Honors Chemistry Midterm Review – Flashcards
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Density |
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Denisty = Mass / Volume |
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Matter |
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Anything that has mass and takes up space |
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Pure Substance |
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Matter with the same fixed composition and properties |
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Element |
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Simplest form of matter, composed of only one type of atom |
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Compound |
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A chemical combination of 2 or more elements in a fixed proportion |
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Organic |
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Carbon-based |
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Mixture |
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A combination of 2 or more substances in which the basic identity of each substance is not charged |
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Heterogenous |
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Not mixed the same throughout |
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Homogenous |
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Mixed the same throughout |
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Solute |
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What is being dissolved Occurs in the lesser extent |
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Solvent |
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What is doing the dissolving Occurs to the greater extent |
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Physical Change |
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A change in which the same substance is present before and after the change |
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Chemical Change |
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A rearrangement of atoms and/or molecules to form one or more new substances with new properties |
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Physical Property |
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A characteristic of matter that is exhibited without a change in identity |
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Chemical Property |
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A property that can only be observed when there is a change in the composition of a substance |
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Extensive Physical Property |
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Does depend on the amount of matter |
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Intensive Physical Property |
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Does not depend on the amount of matter present |
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Distillation |
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A technique used to separate liquids based on their boiling points |
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Fractional Crystallization |
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The separation of substances by their solubility |
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Bond |
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The force holding atoms together in a compound or molecule |
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Molecule |
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Two or more atoms bonded together |
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Compound |
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Two or more different atoms bonded together |
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Diatomic Elements |
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H O N Cl Br I F |
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Covalent Bond |
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Involves the sharing of electrons |
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Linus Pawling |
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Came up with electronegativity |
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Electronegativity |
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Attraction of an atom for a shared pair of electrons |
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Bond Axis |
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Line joining the nuclei of 2 bonded atoms in a molecule |
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Molecular Motion |
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Symmetric, Asymmetric, Bending, Rotating |
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VSEPR Theory |
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Valence Shell Electron Pair Repulsion Predicts the 3D shape of molecules |
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Hybrid Orbitals |
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Equivalent orbitals formed from orbitals of different energies |
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Hybridization |
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The merging of 2 or more unlike orbitals to form an equal number of identical orbitals in an atom |
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Sigma Bonds |
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A bond formed by the direct or end to end overlap of atomic hybrid orbitals |
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Pi Bonds |
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Bond formed by the sideways overlap of P orbitals (Not hybridized) |
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Polyatomic ions |
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Atoms are covalently bonded but the molecule has an overall charge |
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Delocalized Electrons |
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Free to move easily from one atom to the next throughout the metal and don't belong to any particular atom |
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Intermolecular Forces |
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Forces between molecules |
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Intramolecular Forces |
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Forces within a molecules |
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Dipole-Dipole Forces |
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Force of attraction between polar molecules |
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London Forces |
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At any given instant, the distribution of electrons may be unequal and the positive nucleus of 1 atom may be attracted to the electrons of another |
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Momentary Dipole |
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A temporary uneven distribution of electronic charge between an atom at any given instant |
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Vander Waal's Forces |
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Collective name for all intermolecular Forces |
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Avogadro's Number |
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6.02 x 10^23 = 1 mole of something |
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Molecular Formula |
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The actual formula for a compound |
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Empirical Formula |
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The lowest ratio of atoms in a compound |
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Einstein's Theory of Matter and Energy |
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E = mc^2 |
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Planck's Quantum Theory |
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E = h(V shaped frequency thing) |
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Speed of Light |
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c = (Branch thingy for wavelength)(V shaped frequency thing) |
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Newtonian Mechanics |
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Describes the behavior of visible objects at ordinary velocities |
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Quantum Mechanics |
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Describes the behavior of very small objects at speeds near the speed of light |
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Heisenberg Uncertainty Principle |
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It is impossible to know both the exact position and momentum of an electron simultaneously |
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Orbital |
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Where electrons are located (clouds) An orbital can hold 2 electrons |
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Sublevel |
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Contain all the orbitals of a given shape |
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Aufbau Principle |
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An electron occupies the lowest energy orbital that can receive it |
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Hund's Rule |
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Electrons must occupy all of the given orbitals of a sublevel singularly before pairing begins |
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Octet Rule |
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An atom with 8 electrons in its outermost shell is considered stable |
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Doberiener |
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Noticed that Ca, Ba, and Sr all had similar properties and that the mass of Sr was about half-way between Ca and Ba TRIADS |
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John Newlands |
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Law of Octaves Table with 7 rows of 7 |
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Mendeleev |
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Order of increasing mass with 7 in the first two rows and 17 after that |
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Henry Moseley |
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Made table in order of atomic number |