ch 7

Question 1

what does the pauli exclusion says

Answer 1

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

Question 2

when is the shell more stable

Answer 2

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

Question 3

subshell stability

Answer 3

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

Question 4

energy of shells get closer together as n gets

Answer 4

larger

Question 5

effective nuclear charge Z*
the larger Z*

Answer 5

the more stable it is

Question 6

what is Z*

Answer 6

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

Question 7

how many orbitals in s

Answer 7

1

Question 8

how many orbitals in p

Answer 8

3

Question 9

how many orbitals in d

Answer 9

5

Question 10

How many orbitals in f

Answer 10

7

Question 11

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

Answer 11

n^2

Question 12

what is the exception with the transition metal and d subshell

Answer 12

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)

Question 13

electron configuration for anions

Answer 13

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

Question 14

electron configuration for cations

Answer 14

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.

Question 15

isoelectronic species

Answer 15

same number of electrons and same electron configuration

Question 16

what are the most stable ions of atoms?

Answer 16

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

Question 17

Diamagnetic

Answer 17

all electrons are paired

Question 18

paramagnetic

Answer 18

unpaired electrons will be attracted to a magnetic field

Question 19

z effective nuclear charge

Answer 19

nuclear charge that is felt by the valence electron

Question 20

electrons are attracted to the

Answer 20

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

Question 21

nuclear shielding

Answer 21

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

Question 22

core electrons

Answer 22

electrons in the inner shell

Question 23

valence electrons

Answer 23

electrons in the outermost shell

Question 24

valence electrons are attracted and repelled by what

Answer 24

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

Question 25

Zeff formula

Answer 25

Zeff = Z - S
Z=atomic number
S= # of core electrons

Question 26

How does Zeff increases?

Answer 26

Up and right

Question 27

To the righ Zeff

Answer 27

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

Question 28

Moving down Zeff

Answer 28

As we move down a group, the number of core shells increases so shielding increases and Zeff decreases

Question 29

total e formula

Answer 29

total electrons= core + valence
valence electrons can be found in periodic table in family
total electrons is the element #

Question 30

Atomic radius trend

Answer 30

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.

Question 31

Trend for atomic radius for cations

Answer 31

In cations, electrons are removed so it becomes more positive, therefore Zeff increases cause more pull and Atomic radius decreases.

Question 32

Trend for atomic radius for anions

Answer 32

In anions, electrons are added so it becomes negative, therefore there is less pull so less Zeff and the atomic radius is larger.

Question 33

comparing atomic radius between isoelectronic species

Answer 33

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

Question 34

Ionization energy trend

Answer 34

Increases up and right

Question 35

what is ionization energy

Answer 35

How much energy is required to remove the outermost electron from an atom or ion in the gas phase

Question 36

what electrons are easier to remove?

Answer 36

valence

Question 37

Electron Affinity

Answer 37

It is the amount of energy involved with adding an electron to an ion or atom

Question 38

What happens if Ea is negative

Answer 38

energy is released, it goes into a lower state, the atom is more stable and it likes to have an e added

Question 39

what happens if Ea is positive

Answer 39

energy is absorbed, it goes into a higher energy state, the atom is less stable, it does not like to have an e added

Question 40

Trend for Ea

Answer 40

Ea increases upwards and to the right

Question 41

electronegativity trend

Answer 41

upwards and to the right

Question 42

Most electronegative atoms

Answer 42

F>O>N>Cl>Br>I>S>C>H

Question 43

electronegativity measures

Answer 43

the amount of e pull