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46 Cards in this Set
- Front
- Back
How is error calculated?
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Error = experimental value - accepted value
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How is percent error calculated?
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Percent error = |error|/accepted value x100%
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How is degrees Kelvin taken from degrees Celsius?
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K = C + 273
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First to suggest that atoms existed. Believed that they were both invisible and indestructible.
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Democritus
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Modernized information about atoms, and created a set of theories to help explain them.
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Dalton
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First to discover the existence of a negatively charged atomic particle, today known as an electron.
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Thomson
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Discovered the charge of an electron, as well as its mass relative to that of a hydrogen atom.
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Millikan
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Mass of an electron relative to that of a hydrogen atom.
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1/1840
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First to discover the existence of a positively charged atomic particle, today known as an proton.
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Goldstein
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First to discover the existence of a neutral particle, today known as an neutron.
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Chadwick
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Proposed that an atom is mostly empty space, and then each has a nucleus.
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Rutherford
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What could Rutherford's atomic model not explain?
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The chemical properties of elements.
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How is the number of neutrons in an element calculated?
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Neutrons = mass number - atomic number
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Proposed that electrons move in fixed paths about the nucleus of an atom.
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Bohr
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Principle that states that electrons occupy the orbitals of lowest energy first.
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Aufbau Principle
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According to this, an atomic orbital may, at most, have two electrons spinning in opposite directions.
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Pauli Exclusion Principle
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Idea that electrons occupy energy levels in such a way that an energy level is filled entirely by electrons of the same direction of spin.
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Hund's Rule
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How is wavelength and frequency calculated?
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The speed of light = wavelength x frequency
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What is the speed of light?
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2.998 x 10 to the 8 meters per second
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What is Avogadro's constant?
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6.02 x 10 to the -23
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Arranged the elements in a new periodic table in order of mass.
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Mendeleev
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Grouped elements into triads in order to sort them by their chemical properties.
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Dobereiner
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What is the periodic trend for atomic mass?
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Increases down, decreases across.
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What is the periodic trend for ionization energy?
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Increases down, increases across.
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What is the periodic trend for electronegativity?
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Decreases down, increases across.
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What is the periodic trend for nuclear charge?
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Increases down, increases across.
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What is the periodic trend for shielding?
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Increases down, remains constant across.
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What is the periodic trend for ionic size?
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Increases down, decreases across.
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What is electronegativity?
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The ability of an atom to attract electrons when the atom is in a compound.
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What is first ionization energy?
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The energy required to remove an electron from an atom.
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Atoms tend to gain or lose electrons in order to achieve a noble gas structure by the _______.
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Octet rule
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If the components of an alloy are relatively the same size, what kind of alloy is formed?
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Substitutional alloy
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What are the three metallic crystallization patterns?
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Body-centered cubic, face-centered cubic, and hexagonal close-packed.
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If the components of an alloy are relatively different in size, what kind of alloy is formed?
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Interstitial alloy
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Theory that states the the repulsion between electrons causes molecular shapes to change in a way that leaves the electrons as far apart as possible.
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VSEPR (Valence-Shell Electron-Pair Repulsion) Theory
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Bond angle of linear triatomic.
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180 degrees.
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Bond angle of trigonal planar.
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120 degrees.
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Bond angle of bent triatomic.
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105 degrees.
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Bond angle of pyramidal.
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107 degrees.
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Bond angle of tetrahedral.
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109.5 degrees.
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The two weakest attractions between molecules belong in this collective category.
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Van der Waals forces
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Weakest of all molecular attractions. Caused by the motion of electrons.
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Dispersion forced
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Molecular attractions caused by the attraction between polar molecules.
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Dipole-dipole interactions
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Attractive forces in which hydrogen bonds to an electronegative atom and an unshared electron pair of electrons from another electronegative atom.
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Hydrogen bonds
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If hydrogen bonds with any of these elements, then a hydrogen bond is present.
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Nitrogen, oxygen, and fluorine.
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Why are the properties of network solids superior to those of typical solids?
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Melting or breaking down a network solid would requite breaking down the covalent bonds throughout it.
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