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58 Cards in this Set
- Front
- Back
Celsius to Farenheit
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9/5(C) + 32
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Farenheit to Celsius
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5/9(F − 32)
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Density equals
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mass/volume
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Rules for Significant Figures
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All nonzero digits are significant.
Zeroes between two significant figures are themselves significant. Zeroes at the beginning of a number are never significant. Zeroes at the end of a number are significant if a decimal point is written in the number. |
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Accuracy
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the proximity of a measurement to the true value of a quantity
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Precision
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refers to the proximity of several measurements to each other
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One inch to cm
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1 inch = 2.54cm
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AMU = __ grams
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1 amu =1.66054 × 10-24 g
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Scientist and tool credited with discovery of electrons
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J. J. Thompson
cathode tubes |
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Charge/Mass ratio of electron
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1.76 108 coulombs/g
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Discovered the charge of electron in 1906 at UChicago
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Robert Millikan (University of Chicago) determined the charge on the electron in 1909
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First observed radiation
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Henri Becquerel
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alpha particles
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two protons
two neutrons discovered by Ernest Rutherford |
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Beta- Particle
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An emitted electron
Discovered by Ernest Rutherford |
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Beta+ particle
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Positron
Discovered by Ernest Rutherford |
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Gamma radiation/particles
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very fast electromagnetic radiation of subatomic particles
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Dimensions of atoms measured by
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1 Å =10-10 m
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mass spectrometer
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measures atomic weights
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Name of group 6A
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Chalcogens
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Metalloids
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B
Si Ge As Sb Te |
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The Diatomic Molecules
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H ave
N o F ear O f I ce Cl cool B eer |
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Aluminum takes a ___ charge
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Al 3+
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Nitrogen takes a ___ charge
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N 3-
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Chalcogens takes a ___ charge
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Chalcogens: 2-
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Zinc takes on a ___ ion
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Zn 2+
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Calcium takes on a __ charge
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Calcium: 2--
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% element
or % composition |
(#atoms)(#atomic weight)
_____________________ (Formula Weight of compound) all times 100 |
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Avogadro's Number
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6.02*10^23
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An 18g laboratory-sized sample of water contains ____
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18g = 1 mole of H2O
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% Yield
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(Actual/Theoretical) *100
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solutions
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homogeneous mixtures of two or more pure substances
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solvent
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greatest abundance
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Solutes
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smaller
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dissociation
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When an ionic substance dissolves in water, the solvent pulls the individual ions from the crystal and solvates them.
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electrolyte
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An electrolyte is a substances that dissociates into ions when dissolved in water.
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Strong Acids
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HCl, HBr, HI, HClO3, HClO4, HNO3, H2SO4
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Strong bases
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Alkali-OH, Ca, Sr, Ba-OH
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Steps to writing net ionic equations
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Write a balanced molecular equation.
Dissociate all strong electrolytes. Cross out anything that remains unchanged from the left side to the right side of the equation. Write the net ionic equation with the species that remain. |
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Net ionic equation of strong neutralization reactions
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H+ + OH- ==> H2O
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Oxidation Rules
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Oxygen has an oxidation number of −2, except in the peroxide ion in which it has an oxidation number of −1.
Hydrogen is −1 when bonded to a metal, +1 when bonded to a nonmetal. Fluorine always has an oxidation number of −1. The other halogens have an oxidation number of −1 when they are negative; they can have positive oxidation numbers, however, most notably in oxyanions. |
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displacement reactions
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ions oxidize an element.
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Kinetic Energy equation
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KE = 1/2 mv^2
(one-half mass velocity squared) |
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1 cal = ____ J
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1 cal = 4.184 J
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work = ___ x ___
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Work = force x distance
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First Law of Thermodynamics
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Energy is neither created nor destroyed
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Internal Energy
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Potential and kinetic energies all summed up
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Heat equation
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Final temp - Initial temperature
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Endergonic
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Absorbs energy from surroundings
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Exergonic
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Releases energy into surroundings
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Internal Energy:
State function or not? |
Initial Energy IS a state function
q and w are NOT |
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work done by gas = __ ___
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work = -P /\ V
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Enthalpy (Heat) =
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H = E +PV
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If /\H is positive
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Endothermic
/\H=+ |
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If a process has a negative /\H
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It's exothermic
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Enthalpy /\H
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total /\H = /\H products - /\H reactants
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Enthalpy is an ____ property
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extensive
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Hess' Law
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If a reaction is carried out in a series of steps, /\H for the overall reaction will be equal to the sum of enthalpy changes for the individual steps
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/\ H = (Hess' Law)
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/\H = total products - total reactants
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