Atomic Theory 1: quantum model and electron config

Question 1

What are quanta

Answer 1

Very tiny, discreet energy packets/bundles, proposed by Max Planck

Question 2

E = hv (what is each variable)

Answer 2

E = energy (J), h = Planck constant (m), v = Frequency (hz)

Question 3

3 rules of electrons

Answer 3

1. Atoms have energy levels for e-
2. e- do not release or absorb energy when moving in same energy level
3. e- release or absorb energy when moving between energy levels

Question 4

What is the ground state and why does it occur

Answer 4

Things prefer low energy. e- go to lowest energy level, aka ground state, achieved by losing energy

Question 5

What is a shell

Answer 5

A shell is the same as the energy level of the e-

Question 6

What is a subshell

Answer 6

A subshell (s p d f) dictates the shape of an atom, each has a type of orbital

Question 7

What is an orbital

Answer 7

An orbital is the space where an e- can exist

Question 8

Quantum numbers

Answer 8

Used to specify something about the orbitals and e- in order to describe the e- of an atom

Question 9

What is the principle quantum number (n)

Answer 9

Size of atomic orbital, where n = 1, 2, 3…7
7 shells for 7 periods in the periodic table

Question 10

Characteristics of quantum number n

Answer 10

Each allowed energy state is given an int number n
Lowest level = ground state, all other levels = excited states
Energy levels increase down a group

Question 11

What is the angular momentum quantum number (l)

Answer 11

The shape of an atomic orbital, where l = 0, 1, 2, 3
Matches with subshell s, p, d, f
s = 0
p = 1
d = 2
f = 3

Question 12

What is the magnetic quantum number (ml)

Answer 12

The orientation in space of a given atomic orbital where m1 = -1…1

Question 13

Subshell and ml for each l

Answer 13

l = 0, (s subshell), ml = 0 (1 orbital)
l = 1 (p subshell), ml = -1, 0, +1 (3 orbitals)
l = 2 (d subshell), ml = -2, -1, 0, 1, 2 (5 orbitals)
l = 3 (f subshell), ml = -3, -2, -1, 0, 1, 2, 3, (7 orbitals)

Question 14

What are electron configurations

Answer 14

Describes how electrons are arranged in atomic orbitals for a specific element

Question 15

S subshell

Answer 15

1 orbital and 2 e-

Question 16

P subshell

Answer 16

3 orbitals and 6 e-

Question 17

D subshell

Answer 17

5 orbitals and 10 e-

Question 18

F subshell

Answer 18

7 orbitals and 14 e-

Question 19

Formula for max number of electrons depending on energy level

Answer 19

2n^2
1 = 2
2 = 8
3 = 18
4 = 32

Question 20

Pauli Exclusion Principle

Answer 20

No two e- in teh same atom can be described by the same set of 4 quantum numbers

Question 21

Aufbau Principle

Answer 21

When filling orbitals, the lowest energy orbitals available are always filled first

Question 22

Hunds Rule

Answer 22

When orbitals of equal energy are being filled, e- are most stable when each orbitals is singly occupied before they are paired

Question 23

What is core notation

Answer 23

Condensed e- configurations, config of previous noble gas is presented by [noble gas]

Ex. [Ne] 3s^2 3p^4 = sulfur

Question 24

Exceptions (s and d subshells)

Answer 24

d^5 (half full) and d^10 (full) = very stable, an e- from the s subshell may move to an unfilled d-subshell such as d^4 and d^9
Watch out for Cr, Cu, Mo, Ag, Au

Question 25

When are subshells most stable

Answer 25

When exactly half filled or fully filled

Question 26

Electron configurations for anions

Answer 26

Electrons are added to the last unfilled sublevel

Question 27

Electron configurations for cations

Answer 27

Electrons removed from the outermost orbitals with the highest energy first (exceptions: d^10 and d^5)

Question 28

What is the spin quantum number (ms)

Answer 28

Possible spin of an electron