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34 Cards in this Set
- Front
- Back
- 3rd side (hint)
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Number of bonds and lone pairs on a group 3 atom with a positive charge? |
Nonexistent |
Boron |
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Number of bonds and lone pairs on a group 3 atom with a neutral charge? |
3 bonds 0 LPs |
Boron |
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Number of bonds and lone pairs on a group 3 atom with a negative charge? |
4 bonds 0 LPs |
Boron |
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Number of bonds and lone pairs on a group 4 atom with a positive charge? |
3 bonds 0 LPs RARE |
Carbon |
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Number of bonds and lone pairs on a group 4 atom with a neutral charge? |
4 bonds 0 LPs |
Carbon |
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Number of bonds and lone pairs on a group 4 atom with a negative charge? |
3 bonds 1 LP |
Carbon |
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Number of bonds and lone pairs on a group 5 atom with a positive charge? |
4 bonds 0 LPs |
Nitrogen |
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Number of bonds and lone pairs on a group 5 atom with a neutral charge? |
3 bonds 1 LP |
Nitrogen |
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Number of bonds and lone pairs on a group 5 atom with a negative charge? |
2 bonds 2 LPs |
Nitrogen |
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Number of bonds and lone pairs on a group 6 atom with a positive charge? |
3 bonds 2 LPs |
Oxygen |
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Number of bonds and lone pairs on a group 6 atom with a neutral charge? |
2 bonds 2 LPs |
Oxygen |
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Number of bonds and lone pairs on a group 6 atom with a negative charge? |
1 bond 3 LPs |
Oxygen |
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Number of bonds and lone pairs on a group 7 atom with a positive charge? |
2 bonds 2 LPs |
Fluorine |
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Number of bonds and lone pairs on a group 7 atom with a neutral charge? |
1 bond 3 LPs |
Fluorine |
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Number of bonds and lone pairs on a group 7 atom with a negative charge? |
0 bonds 4 LPs ANION |
Fluorine |
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Number of total electron groups, number of bonding and non-bonding groups, and molecular geometry for Linear VSEPR (electron geometry)? |
2 EG 2 BG, 0 NBG, linear MG |
Sp hybridization and 180 degree angles |
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Number of total electron groups, number of bonding and non-bonding groups, and molecular geometry for Trigonal Planar VSEPR (electron geometry)? |
3 EG 3 BG, 0 NBG, trigonal planar MG 2 BG, 1 NBG, bent MG |
Sp2 hybridization and 120 degree bond angles |
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Number of total electron groups, number of bonding and non-bonding groups, and molecular geometry for Tetrahedral VSEPR (electron geometry)? |
4 EP 4 BG, 0 NBG, tetrahedral MG 3 BG, 1 NBG, trigonal pyramidal MG 2 BG, 2 NBG, bent MG |
Sp3 hybridization and 109.5 degree angles |
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Electronegative ranges for bonds |
< .4 nonpolar covalent .4. - 1.6 polar covalent 1.7 & above ionic |
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What determines the type of bond? |
Electronegative difference (1 electronegativity - the other) |
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Electronegativity of relevant atoms |
H= 2.1 B= 2.0 C= 2.5 N= 3.0 O= 3.5 F= 4.0 Cl= 3.0 Br= 2.8 I= 2.5 |
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What constitutes a polar molecule? |
Must have: a net dipole (asymmetry) at least 1 polar bond |
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Describe and rank intermolecular forces from strongest to weakest |
1) full-full/cation-anion 2) full-partial/ion-dipole 3) partial-partial/dipole-dipole H bonding with O, N, and sometimes F 4) london forces All molecules excluding salts |
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How do surface area and polarizability effect IMF strength? |
1) Linear molecues have more surface area than branched ones= greater IMFs 2) Less distortion of electron cloud (less jiggle)= greater IMFs |
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The less energy needed to overcome IMFs... |
...the lower the melting and boiling points and the higher the vapor pressure |
What happens to BP, MP, and vapor pressure? |
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How many electrons fit into each orbital and what is the order of orbitals? |
s= 2, p= 6, d= 10, f= 14 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 7s 7p |
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Arrhenius Acids & Bases |
H+ = acid OH- = base |
Original type |
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Bronsted-Lowry Acids & Bases |
H+ donor = acid H+ acceptor = base |
Results in conjugate acids and bases |
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Lewis Acids & Bases |
electron acceptor = acid electron donor = base |
Results in anion + another molecule |
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Formula for formal charge |
FC= group # - # of bonds - # of lone electrons |
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How many bonds can a (1) positively and (2) negatively charged Carbon have? |
1) 3 2) 3 + a lone pair |
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How to determine lone pairs on a line bond structure |
1) check how many electrons the atom should have (group #) 2) if the atom has a + charge it has less electrons 3) if the atom has a - charge it has more electrons 4) se the number of bonds present to determine the number of lone pairs (electrons should add up to group #) |
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How to determine hybridization |
Add # of bonds to # of groups of lone pairs Sum of 4 = sp3 (4) ex CH4, NH3, H2O Sum of 3 = sp2 (3) ex CH2O, CH3, NHO, O2 Sum of 2 = sp (2 and 2 p) ex CO2, NCF |
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How to determine relative importance of resonance structures |
1) minimize charge 2) make sure - is on more electronegative atom 3) + charge on electronegative atom is okay if all atoms have an octet |
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