orbitals, electron configs, rules, quantum numbers

Question 1

s orbitals exist from what energy level?

Answer 1

n=1

Question 2

p orbitals exist from what energy level?

Answer 2

n=2

Question 3

d orbitals exist from what energy level?

Answer 3

n=3

Question 4

f orbitals exist from what energy level?

Answer 4

n=4

Question 5

how many electrons can an orbital hold?

Answer 5

2

Question 6

shape of s orbitals?

Answer 6

spherical

Question 7

shape of p orbitals?

Answer 7

dumbbell/infinity shaped

Question 8

shape of d orbitals?

Answer 8

4/5 have clover leaf shape. 1 has a dumbbell with a donut shape

Question 9

shape of f orbitals?

Answer 9

goofy ahh shapes is all im gonna say

Question 10

how many s orbitals are there per shell?

Answer 10

1 (2 e-)

Question 11

how many p orbitals are there per shell?

Answer 11

3 (6 e-)

Question 12

how many d orbitals are there per shell?

Answer 12

5 (10 e-)

Question 13

how many f orbitals are there per shell?

Answer 13

7 (14 e-)

Question 14

diff between dxy and dx^2-y^2?

Answer 14

xy= lobes in between x and y axes
x^2-y^2= lobes go along x and y axes

Question 15

what are degenerate orbitals?

Answer 15

orbitals with the same energy level

Question 16

what does the aufbau principle state?

Answer 16

electrons are always filled from the lowest energy levels to the highest energy levels (s<p<d<f)

Question 17

what do we mean by electron configuration?

Answer 17

list of occupations of electrons in orbitals in an tom, in terms of energy and how electrons fill up in an atom

Question 18

core vs valence electrons?

Answer 18

core= electrons below outermost principal energy level
valence= electrons located in the outermost principal energy level

Question 19

what does Hund’s rule state?

Answer 19

in degenerate orbitals, electrons will first spread out in each orbital (parallel spin) and then pair up.

Question 20

preferred state of degenerate orbitals?

Answer 20

all degenerate orbitals want to be either:
- completely empty
- all half full
- all completely full

Question 21

what are the 4 exceptions in typical electron configurations? are these excited states or not?

Answer 21

1. Cr= [Ar] 4s1 3d5
2. Mo= [Kr] 5s1 4d5
3. Cu= [Ar] 4s1 3d10
4. Ag= [Kr] 5s1 4d10
   ** not excited states!! (i know they look like it)

Question 22

what do we mean by paramagnetic? diamagnetic?

Answer 22

paramagnetic= an orbital has at least 1 unpaired electron
diamagnetic= all electrons in an orbital are paired

Question 23

principal energy levels/principal quantum numbers/”shells” are denoted by what letter? what does this represent?

Answer 23

denoted by n
represents electron’s approximate distance from nucleus

Question 24

how to ID a ground state vs excited state electron configuration?

Answer 24

if previous shell(s) are not full, and outermost shell is not full… (ex. 4s1 3d1)… electron is probably excited

Question 25

what order are valence electrons always lost in? what is this based on?

Answer 25

1. valence p e- 2. valence s e- 3. valence d e- based on relative distance from nucleus

Question 26

anion configurations are always written in ___?

Answer 26

noble gas configuration!!

Question 27

what purpose do quantum numbers have?

Answer 27

specify location of an electron in an atom

Question 28

what is described by the angular momentum quantum number (l)? range?

Answer 28

describes the type of orbital in a given shell (s,p,d,f). l= 0, 1, 2, 3

Question 29

which orbital corresponds to which l value?

Answer 29

l= 0 = s l = 1 = p l= 2 = d l=3 = f

Question 30

what does the magnetic quantum number (ml) describe? range?

Answer 30

specifies 1 degenerate orbital type. ml= -3, -2, -1, 0, 1, 2, 3

Question 31

ranges of magnetic quantum number (ml) for each orbital?

Answer 31

s: ml= 0 (no degenerate orbitals) p: ml = -1, 0, 1 d: ml= -2, -1, 0, 1, 2 f: ml= -3, -2, -1, 0, 1, 2, 3

Question 32

what does the spin quantum number describe (ms)? range?

Answer 32

direction of electron spin ms= 1/2 (spin up) ms= -1/2 (spin down)

Question 33

what is the Pauli exclusion principle?

Answer 33

every electron has a unique set of quantum numbers! no 2 electrons in the same atom have exactly the same energy

Question 34

how to find electron configuration of cations? anions? what order are valence electrons lost in?

Answer 34

cations: - write neutral config first - remove e- from valence shells using the psd order anions: - determine charge based on charge trends from PT - add the needed amount of e- to reach the next noble gas! (always write in noble gas config!) valence p first, then valence s, then valence d electrons