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Organic Chemistry lab > Structure and Bonding > Flashcards

Structure and Bonding Flashcards

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1
Q

How is the quantum theory of atomic
structure differs from the Bohr’s theory?

A

The quantum theory explains that electrons
are in 3-dimensional shaped electron clouds that
represent the probability of an electron’s
location. Bohr’s theory explains that the
electrons are in orbits or shells.

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2
Q

What is the difference between an
orbit and an orbital?

A

Orbit is the idea of an electron “orbiting” the
nucleus like planets orbiting the sun. Orbitals are electron clouds that represent the shape of probability for an electron’s location.

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3
Q

What do electron configurations tell us
about the atom?

A

It tells about the detailed location of
electrons in an atom, the specific electron
orbitals that the electrons are found.

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4
Q

How many orbitals are in the fourth
energy level?

A

The 4th level contains s, p, d, and f orbitals,
so the total number of orbitals is 16.

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5
Q

How many orbitals of each type are
there? For s, p, d, and f?

A

s – 1
p – 3
d – 5
f - 7

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6
Q

______ of more than 30 million chemical compounds contain carbon.

A

90%

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7
Q

Origins of Organic Chemistry, Why is it so special?

A

Carbon is group 4A element, it can share 4 valence electrons and form 4
covalent bonds.

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8
Q

Who is often credited as
the father of modern
atomic theory?

A

John Dalton

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9
Q

Postulates by john Dalton

A
  1. Indivisibility of atom (WRONG)
  2. All atoms of the same element are
    identical (WRONG; isotopes)
  3. Different elements have very different
    types of atoms or differ in all respects
    (WRONG; isobars)
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10
Q

Who proposed the
planetary model of the
atom?

A

Niels Bohr

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11
Q

Planetary Model of the Atom, Main point

A
  1. Electrons orbit the nucleus in
    orbits that have a set size and
    energy. (WRONG)
  2. The energy of the orbit is
    related to its size.
  3. Radiation is absorbed or
    emitted when an electron moves
    from one orbit to another.
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12
Q

It states that there is an inherent
uncertainty in the act of measuring a
variable of a particle.

A

Heisenberg Uncertainty Principle

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13
Q

Originally, electrons were thought to orbit around the nucleus in defined paths

A

Electron orbit model

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14
Q

It was discovered that electrons move in waves in a defined space called an electron cloud

A

Electron cloud model

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15
Q

Structure of an atom: small diameter

A

(2 X 10-10 m = 200 pm)

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16
Q

very dense; contains protons and neutrons

A

Nucleus

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17
Q

Diameter of nucleus

A

small (10-15 m)

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18
Q

located in space remindful of a cloud (10-10 m) around nucleus

A

Electrons

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19
Q

number of protons in nucleus

A

The atomic number (Z):

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20
Q

number of protons plus neutrons

A

The mass number (A):

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21
Q

All atoms of same element have the same

A

Z value

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22
Q

atoms of the same element with different
numbers of neutrons and thus different A.

A

Isotopes:

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23
Q

(atomic weight) of an
element is weighted average mass in atomic
mass units (amu) of an element’s naturally
occurring isotopes.

A

atomic mass

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24
Q

There are four different kinds of orbitals for
electrons based on those derived for a hydrogen
atom
▪ Denoted

A

s, p, d, and f

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25
Q

spherical, nucleus at center

A

s orbitals:

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26
Q

dumbbell-shaped, nucleus at middle

A

p orbitals:

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27
Q

elongated dumbbell-shaped, nucleus
at center

A

d orbitals:

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28
Q

tetrahedral, nucleus at center

A

f orbitals:

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29
Q

Orbitals are grouped in ______ of increasing size and energy

A

shells

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30
Q

Each orbital can be occupied by ____________

A

two electrons.

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31
Q

Third shell contains an s orbital (3s), three p orbitals (3p),
and five d orbitals (3d), holds ______ electron

A

18

32
Q

Second shell contains one s orbital (2s) and three p orbitals
(2p), holds _____ electrons

A

eight

33
Q

Lobes of a p orbital are separated by region of zero electron
density,

A

node.

34
Q

(i.e., lowest energy arrangement) of an atom
▪ lists orbitals occupied by its electrons.

A

Ground-state electron configuration

35
Q

Rules ground-state electron configuration

A
  1. Lowest-energy orbitals fill first:
  2. Electrons act as if they were spinning around an axis.
    Electron spin can have only two orientations, up  and down
    . Only two electrons can occupy an orbital, and they must
    be of opposite spin
  3. If two or more empty orbitals of equal energy are
    available, electrons occupy each with spins parallel until
    all orbitals have one electron
36
Q

Principle in 1. Lowest-energy orbitals fill first:

A

(Aufbau (“build-up”) principle)

37
Q

Principle in Electrons act as if they were spinning around an axis.
Electron spin can have only two orientations, up  and down
. Only two electrons can occupy an orbital, and they must
be of opposite spin

A

(Pauli exclusion principle)

38
Q

Principle: 3. If two or more empty orbitals of equal energy are
available, electrons occupy each with spins parallel until
all orbitals have one electron

A

(Hund’s rule).

39
Q

Atoms form bonds because

A

the resulting compound is more
stable than the separate atoms

40
Q

Ionic bonds in salts form by

A

electron transfers

41
Q

(electron dot) show valence electrons of
an atom as dots

A

Lewis structures

42
Q

have a line drawn
between two atoms indicating a 2 e- covalent bond.

A

Kekulé structures

43
Q

Stable molecule results at completed shell,

A

octet (eight dots)
for main-group atoms (two for hydrogen)

44
Q

Atoms with one, two, or three valence electrons form

A

one,
two, or three bonds, respectively.

45
Q

Atoms with four or more valence electrons form as many
bonds as electrons needed to fill the s and p levels of their
valence shells to reach a _____________

A

stable octet.

46
Q

Carbon has four valence electrons (2s

2 2p
2
), forming ________

A

four bonds

47
Q

Valence electrons not used in bonding are called

A

nonbonding electrons, or lone-pair electrons

48
Q

forms when two atoms approach each other
closely so that a singly occupied orbital on one atom
overlaps a singly occupied orbital on the other atom

A

Covalent bond

49
Q

Two models to describe covalent bonding:

A

▪ Valence bond theory
▪ Molecular orbital theory

50
Q

Electrons are paired in the overlapping orbitals and are
attracted to nuclei of both atoms
▪ H–H bond results from the overlap of two singly occupied
hydrogen 1s orbitals

A

Valence Bond Theory:

51
Q

H-H bond is cylindrically symmetrical,

A

sigma (s) bond

52
Q

H–H has bond strength of

A

436 kJ/mol

53
Q

is a factor
that leads to
maximum or
minimum stability.

A

Distance between
nuclei

54
Q

If too close, they
repel because both
are

A

positively
charged

55
Q

If too far apart,
bonding is

A

weak

56
Q

independently observed that carbon
always has four bonds

A

Kekulé and Couper

57
Q

proposed that the four bonds of
carbon have specific spatial directions

A

van’t Hoff and Le Bel

58
Q

sp3 hybrid orbitals: an s orbital and three p orbitals combine to form four

A

equivalent, unsymmetrical, tetrahedral
orbitals

59
Q

C–H bond has a strength of ______ and a length of _____ pm

A

439 kJ/mol and 109 pm

60
Q

The remaining p orbital in sp2 is

A

perpendicular to the plane

61
Q

Two sp2

-hybridized
orbitals overlap to form a

A

s bond.

62
Q

Two sp2

-hybridized
orbitals overlap to form a

A

sigma

bond

63
Q

Electrons in the s bond are

A

centered between nuclei

64
Q

Electrons in the sigma bond

A

occupy regions are on either side
of a line between nuclei

65
Q

Ethylene C=C bond length ____

A

134 pm

66
Q

sp orbital placement of tow p-orbitals

A

perpendicular to the y and z axis

67
Q

H–N–H bond angle in ammonia
(NH3)

A

107.3°

68
Q

C-N-H bond angle is

A

110.3 °

69
Q

where electrons are most likely
to be found (specific energy and general shape) in a molecule

A

molecular orbital

70
Q

MO is lower in energy

A

Additive combination

71
Q

MO is higher in
energy

A

Subtractive combination

72
Q

is from combining p orbital lobes with
the same algebraic sign

A

The additive bonding MO

73
Q

is from combining lobes with
opposite signs

A

The  antibonding MO

74
Q

don’t
have C-H or C-C single
bonds shown. They are
understood.

A

Condensed structures

75
Q

Drawing Skeletal Structures
(Commonly Used)

A

1) Carbon atoms
aren’t usually
shown
2) A carbon atom is assumed to be at each intersection of
two lines (bonds) and at the end of each line.
3) Hydrogen atoms bonded to carbon aren’t shown.
4) Atoms other than carbon and hydrogen ARE shown

76
Q

Electrons occupy ______ around the nucleus.

A

orbitals

Organic Chemistry lab (6 decks)

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