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30 Cards in this Set
- Front
- Back
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Heisenberg's Uncertainty Principle |
States that it impossible at any one time to measure both the velocity and position of an atom/electron |
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Orbital |
A region of space within which there is a high probability of finding an electron |
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Sublevel |
A subdivision of a main energy level and consists of one or more orbitals of the same energy |
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Element |
A suitable that cannot be split into simpler substances by chemical means |
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Triad |
A group of the elements with similar chemical properties in which the atomic weight of the middle element is approximately equal to the average of the other two |
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Newlands' Octaves |
An arrangement of elements in which the first and the eighth element, counting from a particular element, have similar properties |
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Mendeleev's Periodic Law |
When elements are arranged in order of increasing atomic weight, their properties recur periodically |
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Atomic number |
Of an atom is the number of protons in the nucleus of that atom |
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Modern Periodic Law |
When elements are arranged in order of increasing atomic number, the properties of the elements recur periodically |
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Mass number |
Number of protons and neutrons in the nucleus of an atom of that element |
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Isotopes |
Atoms of the same element (they have the same atomic number) which have different mass numbers due to the different number of neutrons in the nucleus |
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Relative Atomic Mass |
The average of the mass numbers of the isotopes of the element As they occur naturally Taking their abundances into account and Expressed on a scale in which the atoms of the carbon 12 isotope have a mass of exactly 12 units |
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The Principle of Mass Spectrometry |
Charged particles moving in a magnetic field are deflected to different extents according to their masses and are thus separated according to their masses |
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Electron Configuration |
Shows the arrangement of electrons in an atom of an element |
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Aufbau Principle |
When building up the electron configuration of an atom in its ground state, the electrons occupy the lowest available energy levels |
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Hund's Rule of Maximum Multiplicity |
When two or more orbitals of equal energy are available, the electrons occupy then singly before filling them in pairs |
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The Pauli Exclusion Principle |
No more than two electrons may occupy an orbital and they must have opposite spin |
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Compound |
A substance that is made up of two or more different elements combined together chemically |
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Octet Rule |
When bonding occurs, atoms tend to reach an electron configuration with eight electrons in the outermost energy level |
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Ion |
A charged atom or group of atoms |
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Ionic Bond |
The force of attraction between oppositely charged ions in a compound. Ionic bonds are always formed by the complete transfer of electrons from one atom to another |
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Transition metal |
One which forms at least one ion with a partially filled d sublevel |
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Molecule |
A group of atoms joined together. It is the smallest particle of an element or compound that can exist independently |
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Valency |
The number of atoms of hydrogen or any other monovalent element with which each atom of the element combines |
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Sigma bond |
The head - on overlap of two orbitals |
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Pi bond |
Formed by the sideways overlap of p orbitals |
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Electronegativity |
The relative attraction that an atom in a molecule has for a shared pair of electrons in a covalent bond |
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Polar Covalent Bond |
A bond in which there is unequal sharing of the pair (or pairs) of electrons. This causes one end of the bond to be slightly positive and the other end to be slightly negative. |
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Intramolecular bonding |
Bonding that takes place within a molecule e.g. covalent |
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Intermolecular forces |
Forces of attraction that exist between molecules e.g. Van der Waals forces and Hydrogen bonding |
