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AP Chemistry > Quantum Theory and the Electronic Structure of Atoms > Flashcards

Quantum Theory and the Electronic Structure of Atoms Flashcards

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1
Q

Electrons

How Light Energy is Determined?

A
  • wavelength
  • frequency
  • energy
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2
Q

Electrons

When are wavelengths seen?

A

When electrons return to ground level

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3
Q

Electrons

Planck’s Constant

A
  • h
  • 6.022E-34 Jᐧs
  • Slope of E∝V
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4
Q

Properties of Light

What is Electromagnetic Radiation

A
  • EMR
  • Properties of Light
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5
Q

Properties of Light

Wavelength

A
  • Length of one wave
  • Meters
  • 𝝀
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6
Q

Properties of Light

Frequency

A
  • Number of wavelengths(or cycles) per sec passing a point
  • 1/s or s^-1 or Hz
  • 𝛎
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7
Q

Properties of Light

Speed of Light

A
  • 2.998E8 m/s
  • c
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8
Q

Properties of light

Amplitude

A
  • Higher is Brighter while Lower is darker
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9
Q

Properties of Light

Equations for Energy, and Light Parts

A
  • c = 𝝀 ᐧ 𝛎
  • E = h𝛎
  • E = hᐧc/𝝀
    * Is the Energy of 1 photon
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10
Q

What are Photons?

A

Particle side of electrons

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11
Q

Planck’s Work

What does delocalized mean?

A

the electron is not with a certain atom or nucleus

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12
Q

Planck’s Work

What is a Quantum

A

A packet of Energy for an electron to jump to the next electron level

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13
Q

Einstein’s work

What is Photon Energy related to?

A
  • Ephoton ∝ 𝛎
  • Ephoton ∝ 1/𝝀
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14
Q

PES equation

A

Ephoton = KEelectron + BEelectron
- BE = binding energy

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15
Q

Bohr’s Work

Energy Equation to move electron in Hydrogen

NOT IMPORTANT FOR TEST

A

ΔE = (-2.178E-18 J )((1/nf^2) - (1/ni^2))

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16
Q

de Broglie’s Work

Mass Equation

A

h/(𝝀v)

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17
Q

Quantum Numbers

Types

A
  • n = Priniciple quantum number
  • l = Angular quantum number
  • m = Magnetic quantum number
  • ms = Magnetic Spin
18
Q

Quantum Numbers

Nodes

A

No possibility for electron(white shell)

19
Q

Quantum Numbers

Principle Quantum Number

A
  • n
  • Integral Number
  • Related to size and energy of orbital
  • Corresponds to Bohr’s energy level
  • More n
    1. Increased Orbital
    2. Increased distance of electron from orbital
    3. Increased Energy
    4. Decreased energy between orbitals
20
Q

Quantum Numbers

Angular Momentum Quantum Number

A
  • Shape
  • l = 0–> (n-1) for each n val
  • if n=3, possible orbitals s(0)–>d(2)
21
Q

Quantum Numbers

Magnetic Quantum Number

A
  • m
  • integers specifying orbital orinetation
  • Values are from -l←→+ l
  • Includes 0
  • Example: l = 2: m=-2,-1,0,1,2 ⇒ 5 orbitals
22
Q

Quantum Numbers

Electron Spin

A
  • Up = + .5 spin
  • Down = - .5 spin
23
Q

Quantum Numbers

Difference between H and Multielectron atoms

A
  • H = subshell E levels that are degenerate(same n-int at same level)
  • Multi = lower orbital energies
    * Subshell of prinicple shell at different energies
24
Q

Quantum Numbers

Rules for Electron Placement

A
  1. Pauli Exclusion Principle
    * No 2 electrons in atom has same 4 quantum numbers
    * electrons in 1/2 filled orbitals have parallel spins
  2. Hund’s Rule
    * One electron for each orbital before doubling up
  3. Aufbau Principle
    * Electron occupy lowest energy level possible
25
Q

Electron Configuration

How do you write Electron Configuration

A
  • Removal Order
  • Ex) Se: [Ar] 3d^10 4s^2 4p^4
26
Q

Electron Configuration

Valence Electrons

A
  • Outermost principle shell
  • Usually S or S and P
27
Q

Electron Configuration

Shortcut using Noble Gases

A
  • Can use closest previous noble gas in brackets then build the rest of the electron config from there
  • Cannot use this for noble gas in ground state
28
Q

Electron Configurations

Electron Configuration Exceptions

A
  • Cr: [Ar] 3d^5 4s^1 (Same with Mo)
  • Cu: [Ar]3d^10 4s^1(Same rule with Au and Ag)
29
Q

Ionization Energy

What is Ionization Energy

A
  • Minimum Energy neede to remove electron from atom or ion
30
Q

Ionization Energy

Ionization Energy Requirements

A
  1. Gas State
  2. Endothermic
  3. Valence electron first
  4. Successive removed for 2nd etc IEs
31
Q

PES

Why are X-rays used?

A
  • Can dislodge electrons
32
Q

PES

Relation between BE and KE

A
  • Inversely Related
33
Q

Magnetic Properties of electrons

Paramagnetic

A
  • one or more unpaired electron
  • attracted by a magnetic field
34
Q

Magnetic Properties of electrons

Diamagnetic

A
  • Paired electrons
  • opposite spins that cancel out their magnetic fields
  • Are not attracted to outside magnetic field
35
Q

Magnetic Properties of electrons

How are they detected

A
  • weighing a substance in the presence of a magnetic field
36
Q

Periodic Trends

Atomic Radius

A
  • Is the distance form the nucleus to the valence electrons
  • Across Period: decreased radius due to higher effective nuclear charge
  • Down Group: Increased radius due to higher n and a greater distance from the nucleus(higher n ==> higher V)
37
Q

Periodic Trends

Cations

A
  • Decreased sized compared to original
  • decreased electrons with same proton number
38
Q

Periodic Trends

Anions

A
  • Increased size
  • Increased electrons with same proton number
  • Electron - Electron Repulsion
39
Q

Ionization Energy

What is the first IE equal to?

A
  • Binding Energy
40
Q

Electron Affinity

Electron Affinity

A
  • Energy released when neutral atoms gain electrons
    1. Needs to be in gas state
    2. M(g) + 1 electron –> M^1-(g) + EA etc(Successive)
  • Exothermic
  • Increased energy leads to Increased negative EA
  • Outer electrons are delocalized: can move around which leads to sea of electrons
41
Q

Periodic Trends

Metallic

A
  • Most = Bottom Left
  • Least = Top Right

AP Chemistry (9 decks)

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