Molecules and Compounds Module Exam Practice Flashcard

Front

What is metallic bonding?

Back

Metallic bonding is the electrostatic attraction between delocalized electrons and positively charged metal ions, allowing metals to conduct electricity and heat.

Front

How does the number of delocalized electrons affect metallic bond strength?

Back

More delocalized electrons result in stronger metallic bonds due to increased electrostatic attraction between the electrons and metal ions.

Front

What is an ionic bond?

Back

An ionic bond is a type of chemical bond formed through the electrostatic attraction between oppositely charged ions, typically between a metal and a nonmetal.

Front

Which element is most likely to form an ionic bond with Fluorine (F)?

Back

Calcium (Ca), a metal, is most likely to form an ionic bond with Fluorine.

Front

What is the name of the compound Fe₂O₃?

Back

Iron (III) Oxide.

Front

What type of ion does sulfur (S) most likely form?

Back

Sulfur (S) most likely forms a negative ion with a -2 charge.

Front

What is malleability in metals?

Back

Malleability is the property of metals that allows them to be hammered or pressed into thin sheets without breaking.

Front

What are valence electrons?

Back

Valence electrons are the electrons in the outermost shell of an atom that are involved in forming bonds.

Front

What is the significance of group number in the periodic table?

Back

The group number indicates the number of valence electrons in the elements of that group, which influences their bonding behavior.

Front

How do metals typically react with nonmetals?

Back

Metals typically lose electrons to nonmetals, forming cations and ionic bonds.