Quantum Mechanics quest

Question 1

Emission spectra are characterized by narrow bright lines of different color T/F

Answer 1

True

Question 2

Imagine an emission spectrum produced by a container of hydrogen gas. Changing the amount of hydrogen in the container will change the color of the lines in the spectrum T/F

Answer 2

False

Question 3

In the previous question, changing the gas in the container from hydrogen to helium will change the colors of the lines occurring in the spectrum T/F

Answer 3

True

Question 4

An absorption spectrum appears as a continuous spectrum interrupted by a series of dark lines T/F

Answer 4

True

Question 5

The wavelengths of the emissions lines produced by an element are different from the wavelengths of the absorption lines produced by the same element

Answer 5

True but bad question

Question 6

Which statement is true?

Answer 6

none of them

Question 7

Why wrong? An atom emits light when it decays to a lower energy level

Answer 7

Electron not atom

Question 8

Why wrong? An electron transition from the n=2 to the n=1 orbit will emit shorter wavelengths than a transition from the n=3 to the n=1

Answer 8

longer not shorter

Question 9

Why wrong? An atom moving from the n=3 to the n=1 energy level absorbs light

Answer 9

electron not atom

Question 10

Why wrong? An electron emits lights when it is excited to a higher energy level

Answer 10

gains not emits

Question 11

How to draw a Bohr model

Answer 11

1. Figure out e,n,p
2. Put P and N in the nucleus
3. Put electrons in rings around paying attention to how many can go in each ring

Question 12

Spectroscopy

Answer 12

The branch of science concerned with the investigation and measurement of the spectra produced when matter interacts with or emits electromagnetic radiation

Question 13

Continuous spectra

Answer 13

Continuous range of frequencies/wavelengths/energies of electromagnetic radiation

Question 14

Line Spectra

Answer 14

A spectra consisting of discrete frequencies of electromagnetic radiation

Question 15

Emission (bright line) spectra

Answer 15

Results from electrons losing energy when they move from an excited state to the ground state

Question 16

Absorption (dark line) spectra

Answer 16

Results when electrons absorb energy to move from ground to excited state

Question 17

Bohr Model

Answer 17

• In the late 19th century, a mathematical formula that related the various wavelengths of hydrogen emissions lines was discovered
• Goal was to recognize that spectral lines are the result of transitions of electrons between energy levels that correspond to photons of light with an energy and frequency related to the energy spacing between levels
• Wrong because only explains for hydrogen atom

Question 18

Light emission you can’t see

Answer 18

1. Lyman- anything-1; ultraviolet
2. Balmer- anything-2; visible
3. Paschen- anything-3; infrared

Question 19

How may electrons can each ring hold?

Answer 19

1. 2
2. 8
3. 18
   4-7. 32

Question 20

The Quantum Mechanics Model

Answer 20

• The Quantum Mechanics Model describes the most likely location of an election
• It like the address of an electron
• There are four quantum numbers

Question 21

Louis de Broglie

Answer 21

determined electrons can act as waves

Question 22

Werner Heisenberg and Erwin Schrodinger

Answer 22

described mathematically the wave properties of electrons with the quantum theory

Question 23

Energy levels and their number of sub levels

Answer 23

1. s
2. s & p
3. s, p, & d
   4-7. s, p, d, & f

Question 24

How many electrons each sub level can hold

Answer 24

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

Question 25

How many orientations each sub level has

Answer 25

s- 1
p- 3
d- 5
f - 7 
- Each orbital holds 2 electrons 
- Size of orbital determines which energy level its in

Question 26

Aufau principle

Answer 26

• An electron occupies the lowest energy orbital that can receive it
• know how to write the tree thing

Question 27

Pauli Exclusion Principle

Answer 27

• No two electrons in the same atom can have the same set of four quantum numbers
• In the orbital diagram, 2 electrons within the same orbital have to have opposite spins
• Up/Down arrow in the same box

Question 28

Hunds rule

Answer 28

• Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron and all singly occupied orbitals must have the same spin state
• Electrons don’t want to be with each other/double up because they have opposite spins
• 3 boxes each with an arrow in the same direction

Question 29

How to write electron configuration

Answer 29

energy level, sub level, number of electrons, follow tree

Question 30

How to write orbital model

Answer 30

Write EL and SL and then number of orbitals with electrons to fill them

Question 31

Orbital diagram what the represent and what they’re represented by

Answer 31

1. Energy level; state; 1-7
2. Sublevel; city; s p d f
3. Orbital; street; box
4. Spin; house number; arrows

Question 32

Ions

Answer 32

• If its +, take away electrons in orbital model and configuration
• If its -, add to orbital model and configuration

Question 33

Energy level

Answer 33

The size of the area where the electron is found

Question 34

Sub level

Answer 34

The shape of the area where the electron is found

Question 35

Orbital

Answer 35

Orientation in space of that area the election is found

Question 36

Abbreviated configuration

Answer 36

• AKA nobel gas configuration
• Find nobel gas (last column) with the closest (but lower) number of electrons, write that, then the rest of the configuration

Question 37

Excited if

Answer 37

It doesn’t follow the tree order