CHEM 103 MODULE 4 EXAM 2022

CHEM 103 MODULE 4 EXAM 2022 Question 1 Click this link to access the Periodic Table. This may be helpful throughout the exam. Write the subshell electron configuration (i.e.1s2 2s2, etc.) for the Fe26 atom. Fe26 = 26 electrons = 1s2 2s2 2p6 3s2 3p6 4s2 3d6 Question 2 Click this link to access the Periodic Table.This may be helpful throughout the exam. Write the subshell electron configuration (i.e.1s2 2s2, etc.) for the S16 atom. S16 = 16 electrons = 1s2 2s2 2p6 3s2 3p4 Question 3 Click this link to access the Periodic Table.This may be helpful throughout the exam. Write the subshell electron configuration (i.e.1s2 2s2, etc.) for the P15 atom and identify which are valence (outer shell) electrons and determine how many valence electrons there are. P15 = 15 electrons = 1s2 2s2 2p6 3s2 3p3 = 5 valence electrons Question 4 Click this link to access the Periodic Table.This may be helpful throughout the exam. * For the following question, use the "Insert Math Equation" tool (indicated by the x icon on the toolbar and then choose arrows from the window which opens). Using up and down arrows, write the orbital diagram for the Ti22 atom. Ti22 = 1s2 2s2 2p6 3s2 3p6 4s2 3d2 ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑ ↑ Question 5 Click this link to access the Periodic Table.This may be helpful throughout the exam. * For the following question, use the "Insert Math Equation" tool (indicated by the x icon on the toolbar and then choose arrows from the window which opens). Using up and down arrows, write the orbital diagram for the V23 atom and identify which are unpaired electrons and determine how many unpaired electrons there are. V23 = 1s2 2s2 2p6 3s2 3p6 4s2 3d3 ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑ ↑ ↑ = 3 unpaired electrons Question 6 Click this link to access the Periodic Table.This may be helpful throughout the exam. Write the subshell electron configuration (i.e.1s2 2s2, etc.) for the Fe26 atom and then identify the last electron to fill and write the 4 quantum numbers (n, l, ml and ms) for this electron. Fe26 = 1s2 2s2 2p6 3s2 3p6 4s2 3d6 : n=3, l=2, ml = ­2, ms = ­1/2 Question 7 Click this link to access the Periodic Table.This may be helpful throughout the exam. 1. Arrange the following elements in a vertical list from smallest (top) to largest (bottom) atomic size: Cl, F, Br 2. Arrange the following elements in a vertical list from highest (top) to lowest (bottom) electronegativity: S, Si, P 3. Arrange the following elements in a vertical list from lowest (top) to highest (bottom) ionization energy: S, Te, Se Your Answer: 1. F Cl Br 2. S P Si 3. Te Se S Question 8 Click this link to access the Periodic Table.This may be helpful throughout the exam. 1. List and explain which of the following atoms forms a positive ion with more difficulty. Sn or I 2. List and explain which of the following is the smaller atom. Sn or Te 1. I forms a positive ion less easily than Sn since ionization potential increases as you go to the right in a period which means that I with the higher ionization potential requires more energy to lose an electron and form a positive ion so it does so less easily. 2. Te is smaller than Sn since atomic size decreases as you go to the right in a period which means that Te which is further to the right is smaller. Question 9 Click this link to access the Periodic Table.This may be helpful throughout the exam. On a piece of scratch paper, draw the orbital configuration of the C6 atom and use it to draw the Lewis structure for the C6 atom. Then choose the correct Lewis structure for C6 from the options listed below. C. Question 10 Click this link to access the Periodic Table.This may be helpful throughout the exam. On a piece of scratch paper, draw the orbital configuration of the As33 atom and use it to draw the Lewis structure for the As33 atom. Then choose the correct Lewis structure for the As33 from the options listed below. Your Answer: As33 = 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p3 ↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓ ↑↓ ↑↓↑↓↑↓↑↓↑↓↑↓ ↑↑↑ B