1. Why is H2O a liquid and H2S a gas at room temperature? 2. Arrange the following in increasing boiling point and explain: He, Br2, NaCl. 3. State the type of bonding between all... 1. Why is H2O a liquid and H2S a gas at room temperature? 2. Arrange the following in increasing boiling point and explain: He, Br2, NaCl. 3. State the type of bonding between all the atoms and species in NH4Cl. 4. Which do you expect to form the strongest ionic bond? NaCl or NaI?
Understand the Problem
The image contains four chemistry questions: explaining the physical state of water and hydrogen sulfide at room temperature, ranking substances by boiling point with explanation, identifying bonding types in ammonium chloride, and comparing ionic bond strength between sodium chloride and sodium iodide. All questions require knowledge of chemistry principles and properties of chemical substances.
Answer
1. Hydrogen bonding in H₂O vs. weak van der Waals forces in H₂S. 2. He < Br₂ < NaCl (based on intermolecular forces). 3. Covalent, ionic, and coordinate covalent bonds. 4. NaCl forms a stronger ionic bond.
- H₂O is a liquid at room temperature due to hydrogen bonding, which is a strong intermolecular force. H₂S is a gas because it only has weak van der Waals forces.
- He < Br₂ < NaCl. He is a noble gas with weak London dispersion forces. Br₂ has stronger London dispersion forces due to its larger size. NaCl is an ionic compound with strong electrostatic forces.
- NH₄Cl has covalent bonds within the ammonium ion (NH₄⁺), ionic bonds between the ammonium ion and chloride ion (Cl⁻), and coordinate covalent bonds between nitrogen and hydrogen in the ammonium ion.
- NaCl is expected to form a stronger ionic bond because chloride is smaller than iodide, leading to a shorter bond length and stronger electrostatic attraction.
Answer for screen readers
- H₂O is a liquid at room temperature due to hydrogen bonding, which is a strong intermolecular force. H₂S is a gas because it only has weak van der Waals forces.
- He < Br₂ < NaCl. He is a noble gas with weak London dispersion forces. Br₂ has stronger London dispersion forces due to its larger size. NaCl is an ionic compound with strong electrostatic forces.
- NH₄Cl has covalent bonds within the ammonium ion (NH₄⁺), ionic bonds between the ammonium ion and chloride ion (Cl⁻), and coordinate covalent bonds between nitrogen and hydrogen in the ammonium ion.
- NaCl is expected to form a stronger ionic bond because chloride is smaller than iodide, leading to a shorter bond length and stronger electrostatic attraction.
More Information
Intermolecular forces and bond strengths determine the state and properties of chemical compounds.
Tips
A common mistake is to confuse intermolecular forces with intramolecular forces (chemical bonds).
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