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 |
