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Chemistry > Unit 6: Electron Structure in Atoms > Flashcards

Unit 6: Electron Structure in Atoms Flashcards

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1
Q

True or false.

light is a wave

A

TRUE

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2
Q

Definition of electromagnetic radiation

A

carries energy through space

  • creates electromagnetic fields
  • creates the electromagnetic spectrum
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3
Q

What is the equation to find either wavelength or frequency?

A

c = λ * V
v=frequency
λ= wavelength
C= speed of light 3.0 x 10^8 m/s

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4
Q

Definition of wavelength

A

The distance between two points (crest or trough) on a wave

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5
Q

Definition of amplitude

A

The distance from a crest or trough to the middle line

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6
Q

Definition of frequency

A

The number of cycles that pass a point per second

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7
Q

How is frequency measure?

A

measured in cycles/second or S-1 or Hertz (Hz)

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8
Q

Horizontal rows on the periodic table are….?

A

periods

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9
Q

What does the periods mean?

A

n= outermost energy level that is occupied with electrons

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10
Q

Definition of black-body radiation

A

The emission of light from hot substances

  • The wavelength of light depends on the temp
  • red hot substances are cooler than white hot substances
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11
Q

Who is Max Planck?

A
  • German physicist
  • assumed that energy can be released by atoms only in discrete “chunks” of some minimum size.
  • atoms cant cont. emit or absorb energy
  • BUNDLES OF ENERGY
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12
Q

Definition of quantum

A

The smallest quantity of energy that can be emitted or absorbed as electromagnetic radiation

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13
Q

What is the equation to find the energy of a single quantum? E=….

A 
E = hv
h= planck's constant 
v= frequency
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14
Q

What is planck’s constant?

A

6.63X10^-34 J*s

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15
Q

What is planck’s quantum theory?

A

energy is always emitted or absorbed in whole number multiples of hv

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16
Q

What is photon emission?

A

This is when light is given off and and electron falls down to a lower energy level

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17
Q

What is photo absorption?

A

This is when light hits an atom and makes an electron jump to a higher energy level

18
Q

What is the photoelectric effect?

A

Light of a certain frequency causes atoms on the surface to emit electrons

19
Q

What did albert einstein come to the conclusion when he put together planck and applied it to the photoelectric effect?

A

Energy hitting the metal is a stream of tiny energy packets

  • energy of photon is proportional to the frequency
  • E (energy of photon) = hv
20
Q

Fill in
____ light frequency= _____ energy photons = ____ to eject electrons

____ light intensity = ____ electrons ejected from atoms

____ light frequency (v) = ____ speed of electrons ejected from atoms

A
  1. Higher, higher, easier
  2. higher, more,
  3. Higher, faster
21
Q

Definition of spectrum?

A

produced when radiation of various wavelengths is separated (light bulbs, stars)

22
Q

Definition of continuous spectrum?

A

contains all wavelengths of light (rainbow)

23
Q

Definition of monochromatic?

A

having only one wavelength of light (laser)

24
Q

Definition of line spectrum?

A

a spectrum containing radiation only of certain wavelengths

25
Q

What are Bohr’s 2 major ideas?

A
  1. electrons exist only in discrete energy levels; quantum numbers
  2. energy is involved in moving an electron from one level to the next
26
Q

What did Louis de Broglie think of?

A

an electron behaves like a wave as it moves around the nucleus and has a specific wavelength - Matter Wave
*the λ of the electron depends on its mass and velocity (called momentum)

27
Q

What is an equation to find λ?

A

λ = h / mv
h=planck’s constant
m=mass
v=velocity

28
Q

What is the Heisenberg uncertainty principle?

A

impossible to know exactly where an electron is around the atom

29
Q

What did Erwin Shrodinger come up with?

A

Developed the wave equation proposal

  • developed wave functions that describe the electrons matter wave
  • the location of electrons is based on these and probability
30
Q

What do orbitals look like and what three ideas go wiith them?

A

look like clouds

  • have diff shapes
  • have diff energies
  • orbitals are diff than orbits (which are simple circles)
31
Q

What are the 3 quantum #’s in the quantum mechanical model?

A
  1. principal quantum number
  2. azimuthal quantum number
  3. magnetic quantum number
32
Q

What is the principal quantum number?

A

n=1, 2, 3, etc

  • gives the level of the orbital
  • as n increases the orbital becomes larger
  • as n increases the electron has more energy and is less tightly bound to the nucleus
  • shell=orbit=energy level
33
Q

What is the azimuthal quantum number?

A

ℓ = 0 to n-1
*defines shape
s, p, d, f
*orbital=subshell
ℓ = 0, orbital letter s, shape= spherical
ℓ = 1, orbital letter p, shape principal (infinity sign)
ℓ = 2, orbital letter d, shape diffuse (four leaf clover)
ℓ = 3, orbital letter f, shape fundamental (crazy shape dont need to know)

34
Q

What is the magnetic quantum number?

A

mℓ = symbol

  • values of ℓ to -ℓ (including 0)
  • defines the orientation in space (x,y,z)
35
Q

What do the 3 numbers for the quantum mechanical model?

A

probable location of an electron

36
Q

What is the 4th quantum number?

A

Ms = the spin magnetic quantum number

  • indicates what direction the electron spins
  • 2 values +1/2 or -1/2
37
Q

Definition of Aufbau principle?

A

electrons enter orbitals with the lowest energy first. this means that electrons must fill the first energy first level before placing any in the second

38
Q

Definition of Pauli exclusion principle?

A

each atomic orbital contains a maximum of two electrons.

39
Q

Definition of Hund’s Rule

A

Electrons enter each orbital of a given type singly and with identical spins before any pairing of electrons of opposite spin occurs within those orbitals
*each orbital of a certain shape receives one electron before you can double them up

40
Q

What is the diff between electron configuration and orbital diagram?

A

the diagram has the arrows and the configuration is just numbers ans letters (ex. 1s^2 2s^2….)

Chemistry (5 decks)

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