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Chapter 4: Problem 126

Draw an s orbital, a \(p\) orbital, and a \(d\) orbital.

Short Answer

Expert verified
An s orbital is a sphere with the nucleus at the center. A p orbital is dumbbell-shaped, with two lobes on opposite sides of the nucleus (e.g., a \(p_z\) orbital has lobes along the z-axis). A d orbital has a cloverleaf-like shape, with four lobes arranged around the nucleus (e.g., a \(d_{xy}\) orbital has lobes aligned with the x and y axes).

Step by step solution

01

Drawing an s Orbital

An s orbital is spherical in shape, with the nucleus at the center. It represents the most basic and symmetric atomic orbital. To draw an s orbital: 1. Draw a small circle to represent the nucleus of the atom. 2. Draw a larger circle surrounding the nucleus to represent the boundary of the spherical s orbital. 3. Shade in the area between the nucleus and the larger circle to represent the electron cloud, where the electron has a high probability of being found.
02

Drawing a p Orbital

A p orbital is shaped like a dumbbell, with two lobes on opposite sides of the nucleus. There are three p orbitals, \(p_x\), \(p_y\), and \(p_z\), which are oriented along the x, y, and z axes, respectively. In this step, we will draw a \(p_z\) orbital: 1. Draw a small circle to represent the nucleus of the atom. 2. Draw two oval or egg-shaped lobes, one above and one below the nucleus, along the vertical z-axis. 3. Shade in the two lobes to represent the electron cloud, where the electron has a high probability of being found.
03

Drawing a d Orbital

A d orbital has a cloverleaf-like shape, with four lobes arranged around the nucleus. There are five d orbitals, which are more complex than the s or p orbitals. In this step, we will draw a \(d_{xy}\) orbital: 1. Draw a small circle to represent the nucleus of the atom. 2. Draw four oval or egg-shaped lobes, arranged in an "X" shape around the nucleus, with each lobe in a different quadrant. The lobes should be aligned with the x and y axes. 3. Shade in the four lobes to represent the electron cloud, where the electron has a high probability of being found.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

s Orbital
The s orbital is the simplest atomic orbital, known for its spherical symmetry around an atom's nucleus. It is the starting point for understanding electron arrangement in atoms. Imagine the nucleus is the sun, and the s orbital is a planet's spherical atmosphere. Electrons within this 'atmosphere' move freely and are equally likely to be found in any direction from the center.

The s orbital can hold up to two electrons, which together fill the first shell of an atom. This first shell is often visualized as a cloud, densest at the center and thinning out with distance, symbolizing the probability of locating an electron.
p Orbital
Stepping up in complexity, the p orbital has a distinctive dumbbell shape, extending along one axis with two lobes on either side of the nucleus. The p orbitals define the second and higher energy levels of atoms, and there are three varieties corresponding to the x, y, and z axes—named px, py, and pz orbitals.

Unlike s orbitals, the shape of p orbitals means there are regions of space—between the lobes—where the probability of finding an electron is zero, known as nodal planes. The spatial orientation of these orbitals dictates much of the chemical bonding and molecular shape theories in chemistry.
d Orbital
More complex still, d orbitals introduce even more elaborate geometries into atomic structure. They possess a four-lobed cloverleaf pattern or, in some cases, a dumbbell with a doughnut-shaped ring around the middle. Each of the five d orbitals—dxy, dxz, dyz, dx2-y2, and dz2—has its unique orientation in 3D space.

These orbitals are significant for elements in the middle of the periodic table, especially transition metals, influencing properties like magnetism, color, and chemical reactivity.
Electron Cloud
The concept of the electron cloud is a cornerstone of modern chemistry and atomic physics. It visualizes the regions in space where there is a high probability of finding an electron around the nucleus. This model moves away from the idea of electrons as particles in fixed orbits, instead embracing quantum mechanics, which describes electrons in terms of probabilities.

The cloud's density reflects where an electron is more likely to be; closer to the nucleus, the cloud is denser. Understanding this concept is vital for grasping how chemical bonds form and why atoms interact in certain patterns.
Atomic Nucleus
At the heart of every atom is the atomic nucleus, a dense core composed of protons, with a positive charge, and neutrons, which are neutral. The intriguing dance of electrons in orbitals occurs all around this central nucleus. Despite its tiny size, the nucleus contains the majority of an atom's mass.

It's the number of protons in the nucleus that determines an element's identity—a concept known as the atomic number. Moreover, the strong nuclear forces binding protons and neutrons in the nucleus contrast sharply with the comparatively vast and less dense electron cloud surrounding them.

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Most popular questions from this chapter

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