Metallic Bonding Review

Which of the following applies to metals?

• Insulators of heat and electricity

• Poor conductors of heat and electricity

• Non-reactive with other elements

• Good conductors of heat and electricity

According to the electron sea model, what is responsible for the properties of metals?

• Attraction between positively charged metal ions and negatively charged electrons

• Movement of protons within the metal compound

• Arrangement of atoms in a regular pattern

• Movement of free electrons within the metal compound

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What is the structure of metallic compounds?

• Irregular arrangement of metal atoms surrounded by a sea of delocalized electrons

• Random arrangement of metal atoms surrounded by a sea of delocalized electrons

• Regular arrangement of metal atoms surrounded by a sea of delocalized electrons

• Regular arrangement of metal atoms surrounded by a sea of localized electrons

In metallic bonding, what happens to the valence electrons?

• They are shared among all the atoms in the metal.

• They are completely lost from the metal.

• They are transferred to other atoms in the metal.

• They are only shared between adjacent atoms.

Which of the following is a characteristic of metallic compounds?

• unequal sharing of electrons

• pairs of shared electrons

• local electrons

• delocalized electrons

• tranferred electrons

What is the main reason for the high electrical conductivity of metals?

• Metals have a low number of electrons in their outermost shell

• Metals have a high atomic number

• Presence of free electrons in the outermost shell of metal atoms

• Metals have a low melting point

What type of bond is illustrated in this image?

• Metallic

• Ionic

• Covalent

• James

• Polar Covalent

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How does metallic bondbondings contribute to the ductility and malleabilityof metals?

• They allow layers of atoms to slide past each other without breaking the bond.

• They create rigid structures that resist deformation.

• They increase the melting point of metals, making them less ductile.

• They make the metal atoms immobile, reducing ductility.

Why do metals tend to have high melting and boiling points?

• Because of the strong covalent bonds between metal atoms

• Due to the presence of weak hydrogen bonds

• Because of the strong attraction between the metal atoms and the sea of electrons

• Due to the high electronegativity of metal atoms

Measure of the tendency of an atom to attract a bonding pair of electrons is known as...

• electronegativity

• bond polarity

• angular momentum

• valence electrons

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