Difference Between Px Py and Pz Orbitals

PX PY和PZ轨道之间的关键区别在于Px orbital has two lobes oriented along the x-axis and the Py orbital has two lobes oriented along the y-axis whereas, the Pz orbital has two lobes oriented along the z-axis.Therefore, the difference between Px Py and Pz orbitals arises from their orientation in space.

Anatomic orbital是一个原子核周围的区域，它具有找到电子的最高概率。原子的轨道可以是轨道，孔，d轨道或轨道。此外，有三个P轨道；它们是PX，PY和PZ轨道。

内容

1.Overview and Key Difference
2.What is a Px Orbital
3.What is a Py Orbital
4.What is a Pz Orbital
5.Similarities Between Px Py and Pz Orbitals
6.Side by Side Comparison – Px vs Py vs Pz Orbitals in Tabular Form
7。概括

What is a Px Orbital?

Px orbital is one of three p orbitals and orients along the x-axis. Moreover, this orbital has two lobes and has a dumbbell shape. Quantum numbers are a set of numbers that help to name atomic orbitals. This system gives a particular atomic orbital a unique name.

量子数：

• Principle quantum number (n) describes the electron shell. Ex: n = 1, 2, 3…
• 方位角量子数或角动量量子数（L）解释了子壳。例如：l = 0、1、2…
• Magnetic quantum number (m) indicates the unique quantum state of an electron. Ex: m = …-2, -1, 0, +1, +2…
• Spin quantum number (s) describes the spin of an electron. Ex: s = ±

When considering the Px orbital, the quantum notation is as follows.

• When n=1, there are no P orbitals.
• When n > 2, and l = 1, there are p orbitals. Then, Px is either m = +1 or m = -1.
• With the increasing n values, the size of the outer lobe of the Px orbital increases gradually while the inner lobe size decrease.

What is a Py Orbital?

Py orbital is one of three p orbitals oriented along the y-axis. This orbital has two lobes. The quantum notation of Py orbital is as follows.

• When n=1, there are no P orbitals.
• When n > 2, and l = 1, there are p orbitals. Then, Py is either m = +1 or m = -1.
• With the increasing n values, the size of the outer lobe of the Py orbital increases gradually while the inner lobe size decrease.

What is a Pz Orbital?

Pz orbital is one of three p orbitals oriented along the z-axis. This orbital has two lobes and has a dumbbell shape. The quantum notation of Py orbital is as follows:

• When n=1, there are no P orbitals.
• When n > 2, and l = 1, there are p orbitals. Then, Pz is either m = 0.
• With the increasing n values, the size of the outer lobe of the Pz orbital increases gradually while the inner lobe size decrease.

What are the Similarities Between Px Py and Pz Orbitals?

• Px Py and Pz Orbitals have a similar shape (dumbbell shape).
• All three P orbitals have a similar size.
• The sizes of these orbitals change with the increase of n value.
• All three orbitals contain two lobes along the same orientation of axis.

What is the Difference Between Px Py and Pz Orbitals?

PX PY与PZ轨道
PX轨道是沿X轴面向轨道的。	Py orbital is a p orbital oriented along the y-axis.	PZ轨道是沿Z轴的P轨道。
Orientation
Along the x-axis	Along the y-axis	沿着Z轴
磁量子数（M）的值
Value for magnetic quantum number (m) is either +1 or -1.	Value for magnetic quantum number (m) is either +1 or -1	磁量子数（M）的值为0（零）

摘要 - PX PY与PZ轨道

There are three p atomic orbitals in an atom. The names Px, Py and Pz, indicate the orientation of the orbital in space. The key difference between Px Py and Pz orbitals is that Px orbital has two lobes oriented along the x-axis and Py orbital has two lobes oriented along the y-axis whereas Pz orbital has two lobes oriented along the z-axis.

Reference:

1. “Atomic Orbital.” Wikipedia, Wikimedia Foundation, 24 Apr. 2018,Available here.
2. Libretexts. “Atomic Orbitals.” Chemistry LibreTexts, Libretexts, 7 Feb. 2018,Available here.
3. Agray，Santosh。“轨道的形状。”化学桌子，Available here.

Image Courtesy:

1.”Px py pz orbitals” By CK-12 Foundation – File:High School Chemistry.pdf, page 268(CC BY-SA 3.0)viaCommons Wikimedia