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| Lewis Theory is a simple way to explain _____ |
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Definition
| why atoms combine to form compounds |
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| Lewis developed his theory before ______ |
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Definition
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| noble gas electron configurations may be obtained if electrons are transferred from _____ to _____ |
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Definition
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| electron transfer occurs between metal & nonmetal atoms when their potential energy equals the difference between the _____ respectively |
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Definition
| ionization energy (IE) & EA (electron affinity) |
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| cations have _____ radii than their parent atoms |
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Definition
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| anions have _____ radii than their parent atoms |
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Definition
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| ionic radius _____ with increasing Z for isoelectronic ions |
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Definition
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| electronegativity generally _____ from left to right across a row & _____ from top to bottom in a group |
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Definition
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| electronegativity difference < 0.4 eV |
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Definition
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| electronegativity difference between 0.4 & 2.0 eV |
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Definition
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| electronegativity difference > 2.0 eV |
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Definition
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| 7 steps for drawing Lewis structures for molecules & polyatomic ions |
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Definition
1. count the total number of valence electrons in the molecule
2. count the total number of valence electrons each atom should have when isoelectronic with a noble gas
3. subtract your total in Step 1 from your total in Step 2 to get the number of shared electrons in the molecule
4. divide your number in Step 3 by two to get the total number of bonds in the molecule
5. draw a "skeletal" structure for the molecule
6. draw in the bonds based on the number you got in Step 4
7. add remaining electrons has lone pairs to atoms that do not have an "octet" |
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Term
| 3 cases of octet rule violation |
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Definition
1. odd electron molecules
2. molecules with atoms lacking an octet
3. molecules with atoms that have an "expanded" octet |
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| 3 considerations when drawing Lewis structures |
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Definition
1. minimize the formal charge
2. place any single positive formal charge on less electronegative atoms
3. place any single negative formal charge on more electronegative atoms |
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Definition
| equivalent Lewis structures that differ in the placement of a multiple bond |
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| atoms interact with each other in an effort to become _____ with a noble gas |
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Definition
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| transition metals typically form cations that are _____ with a noble gas |
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Definition
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| covalent bonds form when nonmetal atoms _____ valence electrons |
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Definition
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| molecules with one or more atoms lacking an octet occurs in molecules containing _____ & _____ atoms |
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Definition
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Definition
| a "fictitious" charge assigned to atoms based on "equal" electron sharing |
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| 2 things that Rutherford's nuclear atom is composed of |
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Definition
1. a small, dense, positively charged nucleus composed of protons & neutrons
2. negatively charged electrons whose orbits take up most of the volume of the atom |
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| light is composed of _____ that travel at a constant _____ |
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Definition
| electromagnetic waves; speed (c) |
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Definition
| the distance between two wave crests |
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Definition
| the number of wave crests that pass a given point in an interval of time |
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| Max Planck (1900) proposed that light exists as _____ called photons |
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Definition
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| electrons are only ejected if the photon energy is greater than the _____ of the metal, which depends on a _____ |
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Definition
| "work function" (w); "threshold" frequency (Vo) |
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| wave theory of light has _____ |
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Definition
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Definition
| series of discrete wavelengths that are either absorbed or emitted by a substance |
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Definition
| series of "missing" wavelengths in a continuous light spectrum |
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Definition
| series of wavelengths that are emitted when a substance is heated |
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Definition
| J. J. Balmer showed that the wavelengths of the visible series in the line spectrum of hydrogen can be reproduced by an empirical equation which was later generalized by Rydberg |
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Definition
| Louis de Broglie derives an equation for the wavelength of a "matter wave" |
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Definition
| orbitals (3D shapes of an electron) |
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| principal quantum number (n) |
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Definition
| overall energy & size of an orbital; any positive integer |
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| angular momentum quantum number (l) |
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Definition
| shape of an orbital; any integer up to n-1 |
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| shape when l = 0 (letter s) |
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Definition
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| shape when l = 1 (letter p) |
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Definition
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| shape when l = 2 (letter d) |
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Definition
| donut shape or four leaf clover shape |
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| magnetic quantum number (Ml) |
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Definition
| spatial orientation of the orbital; between -l and +l |
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Term
| Heisenberg "Uncertainty" principle |
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Definition
| there is a limit on the precision of our measurement of the position & momentum of an electron in an atom |
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| we cannot solve the Schrodinger equation "exactly" for atoms with more than one electron due to _____ |
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Definition
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Definition
| keeps electrons from interacting fully with the nucleus; reason why the orbital energies depend on both n & l |
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Term
sub-shell: ns
# of orbitals:
maximum # of electrons: |
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Definition
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sub-shell: np
# of orbitals:
maximum # of electrons: |
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Definition
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sub-shell: nd
# of orbitals:
maximum # of electrons: |
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Definition
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sub-shell: nf
# of orbitals:
maximum # of electrons: |
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Definition
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Definition
| respond strongly to magnetic fields & can be made into permanent magnets |
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Term
| 2 reasons why anomalies to Aufbau principle occur |
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Definition
1. half & completely filled sub-shells are especially stable since they minimize electron repulsion
2. orbitals with high n are very close in energy |
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Definition
| showed that when the elements were arranged by increasing mass, columns of the elements show repeating properties (the periodic law) |
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Definition
| the energy required to remove the most "loosely bound" electron from an atom |
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Definition
| the energy required to remove the most "loosely bound" electron from a singly charged anion |
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Definition
| the radius of the electron cloud of an atom, calculated from bond lengths in molecules (thus no ARs for noble gases!) |
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| AR _____ from left to right across a period & _____ from top to bottom down a group |
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Definition
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Definition
| the study of heat exchange that accompanies a chemical reaction |
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Definition
| associated with the motion of an object |
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Definition
| "stored" energy associated with the position of an object in a "force field" |
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Definition
only concerned with the state of the system at a certain point in time but not how it got there
ex) internal energy |
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Definition
| a force acting over a distance |
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Definition
| energy transfer between two systems at different temperatures |
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| a state function that depends on the internal energy, volume, & pressure |
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Definition
| the measurement of heat exchange during physical or chemical processes |
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Definition
| the amount of heat required to change the temperature of a substance by 1 degree C |
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Definition
| the amount of heat required to change the temperature of 1 mole of a substance by 1 degree C |
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| specific heat capacity (c or s) |
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Definition
| the amount of heat required to change the temperature of 1 gram of a substance by 1 degree C |
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Definition
| specifies deltaHrxn for a stoichiometric amount of reactants & products |
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Definition
| shows the formation of 1 mole of a compound from its constituent elements in their most stable form |
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| standard enthalpy (or "heat) of formation (deltaHf degree) |
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Definition
| the standard enthalpy change associated with a formation reaction |
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Definition
| the energy change associated with breaking a chemical bond |
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Term
| the molecules in gases have the greatest _____ |
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Definition
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Term
| 101,325 Pa = _____ atm = _____ torr |
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Definition
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Definition
| gas pressure is inversely proportional to its volume if its temperature & amount are held constant |
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Definition
| the volume of a gas is directly proportional to its absolute temperature if its pressure & amount are held constant |
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Term
| The Combined Gas Law (Gay-Lussac, 1802) |
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Definition
| a relationship between gas pressure, volume, & absolute temperature for a constant amount of gas |
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Definition
| equal gas volumes contain the same amount of gas molecules at a given pressure & temperature |
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Definition
P = 1 atm
T = O degrees C (273 K) |
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| units for IGL (P, T, V, amount) |
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Definition
P = atm
T = kelvin
V = liters
amount = moles |
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Term
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Definition
1. gas particles (atoms or molecules) may be treated as point masses
2. gas particles are in constant random motion
3. the forces between gas particles are negligible (no interaction b/w each other)
4. the collisions between gas particles are elastic or they do not lose momentum during a collision
5. the avg kinetic energy of gas particles is related to the absolute temp of the gas |
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Definition
| the movement of gas molecules through a small opening |
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Definition
| when a gas mixes with air (or some other gas) & spreads out over time |
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Definition
| uses the root mean square velocity to show that the rate of effusion or diffusion is inversely proportional to the square root of the molar mass |
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