Electron Configuration And Lewis Structures Flashcards

1
Q

binding energy depends on

A

n and l

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2
Q

difference in binding energy due to having a multi electron system

A

based on z effective, not z

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3
Q

Hunds Rule

A

when e- are added to states if the same energy, a single electron enters each state before a second does

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4
Q

paramagnetic

A

energy state has an unpaired electron

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5
Q

diamagnetic

A

no unpaired electron

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6
Q

most stable electron configurations

A

filled or 1/2 filled

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7
Q

aufbau principle

A

fill energy state 1 at a time, starting with fhe lowest energy

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8
Q

anion

A

ion that gained an electron and has a negative charge

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9
Q

cation

A

ion that lost an electron and is positively charged

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10
Q

transition metals lose what first

A

4s

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11
Q

relationship between IE2 and IE

A

IE2 is always greater than IE

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12
Q

when an ion is by itself charge =

A

oxidation state

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13
Q

isoelectronic

A

same electron configuration

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14
Q

Zeff

A

effective nuclear charge

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15
Q

Zeff trend (and why)

A

▪ increase across periodic table (bc more protons)

▪decrease down periodic table (bc n inc)

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16
Q

ionization energy is always a ______ value

A

positive

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17
Q

ionization energy trends

A

▪inc across periodic table

▪dec down periodic table

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18
Q

Electron affinity

A

ability of an atom to gain electrons

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19
Q

electron affinity = -______

A

change in energy

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20
Q

positive electron affinity means

A

atom wants an electron

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21
Q

electron affinity trends (and why)

A

▪inc across periodic table
▪dec going down
▪bc Zeff

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22
Q

electronegativity

A

the net ability of an atom to attract an electron from another atom

23
Q

electron acceptor

A

atom with high electronegativity

24
Q

electron donor

A

atom with low electronegativity

25
electronegativity trends
▪inc across | ▪dec down
26
msot electronegative element
flourine
27
noble gas electronegativity
0
28
atomic radius trend (and why)
▪Dec across period table (bc Zeff inc) | ▪inc down periodic table (bc n inc)
29
electronegativity inc by what amount across the periodic table?
.5
30
difference of electronegativity causes
a polar molecule
31
ionic bonds
transfer of one or more electrons from one atom to another with a bond
32
ionic bonds are caused by
coulombic attraction
33
covalent bonding
▪a pair of electrons are shared between 2 atoms
34
on covelnt bond graph, the x intercept =
bond length (sharing electrons at a good distance)
35
on covelent binding graph, difference between x intercept and asymptote =
dissociation energy
36
dissociation energy
energy required to seperate bonded atoms
37
deeper well in covalent bonding graph=
stronger bond
38
energy of interaction
nuclear-nuclear repulsion + electron-nucleur attraction + electron-electron repulsion
39
polar covalent
unequal sharing of electrons between 2 atoms w a different electronegativities
40
difference between electronegativities to form a polar covalent bond
.4 < x< 1.7
41
octet rule
electrons distributed in such a way that each element is surrounded by 8 electrons
42
coreect lewis structure has the ________ formal charge
least complicated
43
if a lewis structure only has single bonds it has no ______
resonance structures
44
octet rule exceptions
▪odd number of electrons ▪octet deficient molecules ▪valence shell expansion
45
radical species
molecules with an unpaired electron
46
valence shell expansion
element with n greater than or equal to 3 can have more than 8 electrons around the central atom
47
ionic bonds are between a
mental and nonmetal
48
less than an octet most often occurs with the elements
▪Boron (B) ▪Beryllium (Be) ▪aluminum (Al)
49
covalent bondimg occurs between
2 nonmetals
50
orbital filling exceptions
Cr, Cu
51
Cr electron configuration
▪6 total electrons ▪4s orbital filled with one ▪3d each filled with one
52
Cu electron configuration
▪11 total electrons ▪4s with 1 ▪3d completely filled
53
group with the highest electron affinity
halides
54
methyl group
CH3