This document provides information about electron configuration. It begins by defining electron configuration as the arrangement of electrons in an atom's orbitals, which is described using quantum numbers. It then discusses the three main rules for writing electron configurations: 1) Aufbau principle, which states that electrons fill the lowest available energy levels first, 2) Pauli exclusion principle, which limits each orbital to two electrons of opposite spin, and 3) Hund's rule, which states that degenerate orbitals will fill with one electron each before pairing. The document provides examples of writing full and condensed electron configurations and drawing orbital diagrams for various elements. It includes an activity for students to practice these skills.
module 1 electronic structure of matter.pptxMaryroseBudhi1
Module 1: Electronic Structure of Matter
Objectives: Know atom and its sub - particles
determine the characteristics colors that metal salts emit
what is atom?
atom is the basic unit of chemical element
it composes three subatomic particle
proton with a positively electric charge
electron with a negatively electric charge
neutron no electric charge
What minerals produce the color in fireworks?
Mineral elements provide color in fireworks. Barium produces bright greens; strontium yields deep reds;' copper produces blues/ and sodium yields yellow. other colors can be made by mixing elements; strontium and sodium produce brilliant orange; titanium, zirconium, and magnesium alloys make silvery white; copper and strontium make lavender. gold sparks are produced by iron fillings and small pieces of charcoal. bright flashes and loud bangs come from aluminum powder.
module 1 electronic structure of matter.pptxMaryroseBudhi1
Module 1: Electronic Structure of Matter
Objectives: Know atom and its sub - particles
determine the characteristics colors that metal salts emit
what is atom?
atom is the basic unit of chemical element
it composes three subatomic particle
proton with a positively electric charge
electron with a negatively electric charge
neutron no electric charge
What minerals produce the color in fireworks?
Mineral elements provide color in fireworks. Barium produces bright greens; strontium yields deep reds;' copper produces blues/ and sodium yields yellow. other colors can be made by mixing elements; strontium and sodium produce brilliant orange; titanium, zirconium, and magnesium alloys make silvery white; copper and strontium make lavender. gold sparks are produced by iron fillings and small pieces of charcoal. bright flashes and loud bangs come from aluminum powder.
The slides contains information Regarding Electron Configuration.
1. How electrons arranged in shells
2. Atomic orbitals
3. Electronic Configuration
4. Sublevels
5. Hunds rule
6. Pauli Rule
What are Electron Configurations ex.docxajullo3333
What are Electron Configurations?
The electron configuration of an element describes how electrons are distributed in its atomic orbitals. Electron configurations of atoms follow a standard notation in which all electron-containing atomic subshells with number of electrons are placed in a sequence.
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Under Augustus, the empire experienced the Pax Romana, a 200-year period of relative peace and stability. Augustus reformed the military, established efficient administrative systems, and initiated grand construction projects. The empire's borders expanded, encompassing territories from Britain to Egypt and from Spain to the Euphrates. Roman legions, renowned for their discipline and engineering prowess, secured and maintained these vast territories, building roads, fortifications, and cities that facilitated control and integration.
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Culturally, the Romans were eclectic, absorbing and adapting elements from the civilizations they encountered, particularly the Greeks. Roman art, literature, and philosophy reflected this synthesis, creating a rich cultural tapestry. Latin, the Roman language, became the lingua franca of the Western world, influencing numerous modern languages.
Roman architecture and engineering achievements were monumental. They perfected the arch, vault, and dome, constructing enduring structures like the Colosseum, Pantheon, and aqueducts. These engineering marvels not only showcased Roman ingenuity but also served practical purposes, from public entertainment to water supply.
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The people of Punjab felt alienated from main stream due to denial of their just demands during a long democratic struggle since independence. As it happen all over the word, it led to militant struggle with great loss of lives of military, police and civilian personnel. Killing of Indira Gandhi and massacre of innocent Sikhs in Delhi and other India cities was also associated with this movement.
The French Revolution, which began in 1789, was a period of radical social and political upheaval in France. It marked the decline of absolute monarchies, the rise of secular and democratic republics, and the eventual rise of Napoleon Bonaparte. This revolutionary period is crucial in understanding the transition from feudalism to modernity in Europe.
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Synthetic fiber production is a fascinating and complex field that blends chemistry, engineering, and environmental science. By understanding these aspects, students can gain a comprehensive view of synthetic fiber production, its impact on society and the environment, and the potential for future innovations. Synthetic fibers play a crucial role in modern society, impacting various aspects of daily life, industry, and the environment. ynthetic fibers are integral to modern life, offering a range of benefits from cost-effectiveness and versatility to innovative applications and performance characteristics. While they pose environmental challenges, ongoing research and development aim to create more sustainable and eco-friendly alternatives. Understanding the importance of synthetic fibers helps in appreciating their role in the economy, industry, and daily life, while also emphasizing the need for sustainable practices and innovation.
We all have good and bad thoughts from time to time and situation to situation. We are bombarded daily with spiraling thoughts(both negative and positive) creating all-consuming feel , making us difficult to manage with associated suffering. Good thoughts are like our Mob Signal (Positive thought) amidst noise(negative thought) in the atmosphere. Negative thoughts like noise outweigh positive thoughts. These thoughts often create unwanted confusion, trouble, stress and frustration in our mind as well as chaos in our physical world. Negative thoughts are also known as “distorted thinking”.
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2. OBJECTIVES
1. Define Electron Configuration
2. Discuss the rules in writing electron
configuration
3. Write the full and abbreviated electron
configuration of the elements from any
period of the periodic table.
4. Illustrate the orbital diagram for each
atom based on their electron
configuration
3. WHAT DID YOU REMEMBER?
1. How will you describe the location of electrons revolving
around the nucleus of an atom?
2. What are quantum numbers?
3. What do these quantum numbers describe?
4. How do we compute for the maximum orbitals per
energy level?
5. How do we compute for the maximum number of
electrons per energy level?
6. ELECTRONIC CONFIGURATION OF AN ATOM
- the arrangement of electrons in the orbital of an
atom.
- described by
a. a number that designates the number of principal shell
b. a letter that designates the subshell (orbital)
c. a subscript that designates the number of electrons in
that particular subshell (orbital)
Example:
2p4 indicates 4 electrons in the p subshell of the 2nd
shell.
3d8 indicates 8 electrons in the d subshell of the 3rd
shell.
7. RULES FOR ELECTRON
CONFIGURATIONS
In order to write an electron
configuration, we need to know the
RULES.
3 rules govern electron
configurations.
Aufbau Principle
Pauli Exclusion Principle
Hund’s Rule
Using the orbital filling diagram at
the right will help you figure out
HOW to write them
Start with the 1s orbital. Fill each
orbital completely and then go to
the next one, until all of the
elements have been acounted for.
8. a. AUFBAU (BUILDING-UP) PRINCIPLE
“Electrons in an atom occupy first
the lowest possible energy levels
and/or orbitals.”
Order: 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d
5p 6s 4f 5d 6p 7s 5f 6d 7p
9. NO MORE THAN 2 ELECTRONS IN ANY
ORBITAL…EVER.
The next rule is the Pauli Exclusion Principle.
“No two electrons in the same atom can have the
same set of four quantum numbers, i.e., the
maximum number of electron in an orbital is
limited to two.”
The spins have to be paired.
We usually represent this with an up arrow and a
down arrow.
Since there is only 1 s orbital per energy level,
only 2 electrons fill that orbital.
Wolfgang Pauli, yet
another German Nobel
Prize winner
Quantum numbers describe an electrons position, and no 2
electrons can have the exact same quantum numbers. Because of
that, electrons must have opposite spins from each other in order
to “share” the same orbital.
10. b. PAULI’S EXCLUSION PRINCIPLE
*For 1s orbital:Max electron = 2
one electron: n=1, l=0, ml=0,ms=+½
one electron: n=1, l=0, ml=0,ms=-½
11. HUND’S RULE
Hunds Rule states that when you get
to degenerate orbitals, you fill them
all half way first, and then you start
pairing up the electrons.
What are degenerate orbitals?
Degenerate means they have the
same energy.
So, the 3 p orbitals on each level are
degenerate, because they all have the
same energy.
Similarly, the d and f orbitals are
degenerate too.
Don’t pair up the 2p
electrons until all 3
orbitals are half full.
12. EXCEPTION TO THE RULE
• There are two main exceptions to electron configuration:
chromium and copper.
• In these cases, a completely full or half full d sub-level is
more stable than a partially filled d sub-level, so an
electron from the 4s orbital is excited and rises to a 3d
orbital.
14. SAMPLE PROBLEM Determining Electron Configuration
PLAN:
SOLUTION:
PROBLEM: Using the periodic table give the full and condensed electrons
configurations, partial orbital diagrams showing valence electrons,
and number of inner electrons for the following elements:
(a) potassium (K: Z = 19) (b) molybdenum (Mo: Z = 42) (c) lead (Pb: Z = 82)
Use the atomic number for the number of electrons and the periodic
table for the order of filling for electron orbitals. Condensed
configurations consist of the preceding noble gas and outer electrons.
(a) for K (Z = 19)
1s22s22p63s23p64s1
[Ar] 4s1
4s1
condensed configuration
partial orbital diagram
full configuration
There are 18 inner electrons.
3d 4p
15. (b) for Mo (Z = 42)
1s22s22p63s23p64s23d104p65s14d5
[Kr] 5s14d5
(c) for Pb (Z = 82)
[Xe] 6s24f145d106p2
condensed configuration
partial orbital diagram
full configuration
5s1 4d5
condensed configuration
partial orbital diagram
full configuration 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p2
There are 36 inner electrons
and 6 valence electrons.
6s2 6p2
There are 78 inner electrons
and 4 valence electrons.
5p
16. ACTIVITY
a. Write the expanded/full electron configurations of the
following elements:
1) Calcium
2) potassium
b. Write the abbreviated electron configurations of the
following elements:
3) Aluminum
4) Copper
c. Illustrate the orbital diagram of Rubidium (Rb)
17. ASSESSMENT
1. Write the electron configurations (FULL &
ABBREVIATED) of each of the following atoms.
1. Scandium
2. Gallium
2. Determine what elements are denoted by the following
electron configurations:
3. [Kr] 5s24d105p3 ____________________
4. [Xe] 6s24f145d6 ____________________
c. Illustrate the orbital diagram for number #4.
18. “ We should rather be an ELECTRON so
that we may able absorb and release
energy to be a good and useful particle
moving around the earth…”
-Yours truly-
Words to live by….