Bismuth forms two fluorides: BiF3 and BiF5. As is usually the case, the compound with the metal in the lower oxidation state has more ionic character,whereas that with the metal in the higher oxidation state has more covalent (molecular) character. Predict which bismuth fluoride will have the higher boiling point.

Bismuth forms two fluorides: BiF3 and BiF5. As is usually the case, the compound with the metal in the lower oxidation state has more ionic character,whereas that with the metal in the higher oxidation state has more covalent (molecular) character. Predict which bismuth fluoride will have the higher boiling point.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 59QRT

See similar textbooks

Similar questions

Answer the questions in the table below about the shape of the borane (BH3) molecule. How many electron groups are around the central boron atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central boron atom? (You may need to use the scrollbar to see all the choices.) (choose one) X G <
What word or two-word phrase best describes the shape of the phosphorus tribromide (PBr3 ) molecule? X
Which of the following has the largest covalent radius ? Mg Ca Sr Ba
Calculate the lattice enthalpies, ΔU (also called ΔHL), of the following group 1 fluoride compounds by using the Born–Mayer equation. The radius of Na is 102 pm and the radius of F– is 133 pm. The radius of Cs is 167 pm and the radius of F– is 133 pm.
Like CO2, water has two polar bonds but unlike CO2, water is polar overall. Explain why this is so?
Galium (Ga) is an element in group III with atomic number 31. By referring to the Periodic Table, answer the following questions. Explain how the atomic radius of gallium differs from aluminium. Explain how the electronegativity of gallium differs from aluminium. Explain how the electronegativity of gallium differs from germanium. Explain how the ionisation energy of gallium differs from germanium. Explain how the ionisation energy of gallium differs from indium.
Determine if the following expressions are true or false: True or false 1. Be is the only element of Group 2A that forms covalent compounds. 2. Al forms only tetrahedral compounds. 3. B is metalloid and semiconductor. 4. The SiO44‒ ion is tetrahedral. 5. In compound N2O5, nitrogen has an oxidation number of +5. 6. P forms only covalent compounds. 7. H3PO3 is triprotic acid. 8. HClO4 is explosive. 9. Br2 (l) oxidizes I2 (s). 10. The XeF4 molecule is tetrahedral.
Use Intermolecular Forces to explain why CF4 is a gas at room temperature but CCl 4 is a liquid.
Which of the following is true of the reaction 2H2O(g) -> 2H2(g) + O2(g) ?
Why are lithium halides covalent in nature?
In a hydrogen molecule, the two hydrogen atoms are held together by a single bond with a bond energy of 436 kJ/mol of hydrogen. In other words, to break the H-H bonds in one mole of molecular hydrogen requires the expenditure of 436 kJ of energy. Using the balanced chemical equation for the formation of water from oxygen and hydrogen (shown above), and interpreting the stoichiometric coefficients as mole amounts, how much energy must be expended in breaking the H-H bonds? kJ
Which compound likely has a higher melting point, aluminum chloride AlCl3 or Phosphorus trichloride PCl3? Use the periodic table to support your claim.