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Chapter 6: Problem 61

Which of the following represent impossible combinations of \(n\) and $l ?(\mathbf{a}) 1 p,(\mathbf{b}) 4 s,(\mathbf{c}) 5 f,(\mathbf{d}) 2 d$

Short Answer

Expert verified
The impossible combinations of \(n\) and \(l\) are \(1p\) and \(2d\), as their respective \(l\) values are not within the possible range of \(0\) to \(n-1\).

Step by step solution

01

Option a: 1p

The given combination is \(1p\). Here, \(n=1\) and \(l=1\). Since \(l\) is equal to \(n\), it is not within the possible range of \(0\) to \(n-1\), which means the combination is impossible.
02

Option b: 4s

The given combination is \(4s\). Here, \(n=4\) and \(l=0\). Since the possible range of \(l\) is \(0\) to \(n-1\) or in this case, \(0\) to \(3\), and \(l=0\), the 4s combination is possible.
03

Option c: 5f

The given combination is \(5f\). Here, \(n=5\) and \(l=3\) (as we know, \(f=3\)). The possible range for \(l\) is \(0\) to \(n-1\) or in this case, \(0\) to \(4\). Since \(l=3\), the 5f combination is possible.
04

Option d: 2d

The given combination is \(2d\). Here, \(n=2\) and \(l=2\) (as we know, \(d=2\)). The possible range for \(l\) is \(0\) to \(n-1\) or in this case, \(0\) to \(1\). Since \(l\) is equal to \(n\), it is not within the possible range, which means that the combination is impossible. So, the impossible combinations are \(1p\) and \(2d\).

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Most popular questions from this chapter

(a) The average distance from the nucleus of a 3 s electron in a chlorine atom is smaller than that for a \(3 p\) electron. In light of this fact, which orbital is higher in energy? (b) Would you expect it to require more or less energy to remove a 3 s electron from the chlorine atom, as compared with a $2 p$ electron?

Determine which of the following statements are false and correct them. (a) The frequency of radiation increases as the wavelength increases. (b) Electromagnetic radiation travels through a vacuum at a constant speed, regardless of wavelength. (c) Infrared light has higher frequencies than visible light. (d) The glow from a fireplace, the energy within a microwave oven, and a foghorn blast are all forms of electromagnetic radiation.

Microwave ovens use microwave radiation to heat food. The energy of the microwaves is absorbed by water molecules in food and then transferred to other components of the food. (a) Suppose that the microwave radiation has a wavelength of $10 \mathrm{~cm} .\( How many photons are required to heat \)200 \mathrm{~mL}$ of water from 25 to \(75^{\circ} \mathrm{C} ?\) (b) Suppose the microwave's power is $1000 \mathrm{~W}\( ( 1 watt \)=1\( joule-second \)) .$ How long would you have to heat the water in part (a)?

Does the hydrogen atom "expand" or "contract" when an electron is excited from the \(n=1\) state to the \(n=3\) state?

If a sample of calcium chloride is introduced into a nonluminous flame, the color of the flame turns to orange ("flame test"). The light is emitted because calcium atoms become excited; their return to the ground state results in light emission. (a) The wavelength of this emitted light is $422.7 \mathrm{nm} .\( Calculate its frequency. (b) What is the energy of \)1.00 \mathrm{~mol}$ of these photons (a mole of photons is called an Einstein)? (c) Calculate the energy gap between the excited and ground states for the calcium atom.
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