Chapter 5
Rutherford's model limitations
-electrons flying around would hit into the nucleus -different # of subatomic particles
Unpaired for Cn
0
Unpaired for Fr
1
Niels Bohr
1913- discovered that electrons move around the nucleus in orbits called orbital clouds (planetary model)
Unpaired for V
3
Unpaired electrons for Hs
4
Unpaired for Eu
7
Electrons are located inside orbitals:
95% of the time
Excited state
A state in which an atom has a higher potential energy than it has in its ground state
How to get from ground state to excited state
Absorb energy
Why do objects release different colors of light?
Because they have different amounts of energy; high amount of energy results in a purple color and a ow amount of energy results in a reddish color
Which atomic model is often called the "planetary" model?
Bohr's model
Types of energy that can be released or absorbed
Electricity, light, and heat
Hund's Rule
Electrons want to be by themselves in an orbital
All orbitals have the same shape
False
An atom's electrons can absorb a photon of any energy.
False
In the Quantum Mechanical model, electron clouds are always shaped like spheres.
False
It's possible to know both the momentum (speed) and the location of an electron
False
Scientists can know exactly where an electron is located.
False
What light has a neutral amount of energy?
Green light
What do we call the energy level in which an electron normally resides?
Ground state
Carbon dioxide and other greenhouse gases absorb which type of light?
Infrared
Limitations of Bohr's model
It only worked good for the hydrogen element because it only had 1 electron
Which color of visible light has the most energy?
Purple
Erwin Schrödinger
Quantum mechanical model of the atom; electrons moves in waves instead of set paths; "clouds of probability" which are called orbitals; cannot know exact location of the electrons
Which form of light is used to study the early universe after the Big Bang?
Radio waves
Which light has little energy that could help do back to ground state?
Red light
How to get from excited state to ground state
Release energy
Ground state
The lowest energy state of an atom
Each element in the sun's atmosphere absorbs different frequencies of light.
True
In Bohr's model, electrons can move between orbits by gaining or losing energy.
True
The Quantum Mechanical model could be modified or replaces by another model in the future.
True
Which form of light is used to study the hot stars that form in the universe?
Ultraviolet
Orbitals
an energy state in the atomic model which describes where an element will likely be
Why are emission spectrums of elements special?
because there are no two elements that have the some spectrum ( like finger prints)
D orbitals
clover shaped; dXY, dXZ, dYZ, dZ², dX² - dY²; can hold 10 electrons
P orbitals
dumbbell shaped; pX, pY, pZ; can hold 6 electrons
Pauli Exclusion Principle
each orbital has at most two electrons
Emission spectra
either continuous or line spectra of radiation emitted by substances
Aufbau Principle
electrons occupy the orbitals of lowest energy first
S orbital
spherical shape; s; can hold 2 electrons
F orbitals
their shapes are even more complex than s, p, or d orbitals; can hold a total of 14 electrons in 7 sub-shells
Spectrum
wavelengths of visible light that are separated when a beam of light passes through a prism; range of wavelengths of electromagnetic radiation
