Chapter 8

Question 1

Pauli Exclusion Principle

Answer 1

no two electrons in an atom can have the same 4 quantum numbers

Question 2

What does the Pauli Exclusion Principle imply?

Answer 2

each orbital can have a max of 2 electrons with opposing spins

Question 3

degenerate

Answer 3

orbitals that have the same energy

Question 4

Coulomb’s Law

Answer 4

the potential energy (E) of two charged particles depends on their charges (q1 and q2) and their separation (r)

Question 5

Coulomb’s Law - like charges

Answer 5

potential energy (E) is positive and decreases as the particles get farther apart

Question 6

Coulomb’s Law - opposite charges

Answer 6

potential energy (E) is negative and becomes more negative as the particles get closer together

Question 7

Coulomb’s Law - magnitude

Answer 7

magnitude of interaction between charged particles increases as the charges of the particles increase. An electron with a charge of 1- is more strongly attracted to a nucleus with a charge of 2+ than it would be with a charge of 1+

Question 8

shielding

Answer 8

repulsion of one electron by other electrons shield that electron from the full effects of the nuclear charge

Question 9

effective nuclear charge

Answer 9

charge on an electron after shielding. ex: electron would experience a 1+ charge if the nucleus is 3+ and there’s a 2- charge from other electrons

Question 10

aufbau principle

Answer 10

electrons occupy lowest energy orbitals available

Question 11

Hund’s rule

Answer 11

pattern of filling orbitals with 1 electron first with parallel spins and then pairing

Question 12

inner electron configuration

Answer 12

using the previous nobel gas symbol in brackets, then the remaining electrons

Question 13

valence electrons

Answer 13

main group = those in outermost principle energy level

transition group = also include d electrons in valence electrons

Question 14

core electrons

Answer 14

those in complete principal energy levels and in complete d and f sub levels. ex: 1s2 2s2 2p6 3s2 3p2 has 4 valence electrons (in n=3 principal level) and 10 core

Question 15

periodic table blocks that correspond to quantum sub level

Answer 15

s = rows 1 and 2, d = transition, p = rows 3-8, f = off the table

Question 16

writing electron configuration from periodic table

Answer 16

main group - group number = # of valence electrons; row number = highest principle quantum #
transition (d block) - principal quantum # of d orbitals = n-1. ex: row 4 could have 3d1 in electron config.
inner transition (f block) - fill across each row as row # minus 2

Question 17

relationship between full energy level and overall energy of electrons

Answer 17

full quantum level = stable

elements with electron config. close to noble gas = most reactive

Question 18

bonding radius

Answer 18

nonmetals - 1/2 the distance between two of the atoms bonded together
metals - 1/2 distance between two atoms next to each other in a crystal

Question 19

atomic radius

Answer 19

average bonding radii
as you move down a column, atomic radius increases
as you move right, atomic radius decreases
transition elements have a relatively constant radius

Question 20

effective nuclear charge

Answer 20

charge on outer electrons after shielding. actual nuclear charge - charge shielded by core electrons. ex: nucleus +3 and core electrons -2 would equal +1 effective charge

Question 21

removing electrons

Answer 21

main group cation = remove in reverse order of how they’re filled
transition metal cation = remove from highest n first, this is often s and not d

Question 22

magnetic properties

Answer 22

unpaired electrons = attracted to external magnetic field (paramagnetic)
paired electrons = not attracted to external magnetic field (diamagnetic)

Question 23

ionic radii

Answer 23

cation = much smaller than corresponding atom
anion = much larger than corresponding atom

Question 24

ionization energy

Answer 24

energy required to remove electron from atom or ion is gas state

Question 25

electron affinity

Answer 25

energy change associated with gaining an electron in gas state
not a periodic trend for groups except for 1a- EA becomes more positive as you move down a row
as you move right across a row, EA becomes more negative (adding electron becomes more exothermic)

Question 26

metallic character

Answer 26

decreases as you move right across row

increases as you move down a column