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Electron Configuration and Emission Spectrum: Understanding Atoms and Bright Line Spectra, Lecture notes of Chemistry

Dakota County Technical CollegeChemistry

An in-depth exploration of electron configuration and emission spectra. It explains how the number of principle energy levels and electrons in each level can be determined from an atom's electron configuration. Additionally, it discusses the Bohr model, the production of bright line spectra, and how elements can be identified based on their unique electron configurations.

Typology: Lecture notes

2021/2022

Uploaded on 09/12/2022

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ElectronConfigurationandEmissionSpectrum2020
1
October05,2020
Oct245:37PM
1. By looking at the electron configuration, how
many principle energy levels does phosphorus
have?
2. How many electrons are in each principle
energy level? (I.e.: For oxygen; e‐ configuration
(2‐6), it has 2 in the first energy level and 6 in
the second energy level.
The electron configuration tells us two things about the a tom:
•
How many occupied principle energy levels the element has.
•
How many electrons are in each principle energy level (PEL).
DO NOW: Please open your packet to page 13 and answer the
questions below:
Oct209:18PM
Bohr Model and the
Bright Line Spectrum
Aim:
What does the electron configuration tell us about an atom?
How and why do atoms become excited and produce the
bright line spectrum?
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Download Electron Configuration and Emission Spectrum: Understanding Atoms and Bright Line Spectra and more Lecture notes Chemistry in PDF only on Docsity!

Oct 245:37 PM

  1. By looking at the electron configuration, how many principle energy levels does phosphorus have?
  2. How many electrons are in each principle energy level? (I.e.: For oxygen; e‐ configuration (2‐6), it has 2 in the first energy level and 6 in the second energy level.

The electron configuration tells us two things about the atom:

  • How^ many^ occupied^ principle^ energy^ levels^ the^ element^ has.
  • How many electrons are in each principle energy level (PEL). DO NOW: Please open your packet to page 13 and answer the questions below: Oct 209:18 PM

Bohr Model and the

Bright Line Spectrum

Aim:

What does the electron configuration tell us about an atom?

How and why do atoms become excited and produce the

bright line spectrum?

Oct 246:51 PM Bohr's Theory

  1. Principle energy levels (shells) hold the electrons.
  2. ‐Electrons closer to the nucleus have lower energy (more stable). ‐Electrons farther from the nucleus have higher energy (less stable).
  3. Each energy level holds a maximum number of electrons based on the formula: # e = 2n 2 ; n= the # of principle energy level
  4. Ground state atoms have it's electrons in the lowest energy levels, as close to the nucleus as possible. Nov 284:16 PM

Ground vs. Excited

  • GROUND STATE configurations are shown on the periodic table.

Nov 284:16 PM

  • Bright^ Line^ Emission^ Spectrum:^ energy

released as light when an excited

electron returns to ground state.

  • The^ electron^ goes^ from^ a^ higher^ PEL^ back^ to^ a

lower PEL to release the energy as light.

Nov 284:16 PM

Hydrogen

Helium

Carbon

  • Elements^ can^ be^ identified^ by^ their^ bright^ line^ spectrum,

BECAUSE they have their own unique electron configuration.

Helium Carbon

Nov 2011:02 AM

How are lithium and sodium different in terms of their

electrons?

Hydrogen Helium Carbon

DO NOW QUESTION

Nov 2011:02 AM

How are lithium and sodium different in terms of their

electrons?

Hydrogen Helium Carbon

DO NOW QUESTION

  • The electron configuration for

every element is different

because every atom has their

own number of protons and the

protons=electrons for neutral

atoms.

BECAUSE ALL ELEMENTS HAVE THEIR OWN ELECTRON

CONFIGURATION THEY HAVE THEIR OWN BRIGHT LINE SPECTRUM.

Nov 284:55 PM

  1. Given the following electron configurations, identify each element a. 2881 _________________ b. 28185 _________________ c. 21 _________________ d. 28181 _________________ e. 282 _________________
  2. Given the following electron configurations, determine whether the atom is in the ground state or excited state. Also identify each element. Ground or excited Name of Element a. 28162 _________ __________ b. 241 _________ __________ c. 2871 _________ __________ d. 281 _________ __________ e. 276 _________ __________ Nov 284:55 PM
  3. Write the electron configuration for each of the following elements. a. Boron _________________ b. Chlorine _________________ c. Potassium_________________ d. Zinc_________________ e. Iron_________________
  4. Write the electron configuration for each of the following ions: a. Li+1^ _____________________ c. Ca+2 ______________________ b. O^2 _____________________ d. As+3 ______________________
  5. Identify the noble gas that each of the above ions are isoelectronic with (has a matching electron configuration) a. Li+1^ _____________________ c. Ca+2 ______________________ b. O 2 _____________________ d. As 3

Dec 165:25 PM Dec 165:28 PM