Chem 115 Exam 2
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
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| frequency | cycles/sec
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| wavelength | length
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| amplitude | height
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| higher amplitude | brighter
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| lower amplitude | dimmer
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| high energy | high frequency
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| low energy | low frequency
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| values of n>(equal to) 1; spherical | s orbitals
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| n>(equal to) 2 | p orbitals
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| any orbital can hold a max of how many e-? | two
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| lowest energy state | ground state
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| n goes up | absorption
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| n goes down | emission
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| energy difference for electronic transition | (h/2pi)(1/n(f)^2-1/n(1)^2)
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| c(speed of light)= | wavelength(frequency)
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| atomic radii trend | increase down; decrease right
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| energy required to remove and electron | ionization energy
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| ionization energy trend | down column decrease; across row increase
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| change in energy accompanying the addition of an electron to an atom or ion | electron affinity
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| electron affinity trend | down column decrease; across row increase
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| low IE forms | cations
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| high IE forms | anions
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| core takes how much energy to remove | a whole lot, especially compared to the outer levels
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| metallic trends | increase down; decrease right
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| transferring electrons form one element to another | ionic compounds
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| sharing electrons between atoms of different elements | covalent compounds
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| loses one electron; positive ion | cation
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| gains one electron; negative ion | anion
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| cation usually | metal
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| anion usually | nonmetal
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| covalent bonding is between | nonmetals
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| electrons shared among all the atoms in a solid | metallic bonding (NOT COVALENT -- that's just between two atoms)
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| metal plus metal | metallic bond
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| metal plus non metal | ionic bond
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| non metal plus non metal | covalent bond
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| the enthalpy change that accompanies the revers of one mol of ionic solid separating into gaseous ions | lattive energy
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| do ionic or covalent compounds conduct electricity | ionic
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| electron transfer is a _________ process | endothermic
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| requires energy | exothermic
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| lattice energy trend | decrease down; increase right
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| distance between nuclei at which potential energy is the lowest | bond length
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| requires energy | bond breaking
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| KJ to break bond and bond length | equilibrium
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| electronegativity trend | increase right; decrease down
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| have the same relative placement of atoms bt different locations of bonding and lone electron pairs | resonance structures
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| formal charge | # valence electrons - (unshared valence +1/2 shared electrons)
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| in resonance structures does the bond move or the atom | bond
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| if you can write two or more valid lewis structures, the actual electron distribution is... | an average of the distributions shown
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| VSEPR | Valence shell electron pair repulsion
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| Principle of VSEPR | Valence shell elctron unis around a central atom will arrange themselves so that they are as far from each other as possible
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| two electron units (shape and degree) | linear 180
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| three electron units no lone pairs | trigonal planar 120
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| three electron units one lone pair | bent <120
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| four electron units no lone pairs | tetrahedral 109.5
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| four electron units one lone pair | trigonal pyramidal <109.5
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| four electron units two lone pairs | bent <109.5
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| central atom and five bonding groups | trigonal bipyramidal
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| central atom and six bonding groups | octahedral
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| double bonds effect bond angles similar to | lone pairs
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| an inbalance of charges over the whole molecule | molecular polarity
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| same molecular formula and different physical/chemical properties | constitutional isomer
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| polarity: trans vs cis | trans=non; cis=polar
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| dipole moment | measure of molecular polarity
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| when are covalent bonds polar | when atoms have different electronegativities and share electrons equally
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| titration | slowly adding an acid to a base until the reaction has reached the equivalence point
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| using a known amount of one reagent to determine the amount or concentration of another substance is | standardization
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| Molarity | moles/liters
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| q (enthalpy) | cm(DeltaT) or specific heat X mass X temp change
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| q (reaction) - q (solution)= | 0
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| Which will have a higher lattice energy? A smaller compound or larger | Smaller - tighter bond
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| Which will have a higher lattice energy? An ionic compound with more or less ions? | More - hold tighter bond
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| Is combustion endothermic or exothermic? What about formation | Combustion: exothermic
Formation: endothermic
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| Are stronger bonds short or long? | Short (ex. triple shorter and stronger than double)
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| What is the purpose of standardizing a solution | Determine concentration
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| Of the following, what radiation has the longest wavelength and what has the greatest energy? gamma; ultraviolet; visible | visible: longest wavelength
gamma: greatest energy
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| Why does the atomic radius of main-group elements generally increase down a group? | The principle quantum number (n) of the valence orbitals decrease down a group
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| A double bond has how many pi and how many sigma bonds | One of each
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