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Chem 115 Exam 2
| Question | Answer |
|---|---|
| frequency | cycles/sec |
| wavelength | length |
| amplitude | height |
| higher amplitude | brighter |
| lower amplitude | dimmer |
| high energy | high frequency |
| low energy | low frequency |
| values of n>(equal to) 1; spherical | s orbitals |
| n>(equal to) 2 | p orbitals |
| any orbital can hold a max of how many e-? | two |
| lowest energy state | ground state |
| n goes up | absorption |
| n goes down | emission |
| energy difference for electronic transition | (h/2pi)(1/n(f)^2-1/n(1)^2) |
| c(speed of light)= | wavelength(frequency) |
| atomic radii trend | increase down; decrease right |
| energy required to remove and electron | ionization energy |
| ionization energy trend | down column decrease; across row increase |
| change in energy accompanying the addition of an electron to an atom or ion | electron affinity |
| electron affinity trend | down column decrease; across row increase |
| low IE forms | cations |
| high IE forms | anions |
| core takes how much energy to remove | a whole lot, especially compared to the outer levels |
| metallic trends | increase down; decrease right |
| transferring electrons form one element to another | ionic compounds |
| sharing electrons between atoms of different elements | covalent compounds |
| loses one electron; positive ion | cation |
| gains one electron; negative ion | anion |
| cation usually | metal |
| anion usually | nonmetal |
| covalent bonding is between | nonmetals |
| electrons shared among all the atoms in a solid | metallic bonding (NOT COVALENT -- that's just between two atoms) |
| metal plus metal | metallic bond |
| metal plus non metal | ionic bond |
| non metal plus non metal | covalent bond |
| the enthalpy change that accompanies the revers of one mol of ionic solid separating into gaseous ions | lattive energy |
| do ionic or covalent compounds conduct electricity | ionic |
| electron transfer is a _________ process | endothermic |
| requires energy | exothermic |
| lattice energy trend | decrease down; increase right |
| distance between nuclei at which potential energy is the lowest | bond length |
| requires energy | bond breaking |
| KJ to break bond and bond length | equilibrium |
| electronegativity trend | increase right; decrease down |
| have the same relative placement of atoms bt different locations of bonding and lone electron pairs | resonance structures |
| formal charge | # valence electrons - (unshared valence +1/2 shared electrons) |
| in resonance structures does the bond move or the atom | bond |
| if you can write two or more valid lewis structures, the actual electron distribution is... | an average of the distributions shown |
| VSEPR | Valence shell electron pair repulsion |
| 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 |
| two electron units (shape and degree) | linear 180 |
| three electron units no lone pairs | trigonal planar 120 |
| three electron units one lone pair | bent <120 |
| four electron units no lone pairs | tetrahedral 109.5 |
| four electron units one lone pair | trigonal pyramidal <109.5 |
| four electron units two lone pairs | bent <109.5 |
| central atom and five bonding groups | trigonal bipyramidal |
| central atom and six bonding groups | octahedral |
| double bonds effect bond angles similar to | lone pairs |
| an inbalance of charges over the whole molecule | molecular polarity |
| same molecular formula and different physical/chemical properties | constitutional isomer |
| polarity: trans vs cis | trans=non; cis=polar |
| dipole moment | measure of molecular polarity |
| when are covalent bonds polar | when atoms have different electronegativities and share electrons equally |
| titration | slowly adding an acid to a base until the reaction has reached the equivalence point |
| using a known amount of one reagent to determine the amount or concentration of another substance is | standardization |
| Molarity | moles/liters |
| q (enthalpy) | cm(DeltaT) or specific heat X mass X temp change |
| q (reaction) - q (solution)= | 0 |
| Which will have a higher lattice energy? A smaller compound or larger | Smaller - tighter bond |
| Which will have a higher lattice energy? An ionic compound with more or less ions? | More - hold tighter bond |
| Is combustion endothermic or exothermic? What about formation | Combustion: exothermic Formation: endothermic |
| Are stronger bonds short or long? | Short (ex. triple shorter and stronger than double) |
| What is the purpose of standardizing a solution | Determine concentration |
| Of the following, what radiation has the longest wavelength and what has the greatest energy? gamma; ultraviolet; visible | visible: longest wavelength gamma: greatest energy |
| 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 |
| A double bond has how many pi and how many sigma bonds | One of each |
Created by:
jkmccord11
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