5. A single electron orbits around a nucleus of charge (+Ze). It requires 47.2 eV to excite the electron from third Bohr orbit to the second orbit, calculate: a. The value of Z. b. The radius of the first excited orbit.

5. A single electron orbits around a nucleus of charge (+Ze). It requires 47.2 eV to excite the electron from third Bohr orbit to the second orbit, calculate: a. The value of Z. b. The radius of the first excited orbit.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter2: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 66E: Consider an electron for a hydrogen atom in an excited state. The maximum wavelength of...

See similar textbooks

Related questions

Q: Below are radial probability distributions for the 2s, 2p, 3s, 3p and 3d orbitals in random order.…

A: For the graph 2 and 4, the radial nodes is zero.

Q: -36 Imagine an alternate universe where the value of the Planck constant is 6.62607 × 10 J.s. In…

A: The size and the wavelength of the particle distinguish between the classical and quantum behavior…

Q: German physicist Werner Heisenberg related the uncertainty of an object's position (Δ?) to the…

A: Heisenberg's uncertainty principle tells us that the position and velocity cannot be both measured…

Q: "For an electron the probability that it is in the volume dt is y? dr = (a'n)'e 2/ dt for the 1s…

A: "Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: 6.89 What is the difference between an orbit (Bohr model of the hydrogen atom) and an orbital…

Q: Identify all allowable combinations of quantum numbers for an electron. ?=3,n=3, ?=−1,?=−1,…

A: 1) n=3, l=-1, m=1, ms=-1/2 The possible values of l are 0 to (n-1). Thus for n = 3, l can have…

Q: Below are radial probability distributions for the 2s, 2p, 3s, 3p and 3d orbitals in random order.…

A: Radial distribution curve gives the probability of finding an electron density around the nucleus.

Q: A certain hydrogen electron emitted 434.207nm light as its energy level changed from nexcited = x to…

A: Given that : In transition from level x to y , wavelength of light emitted = 434.207 nm In…

Q: O Use the following radial probability function to justify i. why the B than has a first lower…

A: B has first ionisation energy greather than Be because in the valence cell of boron has 2p1 ,it…

Q: Below are radial probability distributions for the 2s, 2p, 3s, 3p and 3d orbitals in random order.…

A: The number of nodes in radial probability curves is given by the formula=n-l-1 Where, N is principal…

Q: When electromagnetic radiation with a wavelength of 350.0 nm is directed at the surface of a certain…

A: Given : de Broglie wavelength of electron = 14.42 Å = 1.442 X 10-9 m…

Q: Label the radial probability diagram describing the probability of finding an electron at a given…

A: (1)Red colored curve (2p orbital) Radial node for 2p orbital = n-1 (where n= principal quantum…

Q: Please show all work Hydrogen atoms in a gas discharge tube are in their quantum mechanical…

A: Energy of the electrons = 13.2 eV Energy of hydrogen atom in ground state = -13.6 eV After collision…

Q: 23. (a) Calculate the wavelengths of the first three lines of Lyman, Balmer and Paschen series. (b)…

A: given lines of Lyman , balmer , paschen

Q: 3) The plot below shows two radial distribution functions for electrons on the same atom. Use the…

A: The residence of electrons with the maximum probability of determination in the three-dimensional…

Q: a) For an atom, radial distribution function, D(r) =r²R(r), indicates probability distribution of…

Q: ) Draw the graph of 4π r2R2 versus r for the hydrogen atom and explain it. Also compare the…

A: Introduction: We have to draw curve for hydrogen atom for (4πr2R2 Vs r ).

Q: can u help me with my hw? Tysm❤️ Please explain why are they possible and not possible please.…

A: Introduction Principal quantum number: It is represented by the symbol “n”. It denotes the energy…

Q: 17. What are the values for n and l for each of the following: a. 3p b. 4s c. 6d d. 5f

A: The possible values of principal quantum number are n = 1, 2, 3.... The possible values of angular…

Q: Here is a sketch of a 2py orbital. The sketch is about 800 pm wide, the coordinate (x,y,z) axis are…

A: Given the sketch of 2py orbital. For 2py orbital the probability of finding the electron is maximum…

Q: The subshell where value of Principal Quantum number is 4 and value of Azimuthal quantum number is 1…

A: Given :- Principle quantum number = 4 Azimuthal quantum number = 1 To determine :- Subshell to…

Q: Express the speed of the electron in the Bohr model in terms of the fundamental constants (me, e, h,…

Q: The equipment used for aviation communications emits high‑frequency radiowave energy with a…

A: The energy of a photon of a radiation is expressed as:

Q: Question is attached

A: Given electronic configuration: 1s32s22p5

Q: Calculate the energy difference (AE) for the electron transition of n = 3 to n = 1 for 1.00 mol of…

Q: What is the energy for the above frequency / wavelength for one photon and one mole? Step one: Use…

Q: How did Schrödinger’s approach to the electron differ from Bohr’s?

A: Schrödinger’s approach to the electron differ from Bohr’s like

Q: (a) A green laser pointer emits light with a wavelength of532 nm. What is the frequency of this…

Q: For the Li atom, the energy difference between the ground state and the first excited state, in…

A: The ground state electron configuration of lithium (Li) is 1s2 2s1,'and the electron configuration…

Q: The second line of the Balmer series occurs at a wavelength of 486.61 nm. What is the energy…

Q: frequency

Q: When a metal was exposed to photons at a frequency of 1.31 × 105 s-', electrons were emitted with a…

Q: Quantum numbers arise naturally from the mathematics used to describe the possible states of an…

A: Hello. Since your question has multiple sub-parts, we will solve the first three sub-parts for you.…

Q: (a) Find the probability of occupying an electron to energy level at a temperature of (98 °C), if…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Q2. Consider a particle with quantum number n moving in in a one-dimensional box of length I a. Find…

Q: Excited Helium atoms radiate energy in what regions? please explain a)infrared region only b)…

A: Excited helium atom radiate energy in the "visible region". As we all have seen Helium lamps are…

Q: A ground state hydrogen atom absorbs a photon of light having a wavelength of 92.05 nm. What is the…

A: The Rydberg’s formula can be written as follows,

Q: (e) Estimate the total energy of a carbon atom by adding the energies of the populated hydrogenic…

Q: 1.German physicist Werner Heisenberg related the uncertainty of an object's position (Δ?) to the…

A: We will answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: b. Calculate the frequency of this emitted green radiation, in s¹. Show your work. Calculate the…

A: b) Frequency can be calculated using the formula : Frequency (ν)=Speed of light (c)wavelength(λ) c)…

Q: Models of atom (i) similarities and differences between Rutherford and Bohr (ii) similarities and…

A: Rutherford model: In this model, the scientist Rutherford discovered that there is empty space in…

Concept explainers

Atomic Structure

The basic structure of an atom is defined as the component-level of atomic structure of an atom. Precisely speaking an atom consists of three major subatomic particles which are protons, neutrons, and electrons. Many theories have been stated for explaining the structure of an atom.

Shape of the D Orbital

Shapes of orbitals are an approximate representation of boundaries in space for finding electrons occupied in that respective orbital. D orbitals are known to have a clover leaf shape or dumbbell inside where electrons can be found.

Question

5. A single electron orbits around a nucleus of charge (+Ze). It requires 47.2 eV to excite the
electron from third Bohr orbit to the second orbit, calculate:
a. The value of Z.
b. The radius of the first excited orbit.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

The energies of macroscopic objects, as well as those of microscopic objects, are quantized, but the effects of the quantization are not seen because the difference in energy between adjacent states is so small. Apply Bohr’s quantization of angular momentum to the revolution of Earth (mass6.01024kg) , which moves with a speed of 3.0104ms1 in a circular orbit (radius1.51011m) about the sun. The sun can be treated as fixed. Calculate the value of the quantum number n for the present state of the Earthsun system. What would be the effect of an increase in n by 1?
The wave function of an electron in the lowest (that is, ground) state of the hydrogen atom is (r)=( 1 a 0 3 )1/2exp(r a 0 )ao=0.5291010m (a) What is the probability of finding the electron inside a sphere of volume 1.0pm2 , centered at the nucleus (1pm=1012m) ? (b) What is the probability of finding the electron in a volume of 1.0pm2 at a distance of 52.9 pm from the nucleus, in a fixed but arbitrary direction? (c) What is the probability of finding the electron in a spherical shell of 1.0 pm in thickness, at a distance of 52.9 pm from the nucleus?
Suppose an atom in an excited state can return to the ground state in two steps. It first falls to an intermediate state, emitting radiation of wavelength 1 , and then to the ground state, emitting radiation of wavelength 2 . The same atom can also return to the ground state in one step, with the emission of radiation of wavelength . How are 1,2, and related? How are the frequencies of the three radiations related?
What are the allowed values for each of the four quantum numbers: n, l, ml, and ms?
Consider the orbitals shown here in 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 with n=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 with n=4, of an orbital of type (y) in a shell with n=2. Of an orbital of type (z) in a shell with n=3. (d) What is the smallest possible n value for an orbital of type (x)? Of type (y)? Of type (z)? (e) What are the possible I and ml values for an orbital of type (x)? Of type (y)? Of type (z)?
What are the values of E, L, and Lz for an F8+ atom whose electron has the following wavefunctions, listed as n,l,ml? a 1,0,0 b 3,2,2c 2,1,1d 9,6,3.
As the weapons officer aboard the Srarship Chemistry, it is your duty to configure a photon torpedo to remove an electron from the outer hull of an enemy vessel. You know that the work function (the binding energy of the electron) of the hull of the enemy ship is 7.52 1019 J. a. What wavelength does your photon torpedo need to be to eject an electron? b. You find an extra photon torpedo with a wavelength of 259 nm and fire it at the enemy vessel. Does this photon torpedo do any damage to the ship (does it eject an electron)? c. If the hull of the enemy vessel is made of the element with an electron configura tion of [Ar]4s13d10, what metal is this?
Defend and criticize Bohrs model. Why was it reasonable that such a model was proposed, and what evidence was there that it "works"? Why do we no longer "believe" in it?
6.92 The photoelectric effect can he used to measure the value of Planck's constant. Suppose that a photoelectric effect experiment was carried out using light with v=7.501014s1 and ejected electrons were detected with a kinetic energy of 2.501011 J. The experiment was then repeated using light with v=1.001015s1 and the same metal target, and electrons were ejected with kinetic energy of 5.001011 J. Use these data to find a value for Planck’s constant. HINTS: These data are fictional and will give a result that is quite different from the real value of Planck's constant. Be sure that you do not use the real value of Planck's constant in any calculations here. It may help to start by thinking about how you would calculate the metal's binding energy if you already knew Planck's constant.
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 H atom is 1460 nm. What is the initial excited state for the electron (n = ?)?
We can represent both probability and radial probability versus distance from the nucleus for a hydrogen ls orbital as depicted below. What does each graph tell us about the electron in a hydrogen 1s orbital?