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Flashcards in Quantum Mechanics quest Deck (37):
1

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

True

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

False

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

True

4

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

True

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

True but bad question

6

Which statement is true?

none of them

7

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

Electron not atom

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

longer not shorter

9

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

electron not atom

10

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

gains not emits

11

How to draw a Bohr model

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

12

Spectroscopy

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

13

Continuous spectra

Continuous range of frequencies/wavelengths/energies of electromagnetic radiation

14

Line Spectra

A spectra consisting of discrete frequencies of electromagnetic radiation

15

Emission (bright line) spectra

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

16

Absorption (dark line) spectra

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

17

Bohr Model

- 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

18

Light emission you can't see

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

19

How may electrons can each ring hold?

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

20

The Quantum Mechanics Model

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

21

Louis de Broglie

determined electrons can act as waves

22

Werner Heisenberg and Erwin Schrodinger

described mathematically the wave properties of electrons with the quantum theory

23

Energy levels and their number of sub levels

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

24

How many electrons each sub level can hold

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

25

How many orientations each sub level has

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

26

Aufau principle

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

27

Pauli Exclusion Principle

- 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

28

Hunds rule

- 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

29

How to write electron configuration

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

30

How to write orbital model

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

31

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

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

32

Ions

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

33

Energy level

The size of the area where the electron is found

34

Sub level

The shape of the area where the electron is found

35

Orbital

Orientation in space of that area the election is found

36

Abbreviated configuration

- 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

37

Excited if

It doesn't follow the tree order