Unit 3 Electron configuration and periodicity Lundquist -- 2015

Unit 3.1 No note quiz questions, follow along in your packet starting on p. 6

Coulomb’s Law The long distance relationship rule The force of attraction between two objects is proportional to their charges, and inverse to the distance between them The long distance relationship rule Coulomb’s Law

Review with your table Questions Word Bank Attraction Repulsion Neutral Positive Negative Charge Distance Nucleus Force Energy Coulomb’s Law Describe the nature of interaction between protons and electrons in an atom. Review with your table

Which will require more energy to separate?

Which will require more energy to separate?

How many e-?

How many p+?

Which of these e- Will be the easiest (require the least energy) to remove (ionize)? Why?

3 2A 2C How does that compare with these? Which will be easiest to ionize? Rank them

First ionization energy Remove 1 e- in the gas phase of an element 𝑒𝑛𝑒𝑟𝑔𝑦+ 𝐴 𝑔 → 𝐴 𝑔 1+ + 𝑒 − First ionization energy

𝑒𝑛𝑒𝑟𝑔𝑦+ 𝐴 𝑔 → 𝐴 𝑔 1+ + 𝑒 − 𝐴 𝑔 1+ 𝐴 𝑔 Which has less energy?

Why is this an endothermic (requires energy) process? 𝑒𝑛𝑒𝑟𝑔𝑦+ 𝐴 𝑔 → 𝐴 𝑔 1+ + 𝑒 − 𝐴 𝑔 1+ 𝐴 𝑔 Why is this an endothermic (requires energy) process?

𝑒𝑛𝑒𝑟𝑔𝑦+ 𝐻 𝑔 → 𝐻 𝑔 1+ + 𝑒 − The value of the first ionization energy is 1312 𝑘𝐽 𝑚𝑜𝑙 . on the graph on the next page put a horizontal line to indicate the energy of each specie

𝑒𝑛𝑒𝑟𝑔𝑦+ 𝐻 𝑔 → 𝐻 𝑔 1+ + 𝑒 − Why is it negative? What does the difference in the two lines represent?

Remember this analogy? How does your explanation account for the relative charge on H and He the distance of electron(s) from the nucleus? How would you explain the difference in the 1st ionization energy of H with He?

Draw the 1st ionization energy of H and He. PREDICT A VALUE FOR Li

520

496 738 789 1046 1297 1530

Review with your table Questions Word Bank Nucleus Electron Distance energy Level Proton Shell Arrangement Attraction repulsion Positive Negative Charge location Describe the electron structure (location of e-) of the atom Review with your table

Electrons in higher energy levels require less energy to remove

Shells Layers of electrons around the nucleus Energy levels Based on distance from the nucleus Shells

Bohr Models Show electrons in their shell Shows nuclear charge and number of neutrons Outer most shell is known as the valence shell Bohr Models

Do p. 14 & 15

Do All electrons in the same energy level have the same energy?? To answer this we can look at photoelectric spectroscopy data Do All electrons in the same energy level have the same energy??

Photoelectric Spectroscopy Data

PES data What does the x-axis symbolize? What’s the relationship between the 1st ionization energy of H (1312 𝑘𝐽 𝑚𝑜𝑙 ) and the PES data? PES data

He is next How many e- does He have in its first shell? Predict what the PES would look like if The same amount of energy was needed to remove an electron Different amounts of energy were required to remove an electron He is next He

What it actually looks like

Li

What it actually looks like

Lets see them all

Unit 3.2 Electron Configuration

Orbitals & Subshells Subshells Electrons can be ANYWHERE Probability distribution around the nucleus Orbitals Divisions of that distribution based on space and magnetism Orbitals & Subshells

Rules for Electron Configuration Aufbau Principle Lower energy levels fill first Follow the periodic table and you will be fine Rules for Electron Configuration

Write the complete electron configuration for Cl Write the complete electron configuration for I Practice

Noble gas notation Short cut [previous noble gas] any other subshells & orbitals Noble gas notation

1. 2. 3. 4. Note Quiz Questions

6. 5. 6. 7. Note Quiz Questions

Ions The Universe is lazy Noble gasses have the least energy, thus are inert Nonmetals will gain e- to be like noble gasses More e- = more (-) Metals will loose e- to be like noble gasses Less e- = more (+) Ions

Do p. 17 & 18

8. 9. Note Quiz Questions

Orbital Notation Diagram for showing the spin of an electron Hund’s Rule e- won’t double up unless they have to Pauli’s Exclusion Principle Two e- cannot spin in the same direction in the same place Orbital Notation

10. Note Quiz Questions

Do the top of p. 16

Magnetism Diamagnetic No unfilled subshells Paramagnetic At least 1 unfilled subshell Ferromagnetic LOTS of unfilled subshells Found in the middle of the d-block and f-block Magnetism

Do the bottom of p. 16

Quiz Next Class Use and interrupt PES data Write electron configurations Draw an orbital diagram Discuss ionization energy Chem. Quiz Next Class

Unit 3.3 Periodic Trends

Periodic Trends

EXPLAINATIONS Right to left Top to Bottom Increased effective nuclear charge (Zeff) Increased principle energy level (number of shells) EXPLAINATIONS

Atomic Radius Which would be smaller?? As nuclear charge increases there is more attraction for the nucleus so atoms get smaller Atomic Radius

As you gain shells you move further from the nucleus Atomic Radius

Atomic Radius Increases from top to bottom Decreases from left to right

First ionization energy REMEMBER Coulomb’s Law Smaller elements Larger elements First ionization energy

First ionization energy Decreases from top to bottom Increases from left to right

Electronegativity Ability of an atom to attract an electron Scale from 0-4 Same-ish as electron affinity Electronegativity

Ionic Radius Cations (+) Anions (-) Positive ions Negative ions Have LESS e- Same charge in nucleus Pull e- closer in Group 1 – 13 (all metals) Negative ions Have MORE e- More repulsion from more e- Pushes e- further out Groups 15-18 Ionic Radius

Ionic Radius

Do p. 23

1. Note Quiz Questions

2. Note Quiz Questions

3. 5. 4. Note Quiz Questions

6. 7. 8. Note Quiz Questions

10. 9. Note Quiz Questions

THE END Test NEXT PERIOD! 25 MC you will need to 21 to get a 100 1 free response worth 10 points, you will need to earn 7 to get a 100 Multiple Choice homework due NEXT PERIOD! THE END