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Chem 2B > Atomic Theory Chapter 12 > Flashcards

Atomic Theory Chapter 12 Flashcards

1
Q

Wavelength(w)

A

Distance between the adjacent crest of a wave (in m )

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2
Q

Frequency(v)

A

The number of crests passing through a given point per second (in Hz or s^-1)

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3
Q

Speed of light (c)

A

speed of the movement in a given crest
Constant value is: 2.988 x10^8 m/s

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4
Q

Formula for Sped of light

A

c= v(w)

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5
Q

Amplitude

A

Max height of the wave above centerline

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6
Q

Constructive interference

A

When a crest of a wave meets another crest of another wave the amplitude of the waves add together.

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7
Q

Destructive interference

A

a crest of a wave meets a trough of another wave, the two waves cancel each other out

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8
Q

Black body radiation Part 1

A

All non-reflective objects (black-bodies ) emit light (black body radiation).
- Black body room temperature appears black as most of the energy it emits is Infared
- A heated metal emits visible light
- Temp becomes higher, the color of emitted light shifts from red to blue

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9
Q

Photons

A

They are a stream of particles that light is made up of and has energy

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10
Q

Plank’s equation

A

E photon = hv = hc/ w

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11
Q

Plank’s constant

A

h = 6.626 x 10^-34 Js

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12
Q

Law of conservation of Energy

A

Ei + hv = Ef

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13
Q

Electron circular orbits formula

A

En = - Z^2 (RH)/ n^2

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14
Q

Rh constant

A

2.179 x 10^-18

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15
Q

Z

A

atomic number

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16
Q

Law of conservation of energy

A

Eph= hv= Ef-Ei

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17
Q

Black body radiation part 2

A
  • Spectrum of black body radiation is peaked at a characteristic frequency that shifts to shorter wavelength with increasing temperature
    Higher temp = shorter wavelength
  • Classical theory falsely predicts that intensity would increase indefinitely with decreasing wavelength
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18
Q

Energy of light with frequency v

A

Is quantized because energy must be an integer multiple of the photon energy.

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19
Q

Different measurements of wavelength least to greatest

A

pm<nm<mm<m of wavelength

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20
Q

Electromagnetic radiation

A

Eletric and magnetic fields propagate as waves through a vacuum or through a medium.

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21
Q

why is energy of light with frequency(v) is quantized

A

Energy must be the integer multiples of the photon energy.

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22
Q

Emission

A

is the way in which excited atoms emit energy as photons to relax to lower energy levels.

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23
Q

emission spectra of atoms

A

discontinuous

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24
Q

absorption spectra of atoms are

A

discontinuous

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25
Q

Photoelectric effect

A

When more light energy is directed towards a black body object the more electrons are removed to only a certain threshold.

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26
Q

Wave-particle duality Du Brogoli

A

Light (or anything else) can act as both as a wave and as a particle.
Wavelength of the of material particle is inversely proportional to its momentum (and its velocity.
Formula Ξ»= h (Js) /mu (m/s)

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27
Q

Ionization Energy of hydrogen

A

When photon energy is absorbed by a hydrogen atom is just enough to remove an electron from the ground state (n=1), the atom is ionized
H β€”> H^+ (+) e^-

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28
Q

Isolated stationary electron

A

When the final energy state of an electron reaches zero Ef=0

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29
Q

Ionization energy formula

A

Energy of photon being absorbed.
Formula hv= Ef-Ei= 0 - E1 = RH

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30
Q

what is u?

A

the speed of the particle

31
Q

Heisenberg’s uncertainty principle

A

There is a fundamental limit to which with the position of the particle (x) and its momentum (p) can be measured simultaneously.

32
Q

Heisenberg’s uncertainty formula

A

βˆ†π‘₯: uncertainty of measured values of x
βˆ†π‘: uncertainty of measured values of p
βˆ†π‘= m βˆ†u

βˆ†xβˆ†u> h/4(pi)m
βˆ†xβˆ†π‘>h/4(pi)

Product: βˆ†x βˆ†u decreases with increasing mass

33
Q

Heisenberg’s uncertainty principal part 2

A

The more you become more precise in measuring the position (x) more precisely you lose position of the momentum.
βˆ†π‘₯ β€”-> 0
βˆ†π‘ β€”-> inf
inverse happens when you try preciseluy measure the momentum.

34
Q

Wave function πœ“(x)

A

describes a particle exhibiting wavelike properties (quantum particles)

35
Q

Energies (En)

A

n= (1,2,3,… )

36
Q

πœ“n^2 Probability density

A

the probability of finding the particle at a given position (x) and is always positive

37
Q

Quantum mechanics relasonship

A

Quantum # (Energy) (Wave f Prob g/ml
n= 1 E1 πœ“1(x) πœ“1^2(x)
n =2 E2 πœ“2(x) πœ“2^2(x)
n= 3 E3 πœ“3(x) πœ“3^2(x)

38
Q

Wave functions

A

πœ“n (x)= square root(2/L) sin (n(pi)/L x)
En = (n^2h^2/ 8mL^2) where n= 1,2,3….
2
πœ“n is a sine function: Wavelength = 2L/n

39
Q

Particle in a box- Particle densities

A

When solving for wave function = 2L/n
When solving for n value # of nodes = n-1
Probability density becomes zero at nodes of the wave function
# of nodes = n-1

40
Q

r

A

distance from the nuclues

41
Q

πœƒ, πœ™

A

orientation

42
Q

wave function of an electron be factorized into the product of two functions.

A

R(r) is called the radial wave function
Y(πœƒ, πœ‘) called angular wave function

43
Q

Principle Quantum number

A

quantam number represents the overall energy of each orbital. Energy level increases as its distances from the nucleus increases.

44
Q

Angular Momentum quantum number

A

l= 0,1,2,…, (n-1) orbitals with the same l tend to be in the same subshell.
When finding range just remember the n-1 at the end, and there is a given n value.
Finding the total amount of orbitals you need to square amount of n given = n^2

45
Q

Magnetic Quantum numbers

A

m𝑙 = -l, -l+1, …,0,…, l-1, 1 (-3,-2,-1,0,1,2,3)
Determining the range is with given value of l , then simply plug those in -l and +l. Also when finding total number of orbitals = 2l+1

46
Q

Remebers that orbitals in the same shell have…

A

the same energy

47
Q

Subshells

A

a subdivision of electron shells that are separated by electron orbitals. They are s,p,d, and f
s has 2 max electrons
p has 6 max electrons
d has 10 max electrons
f has 14 max electrons
The l value increases by one

48
Q

ml values

A

determined by the value given l value from -l to +l. Ex: 3d has ml = -2, -1, 0, 1, 2 because l value is 2 at d

49
Q

paramagnetic

A

in examining electron configuration there is unpaired electrons they are attracted to magnetic field

50
Q

magnetic properties

A

in electron configuration there is paired electrons and they are slightly repelled in magnetic field

51
Q

s-block

A

1A, 2A, and 8A (holds two electrons)

52
Q

p-block

A

3A-8A (excluding He) (holds 6 electrons

53
Q

d-block

A

3b-8b and 1B-2B (holds 10 electrons)

54
Q

f-block

A

lanthanides and actinides (Bottom 2) (holds 14 electrons)

55
Q

When writing electron configuration

A

the exponents assigned to the s,p,d, and f values coorelate to the position they are in the periodic table from left to right. Ex: H = 1s and He = 1s^2

56
Q

Ionization trend in the periodic table

A

increases the further you move right and up the periodic table

57
Q

Spherical nodes

A

they all start at zero but increase by 1 with every increase in the value of node

58
Q

Angular nodes

A

they are determined by the l formula of a orbital system: s, p, d, and f. Which results in the formula n> or equal to l+1

59
Q

Number of orbitals given within a sign is by n = n^2

A

s = 1
p= 4
d = 9
4 = 16

60
Q

possible values of ms is

A

always 1/2 or -1/2

61
Q

Radius trend in a periodic table

A

from the left and down

62
Q

Trend in atomic radius in the periodic table

A

From left and down

63
Q

conversion of cal to joules

A

1 cal = 4.18 joules

64
Q

zero-point energy

A

vibrational energy of a molecule retain even at the absolute zero of temp. It is a minimal non-zero energy of a quantum mechanical system.

65
Q

An atomic orbital represents.

A

the region of high probability for an electron around the nucleus of an atom

66
Q

Paulie exclusion principle

A

States that two or more identical particles with half-integer spins cannot occupy simultaneously occupy the same quantum space.

67
Q

Rydberg Principle

A

calculates the wavelength of spectral line in many chemical elements. It is a generalization of Balmer series

68
Q

Balmer series

A

1/wavelength = Rh (1/nf^2 -1/ni^2

69
Q

Hund’s rule

A

describes arrangement of electrons in their configurations. Such as in the p block are available, electrons will first occupy separate orbitals with parallel spins.

70
Q

Aufbau principle

A

ground state of an atom or ion, electrons fill subshells of the lowest available energy then they fill subshells to the highest energy. Electrons also attempt to be as far as apart of each other as possible. Chromium and Copper in the 4th row are exceptions to principle.

71
Q

Formula for finding wave length or electron by itself

A

Wave length = h/p = h/mv

72
Q

Mass of electron constant

A

9.109 x 10^-31

73
Q
A

Chem 2B (12 decks)

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