Study Physics 3.11-3.15 Flash Cards

 
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Physics 3.11-3.15

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Specifies the shape, divides the shells into smaller groups of orbital called sub shells
Orbital (angular) Quantum Number

It is impossible to determine the location of atomic particles, and anything that might be used to pinpoint the location would alter its position and change it's future location.
Heisenberg Uncertainty Principle(cont)

Mathmatical system for describing the behavior of such aspects as light molecules atoms and subatomic particles.
Quantum Mechanics

The maximum number of electrons that may occupy a given energy level, the distance represents a specific energy state.
Principle Quantum Number
Non-Metals
Elements that are poor conductors of heat or electricity
The state an electron occupies when it is at its lowest energy level, no energy is emitte dor absorbed in this state
Ground State

When an atom emits or absorbs electromagnetic radiation and an electron moves from one energy level to another and the energy that is emitted or absorbed is equal to the difference between the electron binding energy and values of the initial state and the final state
Bohrs postulate number 2

The exact location of electrons around the nucleus or the location of any subatomic particle must be replaced with the concept of "probable distribution" A given electron or other particle will probably be located in a given region rather than a specific location depending on its energy state.
Heisenberg Uncertainty Principle
Outgrowth of the quantum concept that all forms of energy are released in discrete units or bundles
Qaurta

Electrons are very restricted in their orbits around the nucleus. Their possible location is described by a set of four intergers
Orbital Electrons

Specifies the orientation of the spin axis of an electron
Spin Quantum Number

This number divides the subshell into individual orbitals which hold the electrons
Magnetic Quantum Number

Uniform through out in structure of makeup
Homogeneous Materials

The maximum number of electrons that may occupy the outermost energy level of any atom is eight (8)
Bury-Bohr Principle
(Rule of Octet)
Energy disturbances in space that travel at the speed of light
Photon
X-ray photon that disrupts the electron shell, falling upon, or striking.
Incident

The chemical and physical properties of the elements are periodic functions of their atomic numbers
Periodic Law

The energy required to completely remove an electron from the orbit of an atom
Electron binding energy

Electrons revolve around the nucleus in certain allowed orbits, and no energy is emitted or absorbed by the atom as long as the electrons remain in their original orbits
Bohr's postulate number 1
When an atom absorbes energy, an electron moves to a higher energy level and quickly emits radiation to return to it's lowest possible energy level
Excited State
A chemical compound always contains exactly the same proportion of elements by mass

Law of Definite composition
Negatively charged particles which orbit the nucleus of an atom

Can NEVER under an circumstance exist in the nucleus of an atom


Electrons or orbital electrons
The second stage of the process of pair production
Annihilation Reaction
Energy levels or shells from the nucleus out identified as KLMNOPQ
Orbits
Equal number of protons and electrons.
Electricly Neutral Atom
Principle Qauntum Number Formula
2n(to the second power)

Where N represents the energy level. The maximum electrons per energy level
The interaction between a high energy photon and the nuclear force of an atom
Pair production
In an atom with three or more energy levels when an inner hell electron i ejected and the electrons from higher shells "drop"
Cascade effect
Palladium triad
Heavy Hard dense metals also reffered to as Noble Metals
Platinum Triad
Heave hard dense metals that are nearly inert often called "Noble metal"
The Iron Traid
Heavy hard dense metals are the most magnetic materials known
Periods or series
Each horizontal row that represent an energy level
All of the elements in Group B (all Metals)
Transitional Elements (all metals) which have 1 or 2 valence electrons
Group 8A
Noble Gasses 8 Valence Electrons
Group 7A
Halogens 7 Valence Electrons
Group 2A
Alkali Earth Metals 2 Valence Electron
Group 1A
Alkali Metals 1 Valence Electron
Valence Electrons
The number of each group
Representative Elements
All the elements in "A" group
Families or Groups
Elements with simial chemical and electrical properties from the vertical columns
Mosley
1906 Discovered that the wavelength of X-ray changed in specific amounts as different tagert materials were used
Mendeleyev
Devised the first periodic table fo the elements by arranging elements by their checmial characteristics
Metalloids
Those elements having characteristics of both metals and non-metals
Characterisitics of Non-Metals
When in a solid form are brittle, many exist as gasses in nature
Characteristics of Metals
Luster, Conduct heat, conduct electricity, ductile and malleable
Metals
All but 22 of the known elements classification
Compounds
Substances that may be decomposed into two or more substances by ordinary chemical means
Atom
The smallest fragment of a particular element that is still recognizable as such
Elements
Materials that can not be further decomposed by ordinary chemical means
Heterogeneous Materials
Consisting of or involving dissimilar elements or parts, each keeping their own characteristics
Matter
Anything that occupies space, has a mass, and possesses the property of inertia
Electron energy/Distance from the Nucleus
Farther away=more energy
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