Atom video qNSQ3OQMGI&feature=share.

Slides:



Advertisements
Similar presentations
Electron Configurations Of the three major subatomic particles, the electron plays the most significant role in determining the physical and chemical properties.
Advertisements

Lecture 2410/31/05. Recap from last week Every electron has a unique position in atom each electron has unique set of 4 quantum numbers Electrons fill.
Energy levelSublevel# of orbitals/sublevel n = 11s (l = 0)1 (m l has one value) n = 2 2s (l = 0) 1 (m l has one value) 2p (l = 1) 3 (m l has three values)
Chapter 8 Periodic Properties of the Elements. Electron Spin experiments by Stern and Gerlach showed a beam of silver atoms is split in two by a magnetic.
EXAM #3 MONDAY, NOVEMBER 9 TH (Chapters 6 and 7) Bring a Periodic Table to class Manners reminder Today: Finish Chapter 7 Orbital filling Periodic Properties.
Objectives SWBAT distinguish among the Aufbau principle, the Pauli exclusion principle, and Hund’s rule. SWBAT write electron configurations for selected.
Electron configuration What is electron configuration? Explains the arrangement of electrons within an atom. There is a specific electron configuration.
Electron Configuration
Arrangement of Electrons in Atoms
Electron Configuration Revised by Ferguson Fall 2014.
TRENDS FOUND ON THE PERIODIC TABLE PERIODIC GROUPS ELEMENTS IN THE SAME COLUMN HAVE SIMILAR CHEMICAL AND PHYSICAL PROPERTIES THESE SIMILARITIES ARE OBSERVED.
Electron Configurations
Section 4.3—Electron Structure
Electron Configuration
Bohr Model of the Atom  Bohr’s Atomic Model of Hydrogen  Bohr - electrons exist in energy levels AND defined orbits around the nucleus.  Each orbit.
Periodic Table Electron Configurations. Aufbau Principle – electrons occupy the orbitals of lowest energy first Hund’s Rule - electrons fill orbitals.
Chapter 8: Electron configurations and periodicity Chemistry 1061: Principles of Chemistry I Andy Aspaas, Instructor.
Atom video
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.
Quantum Mechanics n n = The principle quantum number Describes the possible energy levels and pictorially it describes the orbital size. n = 1, 2, 3….
Electron Configuration Revised by Ferguson Spring 2014.
Writing Electron Configuration. Quantum Numbers Quantum numbers define the location of electrons in an atomic orbital. This helps us understand why different.
The Orbitals Erwin Schrödinger (1933 Noble laureate) was the first to successfully apply the concept of the wave nature of matter to electronic structure.
Chapter 5 Orbital Filling Diagrams and Electron Dot Diagrams.
 Electron Configuration is the way electrons are arranged around the nucleus.
Section 4: Electron Configurations
1s orbital 2s orbital 2p orbitals 3s3s orbital Nucleus Electron energy levels have sublevels of different shapes.
-the arrangement of electrons in an atom -a distinct configuration for each element -assume the arrangement with the lowest possible energies (ground-state.
SECTION 3: ELECTRON CONFIGURATIONS CHAPTER 9: ELECTRONS IN ATOMS AND THE PERIODIC TABLE.
Quantum Mechanics. Electron Density Gives the probability that an electron will be found in a particular region of an atom Regions of high electron density.
Electron Configuration
1s2s 2p3s 3p 3d n = 1 n = 2 n = 3. NUCLEUS 1s 2s 2p 3s 3p 3d 4s 4p4d 4f Energy Level SublevelsTotal Orbitals 1s1s1s 2s,p1s+3p = 4 3s,p,d1s+3p+5d = 9 4s,p,d,f1s+3p+5d+7f.
Atomic Electronic Structure
Electron Configurations
Section Electron Configurations. Objectives Arrange electrons in atoms Describe quantum mechanics in terms of atomic orbitals Identify characteristics.
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.
Protons, Neutrons, and Electrons
Electron Configuration and Periodic Trends
Electron Configurations. The way electrons are arranged in atoms.
Arrangement of the Atom
Electron Configurations Where the electrons are in the energy levels and orbitals. The configuration that requires the least energy is the most stable.
Quantum Mechanics. Electron Density Gives the probability that an electron will be found in a particular region of an atom Regions of high electron density.
Quantum Numbers n, l, m, and s – Used to describe an electron in an atom Probable location n – Principal Quantum Number – Represents main energy level.
N - principle quantum number - determines distance from the nucleus and energy l - orbital angular momentum quantum number l = 0, 1, 2,… n-1 m l - magnetic.
The Electron Configuration
Electron Configurations And Orbital Diagrams. Principles for Filling Orbitals Writing electron configurations –
The Electron Configuration
Tro, Principles of Chemistry: A Molecular Approach Chapter 8 Periodic Properties of the Elements Roy Kennedy Massachusetts Bay Community College Wellesley.
Homework # 8 Electron Configuration.
Atomic Orbital Filling Order and Electron Configurations AP Chemistry.
1 2 3 Orbitals and the Periodic Table Orbitals grouped in s, p, d, and f orbitals (sharp, principle, diffuse, and fundamental(fine))Orbitals grouped.
Electron Configuration
Electron Configuration. WHHYYYYY do we need to learn this? When atoms interact, it’s the valence electrons that interact first. Atoms are least stable.
Orbitals and Electron Configurations
Electron Configurations
Electron Configurations
Electron Configurations
Electron Configurations
Unit 1: Structure and Properties of Matter
Electron Configurations
Electron Configuration
Orbitals each sublevel is broken into orbitals
Chapter 5: Electrons in the Atom
3.3 Electron Configuration
How can you express the arrangement of electrons in atoms through electron configurations? In an atom, electrons and the nucleus interact to make the most.
Atomic Electronic Structure
FILLING ORDER – memorize! 1s_ 2s_ 2p_ _ _ 3s_ 3p_ _ _3d _ _ _ _ _
2.4- Quantum Mechanical Model
4 Quantum Numbers (n, l, ml, ms)
Presentation transcript:

Atom video qNSQ3OQMGI&feature=share

Basic Principle: electrons occupy lowest energy levels available

Aufbau Principle -- “Bottom Up Rule”

Electron spin How could an orbital hold two electrons without electrostatic repulsion?  Stern-Gerlach Experiment

1 1 s value of energy level sublevel no. of electrons spdf NOTATION for H, atomic number = 1 spdf Notation Orbital Box Notation Arrows show electron spin (+½ or -½) ORBITAL BOX NOTATION for He, atomic number = 2 1s1s 2 1s1s  2 ways to write electron configurations

Example: Determine the electron configuration and orbital notation for the ground state neon atom. An orbital can contain a maximum of 2 electrons, and they must have the opposite “spin.” Pauli exclusion principle

Hund’s Rule - Write the ground state configuration and the orbital diagram for oxygen in its ground state

Outer electron configuration for the elements

Using the periodic table to know configurations Period Ne Ar Kr Xe

Valence e ’ s for “main group” elements

Rules for Filling Orbitals Bottom-up (Aufbau’s principle) Fill orbitals singly before doubling up (Hund’s Rule) Paired electrons have opposite spin (Pauli exclusion principle) Basic Principle: electrons occupy lowest energy levels available

Identify examples of the following principles: 1) Aufbau 2) Hund’s rule 3) Pauli exclusion

Shorthand notation practice Examples ●Aluminum: 1s 2 2s 2 2p 6 3s 2 3p 1 [Ne]3s 2 3p 1 ●Calcium: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 [Ar]4s 2 ●Nickel: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 8 [Ar]4s 2 3d 8 {or [Ar]3d 8 4s 2 } ●Iodine: [Kr]5s 2 4d 10 5p 5 {or [Kr]4d 10 5s 2 5p 5 } ●Astatine (At): [Xe]6s 2 4f 14 5d 10 6p 5 {or [Xe]4f 14 5d 10 6s 2 6p 5 } [ Noble Gas Core ] + higher energy electrons

Electron configuration for As

Note: Not written according to Aufbau, but grouping according to n

Orbital energy ladder s p n = 2 s d p n = 3 f s d p n = 4 s n = 1 Energy

Phosphorus Symbol: P Atomic Number: 15 Full Configuration: 1s 2 2s 2 2p 6 3s 2 3p 3 Valence Configuration: 3s 2 3p 3 Shorthand Configuration: [Ne]3s 2 3p 3    1s 2s 2p 3s 3p Box Notation

Quantum numbers and orbital energies Each electron in an atom has a unique set of quantum numbers to define it { n, l, m l, m s } n = principal quantum number –electron’s energy depends principally on this l = azimuthal quantum number –for orbitals of same n, l distinguishes different shapes (angular momentum) m l = magnetic quantum number –for orbitals of same n & l, m l distinguishes different orientations in space m s = spin quantum number –for orbitals of same n, l & m l, m s identifies the two possible spin orientations

Energy levelSublevel# of orbitals/sublevel n = 11s (l = 0)1 (m l has one value) n = 2 2s (l = 0) 1 (m l has one value) 2p (l = 1) 3 (m l has three values) n = 3 3s (l = 0) 1 (m l has one value) 3p (l = 1) 3 (m l has three values) 3d (l = 2) 5 (m l has five values) n = principal quantum number (energy) l = azimuthal quantum number (shape) m l = magnetic quantum number (orientation) Quantum numbers and orbital energies Each atom’s electron has a unique set of quantum numbers to define it { n, l, m l, m s }

21 Concept: Each electron in an atom has a unique set of quantum numbers to define it { n, l, m l, m s }

Quantum numbers: unique set for each e - s orbitals p orbitals d orbitals f orbitals l = 0 l = 1 l = 2 l = 3 m l = 0 m l = -1, 0, 1 m l = -2, -1, 0, 1, 2 m l =-3,-2,-1,0,1,2,3 An s subshell A p subshell A d subshell An f subshell One s orbital Three p orbitals Five d orbitals Seven f orbitals For n=1 l=0 an s subshell (with 1 orbital) For n=2 l=0,1 an s subshell and a p subshell (with 3 orbitals) For n=3 l=0,1,2 an s subshell, a p subshell, a d subshell (with 5 orbitals) For n=4 l=0,1,2,3 an s subshell, a p subshell, a d subshell, an f subshell (with 7 orbitals)

Electronic configuration of Br 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 5 [Ar] 3d 10 4s 2 4p 5 [Ar] = “noble gas core” [Ar]3d 10 = “pseudo noble gas core” (electrons that tend not to react) Atom’s reactivity is determined by valence electrons valence e’s in Br: 4s 2 4p 5 highest n electrons

Valence e - shells for transition metalsmain group elements transition metals v. main group elements d orbitals sometimes included in valence shell d orbitals not included in valence shell (pseudo noble gas cores)

Rule-of-thumb for valence electrons Examples ●Sulfur: 1s 2 2s 2 2p 6 3s 2 3p 4 or [Ne]3s 2 3p 4 valence electrons: 3s 2 3p 4 ●Strontium: [Kr]5s 2 valence electrons: 5s 2 ●Gallium: [Ar]4s 2 3d 10 4p 1 valence electrons: 4s 2 4p 1 ●Vanadium: [Ar]4s 2 3d 3 valence electrons: 4s 2 or 3d 3 4s 2 Identify all electrons at the highest principal quantum number (n) Use on exams, but recognize limitations Use Table 8.9 for online HW

Selenium’s valence electrons Pseudo noble gas core includes:  noble gas electron core  d electrons (not very reactive) Written for increasing energy:

Core and valence electrons in Germanium Pseudo noble gas core includes:  noble gas core  d electrons Written for increasing energy:

d-block: some exceptions to the Aufbau principle Fig. 8.9: Use this table for online homework

Paramagnetic : atoms with unpaired electrons that are weakly attracted to a magnet. Diamagnetic : atoms with paired electrons that are not attracted to a magnet. Paramagnetic : atoms with unpaired electrons that are weakly attracted to a magnet. Diamagnetic : atoms with paired electrons that are not attracted to a magnet. Electron spin & magnetism For the ground state oxygen atom: spdf configuration: orbital box notation:

Apparatus for measuring magnetic properties