Activity 2.1: Electron Configuration and Orbital Diagrams Directions: Write the complete electron configuration of the following elements and draw their orbital diagrams. State whether the element is paramagnetic or diamagnetic. The first one is done for you. Number Magnetic Property Element of Electron Orbital Diagram electrons Configuration 1レ 1 Lithium 3 Paramagnetic 1s22s1 1s 2s 2p 3s Oxygen Fluorine Bromine Silicon Zinc

Activity 2.1: Electron Configuration and Orbital Diagrams Directions: Write the complete electron configuration of the following elements and draw their orbital diagrams. State whether the element is paramagnetic or diamagnetic. The first one is done for you. Number Magnetic Property Element of Electron Orbital Diagram electrons Configuration 1レ 1 Lithium 3 Paramagnetic 1s22s1 1s 2s 2p 3s Oxygen Fluorine Bromine Silicon Zinc

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Using the graph of successive ionization energies what element could the graph represent? Al Si CI Ionization Energy (kJ/mol) 35000 30000 25000 20000 15000 10000 5000 0 IE1 IE2 Successive lonization Energies IE3 IE4 IES IE6 IE7 Briefly explain how you knew which element the graph represented? Make sure to discuss core and valence electrons and relative energies. B I U X2 X2 IE8
Shown below is a representation of part of an orbital energy diagram (using parentheses and arrows to represent orbitals and electrons).Write the set of quantum numbers for each of the electrons that have been circled. -1 0 +1 5p
Each of the statements below attempts to explain why some periodic property varies predictably among elements in the periodic table. Determine if each statement is true or false. Within a period, elements with higher atomic numbers have atoms of smaller radius because the valance electrons are in higher principal energy levels. Within a family, elements with higher atomic numbers have lower ionization energy because the valance electrons are in higher principal energy levels. Within a period, elements with higher atomic numbers have higher ionization energy because the valance electrons are in higher principal energy levels. Within a family, elements with higher atomic numbers have higher electronegativity because the atoms have higher effective nuclear charge. Within a period, elements with lower atomic numbers require more energy to remove an electron from the atom, because the valance electrons are in higher principal energy levels. Within a period, elements with lower atomic…
1. Fill in the electron configurations for the elements given in the table. Use the orbital filling diagram to complete the table.. Element 14 Electron Configurations for Some Selected Elements Orbital filling 1s 2s 2p, 2p, 2p, 38 CI Electron configuration 1s 2s 2 ho chistedom
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4. Calcium has 20 electrons in total. The ionization energy for the first 18 have been graphed below. Provide appropriate labels for the two empty boxes. IONISATION ENERGY (kJ mol¹) 120000 100000 80000 60000 40000 20000 O IE3: REMOVAL OF ELECTRON FROM 3p 1 2 3 IE 17: REMOVAL OF ELECTRON FROM 2s 4 5 6 7 NUMBER OF ELECTRONS REMOVED 8 9 10 11 12 13 14 15 16 17 18
Fix any errors in these proposed electron configurations. number of electrons in atom 32 20 12 proposed electron configuration 6 10 1s² 1p 2s²³ 2p 2d¹ 35² 3p 6 1s 2s² 2p 3s 3p 3d 5 2 2 8 2 1s 2s 2p X
Part A: How does ionization energy change down a group? increases from left to right decreases from left to right increases from top to bottom decreases from top to bottom Part B: Why is Ionization energy smaller for larger atoms? Sheilding. The nucleus cannot hold onto the electrons as well and loses them easier Shielding. The nucleus holds onto the electrons stronger and does not lose them easily There is no explanation Part C: According to the trend, which of these 4 elements has the largest ionization energy? Be (atomic# 4) Sr (atomic# 38) F (atomic# 9) I (atomic# 53) Part D: According to the trend, which of these 4 elements has the smallest ionization energy? Be (atomic# 4) Sr (atomic# 38) F (atomic# 9)…