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Chapter 7: Problem 35

The work function is the energy required to remove an electron from an atom on the surface of a metal. How does this definition differ from that for ionization energy?

Short Answer

Expert verified
The work function (\(\Phi\)) is the minimum energy required to remove an electron from the surface of a metal atom, depending on the type of metal and its surface condition. In contrast, ionization energy is the energy required to remove an electron from a gaseous atom or ion and is a property of individual elements. The processes involved in both phenomena are different, with work function focusing on the interaction between electrons and the metal surface, while ionization energy considers the interaction between electrons and the nucleus of the atom or ion. Work function is a property of metals, while ionization energy applies to any element. Generally, work function values are lower than ionization energy values, as electrons on the metal surface are loosely bound and more easily removed than electrons tightly bound to atoms in the gaseous state.

Step by step solution

01

Definition of Work Function

The work function refers to the minimum amount of energy required to remove an electron from the surface of a metal atom. This is often denoted by the symbol \(\Phi\). In general, the work function depends on the type of metal, its surface condition, and any additional surface treatments.
02

Definition of Ionization Energy

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. It is typically expressed in units of electron volts (eV) and is a property of individual elements and their electron configurations. In general, ionization energy increases across a period and decreases down a group in the periodic table.
03

Comparison of Processes

The work function is associated with removing an electron from the surface of a metal atom, whereas ionization energy deals with the removal of an electron from a gaseous atom or ion. The processes involved in both phenomena are different: work function focuses on the interaction between the electrons and the metal surface, while ionization energy considers the interaction between the electrons and the nucleus of the atom or ion.
04

Comparison of Materials

Work function is a property of metals, specifically the surface of the metal. It is related to the ability of a metal to emit or absorb electrons. On the other hand, ionization energy is a property of individual elements and their electron configurations. This means that ionization energy can be defined for any element, whereas the work function can only be defined for metals.
05

Comparison of Energy Requirements

The work function is the energy required to remove an electron from the surface of a metal. It generally has lower values compared to the ionization energy of most elements. This is because the electrons on the metal surface are loosely bound and can be more easily removed than the electrons tightly bound to individual atoms in the gaseous state. In summary, the work function and ionization energy are related concepts but differ in terms of their definitions, processes involved, and materials they apply to.

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Most popular questions from this chapter

Does a photon of visible light \((\lambda \approx 400\) to \(700 \mathrm{~nm}\) ) have sufficient energy to excite an electron in a hydrogen atom from the \(n=1\) to the \(n=5\) energy state? from the \(n=2\) to the \(n=6\) energy state?

Identify the following elements. a. An excited state of this element has the electron configuration \(1 s^{2} 2 s^{2} 2 p^{5} 3 s^{1}\). b. The ground-state electron configuration is \([\mathrm{Ne}] 3 s^{2} 3 p^{4}\). c. An excited state of this element has the electron configuration \([\mathrm{Kr}] 5 s^{2} 4 d^{6} 5 p^{2} 6 s^{1}\) d. The ground-state electron configuration contains three unpaired \(6 p\) electrons.

Which of the following electron configurations correspond to an excited state? Identify the atoms and write the ground-state electron configuration where appropriate. a. \(1 s^{2} 2 s^{2} 3 p^{1}\) b. \(1 s^{2} 2 s^{2} 2 p^{6}\) c. \(1 s^{2} 2 s^{2} 2 p^{4} 3 s^{1}\) d. \([\mathrm{Ar}] 4 s^{2} 3 d^{5} 4 p^{1}\) How many unpaired electrons are present in each of these species?

Many times the claim is made that subshells half-filled with electrons are particularly stable. Can you suggest a possible physical basis for this claim?

Consider an electron for a hydrogen atom in an excited state. The maximum wavelength of electromagnetic radiation that can completely remove (ionize) the electron from the \(\mathrm{H}\) atom is \(1460 \mathrm{~nm} .\) What is the initial excited state for the electron \((n=?) ?\)
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