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Chapter 5: Problem 109

Write the abbreviated electron configuration and group number for each of the following elements: \((5.4)\) a. \(\mathrm{Zn}\) b. I c. V d. Sr

Short Answer

Expert verified
Zn: [Ar] 4s虏 3d鹿鈦�, Group 12; I: [Kr] 5s虏 4d鹿鈦� 5p鈦�, Group 17; V: [Ar] 4s虏 3d鲁, Group 5; Sr: [Kr] 5s虏, Group 2.

Step by step solution

01

Understanding Electron Configuration

Elements are represented by their atomic number, which determines the electron configuration. Electrons fill orbitals following the pattern: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, and so on. For abbreviated configurations, we start from the nearest previous noble gas.
02

Abbreviated Electron Configuration for \(\text{Zn}\)

Zinc (Zn) has an atomic number of 30. The nearest previous noble gas is Argon (Ar), which has an atomic number of 18. Therefore, the configuration is: \[ \text{[Ar]} 4s^2 3d^{10} \] Zinc belongs to Group 12.
03

Abbreviated Electron Configuration for \(\text{I}\)

Iodine (I) has an atomic number of 53. The nearest previous noble gas is Krypton (Kr), which has an atomic number of 36. Therefore, the configuration is: \[ \text{[Kr]} 5s^2 4d^{10} 5p^5 \] Iodine belongs to Group 17.
04

Abbreviated Electron Configuration for \(\text{V}\)

Vanadium (V) has an atomic number of 23. The nearest previous noble gas is Argon (Ar), which has an atomic number of 18. Therefore, the configuration is: \[ \text{[Ar]} 4s^2 3d^3 \] Vanadium belongs to Group 5.
05

Abbreviated Electron Configuration for \(\text{Sr}\)

Strontium (Sr) has an atomic number of 38. The nearest previous noble gas is Krypton (Kr), which has an atomic number of 36. Therefore, the configuration is: \[ \text{[Kr]} 5s^2 \] Strontium belongs to Group 2.

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Key Concepts

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

Electron Orbitals
Electron orbitals are regions of space around the nucleus where electrons are most likely to be found. Electrons occupy orbitals in a specific order based on increasing energy levels.
The main types of orbitals include:
  • s-orbitals: can hold up to 2 electrons and have a spherical shape
  • p-orbitals: can hold up to 6 electrons and have a dumbbell shape
  • d-orbitals: can hold up to 10 electrons and have a more complex shape
  • f-orbitals: can hold up to 14 electrons and have an even more complex shape

The sequence in which these orbitals are filled follows the pattern: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, and so forth. This filling order is determined by the Aufbau principle, which states electrons fill the lowest energy orbitals first.
When writing an electron configuration, each occupied orbital and the number of electrons in it is noted. For example, the electron configuration of Carbon (atomic number 6) is 1s2 2s2 2p2, indicating 2 electrons in the 1s orbital, 2 in the 2s orbital, and 2 in the 2p orbital.
Atomic Number
The atomic number of an element is the number of protons in its nucleus. It is unique to each element and determines its position in the periodic table. Because atoms are electrically neutral, the number of electrons in an atom is equal to its atomic number.
Atomic numbers are significant because they define the chemical properties of an element and distinguish one element from another. For instance, Hydrogen has an atomic number of 1, while Helium has an atomic number of 2.
During electron configuration, we use the atomic number to determine the total number of electrons. As we see in the exercise above:
  • Zinc (Zn) has an atomic number of 30, so it has 30 electrons.
  • Iodine (I) has an atomic number of 53, so it has 53 electrons.
  • Vanadium (V) has an atomic number of 23, so it has 23 electrons.
  • Strontium (Sr) has an atomic number of 38, so it has 38 electrons.
Noble Gases
Noble gases are a group of elements in Group 18 of the periodic table. They are highly stable due to their full valence electron shell, which reduces their tendency to react with other elements.
The noble gases include: Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), and Radon (Rn).
In electron configurations, noble gases are used as a shorthand to simplify complex configurations. This is known as the abbreviated electron configuration, where the symbol of the nearest preceding noble gas is used to represent all the electron configuration up to that point. For example:
  • For Zinc (Zn): [Ar] 4s2 3d10. Here, Argon (Ar) represents the configuration up to the 18th electron.
  • For Iodine (I): [Kr] 5s2 4d10 5p5. Here, Krypton (Kr) represents the configuration up to the 36th electron.
  • For Vanadium (V): [Ar] 4s2 3d3. Again, Argon (Ar) stands for the configuration until the 18th electron.
  • For Strontium (Sr): [Kr] 5s2. Krypton (Kr) represents all configurations up to the 36th electron.
This method drastically reduces the complexity involved in writing electron configurations for elements with a large number of electrons.

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Most popular questions from this chapter

Select the element in each pair with the higher ionization energy. a. \(\mathrm{O}\) or \(\mathrm{Ne}\) b. \(\mathrm{K}\) or \(\mathrm{Br}\) c. \(\mathrm{Ca}\) or \(\mathrm{Ba}\) d. \(\mathrm{N}\) or \(\mathrm{Ne}\)

a. What is the atomic number of In? b. How many electrons are in an atom of In? c. Use the sublevel blocks on the periodic table to write the electron configuration and abbreviated electron configuration for an atom of In. d. Write the group number and draw the Lewis symbol for In. e. Which is larger, an atom of indium or an atom of iodine? f. Which has a higher ionization energy, an atom of indium or an atom of iodine?

Give the symbol of the element with each of the following electron or abbreviated electron configurations: a. \(1 s^{2} 2 s^{2} 2 p^{4}\) b. \([\mathrm{Ne}] 3 s^{2}\) c. \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}\) d. \([\mathrm{Ne}] 3 s^{2} 3 p^{1}\)

Consider three elements with the following abbreviated electron configurations: \((5.4,5.5,5.6)\) \(\mathrm{X}=[\mathrm{Ar}] 4 s^{2} \quad \mathrm{Y}=[\mathrm{Ne}] 3 s^{2} 3 p^{4} \quad \mathrm{Z}=[\mathrm{Ar}] 4 s^{2} 3 d^{10} 4 p^{4}\) a. Identify each element as a metal, nonmetal, or metalloid. b. Which element has the largest atomic size? c. Which element has the highest ionization energy? d. Which element has the smallest atomic size?

Complete each of the following statements a to d using 1,2 , or 3 : 1\. decreases 2\. increases 3\. remains the same Going from left to right across Period 3 , a. the ionization energy b. the atomic size c. the metallic character d. the number of valence electrons
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