BL Ch 8 Bonding

Open Ended

How do the three basic types of chemical bonds (ionic, covalent, and metallic) differ in terms of electron behavior?

Multiple Choice

Which of the following best describes the significance of understanding chemical bonding in chemistry?

• It helps explain the properties and behaviors of substances.

• It is only important for laboratory experiments.

• It is mainly used for naming compounds.

• It has no real-world applications.

Multiple Choice

Which statement best describes the octet rule as explained by Lewis symbols?

• Atoms tend to gain, lose, or share electrons until they have eight valence electrons.

• Atoms always lose electrons to form compounds.

• Atoms do not change their electron configuration when bonding.

• Atoms only share electrons when forming compounds.

Open Ended

Explain how the transfer of electrons between sodium and chlorine leads to the formation of an ionic compound.

Multiple Select

Which of the following steps are involved in the Born-Haber cycle for the formation of NaCl?

• Converting elements to gaseous atoms

• Making ions from atoms

• Combining ions to form a solid

• Dissolving NaCl in water

Multiple Choice

According to Coulomb’s law, what happens to the lattice energy if the distance between ions increases?

• Lattice energy decreases

• Lattice energy increases

• Lattice energy remains the same

• Lattice energy becomes zero

Multiple Select

Which factors will increase the lattice energy of an ionic compound?

• Increasing the charge on the ions

• Decreasing the size of the ions

• Decreasing the charge on the ions

• Increasing the size of the ions

Multiple Select

Which of the following are types of electrostatic interactions present in covalent bonds?

• Attractions between electrons and nuclei

• Repulsions between electrons

• Repulsions between nuclei

• Attractions between nuclei

Multiple Choice

Which of the following statements best describes what must occur for a covalent bond to form between two atoms?

• The attractions between electrons and nuclei must be greater than the repulsions.

• The repulsions between electrons and nuclei must be greater than the attractions.

• There must be no electrostatic interactions.

• Atoms must lose electrons completely.

Multiple Choice

In a Lewis structure, what does a single line between two atoms represent?

• A pair of shared electrons (a single bond)

• A lone pair of electrons

• A double bond

• A triple bond

Open Ended

Explain the difference between a single, double, and triple bond in terms of electron sharing and provide an example of each.

Multiple Choice

Which direction does electronegativity generally increase on the periodic table?

• From left to right across a period and from bottom to top of a group

• From right to left across a period and from top to bottom of a group

• From left to right across a period and from top to bottom of a group

• From right to left across a period and from bottom to top of a group

Multiple Choice

Which of the following best describes a polar covalent bond?

• A bond where electrons are shared equally between atoms

• A bond where electrons are transferred from one atom to another

• A bond where electrons are shared unequally between atoms

• A bond that only occurs between metals

Multiple Choice

Based on the table and diagrams, which hydrogen halide has the most polar bond and why?

• HF, because it has the largest electronegativity difference and dipole moment

• HCl, because it has the longest bond length

• HBr, because it has the smallest dipole moment

• HI, because it has the smallest electronegativity difference

Open Ended

Explain how the concept of dipole moment relates to the polarity of a molecule. Use the information from the slides to support your answer.

Multiple Select

Which of the following statements about determining if a compound is ionic or covalent are correct?

• Metal + nonmetal is usually ionic

• Nonmetal + nonmetal is usually covalent

• Electronegativity difference can be used to help determine bond type

• All compounds with low melting points are ionic

Open Ended

How do the properties of ionic, covalent, and metallic bonds influence the behavior of substances in everyday life?

Multiple Choice

What is the first step in writing the Lewis structure for a covalent molecule such as PCl3?

• Write the symbols for the atoms and connect them with bonds

• Sum the valence electrons from all atoms, taking into account overall charge

• Subtract electrons for each positive charge

• Add electrons for each negative charge

Multiple Choice

What are the three basic types of chemical bonds discussed in this lesson?

• Ionic, Covalent, Metallic

• Ionic, Hydrogen, Metallic

• Covalent, Metallic, Hydrogen

• Ionic, Covalent, Hydrogen

Multiple Choice

What is the next step after completing the octets around all atoms bonded to the central atom when writing Lewis structures?

• Assign formal charges to each atom

• Place any leftover electrons on the central atom

• Try multiple bonds if the central atom does not have an octet

• Start over with a different central atom

Multiple Choice

If there are not enough electrons to give the central atom an octet, what should you do according to the steps for writing Lewis structures?

• Add more atoms to the molecule

• Try multiple bonds

• Remove electrons from the molecule

• Assign formal charges

Multiple Select

Select all the correct statements about formal charge and dominant Lewis structures.

• The dominant Lewis structure has formal charges closest to zero.

• A negative formal charge should be placed on the most electronegative atom.

• Formal charge is calculated as valence electrons minus half the bonding electrons minus all nonbonding electrons.

• The dominant Lewis structure always has all atoms with zero formal charge.

Open Ended

Explain the importance of assigning formal charges when drawing Lewis structures. How does it help in determining the best Lewis structure for a molecule?

Multiple Choice

Which of the following statements about the best Lewis structure for ozone (O3) is correct?

• The Lewis structure matches the observed bond lengths in nature.

• Both O to O connections are different in nature.

• The Lewis structure does not agree with what is observed in nature.

• Ozone has only single bonds between oxygen atoms.