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Organic Chem > Lecture 2 > Flashcards

Lecture 2 Flashcards

(61 cards)

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1
Q

Nucleus is consist of?

A

Protons and neutrons (most of the mass)

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2
Q

Sorrounded by ___ in a large vol of space

A

Electrons (most of the volume)

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3
Q

What can be known in Quantum mechanicsl model?

A

Electron exact location can’t be known,only the Electron density

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4
Q

The propability that the electron will be in a certain region of space (orbital) at a given instant)

A

Electron Density

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5
Q

Where the electrons circle around

A

Orbitals

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6
Q

Used to describe orbitals

A

Quantum numbers

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7
Q

4 types of quantum number

A
  1. Principal
  2. Azithmutal/angular momentum
  3. Magnetic
  4. Electron spin
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8
Q

Symbols of each quantum nos.

A
  1. Principal - n
  2. Azithmutal/angular momentum - l
  3. Magnetic - ml
  4. Electron spin - ms
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9
Q

Meaning of principal

A

Size (energy level, shell)

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10
Q

Meaning of azimuthal or nagular movemont

A

Shape (subshell)

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11
Q

Meaning of magnetic

A

Orientation (orbital)

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12
Q

Meaning of electron spin

A

Direction

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13
Q

Possible value of principal

A

Postive integers

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14
Q

Possible value of azimuthal

A

S,p,d,f

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15
Q

Positive value of magnetic

A

-1 to +1

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16
Q

Positive value of electron spin

A

-1/2,+1/2

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17
Q

Describes the orbitals occupied by the atom’s electrons when they are all in the available orbitals with the lowest energy

A

Ground state electron configuration

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18
Q

4 rules in electron configuration

A
  1. Aufbau principle
  2. Hand’s rule
  3. Pauli’ exclusion principle
  4. Heisenberg-s uncertainty principle
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19
Q

Electrons below the outermost shell

A

Core electrons

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20
Q

Electrons in the outermost shell

A

Valence electron

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21
Q

Attractive force between two atom or ion

A

Chemical bond

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22
Q

What happens in chemical bond?

A

More stable and lower in energy than separate atoms

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23
Q

Most stable, outershell has eight electron and has no electrons of higher energy.

A

Octet rule

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24
Q

Exception in octet rule (2 element)

A

Hydrogen and helium (can occupy 2 electron)

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25
Chemistry of main group elements is governed by their tendency to take on the electron configuration of the nearest _____.
Noble gas
26
Two types of chemical bond
Ionic and covalent
27
Attractive forces between opposite charges
Electrostatic attraction
28
Bond formed as a result of the electrostatic attraction between ions
Ionic bond
29
Ionic bond formed from the ____ and ____.
Transfer of electrons Reaction of metal with non metal
30
Sharing electrons between two nuclei
Covalent bond
31
Compunds formed by covalent bonds
Molecular compounds
32
Measure of the ability of an atom to pull the bonding electrons toward itself
Electronegativity
33
Electronegativity in periodic table
Increasing from left to right and down to up
34
Two types of covalent bond
Polar and non polar covalent bond
35
Same electronegativity
Nonpolar
36
Different electronegativity
Polar covalent bond
37
No electron shared Opposite charges attract each other
Ionic bond
38
Electron shared Same electronegativity
Polar covalent bond
39
Electron shared equally Different electronegativity
Non polar covalent bond
40
Electronegativity difference of non polar
Less than 0.4
41
Electronegativity differenec of polar
Between 0.4 and 1.8
42
Electronegativity difference of ionic
More than 1.8
43
Polar molecules have ____
Dipoles
44
A pair of equal and oppositely charged poles separated by a distance
Dipole
45
measure of dipole
Dipole Moment
46
how to get dipole
magnitude of the charge on either atom x distance between the two charges
47
Two chemical structures with definition Lewis Structures – electron-dot structures Kekulé Structures – line-bond structures
Lewis Structures – electron-dot structures Kekulé Structures – line-bond structures
48
4 elements in chemical structure
• Chemical symbols • Covalent bond • Nonbonding/lone-pair electrons • Formal charges
49
not an actual charge used for bookkeeping of electrons the charge the atom would have if each bonding electron pair in the molecule were shared equally between atoms
Formal charge
50
the difference between the number of valence electrons an atom has when it is not bonded to any other atoms and the number it “owns” when it is bonded
Formal charge
51
omitting of the covalent bonds and listing atoms bonded to a particular carbon (or nitrogen or oxygen) next to it (with a subscript if there is more than one of a particular atom).
Condensed Structures
52
condensed and kekule structure rules
*reviewer
53
rules in skeletal structure
• Carbon atoms aren’t usually shown. • A carbon atom is assumed to be at each intersection of two lines (bonds) and at the end of each line. • Hydrogen atoms bonded to carbon aren’t shown. • Atoms other than carbon and hydrogen are shown.
54
3 3D structures and its meanings
• Perspective Drawing – shows 3D shape • Ball-and-Stick Model – shows bond angles accurately • Space-Filling Model – shows atoms in scale
55
bond lies in the plane of the paper (staight line)
normal bond
56
bond extends backwards, away from the viewer, so effectively into the paper(broken lines)
dashed bond
57
bond protudes forwards, toward the viewer, so efffectively out of the paper
wedged bond
58
Geometry based on arrangement of atoms in a molecule
Molecular geometry
59
Geometry based on arrangement of atoms in a molecule that is defined by bond angles
Molecular geometry
60
Geometry based on valence electron pairs (bonding and non-bonding) around a central atom
Electron pair geometry
61
model for the prediction of molecular geometry based on the minimization of electron repulsion between regions of electron density around an atom
VALENCE-SHELL ELECTRON-PAIR REPULSION (VSEPR) MODEL

Organic Chem (3 decks)

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