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Chapter 5: Problem 44

Use the sublevel blocks on the periodic table to write an abbreviated electron configuration for an atom of each of the following: a. vanadium b. palladium c. zinc d. cesium

Short Answer

Expert verified
Vanadium: [Ar] 4s虏 3d鲁, Palladium: [Kr] 4d鹿鈦�, Zinc: [Ar] 4s虏 3d鹿鈦�, Cesium: [Xe] 6s鹿.

Step by step solution

01

Understand Electron Configuration

Electron configuration describes the distribution of electrons in the atomic orbitals of an atom. The periodic table can be divided into blocks corresponding to the energy sublevels being filled: s, p, d, and f.
02

Locate Each Element on the Periodic Table

Identify the position of each element (vanadium, palladium, zinc, and cesium) on the periodic table to determine their atomic numbers and the orbitals filling sequence.
03

Vanadium (V)

Vanadium has an atomic number of 23. Using the sequence of filling: 1s, 2s, 2p, 3s, 3p, 4s, 3d,..., the electron configuration for vanadium is: 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鲁. The abbreviated electron configuration is [Ar] 4s虏 3d鲁.
04

Palladium (Pd)

Palladium has an atomic number of 46. Following the electron filling sequence: 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦� 4p鈦� 5s虏 4d鈦� (by considering stability it completes 4d). The abbreviated electron configuration is [Kr] 4d鹿鈦�.
05

Zinc (Zn)

Zinc has an atomic number of 30. Using the sequence of filling: 1s, 2s, 2p, 3s, 3p, 4s, 3d, the electron configuration for zinc is: 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦�. The abbreviated electron configuration is [Ar] 4s虏 3d鹿鈦�.
06

Cesium (Cs)

Cesium has an atomic number of 55. Use the filling sequence to write its electron configuration: 1s虏 2s虏 2p鈦� 3s虏 3p鈦� 4s虏 3d鹿鈦� 4p鈦� 5s虏 4d鹿鈦� 5p鈦� 6s鹿. The abbreviated electron configuration is [Xe] 6s鹿.

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Key Concepts

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

periodic table
The periodic table is a powerful tool for understanding elements and their properties.
It organizes elements by increasing atomic number, which is the number of protons in an atom's nucleus.
The table is divided into blocks鈥攕, p, d, and f鈥攂ased on the energy sublevels being filled with electrons. The table's structure helps predict the chemical behavior of elements.
atomic orbitals
Atomic orbitals are regions around an atom's nucleus where electrons are likely found.
These orbitals include the s, p, d, and f sublevels.
Each has a unique shape and energy level.
  • s orbitals are spherical.
  • p orbitals are dumbbell-shaped.
  • d and f orbitals have more complex shapes.
Understanding these shapes is crucial for grasping how atoms bond and interact.
abbreviated electron configuration
An abbreviated electron configuration shortens the full electron configuration.
It uses the nearest noble gas symbol in brackets to represent filled electron shells.
For example, the configuration for zinc (Zn) with atomic number 30 is [Ar] 4s虏 3d鹿鈦�.
This method saves time and simplifies complex configurations, making it easier to understand and write.
electron filling sequence
The electron filling sequence or Aufbau principle determines how electrons populate atomic orbitals.
Electrons fill orbitals starting from the lowest energy level to the highest.
The sequence typically follows: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p...
This sequence is essential for writing correct electron configurations.
atomic number
The atomic number of an element is the count of protons in its nucleus.
It is unique to each element and determines its position on the periodic table.
For instance, vanadium (V) has an atomic number of 23.
Knowing an element鈥檚 atomic number is crucial for finding its electron configuration and understanding its chemical properties.

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Most popular questions from this chapter

Place the following types of electromagnetic radiation in order of decreasing wavelengths: FM radio station, red color in neon lights, and cell phone.

Select the more metallic element in each pair. \((5.6)\) a. P or \(\mathrm{Bi}\) b. \(\mathrm{S}\) or \(\mathrm{Te}\) c. Rb or In d. Li or Ne

Place the following in order of increasing metallic character: Na, P, Al, Ar

Write the group number using both \(\mathrm{A} / \mathrm{B}\) and 1 to 18 notations for elements that have the following outer electron configuration: a. \(2 s^{2}\) b. \(3 s^{2} 3 p^{3}\) c. \(4 s^{2} 3 d^{5}\) d. \(5 s^{2} 4 d^{10} 5 p^{4}\)

Which of the following orbitals are not possible in an atom: \(3 f\), \(4 p, 5 d\), and \(6 p ?(5.3)\)
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