1D.1

[Ayush Ray 1I]

Which of the following increase when the electron in a hydrogen atom undergoes a transition from the 1s-orbital to a 2p-orbital?
(a) Energy of the electron.
(b) Value of n.
(c) Value of l.
(d) Radius of the atom.

[Marykate Abad 3L]

All of them increase

[Ayush Ray 1I]

Why is that

[Victoria Li 1L]

Which of the following increase when the electron in a hydrogen atom undergoes a transition from the 1s-orbital to a 2p-orbital?
(a) Energy of the electron.
(b) Value of n.
(c) Value of l.
(d) Radius of the atom.

Not entirely sure, but I think all of them increase because:

(a) the electron must absorb energy to jump to a higher state/orbital.
(b) the principle quantum number, or n, describes the electron's shell e.g. 1, 2, 3 etc. Going from 1s to 2p is going up a shell.
(c) l is the angular momentum quantum number, which is also equal to n–1. So the electron went from l=0 to l=1.
(d) radius increases, because the electron went up a shell and is thus farther from the nucleus.

[Mariah]

Im kind of confused about this, what would cause an electron to transition into a higher energy level in the first place? Do they do this on their own or because of some outside force?

[Jocelyn Thorp 1A]

Im kind of confused about this, what would cause an electron to transition into a higher energy level in the first place? Do they do this on their own or because of some outside force?

they can get excited by light, and the energy from the photon allows them to make the transition.