Exploring Ionic Bonding Concepts

Why do atoms bond?

• To increase their energy state

• To become unstable

• To lose all their electrons

• To achieve a full outer shell of electrons

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What is the most stable condition for atoms?

• Being in a high energy state

• Having more protons than electrons

• Having no electrons

• Having a complete set of valence electrons

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Which type of bond involves the transfer of electrons?

• Ionic bond

• Covalent bond

• Hydrogen bond

• Metallic bond

What type of bond is characterized by the sharing of electrons?

• Van der Waals bond

• Ionic bond

• Metallic bond

• Covalent bond

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What is required for an ionic bond to form?

• A metal and a metalloid

• Two nonmetals

• Two metals

• A metal and a nonmetal

What happens to sodium and fluorine during the formation of an ionic bond?

• Both share electrons equally

• Fluorine gives an electron to sodium

• Sodium gives an electron to fluorine

• Both lose electrons

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What is a crystal lattice?

• A two-dimensional structure of atoms

• A three-dimensional structure of alternating positive and negative ions

• A random arrangement of ions

• A single layer of atoms

Why do ionic compounds have high boiling points?

• Because of the strong attraction between positive and negative ions

• Because they have weak bonds

• Because they are made of metals

• Because they are liquids at room temperature

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Why are ionic compounds poor conductors of electricity in solid form?

• Because they have no electrons

• Because the ions do not move freely

• Because they are liquids

• Because they are metals

What happens when an ionic compound is cleaved?

• It forms a new compound

• It becomes a gas

• It melts

• It breaks along planes with flat surfaces