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35 Cards in this Set
- Front
- Back
- 3rd side (hint)
Z |
Atomic number- # of protons in the nucleus |
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A |
Mass number- total # of protons and neutrons |
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Isotopes |
Atoms of the same atomic number but different mass number |
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Nuclear model- |
An atom of atomic number Z consists of a nucleus of charge +Ze surrounded by electrons each of charge -e |
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e |
Elementary charge = 1.6022 x 10^-19 C |
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c |
Speed of light = 2.998 x 10^8m/s |
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h |
Planck’s constant = 6.626 x 10^-34 Js |
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NA |
Avogadro’s number = 6.022 x 10^23 mol^-1 |
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k |
Bolzmann’s constant = 1.3806 x 10^-23 J/K |
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R=NA k |
Gas constant= 8.3145 J/(mol K) |
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F = NA e |
Faraday’s constant = 9.6485 x 10^4 C/mol |
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Atomic orbitals |
Regions of space where electrons are most likely to be found, with no more than two electrons in any one orbital. atomic orbitals are arranged in shells around the nucleus, each shell is characterized by its principle quantum number, n = 1, 2, ... a shell consists of n^2 individual orbitals, which are grouped together into n subshells; these subshells, and the orbitals they contain, are denoted s, p, d, and f. |
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Periodic table |
The vertical columns of the table are called groups and are numbered from 1-18. Successive rows of the the table are called periods, the number of the period being equal to the principle quantum number of the valence shell, the outermost shell. The periodic table is divided into s, p, d, and f blocks. The d block (groups 3-11) are known as transition metals; the f block (lanthanides period 6 and actinides period 7) are known as inner transition metals; s block are groups 1-2; p block groups 13-18. |
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Common group names |
Group 1 = Alkali metals Group 2 = alkaline earth metals Group 17 = halogens Group 18 = Noble gases Broadly speaking, the elements towards the left of the periodic table are metals and those toward the right are non-metals; the two classes of substances meet at a diagonal line running from boron to polonium, which constitute the metalloids, with properties intermediate between those of metals and non-metals. |
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Anion |
When an atom gains one or more electrons it becomes negatively charged |
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Cation |
When an atom loses one or more electrons it becomes positively charged |
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Oxidation number |
The charge number of an ion. ie. Mg^2+ has two fewer electrons than protons. O^2- has two more electrons than protons. |
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Chemical bond |
Link between atoms |
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Ionic bonds |
Typically, but far from universally, contain a metallic element and consist of cations and anions in a crystalline array. The bond does not just exist between two individual ions. For this reason, the smallest unit of an ionic compound is called a formula unit. NaCl consist of Na^+ and Cl^- the formula unit is sodium chloride because the crystalline structure exist in a one to one ratio |
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Covalent bonds |
Consist of discrete molecules. The bonds between atoms consist of shared electrons |
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Hypervalent |
Atoms of period 3 and later can accommodate more than eight electrons in their valence shell. |
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Resonance VS |
When more than one Lewis structure can be written for a molecule, a blending of the structures may occur and distribute multiple-bond character over the molecule. |
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VSEPR |
Valence-shell electron pair repulsion theory. The regions of high electron density, as represented by bonds- whether single or multiple- and lone pairs, take up orientation around the central atom that maximize their separations. Lone pairs are assumed to repel bonding pairs more strongly than bonding pairs repel each other. |
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Polar bonds |
Unequal sharing of electron pairs in a covalent bond results in one atom having a partial positive charge and the other atom a partial negative charge. The juxtaposition of equal and opposite partial charges constitutes an electric dipole |
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Electronegativity |
The ability of an atom to attract electrons to itself |
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Properties of bulk matter |
Mass: measured in kg; 1kg = 2.205 lbs Volume: 1m^3: 1dm^3 = 1L Amount of substance: mole; 1mole = 6.022 x 10^23 (the number of carbon atoms in exactly 12g of carbon-12) |
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Extensive property |
Property that depends on the amount of substance present in the sample. (Volume, mass) |
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Intensive property |
A property that is independent of the amount of substance. (Color, density, melting point, boiling point, specific heat, etc) |
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Pressure |
Force/Area: 1pascal or 1bar = 10^5 Pa or 1atm = 101325Pa |
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Perfect gas |
Also called ideal gas, pV = nRT R = gas constant 8.3145 J/(mol K) All gases obey the perfect gas equation ever more closely as the pressure is reduced towards zero. |
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Boyle’s law |
Pressure is inversely proportional to the volume p ~ 1/V |
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Charles’s law |
Pressure is proportional to temperature p ~ T |
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Avogadro’s principle |
Volume is proportional to the amount of substance |
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Limiting law |
A law that becomes increasingly valid in a particular limit. Ex: in the ideal gas equation, as the pressure is reduced to zero |
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Dalton’s law |
A mixture of perfect gases behaves like a single perfect gas. The total pressure of such a mixture is the sum of the pressures to which each gas would give rise if it occupied the container alone. p = pA + pB + ... Each pressure can be calculated, individually, by the perfect gas equation |
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