Question

What is incorrect about this orbital
diagram?
1s
2s
2p
tilt
(A)
Both arrows in the 2p box should
be pointing up
(B)
There is nothing incorrect with this
diagram
In the 2p box there should only be
I electron in the first 2p box and
one in the 2nd 2p box
(D)
All the arrows should be pointing
up​

Answer 1

Answer:

D

Explanation:

all the arrows should be pointing up is not true

Answer 2

Answer:

(D)

(D)All the arrows should be pointing up.

Explanation:

orbital diagram:

Orbital diagrams are pictorial descriptions of the electrons in an atom. Three rules are useful in forming orbital diagrams. According to the Auf Bau Principle, each electron occupies the lowest energy orbital. The Pauli Exclusion Principle says that only two electrons can fit into an single orbital.

"There are four basic types of orbitals: s, p, d, and f. An s orbital has a spherical shape and can hold two electrons.

"There is 1 orbital in the 1s sublevel.

A p orbital has the approximate shape of a pair of lobes on opposite sides of the nucleus, or a somewhat dumbbell shape. An electron in a p orbital has equal probability of being in either half.

"There is only one orbital in the 2s subshell. But, there are three orbitals in the 2p subshell because there are three directions in which a p orbital can point."

"We have the "p" shape. There are three 2p orbitals and they are all oriented perpendicular to each other.

"When assigning electrons to orbitals, we must follow a set of three rules: the Aufbau Principle, the Pauli-Exclusion Principle, and Hund's Rule".

The project code is #SPJ3