Physical Science Review

Which statement about covalent bonds is true?

• Covalent bonds are generally stronger than ionic bonds because they overlap electrons to fill their outer shell.

• Covalent bonds are generally stronger than ionic bonds because they form full oppositely charged particles.

• Covalent bonds are generally weaker than ionic bonds because they form full oppositely charged particles.

• Covalent bonds are generally weaker than ionic bonds because they overlap electrons to fill their outer shell.

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The formation of lithium fluoride (seen here) is due to

• increased stability in the completion of fluorine's outer shell.

• decreased attraction between the lithium and fluoride ions.

• a stronger pull by the lithium atom on its valence electron.

• the addition of an outer (higher) energy level in the fluoride ion.

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The illustration depicts the formation of an ionic chemical bond between lithium and fluorine atoms. Why is the resulting compound more stable than the individual atoms?

• The shared electron from lithium to fluorine provides each atom with a full outer energy level.

• The transferred electron from lithium to fluorine provides each atom with a full outer energy level.

• The transferred electron from lithium to fluorine provides each atom with an empty outer energy level.

• The shared electron from lithium to fluorine provides each atom with an empty outer energy level.

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The electrons of carbon and hydrogen are _____________ in this molecule of methane.

• transferred

• shared

• charged

• donated

The illustration depicts the formation of an ionic chemical bond between lithium and fluorine atoms. Why is the resulting compound more stable than the individual atoms?

• The transferred electron from lithium to fluorine provides each atom with a full outer energy level.

• The shared electron from lithium to fluorine provides each atom with a full outer energy level.

• The shared electron from lithium to fluorine provides each atom with an empty outer energy level.

• The transferred electron from lithium to fluorine provides each atom with an empty outer energy level.

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Hard well organized solid Atoms are tightly packed together Crystalline arrangement High melting and boiling points The characteristics listed above describe which of the following?

• diatomic molecules.

• ionic compounds.

• covalent compounds.

• molecular compounds.

The electrons of carbon and hydrogen are _____________ in this molecule of methane.

• shared

• charged

• donated

• transferred

Which statement accurately describes covalent bonds?

• Covalent bonds break apart when dissolved in water and allow for the conduction of electricity.

• Covalent bonds are typical of carbon compounds.

• Covalent bonds are created by the attractions between oppositiely charged ions.

• Covalent bonds are formed by metals and nonmetals.

Hard well organized solid Atoms are tightly packed together Crystalline arrangement High melting and boiling points The characteristics listed describe

• ionic compounds.

• diatomic molecules.

• molecular compounds.

• covalent compounds.

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In solid NaCl, each sodium ion is surrounded by six chlorine ions and each chlorine ion is surrounded by six sodium ions. This arrangement results in a

• high melting point and crystalline structure.

• malleable noncrystalline structure.

• weak crystalline solid that conducts electricity.

• ductile, malleable solid with mobile electrons.

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