CHM 103: Chapter 3
30 Cards in this Set
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Pauli Exclusion Principle
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An atom orbital may describe at most 2 electrons, each with opposite spin direction.
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Hund's rule
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if two or more orbitals of equal energy are available, electrons will occupy them singly before filling them in pairs.
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Does this diagram follow or violate Hund's rule?
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Violates, 2p should have 3 singular electrons
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Does this diagram follow or violate Hund's rule?
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Follows
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Does this diagram follow or violate Hund's rule?
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follows
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electron configuration
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the arrangment of electrons in the orbitals of an atom or molecule
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Valence Electrons
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electrons in outermost energy level of an atom.
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Atoms and ions are considered "isoelectronic" if they have the same
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number of electrons (or electron configuration)
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Electron configuration - complete & shorthand for Sulfur (16)
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S=1s22s22p63s23p4
shorthand
S(16) = [Ne]3s23p4
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Electron configuration - complete & shorthand for Chromium (24)
*special case*
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Cr=1s22s22p63s23p64s13d5
Shorthand
[Ar]=4s13d5
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shorthand” electron configuration for the Iodine atom
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[Kr] 5s2 4d10 5p5
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The distinguishing electron for a Noble Gas is: (what orbital)
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in a p orbital
Specifically, it's "np6," where:
"n" refers to the particular shell (energy level)-also the period
"p" refers to the subshell (the type of orbital)
the "6" indicates that the distinguishing electron is the 6th electron to go into that p subshell
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The distinguishing electron for a Halogen is
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in a p orbital
Specifically, it's "np5,"
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The distinguishing electron for an Alkaline Earth Metal is
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in an s orbital
specifically, it's "ns2"
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The distinguishing electron for a Transition Metal is
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in a d orbital
Realize that d subshells don't occur in the first or second energy levels: So the first d subshell occurs in the third energy level (the third shell).
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The distinguishing electron for an Inner Transition Metal is
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in an f orbital
all 14 of them have their distinguishing electron in a 4f orbital, the f subshells don't occur in the first, second, or third energy levels:
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What subshells are in the third energy level (third shell) of an atom?
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Energy level #3 (shell #3) has 3 subshells: s, p, and d.
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The number of f orbitals in an f subshell is
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7
Because each orbital can hold two electrons, f subshells can hold a total of 14 electrons.
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Atomic Radius
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-half of the distance between the nuclei of the identical atoms
-increases to lower left
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Which element has the smallest atomic radius (meaning smallest electron cloud)?
A.Cs
B.I
C.F
D.Li
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C. Though F has 9 e' (+6 e' than Li), consider:
These 6 add. e` are all in the same shell, same distance from the nucleus, & unable to shield one another from the (+) charge of the nucleus.
The 6 add. protons (to Li) make the e' in the 2nd shell "feel" a much greater effective nuclear…
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The maximum number of electrons that can occupy a p orbital is
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2
Regardless of the type -- s, p, d or f -- all orbitals can hold at most two electrons.
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State the maximum number of electrons that can occupy each sub-shell/orbital
S-block
P block
D block
F block
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s 2
p 6
d 10
f 14
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representative elements
-element located in the s area or the first 5 columns of the p area
-distinguishing electron partially or completely fills an s subshell or partially fills a p subshell
-4 most abundant elements in the body: H, O, C and N are all representative elements
-some …
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halogens - the highly reactive elements of Group 17 on the periodic table
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Alkaline Earth Metals
the metals in Group 2
2 valence electrons
QUITE reactive
lose 2 electrons to become stable
ion charge of +2
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Alkaline Earth Metals
the metals in Group 2
2 valence electrons
QUITE reactive
lose 2 electrons to become stable
ion charge of +2
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transition metals
The elements in groups 3 through 12 in the periodic table. hard metals with high melting points and ions of different colors
ex. iron, cobalt, copper, silver, platinum,
The metallic elements of Groups 3 through 12 on the periodic table
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non-metals
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Metalloids
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post-transition metals
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CHM 103: Chapter 4