Electron Configuration Chem Worksheet 5 6 Answer Key Introduction:
Chemistry can be a challenging subject for many students, especially when it comes to electron configuration. But understanding this topic is essential for anyone who wants to pursue a career in science or engineering. Today, we will dive into one of the most important tools for mastering electron configuration: Worksheet 5-6. This worksheet is designed to help students understand the rules for writing electron configurations and applying them to atoms and ions. In this blog post, we will provide answers to the worksheet and explain the reasoning behind each one, which will help students gain a deeper understanding of electron configuration in chemistry.
Blog Body:
Question 1: What are the electron configurations for the following elements?
a) Carbon (C) – 1s2 2s2 2p2
b) Iron (Fe) – 1s2 2s2 2p6 3s2 3p6 4s2 3d6
c) Chlorine (Cl) – 1s2 2s2 2p6 3s2 3p5
Explanation: All three of these elements have different numbers of electrons, which means they have different electron configurations. Carbon has a total of six electrons, Iron has 26 electrons, and Chlorine has 17 electrons. To write their electron configurations, we must follow the rules of the Aufbau principle, the Pauli Exclusion principle, and Hund’s rule.
Question 2: What are the electron configurations for the following ions?
a) Na+ – 1s2 2s2 2p6
b) Br− – 1s2 2s2 2p6 3s2 3p6
c) Ca2+ – 1s2 2s2 2p6 3s2 3p6
Explanation: When an atom loses or gains electrons, it becomes an ion with a new electron configuration. Na+ has lost one electron, which means it has one fewer electron than its neutral state. Br− has gained one electron, which means it has one more electron than its neutral state. Ca2+ has lost two electrons, which means it has two fewer electrons than its neutral state.
Question 3: What is the shorthand electron configuration for the following elements?
a) Nitrogen (N) – [He] 2s2 2p3
b) Bromine (Br) – [Ar] 3d10 4s2 4p5
c) Chromium (Cr) – [Ar] 3d5 4s1
Explanation: Shorthand electron configurations represent the outermost electrons of an atom or ion by using the noble gas configuration as a starting point. They help to simplify the notation for atoms that have a large number of electrons. Nitrogen’s electron configuration can be represented by the noble gas helium plus the outermost electrons. Bromine’s electron configuration can be represented by the noble gas argon plus the outermost electrons. Chromium’s electron configuration can be represented by the noble gas argon plus the outermost electrons of 3d5 and 4s1.
Question 4: What is the electron configuration for the following excited states?
a) Neon (Ne) – 1s2 2s2 2p6
b) Calcium (Ca) – 1s2 2s2 2p6 3s1 3p5 4s1
c) Iron (Fe) – 1s2 2s2 2p6 3s2 3p6 4s1 3d5
Explanation: Excited states occur when an electron is excited to a higher energy level by gaining energy through a photon or other means. Neon’s electron configuration is normally 1s2 2s2 2p6, but in its excited state, it still has the same electron configuration because none of its electrons have changed energy levels. Calcium’s electron configuration is 1s2 2s2 2p6 3s2 3p6 4s2 in its ground state, but it becomes 1s2 2s2 2p6 3s1 3p5 4s1 in its excited state because one electron has moved from the 4s subshell to the 3p subshell. Iron’s electron configuration is 1s2 2s2 2p6 3s2 3p6 4s2 3d6 in its ground state, but it becomes 1s2 2s2 2p6 3s2 3p6 4s1 3d5 in its excited state because one electron has moved from the 4s subshell to the 3d subshell.
Conclusion:
In conclusion, electron configuration is a crucial topic in chemistry that requires a thorough understanding of the rules and principles behind it. By answering the questions in Worksheet 5-6, students can learn the basics of electron configuration and how to apply these rules to different elements and ions. We hope this blog post has provided valuable insight and helped you gain a better understanding of this complex topic. With practice and determination, mastering electron configuration will become second nature, and you will be well on your way to becoming a successful chemist or engineer.
