Chemistry Lecture Final – Flashcards

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how to tell if an element is atomic or molecular
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Atomic = an element that does not exist in nature diatomically
molecular = an element that is diatomic in nature (Br, I, N, Cl, H, O, F)
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how to identify a molecular compound
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has two or more covalently bonded nonmetals
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ACETATE
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C2H302-
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CARBONATE
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CO3 2-
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HYDROGEN CARBONATE (BICARBONATE)
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HCO3 2-
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HYDROXIDE
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OH-
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NITRITE
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NO2 -
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NITRATE
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NO3 -
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CHROMATE
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CRO4 2-
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DICHROMATE
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CR2O7 2-
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PHOSPHATE
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PO4 3-
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HYDROGEN PHOSPHATE
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HPO4 2-
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DIHYDROGEN PHOSPHATE
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H2PO4 -
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AMMONIUM
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NH4 +
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HYPOCHLORITE
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CLO -
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CHLORITE
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CLO2 -
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CHLORATE
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CLO3 -
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PERCHLORATE
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CLO4 -
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PERMANGANATE
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MN04 -
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SULFITE
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SO3 2-
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HYDROGEN SULFITE (BISULFITE)
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HSO3 -
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SULFATE
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SO4 2-
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HYDROGEN SULFATE (BISULFATE)
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HSO4 -
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CYANIDE
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CN -
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PEROXIDE
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O2 2-
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how to identify a OXYACID
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contain hydrogen oxygen and some other nonmetal
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how to identify hydrocarbon
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compound containing only carbon and hydrogen
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how to identify a functionalized hydrocarbon
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contains on OH functional group
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molarity
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mols of substance / liters of soln
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oxidation
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loss of electrons
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reduction
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gain of electrons
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What are the postulates of John Daltons atomic theory of matter
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1) all matter is composed of indivisible and indestructible atoms
2) an element is a type of matter composed of only one type of atom
3) a compound or molecule is a type of matter composed of two or more elements chemically combined in fixed proportions
4) A chemical reaction is where a substance is changed into a new substance
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what are the three temp scales measured relative too
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Fahrenheit - measured relative to salt water
Celsius - measured relative to pure water
Kelvin - absolute, measured relative to motion of atoms
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formula for Celsius to kelvin
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C + 273.15
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how to get to Fahrenheit from celcius
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F-32/1.8
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the law of conservation of matter
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matter is neither created nor destroyed
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the law of multiple proportions
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elements can combine in more than one set of proportions, with each set of proportions corresponding to a diff compound
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the law of definite proportions
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all samples of a given compound have the same proportions of their constituent elements
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what are cathode ray particles and who discovered them
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electron streams, JJ Thompson
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what is the definition of wavelength
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the distance between any adjacent identical points on a wave
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shorter wavelength = ?
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higher energies
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what is heat
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energy in transit
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the first law of thermodynamics
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says that the total energy in the universe is constant
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energy is released in a chemical reaction when
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bonds are formed
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energy is consumed in during a chemical reaction when
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bonds are broken
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fuels always have what type of enthalpy
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a negative enthalpy, ie negative delta H
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fuels are endo or exothermic
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exothermic
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standard state enthalpies are measured at what temp and pressure
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25 C and 1 atm
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amplitude
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vertical height of a wave or depth of a trough
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frequency
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the number of wave crests that pass a through a stationary point in a given period of time
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equation to find frequency (V)
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frequency (v) = speed of light (c)/ wavelength (lambda)
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unit used to define frequency
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hertz (hz)
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what is the photoelectric effect
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the observation that many metals emit electrons when light shines upon them
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how to measure the energy of a photon
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energy (E) = h(plancks constant)*v(frequency)/wavelength (lambda)
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Heisenberg's uncertainty principle
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the more accurately you know the position of an electron the less accurately you know the position and vice versa
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principal quantum number (n) represents what
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size and energy of the orbital (n can be 1-8)
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angualar momentum quantum number (L)represents what
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shape of the orbital (n-1)
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magnetic quantum number (m sub L) represents what
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orientation in space (-L through +L)
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shape of the s orbital
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spherical
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shape of the p orbital
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dumbbell
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shape of the d orbital
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double dumbbell
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first ionization energy
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minimum energy required to completely remove an electron from a ground state atom In the gas phase
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hunds rule
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every orbital in a subshell must be singly occupied before any one orbital is doubly occupied, all singly occupied must have same spin
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pauli exclusion principle
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no two electrons in an atom can have the same four quantum numbers (must have opposite spin)
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how to know if something will interact with magnet
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full subshell = wont interact
not full subshell = will interact
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five basic shapes of VSEPR theory
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linear
bent
trigonal planar
trigonal pyramidal
tetrahedral
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linear bond angle
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180 degrees
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trigonal planar bond angle
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120 degrees
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bent bond angle
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109.5 or 120 degrees
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tetrahedral bond angle
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109.5
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trigonal pyramidal bond angle
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109.5
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how to tell if a molecule is polar by looks
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central atom has one or more lone pairs = polar
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how to tell if a molecule is non polar by looks
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central atom has no lone pairs and all of the outer atoms are identical = non polar
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second way to tell if a molecule is polar by looks
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central atom has no lone pairs and the outer atoms are not identical = polar
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how to tell if something will have a resonance hybrid
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central atom bonded to more than one oxygen with double or triple bonds it is a tipoff
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what are the three postulates of kinetic molecular theory
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1) the size of a particle is negligibly small
2) the avg kinetic energy of a particle is proportional to them temp in K
3) the collisions between particles and their containers are elastic
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three types of intermolecular forces
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dispersion (London forces)
Dipole-Dipole forces
Hydrogen Bonding
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dispersion forces exist where
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in all molecules
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dipole-dipole forces exist where
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in polar molecules
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hydrogen bonding forces exist where
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in polar molecules where H atoms are bonded to FON, super dipole force
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how to change from liquid to gas
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increase heat or reduce pressure
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gasses are least ideal when
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high pressure and low temp
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a molecules weight relates to dispersion forces how
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the heavier the molecule the higher the dispersion forces
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how does boiling point relate to intermolecular forces
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higher boiling point = stronger IMF
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how do IMF relate to viscosity
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high IMF = high viscosity
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boiling occurs when the pressure of the vapor...
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when the pressure of the vapor equals the pressure being exerted from surroundings
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