The following ionization ionization energy are for a 4th row element. Which one?
ID: 483337 • Letter: T
Question
The following ionization ionization energy are for a 4th row element. Which one? Periodic properties. Which atom is larger, cesium or potassium? Why? Which ion is larger, Br^- or Sr^2+ Why? What is larger, K or K^+ ? Why? Which has the higher 1st ionization energy, A1 or In? Why? Which has the higher 1 st ionization energy, greaterthanorequalto or Br? Why? What is the mass % composition by element of POCl_3 ? What is the empirical formula for a compound with 54.46% rubidium, 25.154% selenium, and 20.39% oxygen?Explanation / Answer
8. A. potassium is larger than cesium because ,from top to bottom in group the atomic size increases,hence these are first group elements(H,Li,Na,K,Rb,Cs,Fr)
B. Br- is larger than Sr+2 -, because bromine ion has larger ionic radious.
C.K is larger than K+, because K+has Ar configuration, ,it is of smaller size than K
D. Al has the larger first ionisation value than In, Al= 577kj/mol, In= 558kj/mol
E. Br has larger first ionizationenthaly tha Br, Ge =760kj/mol and Br= 1142kj/mol
9. POCl3, percent mass composition Cl= 69.365% ( 3 atoms)
O= 10.434%
P=20.200%
10. (Rb) 54.46/85.46= 0.637, (Se) 25.154/78.96=0.318, (O)20.39/16=1.274
by deviding each term with least value Rb= 2, Se= 1, O= 4
SO THE EMPERICAL FORMULA = Rb2SeO4
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.