Question

1. Calculate the energy (in kJ/mol) of the Lyman series line for hydrogen that is, the...

1. Calculate the energy (in kJ/mol) of the Lyman series line for hydrogen that is, the transition from n=2 to n=1 (1 kJ/mol= 8.6 cm^-1)

2. Would you expect the energy of the same transition as in the first problem to be greater or less for the helium ion, He^+? Why? Make a sketch to relative scale the energy levels that give rise to the Lyman bands in H-atoms and He^+.

Homework Answers

Answer #1

1) We use Rydberg equation

wavenumber of transition = 109737.3 cm-1 ( 1/n1^2 -1/n2^2)   is formula for Hydrogen atom

wavenumber = 109737.3 ( 1/1^2 - 1/2^2) = 82302.975 cm-1e

we have 1KJ/mol = 8.6 cm-1

E in KJ/mol for tranistion = ( 82302.975 /8.6) = 9570 KJ/mol

2) for He^+ atom , Z = 2 ( atomic number)

waveunumver = Z^2 x 109737.3 ( 1/n1^2 -1/n^2)

since Z =2 , Z^2 = 4 , hence we expect higher wavenumbe and thus higher energy.

Orbitals are closer as nuclear charge increases from H to He, hence energy for transition increases as orbitals have higher energy in He^+

E for transitionof He+ = 4 x E for transition for case of H atom   

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Calculate the energy and wavelength of the first line in the Lyman series. What are the...
Calculate the energy and wavelength of the first line in the Lyman series. What are the values of n for the levels the electron is jumping between? nf=1 for Lyman series, the first line will start at ni = nf+1 = 2, ΔE=10.2eV, λ=121.6 nm
Calculate the energy and wavelength of the second line in the Lyman series. What are the...
Calculate the energy and wavelength of the second line in the Lyman series. What are the values of n for the levels the electron is jumping between? Calculate the energy and wavelength of the first line in the Balmer series. What are the values of n for the levels the electron is jumping between? For the first line of the Paschen series, what are the initial and final energy levels?
For a hydrogen atom, calculate the wavelength of an emitted photon in the Lyman series that...
For a hydrogen atom, calculate the wavelength of an emitted photon in the Lyman series that results from the transition n = 3 to n = 1. The Rydberg constant is 2.18 x 10^-18 J.
The electronic energy levels for a Helium ion He+ (ie a nuclear charge of +2e and...
The electronic energy levels for a Helium ion He+ (ie a nuclear charge of +2e and a single bound electron of –e) are similar to that of the hydrogen atom (ie a nuclear charge of +e and a single bound electron of charge –e), except for an extra factor of 4 corresponding to the square of the nuclear charge changing from (+e)2 for hydrogen to (+2e)2 for Helium. Thus, the electronic energy levels for Helium are 4 times the electronic...
1. What is the energy in eV and wavelength in µm of a photon that, when...
1. What is the energy in eV and wavelength in µm of a photon that, when absorbed by a hydrogen atom, could cause a transition from the n= 4 to the n= 8 energy level? a) energy in eV b) wavelength in µm 2. The so-called Lyman-αphoton is the lowest energy photon in the Lyman series of hydrogen and results from an electron transitioning from the n= 2 to the n= 1 energy level. Determine the energy in eV and...
The Balmer lines are from a) The transition of hydrogen atoms into the lowest energy level...
The Balmer lines are from a) The transition of hydrogen atoms into the lowest energy level b) The transition of hydrogen atoms into the n=2 level. c) The transition of helium atoms into the lowest energy level. d) The transition of oxygen atoms to the lowest energy level. Emission lines are caused when an electron moves ____ energy; Absorption lines are caused when an electron moves ______ energy a) to higher; to lower b) to a higher n; to a...
How much energy in kJ is needed to excite 1 mol of H atoms to the...
How much energy in kJ is needed to excite 1 mol of H atoms to the stationary state with quantum number n = 6 from their ground state? B) Calculate the frequency in Hz of emitted light when electrons fall back to their grounds state from their state in part A.
a) the first ionization energies (IE) of hydrogen and helium are about 1300 kJ/ mol and...
a) the first ionization energies (IE) of hydrogen and helium are about 1300 kJ/ mol and 2300 kJ/ mol respectively. Yet the electron removed from both of these originated in a 1s orbital. Explain in 1-3 sentences the large IE difference observed between these elements . b) Another particulary interesting exception to the trend in 1st ionization energy is found by comparing N and O. The 1st IE is higher for N than O, even though O has 1 more...
1. The following successive ionization energies are for a particular metal: IE1 = 578 kJ mol-1...
1. The following successive ionization energies are for a particular metal: IE1 = 578 kJ mol-1 IE2 = 1820 kJ mol-1 IE3 = 2750 kJ mol-1 IE4 = 11600 kJ mol-1 Based on these ionization energies, what charge ion would you expect to be the most stable? Briefly explain. Write shorthand electronic configurations for the atoms/ions below: Na V3+ S2- Which statement is true of an endothermic reactions? Briefly explain your choice. Weak bonds break and strong bonds form Strong...
The pairing energy for the free ion Fe2+ is 229 kJ/mol. 10Dq for [Fe(H2O)6]2+ is 10,400...
The pairing energy for the free ion Fe2+ is 229 kJ/mol. 10Dq for [Fe(H2O)6]2+ is 10,400 cm-1, and the ratio of the Racah parameter B in the complex to the value in the free ion is 0.8 (usually designated as β in the literature). Calculate the energy difference between the high and low spin possibilities for [Fe(H2O)6]2+ . Use cm-1 as your energy units.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT