Organic Chemistry Exam 1 Test Questions – Flashcards
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where is carbon located in the periodic table? |
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2nd row |
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atoms to the left of carbon tend to |
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give up electrons |
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atoms to the right of carbon tend to |
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receive electrons |
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what prevents the positively charged nucleus from drawing in the negative electrons? |
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kinetic energy of the electrons |
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where does the mass of an atoms mostly come from? the volume? |
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mass-protons and neutrons=nucleus volume-electrons |
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atomic number |
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number of protons in a nucleus OR number of electrons on a neutral atom |
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mass number |
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number of protons and neutrons |
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isotopes |
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have the same atomic numbers BUT different mass numbers because they have a different number of neutrons |
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half-life |
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time it takes for 1/2 of the nuclei to decay |
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atomic weight |
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average weighted mass of an element's atoms |
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molecular weight |
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sum of atomic weights of all the atoms in a molecule |
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wave equation |
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describes the behavior of an electron |
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wave function or orbital |
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is the solution to a wave equation and tells 1. energy of electron 2.where it is most likely to be found |
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quantum mechanics |
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characterizes movement of an electron around the nucleus like the wave motion of a guitar string |
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atomic orbital |
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3-D region of volume where an e- is most likely to be found |
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the closer an atomic orbital is to the nucleus, the _______ it's energy |
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lower |
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degenerate orbitals |
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orbitals with the same energy |
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what are the 3 principles that are considered in ground state electron configurations? |
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1. aufbau 2. pauli-exclusion 3. hund's rule |
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aufbau principle |
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an electron would rather occupy an available atomic orbital of the least energy (closer to the nucleus) |
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pauli-exclusion principle |
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1. max of 2 e- in each atomic orbital 2. they must be of opposite spin |
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hund's rule |
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an e- would rather occupy an empty atomic orbital before one that already has an e- to minimize electron repulsion |
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electropositive where are they found? |
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elements that readily lose an e- and become + charged; 1st column: the alkali metals |
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electronegative |
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elements that will readily gain an electron and become positive; column 17 |
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ionic bond |
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bond due to only electrostatic attractions (attraction b/t opposite charges) and where electrons are transferred and NOT shared |
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if a hydrogen atom loses its only e- then it becomes |
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positive ion: a proton |
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if a hydrogen atom gains an e- to have 2 electrons in its outer shell it is a |
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negatively charged ion: a hydride ion |
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nonpolar covalent bond |
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electrons are shared equally |
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polar covalent bond |
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the atoms of the bond have different electronegativities,therefore the e- are NOT shared equally |
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the greater the difference of the electronegativity in a polar bond the more ___________ the bond is |
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polar |
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what type of bond has a dipole? |
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a polar bond |
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dipole |
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a polar bond that has a - and + end |
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dipole moment |
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the size of the dipole in a polar bond |
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what is the formula used to determine the dipole moment? |
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?=e x d
?= dipole moment
e= magnitude of charge
d= distance between the charges |
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what is the charge on an electron in electrostatic units (esu)? |
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4.8 x 10-10 esu |
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a bond length of 1.39A would be what value in cm? |
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1.39 x 10-8 cm |
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6.97 esu cm or 6.97 x 10-18 esu cm would be what value in D (debye) units? |
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6.97 D |
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electrostatic potential maps |
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show the distribution of charge in a molecule |
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in an electrostatic map what does blue and red represent? what is most attracted to them? |
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red- most negative electrostatic potential: attracts + charge blue- most positive electrostatic potential attracts negative charge |
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why in the electrostatic potential maps for LiH and HF was the H in LiH larger? |
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Because a potential map marks the edges of a molecule's electron cloud and the electron cloud around the H in LiH is largest because it has more electrons around it than the other H in HF. |
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Lewis structure |
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uses dots to represent valence electrons |
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formal charge |
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FC=valence electrons - (lone pair electrons + 1/2 bonding electrons) |
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free radical or radical |
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any species with a single lone pair electron |
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kekule structures |
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lone pair e- are not shown except to make a point |
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in a neutral atom how many lone pairs should these atoms ALWAYS have? nitrogen- oxygen- halogen (such as chlorine)- |
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N-1 O-2 Halogen-3 |
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condensed structures |
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don't show covalent bonds and list atoms bonded together |
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Heisenberg uncertainty principle |
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cannot determine location and momentum of an electron simultaneously |
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is the electron density more or less in 2s than in 1s? |
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the e- density in 2s is less because it is a larger sphere that is farther away from the nucleus |
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radial node |
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node found in spherical atomic orbital (s), probability of finding a e- is 0 |
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nodal plane |
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node of the p orbital |
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molecular orbital theory (MO) |
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covalent bonds form when AO combine to form MO |
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? bond |
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formed when two "s" orbitals overlap or two "p" orbitals overlap end on end |
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? bond |
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formed when two "p" atomic orbitals overlap side to side |
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which bonds are cylindrically symmetrical? which aren't? |
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? is NOT ? is |
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maximum stability= |
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minimal energy |
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bond length |
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when maximum stability is achieved (which means minimal energy) |
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bond dissociation energy |
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energy needed to break a bond or energy that is released when the bond forms |
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when a covalent bond is formed, what happens in terms of energy? |
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energy is released when a covalent bond is formed |
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explain ? bonding |
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is constructive; e- are most likely in between nuclei, attracting them and increasing e- density which binds atoms |
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explain ?* bonding |
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destructive, there is a node so no e- will be there. the two + nuclei will repel each other |
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how does the amount of overlap affect the strength of a bond? |
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the greater the overlap=stronger covalent bond |
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the strongest covalent bonds are formed by e- that occupy MO with the ______ energy. Why? |
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least; because the lower the energy, the more stable |
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how many nodes do these have (for s and p)? ? ? ?* ?* |
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?- s:0 p:2 ?- p:1 ?*- s:1 p:3 ?*- p:2 |
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in terms of overlap, which is greater: p orbitals overlapping side to side or end to end? |
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end to end |
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which is more stronger? ? ? ?* ?* place them in order |
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a ? is stronger than ? because it is more stable (less energy). ?>?>?*>?* |
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When 2 p AO form 2 MO, the AO of the more EN will contribute more to ______ while the least EN will for the _______ |
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more EN: bonding lesser: antibonding |
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VSEPR |
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valence shell electron pair repulsion: minimization of e- repulsion by the positioning of lone pairs as far as possible |
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what are the bond angles in methane, or any tetrahedron? |
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109.5 |
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in organic chemistry, all single bonds are ____ bonds |
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? bonds |
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trigonal planar bond angle what compound uses this? |
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120 ethene (ethylene) |
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what are in the different bonds in terms of ? and ?? |
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single: 1 ? double: 1 ? and 1 ? triple: 1 ? and 2 ? |
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what is the strongest and shortest bond? why? |
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triple; b/c its held together by 6 e- |
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what is the angle for a triple bond? |
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180 |