Electron Configurations of Atoms flash/atomic_electron_configurations_s1.swf q0 sim s1 q0 q1 sim s2 q1 q2 sim s3 q2 q3 sim s4 q3 q4 sim s5 q4 q5 sim s6 q5 q6 sim s7 q6 q7 sim s8 q7 q8 sim s9 q8 q9 sim s10 q9 q10 sim s11 q10 q11 sim s12 q11 q12 sim s13 q12 q13 sim q13 INTRODUCTION The orbitals that electrons occupy in a multielectron atom in the ground state define an atom's electron configuration. Electron configurations are determined by assigning electrons to available orbitals to give the lowest energy configuration. This simulation displays the electron configurations for the elements in relation to the element’s position on the periodic table. To use the simulation, click on an element in the periodic table. The electron configuration will be displayed in the “box” or “dash” notation as well as in the noble gas notation. QUESTION 1 OF 12 Examine the electron configurations of the alkali metals of Group 1A. Which type of orbital does the electron highest on the filling diagram occupy? s p d f 0 1 standard %CORRECT% Alkali metals in Group 1A all have electron configurations with a single electron in the highest s orbital. %INCORRECT% Choose the elements H, Li, Na, K, etc. Examine the highest orbital that is occupied by at least one electron. QUESTION 2 OF 12 Now examine the electron configurations of the alkaline earth metals of Group 2A. Which type of orbital is the highest filled of these elements? s p d f 0 1 standard %CORRECT% Alkaline earth metals in Group 2A all have electron configurations with their highest s orbitals filled with two electrons. %INCORRECT% QUESTION 3 OF 12 Now examine the elements moving left to right from B to Ne. What subshell is being filled moving through these elements? 2p 0.0 false standard %CORRECT% When moving across the periodic table from B to Ne, each additional electron is added to a 2p orbital. %INCORRECT% Enter a subshell name such as 1s, 3p, or 3d. QUESTION 4 OF 12 What subshell is being filled between Al and Ar? 3p 0.0 false standard %CORRECT% All the elements in periodic groups 3A - 8A have their highest electrons filling p orbitals. %INCORRECT% QUESTION 5 OF 12 What orbital type is filled throughout the transition metal B Groups? s p d f 2 1 standard %CORRECT% The transition metals are often referred to as “d-group” elements. %INCORRECT% QUESTION 6 OF 12 What types of orbitals are filled throughout the Lanthanide and Actinide series? s p d f 3 1 standard %CORRECT% Elements in the two series separated out at the bottom of the periodic table are associated with filling f orbitals. %INCORRECT% The Lanthanide and Actinide series are the two rows separated out at the bottom of the periodic table. QUESTION 7 OF 12 The periodic table is often considered to be formed of separate “blocks,” based on the types of orbitals filled in each region. Click on an element within the s-block of the periodic table. sim 1A,2A 1 standard %CORRECT% Groups 1A and 2A comprise the s-block. %INCORRECT% QUESTION 8 OF 12 Click on a p-block element. sim 3A,4A,5A,6A,7A,8A 1 standard %CORRECT% The right side of the periodic table comprising Groups 3A - 8A make up the p-block. %INCORRECT% QUESTION 9 OF 12 Click on a d-block element. sim 1B,2B,3B,4B,5B,6B,7B,8B 1 standard %CORRECT% The central portion of the periodic table comprising Groups 3B - 2B make up the d-block. %INCORRECT% QUESTION 10 OF 12 Click on a f-block element. sim f-block 1 standard %CORRECT% The Lanthanides and Actinides make up the f-block. %INCORRECT% QUESTION 11 OF 12 Consider the width of each block and its relation to the subshell being filled. Complete the table to the right. 1 0.0 false 3 0.0 false 5 0.0 false 7 0.0 false 2 0.0 false 6 0.0 false 10 0.0 false 14 0.0 false standard %CORRECT% Notice that the number of elements across each block is twice the number of orbitals filled in the subshell. %INCORRECT% QUESTION 12 OF 12 Finally, consider the manner in which a subshell is filled. Move across the p-block from B to Ne. Indicate whether each of the following statements is true or false. A. Each orbital fills with two electrons before the next is filled with a single electron. B. Electrons "spread out" into different orbitals before pairing up into individual orbitals. C. Electrons fill orbitals with the same spin before "spin pairing." true false 1 2 true false 0 2 true false 0 2 standard %CORRECT% This is a summary of Hund’s Rule. %INCORRECT% SUMMARY An element’s electron configuration is directly related to that element’s position on the periodic table. The highest occupied orbitals are identified by the “block” in which the element lies on the table. The electron configuration can be summarized by “walking through” the table, filling each subshell in order until reaching the element.