Chapter 6: Q64E (page 337)
Question:Write the electron configurations for the following atoms or ions:
(a) B3+
(b) O–
(c) Cl3+
(d) Ca2+
(e) Ti
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What is the energy in joules and the wavelength in meters of the photon produced when an electron falls from then= 5 to then= 3 level in a\({\bf{H}}{{\bf{e}}^ + }\)ion (\(Z = {\rm{ }}{\bf{2}}\)for\({\bf{H}}{{\bf{e}}^{\bf{ + }}}\))?
Question:Based on their positions in the periodic table, predict which has the largest first ionization energy: Mg, Ba, B, O, Te.
What does it mean to say that the energy of the electrons in an atom is quantized?
Question:Consider the orbitals shown here in the outline.
(a) What is the maximum number of electrons contained in an orbital of type (x)? Of type (y)? Of type (z)?
(b) How many orbitals of type (x) are found in a shell withn= 2? How many of type (y)? How many of type (z)?
(c) Write a set of quantum numbers for an electron in an orbital of type (x) in a shell withn= 4. Of an orbital of type
(y) in a shell withn= 2. Of an orbital of type (z) in a shell withn= 3.
(d) What is the smallest possiblenvalue for an orbital of type (x)? Of type (y)? Of type (z)?
(e) What are the possiblelandmlvalues for an orbital of type (x)? Of type (y)? Of type (z)?
Which main group atom would be expected to have the lowest second ionization energy?
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