Interpretation:
The compound having higher melting point between
Concept Introduction:
Coulomb’s law:
It states that the magnitude of the electrostatic force between two point charges is directly proportional to the product of the magnitudes of the charges and inversely proportional to the square of the distance between them.
Where,
Periodic trend of size:
Atomic radius decreases from left to right within a period. This is due to the increase in the number of protons and electrons across a period. One proton has a greater effect than one electron; thus, electrons are pulled towards the nucleus, resulting in a smaller radius and smaller size. Atomic radius increases from top to bottom within a group. This is due to electron shielding.
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Chapter 9 Solutions
OWLV2 FOR MOORE/STANITSKI'S CHEMISTRY:
- Consider these ionic compounds: KCl, CaS, CaO, SrSe, and LiF. Without looking up any values, predict the order of melting points from lowest to highest. Explain the reasons for your predictions.arrow_forwardThe melting point of TiCl4 (-24°C) lies below those ofTiF4 (284°C) and TiBr4 (38°C). Explain why by considering the covalent-ionic nature of these compounds and theintermolecular forces in each case.arrow_forwardWhy do salt crystals have a cubical shape?arrow_forward
- ● Explain why higher average kinetic energy results in higher vapor pressure in terms of IMFs.arrow_forwardDefine the term crystalline lattice?arrow_forwardFor each of the following pairs of substances, predict which member of the pair will have the higher melting point, and indicate why.arrow_forward
- Which compound will be more likely to exist as a hydrated solid? O KCl CuSO4arrow_forwardDistinguish sodium chloride structure and diamond structure. Provide an illustration to support your explanationarrow_forwardIn terms of intermolecular forces, explain why the boiling point of Br2(59°C) is lower than that of iodine monochloride ICl (97°C), even though they have nearly the same molar mass.arrow_forward
- The student finds the following particulate model of AgCl(s). Assuming the crystal structures are similar, how should the student modify the model to represent CuCl(s)? Justify your answer in terms of the radius and arrangement of electrons in the ions.arrow_forwardConsider the following materials: 1) liquid methane (CH4) 2) liquid water (H2O), 3) solid sodium fluoride (NaF) and 4) liquid solution of NaF in water. Describe the types of forces which hold the ions and/or molecules together in each of these materials.arrow_forwardWhich compound likely has a higher melting point, aluminum chloride AlCl3 or Phosphorus trichloride PCl3? Use the periodic table to support your claim.arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
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