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CCP 3.1 > 2. Structure and Bonding [revised] > Flashcards

2. Structure and Bonding [revised] Flashcards

1
Q

explains that electrons are in 3-dimensional shaped electron clouds that represent the probability of an electron’s location.

A

QUANTUM THEORY

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2
Q

explains that the electrons are in orbits or shells.

A

BOHR’S THEORY

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3
Q

the idea of an electron “orbiting” the
nucleus like planets orbiting the sun.

A

orbit

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4
Q

electron clouds that represent the shape of probability for an electron’s location.

A

orbitals

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5
Q

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

A

electron configuration

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6
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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7
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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8
Q

__% of more than 30 million chemical compounds contain carbon.

A

90%

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9
Q

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

A

JOHN DALTON

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10
Q

TRUE OR FALSE

  1. Indivisibility of atom
  2. All atoms of the same element are
    identical
  3. Different elements have very different
    types of atoms or differ in all respects
A
  1. wrong
  2. wrong, isotopes
  3. wrong, isobars
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11
Q

Who proposed the planetary model of the
atom?

A

Niels Bohr

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12
Q

TRUE OR FALSE

  1. Electrons orbit the nucleus in
    orbits that have a set size and energy.
  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.
A
  1. wrong
  2. true
  3. true
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13
Q

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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14
Q

model when electrons where originally thought to orbit around the nucleus in defined paths

A

electron orbit model

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15
Q

model when it was discovered that electrons move in waves in a defined space called an electron cloud

A

electron cloud model

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16
Q

Structure of an atom: small diameter size

A

2 x 10-10 m = 200 pm

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17
Q

very dense; contains protons and neutrons

▪ protons (positively charged)
▪ neutrons (neutral)
▪ small (10-15 m)

A

nucleus

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18
Q

▪ negatively charged
▪ 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

All atoms of same element have the same Z value

A

atomic number (Z)

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20
Q

number of protons plus neutrons

A

mass number (A)

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21
Q

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

A

isotopes

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22
Q

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

A

The atomic mass

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23
Q

four different kinds of orbitals for electrons based on those derived for a hydrogen atom

A

s, p, d, f

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24
Q

most important orbitals in organic and biological chemistry

A

s and p orbitals

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24
Q

spherical, nucleus at center

A

s orbitals

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25
Q

dumbbell-shaped, nucleus at middle

A

p orbitals

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26
Q

elongated dumbbell-shaped, nucleus at center

A

d orbitals

27
Q

tetrahedral, nucleus at center

A

f orbitals

28
Q

____ are grouped in shells of increasing size and energy

A

orbitals

29
Q

Each orbital can be occupied by how many electrons

A

two electrons

30
Q

First shell contains one s orbital, denoted as 1s, holds only ___ electrons

A

2 electrons

31
Q

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

A

8 electrons

32
Q

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

A

18

33
Q

Lobes of a p orbital are separated by region of zero electron density, which is called a _____.

A

node

34
Q

▪ lists orbitals occupied by its electrons.

(i.e., lowest energy arrangement)

A

Ground-state electron configuration

35
Q

states that the lowest-energy orbitals must be filled first

A

Aufbau (“build-up”) principle

36
Q

states that only two electrons can occupy an orbital, and they must be of opposite spin to have unique wave equations

A

Pauli exclusion principle

37
Q

states that 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

38
Q

_____ bonds in salts form by electron transfers

A

ionic

39
Q

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

A

Lewis structures

40
Q

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

A

Kekulé structures

41
Q

Valence electrons not used in bonding are called

A

nonbonding electrons, or lone-pair electrons

42
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

43
Q

▪ Two models to describe covalent bonding:

A

▪ Valence bond theory
▪ Molecular orbital theory

44
Q

Electrons are paired in the overlapping orbitals and are attracted to nuclei of both atoms

A

Valence Bond Theory

45
Q

Who independently observed that carbon always has four bonds

A

Kekulé and Couper

46
Q

Who proposed that the four bonds of carbon have specific spatial directions

A

van’t Hoff and Le Bel

47
Q

s orbital and three p orbitals combine to form four equivalent, unsymmetrical, tetrahedral orbitals

Bond angle: 109.5°: the tetrahedral angle.

A

sp3 hybrid orbitals

48
Q

2s orbital combines with two 2p orbitals, giving 3 orbitals. This results in a double bond.
▪ 120° angles
▪ The remaining p orbital is perpendicular to the plane

A

sp2 hybrid orbitals

49
Q

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

▪ Additive combination (bonding) MO is lower in energy
▪ Subtractive combination (antibonding) MO is higher in
energy

A

molecular orbital (MO)

50
Q

The π _____ MO is from combining p orbital lobes with the same algebraic sign

A

π bonding

51
Q

The π _____ MO is from combining lobes with opposite signs

A

π antibonding

52
Q

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

A

Condensed structures

53
Q

charged nucleus containing positively charged protons and neutrally charged neutrons surrounded by negatively charged electrons

A

Atom

54
Q

Electronic structure of an atom is described by

A

wave equation

55
Q

__ orbitals are spherical, __ orbitals are dumbbell-shaped

A

s orbitals
p orbitals

56
Q

electron pair is shared between atoms

A

Covalent bonds

57
Q

electron sharing occurs by overlap of
two atomic orbitals

A

Valence bond theory

58
Q

bonds result from combination of atomic orbitals to give molecular orbitals, which belong to the entire molecule

A

Molecular orbital (MO) theory

59
Q

Circular cross-section and are formed by
head-on interaction

A

Sigma (σ)bonds

60
Q

“dumbbell” shape from sideways interaction of p orbitals

A

Pi (π) bonds

61
Q

In single bonds with tetrahedral geometry, carbon has four ____ hybrid orbitals

A

sp3 hybrid orbitals

62
Q

In double bonds with planar geometry, carbon uses three equivalent ___ hybrid orbitals and one unhybridized p orbital

A

sp2 hybrid orbitals

63
Q

Carbon uses two equivalent __ hybrid orbitals to form a triple bond with linear geometry, with two unhybridized p orbitals

A

sp hybrid orbitals

64
Q

Atoms such as nitrogen and oxygen hybridize to form strong, oriented bonds
▪ The nitrogen atom in ammonia and the oxygen atom in water are ___ hybridized

A

sp3 hybridized

CCP 3.1 (4 decks)

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