Interpretation:
The reason why the first ionization energy of chlorine is greater than sulfur while the second ionization energy are nearly same has to be given.
Concept Introduction:
Ionization energy:
The ionization energy of an atom is the amount of energy required to remove an electron from the gaseous form of that atom or ion.
Example:
As moving across the period the atomic radius decreases therefore the outer electrons are closer to the nucleus and more strongly held by the nucleus and thus it requires a lot of energy to remove the outermost electron.
Second Ionization energy:
The energy required to remove a second electron from a singly charged gaseous cation is called as second ionization energy.
Example:
The second ionization energy of sodium is
The second ionization energy is almost ten times greater than the first ionization energy because the number of electrons causing repulsions is reduced.
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Chapter 1 Solutions
CHEMICAL PRINCIPLES (LL) W/ACCESS
- Assign a correct set of four quantum numbers for (a) Each electron in a nitrogen atom. (b) The valence electron in a sodium atom. (c) A 3d electron in a nickel atom.arrow_forwardWhat is the maximum number of electrons that can occupy a f subshell (l = 3)?arrow_forwardInvestigating Energy Levels Consider the hypothetical atom X that has one electron like the H atom but has different energy levels. The energies of an electron in an X atom are described by the equation E=RHn3 where RH is the same as for hydrogen (2.179 1018 J). Answer the following questions, without calculating energy values. a How would the ground-state energy levels of X and H compare? b Would the energy of an electron in the n = 2 level of H be higher or lower than that of an electron in the n = 2 level of X? Explain your answer. c How do the spacings of the energy levels of X and H compare? d Which would involve the emission of a higher frequency of light, the transition of an electron in an H atom from the n = 5 to the n = 3 level or a similar transition in an X atom? e Which atom, X or H, would require more energy to completely remove its electron? f A photon corresponding to a particular frequency of blue light produces a transition from the n = 2 to the n = 5 level of a hydrogen atom. Could this photon produce the same transition (n = 12 to n = 5) in an atom of X? Explain.arrow_forward
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