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91 Cards in this Set
- Front
- Back
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precision
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how close numbers are to each other
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accuracy
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how close numbers are to actual answer
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Mass %
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(mass dissolved / mass solution) x 100
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Law of Conservation of Mass
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mass consumed = mass produced
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Law of Definate Proportions
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mass ratios of elements in a compound are fixed
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Law of Multiple Proportions
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If 2 elements combine to form more than one product, mass of one element will be a fixed mass while the other element differs by an integer ratio
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Summary (3 parts) Dalton's Theory of Atoms
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1) All matter is made up of tiny, invisible, and indivisible particles
2)There are different kinds of atoms that are distinguished by their masses 3)atoms combine in integer ratios to form compounds |
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Evidence in support of Rutherford Model
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Gold-foil experiment--small nucleus
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Isotopes
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elements with the same # of protons, different # electrons
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Metals (characteristics)
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left side, luster, malleable, ductile, good conductors, form cations (atoms with + charge)
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Non-metals (characteristics)
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right side, dull, brittle, bad conductors, form anions (- charged)
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Metalliods (characteristics)
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jagged line, Se,Ge,As etc., intermediate properties
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What makes up a Chemical Formula?
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a)type of atoms present
b)quantaties c)arrangement |
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Emperical Formula
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relative # of atoms formed
(1 C for ever 2 H) |
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Molecular Formula
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actual # atoms in molecule
(2 C and 4 H) |
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Ionic molecules
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contain large networks of cations and anions
ex. NaCl |
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Density
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m (g) / V (L)
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Determine Chemical Formula?
(given molecules/mass) |
1) convert mass to grams
2)divide by lowest choice to get an integer 3)place integer as coefficient |
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Find Molecular Formula?
(given imperical formula) |
1) given mass/mass of compound=integer
2) multiply coefficients by integer |
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Oxidation #'s
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e- gained or lost in rxn
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Naming Ionic Compounds
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1)monatomic=no change in name
2)monatomic + transition metal= transition metal(#) ---ide |
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Naming Binary Compounds
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1)Acics (H + NM)= Hydrogen ---ide
2)NM + NM = use prefix (mono, di, tri, tetra, penta) |
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Limiting Reactants
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1)Given 2 masses
2)Use stoicheometry to find masses of products given by both 3)element that produces the least product is limiting |
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% Yeild
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observed mass/actual mass x 100
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Strong electrolytes
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good conductors of electricity, dissociate into ions
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Weak electrolytes
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moderate conductors b/c they do not compleatly dissociate
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Non-electolytes
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non-conductors, Do not dissociate
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What make up strong electolytes?
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usually ionic compouns (M + NM)
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What makes up weak electolytes?
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usually molecular compounds (NM + NM)
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Precipitation RxN
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forms a solid
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Acid/Base RxN
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substance produce H+ in water, react with bases
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Strong Acid + Srong Base
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H+ + OH- = h2o
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How to balance redox rxn
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a)balance atoms other than water
b)balance o2 with h2o c)balance H with H+ d)balance charge with e- |
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equivalence point
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point in titration where A is completly consumed by B
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As pressure increases--volume?
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decreases
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as T increases, volume
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increases
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as moles increase, volume
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increases
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Ideal Gas Law
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PV=nRT
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Kinetic Theroy of Gases (3 parts)
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1)Gases have kinetic energy-no prefered direction of motion
2)Gases are compressible-distance between particles is large relative to size 3)Gases are weakly attracted to themselves-force between particles is weak |
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Root mean squared
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square root of (3RT/u) u=speed of particles
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2 ways to measure heat
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1)bomb calorimeter
2)coffee cup calorimeter |
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Q=
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mc(change in)T
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Enthalpy
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heat transferred into or out of a system
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Standard Enthalpy of Formation (delta Hf)
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delta H for formation of 1 mol of compound from its elements
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Diffraction
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light composed of waves that interfere with each other
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wavelength
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distance between crests/troughs of waves
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velocity (of wave)
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rate at which crests move
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frequency
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number of crests to pass a point in 1 sec
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velocity=
(for waves) |
wavelenght(frequency)
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Electromagnetic radiation is composed of
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oscillating elecric and magnetic fields
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Elecromagnetic Radiation Spectrum
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x-rays »» visable light »» infared »» microwaves »» radio waves
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Blackbody radiation
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as objects are heated they emit light
E=hv (v=frequency) |
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Photoelectric effect
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if frequency of light is less than the threshold frequency»»e- emitted
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mv²=
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k/r
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n quantum number
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1,2,3. . .
energy level |
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quantum number L
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0, 1, 2. . .n-1
wave shape |
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m quantum number
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-L to +L
wave orientation |
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e- fill orbitals in order
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low E to high E
most -E, most stable E=Energy |
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Pauli exclusion principle
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every e- has a different set of quantum #s
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Hun's Rule
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For orbitals of identical E, the e- fills orbital w/ a single e- first
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paramagnetic
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unpaired e-
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radius of an atom
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distance from outermost e- to nucleus
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As shell # increases, size
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increases
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as charge increases, size
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decreases
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Isoelectronic Ions
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ions with the same # e-
charge increases, size decreases |
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Ionization Energy (definition and trend)
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E need to remove an outher e-
Decreases down a column and across a period |
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Electron Affinity (definition and trend)
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always -
attraction between e- Increases down a column and across (left) a period |
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Properties of Covalent Bonds (2)
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1)fewer bonds»»more reactive
2)more bonds»»shorter distance between atoms |
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Electronegativity (definition and trend)
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tendency to attract e-
decreases down a column and across (left) a period |
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Electronegativy in relation to polarity of a bond
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EN > 1.7 (ionic bond)
EN < 1.7 (polar covalent bond) EN = 0 (covalent bond) |
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multiple bonds occupy (more/less) space than single bonds
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more
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lone pairs occupy (more/less) space then bonding e- pairs
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more
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General conclusion about dipoles in identical atoms
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asymetrical arrangement of identical atoms results in a nonpolar molecule
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Bond dissociation Energy
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E needed to break said bond
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Alkanes
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CnH2n+2
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Alkenes
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CnH2n
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Alkynes
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CnH2n-2
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Alcohols
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-OH
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Carboxylic Acid
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C=O and -OH
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sigma bonds
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e- concentrated between nuclei (single bonds)
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2 properties of pi bonds
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1)weaker than sigma bonds
2)restricted rotation |
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Bond Order
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quantitative strength of bond holding nuclei together
[e- in non bonding MO - e- in antibonding MO]/2 |
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surface tension
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more bonds below the surface, more stable
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Heat of vaporization
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E required to break intermolecular bonds in a liquid--forming a gas
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Vapor Pressure (formula)
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as T decreases, VP decreases
heat vap/R [(1/Ti)-(1/Tf)] |
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Enthalpy of fusion
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E needed to weaked bonds in a solid--forming a liquid
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Enthalpy of Sublimation
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E required to break IM bonds in a solid
Hs= Hv + Hf |
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normal melting point
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temp of phase transition s»»l at 1 atm pressure
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Normal boiling pt
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temp of phase transition from l»»g at 1 atm pressure
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ppb equation
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(mass solute/mass solution)x 10^9
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Henry's Law
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[gas]=k x P
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