10.4 Energy Levels of Electrons Electrons move in definite energy levels; these are labeled 1 - 7 Each level has sublevel(s) which are probability shapes.

Slides:



Advertisements
Similar presentations
Atomic Orbitals & Electron Configurations
Advertisements

Atomic Orbitals & Electron Configurations
Objectives To learn about the shapes of the s, p and d orbitals
Electron Configurations. Electron Configuration Electron configuration – the ____________ of electrons in an atom.
Section 11.3 Atomic Orbitals 1.To learn about the shapes of the s, p and d orbitals 2.To review the energy levels and orbitals of the wave mechanical model.
Electron Configuration
Chemical Periodicity. History Dmitri Mendeleev (1834 – 1907) – Russian chemist – Noticed regular (periodic) recurrence of chemical and physical properties.
Chapter 13 Chemical Periodicity.
Electron Configurations
Electron Configurations
Levels/Shells Principal Quantum Number (1-7) (2 x level 2 ) determines the amount of electrons that can fit into that energy level Electron Organization.
Question of the Day—get a calculator Calculate the total tuition saved if you took all 28 hours of dual credit available at FHS at the Stark State tuition.
The Periodic Table I. History of the Periodic Table (p )  Mendeleev  Mosely.
Reading the Periodic Table Objectives: 1. Explain why elements in a group have similar properties. 2. Identify the four blocks of the periodic table. Key.
Unit 3 Periodic Table and Valence electrons
-the arrangement of electrons in an atom -a distinct configuration for each element -assume the arrangement with the lowest possible energies (ground-state.
1 Chapter 7 Atomic Structure. 2 The Periodic Table n Developed independently by German Julius Lothar Meyer and Russian Dmitri Mendeleev (1870”s) n Didn’t.
Electron Configuration
Unit 3 Periodic Table and Valence electrons
C. Johannesson Aufbau Principle Electron Configuration.
Electron Configurations
Section Electron Configurations. Objectives Arrange electrons in atoms Describe quantum mechanics in terms of atomic orbitals Identify characteristics.
Electron Configuration!. s, p, d, and f The different sections of the Periodic Table are very important in understanding Electron Configuration. There.
Section 5.2.  If this rock were to tumble over, it would end up at a lower height. It would have less energy than before, but its position would be more.
Periodic Table and Configuration. Demetri Mendeleev Created modern periodic table (late 1800’s) Arranged by increasing atomic mass Similar elements found.
Chap 3 Electron Configurations & Quantum Numbers.
Electron Configurations Chapter 5. Aufbau Principle  Aufbau Principle: Electrons occupy the lowest energy orbital available.
CHAPTER 5 Electrons in Atoms. Development of Atomic Models Dalton – Remember atomic theory? – Atom considered indivisible Thomson – “plum pudding atom”
 Elements are arranged according to atomic number  Number of protons  Not atomic mass.
Electron Configurations Where the electrons are in the energy levels and orbitals. The configuration that requires the least energy is the most stable.
© 2014 Pearson Education, Inc. Sherril Soman Grand Valley State University Lecture Presentation Chapter 8-2 Periodic Properties of the Element.
The Periodic Table.  Go to page 154  Complete the Inquiry Activity.  You have 10 minutes to construct the table and answer the corresponding questions.
Electron Configurations Today we are going to assign addresses to each electron. The energy diagram shows where we put the electrons in every atom BUT.
. + ic. History u Russian scientist Dmitri Mendeleev taught chemistry in terms of properties. u Mid molar masses of elements were known. u Wrote.
Overview of the Periodic Table.  First periodic table  Elements were originally arranged in rows by ATOMIC MASS  He noticed that when arranged.
Periodic Trends. The Periodic Law When arranged by increasing atomic number, the chemical elements display a regular and repeating pattern of chemical.
Atomic Orbital Filling Order and Electron Configurations AP Chemistry.
Aim: How are Elements Organized in the Periodic Table?
Chapter 11 “Electron Configuration & Quantum Numbers”
Electron Configuration
Electron Configuration
Electron Configurations and Periodicity.
5.3 ELECTRON CONFIGURATIONS
Periodic Table Geography
1.1 Atoms, Elements and the Periodic Table
FILLING ORDER – memorize! 1s_ 2s_ 2p_ _ _ 3s_ 3p_ _ _3d _ _ _ _ _
Electrons.
Electron Configuration
Electrons in Atoms.
IV. Electron Configuration (p , )
IV. Electron Configuration (p , )
Electron Configuration
IV. Electron Configuration (p , )
Electron configuration
Electron Configuration
IV. Electron Configuration (p , )
Unit 2 Test Clicker Review
Periodic table terms.
Modern Atomic Model.
Energy Levels & Orbitals
Sec.3 Electron Configurations (p )
FILLING ORDER – memorize! 1s_ 2s_ 2p_ _ _ 3s_ 3p_ _ _3d _ _ _ _ _
Periodic Table: Periods: Are the horizontal rows on the
IV. Electron Configuration (p , )
Electron Configuration (p )
IV. Electron Configuration (p , )
IV. Electron Configuration (p , )
Electron configuration
IV. Electron Configuration (p , )
FILLING ORDER – memorize! 1s_ 2s_ 2p_ _ _ 3s_ 3p_ _ _3d _ _ _ _ _
Presentation transcript:

10.4 Energy Levels of Electrons Electrons move in definite energy levels; these are labeled Each level has sublevel(s) which are probability shapes that show where the electrons may be at any one time. Also known as orbitals. S orbital can hold up to 2 electrons (0, 1, 2) p orbital can hold up to 6 electrons (0-6) d orbital can hold up to 10 electrons (0-10) f orbital can hold up to 14 electrons (0-14) Aufbau chart shows how electrons fill into the main energy levels and the sublevels or orbitals

Energy Levels and Sublevels 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f

Aufbau Diagram or Chart 1s START HERE and follow 2s 2p the arrows! 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f

Electron Configuration 4 Be 1s 2 2s 2 15 P 1s 2 2s 2 2p 6 3s 2 3p 3 25 Mn 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 5

Pauli Exclusion Principle Pauli exclusion principle states that no more than 2 electrons can be in the same suborbital. Even so, this would cause them to have precisely the same quantum address. So Pauli decided there has to be a way to tell one electron from another. In other words, they must differ by at least one quantum number!

Pauli Exclusion Principle So they invented spin (+1/2 or -1/2) called spin up and spin down. Has nothing to do with the direction of the electron--we don’ t know how they move just where they may be at with 90% chance of finding it inside the energy level and orbital designated.

Hund’s Rule Hund’s rule states that electrons fill unpaired until there is no more room then they will pair (applies to p, d and f orbitals)

Orbital Diagrams S orbitals get one box P orbitals get 3 boxes (2 e- per box) D orbitals get 5 boxes and f gets 7

Orbital Diagrams (cont.) Insert electrons (using arrows into each box according to Hund’s and Pauli) 2 p 3

Answer 2p 3 (arrows can all point up or down) Now try 4f 10

Answer to 4f 10 Arrows may point up or down if they are in boxes individually; however, if there are 2 electrons in a box, one must point up and one down.

Electrons and the Periodic Table Revisited History of the Table Periodic Law Important People

Mendeleev Mendeleev was a Russian chemist who arranged the known elements in vertical columns in order of increasing mass and noticed a pattern in physical and chemical properties

Mosley Mosley was a British physicist who determined the atomic number (number of protons) of the atoms of elements and then arranged the elements according to their atomic number.

Periods and Groups Periods of the periodic table are the rows across Groups or Families are columns on the periodic table. Currently we have 18 groups. We will use the 1-18 designations not the A/B or Roman Numerals

Areas of the Periodic Table Representative elements or Main Group are those that are in Groups 1, 2, 13, 14, 15, 16, 17, 18 Transition elements are Groups , also called the Heavy Metals

Inner Transition Rare Earth elements that are located in the bottom two rows (away from the rest of the table) of the periodic table

Periodic Table GROUP NUMBERS Heavy Metals or Transition elements Main group Main Group or Representative elements Inner Transition Elements Period Numbers

Groups with names Group 1 = Alkali Metals Group 2 = Alkaline Earth Metals Group 18 = Inert or Noble Gases Group 17 = Halogens

Periodic Table and Electron Configuration The light metals compose the s block. The transition elements are the d block. The nonmetals are p block. The inner transition (rare earth) metals are the f block.

Periodic Table f 5f s block d block p block f block Noble (inert) gases

Complete the electron configurations for the Noble Gases (Hint: Group 18) He 1s 2 Ne 1s 2 2s 2 2p 6 Ar = 1s 2 2s 2 2p 6 3s 2 3p 6 Kr = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 1 0 4p 6 Xe = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 Rn = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 5d 1 0 6p 6 Except He, do you see a trend in all of the noble gas configurations? What do they all end in?

Shorthand Notation We use the noble gases in shorthand notation Find the closest noble gas that has an atomic number LESS than that of the element

Example Ex. K What is K’s atomic number? 19 Closest noble gas? Ar What is Ar’s atomic number? 18 = 1s 2 2s 2 2p 6 3s 2 3p 6 = [Ar] 4s 1 = Means the first 18 electrons are arranged like argon and the last electron is called the VALENCE ELECTRON (outermost shell)

Example for you to try You try Ba Ba = [Xe] 6s 2 Try Pb Pb = [Xe] 6s 2 4f 14 5d 10 6p 2