Chapter 3

Question 1

n

Answer 1

principal quantum number (energy)

Question 2

l

Answer 2

angular momentum quatum number (shape)

-l=0 to n-1

Question 3

ml

Answer 3

magnetic quantum number (how many of each shape)

ml=-l to 0 to+l

Question 4

ms

Answer 4

spin quantum number (e- pointing up or down)
up=+1/2
down=-1/2

Question 5

pauli exclusion principle

Answer 5

no two electrons can have the same four quantum numbers. They need to differ by at least one value

Question 6

Aufbau principle

Answer 6

first you fill in lower energy levels then higher energy levels

Question 7

periodic table s block

Answer 7

first two groups

Question 8

periodic table p block

Answer 8

last 6 groups that are on the left of the transition metals

Question 9

periodic table d block

Answer 9

transition metals

Question 10

peridodic table f block

Answer 10

the two rows below the periodic table

Question 11

hunds rule

Answer 11

in filling degenerate orbitals (orbitals of the same energy; p-set or d-set or f-set) e- goes in one at a time until each degenerate orbital has one e-, before pairing occurs

Question 12

triplet state

Answer 12

triplet state is an unique state in degerate orbitals (p-set or d-set f-set), when either the degenerate set of orgitals is 1/2 full (i.e. one e- in each) orcompletely full (i.e. two e- in each)
-this is an inherently lower energy state…elements aways like to go to lower energy

Question 13

triplet state exceptions

Answer 13

chromium and copper

• chromium=4s1 3d5
• copper=4s1 3d10

Question 14

noble gas shorthand

Answer 14

you use noble gases to equate to a number of e- in filled orbitals

Question 15

electrons can be split into two major groups

Answer 15

core electrons and valence electrons

Question 16

core electrons

Answer 16

e- that are not in the outtermost principle quantum level…often (but not always) found in the noble gas portion of noble gas shorthand. they are coser to the nucleus.

Question 17

valence electrons

Answer 17

e- that are in that outtermost level of e- configuration. valence e- do all the chemistry!

Question 18

what do group numbers tell you

Answer 18

the number of valence electrons and the idea of the Zeff value

Question 19

Zeff

Answer 19

effective nuclear charge. it is the positive charge that the valence e-‘s feel from the nucleus. the total charge of the nucleus is shielded from valence e- by core e-.

Question 20

Zeff equation

Answer 20

Zeff=Z-S
Zeff=effective nuclear charge
Z=atomic # (# of protons)
S=# of core electrons (# of shielding e-s)

Question 21

electronegativity

Answer 21

increased up and to the right of the periodic table.

Question 22

Zeff trend

Answer 22

increases up and to the right of the periodic table (the same as the electronegativity trends)

Question 23

atomic radius (size)

Answer 23

the larger the Zeff the smaller the size of the atom/element. Greater Zeff holds valence e- tighter and closer
increases down and to the left of the periodic table

Question 24

charged ions

Answer 24

• negative charged ions (anions) are always bigger than their neutral counterpart…because of e-/e- repulsions the ion expands to minimize the e-/e- repulsions
• positive charged ions (cations) are always smaller than their neutral counterpart…because larger nuclear charge holds e- closer/tighter

Question 25

isoelectronic elements

Answer 25

- same number of electrons - due to gaining/losing electrons some elements can have the same # - are ones that have the same number of e- because of charge

Question 26

isoelectronic size

Answer 26

the one with the largest number of protons will be the smallest

Question 27

ionization energy

Answer 27

the energy required (endothermic-+) to remove an electron from an element in the gaseous state, each less of an e- has an ionization energy (energy required to lose an e-) - is same in trend as Zeff (increasing up and to the right of the periodic table) - elements can have more than one ionization energy-always a huge energy to lose an electron in a noble gas e- configuration (cation now isoelectronic w/ noble gas)

Question 28

triplet state beware

Answer 28

if an element is leaving a triplet state, this will be more energetically costly than an element entering a triplet state (so long as in the same n-level)

Question 29

cation affect on atomic size

Answer 29

cation=postive charge | cations are always smaller then their neutral counterpart

Question 30

anion affect on atomic size

Answer 30

anion=negative charge | anions are always larger then their neitral counterpart

Question 31

isoelectronics affect on atomic radius

Answer 31

isoelectronic=same # of e- - the greater number of protons, the smaller the size - the fewer number of protons, the greater the size

Question 32

successive ionization energies

Answer 32

- looking at loss of more than one electron | - a noble gas triplet state is always involved

Question 33

kaddycorner relationship

Answer 33

the vertical direction always wins

Question 34

metallic character

Answer 34

electropositivity -an elements inherent desire to lose e- increases down and to the left

Question 35

paramagnetism

Answer 35

results from an element having unpaired e- in valence shell (paramagnetic elements are attracted to an external magnetic field)

Question 36

diamagnetism

Answer 36

results from an element having all paired e- in valence shell (diamagnetic elements are repelled from an external magnetic field)