How are the lines in atomic emission spectra produced?
Group of answer choices
electrons absorb a specific amount of energy and become excited
electrons release a specific amount of energy, moving to a higher energy state
electrons release a specific amount of energy, moving to a lower energy state
electrons absorb a specific amount of energy, moving to a lower energy state
The lines in atomic emission spectra are produced due to the fact that " electrons release a specific amount of energy, moving to a lower energy state."
When electron comes from higher energy to lower energy level then it releases energy , and the specific wavelength related to energy released can be seen by us.
Greater the energy gap between higher and lower energy level of the atom higher will be the released energy.
How are the lines in atomic emission spectra produced? Group of answer choices electrons absorb a...
How are emission line spectra produced? As stated by Kirchhoff. How are emission line spectra produced? At an atomic level
42) is the phenomenon whereby the electrons of an atom absorb energy as they transition from lower energy orbitals to higher energy ones. (1 point) 43) How many 7f orbitals are there? (1 point) 45) For the hydrogen emission spectrum, which of the following would be generated by the return of energetic electrons to the ground state: Paschen lines, Bohr lines, Lyman lines, Einstein lines, Bunsen lines, or Balmer lines? (1 point) 47) Condensed phosphates with three or more units...
Match each definition with the appropriate name. Choices: absorption, emission, excited state, ionization, ground state, transition. • any energy state of an atom except the ground state. • the lowest energy state of an atom. • a photon of light causes an electron to jump to a higher energy state. • a photon strikes an atomic electron and removes it from the atom. • an electron falls to a lower energy state and a photon is created. • a jump...
I was having trouble with some lab question on atomic emission
spectra.
Also answer the following questions about your observations: Are the lines present in the hydrogen spectrum the same lines predicted by the Bohr model the atom? Which lines, if any, are missing? Why might there be lines missing? Compare the spectral lines from your unknown substance to the other spectra you observed. Based on these comparisons, what is the identity of the unknown substance? Are there any general...
Part I Determine whether each of the following statements concerning line spectra are true or false. 1. Electrons can absorb energy from being heated in a flame. 2. Electrons are stable in excited states. 3. Electrons release energy as they return to the ground state. 4. Photons are produced when electrons release energy. 5. The energy of the photon can have any value. 6. The energy of the photon is related to the energy levels of the electron orbitals. 7....
Use the following information to answer the next question/ The following diagram represents the emission lines that are produced for the Balmer Series of hydrogen. Each line is produced as an electron makes a transition from a higher Bohr energy level to n-2. Balmer Series Spectral Line Wavelengths I I 300 mm 400 nm 500 nm 600 nm 700 nm The electromagnetic radiation represented by emission line I in the diagram has ai frequency than the electromagnetic radiation represented by...
i
always like(:
IV a) Circle the electromagnetic radiation produced when hydrogen atoms absorb energy and electrons jump back from higher energy level to first energy level (as observed in Lyman series atomic emission experiment)- 1) IR 2) UV 3) visible range (8) IV b) Calculate wavelength and energy of radiation that has a frequency of 6.0 x 10 Hz Formulas are: V frequency x wavelength and Energy = frequency x Planck's constant [constant values are: V = 3.0 x...
Activity 26-5. Atomic spectra [Accompanies Section 26-5] A certain type of atom (not hydrogen) has three energy levels numbered 1, 2, and 3, as shown in the upper illustration. There are three possible transitions between these levels that lead to emission of a photon: 3 → 1, 3 → 2, and 2 → 1. The lower illustration shows the emission spectrum from a gas of these atoms. There are three emission lines, A, B, and C. (a) Rank the photons...
The problem with free radicals is that they tend to Group of answer choices activate protons and become charged compounds attract lightening. have extra electrons, making them acidic release electrons that cause damage to surrounding tissue steal electrons from neighboring compounds
Access the fluorescence excitation and emission spectra for phenylalanine, tyrosine, and tryptophan using the Internet. Answer the following four questions. a. Estimate peak wavelengths for absorption (at λ> 230nm) and emission (at λ> 250nm) for each amino acid. b. How are the peak absorption wavelengths related to the peak emission wavelengths? For example, is the emitted light at lower or higher energy than the absorbed light? Briefly explain. c. Which amino acid shows the biggest energy change from absorption to...