(A)
Interpretation:
The compound with higher boiling point from MgBr2 or PBr needs to be determined.
Concept Introduction:
To determine the boiling point of any compound, electronegativity difference of the elements of the compound needs to be calculated. As the electronegativity difference increases, boiling point also increases because more electronegative compound means high bond energy and that higher energy needs too much temperature to boil. This concept can be used to determine the boiling point of the given compounds.
(B)
Interpretation:
The compound with higher boiling point from OsO4 or SrO needs to be determined.
Concept Introduction:
To determine the boiling point of any compound, electronegativity difference of the elements of the compound needs to be calculated. As the electronegativity difference increases, boiling point also increases because more electronegative compound means high bond energy and that higher energy needs too much temperature to boil. This concept can be used to determine the boiling point of the given compounds.
(C)
Interpretation:
The compound with higher boiling point from Cl2O or Al2O3 needs to be determined.
Concept Introduction:
To determine the boiling point of any compound, electronegativity difference of the elements of the compound needs to be calculated. As the electronegativity difference increases, boiling point also increases because more electronegative compound means high bond energy and that higher energy needs too much temperature to boil. This concept can be used to determine the boiling point of the given compounds.
Trending nowThis is a popular solution!
Chapter 3 Solutions
Principles of Modern Chemistry
- 1) Using principles of chemical bonding and/or intermolecular forces, explain each of the following. (a) Xenon has a higher boiling point than neon has. (b) Solid copper is an excellent conductor of electricity, but solid copper chloride is not. (c) SiO2 melts at a very high temperature, while CO2 is a gas at room temperature, even though Si and C are in the same chemical family. (d) Molecules of NF3 are polar, but those of BF3 are not. 2) Using principles of chemical bonding and/or intermolecular forces, explain each of the following: (a) MgCl2 and SiCl4 (b) MgCl2 and MgF2 (c) F2 and Br2 (d) F2 and N2 Note: Please Briefly Explainarrow_forwardwhat are ALL the aqueous chemical species in (CH3)3NHClarrow_forwardDraw a Lewis structure for each of the following molecules and ions. In each case, the atoms can be connected in only one way. (a) Br2 (b) H2S (c) N2H4 (d) N2H2 (e) CN- (f) NH4+ (g) N2 (h) O2arrow_forward
- Compare the magnitude of the lattice energy for each of the following two ion pairs. (a) Ni²+ and O²- separated by a distance of 220 pm (b) Mn²+ and O²- separated by a distance of 431 pmarrow_forwardAn elemental analysis of a hydrocarbon, which contains only carbon and hydrogen, shows the mass%: element mass% carbon 92.26 hydrogen 7.743 (A) * Determine the empirical formula of the hydrocarbon. (B) The compound has a molar mass of 26.04 g/mol. Determine its molecular formula. (C, Draw the Lewis structure of the molecular compound. Count the total number of sigma bonds and pi bonds each, present in the molecule. (D, What is the hybridization of carbon in the molecule? Explain.arrow_forwardPredict which element in each of the following pairs is more electronegative according to the general electronegativity trends in the periodic table: (a) N or O (b) Br or Se (c) F or Cl (d) Si or Carrow_forward
- Use principles of atomic structure to answer each of the following: (1] (a) The radius of the Ca atom is 197 pm; the radius of the Ca2* ion is 99 pm. Account for the difference. (b) The lattice energy of CaO(s) is –3460 kJ/mol; the lattice energy of K20 is –2240 kJ/mol. Account for the difference. (c) Given these ionization values, explain the difference between Ca and K with regard to their first and second ionization energies. Element First lonization Energy (kJ/mol) Second lonization Energy (kJ/mol) K 419 3050 Ca 590 1140 (d) The first ionization energy of Mg is 738 kJ/mol and that of Al is 578 kJ/mol. Account for this difference.arrow_forwardIn the mountains, water in an open container will boil when(a) its critical temperature exceeds room temperature.(b) its vapor pressure equals atmospheric pressure.(c) its temperature is 100 °C.(d) enough energy is supplied to break covalent bonds.(e) none of these is correct.arrow_forwardThe atomic number of sulfur is 16. Sulfur combines withhydrogen by covalent bonding to form a compound, hydrogensulfide. Based on the number of valence electrons in a sulfuratom, predict the molecular formula of the compound.(A) HS(B) HS2(C) H2S(D) H4Sarrow_forward
- Which of the following compound is polar covalent? If a sample of helium gas has a volume of 120 mL and a pressure of 850 mm Hg, what is the new volume if the pressure is changed to 425 mm Hg ?arrow_forward18.) Choose all the statements that are correct. (1) Like atomic size, electronegativity decreases going across a period and increases going down a group. (2) The second most electronegative element is chlorine. (3) Electronegativity is directly proportional to atomic number. (4) Like ionization energy, electronegativity increases going across a period and decreases going down a group. (5) Electronegativity is a measure of the ability of an atom to attract electrons and form a negative ion. (6) Electronegativity is a measure of the ability of an atom in a molecule to attract electrons go itself. (7) Electronegativity was first proposed by Linus Pauling. Group of answer choices (2) (1) (4) (3) (5) (7) (6)arrow_forwardWhich of the following is true of the reaction 2H2O(g) -> 2H2(g) + O2(g) ?arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning