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Chapter 2: Problem 11

Neutral atoms of chlorine are bombarded by high-energy photons, causing the ejection of electrons from the various filled subshells. Electrons originally from which subshell would have the highest velocity after being ejected? (A) 1s (B) 2p (C) 3p (D) 3d

Short Answer

Expert verified
(A) 1s

Step by step solution

01

Identify the closest subshell to the nucleus

From the given options, the 1s subshell is closest to the nucleus. Being in the lowest energy level (n=1), it is the most tightly bound to the nucleus.
02

Reason the kinetic energy after ejection

When the photon bombards the atom, electron from the 1s subshell absorbs more energy than the others because it has to overcome the largest attractive force from the nucleus. Thus, its resultant kinetic energy after ejection would be highest.
03

Choose the correct sub-shell

Since electrons in the 1s subshell will have the highest velocity after being ejected, the correct option is (A) 1s.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Subshells
Subshells are divisions of electron shells. Each shell around an atom's nucleus can contain one or more subshells. These are labeled as s, p, d, and f. Subshells reflect different energy levels and shapes of the space where electrons are found. The 1s subshell is closest to the nucleus. It represents the ground state鈥攖he lowest energy state鈥攐f a chlorine atom.
  • The '1' signifies the principal quantum number, n, indicating the shell's principal energy level.
  • The 's' indicates the type of subshell, which determines the shape of the electron's probability cloud.
Subshells further out from the nucleus such as 2p and 3p have more energy due to reduced nuclear attraction. The electrons in these subshells are less tightly bound to the nucleus.
Kinetic Energy
Kinetic energy refers to the energy an electron has after being ejected from an atom by a photon. Upon ejection, electrons gain velocity, leading to increased kinetic energy. When a high-energy photon bombards an atom, it transfers energy to an electron.
  • Electrons closer to the nucleus, like those in the 1s subshell, need more energy to be ejected since they experience stronger attraction forces.
  • This initial energy absorption translates into high kinetic energy, causing the electron to move faster once it is free.
This is why 1s electrons, despite requiring more energy to be freed, will possess the greatest velocity and kinetic energy post-ejection.
Chlorine Atoms
Chlorine is a chemical element with the atomic number 17, meaning it has 17 protons in its nucleus. In its neutral state, chlorine has 17 electrons distributed across different subshells.
  • The electron configuration for chlorine is 1s虏 2s虏 2p鈦� 3s虏 3p鈦�, indicating its electrons' distribution within subshells.
  • The electrons in its outer shell (3p) are usually involved in bonding and chemical reactions, but when bombarded with high-energy photons, any electron can potentially be ejected.
Understanding chlorine's electron arrangement helps in predicting the effects of external energy, like photon bombardment, on its atoms.
High-Energy Photons
High-energy photons carry enough energy to interact with electrons bound to an atom's nucleus, leading to electron ejection. Photon energy is typically measured in electron volts (eV) and varies depending on the wavelength.
  • When photons collide with electrons, they can transfer their energy, kicking the electron out of its orbit if the photon energy exceeds the electron's binding energy.
  • In the case of chlorine, this interaction results in the ejection of electrons, particularly from tightly bound subshells like 1s due to their high binding energy.
Photon collisions help scientists understand multitudes of atomic behaviors and the structure of atoms.

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Most popular questions from this chapter

A stock solution of 0.100 \(\mathrm{M}\) cobalt (II) chloride is used to create several solutions, indicated in the data table below: \(\begin{array}{|c|c|c|}\hline \text { Sample } & {\text { Volume } \mathrm{CoCl}_{2}} & {\text { Volume }} \\ \hline & {(\mathrm{mL})} & {\mathrm{H}_{2} \mathrm{O}(\mathrm{mL})} \\ \hline 1 & {20.00} & {0} \\\ \hline 2 & {15.00} & {5.00} \\ \hline 3 & {10.00} & {10.00} \\ \hline 4 & {5.00} & {15.00} \\ \hline\end{array}\) (a) In order to achieve the degree of accuracy shown in the table above, select which of the following pieces of laboratory equipment could be used when measuring out the CoCl_{2} : \(150-\mathrm{mL}\) beaker \(\quad 400-\mathrm{mL}\) beaker \(\quad 250-\mathrm{mL}\) Erlenmeyer flask \(\begin{array}{ll}{\text { 50-mL buret }} & {\text { 50-mL graduated }} \\ {} & {\text { cylinder }}\end{array} \quad 100\) -mL graduated cylinder (b) Calculate the concentration of the CoCl, in each sample. The solutions are then placed in cuvettes before being inserted into a spectrophotometer calibrated to 560 \(\mathrm{nm}\) and their values are measured, yielding the data below: \(\begin{array}{|c|c|}\hline \text { Sample } & {\text { Absorbance }} \\\ \hline 1 & {0.485} \\ \hline 2 & {0.364} \\ \hline 3 & {0.243} \\ \hline 4 & {0.121} \\ \hline\end{array}\) (c) If gloves are not worn when handling the cuvettes, how might this affect the absorbance values gathered? (d) If the path length of the cuvette is \(1.00 \mathrm{cm},\) what is the molar absorptivity value for \(\mathrm{CoCl}_{2}\) at 560 \(\mathrm{nm}\) ? (e) On the axes on the next page, plot a graph of absorbance vs. concentrrion. The \(y\) -axes scale is set, and be sure to scale the \(x\) -axes appropriately (f) What would the absorbance values be for \(\mathrm{CoCl}_{2}\) , solutions at the following concentrations? (i) 0.067 (ii) 0.180 \(\mathrm{M}\)

\(2 \mathrm{Ag}^{+}(a q)+\mathrm{Fe}(s) \rightarrow 2 \mathrm{Ag}(s)+\mathrm{Fe}^{2+}(a q)\) Which of the following would cause an increase in potential in the voltaic cell described by the above reaction? (A) Increasing \(\left[\mathrm{Fe}^{2+}\right]\) (B) Adding more \(\mathrm{Fe}(s)\) (C) Decreasing \(\left[\mathrm{Fe}^{2+}\right]\) (D) Removing some \(\mathrm{Fe}(s)\)

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A sample of \(\mathrm{H}_{2} \mathrm{S}\) gas is placed in an evacuated, sealed container and heated until the following decomposition reaction occurs at \(1000 \mathrm{K} :\) $$2 \mathrm{H}_{2} \mathrm{S}(g) \rightarrow 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g) \qquad K_{\mathrm{c}}=1.0 \times 10^{-6}$$ As the reaction progresses at a constant temperature of 1000 K, how does the value for the Gibbs free energy constant for the reaction change? (A) It stays constant. (B) It increases exponentially. (C) It increases linearly. (D) It decreases exponentially.

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