- physical model, upgrade from planetary - incorporated new discoveries into Rutherford's nucleic model (like photoelectric effect) - based off of the simplest element, HYDROGEN , didn't explain those with more than one electron theorized that... electron is only found in specific orbits each possible electron is quantized (has specific amount of energy they must give off or gain a quantum in order to change their orbit the electrons CLOSEST TO THE NUCLEUS ARE LOWER ENERGY, THE ELECTRONS FURTHEST ARE HIGH ENERGY

takes Bohr's model from HYDROGEN to everything else - created quantum mechanical model EQUATIONS based off of later inconsistent evidence with Bohr's model - 'quantum mechanical model' derived from equations - mathematical rather than physical - most modern description of atoms and their electrons - if you GRAPH equation, you make orbital shapes like Bohr's, electrons are quantized UNLIKE Bohr's, the path an electron takes around the nucleus is non-exact, and uses PROBABILITY that an electron is in any location (like windmill blades)

represents the locations where an electron is likely to be found in a certain volume of space; it is not possible to know where one is in the cloud at any moment - high density= higher probability, low density= low probability - no boundary, as electron COULD be very far from nucleus, usually limited to location 90% of the time

CH 5 Electrons in Atoms Flashcards by Hannah Siegel

Bohr’s atomic model

physical model, upgrade from planetary
incorporated new discoveries into Rutherford’s nucleic model (like photoelectric effect)
based off of the simplest element, HYDROGEN**, didn’t explain those with more than one electron

theorized that…

electron is only found in specific orbits
each possible electron is quantized (has specific amount of energy
they must give off or gain a quantum in order to change their orbit
the electrons CLOSEST TO THE NUCLEUS ARE LOWER ENERGY, THE ELECTRONS FURTHEST ARE HIGH ENERGY

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Schrödinger

*takes Bohr’s model from HYDROGEN to everything else

created quantum mechanical model EQUATIONS based off of later inconsistent evidence with Bohr’s model
‘quantum mechanical model’ derived from equations
mathematical rather than physical
most modern description of atoms and their electrons
if you GRAPH equation, you make orbital shapes
like Bohr’s, electrons are quantized
UNLIKE Bohr’s, the path an electron takes around the nucleus is non-exact, and uses PROBABILITY that an electron is in any location (like windmill blades)

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what are Bohr’s quantized orbits similar to?

PRIMARY ENERGY LEVELS, rungs on a ladder, unevenly spaced at times (need different quantums)

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what couldn’t Rutherfords’ model explain?

the changing of physical properties elements underwent in fire, etc. (what we now know as chemical reactions, interaction of electrons)

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electron cloud

represents the locations where an electron is likely to be found in a certain volume of space; it is not possible to know where one is in the cloud at any moment

high density= higher probability, low density= low probability
no boundary, as electron COULD be very far from nucleus, usually limited to location 90% of the time

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solutions to schrödinger’s equation give…

the energy level an electron can have

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Light calcs

E=hv

C=lambda v

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Aufbau principle

electrons fill from lowest to highest energy level
(lowest energy first)
sublevel orbitals always equal (4s #1 = 4s #2)

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Pauli Exclusion Principle

each orbital describes 2 electrons

must have opposite spins

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Hund’s Rule

everyone gets one electron before anybody at the same energy level gets 2

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issues w/ Rutherford’s model

doesn’t account for:

proton/e- attractions
metals changing color when heated (iron which is brown going from red to white)
solutions showing bright line spectrums when heated

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define energy level

an area around the nucleus where orbitals exist

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define orbitals

a place in an energy level where there is a chance of locating two electrons (technically electron cloud OF the nrg level)

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define orientation

a different location of the orbital and their electrons

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what is the difference between 1s v. 2s

2s occupies more volume, but can hold same number of electrons

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what is the purpose of electron configuration exceptions?

to create a more stable atom

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number of orbitals formula

n^2

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number of electrons formula

2n^2

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Hantaro Nagaoka

suggests that an atom has a central nucleus and that electrons move in rings like those of Saturn

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Louis de Broglie

proposes that moving particles like electrons have some properties of waves

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In a atom, electrons and the nucleus interact to…

make the most stable arrangement possible

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the y axis of an aufbau diagram is

increasing energy

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exceptions

column 6, 11

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Isaac Newton

tried to explain behavior of light by assuming it consists of particles

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by 1900, scientists had evidence that light was made of

WAVES

waves of light have certain properties

amplitude, wavelength, frequency

amplitude

height from zero to crest

frequency

m/s also Hz or s-1

wavelength

electromagnetic radiation

includes visible light, UV, X-rays, gamma

3.00 x 10^8 m/s (C)

speed of light

when sunlight (white) passes through a prism...

it separates into a spectrum of colors

violet light

400 nm -470 nm

blue light

470 nm - 530 nm

green light

530 nm - 580 nm

yellow light

580 nm - 620 nm

orange light

620 nm - 700 nm

red light

700 nm

radio

100-1 m

micro

1^-1 to 1^-3

infared

10^-4 to 10^-6

10^-7 to 10^-10

x-rays

10^-11 to 10^-12

gamma

10^-13

atomic emission spectra

``` BRIGHT LINE (when an electric current is passed through an element, the electrons are energized, then emit light) ```

when electrons gain energy

they move up to higher energy levels

when electrons lose energy by emitting light

they return to lower energy levels

regular light put through a prism creates a...

rainbow

energized light (helium lamp) put through a prism creates an...

atomic emission spectrum made up by several specific lines of color

no two element's atomic emission spectra are

the same; therefore they can be used to identify elements (often used to analyze stars/astronomical bodies)

scientists who discovered E=hv

Max Planck; trying to understand color changes while heated, could explain if he assumed energy of a body changes in small discrete units (quanta) *quantization of energy

h, or 6.626 x 10-34 JxS is called

Planck's constant

the energy of a quantum equals

a small energy charge discharges or absorbs

low-frequency radiation

a large energy change discharges or absorbs

high-frequency radiation

_______ used Planck's quantum theory to explain ____

Albert Einstein; the photoelectric effect

the photoelectric effect

electrons are emitted when a specific light, at or above the threshold frequency, shines on a metal; classical physics (light=energy in waves) could not explain

threshold frequency

the frequency a light must reach to emit electrons from a metal (photoelectric effect); above it, the electrons travel faster

Albert Einstein's explanation of the photoelectric effect

he proposed that light could be described as quanta of energy that behave like particles, or PHOTONS quantized according to Planck's forumla

photons in a monochromatic (same frequency) beam have

the same energy

electrons are ejected when

freuquency/energy are too low

light behaves as

waves and particles

when an electron has its lowest possible energy it is in its

ground state

the step of an emission of an electron is also known as

electronic transition

the light emitted by an electron moving from a HIGHER to a LOWER energy level has frequency ______ to the energy change of an electron.

DIRECTLY PROPORTIONAL

this causes

the lines of specific frequency in an atomic emission spectrum

Warner Heisenberg

``` uncertainty principle (we can know either velocity or location of electron, not either, since we must trap it an a magnetic field to find location) ```

Bohr's model explains the _______ of all atoms because______

atomic emission spectra; it predicts the quanta of energy (light) atoms give off as they jump between energy levels (energized)

more closely spaced spectral lines mean

energy levels are closer together, occurs at increased values of n

there is a limit to the frequency of emitted light because

with a high enough energy, the e- completely escapes atom

Clinton Davisson and Lester Germer

confirmed de Broglie's theory of matter waves by showing the reflections of electrons off of metals that acted like waves (caused by X-rays)

wavelike properties of electrons are useful because_____

they are used in electron microscopes to show very small objects

de Broglie's equation

predicts that all moving objects have wavelike behavior, but mass must be very small for the wavelength to be large enough to observe (must travel at much higher velocity) -set stage for new way to describe motion of subatomic particles...QUANTUM MECHANICS versus classical mechanics for big things, quantum is used on small things which act like waves and particles)

atomic spectra are produced as

atoms emit light as excited electrons DROP DOWN in energy levels

the leftmost atomic emission band show the

GREATEST energy change

electromagnetic light in order of biggest to smallest wavelength

radio, micro, infared, UV, X-rays, gamma