Understanding electron configuration is a fundamental aspect of chemistry that lays the groundwork for comprehending the behavior of elements and their interactions. Chemistry Worksheet 5 and 6 delve into the intricacies of electron configuration, providing a valuable opportunity to solidify your knowledge. In this comprehensive guide, we will not only furnish you with the answer key to these worksheets but also provide insightful explanations to ensure you grasp the underlying concepts.
Table of Contents
- Introduction to Electron Configuration
- Chemistry Worksheet 5: Answer Key and Explanations
- Chemistry Worksheet 6: Answer Key and Explanations
- Practical Applications of Electron Configuration
- Conclusion
1. Introduction to Electron Configuration
Before we dive into the answer key for Chemistry Worksheet 5 and 6, let’s establish a clear understanding of electron configuration. In essence, electron configuration refers to the arrangement of electrons within an atom. Electrons occupy different energy levels or shells, and each energy level has a specific number of subshells, which further contain orbitals.
2. Chemistry Worksheet 5: Answer Key and Explanations
Chemistry Worksheet 5 focuses on applying the principles of electron configuration to elements. Here are the answers along with explanations for some select questions:
Question 1: Write the electron configuration for oxygen (O).
Answer: 1s² 2s² 2p⁴. Explanation: Oxygen has 8 electrons. The electron configuration follows the pattern of filling the 1s orbital first, then the 2s orbital, and finally, the 2p orbitals.
Question 5: How many unpaired electrons are there in a phosphorus (P) atom?
Answer: 3. Explanation: The electron configuration of phosphorus is 1s² 2s² 2p⁶ 3s² 3p³. There are three unpaired electrons in the 3p subshell.
Question 8: What is the electron configuration of chromium (Cr)?
Answer: [Ar] 3d⁵ 4s¹. Explanation: Chromium’s electron configuration is an exception due to its stability. It is more stable to have a half-filled d subshell (3d⁵) and a singly filled s subshell (4s¹) rather than having a completely filled 4s subshell.
3. Chemistry Worksheet 6: Answer Key and Explanations
Chemistry Worksheet 6 delves into more complex electron configuration scenarios and introduces the concept of Hund’s rule. Here are the answers and explanations for a few questions:
Question 2: Write the electron configuration for nickel (Ni).
Answer: [Ar] 3d⁸ 4s². Explanation: Nickel’s electron configuration fills the 3d subshell with 8 electrons and the 4s subshell with 2 electrons.
Question 4: Using Hund’s rule, explain why the 3p subshell is singly occupied in phosphorus (P) electron configuration.
Answer: According to Hund’s rule, electrons prefer to occupy empty orbitals within the same energy level before pairing up. In the case of phosphorus, placing three electrons in separate 3p orbitals maximizes the number of half-filled orbitals, leading to greater stability.
Question 6: How does the electron configuration of cation differ from its neutral atom?
Answer: Cations have fewer electrons than their neutral atoms. Electrons are removed from the highest energy level (outermost shell) first. For example, the electron configuration of a sodium (Na) cation is 1s² 2s² 2p⁶.
4. Practical Applications of Electron Configuration
Understanding electron configuration has far-reaching implications across various scientific and industrial domains:
- Periodic Trends: Electron configuration elucidates periodic trends, such as ionization energy and atomic size, which are crucial for predicting and explaining element behaviors.
- Chemical Bonding: Electron configuration guides the formation of chemical bonds and helps explain the stability of different compounds.
- Spectroscopy: Electron configuration is integral to interpreting spectroscopic data, enabling scientists to identify elements and study their properties.
5. Conclusion
Mastery of electron configuration is pivotal in unraveling the intricacies of the chemical world. Chemistry Worksheet 5 and 6 have provided us with a platform to solidify our comprehension. By grasping the nuances of electron arrangement and Hund’s rule, you have taken a significant step toward comprehending the behavior of elements and their interactions. Remember, electron configuration is not merely a theoretical concept; it underpins the very foundation of chemistry, enabling us to make sense of the diverse and wondrous array of elements that constitute our universe.
