5. The electron in a hydrogen atom makes a transition from the energy state (ni) to the state (nf = 2). If the emitted photon has a wavelength of 433 nm. Determine the magnitude of (ni):

Q: Calculate the energy (in joules) of a photon with a wavelength of 5.00 × 10° nm

A: Answer Energy of a photon = 3.9756*10-20 J

Q: Hydrogen atoms absorb energy so that the electrons are excited to the energy level n = 7. Electrons…

A: Rydberg equation is given by:

Q: Atoms can be ionized by thermal collisions, such as at the high temperatures found in the solar…

A: We make use of the formula for the energy of Hydrogen atom and Hydrogen like atoms, to get the…

Q: The energy of a mole of photons of red light from a laser is 175 kJ/mol. Calculate the energy of one…

A:

Q: Sodium metal requires a photon with a minimum energy of 4.41 x10-19 J to emit electrons. What is the…

A: As you have asked part (c), solving the same for you: (c)

Q: Heated lithium atoms emit photons of light with an energy of 2.961 × 10−19 J. Calculate the…

A: Given: Energy 2.961x10-19 J The distance between consecutive troughs or peaks is said to be the…

Q: An excited hydrogen atom emits a photon with a wavelength of 656.4 nm.In what what color will this…

A: Passing of white light through a sample with hydrogens, the electron in it gets excited to higher…

Q: A violet line occurs at 435.8 nm in the emission spectrum of mercury. What amount of energy, in…

A: Given:          Wavelength= 435.8 nm

Q: A photon has a wavelength of 705 nm. Calculate the energy of the photon in joules.

A: The energy of the photon in joules has to be given, Convert nanometers into meters.

Q: Consider a photon with wavelength 707 nm. What is the energy of a mole of photons of this wavelength…

A:

Q: An excited hydrogen atom emits light with a wavelength of 656.7 nm to reach the energy level for…

A: nfinal = 2ninitial = ?change in energy during transition is given below.

Q: 1- Calculate the wavelength of a photon emitted during a transition from the n = 4 state to the n =…

A: Recall the following relation to calculate the wavelength of a photon emitted…

Q: What is the energy of a photon with a wavelength of 655nm?

A: Given information: Wavelength of a photon is 655 nm

Q: Consider an atom of hydrogen that absorbs light of a wavelength 955.8 nm. What is the energy, in J,…

A: To solve this problem we will use the formula  E = hc/λ    Where  E = energy  h = planks constant  =…

Q: An excited hydrogen atom emits light with a wavelength of 383.8 nm to reach the energy level for…

A: Given : Wavelength = 383.8nm nf = 2

Q: 7.33 In addition to continuous radiation, fluorescent lamps emit some visible lines from mercury. A…

A:

Q: When photons with a wavelength of 300 nm fall on lithium metal, electrons with kinetic energy of 150…

A: Please find your solution below : Given, Wavelength of photon = 300 nm = 300 × 10-9 m Kinetic energy…

Q: It takes 208.4 KJ of energy to remove 1 mole of electrons from an atom on the surface of rubidium…

A: How much energy does it take to remove a single electron from an atom on the surface of solid…

Q: The laser in an audio compact disc player uses light with a wavelength of 7.80 x 10-7 m. Calculate…

A: Every light with a wavelength have an associated frequency and energy value.

Q: What is the maximum number of orbitals that can be identified by the following set of quantum…

A: we have to calculate the number of orbitals

Q: The blue color in fireworks is often achieved by heating copper (I) chloride, CuCl, to about 1200°…

A: Energy of Photon:  E = hv  Where  E = energy  h = plank constant  v = frequency As we know that  v =…

Q: An electron in the hydrogen atom makes a transition from an energy state of principal quantum…

A: Given data,ni=?n=2λ=434nm=434×10-9m

Q: 9. The lowest energy level of the electron in a Hydrogen atom is -13.6 eV. What would be the…

A: Answer:- This question is answered by using the simple concept of calculation of energy change…

Q: The yellow light given off by a sodium vapor lamp used for public lighting has a wavelength of 589…

A: The frequency of yellow light with a wavelength of 589 nm is calculated as,

Q: b. You are an engineer designing a switch that works by the photoelectric effect. The metal you wish…

A: A device requires 6.7*10-19 J/atom for ionization. The light falling on the metal has a wavelength…

Q: How much energy, in aJ, is required for an electron in a hydrogen atom to make a transition from the…

A: Given: The initial and final energy level of the hydrogen atom is 2 and 3, respectively.

Q: An excited hydrogen atom emits light with a wavelength of 410.4 nm to reach the energy level for…

A: Given : Wavelength = 410.4nm  nf =  2

Q: An excited hydrogen atom emits light with a wavelength of 389.1 nm to reach the energy level for…

A:

Q: It takes 495.0 kJ of energy to remove 1 mole of electron from an atom on the surface of sodium…

A: The amount of energy required to remove 1 mole of electron from an atom on the surface of sodium…

Q: 7.63 The photoelectric effect is illustrated in a plot of the kinetic energies of electrons ejected…

A:

Q: Heated lithium atoms emit photons of light with an energy of 2.961 × 10−19 J. Calculate the…

A:

Q: Microwave ovens heat food by creating microwave electromagnetic radiation that is absorbed by water…

A: The amount of heat required to raise temperature is calculated as,

Q: 20.) How many orbitals are possible for a principal quantum number n = 3 and angular quantum number…

A: Given, Principal quantum number   n = 3 Angular quantum number or azimuthal quantum number  "l" =1.…

Q: What is the energy in joules for a photon with a wavelength of 620. nm?

A: Ans given as follows

Q: The photoelectric effect can be used in engineering designs for practical applications. For example,…

A: Energy = 2.0 x 10-20 J

Q: An excited hydrogen atom emits light with a wavelength of 486.4 nm to reach the energy level for…

A: Given, wavelength = 486.4nm Let the electron makes transition from principal quantum level , n to 2.…

Q: The laser in an audio CD player uses light with a wavelength of 7.80 x 102 nm. Calculate the…

A:

Q: The light emitted from one of the following electronic transitions (n=4 to n = 3 or n = 3 to n = 2)…

A: Energy emitted in the transition from n=3 to n=2 is more than energy emitted in the transition from…

Q: Sodium atoms emit light with a wavelength of 330 nm when an electron moves from a 4p orbital to a 3s…

A: Since the light i.e photon is emitted due to the transition  hence the energy of light or photon…

Q: 7. A mole of photons has an energy of 1609 kJ/mol. Calculate the wavelength that corresponds to this…

A: Photon is the smallest constituent particle of light. The energy (E) of a photon is given as: E=hcλ…

Q: How much energy do single photons of 453 nm and 482 nm have

A: Energy of photon is given by E = hc/λ where E = energy of photon  h = Planks constant = 6.626 X…

Q: Calculate the wavelength of light emitted from a hydrogen atom when it undergoes a transition from…

A:

Q: 5. Is there a line in the Paschen series at 1.043 x 106 m? Explain with calculations. Calculate the…

A: Paschen series is a part of hydrogen spectra in which the electron in n=3 excites to higher levels…

Quantum Chemistry

Quantum chemistry deals with the properties of chemical systems and their reactions. The branch of chemistry which is more concerned with quantum chemistry is physical chemistry. It is a more sophisticated field of theoretical physics which is concerned towards the application of physical concepts towards various chemical aspects such as, formation of atoms, chemical structure descriptions, chemical bond strength, hybridization, conjugation etc. Quantum chemistry mainly studies the various states i.e., ground state, excited state, transition states of the individual atoms or molecules taking place during any chemical reaction. The laws of motion explained by various scientists, which are termed as “classical mechanics” were not acceptable in terms of electrons, protons, atoms, light etc. Thus, a new theory named “quantum mechanics” emerged to understand the basic framework of various atomic and subatomic particles.