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Organic Chem > Lecture 2 > Flashcards

Lecture 2 Flashcards

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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
Q

Chemistry of main group elements is governed by their tendency to take on the electron configuration of the nearest _____.

A

Noble gas

26
Q

Two types of chemical bond

A

Ionic and covalent

27
Q

Attractive forces between opposite charges

A

Electrostatic attraction

28
Q

Bond formed as a result of the electrostatic attraction between ions

A

Ionic bond

29
Q

Ionic bond formed from the ____ and ____.

A

Transfer of electrons
Reaction of metal with non metal

30
Q

Sharing electrons between two nuclei

A

Covalent bond

31
Q

Compunds formed by covalent bonds

A

Molecular compounds

32
Q

Measure of the ability of an atom to pull the bonding electrons toward itself

A

Electronegativity

33
Q

Electronegativity in periodic table

A

Increasing from left to right and down to up

34
Q

Two types of covalent bond

A

Polar and non polar covalent bond

35
Q

Same electronegativity

A

Nonpolar

36
Q

Different electronegativity

A

Polar covalent bond

37
Q

No electron shared
Opposite charges attract each other

A

Ionic bond

38
Q

Electron shared
Same electronegativity

A

Polar covalent bond

39
Q

Electron shared equally
Different electronegativity

A

Non polar covalent bond

40
Q

Electronegativity difference of non polar

A

Less than 0.4

41
Q

Electronegativity differenec of polar

A

Between 0.4 and 1.8

42
Q

Electronegativity difference of ionic

A

More than 1.8

43
Q

Polar molecules have ____

A

Dipoles

44
Q

A pair of equal and oppositely charged poles separated by a distance

A

Dipole

45
Q

measure of dipole

A

Dipole Moment

46
Q

how to get dipole

A

magnitude of the charge on either atom x distance between the two charges

47
Q

Two chemical structures with definition Lewis Structures – electron-dot structures
Kekulé Structures – line-bond structures

A

Lewis Structures – electron-dot structures
Kekulé Structures – line-bond structures

48
Q

4 elements in chemical structure

A

• Chemical symbols
• Covalent bond
• Nonbonding/lone-pair electrons
• Formal charges

49
Q

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

A

Formal charge

50
Q

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

A

Formal charge

51
Q

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).

A

Condensed Structures

52
Q

condensed and kekule structure rules

A

*reviewer

53
Q

rules in skeletal structure

A

• 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
Q

3 3D structures and its meanings

A

• Perspective Drawing – shows 3D shape
• Ball-and-Stick Model – shows bond angles accurately
• Space-Filling Model – shows atoms in scale

55
Q

bond lies in the plane of the paper (staight line)

A

normal bond

56
Q

bond extends backwards, away from the viewer, so effectively into the paper(broken lines)

A

dashed bond

57
Q

bond protudes forwards, toward the viewer, so efffectively out of the paper

A

wedged bond

58
Q

Geometry based on arrangement of atoms in a molecule

A

Molecular geometry

59
Q

Geometry based on arrangement of atoms in a molecule that is defined by bond angles

A

Molecular geometry

60
Q

Geometry based on valence electron pairs (bonding and non-bonding) around a central atom

A

Electron pair geometry

61
Q

model for the prediction of molecular geometry based on the minimization of electron repulsion between regions of electron density around an atom

A

VALENCE-SHELL ELECTRON-PAIR
REPULSION (VSEPR) MODEL

Organic Chem (3 decks)

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