Ionic and Metallic Bonds

What is the definition of ionic bonding?

• A type of chemical bond where atoms share electrons equally.

• A type of chemical bond where atoms transfer electrons to achieve a full outer shell.

• A type of bond formed by the sharing of electron pairs between atoms.

• A type of bond that occurs between metal atoms.

Tags

NGSS.HS-PS1-3

Which of the following is a characteristic of metallic bonds?

• They involve the transfer of electrons between atoms.

• They are formed by the sharing of electron pairs between atoms.

• They involve a 'sea of electrons' that are free to move around.

• They occur only between non-metal atoms.

How are ions formed?

• By the sharing of electrons between atoms.

• By the transfer of electrons from one atom to another.

• By the splitting of atoms into smaller particles.

• By the fusion of two or more atoms.

Compare ionic and metallic bonds in terms of electron movement.

• In ionic bonds, electrons are shared; in metallic bonds, electrons are transferred.

• In ionic bonds, electrons are transferred; in metallic bonds, electrons are shared.

• In ionic bonds, electrons are transferred; in metallic bonds, electrons are free to move.

• In ionic bonds, electrons are free to move; in metallic bonds, electrons are transferred.

Which property is typical of ionic compounds?

• High electrical conductivity in solid state.

• High melting and boiling points.

• Malleability and ductility.

• Low solubility in water.

Tags

NGSS.HS-PS1-3

What is one application of metallic bonding?

• Used in the formation of salts.

• Used in the creation of alloys for construction materials.

• Used in the formation of covalent compounds.

• Used in the production of non-conductive materials.

Explain why ionic compounds tend to have high melting points.

• Because the ions are held together by weak forces.

• Because the ions are held together by strong electrostatic forces.

• Because the ions are free to move around.

• Because the ions are held together by covalent bonds.

Tags

NGSS.HS-PS2-4

Which of the following best describes the electron sea model in metallic bonding?

• Electrons are fixed in place and do not move.

• Electrons are shared between two specific atoms.

• Electrons are delocalized and move freely throughout the metal lattice.

• Electrons are transferred from one atom to another.

What happens to the electrical conductivity of ionic compounds when they are dissolved in water?

• It decreases because the ions are no longer present.

• It increases because the ions are free to move.

• It remains the same because the ions are still bonded.

• It decreases because the ions form covalent bonds.

Identify a key difference between ionic and metallic bonds in terms of structure.

• Ionic bonds form a lattice structure; metallic bonds form a molecular structure.

• Ionic bonds form a molecular structure; metallic bonds form a lattice structure.

• Ionic bonds form a lattice structure; metallic bonds have a 'sea of electrons'.

• Ionic bonds have a 'sea of electrons'; metallic bonds form a lattice structure.