How Electrons are Configured in Energy Shells   The lowest energy arrangement of electrons is the most stable. When electrons are arranged in the lowest.

Slides:

Advertisements

Similar presentations

Bohr Model of the Atom Electrons reside in specific energy levels most of the time. When electrons are excited, they can jump from one energy level to.

Advertisements

Electronic Configuration Pauli exclusion principle – no two electrons in an atom can have the same four quantum numbers.

S- orbitals (l=0) p- orbital (l=1) d-orbital (l=2)

Chapter 5 Models of the Atom.

Chapter 5 Electronic Structure and Periodic Trends

ELECTRON CONFIGURATION. LABEL THE SUBLEVELS (1 S, 2 S, …)

Quantum Mechanical Model: Electron Configurations

11.4 A,B. Definitions Orbital – a three dimensional region in which there is a high probability of finding an electron in an atom (represented by orbital.

 Number that specifies the properties of the atomic orbitals  Tells us the distance from the nucleus and the shape of the orbital.

Electrons in Atoms.  So, you live on Aspen St., but what is your exact address?  We know that electrons can occupy energy levels, but they can also.

Orbital Model/Electron Cloud Model The energy levels of electrons are labeled by principal quantum numbers (n) Each energy sublevel corresponds to an orbital.

Electron Energy Level Notes Energy levels are broken up into sublevels: There are at least 4 possible types of sublevels—given labels: s, p, d, or f.

Electron Configurations Objectives: 3.0 Use the periodic table to identify periodic trends, including atomic radii, ionization energy, electronegativity,

Atomic Structure. Electron Configurations The way electrons are arranged around the nucleus.

ELECTRON CONFIGURATION The arrangement of electrons in an atom Each element has a distinct electron configuration Electron configuration describes the.

Writing Electron Configuration. Quantum Numbers Quantum numbers define the location of electrons in an atomic orbital. This helps us understand why different.

Chapter 5 Orbital Filling Diagrams and Electron Dot Diagrams.

Four Quantum Numbers: –Specify the “address” (zip code) of each electron in an atom.

 Electron Configuration is the way electrons are arranged around the nucleus.

Electron Arrangements Electron Configurations. Learning Objectives Express the arrangement of electrons in atoms using electron configurations Electron.

Unit 4: The Atom & the Electron Configurtation James Hutchison.

Chapter 5 Electrons in Atoms.

October 5 th, 2015 What is the atomic mass of hafnium if, out of every 100 atoms, 5 have mass 176, 19 have mass 177, 27 have mass 178, 14 have mass 179,

Electron Configurations. Schrodinger’s Quantum Model Principal Energy Levels - A region around the nucleus of an atom where the electron is likely to.

Electron Configurations Unit 3. What are electron configurations? According to the wave mechanical model, the electrons in an atom move around in the.

Electron Configuration and Periodic Trends

Electron Configuration. Objectives Describe the relationship between orbitals and energy levels for the electrons of an atom Describe the relationship.

Electron Arrangement in Atoms.  Electron configurations  Aufbau principle  Pauli exclusion principle  Hund’s rule.

Electron Configurations. The way electrons are arranged in atoms.

Arrangement of the Atom

Electron Configurations

Arrangement of e- e- are arranged in ENERGY LEVELS There are 7 energy levels Level 1 is closest to the nucleus and has the lowest energy Level 7 is farthest.

Atomic (Hotels) Theory  Floors of the hotel are known as energy levels  The period corresponds to the floor. The number of the floor is called the Principle.

QUANTUM MECHANICAL MODEL  Determines the allowed energies an electron can have  Determines how likely it is to find the electron in various locations.

Section 4-3 Electron Configurations. Quantum Mechanical Model Energy Levels have sublevels Each sublevel contains orbitals –Orbital – a 3-D region around.

Chapter 5 Quantum Numbers Part 1. Quantum Numbers There are four quantum numbers that describe the properties of an electron and the “orbital” that it.

Construction of an Atom Notes. Heisenberg Uncertainty Principle States that we cannot know the position and the speed of a moving object simultaneously.

The Quantum Mechanical Model of the Atom. Schrodinger The quantum mechanical model determines the energy an electron can have and the PROBABILITY of finding.

Electron Configuration Atomic Structure and. Orbital (“electron cloud”) – Region in space where there is 90% probability of finding an e - Each orbital.

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.

What are electron configurations? The way electrons are arranged in atoms. Used to indicate which orbitals (energy levels) are occupied by electrons for.

Bohr model and electron configuration. Bohr’s Model Why don’t the electrons fall into the nucleus? Move like planets around the sun. In circular orbits.

I. Electron Configurations A.Principal energy levels B.Energy sublevels C.Orbitals.

The Quantum Mechanical Model of an Atom Ch 5 (pg. 131)

Electron Configuration

Electron Configuration

Chapter 5 Quantum Numbers.

Arrangement of Electrons in Atoms

Atomic Spectra One idea in early 20th century was that an electron (e-) traveled about the nucleus in an orbit. (planetary model)

Basic Chemistry Chapter 5 Electronic Structure and Periodic Trends

ELECTRONS IN ATOMS.

Unit 3 – Electron Configurations Part F: Electron Configurations II

ELECTRON CONFIGURATIONS

Orbitals each sublevel is broken into orbitals

Chapter 5 Electronic Structure and Periodic Trends

Chapter 5 Quantum Numbers Part 1.

Unit 3 – Electron Configurations Part F: Electron Configurations II

Atomic Orbitals The energy levels of electrons are labeled by principal quantum numbers (n) Each energy sublevel corresponds to an orbital of a different.

Electron Arrangement in Atoms

Electron Arrangement.

3.3 Electron Configuration

Chapter 5 Electrons In Atoms 5.2 Electron Arrangement in Atoms

Atomic Orbitals and Electron Arrangement

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 Structure Orbital Diagrams.

Section 5.2 – Electron Arrangement in Atoms

Where exactly are the electrons? It’s all a little cloudy!

QUANTUM MECHANICAL MODEL

ELECTRONS IN ATOMS.

Presentation transcript:

How Electrons are Configured in Energy Shells

  The lowest energy arrangement of electrons is the most stable. When electrons are arranged in the lowest possible energy arrangement it is called the electron’s ground-state electron configuration. Electron’s Lowest State

  Three rules (principles) define how electrons are arranged in orbit around an atom’s nucleus.  First Rule:  Aufbau’s principal states that each electron occupies the lowest energy orbital available. Rules for Placing Electrons in Energy Shells

  Pauli’s exclusion principal states that a maximum of two electrons may occupy a single atomic orbital but only if they spin in opposite directions.  Hund’s Rule states that single electrons with the same spin must each occupy an equal-energy orbital before additional electrons with different spins can occupy the same orbitals. 2 nd & 3 rd Rule

  There are seven principal energy levels (shells).  Each principal energy level contains sublevels.  Each sublevel contains orbitals. The orbitals are where the electrons reside.  Each orbital allows only two electrons. Energy Levels & Sublevels

  The sublevels are designated s, p, d and f.  The s sublevels are spherical, contain one orbital, and can hold a total of two electrons.  The p sublevels resemble dumbbells. There are three p orbitals each allowing two electrons. The total number of electrons able to occupy the p sublevels is six. s & p Sublevels

  The shapes of the d and the f sublevels become more complicated. The d sublevels have five orbitals and can hold a maximum of 10 electrons while f sublevels contains 7 orbitals and can hold a maximum of 14 electrons.  The superscripts inform us how many electrons are residing in an orbital. d & f Sublevels