Chapter 07: The Quantum-Mechanical Model of the Atom Flashcards

1
Q

Light

A

A form of electromagnetic radiation

Composed of perpendicular oscillating waves
(one = electric field, other = magnetic field)

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2
Q

Electric field

A

A region where an electrically charged particle experiences a force

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3
Q

Magnetic field

A

A region where a magnetized perticle experiences a force

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4
Q

Speed of light

A

c

c = 3.00 × 108 m/s

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5
Q

Wavelength

A

λ (lambda)

The distance between identical points on successive waves

*Inversely proportional to frequency

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6
Q

Amplitude

A

The verticle distance from the midline of a wave to the peak (or trough)

A measure of light intensity

*Directly proportional to total energy of wave
(larger amplitude = more force)

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7
Q

Frequency

A
  • v* (nu)
  • v* = c / λ

The number of waves that pass through a particular point in a given period of time

hertz (Hz) or cycles per second (1 s-1)

1 Hz = 1 s-1

*Directly proportional to total energy of a wave
(More frequency = more total force)

*Inversely proportional to wavelenth

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8
Q

Electromagnetic spectrum

A

Low energy to high:

radio
microwave
infared
visible light
ultraviolet
X-ray
gamma ray

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9
Q

Interference

A

The interaction between waves

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10
Q

Constructive interference

A

Occurs when waves that are in phase interact so that they add to make a larger wave

*Amplitudes are summed making the larger wave

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11
Q

Destructive interference

A

Occurs when waves that are out of phase interact so that they cancel each other out (flat line)

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12
Q

Diffraction

A

Occurs when a traveling wave encounters an obstacle or opening in a barrier that is about the same size as its wavelengh and it bends (diffracts) around it

*Waves diffract

**Particles DO NOT diffract (they just pass through opening)

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13
Q

Interference pattern

A

Inherent characteristic of all waves

Light is diffracted through two slits creating an alternating pattern

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14
Q

Photoelectric effect

A

The observation that many metals emit electrons when light shines on their surface

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15
Q

Quanta or photons

A

Light energy delivered to atoms in “packets”

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16
Q

Photon energy

A

E

E = hv

v = c/λ

Thus:

E = hc/λ

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17
Q

Planck’s constant

A

h

h = 6.626 × 10-34 J×s

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18
Q

Threshold frequency

A

Reached when the energy of a photon is equal to the binding energy of emitted electron

hv = Φ

or E = Φ

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19
Q

Binding energy of emitted electron

20
Q

Kinetic energy of an ejected electron

A

KE = hv - Φ

Excess energy of a photon that is transferred to an electron in the form of kinetic energy

21
Q

Wave-particle duality of light

A

Sometimes light appears to behave like a wave, other times like a particle

Behavior observed depends on experiment

22
Q

Number of photons

A

Number of photons = Epulse / Ephoton

*Ephoton = hc/λ

23
Q

Atomic spectroscopy

A

The study of the electromagnetic radiation absorbed and emitted by atoms

24
Q

Emission spectrum

A

The “fingerprint” of an element in the form of a series of bright lines

Can be used to identify an element

25
Bohr model of the atom (4)
1. Energy of atom is quantized (can only have very specific amounts of energy 2. Amount of energy in atom relates to electron's position in atom 3. Electrons travel in orbits/fixed distance from nucleus \*Energy of electron proportional to distance 4. Electrons emit radiation when they "jump" from an orbit with higher energy down to lower energy orbit \*Distance determins energy of photon of light produced
26
de Broglie relation
Wavelength inversely proportional to momentum (m*v*) λ = h/m*v* (Wavelength = h/mass \* frequency)
27
Complimentary properties
The more you know about one property, the less you know about the other When **wave** **nature** (interference pattern) is observed, **particle** **nature** (position/which slit electron passes through) cannot be, and vice versa
28
Heisenberg uncertainty principle
Product of uncertainties in both position and speed of a particle is inversely proportional to its mass Δx × mΔ*v* ≥ h/4π Δx = position uncertainty Δ*v* = velocity uncertainty m = mass
29
Indeterminacy
Indefinite future = can only predict **probability**
30
Orbital
A probability distribution map of a region where the electron is likely to be found
31
Quantum numbers (4)
1. Principal quantum number, n 2. Angular momentum quantum number, l 3. Magnetic quantum number, ml 4. Spin quantum number, ms
32
Principal quantum number
n Indicates the orbital (Bohr's energy level) \*As n gets larger, amount of energy between orbitals gets smaller
33
Equation for energy of a hydrogen electron
**En = -RH (1/n2)** RH is Rydberg constant for hydrogen RH = 2.18 × 10-18 J
34
Angular momentum quantum number
l Angu**l**ar momentum = what kind of/angle of orbit **l =** 0, 1,... **n-1** ``` l = 0 → s l = 1 → p l = 2 → d l = 3 → f ``` e.g. n = 2 l = [0, 1]
35
Magnetic quantum number
ml **ml = [-l, l]** e.g. n = 2 l = [0, 2] → d orbital ml = [-2, 2] → 5 d orbitals
36
Spin quantum number
**ms** Specifies the orientation of the spin of the electron Value is either: +1/2 (spins up) or -1/2 (spins down)
37
Describing an orbital (3)
1. n, l, ml describes one orbital 2. Orbitals with same **n** value = same **principal energy level** (shell) 3. Orbitals with the same values of **n & l** = same **sublevel** (subshell)
38
Equation for energy transition in hydrogen
ΔE = Efinal - Einitial **ΔEH atom = -2.18 × 10-18 J (1/n2final - 1/n2initial)** Energy emitted by electron is carried away by the releated photon, thus: **Ephoton = -ΔE**
39
Probability density
The probability of finding an electron at a **particular** **point** in space Probability decreases as distance from nucleus increases
40
Radial distribution function
**Total probability** of finding an electron at a **certain** **distance** *r* from the nucleus Volume of shell also increases with distance from nucleus
41
Nodes
Where the probability drops to zero, for both probabilities
42
s orbital
l = 0 spherical shape 1 s orbital
43
p orbital
l = 1 shaped like two balloons -1, 0, 1 3 p orbitals
44
d orbital
l = 2 shaped like four balloons -2, -1, 0, 1, 2 5 d orbitals
45
f orbital
l = 3 shaped like eight balloons -3, -2, -1, 0, 1, 2, 3 7 f orbitals