Today's class
Ms.K hand out some worksheet today's class. one of them was pattern in electron configuration. One of the many patterns contained in the periodic table is that of electron configuration. In this activity, you will identify these patterns. Later, you will use these patterns to determine the order in which electrons fill the orbitals of an atom.
Valence electrons
Valence electrons are electrons that are in the highest principal energy level of an atom. Each of the group 1A elements has one electron in its highest energy level; each elements has one valence electron.This is no coincidence. The group 1A elements have similar chemical properties because they all have the same number of valence electron configuration of s1. Like wise, each group 2A elements has a valence electron configuration of s2. Tomorrow's scribe is Yonas
Showing posts with label electron configuration. Show all posts
Showing posts with label electron configuration. Show all posts
Thursday, March 12, 2009
Tuesday, March 10, 2009
03/10/09
TODAY'S CLASS:
Ms. K read through the GR 12 CHEMISTRY Atomic Structure: ELECTRON CONFIGURATIONS handout.
Introduced in the handout was electron configuration, being the arrangement of electrons in an atom. Atom's always want to be in their lowest-energy system possible, to remain most stable. The three rules/principles of how orbitals are filled are:
a) The Aufbau principle
- which states that each electron fills the lowest energy orbital available. For example, the aufbau diagram shows how the energy increases from 1s, 2s, 2p,3s,3p and so on.
b) The Pauli exclusion principle
- which states that a maximum of two electrons may occupy an orbital, but only if the electrons have opposite spins. The opposite spins are represented by two arrows, one pointing up, and the other pointing down.
c) Hund's rule
- which states that single electrons with the same spin must sit in each equal orbital before electrons with opposite spins can fill the same orbitals.
We also learned how to use a sublevel diagram, which will help when remembering how to fill orbitals. It is on page 2 of the handout, or uploaded below.
We were then assigned the 'Problems on Electron Configurations' on the back page.
I hope I blogged properly! Have a good night. Yonas, you can scribe
Ms. K read through the GR 12 CHEMISTRY Atomic Structure: ELECTRON CONFIGURATIONS handout.
Introduced in the handout was electron configuration, being the arrangement of electrons in an atom. Atom's always want to be in their lowest-energy system possible, to remain most stable. The three rules/principles of how orbitals are filled are:
a) The Aufbau principle
- which states that each electron fills the lowest energy orbital available. For example, the aufbau diagram shows how the energy increases from 1s, 2s, 2p,3s,3p and so on.
b) The Pauli exclusion principle
- which states that a maximum of two electrons may occupy an orbital, but only if the electrons have opposite spins. The opposite spins are represented by two arrows, one pointing up, and the other pointing down.
c) Hund's rule
- which states that single electrons with the same spin must sit in each equal orbital before electrons with opposite spins can fill the same orbitals.
We also learned how to use a sublevel diagram, which will help when remembering how to fill orbitals. It is on page 2 of the handout, or uploaded below.
We were then assigned the 'Problems on Electron Configurations' on the back page.
I hope I blogged properly! Have a good night. Yonas, you can scribe
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