar covalent compounds dissolve in water, while nonpolar covalent compounds do not
• Covalent compounds are poor electrical conductors because they lack free-moving ions or electrons.


  True
• What forms the sea of electrons in metallic bonding?

  Delocalized outer electrons
• Metallic compounds have high melting and boiling points due to strong attractive forces between ions and delocalized electrons
• Metallic bonding is used in structural materials like steel and aluminum due to its excellent electrical and thermal conductivity
• What is chemical bonding?

  Attractive forces between atoms
• In covalent bonds, atoms share electrons
• How are ionic bonds formed?

  Transfer of electrons
• Match the property with the correct bonding type:

  Electron transfer ↔️ Ionic bonding

  Electron sharing ↔️ Covalent bonding
• Metallic bonding involves a sea of delocalized electrons.


  True
• What forms the bond in metallic bonding?

  Sea of electrons
• Match the bond type with its bond formation:

  Ionic ↔️ Electron transfer

  Covalent ↔️ Electron sharing

  Metallic ↔️ Delocalized electrons