Unit 2: Compound Structure and Properties

Apply Coulomb’s Law and electronic structure to compare electronegativity values for two elements.

1. Explain why Fluorine (F) is more electronegative than Bromine (Br)

Classify a bond as ionic, non-polar covalent, polar covalent, or metallic using periodic trends or electronegativity values.

1. Classify each as non-polar covalent, polar covalent, ionic, or metallic: Mg-O, B-F, Na-Na, O-O?

Assign partial charges to atoms in a bond based on electronegativity.

1. Assign the partial charges to the polar covalent molecule carbon monoxide (CO)

Recognize that ionic and covalent bonds exist on a continuum, with polar covalent bonds in between.

1. Given an example of a covalent bond that has greater ionic character than a N-O bond?

Describe the nature of bonding in terms of electron donation, acceptance, sharing, or delocalization.

1. Match the descriptors to ionic, covalent, or metallic bonding: electron sharing, electron donating, delocalized electrons, electron accepting, non-directional bonding.

Examine a potential energy vs. distance graph to determine bond length and bond energy.

1. What is the bond length on bond energy of the bond depicted in the graph.

Identify the bond order of a bond.

1. Determine the bond order for molecules such as O₂, N₂, and CO.

Compare the relative strength and length of single, double, and triple bonds.

1. Use Coulomb’s Law to compare the strength of bonds in molecules such as HCl, NaCl, and F₂.

Apply Coulomb’s Law to compare the strength of given bonds.

Sketch a simple lattice structure for an ionic solid.

1. Sketch the crystal lattice of NaCl, correctly labeling relative sizes and charges of each ion

Sketch a simple model of a metallic solid.

1. Sketch a particle diagram of a copper (Cu). Be sure to correctly show charge and location of the positively charged ions and electrons.

Determine if two metals will form an interstitial or substitutional alloy based on their relative sizes.

1. Does the image below represent a substiutional or interstitial alloy. Justify your answer.

Compare the main properties of interstitial and substitutional alloys.

1. Fill in the blanks for the generalized properties of alloys. __________ alloys increase the strength, hardness and rigidity of metals while _____________retain the high malleability and ductility of metals.

Draw a Lewis structure that obeys the octet rule given a molecular formula.

1. Draw the lewis structure of NH₃

Evaluate a Lewis structure to determine if it is valid.

1. Explain why O₂ does not contain triple bond

Complete a partial Lewis structure so that it obeys the octet rule.

1. Complete the skeleton structure of diatomic nitrogen (N₂), showing all bonding and non-bonding electrons. N-N

Draw a Lewis structure with resonance when multiple valid configurations exist.

1. Draw the lewis structure of ozone (O₃), showing all equally valid resonance structures.

Complete a partial Lewis structure so that it minimizes formal charges.

1. Place all bonding and non-bonding electrons on the skeleton structure for N₂O. N-N-O

Choose the best Lewis structure from several valid options based on formal charge.

1. Determine which of the following lewis structures minimizes formal charge.

Identify the VSEPR geometry for a given molecule.

1. What is the VSEPR geometry of methane CH₄?

Assign bond angles based on hybridization (up to sp³).

1. What are the bond angles of BF₃, H₂O, and CO₂?

Justify the properties of a compound based on its geometry (e.g., presence of a dipole moment).

1. Explain if CH₄ and H₂O are polar base on their VSEPR geometries.

Quantify the number of pi and sigma bonds in a molecule.

1. How many sigma and pi bonds are in ethane (C₂H₆), ethene (C₂H₄), and Ethyne (C₂H₂)?

Identify two molecules as geometric isomers.

1. Are the molecules below resonance structure, geometric isomers, or neither

Compare the bond strength of sigma and pi bonds.

1. Justify whether a sigma or pi bond is stronger.