Question

The Li+2 ion contains only one electron and is therefore a hydrogen-like ion that can be...

The Li+2 ion contains only one electron and is therefore a hydrogen-like ion that can be described by the Bohr model. Calculate the wavelengths of the lowest energy transitions in the Lyman and Brackett series for the Li+2 ion.

Homework Answers

Answer #1

1)

for Lyman series, the lowest energy transition from n=2 to n=1

Here photon will be emitted

1/lambda = R*Z^2* (1/nf^2 - 1/ni^2)

R is Rydberg constant. R = 1.097*10^7

Here Z = 3

1/lambda = R*Z^2* (1/nf^2 - 1/ni^2)

1/lambda = 1.097*10^7*3^2* (1/1^2 - 1/2^2)

lambda = 1.35*10^-8 m

lambda = 14 nm

Answer: 1.35*10^-8 m

2)

for Brackett series, the lowest energy transition from n=5 to n=4

Here photon will be emitted

1/lambda = R*Z^2* (1/nf^2 - 1/ni^2)

R is Rydberg constant. R = 1.097*10^7

Here Z = 3

1/lambda = R*Z^2* (1/nf^2 - 1/ni^2)

1/lambda = 1.097*10^7*3^2* (1/4^2 - 1/5^2)

lambda = 4.50*10^-7 m

lambda = 450 nm

Answer: 4.50*10^-7 m

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
Consider a Li++ ion as described by the Bohr model. (a) At some other time, the...
Consider a Li++ ion as described by the Bohr model. (a) At some other time, the electron in n=4 state. What possible wavelength of radiation emitted by this atom? Write the algebraic expression(s) and draw the diagram to illustrate the transitions. (b) What is the ground state energy of this system in eV? Write the expression and evaluate it. What value of the quantum number n does this correspond to? (c) Now assume the electron is in the n=1 state....
Atoms can be ionized by thermal collisions at very high temperatures. One such ion is Cr23+,...
Atoms can be ionized by thermal collisions at very high temperatures. One such ion is Cr23+, a chromium atom with only a single electron. (a) By what factor are the energies of its hydrogen-like levels greater than those of hydrogen? (b) What is the wavelength of the first line in this ion's Lyman series?   nm
In the ground state of the Hydrogen atom the energy of the electron is E0 =...
In the ground state of the Hydrogen atom the energy of the electron is E0 = -13.61 eV. What is the energy of the electron in the ground state of the He+ion? _____??? What is the energy of the electron in the ground state of the Li++ ion? _____??? The electron in the He+ ion is excited to the n = 2 principal state. What is the energy of the electron now? _____??? What is the energy of the electron...
The Bohr Model of the hydrogen atom proposed that there were very specific energy states that...
The Bohr Model of the hydrogen atom proposed that there were very specific energy states that the electron could be in. These states were called stationary orbits or stationary states. Higher energy states were further from the nucleus. These orbits were thought to be essentially spherical shells in which the electrons orbited at a fixed radius or distance from the nucleus. The smallest orbit is represented by n=1, the next smallest n=2, and so on, where n is a positive...
1). The Bohr Model of the hydrogen atom proposed that there were very specific energy states...
1). The Bohr Model of the hydrogen atom proposed that there were very specific energy states that the electron could be in. These states were called stationary orbits or stationary states. Higher energy states were further from the nucleus. These orbits were thought to be essentially spherical shells in which the electrons orbited at a fixed radius or distance from the nucleus. The smallest orbit is represented by n=1, the next smallest n=2, and so on, where n is a...
Consider an n-doped semiconductor with an effective electron mass equal to one half the free electron...
Consider an n-doped semiconductor with an effective electron mass equal to one half the free electron mass, and a dielectric constant of 2. Which of the following statements is correct? More than one is correct A. The impurity will look like a hydrogen atom, but with a hole circling it instead of an electron B. The impurities will look like Hydrogen atoms, but smaller in size than a Hydrogen atom in free space C. The impurity will look like a...
The ionized helium atom can be treated with a Bohr model with nuclear charge Z=2. The...
The ionized helium atom can be treated with a Bohr model with nuclear charge Z=2. The resulting energy levels are four times those of the hydrogen atom: Ehelium=4Ehydrogen= -(54.4eV)/n^2 From those energy levels, calculate the wavelengths of spectral lines from ionized helium for transitions that end on nf=1. Do any of these lie in the visible range? Would any spectral lines of ionized helium lie in the visible range?
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...
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. We can observe the wavelengths emitted from Hydrogen. When Hydrogen electrons transition between states, they...
1. We can observe the wavelengths emitted from Hydrogen. When Hydrogen electrons transition between states, they absorb or emit a particle of light called a photon with energy E=hf. Here f is the frequency of light and h is a constant. a. How much energy does an electron in the n=1 (lowest-energy) state of Hydrogen have? Repeat for n=2 and n=3. b. How much energy is emitted if an electron in the n=3 state transitions to the n=2 state? c....
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT