Math  /  Algebra

Question3 8 points
In units of hRh R, what is the amount of energy associated with the transition from n=4n=4 to n=1n=1 in the hydrogen emission spectrum? ( h is Planck's constant and R=3.3×1015 HzR=3.3 \times 10^{15} \mathrm{~Hz} in the Rydberg equation, although you don't need to use these numbers in this problem.) 116hR\frac{1}{16} h R 34hR\frac{3}{4} h R 14hR\frac{1}{4} h R 1516hR\frac{15}{16} h R 4 8 points

Studdy Solution

STEP 1

What is this asking? How much energy is released when an electron in a hydrogen atom jumps from a higher energy level (n=4) to a lower energy level (n=1), expressed in terms of *hR*? Watch out! Don't forget that the energy change is negative since energy is *released*!
But we're asked for the *amount* of energy, which is positive.

STEP 2

1. Rydberg Formula
2. Calculate the Energy Change

STEP 3

Alright, let's **start** with the Rydberg formula, which describes the energy change when an electron transitions between energy levels in a hydrogen atom.
It's like a secret code for the atom's energy!
The formula is: ΔE=hR(1nf21ni2) \Delta E = -hR \left( \frac{1}{n_f^2} - \frac{1}{n_i^2} \right) Where ΔE\Delta E is the **change in energy**, *h* is **Planck's constant**, *R* is the **Rydberg constant**, nin_i is the **initial energy level** of the electron, and nfn_f is the **final energy level**.

STEP 4

Remember, a *negative* ΔE\Delta E means energy is *released*, while a *positive* ΔE\Delta E means energy is *absorbed*.
We're dealing with *emission* here, so we expect a negative value for ΔE\Delta E.

STEP 5

Let's **plug in** our values.
We're given ni=4n_i = 4 (the **initial level**) and nf=1n_f = 1 (the **final level**).
So, we have: ΔE=hR(112142) \Delta E = -hR \left( \frac{1}{1^2} - \frac{1}{4^2} \right)

STEP 6

Now, let's **simplify** those fractions: ΔE=hR(11116) \Delta E = -hR \left( \frac{1}{1} - \frac{1}{16} \right) ΔE=hR(1116) \Delta E = -hR \left( 1 - \frac{1}{16} \right)

STEP 7

To subtract the fractions, we need a **common denominator**, which is **16**: ΔE=hR(1616116) \Delta E = -hR \left( \frac{16}{16} - \frac{1}{16} \right)

STEP 8

Now, **subtract**: ΔE=hR(16116) \Delta E = -hR \left( \frac{16 - 1}{16} \right) ΔE=hR(1516) \Delta E = -hR \left( \frac{15}{16} \right) ΔE=1516hR \Delta E = -\frac{15}{16} hR

STEP 9

The **energy change** is 1516hR-\frac{15}{16} hR.
Since the question asks for the *amount* of energy, we take the absolute value, making it positive: ΔE=1516hR |\Delta E| = \frac{15}{16} hR

STEP 10

The amount of energy associated with the transition is 1516hR\frac{15}{16} hR.

Was this helpful?

Studdy solves anything!

banner

Start learning now

Download Studdy AI Tutor now. Learn with ease and get all help you need to be successful at school.

ParentsInfluencer programContactPolicyTerms
TwitterInstagramFacebookTikTokDiscord