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Consider two hypothetical elements, W and Z. Element W has an electron affinity of ?150 kJ/mol, and element Z has an electron affinity of ?38 kJ/mol.
• a. If you have a W? ion and a Z? ion, from which ion would it require more energy to remove an electron? Explain your answer.
• b. If elements W and Z are in the same period of the periodic table, which atom would you expect to have the greater atomic radius? Why?
• c. Assuming that the elements are in the same period, which element would you expect to have the smaller first ionization energy?
• d. Do the valence electrons in element Z feel a greater effective nuclear charge than those in element W? Explain how you arrived at your answer.
Irradiation of di-t-butyl ketone in a solution of carbon tetrachloride produces pivaldehyd (2,2-dimethylpropanal), chloroform, isobutene, t-butyl chloride, and carbon Monoxide. Suggest a mechanism which accounts for the formation of each product.
Compute the number of moles of Chlorine atoms in 3.01×10^24 formula units of magnesium chloride,MgCl2 .
If the final tempurature of the combined water is 42.0 degrees C and the heat capacity of the calorimeter is 26.3 J/degrees C , calculate the mass of the water originally in the calorimeter
Geometric isomers illustration, This is more of a theoretical question I think. Co(NH3)5ClBr has two compounds for that one formula.
calculate the initial slopes of the plots of the compressibility factor z vs p at 300k and 600k.
Draw the missing intermediate and add curved arrows for the production of phenylethyne by the double dehydrohalogenation
Nitrogen dioxide and water react to produce nitric acid HNO3 and nitrogen monoxide.
An oxygen tank kept at 20.0?C contains 28.0 moles of oxygen and the gauge reads 31.0 atm. After two weeks, the gauge reads 20.7 atm. How much oxygen was used during the two-week period?
prepared by adding 45.0 mL of 0.15 M NaF to 35.0 mL of 0.10 M HF. What is the pH of the final solution?
Aluminum reacts with excess hydrochloric acid to form aqueous aluminum chloride and 36.8 mL of hydrogen gas over water at 27°C and 764 mmHg. How many grams of aluminum reacted?
What mass of CaCO3 will produce 8.0 L of CO2, measured at standard temperature and pressure conditions? Molar mass of CaCO3 = 100. g per mole.
Find the mass of urea (CH4N2O) needed to prepare 50.8 g of a solution in water in which the mole fraction of urea is 7.55×10?2.
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