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Chapter 7: Problem 20

Is the following statement true or false? The hydrogen atom has a 3s orbital. Explain.

Short Answer

Expert verified
The statement "The hydrogen atom has a 3s orbital" is false. The hydrogen atom has only one electron, which occupies the 1s orbital, and does not have any electrons in higher energy level orbitals, such as the 3s orbital.

Step by step solution

01

Understand Atomic Orbitals

An atomic orbital is a mathematical function that describes the behavior of electrons in atoms. Atomic orbitals can be classified based on their energy levels and shapes, using the quantum numbers n, l, and m. The principal quantum number (n) represents the energy level and size of the orbital. The angular momentum quantum number (l) represents the shape of the orbital. For a given energy level n, the value of l can range from 0 to (n-1). When l = 0, it is referred to as an s-orbital, which is spherical in shape.
02

Analyze the Hydrogen Atom

The hydrogen atom has only one electron in its simplest form. The electron configuration for a hydrogen atom can be represented as 1s¹, meaning that its one electron resides in the 1s orbital.
03

Evaluate the Statement

The statement "The hydrogen atom has a 3s orbital" implies that the hydrogen atom has an electron in the 3s orbital. Since hydrogen has only one electron and it occupies the 1s orbital (lowest energy level), the hydrogen atom does not have an electron in the 3s orbital.
04

Conclusion

The statement "The hydrogen atom has a 3s orbital" is false. The hydrogen atom has only one electron, which occupies the 1s orbital, and does not have any electrons in higher energy level orbitals, such as the 3s orbital.

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Most popular questions from this chapter

The Heisenberg uncertainty principle can be expressed in the form $$\Delta E \cdot \Delta t \geq \frac{h}{4 \pi}$$ where \(E\) represents energy and \(t\) represents time. Show that the units for this form are the same as the units for the form used in this chapter: $$\Delta x \cdot \Delta(m v) \geq \frac{h}{4 \pi}$$

Which of the following electron configurations correspond to an excited state? Identify the atoms and write the ground-state electron configuration where appropriate. a. 1\(s^{2} 2 s^{2} 3 p^{1}\) b. 1\(s^{2} 2 s^{2} 2 p^{6}\) c. 1\(s^{2} 2 s^{2} 2 p^{4} 3 s^{1}\) d. \([\mathrm{Ar}] 4 s^{2} 3 d^{5} 4 p^{1}\) How many unpaired electrons are present in each of these species?

An ionic compound of potassium and oxygen has the empirical formula KO. Would you expect this compound to be potassium(II) oxide or potassium peroxide? Explain.

Element 106 has been named seaborgium, Sg, in honor of Glenn Seaborg, discoverer of the first transuranium element. a. Write the expected electron configuration for element 106. b. What other element would be most like element 106 in its properties? c. Predict the formula for a possible oxide and a possible oxyanion of element 106.

The wave function for the 2\(p_{z}\) orbital in the hydrogen atom is $$\psi_{2 p_{z}}=\frac{1}{4 \sqrt{2 \pi}}\left(\frac{Z}{a_{0}}\right)^{3 / 2} \sigma \mathrm{e}^{-\sigma / 2} \cos \theta$$ where \(a_{0}\) is the value for the radius of the first Bohr orbit in meters \(\left(5.29 \times 10^{-11}\right), \sigma\) is \(Z\left(r / a_{0}\right), r\) is the value for the distance from the nucleus in meters, and \(\theta\) is an angle. Calculate the value of \(\psi_{2 p_{z}}^{2}\) at \(r=a_{0}\) for \(\theta=0^{\circ}\left(z \text { axis ) and for } \theta=90^{\circ}\right.\) (xy plane).
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