Quantam Mechanics

Question 1

A new model

Answer 1

The Rutherford model did explain what kept the -e’s from crashing into the the nucleus

Question 2

ground state

Answer 2

the normal configuration for an atom. all e-s are at their lowest possible energy state

Question 3

Exited state

Answer 3

when energy is added to an atom through heat or electricity some electrons jump up to higher energy levels

Question 4

absorption

Answer 4

when electrons go into higher levels but don’t stay there

Question 5

emission

Answer 5

when the electrons go back to the ground state and it releases energy. and it does this in the form of light. we call this a photon

Question 6

What kind of wave is light

Answer 6

electromagnetic wave

Question 7

spectrum of light

Answer 7

radio, microwave, infrared, visible, ultraviolet, x-ray, gamma ray
radio is the largest wavelength, gamma is the smallest,
radio has the least hertz gamma and the most

Question 8

how fast do electromagnetic waves travel

Answer 8

2x10 to the power of 8 m/s

Question 9

wavelength

Answer 9

the distance from crest to crest or trough to trough (measured in nm)

Question 10

frequency

Answer 10

the number wave lengths that pass per second (hertz- hz)

Question 11

what is the formula for speed

Answer 11

speed= wavelength x frequency

Question 12

c = λf or v

Answer 12

c= speed of light (m/s) λ= wavelenght n/m f or v= frequency
formula for the speed of a wave

Question 13

Werner heisenberg= Particles behave like waves

Answer 13

showed that we could not know the speed and location of e’s at the same time (uncertainty principle)

Question 14

Erwin shrödinger= Particles behave like waves

Answer 14

came up with the equation to show where the electrons could be along paths called wave functions

Question 15

what does light behave like

Answer 15

light can also behave like a particle as it does in the photoelectric effect but it can also behave like a wave

Question 16

photoelectric effect

Answer 16

when the light of certain frequencies shines on a metal, electrons are emitted

Question 17

what did Albert Einstein win his award for

Answer 17

the photo-electric effect

Question 18

Quantum Numbers

Answer 18

a set of 4 characters that describe the properties of each electron (every electron has its own 4-character code)

Question 19

Orbital

Answer 19

an orbital is a 3-dimensional space around the nucleus that indicates the location of an e 90% of the time

Question 20

Principal quantam number (1)

Answer 20

-symbolized by n=1,2,3 etc…
-indicates the main energy level
-occupied by the e (also called the shells)
-as n increases distance from the nucleus increases

Question 21

azimuthal quantam number(2)

Answer 21

• symbolized by l=s,p,d,f or g hypothetically
  -indicates the shape of the orbital
  -different orbitals within the same energy levels called sublevels
  -the max number of sublevels (orbital shapes) in an energy level equals the principal quantum number n

Question 22

Magnetic quantum number (3)

Answer 22

-within sublevels, these are the orbitals
-indicates the orientation of the orbital around the nucleus
-each orientation can hold two e’s
-there are n squared orbitals per energy level

Question 23

what does the s orbital look like

Answer 23

a circle

Question 24

what does the p orbital look like

Answer 24

two ovals coming out from the center

Question 25

what does the d sublevel look like

Answer 25

clover leaf with the ovals

Question 26

what does the f sublevel look like

Answer 26

six ovals coming out of the center

Question 27

Spin Quantum number (4)

Answer 27

-has only two possible values 1/2 or negative 1/2 -indicated the directions of the spins a single orbital orientation has the ability to hold a max of two e's which must have opposite spins

Question 28

what is the electron configuration

Answer 28

arrangement of electrons in an atom

Question 29

why are atoms lazy

Answer 29

they want to be in the lowest energy state possible

Question 30

ground state electron configuration

Answer 30

this is the lowest energy arrangement of electrons for each element

Question 31

three rules that govern electron placement

Answer 31

Aufbau principle Hunds Rule Pauli Exculsion Principle

Question 32

Aufbau Principle

Answer 32

an electron occupies the lowest energy orbital that can receive it (lowest energy first)

Question 33

Hunds Rule

Answer 33

orbitals of equal energy are each occupied by 1 electron of the same before any orbital is occupied by a 2nd electron

Question 34

Pauli Exclusion principle

Answer 34

no two electrons in the same atom can have the same set of 4 quantum numbers (opposite spins) no two electrons can have the same numbers

Question 35

electromagnetic radiation

Answer 35

Electromagnetic radiation in chemistry refers to energy that travels through space in the form of waves, which include visible light, ultraviolet, infrared, and other forms of radiation. c=λ⋅ν

Question 36

Electromagnetic Spectrum

Answer 36

refers to the entire range of electromagnetic radiation which is categorized by wavelength or frequency that can interact with matter.

Question 37

Interference pattern

Answer 37

refers to a pattern of light or other waves that occurs when two or more waves overlap and combine. this is a result of wave interference

Question 38

Emission spectrum

Answer 38

refers to the range of wavelengths of light emitted by atoms or molecules. it is unique for every element because every element has a different electron configuration

Question 39

Heisenberg uncertainty principle

Answer 39

In chemistry, it helps explain electron behavior and atomic orbitals. it talks about how it is impossible to know the position and momentum of a particle (like an electron) at the same time

Question 40

orbitals

Answer 40

a region where the atom is 90% of the time. (s,p,d, and f) base on the mathematical equation that schrödinger did which describes the wave-like behavior of electrons

Question 41

what did Schrödinger do for this

Answer 41

The Schrödinger equation explains the quantization of energy levels in atoms. It is fundamental to understanding the electron configurations in atoms and how electrons occupy specific orbitals.