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CHEM 1000 > Quantum: Mechanical Model of the Atom > Flashcards

Quantum: Mechanical Model of the Atom Flashcards

1
Q

What is electromagnetic radiation?

A

type of energy comprised of an electrical and magnetic component which are perpendicular to each other

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2
Q

What does amplitude, wave length, and frequency mean?

A

amplitude is the vertical height of the crests

wave length is distance between two adjacent crests

frequency is the number of cycles that pass through a stationary point at a single time

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3
Q

What is the wave equation?

A

frequency=speed of light/wavelength

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4
Q

What is the speed of light?

A

3.00x10^8 m/s

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5
Q

What is constructive interference?

A

When two waves of equal amplitude that are in phase interact with each other they will produce a wave that is twice the amplitude

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6
Q

What is destructive interference?

A

two waves of equal amplitude that are out of phase interact with each other they will cancel each other out

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7
Q

What is diffraction?

A

when a wave encounters an obstacle or a slit it bends around it and acts like its a new point source

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8
Q

What is the photoelectric effect?

A

can be observed by shining a high frequency, low intensity light on a metal, light acts like a particle, electrons are emitted

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9
Q

What is the formula for the number of photons?

A

Energy of pulse divided by energy of photons

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10
Q

What is the formula to find the energy of photons?

A

energy=(planck constant)(speed of light)/wavelength in m

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11
Q

What is planck’s constant?

A

6.63x10^-34 J s

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12
Q

How can you convert nanometers to meters?

A

divide by 10^9

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13
Q

What is emission spectrum?

A

light emitted by an element can be
separated into its various wavelengths by passing it through a prism yielding a series of bright lines which is the emission spectrum

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14
Q

What is true of the bohr atom?

A
  1. e- move in circular orbits
  2. e- has only a fixed set of allowed orbits, of a certain potential energy
  3. e- can only pass from one allowed orbit to another (absorbing energy)
  4. Passing from a higher to a lower orbit emits light (returning to ground state)
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15
Q

What is the formula for the energy of an electron in a hydrogen atom?

A

E=-2.18x10^-18(1/n^2)

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16
Q

What is the formula for the difference in energy of an electron in a hydrogen or hydrogen like atom? What is z represent?

A

delta E=-2.18x10^-18(z^2/nf^2-z^2/ni^2)

z is atomic number, 1 for hydrogen, 2 for he+, 3 for Li2+….

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17
Q

What are the problems with the Bohr atom?

A

cannot explain emission spectrum for multi-electron atoms and no reasoning for the fixed, quantized orbits

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18
Q

What is the de Broglie wavelength formula?

A

wavelength=plank constant/mass x frequency

19
Q

What is the formula for Heisenberg’s uncertainty principles? What do variables represent?

A

(delta x)(mdeltav)=h/4pi

delta x is uncertainty is electron position (in typical atom this is size of atom)

delta v is uncertainty in electron velocity

m is mass and h is planck constant

20
Q

What is schrodinger equation? What does it allow us to solve for? What do variables represent?

A

(H)(trident)=(E)(trident)

solve for electron position within an atom by giving a wavefunction

trident if wavefunction (orbital)

H represents total KE and PE of electron

E is total energy of electron

21
Q

What is n, l, ml?

A

n is overall size of orbital

l is the shape of orbital

ml is the orientation of orbital

22
Q

If question said light is emitted and you found energy of photon and you need delta e what do you do to E value to make it delta E?

A

Make it negative because atom emitted a photon (light)

23
Q

In n is 3 what is the possible values of l?

A

3-1=2

l=0,1,2

24
Q

What is the orbital for each value of l from 0-3?

A

0 means s orbital
1 means p orbital
2 means d orbital
3 means f orbital

25
Q

If n is 2 what are the values of ml? If n is 4?

A

-1,0,1

-3,-2,-1,0,1,2,3

26
Q

What is the number of sublevels in a level equal to? Example?

A

n

n is 3, s+p+d, 3 sublevels

27
Q

What is the number of orbitals in a sublevel equal to? Example?

A

2(value of l)+1

l=1, 2(1)+1=3, 3 p orbitals

28
Q

What is the number of orbitals in any level equal to? Example?

A

n^2

n=1, 1^2=1, 1 s orbital

29
Q

What is a radial distribution function?

A

Graph that shows the probability of finding an electron at a given position

30
Q

What is a radial node? What is formula to calculate? Example?

A

RN=n-l-1

Probability of finding an electron is 0

2s orbital=2-0-1=1 radial node

31
Q

What is an angular mode? Where can you find one?

A

Plane area around nucleus where probability of finding an electron is zero

On all p orbital, between the two parts

32
Q

Do we see angular nodes on a RDF?

A

No because AN are a plane and don’t exist on a singular radius

33
Q

What is the ground state of an atom?

A

Lowest energy state

34
Q

What is the spin of an electron represented by? What are the values and what do they mean?

A

ms

+1/2 means spin up and -1/2 means spin down

35
Q

Can two electrons in the an atom have the same four quantum numbers?

A

No

36
Q

What is Coulomb’s Law?

A

Electrons repel each other and are attracted to positive charge of nucleus

Therefore the magnitude of the interaction between an electron and nucleus will increase as the number of protons increase

37
Q

What is shielding?

A

Electrons can shied other electrons from the force of nucleus

Electrons in inner orbitals shield more than electrons in the same orbital

38
Q

What is penetration? What is penetrating ability of orbitals in general?

A

Electrons in outer orbitals with rad probabilities that overlap an inner orbitals will experience less shielding

s>p>d

39
Q

How can you tell which electrons are valence electrons when looking at electron configuration or orbital diagram?

A

Highest n value is valence electrons

40
Q

What do we usually fill first 4s or 3d? What are the two exceptions?

A

Usually 4s

Copper and chromium which fill 4s^1 instead of 4s^2

41
Q

How do you find electron configurations for ions?

A

Anions just add the number of electrons indicated by charge

Cations remove electrons from orbitals with highest value of n and then from highest value of l

42
Q

What is paramagnetic vs diamagnetic?

A

Paramagnetic means unpaired electrons and is attracted to external magnetic field

Diamagnetic means all paired electrons and it is not attracted to external magnetic field

43
Q

Formula for frequency?

A

Energy divided by plank constant

CHEM 1000 (8 decks)

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