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We know that 99.985% of all hydrogen atoms are hydrogen-1. Only 0.015% are hydrogen-2 atom What is the approximate atomic mass of hydrogen?
To get the atomic mass of an element, we must take a weighted average of the atomic masses of its . That is, we multiply the atomic mass of each...
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Which of the transitions in the hydrogen atom energy-level is the longest wavelength photon?
I'm not entirely sure that I understand your question, but the longest wavelength would belong to the red colored light. When an electron drops from energy level 3 to...
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How do you calculate the wavelength of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level? Recall that for hydrogen $E_n = -2.18 xx 10^-18 J(1/n^2)$
Note that you were given only one energy state. If you consider two energy states, from $n = 4$ to $n = 1$, we have: $E_1 - E_4 =...
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An electron in an hydrogen atom makes a transition from the ground state, $n=1$, to the excited state, $n=5$. Calculate the energy in Joules, frequency in Hertz $(1/s)$, and wavelength in $nm$ of the photon?
Wavelength You use the Rydberg formula to calculate the wavelength, λ: $color(blue)(bar(ul(|color(white)(a/a) 1/λ = RZ^2(1/n_2^2 -1/n_1^2)color(white)(a/a)|)))" "$ where $R =$ the Rydberg constant ($1.097 × 10^7color(white)(l)...
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How do we work out the frequency of transition for an electronic transition of the hydrogen ATOM, whose electron jumps from $n=2$ to $n=5$?
And for this process we use the , $1/lambda_("vacuum")=R{1/(1/n_1^2-1/n_2^2)}$,......... ......where $R="the Rydberg constant,"$ $1.097 xx 10^7 *m^(−1);$ $n_1=2, n_2=5$........ $1/lambda_("vacuum")=1.097xx10^7*m^-1{1/(1/2^2-1/5^2)}$ $1/lambda_("vacuum")=1.097xx10^7*m^-1{1/(1/4-1/25)}=52238095.2*m^-1$ And thus $lambda=8.90xx10^-8*m$, if I have done my...
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An electron in a hydrogen atom drops from energy level n=5 to n=3. What is the energy transition using the Rydberg equation?
The energy transition will be equal to $1.55 * 10^(-19)"J"$. So, you know your energy levels to be n = 5 and n = 3. Rydberg's equation will allow...
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A photon on a hydrogen atom excited an electron from $n = 1$ to make a transition to $n=3$. What is the wavelength (in run) pertaining to this transition and was the transition emitting or absorbing in nature?
In order to solve this question we will use the Bohr Model. The change in energy according to Bohr can be calculated by: $DeltaE=-2.178xx10^(-18)Z^(2)J(1/(n_("final")^2)-1/(n_("initial")^2))$ Here, the initial level is $n_("initial")=1$...
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What is the difference in energy between the lowest energy state of the
hydrogen atom, and the next higher energy level (i.e. the difference in energy
between the 2 lowest energy states)?
As a preface, since you have asked for the "difference in energy", I will give an answer that has no sign. That is, I will give $|DeltaE|$, a magnitude....
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An electron in a mercury atom jumps from level $a$ to level $g$ by absorbing a single photon. How do you determine the energy of the photon in joules?
Relativistic effects are present here... but I assume that the transition from level $a$ to level $g$: has $DeltaL = pm 1$ (the total change in angular momentum is...
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In a solution if substance A makes up 1%, substance B makes up 9%, substance C makes up 20% and substance D makes up 70%, which substance would generally function as the solvent?
A is the component of the solution which is present in the greatest quantity. Quantitatively the answer is within the question, substance D will be considered the solvent since it's...
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