Magnetism & Electron Configuration Lab Exercise 3.6.1

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Presentation transcript:

Magnetism & Electron Configuration Lab Exercise 3.6.1

Standard Notation of Fluorine Number of electrons in the sub level 2,2,5 1s2 2s2 2p5 Main Energy Level Numbers 1, 2, 2 Sublevels

Shorthand Notation Use the last noble gas that is located in the periodic table right before the element. Write the symbol of the noble gas in brackets. Write the remaining configuration after the brackets. Ex: Fluorine: [He] 2s2 2p5

Condensed ground-state electron configurations in the first three periods.

Magnetism & Electron Configuration: Why is iron magnetic and some metals like copper, nickel, zinc etc are not magnetic? When electrons are paired together, their opposite spins cancel each other. Therefore, no net magnetic field exists. Substances with some unpaired electrons will have a net magnetic field and will attract more to an external field. Materials can be classified as diamagnetic, paramagnetic or ferromagnetic.

Diamagnetic all the electron are paired there is no permanent net magnetic moment Most elements in the periodic table, including copper, silver, and gold, are diamagnetic. Example: Zinc The electron configuration of Znis [Ar] 3d10 4s2. All electrons are paired, and therefore Zn is diamagnetic. The most common ionized form of zinc, Zn(2+) is also diamagnetic. The electron configuration of Zn(2+) is [Ar] 3d10. All electrons are paired, and therefore the Zn(2+) cation is diamagnetic

Have some unpaired electrons Paramagnetic Weakly magnetic Have some unpaired electrons Examples: magnesium, molybdenum, lithium, and tantalum.

exhibit a strong attraction to magnetic fields Ferromagnetic Strongly magnetic exhibit a strong attraction to magnetic fields have some unpaired electrons so their atoms have a net magnetic moment.

Magnetic Properties of Transition Metal Ions Paramagnetic substances are attracted by an external magnetic field. Diamagnetic Species with all paired e’s, not attracted

SAMPLE PROBLEM 8.7 Writing Electron Configurations and Predicting Magnetic Behavior of Transition Metal Ions PROBLEM: Use condensed electron configurations to write the reaction for the formation of each transition metal ion, and predict whether the ion is paramagnetic. (a) Mn2+(Z = 25) (b) Cr3+(Z = 24) (c) Hg2+(Z = 80) PLAN: Write the electron configuration and remove electrons starting with ns to match the charge on the ion. If the remaining configuration has unpaired electrons, it is paramagnetic. SOLUTION: (a) Mn2+(Z = 25) Mn([Ar]4s23d5) Mn2+ ([Ar] 3d5) + 2e- paramagnetic (b) Cr3+(Z = 24) Cr([Ar]4s23d6) Cr3+ ([Ar] 3d5) + 3e- paramagnetic (c) Hg2+(Z = 80) Hg([Xe]6s24f145d10) Hg2+ ([Xe] 4f145d10) + 2e- not paramagnetic (is diamagnetic)

# of unpaired electrons Hund’s rule of maximum multiplicity “Multiplicity” is a measure of the number of unpaired electrons. Multiplicity = number of unpaired electrons + 1 # of unpaired electrons Multiplicity Common Name 1 singlet 2 doublet 3 triplet 4 quartet Hund’s rule: Electrons must be placed in the orbitals of a subshell so as to give the maximum total spin. i.e. put as many unpaired electrons as possible in a subshell to get the most stable arrangement.