37. Write the ground-state electron configurations of the following ions. (1) CH 2** (ii) Gas- w...
Ne of the Elem ury 37. Write the ground-state electron configurations of the following ions. (2x 4 pts) OCH (ii) Ga3 38. What is the wavelength of a photon (in nanometers) emitted during a transition from the n= 5 state to the ni = 2 state in the hydrogen atom? (10 pts]
1) Calculate the wavelength, in nanometers, of the spectral line produced when an electron in a hydrogen atom undergoes the transition from the energy level n = 7 to the level n = 2 2) A ground state hydrogen atom absorbs a photon of light having a wavelength of 94.92 nm. What is the final state of the hydrogen atom? Consider values for physical constants.
5. Electron in an Infinite Potential Well a) Calculate the ground state and two next highest energy levels for an electron confined to an infinitely high potential well of width l = 1.00E-10 m (roughly the diameter of a hydrogen atom in its ground state). b) If a photon were emitted when an electron jumps from n = 2 to n = 1, what would it's wavelength be? In which part of the spectrum does this lie?
(a) Use the noble-gas notation and write the ground-state electronic configurations of the following ions: (i) S2- (ii) Sn4+ (iii) Mn2+ (b) Write the equation representing the 2nd ionization energy for Co. (c) The electron affinity of Cs is 45 kJ/mol. Write the equation for which this is the energy change. (d) Each of the following oxides reacts with water to produce an acid or a base, depending on whether the oxide is an acidic or a basic oxide. Give...
Use the Bohr model to address this question. When a hydrogen atom makes a transition from the 5^th energy level to the 2^hd, counting the ground level as the first, what is the energy of the emitted photon? Express the answer in electron volts. What is the wavelength, in nanometers, of the emitted photon? What is the radius, in nanometers, of the hydrogen atom in its initial (5^th) energy level?
An electron in the hydrogen atom make a transition from the ground state to an excited level by absorbing energy from a photon. The wavelength of the photon is 95.0 nm. What is the final level that the electron can reach?
5. What is the wavelength, in nanometer, of light emitted when the electron in a hydrogen atom undergoes a transition from level n 6 to level n 1? Write the noble gas core electron configuration and draw the orbital diagram for the ground 6. state arsenic atom.
1. An electron transitions from the n = 6 to the n = 4 quantum state of the hydrogen atom. Is photon absorbed or emitted for the associated electron transition? What is the wavelength of the associated photon? Energy levels: En = -2.1810-18J ; Speed of light: c=3.00 ; Plank constant: h=6.63
Question 4 1 pts An electron in a hydrogen atom makes a transition from the n 11 to the n 4 energy state. Determine the wavelength of the emitted photon (in nm). Enter an integer.
1. Write the ground-state electron configurations for: a. Ti3+ b. Ru2+ 2. How many electrons are in the valence d-orbitals in these transition metal ions and complexes? a. Cu b. [Co(en),(H20)212 c. [Mo(EDTA)]C104 (EDTA is a tetraanion.) d. K}[ReC1]