Question 19 Which of the following is true about emission spectra? emission of energy from elements occurs when electrons move from lower energy levels to higher energy levels individual elements emit continuous spectra the emission of individual elements are unique and can be used to identify the element a spectroscope uses diffraction or dispersion to separate continuous spectra into line spectra

Q: The spectrum of a star is which kind: continuous, emission, or absorption? Why?

A: We have to tell which is spectrum of a star is which kind: continuous, emission, or absorption

Q: Three of the known wavelengths of the emission spectrum of helium are 402.6 nm, 447.1 nm and 587.5…

A: Electromagnetic spectrum involves different radiations from the lowest to the highest frequency…

Q: The line emission spectrum of atomic hydrogen is explained as follows

A: The energy of the electron in the line emission spectrum of atomic hydrogen is quantized as number…

Q: A. Light blue Which color of light corresponds to the shortest wavelength? B. Violet Which color of…

A: When any electron from lower energy level goes to higher energy level, it absorbs energy. Then, if…

Q: Use the References to access important values if needed for this question. The wavelength of a…

A: To Convert given wavelength (nm) of a color of orange light to  energy (kJ/photon)  given:…

Q: Some elements do not produce a visible color during a flame test. However, the electrons are still…

A: Here we have to explain why some emission of radiations are colour and others are not during come…

Q: light associated with transitions between energy levels An electronic transition occurs from n = 5…

A:

Q: A nitrogen laser puts out a pulse containing 27.0 m) of energy at a wavelength of 337.1 nm. How many…

A: Total Energy = (n × h × c)/√  √ = wavelength

Q: need help with this problem: Bohr postulated quantized atomic orbits by suggesting that observed…

A: In the early 20th century, scientists were grappling with the perplexing behavior of atoms,…

Q: Light is given off by a sodium- or mercury-containing streetlight when the atoms are excited. The…

A: •Light is electromagnetic radiation which wavelength lies in visible region.

Q: According to Bohr's model, Which emission results in the highest energ photon? * -shell (n=4) shell…

A: according to Bohr's model and electron would absorb energy in the form of photons to get excited to…

Q: Using the figure provided, pick an emission line in the Paschen series for a hydrogen atom and…

A: The different series of spectral lines like Lyman series, Balmer series, Paschen series, Brackett…

Q: [References] The portion of the electromagnetic spectrum between wavelengths of approximately 400…

A:

Q: Part A An electron in a hydrogen atom relaxes to the n = 4 level, emitting light of 74 THz. What is…

A: The energy of electron in nth orbit of hydrogen atom is given by  En = -2.18×10-18n2 J/atom When an…

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

A:

Q: The minimum energy needed to eject electrons from chromium metal via the photoelectric effect is 434…

A: The relation between the energy and wavelength of radiation is as follows, Given: The minimum…

Q: energy of red line: wavelength of light blue line: frequency of light blue line: energy of light…

A: Answer of this question :-

Q: Explain why different elements produce different spectral absorption and emission lines.

A: The spectral absorption and emission lines. The absorption spectra is produced when the atom absorbs…

Q: describe an atomic emission process ( as it gives rise to a portion of an emission spectrum)

A: The chemical compound emits electromagnetic radiations when transition occurs from high energy state…

Q: Match the evidence and reasoning to support the claim: Light is a particle. Evidence: I. Light…

A:

Q: Using your knowledge of the absorption and emission processes, why are only specific colors absorbed…

A: The electrons in an atom or molecule can only occupy certain allowed energy levels. When an electron…

Q: Which transition would correspond to the highest frequency of light emitted? Select one:

A: Answer is  n=4 to n = 1

Q: Calculate the energy of the photon emitted when an electron in a hydrogen atom moves from n=4 to…

A:

Q: • Write an energy diagram below showing why the hydrogen emission spectrum has 4 lines in the…

A: ⏹️ Approach to solving the question: Here's a detailed explanation of why the hydrogen emission…

Q: 4. Deuterium is an isotope of hydrogen with 1 proton and 1 neutron in its nucleus (deuterium = ²H).…

A: Q - Deuterium is an isotope of hydrogen with 1 proton and 1 neutron in its nucleus (deuterium = 2H).…

Q: The line of colors that appear in a line emission spectrum is due to the intensity of light absorbed…

A: In this question we need to explain the reason for the line of colors that appear in a line emission…

Q: Radio wave Shortest Wavelength Infrared Second Longest Wavelength Gamma ray Longest Wavelength

A:

Q: Question 3: A hydrogen atom in the ground state interacts with a photon with a wavelength of 3.650 x…

A: Energy of a energy of photon hx2 =heλ      e=speed of light and λ=wavelengthh=6.63×10-34 J Sc=3×108…

Q: Describe Bohr’s Model of Atomic Quantization?

A: An atom consists of electrons, protons, and neutrons.

Q: When a gas such as Neon is heated and emits light that is then placed in a prism and an emission…

A: The emission spectrum of a chemical element or chemical compound is a spectrum of electromagnetic…

Q: n=2 PHOTON n=2 РHOTON n=1 n=1« FIGURE I FIGURE II Which figure correctly represents when LIGHT IS…

A: An electron jumps to a higher state when it absorbs energy or photons. An electron returns to a…

Q: Calculate the wavelength of yellow light in nanometers if the light has a frequency of 4.14 x 1014…

A: Given information: frequency = 4.14 x 1014 s-1

Q: Why does each element have a unique atomic emission spectrum? Use the following vocabulary in your…

A: Given: Each element has a unique atomic emission spectrum.

Q: if an electron transition between energy levels 4 and 1 leads to a photon of blue light being…

A: The atoms of elements possess electrons in the valence shell along with their presence in the inner…

Q: a A photon with a wavelength of 93.8 nm strikes a hydrogen atom, and light is emitted by the atom.…

A: Wavelength = 93.8 nm

Q: Visible light makes up the largest portion of the electromagnetic spectrui True False

A: Visible light is which can be see by human eyes.

Q: Using these data, find the experimentally determined value of Planck's constant, ℎh , and the…

A: The value of plancks constant h = 6.63 x 10-34 J sAverage value of frequency = 3x1015 /sAverage…

Q: Electrons in the n = 5 energy level emit light with energy equal -275.687 kJ/mol (the negative sign…

A:

Q: What

A: We have to choose Correct option

Q: For the hydrogen atom, which electronic transition results in a red colored emission line?  n=4…

A: In hydrogen atom, the transition corresponding to Balmer series lie in visible region of the…

Q: What is needed for an electron to jump  to a higher energy level? What happens when an "excited"…

A: Absorption of energy in molecules.

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.