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Chemistry A2 > Electromagnetic Radiation, Quantum Numbers and Arrangement of Electrons > Flashcards

Electromagnetic Radiation, Quantum Numbers and Arrangement of Electrons Flashcards

0
Q

Electromagnetic radiation is ____ and ____; travels in ____

A

Light, energy, waves

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1
Q

–Electromagnetic radiation–

A

–ELECTROMAGNETIC RADIATION–

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2
Q

Left side of the spectrum: ____ wavelengths and ____ frequencies

A

Longer, lower

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3
Q

Right side of the spectrum: ____ wavelengths and ____ frequencies

A

Shorter, higher

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4
Q

Wavelength*

  • symbol:
  • unit:
A

Distance between corresponding points on adjacent waves

  • λ
  • Nanometers (Nm)
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5
Q

Frequency*

  • symbol:
  • unit:
A

The number of waves that pass a given point in a specific time (usually 1 second)

  • ν
  • Hertz (Hz) number of waves/second
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6
Q

Speed*

  • symbol:
  • unit:
A

How fast the light form travels

  • c
  • meters/second (m/s)
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7
Q

The relationship between wavelength (λ) and frequency (ν) is ____ proportional

A

Inversely

  • λ decreases (shorter) then ν increases (more # waves/second)
  • λ increases (longer) then ν decreases (less # waves/second)
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8
Q

Quantum*

A

Minimum quantity of energy that can be gained or lost by an atom

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9
Q

Photon*

A

“Tiny packet” of energy released

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10
Q

____ and ____ both indicate that energy is like matter that they come in little bundles like a particle traveling in waves… but no not have mass or volume

A

Quanta, photons

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11
Q

Dual-wave particle nature

A
  • photons (quanta)–energy traveling in waves, like matter in small packets
  • electron–matter with mass + volume, like energy, movement is as waves
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12
Q

Photoelectric effect*

A

When light is put into atoms there is a change in the electrons
-occurs at specific wavelength and frequency of energy

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13
Q

Energy has a ____ relationship

A

Direct

  • as frequency increases then energy increases
  • as frequency decreases then energy decreases
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14
Q

States of an atom

A

STATES OF AN ATOM

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15
Q

What are the 2 states of an atom?

A
  1. Ground

2. Excited

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16
Q

Ground state

A

Lowest energy state of atom, electrons in normal positive/lowest energy

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17
Q

Excited state

A

High energy state of an atom, photons of energy are added so electrons are at highest energy positions

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18
Q
  • adding ____ to an atom in a set amount causes electrons to move from ____ state to ____ state
  • when electrons return to the ____, atoms release the ____ and part of it is visible as ____ ____
A

Energy, ground, excited

Ground, energy, one color

19
Q

Spectrum*

A

Visible light radiation is divided into bands of color

-produced by a spectroscope~ instrument with a prism or diffraction that can separate electromagnetic radiation by specific wavelengths

20
Q

What are the 3 types of spectrums?

A
  1. Continuos
  2. Emission
  3. Absorption
21
Q
  1. Continuous spectrum
A
  • unbroken bands of color for the wavelengths in visible part of electromagnetic radiation
  • no spaces/division between colors
  • stars+sun/lightbulbs
22
Q
  1. Emission spectrum
A
  • separate bands of color that are separated apart at specific wavelength
  • specific for each element
  • one color spectrum is visible with eyes
23
Q
  1. Absorption spectrum
A
  • bands of color with dark lines where energy (light) is absorbed
  • dark lines determine composition
  • dark lines match up with bright line
24
-Quantum numbers-
--QUANTUM NUMBERS--
25
Bohr
Developed a model of the atom- "planetary model" | -his model only worked for hydrogen
26
De Brogile
Determined electrons have wave-like properties | -found electrons exist at specific frequencies (energy waves)
27
Heisenberg Uncertainty Principle
States it's not possible to determine both the position (location) and the velocity (speed) of the electron at the same time
28
Orbital*
3 dimensional region above and around the nucleus where electrons are located - different types and positions in the electron cloud - they can only hold two electrons
29
2. Angular momentum quantum number
- indicates shape of orbital - symbol: cursive L - range: 0 to 3 - represents sublevels within an energy level - sublevels s,p,d,f
30
3. Magnetic quantum number
- indicates orientation of orbital around nucleus (x-y-z axes) - symbol: m - range: +3 to -3 - represents number of orbitals within each sublevel - orbitals hold up to 2 electrons
31
4. Spin quantum number
- indicates spin direction of electron - symbol: s - range: +1/2 to -1/2 - spin must be in opposite directions like up or down; left or right
32
-arrangement of electrons-
--ARRANGEMENT OF ELECTRONS--
33
Electron arrangement*
- show how electrons occur in orbitals of atom - different for each element --> elements have diff # of electrons - show ground state for electrons
34
Aufbau principle*
- electrons must fill lowest energy orbitals - exceptions-groups with Cr/Cu (lowest energy in 3d not 4s) - also with elements in the same group below them
35
Pauli exclusion principle*
- no two electrons in an element will have the same set of quantum numbers - only 2 electrons per orbital and must have opposite spins
36
Hund's rule*
-electrons are distributed among the orbitals (with the same energy) in order to give a maximum number of unpaired electrons
37
What are the 3 types of electron arrangement
1. Orbital notation 2. Electron configuration notation 3. Noble gas notation
38
1. Orbital notation
- line to represent orbital | - arrows show electrons --> max 2, opposite directions
39
2. Electron configuration notation
- principle quantum number - sublevel letter for angular momentum quantum number - superscript for number of electron
40
3. Noble gas notation
-chemical symbol of noble gas in [ ] for filled energy level * Use noble gas in period before the element - continue with principal quantum number and sublevel letter for angular momentum quantum number - superscript for number of electrons
41
Why use electron dot diagram?
- show number of valence electrons - most atoms can hold and want to hold 8 electrons in their valence shell in order to be chemically stable Chemical stability = full valence shell (octet) Full s and p orbitals
42
Filling electron dot diagram
- determine number of valence electron | - electron dot diagrams are more simplistic than writing out full energy level diagram
43
Quantum numbers*
Specify properties (locations) of orbitals and property (spin) of electron
44
What are the 4 different quantum numbers?
1. Principle (main level) 2. Angular (shape) 3. Magnetic (orientation) 4. Spin (electron spin)
45
1. Principle quantum number
-indicates main level (distance from nucleus) -symbol: n -range: 1 to 7 -corresponds to energy level (period #) n=1: 2e n=2: 8e n=3: 18e n=4: 32e

Chemistry A2 (2 decks)

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