2.1 Chemical bonds: ionic, covalent, and metallic

• Ionic compounds are crystalline solids at room temperature


  True
• What types of atoms form covalent bonds?

  Non-metal and non-metal
• What properties do metallic bonds result in?

  High electrical and thermal conductivity
• Covalent compounds can be gases, liquids, or solids
• What type of structure do ionic compounds form?

  Crystalline lattice
• What type of structure do covalent bonds form?

  Molecules
• What are the three main types of chemical bonds?

  Ionic, covalent, metallic
• Covalent bonds create molecules where atoms are held together by shared electrons
• Examples of molecules formed via covalent bonding include hydrogen (H₂) and oxygen
• In metallic bonds, valence electrons are delocalized
• The ability of atoms to slide past each other in metals results in their malleability and ductility
• What determines the type of chemical bond formed between two atoms?

  Electronegativity differences
• In what type of solvents are ionic compounds often soluble?

  Polar solvents
• The melting and boiling points of covalent compounds are generally lower than ionic compounds.
• Ionic bonds are formed by the transfer of electrons
• Covalent compounds have a wide range of melting and boiling points


  True
• Match the bond type with its definition:

  Ionic bond ↔️ Transfer of electrons

  Covalent bond ↔️ Sharing of electrons

  Metallic bond ↔️ Delocalization of electrons
• What is the role of valence electrons in metallic bonds?

  They delocalize
• Ionic compounds conduct electricity when dissolved or molten

  True
• Covalent compounds generally have lower melting and boiling points than ionic compounds


  True
• Arrange the bond types by their melting and boiling points from highest to lowest:

  1️⃣ Ionic

  2️⃣ Metallic

  3️⃣ Covalent
• The melting and boiling points of covalent compounds are generally lower than ionic compounds.

  True
• Match the characteristic with its property for covalent bonds:

  Structure ↔️ Molecular

  Melting and Boiling Points ↔️ Lower than ionic compounds

  Conductivity ↔️ Poor conductors
• Metallic bonds result in high electrical and thermal conductivity.


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

  Ionic Bond ↔️ Electron transfer

  Covalent Bond ↔️ Electron sharing

  Metallic Bond ↔️ Delocalization of electrons
• Ionic bonds involve the formation of positively charged cations and negatively charged anions.
• Ionic compounds conduct electricity when in solid form.

  False
• Covalent compounds are poor conductors of electricity.


  True
• Metallic bonds are formed by the delocalization of valence electrons
• The delocalized electrons in metallic bonds allow for high electrical and thermal conductivity
• What is the general trend for the melting and boiling points of covalent compounds compared to ionic compounds?

  Generally lower
• What is the structure of metallic bonds described as?

  Sea of electrons
• Order the types of chemical bonds based on their formation process:

  1️⃣ Ionic bonds: Electron transfer from metal to non-metal

  2️⃣ Covalent bonds: Electron sharing between two non-metals

  3️⃣ Metallic bonds: Delocalization of electrons among metal atoms
• Which type of bond has generally high melting and boiling points?

  Ionic bonds
• Water is an example of a molecule formed by covalent bonding.
• What type of solvents do ionic compounds dissolve in?

  Polar
• What are chemical bonds?

  Attractive forces between atoms
• Which types of atoms form ionic bonds?

  Metal and non-metal
• Covalent bonds are formed by the sharing of electrons
• Metallic bonds are formed by the delocalization of valence electrons