1 vote
1k views

### atomic orbital probability graph for p and s orbitals [duplicate]

In the probability density graphs of s and p and even other orbitals start from nucleus as shown in the picture given below they all start from nucleus i.e. there is good probability of electrons of ...
• 363
70 views

### Non-mathematical explanation for why the 3d orbital generally has higher energy than the 3p orbital [duplicate]

Why does the angular momentum of orbitals(l) affect the orbital's energy? Please provide a qualitative answer.
• 21
111k views

### What is the inert pair effect?

I was reading about the p-block elements and found that the inert pair effect is mentioned everywhere in this topic. However, the book does not explain it very well. So, what is the inert pair effect? ...
• 577
8k views

### How do orbitals coexist with a nucleus?

Many diagrams of orbitals I've seen involve electrons moving through a center point—where the nucleus is. How can this be? Clearly they don't actually pass through the nucleus, so what does happen?
• 827
83k views

### Why is the vanadium(3+) ion paramagnetic?

I know that the electron configuration of vanadium is $[\ce{Ar}]\mathrm{4s^2 3d^3}$. None of the electrons in the 3d subshell are paired. Once it loses these three electrons, shouldn't the remainder ...
• 1,105
8k views

### Difference between actual position of electron and Radial Distribution Probability

Its known that the radius of maximum probability of 2s orbitals is more than that of 2p orbitals. It means that the maximum probability of finding an electron in an 2s is further away from electron ...
• 749
17k views

### Why are all the orbitals that have the same principal number in Hydrogen degenerate?

In hydrogen, all orbitals with the same principal quantum number 'n' (1,2,3...) are degenerate, regardless of the orbital angular momentum quantum number'l' (0,1...n-1 or s,p,d..). However, in atoms ...
• 9,804
2k views

### How are subshells and shells arranged in an atom?

If $\mathrm{2s}$ and $\mathrm{2p}$ are in the second energy level, and $\mathrm{3s}$, $\mathrm{3p}$, and $\mathrm{3d}$ are in the next (3rd) energy level, how are these subshells arranged in space in ...
• 41
1k views

### Are empty orbitals degenerate?

This is apparently a true statement: "In a hydrogen atom, the 2s and 2p subshells have the same energy." Why is this the case? Why would they be of the same energy? Wouldn't the 2p be slightly ...
• 19k
2k views

### Why are s orbitals more “penetrating” than p orbitals?

In polyelectronic atoms, the reduction in the net central force due to electron-electron repulsion is accounted for through an effective nuclear charge that depends on a “shielding effect” of inner ...
1 vote
2k views

### Why does a neutral atom of beryllium not have any electrons in a p orbital?

Here's what I understand about quantum number and orbitals, please correct me if anything is wrong: Electrons enter into these different types of orbitals because they have a higher/lower amount of ...
• 31
2k views

### What is the correct order of subshell energies? [duplicate]

I was taught in high school that the order is given by the Aufbau Principle: 1s>2s>2p>3s>3p>4s>3d>4p>5s>4d>5p>6s>4f>5d>6p... Why is the 3d subshell higher in energy than the 4s subshell if it is in a ...
• 143
179 views

### Are the electrons in an atom always 'locked' with their proton?

Suppose you have a single atom, say carbon, carbon has six electrons, and six protons. Now is there anything associating the six protons locking the six electrons other than coulombic forces? When we ...
• 426
485 views

### Does the radius of the atom change when an electron is excited?

The radius of the atom increases when the electron in a hydrogen atom undergoes a transition from the 1s-orbital to a 2p-orbital. How is this possible? Why does exciting an electron to a higher ...
• 2,079