ch 7 Flashcards

1
Q

what does the pauli exclusion says

A

no 2 e can have the same 4 quantum numbers and the two e in an orbital must have opposite spins

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2
Q

when is the shell more stable

A

the smaller it is the more stable
1 is more stable than 2 and so on

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3
Q

subshell stability

A

s is more stable than p and so on
s>p>d>f

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4
Q

energy of shells get closer together as n gets

A

larger

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5
Q

effective nuclear charge Z*
the larger Z*

A

the more stable it is

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6
Q

what is Z*

A

is the net force attraction experinced by the outermost electron in an atom

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7
Q

how many orbitals in s

A

1

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8
Q

how many orbitals in p

A

3

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9
Q

how many orbitals in d

A

5

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10
Q

How many orbitals in f

A

7

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11
Q

How to find the total number of orbitals in a given shell

A

n^2

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12
Q

what is the exception with the transition metal and d subshell

A

d subshells prefer to be totally filled or half filled rather than partially filled

the exceptions include everything under Cr and Cu (Mo, Ag, Au)

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13
Q

electron configuration for anions

A

Write out the electron configuration for neutral element
Fill in the desired number of electrons by adding electrons to the highest energy subshell

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14
Q

electron configuration for cations

A

write out the electron configuration for neutral element
remove the desired number of e from first removing from the highest n level and highest energy subshell.

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15
Q

isoelectronic species

A

same number of electrons and same electron configuration

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16
Q

what are the most stable ions of atoms?

A

the most stable ions of atoms are isoelectronic with noble gases or half filled shells.

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17
Q

Diamagnetic

A

all electrons are paired

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18
Q

paramagnetic

A

unpaired electrons will be attracted to a magnetic field

19
Q

z effective nuclear charge

A

nuclear charge that is felt by the valence electron

20
Q

electrons are attracted to the

A

nucleus. the closer they are, the stronger the attraction to the nucleus

21
Q

nuclear shielding

A

inner electrons shield outer electrons from the attractive force of the nucleus

22
Q

core electrons

A

electrons in the inner shell

23
Q

valence electrons

A

electrons in the outermost shell

24
Q

valence electrons are attracted and repelled by what

A

valence electrons are attracted by the positively charged nucleus and repelled by the core electrons

25
Zeff formula
Zeff = Z - S Z=atomic number S= # of core electrons
26
How does Zeff increases?
Up and right
27
To the righ Zeff
as we move to the right in the periodic table , the # of protons increases so Zeff increases because protons are positively charged and so the pulling effect is higher
28
Moving down Zeff
As we move down a group, the number of core shells increases so shielding increases and Zeff decreases
29
total e formula
total electrons= core + valence valence electrons can be found in periodic table in family total electrons is the element #
30
Atomic radius trend
Atomic radius increases down and to the left because as we go down the number of shells increases, Z eff decreases so the radius is larger.
31
Trend for atomic radius for cations
In cations, electrons are removed so it becomes more positive, therefore Zeff increases cause more pull and Atomic radius decreases.
32
Trend for atomic radius for anions
In anions, electrons are added so it becomes negative, therefore there is less pull so less Zeff and the atomic radius is larger.
33
comparing atomic radius between isoelectronic species
Isoelectronic species have the same number of electrons. To compare what AR is larger compare the # of protons (equals to Z the atomic number in the periodic table) more protons means stronger pull, wich means smaller AR less protons than electrons means weaker pull and larger AR
34
Ionization energy trend
Increases up and right
35
what is ionization energy
How much energy is required to remove the outermost electron from an atom or ion in the gas phase
36
what electrons are easier to remove?
valence
37
Electron Affinity
It is the amount of energy involved with adding an electron to an ion or atom
38
What happens if Ea is negative
energy is released, it goes into a lower state, the atom is more stable and it likes to have an e added
39
what happens if Ea is positive
energy is absorbed, it goes into a higher energy state, the atom is less stable, it does not like to have an e added
40
Trend for Ea
Ea increases upwards and to the right
41
electronegativity trend
upwards and to the right
42
Most electronegative atoms
F>O>N>Cl>Br>I>S>C>H
43
electronegativity measures
the amount of e pull
44