Chapter 5-Electron Configuration

Question 1

What can be used to determine electron arrangement in an atom?

Answer 1

set of 3 rules: aufbau principle, Pauli exclusion principle, Hund’s rule

Question 2

All atoms can be described with orbitals similar to…

Answer 2

Hydrogen’s orbitals

Question 3

electron configuration

Answer 3

arrangement of e’s in an atom

Question 4

E’s assume the arrangement that gives the atom the _____ energy possible

Answer 4

lowest

Question 5

ground state e configuration

Answer 5

most stable, lowest energy arrangement of e’s

Question 6

aufbau principle

Answer 6

each e occupies lowest energy orbital available

Question 7

aufbau diagram

Answer 7

shows sequence of atomic orbitals from lowest to highest energy

Question 8

aufbau: all orbitals related to an energy sublevel are of…

Answer 8

equal energy

ex. all three 2p orbitals are of equal energy

Question 9

aufbau: in a multi-e atom, the energy sublevels w/in a principal energy level have…

Answer 9

different energies

ex. the three 2p orbitals are of higher energy than the 2s orbital

Question 10

aufbau: orbitals related to energy sublevels w/in one principal energy level can ____ orbitals related to energy sublevels w/in another principal level

Answer 10

overlap

ex. 4s sublevel has lower energy than 3d sublevel

Question 11

e’s in orbitals are represented by ____ in _____

Answer 11

arrows…boxes

Question 12

empty box represents

Answer 12

unoccupied orbital

Question 13

pauli exclusion principle

Answer 13

max of 2 e’s can occupy a single atomic orbital, but only if they have opposite spins

by Wolfgang Pauli after observing excited atoms

Question 14

max number of e’s related to each principal energy level is…

Answer 14

2n^2

Question 15

Hund’s rule

Answer 15

single e’s w/ same spin must occupy each equal-energy orbital before additional e’s w/ opposite spins can occupy the same orbitals

ex. ^ ^ ^, then ^v ^ ^

Question 16

ways to represent e configuration

Answer 16

orbital diagrams

electron configuration notation

Question 17

orbital diagram

Answer 17

arrows in boxes

each box labeled with principal quantum # and sublevel associated w/ orbital

Question 18

electron configuration notation

Answer 18

1s^2 2s^2…

doesn’t usually show the orbital distributions of e’s related to a sublevel

Question 19

noble gas notation

Answer 19

shortcut e configuration w/ noble gas
has ns^2 and np^6 full

[Ne]3s^2

Question 20

noble gases

Answer 20

elements in last column of periodic table
8 e’s in outermost orbital
stable

Question 21

exceptions to Aufbau Rule

Answer 21

chromium: [Ar]4s1,3d5
copper: [Ar]4s1,3d10

to be more stable, draw box diagram to see (look at video)

Question 22

valence e’s

Answer 22

e’s in outermost orbitals

OCCUPY THE S AND P OF THE SAME HIGHEST ENERGY LEVEL

Question 23

what do valence e’s determine?

Answer 23

chemical properties of an element

Question 24

why do scientists only show valence e’s in e-dot structures?

Answer 24

since these e’s are involved in forming chemical bonds

Question 25

electron dot structure

Answer 25

element's symbol w/ dots around it representing the valence e's

Question 26

who devised the electron dot structure method?

Answer 26

G.N. Lewis (American chemist)

Question 27

Aufbau rule is also called the what?

Answer 27

diagonal rule

Question 28

Which rule supports the box diagram?

Answer 28

Hund's rule

Question 29

isoletric

Answer 29

when atoms have same e configuration

Question 30

How do you determine an atom's charge?

Answer 30

write out e configuration and see if it would be easier to take in e's or lose e's gain: (-) charge lose: (+) charge

Question 31

How to write e configuration of atoms with a charge

Answer 31

ex. Pd^(+2) [Kr]5s2,4d8 --> [Kr]4d8 lose 2 e's (take from outermost orbital w/ highest energy level)

Question 32

diamagnetic

Answer 32

paired e's ^v ^v

Question 33

paramagnetic

Answer 33

unpaired e's aligned w/ a magnetic field ^

Question 34

farromagnetic

Answer 34

unpaired e's that remain aligned when no magnetic field exists *Fe the only element

Question 35

Periodic Table (where are the sublevels located?)

Answer 35

(look at skitch)

Question 36

positive ions are ____ and negative ions are ____

Answer 36

metal non metals

Question 37

In which principal energy level do the different sublevels begin to overlap?

Answer 37

n=4 | the d's

Question 38

what does each sublevel look like?

Answer 38

Spherical: sphere Principal: dumbbell Diffuse: donut shape Fundamental: multiple

Question 39

How many e's can each sublevel hold?

Answer 39

s: 2 p: 6 d: 10 f: 14