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Organic Chem I - UKY > Review of Gen Chem - Ch. 1 > Flashcards

Review of Gen Chem - Ch. 1 Flashcards

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1
Q

What is a HDI? What is it used to calculate?

A

Hydrogen Deficiency Index; Used to determine molecular formula and structure of compounds based on the degrees of unsaturation

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2
Q

Define saturated compounds

A

Possess the maximum number of hydrogen atoms possible relative to the number of carbon atoms present

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3
Q

Define unsaturated compounds

A

compounds with pi bonds/rings that possess less than the maximum number of hydrogen atoms

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4
Q

What is the formula to calculate HDI? What are the terms?

A

.5(2C + 2 + N - H - X)
C - Carbon
N - Nitrogen
X - Halogens

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5
Q

What are present in the structures when HDI is 0? 1? 2?

A

0 - no pi bonds; all sigma bonds
1 - 1 double bond OR 1 ring
2 - 2 rings, 2 double bonds, OR 1 ring and 1 double bond, OR 1 triple bond

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6
Q

What is the Structural Theory of Matter?

A

States that each element will form predictable number of bonds

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7
Q

How many bonds will form for each of the following elements: Carbon, Nitrogen, Oxygen, Halogens?

A

Carbon - 4
Nitrogen - 3
Oxygen - 2
Halogens - 1

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8
Q

List the steps to drawing Constitutional Isomers

A
  1. Determine Valencies
  2. Connect high valent atoms and place the lowest at the ends
  3. Consider other ways to connect
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9
Q

What is a constitutional isomer?

A

A compound/structure that has the same molecular formula as another but different structures

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10
Q

What is a covalent bond?

A

Result of two atoms sharing a pair of electrons

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11
Q

When there is a covalent bond, what forces should be accounted for?

A
  1. force of repulsion between 2 electrons
  2. force of repulsion between 2 positive nuclei
  3. force of attraction between 2 above
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12
Q

Define the octet rules

A

Small structures are combined based on trends that achieve electron configuration with full valence shell

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13
Q

What are the steps to drawing Lewis Structures?

A
  1. Draw individual atoms and count valence electrons
  2. Connect atoms forming multiple bonds
  3. Connect hydrogen atoms
  4. Connect unpaired electrons to complete octets
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14
Q

How are octets achieved?

A

when existing electrons are shared

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15
Q

Define formal charge

A

associated with any atom that does not exhibit appropriate number of valence electrons

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16
Q

What are the steps to calculate formal charge? What is the formula?

A
  1. Find valence electrons needed
  2. Find valence electrons present
  3. Find the difference

Formula: VE - (Dots + Lines)

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17
Q

Define electronegativity

A

Measure of the ability of atoms to attract electrons

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18
Q

What is the trend of electronegativity on the periodic table?

A

Increases across a period and bottom to top; the closer to fluorine

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19
Q

How are bonds classified according to electronegativity?

A

Covalent Bonds - difference less than 0.5
Polar Covalent Bonds - difference greater than 0.5 and less than 1.7
Ionic Bonds - difference less than 1.7

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20
Q

Steps to identify dipole moments

A
  1. Find all polar-covalent bonds
  2. Determine direction of dipoles
  3. Locate partial charges
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21
Q

What are electrostatic potential maps?

A

3D rainbow like images visualizing partial charges

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22
Q

Where on the periodic table are the atomic orbitals located?

A

S - groups 1 & 2
D - groups 3-12
P - groups 13-18
F - bottom transition metals

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23
Q

What is an orbital?

A

region of space occupied by electrons that contain 90-95% of electron density

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24
Q

What are the shapes of atomic orbitals?

A

S- sphere
P - dumbbell
D - clover

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25
Define degenerate orbitals
orbitals with the same energy
26
How do nodes relate to energy of the orbitals?
The more nodes the more energy
27
Define Aufbau Prinicple
Lowest energy orbital filled first
28
Pauli Exclusion Principle
orbitals can only have 2 electrons with opposite spin
29
Define Hund's Rule
In degenerate orbitals, each is filled with one electron before given a second
30
Define valence bond theory
sharing of electron density between 2 atoms as a result of constructive interference of atomic orbitals
31
Define constructive interference
produces a wave with large amplitude
32
Define destructive interference
waves cancel each other producing a node
33
What kind of bonds are present in a triple bond? Double bond? Single bond?
Triple: 1 sigma, 2 pi Double: 1 sigma, 1 pi Single: 1 sigma
34
Define steric number
number of electron pairs and bonded atoms of an element
35
Define Molecular Orbital
new orbital produced when atomic orbitals are combined
36
Describe the difference between an atomic orbital and a molecular orbital
AOs are individual atoms and MOs are entire molecules and is considered a single entity held together by many electron clouds
37
Define Bonding Molecular Orbital
lower energy orbital; result of constructive interference of the original 2 AOs
38
Define Antibonding Molecular Orbital
higher energy MO; result of destructive interference (has nodes which create more energy)
39
Define HOMO
Highest Occupied Molecular Orbital; highest energy of those MOs that are occupied
40
Define LUMO
Lowest Unoccupied Molecular Orbital; lowest energy of those unoccupied
41
Why can Carbon form 4 bonds?
When carbon is in the excited state, the electron configuration has 4 half filled degenerate orbitals, allowing it to form 4 bonds. These orbitals are sp3 hybridized and create unsymmetrical lobes where the front lobe is much larger, which is more efficient in forming bonds.
42
What are the conditions for a tetrahedral geometry?
sp3 and no lone pairs
43
What are the conditions for a trigonal pyramidal geometry?
sp3 with 1 lone pair
44
What are the conditions for a bent geometry?
sp3 with 2 lone pairs OR sp2 with 1 lone pair
45
What are the conditions of a trigonal planar geometry?
sp2 with No lone pairs
46
What are the conditions for a linear geometry?
sp with No lone pairs
47
Why will octane and water not mix?
The polarity is different and like dissolves like
48
Explain how constitutional isomers of C2H6O can have different polarities?
The intermolecular force in one isomer may be stronger in the other
49
For every degree of unsaturation, there are _____ missing.
2 Hydrogen atoms
50
Unpaired electrons tell you how many ______ ______ ______ with that atoms in ______ ______ _______.
Bonds will form; neutral organic molecules
51
How many non hydrogen atoms must there be to draw a ring?
3
52
Define heteroatom
Non-carbon/non-hydrogen atoms
53
What is the pattern of formal charge for Carbon?
4 bonds = 0; 3 bonds and 0 lone pairs = +1; 3 bonds and 1 lone pair = -1
54
What is the pattern of formal charge for oxygen?
1 bond and 3 lone Paris = -1; 2 bonds and 2 lone pairs = 0; 3 bonds and 1 lone pair = +1
55
What is the pattern of formal charge for Nitrogen?
3 bonds and 1 lone pair = 0; 4 bonds = +1; 2 bonds and 2 lone pairs = -1
56
Why are Bromine-Carbon bonds considered to be polar covalent?
Though the electronegativity difference is 0.3, Bromine is a much large atom than Carbon so…. - the orbitals do not overlap well and create a very weak bond - Bromine only wants 6 VE as well so it causes a weird bond to occur
57
What does n stand for?
Principle Quantum Number; period the element is located in
58
What makes up a sp3 hybridization?
Atomic s-orbital and 3 atomic p-orbitals that make 4 sp3 orbitals
59
What makes up an sp2 hybridization?
Combination of 2s AO and 2 p AOs with one remaining 2p AO
60
What makes up an sp hybridization?
One 2s orbital and one 2p orbital that form 2 sp2 hybrid orbitals
61
Sigma bonds are ____ in energy than pi bonds because the energy is _____ _____ ____ while in pi bonds the energy ____ ____ ____ ____ (either _____ or ____)
Lower; shared between atoms; resides on one side; top or bottom
62
List the three main intermolecular forces from strongest to weakest
1. Hydrogen Bonding 2. Dipole-Dipole Interactions 3. London Dispersion Forces
63
What is the formula to determine the maximum number of hydrogen and halogens within a structure?
2n + 2, where n = number of carbons

Organic Chem I - UKY (3 decks)

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