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To determine the electron configuration of any of the first 38 elements of the periodic table. To determine the identity of an element from its electron configuration. To complete an orbital diagram using arrows to represent electrons.
ORBITAL DIAGRAM Y ↿⇂ 1s ↿⇂ 2s ↿ ↿ ↿ 2p N Fill orbitals with “up” before “down” to maximize number of unpaired electrons. ↿⇂ 1s ↿⇂ 2s ↿⇂ ↿⇂ ↿⇂ 2p Na ↿⇂ 3s ↿⇂ 3s Fe ↿⇂ ↿⇂ ↿⇂ 3p ↿⇂ 4s ↿⇂ ↿⇂ ↿⇂ ↿⇂ ↿⇂ 3d Let’s only worry about the outermost orbitals for Fe.
• Each orbital can contain 0, 1, or 2 electrons (and no more!). • Electrons always fill up the lowest energy orbital first. The lowest energy orbital is in shell 1 and subshell s. The subshells contained within a shell are ordered in this way: • Lowest energy s < p < d < f highest energy
Chemistry: Orbital Diagrams. Using forward slashes ( / ) and backslashes ( \ ), construct the orbital diagram for each of the following elements. Orbitals...
orbitals. Electrons in orbitals are shown using arrows, where the direction of the arrow indicates the spin state of the electron. For example, in the diagram that follows, the upward ( ) and downward ( ) arrows indicate electrons in different spin states.
The orbital occupied by the 1st and 2nd electrons make up shell one, and the 4 orbitals occupied 3rd by the through 10th electrons make up shell two. As we’ll see, when atoms bond together into molecules, the orbitals change shape and in many cases the orbitals of multiple atoms merge.
An orbital is a region in 3-D space where there is a high probability of finding the electron. An orbital is, so to speak, a house where the electron resides. Only two electrons can occupy an orbital, and they must do so with opposite spin quantum numbers ms. In other words, they must be paired.
