a. Radiation from a sodium lamp, such as a streetlight, appears as yellow light and has a wavelength of 589 nm. A burst of yellow light from the lamp contains 609 kJ of energy.  How many moles of photons are contained in the burst of light?  b. Consider the hydrogen atom with one electron.  Determine the wavelength of the photon emitted when the electron drops from a 4d orbital to a 2p orbital in a hydrogen atom. c. Draw the complete orbital diagram (line and arrows) for Sr2+.  Label all orbitals.  Hint:  it might be useful to first write the full electron configuration, then do the orbital diagram. d. Draw the complete orbital diagram (line and arrows) for Co2+.  Label all orbitals.  Hint:  it might be useful to first write the full electron configuration, then do the orbital diagram.

Q: b. Which involves the emission of more energy in the H atom, an electron moving from n=4 to n=1 or…

A: we have to determine the transition that emits more energy

Q: A Are any of them s orbitals? List the s orbitals, if any. Are any of them p orbitals? List the p…

A: There are 4 types of orbitals. These are - s, p, d, f.The shapes of orbitals are :s-orbital : It is…

Q: An electron is excited from the n=1 ground state to the n=3 state in a hydrogen atom. Which of the…

A:

Q: This energy diagram shows the allowed energy levels of an electron in a certain atom. (Note: the SI…

A: Part (A) Recall that the electron in the ground state has the lowest energy. Thus, EA​=250zJ Part…

Q: The electron microscope has been widely used to obtain highly magnified images of biological and…

A: Given: Mass of electron = 9.38 × 106 m/s.

Q: 5. How many electrons can sublevel 2p hold? Orbital Diagrams and Electron Configurations A. Complete…

A: • Here, in first question we have to write the maximum number of electron for the 20 orbital.  •…

Q: Create an analogy to explain the four quantum numbers 3. Use quantum number and the Pauli Exclusion…

A:

Q: What is the maximum number of orbitals that can be identified by the quantum numbers n=3, l = 3, ml…

A: No two electrons can have same set of quantum numbers.

Q: The microwave from the introduction emits radiation at 2,450 MHz. You want to make a mug cake after…

A:

Q: An electron in an atom falls from the second to the first energy level and emits a photon of green…

A: In question it is given that when electron falls from 2nd energy level to 1st, green light…

Q: For the fourth-shell orbital shown below, what are the principal quantum number, n, and the angular…

A:

Q: Choose the correct reason why an electron in a d-orbital cannot make a transition into an s-orbital.…

A:

Q: Consider three different light waves in the visible spectrum: A, B, and C. The energy of Wave A is…

A: The energy of the radiation is quantized. The smallest unit of energy of the radiation is known as…

Q: What is the maximum number of electrons that can be contained in an atom’s orbitals having the…

A: The number of electrons in a shell is calculated by the formula, number of electrons=2n2 Where, n…

Q: Which of the following best describes the quantization of energy in atoms? Select one: a. Electrons…

A:

Q: shells a. Without referring to Table 6.2 in your textbook, predict the number of subshells in the…

A: Ans n=4 , l= 0 ,1,2,3

Q: How many photons of frequency 1.50 x 1014 s-1 are needed to give 30.1 J of energy? A. 9.94 x 10^-20…

A:

Q: 2. Electrons are in different orbitals outside of the nucleus. As we know, the nucleus is positively…

A:

Q: which atom would have an electron with the following quantum numbers n=3 I=2 m1=0 ms=-1/2? A. Na…

A:

Q: 4. If the hydrogen atom is in an n = 3, l = 2 state, what is a possible value for l after a photon…

A: Option a (l = 3) is indeed a possible value for the angular momentum (l) after the emission of a…

Q: Write out a possible set of quantum numbers for an electron in each of the followin a. a 3p electron…

A: Quantum numbers: 1. Principal quantum number (n) : 0, 1, 2, 3 ...... 2. Azimuthal quantum number (l)…

Q: B. Given the following information of the three electrons: Quantum Number Electron A Electron B…

A:

Q: a. What is the maximum number of electrons that can go into the first shell? The second shell? b.…

A:

Q: an emission with a frequency of 6.33x 1012 Hz. a. calculate the wavelength, is this emission high…

A: We will calculate wavelength and energy

Q: Which electron energy level transition corresponds to a hydrogen atom absorbing a visible light…

A: Here we have to find the elctron energy level transition corresponds to a hydrogen atom absorbing a…

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.