__ proposed a model where most of an atoms mass and all the positive charge was in the nucleus.
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arranged
Rutherford's model did not explain how electrons __ around the nucleus.
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emission of light
They discovered that an element's chemical behavior is related to the arrangement of the electrons in its atoms through the __.
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electromagnetic radiation
a form of energy that exhibits wavelike behavior as it travels through space
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light
\___ is part of the electromagnetic spectrum
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wavelength
is the distance between identical points on successive waves
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amplitude
is the vertical distance from the midline of a wave to the peak or through
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frequency
the number of waves that pass though a particular point in 1 second (Hz= 1cycle/s)
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3.00 x 10 (8)
speed of light in a vacuum
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colors; frequencies
different __ mean different __ and wavelengths being emitted.
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Maxwell
__ proposed that visible light consists of electromagnetic waves. (1873)
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different wavelengths
This wave model could not explain the emissions of __.
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Max Planck (1858-1947)
__ researched this and concluded that matter can gain or lose energy only in small, specific amounts called quanta.
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quantum
the minimum amount of energy that can be gained or lost by an atom
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Planck's constant is h
h= 6.63 x 10 (-34) J.s
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photoelectric effect
electrons are emitted from a metal's surface when light of a certain frequency or higher than a certain frequency, shines on the surface.
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Einstein
"Photoelectric Effect" was solved by __ in 1905
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1. wave nature 2. particle nature
Light has both : 1.___ and 2.___
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photons
a massless particle that carries a quantum of energy
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atomic spectrum
of an element is the set of frequencies of the electromagnetic waves emitted by atoms of the element
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intense flame or electricity
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electrons
Parts of the atomic spectrum:
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All elements emit light when vaporized in an __ or when __ is passed through their gaseous state.
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When in a flame or electricity is passed,, __ absorb energy and then give off energy in the form of light.
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Niels Bohr (1885-1962)
__ was the first who saw the connection between the wavelengths an element emits and its atomic structure.
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quantized
Bohr postulated that to get spectral lines, the energy of the electron in the atom must be __ (specific amount of energy)
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hydrogen atom
Bohr used Rutherford's planetary model to develop a model of the __.
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orbits; energy
In Bohr's atom, electrons move around the nucleus in __ that possessed different amounts of __.
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quantum number (n)
each orbit was identified by a __.
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ground state
lowest energy level, n=1, closest to the nucleus
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excited state
a level of higher energy, n=2 or greater
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absorb
electron could __ energy and jump to a higher energy level
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1. e can only have specific (quantized) energy values
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2. light is emitted as e moves from one energy level to a lower energy level
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3. From ground state (lowest energy) to the excited state (higher energy)
Bohr's model of the atom (1913) in which three rules.
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failed to explain the spectrum of any other element
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not explain the chemical behavior of atoms
Bohr's model explained the hydrogen atom, but it__.
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It also failed in __.
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developed the idea of quantized energy levels and laid the groundwork for atomic models.
Bohr's model was incorrect but it__.
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He answered the question of why electrons must be restricted to specific distances from the nucleus.
What did Louis de Broglie contribute? (he was french)
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particle and a wave
In 1924, De Broglie reasoned that e is both a __ and __.
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mass and velocity
He derived a mathematical relationship between the __ and __ of a moving particle and the wavelength that it would exhibit.
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wavelength symbol=h/mv
De Broglie formula
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wavelengths, frequencies, and energies
De Broglie's conclusion was that electrons and other moving particles do have wavelength characteristics. If an electrons has a wavelike motion and is restricted, only certain ___ are possible.
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Heisenberg Uncertainty Principle
states that it is impossible to know precisely both the velocity and position of a particle at the same time
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probability; region
The only quantity that can be known is the __ for an electron to occupy a certain __ around the nucleus.
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Schrodinger
In 1926, __ derived an equation that described both the particle and wave nature of the electron of a hydrogen atom.
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of other elements
Schrodinger's new atomic model applies equally well to atoms __.
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quantum mechanical model
Electrons have no precise orbits
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Electrons exist in certain region surrounding the nucleus.
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The region around the nucleus can be described as a blurry cloud of negative change
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electron density
the density of an electron cloud
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atomic orbital
a region around the nucleus of an atom where an electron with a given energy is likely to be found
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principle quantum number (n)
indicates the main energy levels surrounding the nucleus. It symbolized by n, and is a whole number 1-7.
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The Angular Momentum Quantum Number (l)
indicates the shape of an orbital. These are represented by s, p, d, f
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the magnetic quantum number (ml)
this is the orientation of the orbital in three-dimensional space
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electron spin
electrons have a spin of clockwise or counter clockwise.
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electron configuration
it is the distribution of electrons among the orbitals of an atom
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It describes where the electrons are found and what energy they posses.
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It is an address for electrons
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electron address
An __ consist of principle quantum number and it's orbital quantum number.
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Aufbau principle
electrons are added one at a time to the lowest energy orbitals available until all the electrons of the atom have been accounted for.
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Pauli Exclusion principle
an orbital can hold a maximum of 2 electrons and they must spin in opposite direction.
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Hund's rule
the electrons occupy energy orbitals so that a maximum number of unpaired electrons results.
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orbital diagram
is a visual representation of electron configuration
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uses lines or boxes to represent the orbital
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uses arrows to represent electrons
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electrons configuration- uses numbers, letters, and superscripts (electrons)
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valence electrons
the electrons the outermost shell that are responsible for an atom's chemical behavior
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short-hand electron configuration
focuses on valence electrons (configuration)
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uses noble gases in brackets and then the valence electron configuration ex. Li= [He]2s(1)
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s-block
group 1a and 2a
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p-block
group 3a to group 8a
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d- block
transition metals, the middle of the periodic table
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f- block
innertransition metals, the two rows under the table
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electron dot structure
consists of the element's symbol surrounded by dots
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The element's symbol represents the atomic nucleus and inner-level electrons
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The dots represents the atom's valence electrons
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In writing an atom's electron dot structure, dots are placed one at a time on the four sides of the symbol and then paired up until all are used.
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okay
Do not forget to study the math proportion of the test. IMPORTANT TO KNOW!!! Type in "okay" to get the answer correct
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Frequencies
Bohr's model of the atom predicted the __ of the lines in hydrogen's atomic emission spectrum.
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Lower
According to Bohr's atomic model, the smaller an electron's orbit, the __ the atom's energy level
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Higher
According to Bohr's atomic model, the larger an electron's orbit, the __ the atom's energy level.
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Electron
Bohr proposed that when energy is added to a hydrogen atom, it's __ moves to a higher-energy orbit
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Energy levels
According to Bohr's atomic model, the hydrogen atom emits a photon corresponding to the difference between the __ associated with the two orbits it transitions between.
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Atomic emission spectrum
Bohr's atomic model failed to explain the __ of elements other than hydrogen c
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Quantum mechanical model of the atom
The modern model of the atom that treats electrons as waves
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Atomic orbital
A three-dimensional region around the nucleus representing the probability of finding an electron
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Schrödinger wave equation
Originally applied to the hydrogen atom, it led to the quantum mechanical model of the atom
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Do not
Atomic orbitals __ have an exactly defined size
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Two
Each orbital may contain at most __ electrons
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Spherically shaped
All s orbitals are __
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Ground state
The lowest allowable energy state of an atom is called its __
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n
A principal energy has __ energy sub levels
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Orbitals
The maximum number of __ related to each principal energy level equals 2n*2
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Three
There are __ equal energy p orbitals.
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2s and 2p
Hydrogen's principal energy level 2 consists of __ orbitals.
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Three?
Hydrogen's principal energy level 3 consists of __ orbitals.
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