Questions tagged [atomic-structure]

For questions about the various atomic structure theories, including the Bohr theory. Not to be confused with the actual arrangement of atoms in macroscopic solids ([solid-state-chemistry]) or newer quantum concepts ([quantum-chemistry])

Filter by
Sorted by
Tagged with
1
vote
0answers
10 views

Lother Mayer curve

While studying about atomic trends, I encountered the Lothar Meyer curve: Similar graph found on internet If the covalent radius decreases across a period, why is the graph of atomic volume ...
-2
votes
1answer
40 views

Which electron should be considered the last one?

Today I came across a problem which asked some quantum number informations regarding the last electron of Zinc. Now as far as I have studied 4s subshell is filled in preference to 3d subshell bcos of ...
1
vote
0answers
32 views

Calculating electrons emitted when quantum yield is given

In a problem, the wavelength $\lambda$ of a monochromatic light, power $P$ of the source, and work function $\phi$ of the metal on which the light is shown is given. Quantum yield is $n$. I have to ...
2
votes
1answer
145 views

What is the average distance between electron 'shells' in an atom? Or between the innermost shell and the nucleus? [closed]

Somehow, I've never come across any mention of the actual, physical distances between, say the 1s and 2s shells in an atom, whether large or small.... I know that p, d and f (and g?) shells are oddly ...
1
vote
1answer
53 views

How is most probable radius in quantum mechanical model equal to Bohr's radius in hydrogen atom

Most probable radius in 1s orbital for hydrogen electron is $\pu{0.529E-10 m}$ which is Bohr radius. But energy of electron in hydrogen atom is proportional to mean radial distance in atom. In this ...
-5
votes
2answers
87 views

What would happen if the alpha particles directly hit the electrons in the gold foil in Rutherford's experiment? [closed]

What would happen if the alpha particles directly hit the electrons in the gold foil in Rutherford's experiment? Would it get ionized or is there no probability of such a thing happening ?
0
votes
1answer
73 views

What is the radial probability distribution function and what is its significance? [duplicate]

Below I have given three graphs for the $\ce{1s}$ orbital. $R(r)$ is the radial part of the wave function of the electron. $R^2(r)$ is the radial part of the wave function of the electron multiplied ...
5
votes
2answers
155 views

Why is potassium less dense than sodium?

Potassium has a density of $\pu{0.86g/cm3}$ and sodium has a density of $\pu{0.97g/cm3}$,even though potassium is below sodium and one might expect the alkali metals to exhibit monotonously increasing ...
1
vote
0answers
25 views

molecular orbital theory and crystal field theory confusions

I am a high school student and I am very confused in Molecular orbital theory, it says that when two orbitals overlaps in the same phase, they form antibonding orbitals and when they overlap in ...
2
votes
2answers
130 views

What does Bohr's model predict if the mass of an electron becomes 10 times its actual mass? [closed]

If the mass of an electron becomes 10 times its actual mass, which of the following statements is correct regarding Bohr's model: Velocity of electron increases by 10 times. Orbit radius decreases by ...
-3
votes
2answers
56 views

Will a Crooke's Tube stop working after sometime? [closed]

A Crooke's Tube is a cold-cathode tube, wherein electrons are released from the cathode when ionised gas particles strike it with speed. Following a chain reaction, other gas particles also get ...
4
votes
0answers
23 views

Practical to measure topography of a large area (mm-scale) with scanning probe microscopy (SPM)?

I'm currently very new to nanotechnology. I do understand that it is possible to achieve an excellent topography image of a sample by SPM. However, is it possible to do SPM over a large area (for ...
-5
votes
1answer
24 views

what is the use of finding out the radius of an atom [closed]

I happen to come across this, but what is the radius of an atom, velocity, KE, PE, etc.. actually used for? like the formula r=0.529n^2/z and so on
3
votes
1answer
90 views

Why is strontium(II) ion bigger than krypton atom?

$\ce{Sr^2+}$ is exactly the same as $\ce{Kr}$, in terms of electrons and orbitals. The only difference between the two, is that $\ce{Sr^2+}$ has a couple of extra protons in the nucleus (and probably ...
0
votes
0answers
68 views

Why are electrons filled in fourth shell before the third shell is filled?

I am a beginner and am learning about atomic structure and I am getting confusions regarding the aufbau principle. It is said that the electrons will be filled first in lowest available energy level. ...
3
votes
1answer
55 views

Is the effective nuclear charge only defined for valence electrons?

I've just been taught about the effective nuclear charge and screening effect in school. I'd like to ask and confirm if the effective nuclear charge is only defined for valence electrons. If not then ...
7
votes
1answer
135 views

Basics of wave-mechanical model of atom

Why is it that for the $\mathrm{d}$ subshell we have $\ \ \mathrm{d}_{xy}, \ \ \mathrm{d}_{yz}, \ \ \mathrm{d}_{xz}, \ \ \mathrm{d}_{x^{2}-y^{2}},$ and $\mathrm{d}_{z^{2}}$ orbitals only? Why aren't ...
1
vote
1answer
91 views

Excitation of electron in Niels Bohr's atomic model

Professor taught us that an electron gains or looses only those energies which are equal to difference in two energy levels. That is $E_1 + \Delta E = E_2$ or $E_1 + \Delta E = E_3.$ What if we give, ...
1
vote
2answers
147 views

Why can't the energy of an electron exceed 0 eV?

Today we were learning about atomic structure, our teacher introduced the mathematics of the 'Niels Bohr Model of Atom', and calculated the value of total energy $\frac{-13.6z^2}{n^2} \pu{eV}$. He ...
15
votes
1answer
3k views

Why does hydrogen burn with a pale blue flame while its emission spectral lines are red in colour?

I was studying oxidising flames and realized that sodium burns with a bright yellow flame the wavelength of which is around 588 nm. Then I searched for emission spectra of sodium and found that the ...
0
votes
0answers
42 views

Why is atomic mass unit/unified atomic mass defined against Carbon 12?

I have searched the web all over this question and I have not really found an answer to my satisfaction. From my understanding of the topic so far, I understand that reason why concept of unified ...
0
votes
1answer
23 views

When is the n+l rule followed when working with energy of different orbitals?

While going through my book, I came across a problem which gave some options about the order of energy of 3s, 3p and 3d orbitals of hydrogen atom. The correct answer was given as: 3s, 3p and 3d ...
3
votes
0answers
54 views

How would one separate a mixture of isotopes (different nuclear spins) at temperatures near 0 Kelvin?

Suppose we have two isotopes of the same element. For example, isotope A could have a nuclear spin I = 0, isotope B could have nuclear spin I = 3/2. Let us say we have a compound where this element is ...
3
votes
0answers
41 views

Origin of the D1 line of sodium

According to the fine structure formula for exact energies (Sommerfield formula) $$E_{jn} = -m_\mathrm{e}c^2\left[1 - \left(1 + \left[\frac{\alpha}{n - j - \frac 1 2 + \sqrt{\left(j + \frac 1 2\right)^...
4
votes
1answer
203 views

Flame Test of Alkali Metals and Alkaline Earth Metals

The flame test colors for alkali metal and alkaline earth metal salts are well known, but what about the metals themselves? Do they also give rise to the same colors (eg, brick red for Ca, pale green ...
-3
votes
1answer
57 views

I am confused with intensity of spectral lines …? [closed]

Example : FOR BALMER SERIES . HOW ? For (n2 to n1) : (2 to 1) > (3to1) > (4to 1) > (5 to 1) .....so on ......? please help me , I am unable to get that how the intensity of spectral lines ...
0
votes
0answers
37 views

Diatomic molecule under pressure

If we put a diatomic molecule under pressure the interatomic distance will be decreased and according to this graph the potential energy of the bonding molecular orbital will be increased. What will ...
-1
votes
1answer
46 views

If electrons absorb photons to reach higher energy levels in Bohr's atom, why do they have lesser kinetic energy?

In Bohr's atomic model, an electron can jump to a higher energy level by absorbing a photon with energy equal to the difference in energy between 2 energy levels. This should mean that the electron ...
0
votes
1answer
85 views

How does an electron identify whether to absorb a photon of a certain wavelength or not in absorption spectrum? [closed]

How would an electron identify the specific photons of a certain wavelength which are to be absorbed in a Hydrogen atom while creating an absorption spectrum? Well, I was thinking of it like this- Way-...
5
votes
1answer
1k views

Why is it that protons and electrons undergo the same amount of deflection in an electric field if they have the same energy?

The question I have is with respect to this diagram. Which depicts a stream of protons and electrons entering a proton field with equal energy. Why is it that in the case where the energy of protons ...
2
votes
0answers
136 views

Why does titanium have lower affinity than scandium?

Electron affinity of atoms in the same row usually increases with the atomic number until the shell or half-shell gets full, and then it drops down. Some transition metals are exceptions from the rule,...
-2
votes
1answer
66 views

Why does boron have a lower affinity than oxygen? [closed]

Electron affinity of oxygen is 141 kJ/mol and electron affinity of boron is 27 kJ/mol. I suspect it is because boron nucleus is much better shielded than oxygen nucleus (in the p-shell), but I am not ...
1
vote
2answers
84 views

Relationship between Quantum Numbers and the Wave-function

I recently started learning about quantum mechanics and its applciations in atomic structure in chemistry. In this inorganic textbook Inorganic Chemistry, it describes "Each of the wavefunctions ...
0
votes
0answers
42 views

Why does dissolved oxygen concentration decrease with increasing atomic number of metals?

I am looking at how metal ions ($\ce{Fe^2+}$, $\ce{Ni^2+}$, $\ce{Cu^2+}$, $\ce{Zn^2+}$, and $\ce{Ag+}$) affect the biochemical oxygen demand in water and used the Winkler's method to find out the ...
1
vote
1answer
47 views

Rutherford's Alpha Ray Scattering Experiment & Plum-Pudding Model

My teacher said, "Rutherford thought that all the Alpha particles would directly go through the gold foil without any collision if the plum pudding model was right. Because, as said in plum ...
0
votes
1answer
97 views

Schrodinger's Equation and Wave Function

So I understand that there exists the shrodinger's equation, which on solving,gives the wave function of an electron. The wave function as I understand, gives all possible information about an ...
-1
votes
1answer
36 views

How to explain the relation between atomic number and energy of orbitals? [closed]

I came across a certain line in my textbook that says: "As the atomic number increases the energy of orbitals decreases" Can someone please explain how this happens? My explanation is: As ...
-1
votes
1answer
80 views

Why is oxygen sp2 hybridised in acetate ion [closed]

The oxygen atom with the negative charge on the acetate ion is said to be sp2 hybridised but I can seem to figure out how I feel I may not have out much effort into this question so even a link to a ...
-2
votes
1answer
61 views

Distance of subshells from nucleus [closed]

Which subshell is more closer to the nucleus.4f or 6s? 6s gets filled first so does it have to be more closer to the nucleus?
4
votes
0answers
52 views

Did JJ Thomson know about Eugen Goldstein’s experiment discovering canal rays?

We learn that JJ Thomson discovered the electron in 1897. Several years EARLIER in 1886, Eugen Goldstein performs the same experiment but with the anode and cathode switched to produce positively ...
-1
votes
1answer
91 views

What does orbital mean, exactly? [duplicate]

My teacher told me that orbital is the probability distribution data of the electron around nucleus which is amplitude data in a way. An example of how my teacher actually told what it means involves ...
4
votes
3answers
376 views

Does electron mass decrease when it changes its orbit?

I have studied this in my chapter atomic structure that when an electron changes its orbit from lower energy to higher energy state , it does not state in my book that it moves there but that it ...
1
vote
2answers
159 views

Why isoelectronic species give similar spectral lines?

In my perspective those species should give similar spectra those which have same energy of different energy levels as the transition would yeild same energy photon But still the answer to this ...
2
votes
1answer
130 views

Do electrons of opposite spin attract each other? [closed]

Electrons of opposite spin create magnetic fields that are opposite to each other. So, is it possible that, 'such electron pairs attract each other' or ' they distract each other less than electron of ...
-1
votes
2answers
90 views

What happens if we continuously hit an atom with photons

My sir told me that Energy required to remove an electron from one orbit to another depends on hf * n. Where n means the no of photons that will strike on a metal surface and hf is energy of one ...
0
votes
1answer
87 views

What does Pauli’s exclusion principle mean in atomic or fundamental way? [closed]

It means is that no electron can have same n , l and $m_l$ but can have two different spin quantum number. I want to know why is this rule valid?Means there must be some other things happening also ...
-1
votes
1answer
26 views

Relation of Energy required to change an orbit by electron of H atom with spectrum

We have the value for expression of line spectrum of hydrogen. $\Delta E = 13.6 \cdot Z^2 \cdot \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right)$ Amount of energy required by electron to change its ...
0
votes
0answers
27 views

Finding excited stage of electron from its potential energy

The potential energy of an electron in the hydrogen atom is $\pu{-6.8 eV}.$ Indicate the excited stage in which electron is present. Total energy would be equal to $\pu{-3.4 eV}.$ I used the formula $...
0
votes
1answer
63 views

hydrogen spectrum

In the spectrum of atomic hydrogen, several lines are generally classified together as belonging to a series (for example, Balmer series, Lyman series, Paschen series), What is common to the lines ...
1
vote
0answers
67 views

Do different eigenstates of total angular momentum have necessarily different energies?

Let $H$ be the Hamiltonian of a specific atom and $J$ the total angular momentum. Since $H$ and $J$ commute, they have common eigenstate. So we can label the atomic states by their energy and total ...