25.5 Atomic Structure

Question 1

emission spectrum

Answer 1

unique energetic fingerprint of an atom

Question 2

Ephoton equation (2)

Answer 2

1) Ephoton = h f

2) Ephoton = h (c/λ)

Question 3

what does the bohr model predict for an emission spectra?

Answer 3

elements will have a line emission spectra instead of a continuous spectra
=> only photons with certain energies will be absorbed or released

Question 4

Bohr atom

Answer 4

atom with only 1 electron

Question 5

how does the distance between energy levels change as you increase n?

Answer 5

distance between energy levels DECREASE with increasing n

Question 6

what does a positive or negative ΔEn indicate?

Answer 6

\+ΔEn = E absorbed (photon absorbed, electron jumps)  
-ΔEn = E released (photon emitted, electron falls)

Question 7

quantization

Answer 7

electrons held by an atom only exist at discrete energy levels

Question 8

how does an electron in a higher energy shell compared to one in a lower energy shell

Answer 8

1) higher energy in higher energy shell

2) farther distance from nucleus in higher energy shell

Question 9

orbital

Answer 9

3D region around nucleus in which electron is most likely to be found

Question 10

subshells

Answer 10

complex orbital shapes that describe the most probable regions an electron will occupy (four types exist: s, p, d, f)

Question 11

what happens as you increase the number of energy shells

Answer 11

gain one more subshell (s -> p -> d -> f)

Question 12

how many spin sates can an electron have?

Answer 12

2 (an orbital can occupy one up, one down)

Question 13

electron configuration basic principles (3)

Answer 13

1) Aufbau principle
2) Hund’s rule
3) Pauli exclusion principle

Question 14

Aufbau principle

Answer 14

electrons occupy lowest E orbitals first

Question 15

Hund’s rule

Answer 15

electrons in same subshell occupy availabale orbitals singly first

Question 16

Pauli exclusion principle

Answer 16

only two electrons in any orbital

Question 17

s subshell (# of orbital orientations, max # electrons)

Answer 17

1 orbital orientations

2 electrons

Question 18

p subshell (# of orbital orientations, max # electrons)

Answer 18

3 orbital orientations

6 electrons

Question 19

d subshell (# of orbital orientations, max # electrons)

Answer 19

5 orbital orientations

10 electrons

Question 20

f subshell (# of orbital orientations, max # electrons)

Answer 20

7 orbital orientations

14 electrons

Question 21

noble gases

Answer 21

elements that have all subshells in outermost electron shell filled (full octets)

Question 22

diamagnetic atoms

Answer 22

atoms with all electrons spin-paired

Question 23

paramagnetic atoms

Answer 23

atoms where not all electrons spin-paired

Question 24

diamagnetic atom properties (3)

Answer 24

1) even # of electrons
2) all occupied subshells are filled
3) not attracted to external magnetic field

Question 25

paramagnetic atom properties (2)

Answer 25

1) NOT all occupied subshells are filled

2) attracted to external magnetic field

Question 26

can paramagnetic atoms have even # of electrons

Answer 26

yes (can be even or odd)

=> odd # electrons is definitely paramagnetic though

Question 27

what does the block an atom is in indicate?

Answer 27

block name = highest-energy subshell that contains an electron

Question 28

what is often used as starting points for writing out the electron configurations of an atom?

Answer 28

[noble gases]

Question 29

d block exception

Answer 29

subtract 1 from period #

Question 30

f block exception

Answer 30

subtract 2 from period #

Question 31

what are the anomalous electron configuarion atoms?

Answer 31

Atoms in the Cr and Cu families
- have nd(4) or nd(9) as highest occupied E subshell, so will take one from the previous s subshell to fill up d orbitals

Question 32

isoelectronic atoms

Answer 32

atoms/ions of different elements but have the same electron configuration

Question 33

what electrons are ionized from an atom first?

Answer 33

the valence shell (highest energy orbital) ]

=> except for transition metals: ionize the s orbital electrons, then lose d electrons

Question 34

excited atom

Answer 34

different electron configuration, but will still have same number of electrons (just an electron jumps up to higher level unexpectedly)