Electron Movement and Organization 3.30.15 Objectives: Identify electron properties Understand how...

Electron Movement and Organization3.30.15

Objectives:• Identify electron properties • Understand how electrons move within an atom.

Electron Movement and Organization3.31.15

Objectives:• Identify electron properties • Understand how electrons move within an atom.

Characteristics of Electrons Characteristics of Electrons

1. What are some properties of electrons?

2. How do electrons move within an atom?

Electron Movement and Organization3.18.15

Objectives:• Identify electron properties • Understand how electrons move within an atom.

Electron Movement and Organization4.1.15

Objectives:• Identify electron properties • Understand how electrons move within an atom.

Like Properties: WavelengthLike Properties: Wavelength• Wavelength: length of wave from two neighboring crest.

Wave-Like Properties: FrequencyWave-Like Properties: FrequencyFrequency (Hz) : how many waves pass a certain point per second. Units: Hertz (Hz.)= (waves/second)

Wave-Like Properties: EnergyWave-Like Properties: Energy• Temperature : Represents amount of energy emitted from

light particles. • Photons: Light particles classified by energy emitted.

*Electron movement dependent upon type of photons absorbed or released.

Electrons: Wave-Like PropertiesElectrons: Wave-Like Properties

a. Relationship b/w wavelength and frequency?b.Relationship b/w wavelength and energy emission?c.Relationship b/w frequency and energy emission?

Electron MovementElectron Movement•Electrons can take different paths around the nucleus.

*Electrons constantly move to different energy levels in the electron cloud.

*Direction of e- movement is dependent upon energy absorbed or released.

Erwin Schrodinger

Electron Movement Around NucleusElectron Movement Around Nucleus

A maximum of 2 electrons can move in each orbital.

Electron MovementElectron Movement•Electrons can take different paths around the nucleus.

*Electrons constantly move to different energy levels in the electron cloud.

*Direction of e- movement is dependent upon energy absorbed or released.

Erwin Schrodinger

Electron MovementElectron Movement

1. Ground state of H Atom (lowest energy level for e-)2. A photon (light particle) is absorbed by H’s electron. Electron becomes excited and jumps to higher energy level.3. E- returns to ground state and emits (releases) the photon.

Emitted photon’s wavelength can be detected by scientists. (Infrared region at room temp; Visble region at higher temps.)

1. 2. 3.

Flame Test LabFlame Test Lab

Purpose: To classify atoms and identify electron movement in atoms.

Electron Movement and Organization4.13.15

Objectives:• Identify electron properties • Understand how electrons move within an atom. • Understand how electrons are arranged in an atom.

Electromagnetic Spectrum AnalysisElectromagnetic Spectrum Analysis

a. Relationship b/w wavelength and frequency?b.Relationship b/w wavelength and energy emission?c.Relationship b/w frequency and energy emission?

Emission Spectrums

•Emission spectrum for each element is unique.

Visible Region of EM Spectrum

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Electron Movement and Organization4.14.15

Objectives:• Identify electron properties • Understand how electrons move within an atom. • Understand how electrons are arranged in an atom.

Electron Probability Lab Electron Probability Lab

Purpose: To determine which energy level an electron would prefer to be on in an atom.

Class’s Hypothesis:

-1st energy level-closest to nucleus (12 students)

-Highest energy level-farthest from nucleus(6 students)

Energy Levels and the Periodic TableAssociate energy levels with rows on periodic table.

Electron Movement and Organization4.15.15

Objectives:• Identify electron properties • Understand how electrons move within an atom. • Understand how electron arrangement determines

chemical reactivity.

Electron Probability Lab Electron Probability Lab

Class’s Hypothesis:

-1st energy level-closest to nucleus (12 students)

-Highest energy level-farthest from nucleus(6 students)

Class’s Results: Lab Group

Energy Level 1(# of times)

Energy Level 2(# of times)

Energy Level 3 (# of times)

1

2

3

4

5

6

7

8

9

Electromagnetic Spectrum Analysis Qts. Electromagnetic Spectrum Analysis Qts.

Emission Spectrums

•Emission spectrum for each element is unique.

Locating an ElectronLocating an Electron

Is it possible to know the exact location of an electron at any moment in time?•Very difficult to locate an electron because:

- moving extremely fast

-continuously bombarded by light particles, which changes the path of the electron.

-When locate an electron with a photon from a microscope, it changes its direction in unpredictable ways.

Photon

Before

Photon changes wavelength

After

Heisenberg Uncertainty Principle

It is not possible to know the exact location of an electron, just probable location.

Energy LevelsEnergy Levels

• Limited number of electrons on each energy level.

• 2n2 Rule determines the maximum number of electrons on each energy level.

Electron ArrangementElectron Arrangement

• Different for each element.

Periodic Table and Valence Electrons

Electron ArrangementElectron Arrangement

• Different for each element.

• Valence Electrons

Electron Movement in Energy LevelsElectron Movement in Energy Levels

•Quantum of energy: •Specific energy that is absorbed or emitted by electrons.• Energy difference between two energy levels. •Scientist can calculate energy emitted by electrons.•Determine what energy levels electrons move between in an atom.

Electron Probability LabElectron Probability Lab

l–Quantum Numberl -number :

• Sublevels within an energy level.

• Sublevels identify the shape of the orbitals.

• There are four different sublevels: s, p, d, f

Orbital ShapesOrbital Shapes

A maximum of 2 electrons can move in each orbital.

Orbitals and Energy RequirementOrbitals and Energy Requirement• Electron movement defines orbital shapes for each

sublevel.

• Electrons need energy to move in orbital shapes.

Sublevel’s Orbitals Energy for electron movement(Rank in increasing amount of energy)

S-orbital

P-orbital

D-orbital

F-orbital

Electron ConfigurationElectron Configuration• Electron Configuration: The probable

arrangement of electrons in the ground state of an atom.

Electron Configuration Rules:

• Aufbau Principle: Electrons will move in an orbital of lower energy first. (Electrons are lazy!)

• Pauli Exclusion Principle: Only two electrons can move in an orbital at the same time.

• Hund’s Rule: When electrons can move in orbitals of the same energy, they will prefer to be alone before pairing up. (Electrons are selfish!)

Electron Movement and Organization3.25.15

Due:• Electron Probability Lab

Objectives:• Understand how electrons move within atoms.

• Distinguish between atoms based on their different electron arrangements.

Bell Ringer: Electron Arrangement1. What atomic model best explains electron arrangement?

2. a. What is the n-quantum number?

b. T or F: Electron move around the nucleus in

an exact path.

3. a. What is the l-quantum number?

b. Illustrate the s, p, d, f atomic orbitals?

c. How many electrons can move in each atomic orbital at any one time?

Orbital ShapesOrbital Shapes

A maximum of 2 electrons can move in each orbital.

Orbitals and Periodic Table

Bell Ringer: Electron Arrangement1. What atomic model best explains electron arrangement?

2. a. What is the n-quantum number?

b. T or F: Electron move around the nucleus in

an exact path.

3. a. What is the l-quantum number?

b. Illustrate the s, p, d, f atomic orbitals?

c. How many electrons can move in each atomic orbital at any one time?

Electron Configuration Electron Configuration

Electron Configuration: Bell RingerElectron Configuration: Bell Ringer

1. What is electron configuration for an element?

2. How does the periodic table help you determine electron configuration for an element? Be specific with your explanation.

Electron Sublevels (atomic orbitals)Electron Sublevels (atomic orbitals) Diagonal Rule Diagonal Rule

3. Use the diagram to determine the type of sublevels (orbitals) in each energy level?1st: 2nd:3rd:4th:5th:6th:7th:

2. What do you suppose the yellow arrows represent?

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Periodic Table and Electron Configuration

Orbital ShapesOrbital Shapes

A maximum of 2 electrons can move in each orbital.

Electron Configuration: Exit SlipElectron Configuration: Exit Slip

Br:

Ar:

Fe

Electron ConfigurationElectron Configuration• Electron Configuration: The probable

arrangement of electrons in the ground state of an atom.

Electron Configuration Rules:

• Aufbau Principle: Electrons will move in an orbital of lower energy first. (Electrons are lazy!)

• Pauli Exclusion Principle: Only two electrons can move in an orbital at the same time.

• Hund’s Rule: When electrons can move in orbitals of the same energy, they will prefer to be alone before pairing up. (Electrons are selfish!)

m- Quantum Numberm –number:

• Orientations for each atomic orbital.

• Orbital orientations: The different ways an electron can make an orbital in 3-D space.

S-Orbital OrientationS-Orbital Orientation

• Maximum # of s-orbital electrons on an energy level? • How many s-orbital orientations are possible on an energy

level?

P-orbital OrientationsP-orbital Orientations• Maximum # of p-orbital electrons on an energy level?• How many p-orbital orientations are possible on an energy

level?

D-orbital OrientationsD-orbital Orientations• Maximum # of d-orbital electrons on an energy level?

• How many d-orbital orientations are possible on an energy level?

F-orbital OrientationsF-orbital Orientations•Maximum # of f-orbital electrons on an energy level?•How many f-orbital orientations are possible on an energy level?

Orbital Orientations

Electron Movement and Organization11.05.14

Infinite Campus:• Electron Probability Lab (15pts.)

Objectives:• Understand how electrons move within atoms

• Distinguish between atoms based on their different electron arrangements.

Electron Configuration with orbital notationElectron Configuration with orbital notation1. Define the first three quantum numbers.

2. Write the electron configuration (n,l,m quantum numbers) for each element below:

H:

Li:

C:

V:

Electron Configuration Orbital NotationElectron Configuration Orbital Notation

S-Quantum NumbersS-number :

• The direction an electron spins in an orbital.

• If paired, the electrons will spin in opposite directions.

Electron Configuration: Bell Ringer Electron Configuration: Bell Ringer

1. a. Determine the electron configuration of a neutral Br atom and include the orbital notations.

b. How many unpaired electrons?

c. How many valence electrons does Br have?

d. How many types of sublevels (orbitals) use Hund’s rule?

Orbitals and Periodic Table

Nuclear Chemistry and Electron Arrangement ExamNuclear Chemistry and Electron Arrangement Exam

Balancing Redox Reactions: Acidic Balancing Redox Reactions: Acidic Solutions Solutions

Cu (s) + NO3- (aq) ----> Cu2+ (aq) + NO2 (g)