Pauli exclusion - CORRECT ANSWER no two electrons can have the same 4 numbers
Hunds rule - CORRECT ANSWER dont pair up electrons until you have too
n - CORRECT ANSWER principle quantum number
-size
-n=row on table
l - CORRECT ANSWER azimuthal number
-shape of orbital
,-(n-1)
m - CORRECT ANSWER magnetic quantum number
-orientation of the particle in space
-includes 0
-number of orbitals possible
spin quantum number - CORRECT ANSWER tells about the spin of the electron
(pauli exclusion principle)
d block
f block - CORRECT ANSWER d block= 1 number less
f block= 2 number less
d block valence electrons - CORRECT ANSWER count d and s shell
what are the electron configuration exceptions - CORRECT ANSWER chromium (cr) group and copper
(cu) group
even numbers= - CORRECT ANSWER diamagnetic (exceptions are 10,16)
odd numbers - CORRECT ANSWER paramagnetic
unpaired
,ionic bonds have _____ mp, ______ bp, brittle, hard - CORRECT ANSWER high high
what is lattice energy - CORRECT ANSWER energy required to separate an ionic compound cations from
its anions
lattice energy formula - CORRECT ANSWER (charges)/bond distance
-greater charge = greater lattice energy
-shorter bond distance= greater lattice energy
Which of the following has the largest lattice energy
Li-F
Li-Cl
Li-Br
Li-I - CORRECT ANSWER Li-F
since it has the smallest size distance
due to F being a smaller atom compared to the others
metalloids - CORRECT ANSWER
is gas compressible - CORRECT ANSWER yes
conforms to volume and shape
simple unit cell atoms - CORRECT ANSWER 1
, body centered unit cell atoms - CORRECT ANSWER 2
face centered unit cell atoms - CORRECT ANSWER 4
amorphous solid - CORRECT ANSWER no ordered 3D arrangement
alkali metals have ________ ionization energy thus have high _________ - CORRECT ANSWER low
ionization energy
high reactivity
electron affinity - CORRECT ANSWER energy released when an electron is added to an atom in the gas
phase
-exothermic reaction
-exceptions : Be, N, Noble gases= 0
-Ne has no electron affinity
Ionization energy - CORRECT ANSWER minimum energy needed to remove an electron from an atom in
the gas phase
Why does ionization energy decrease as you move down a group - CORRECT ANSWER 1. electron
shielding: making it easier for outer electrons to be removed
Why does ionization energy increase as you move across a period - CORRECT ANSWER atomic radius
decreases thus the outer electrons become attracted to the nuclelus
becomes harder to remove the outer electron
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