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Chem 31 > Module 2: Bonding and Structure of Organic Compounds > Flashcards

Module 2: Bonding and Structure of Organic Compounds Flashcards

1
Q

The best Lewis structure is the one with the?

A

fewest charges

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2
Q

To determine the geometry:

A

[1] Draw a valid Lewis structure
[2] Count groups around a given atom

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3
Q

If two or more degenerate orbitals are available, one electron is placed in each orbitals with their spins parallel until all are half-full.

A

Hund’s rule

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4
Q

A π bond is formed by side-by-side overlap of?

A

two 2p orbitals

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5
Q

A _____________ is formed by side-by-side overlap of two 2p orbitals.

A

π bond

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6
Q

σ bonds are __________ than π bonds

A

stronger

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7
Q

What orbitals do the first-and second-row atoms use to form bonds?

A

s and p orbitals

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8
Q

It is based on the fact that electron pairs repel each other, so we need to consider the lone pairs.

A

VSEPR

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9
Q

All single bonds are?

A

sigma bonds

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10
Q

Rule 2 in electron configuration

A

Pauli exclusion principle

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11
Q

type of covalent bond: between unhybridized parallel p orbitals

A

pi bond

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12
Q

_________________ down a column of the periodic table as the size of an atom increases

A

increases

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13
Q

To summarize, a C=C bond consists of?

A

one sigma bond and one pi bond

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14
Q

trend: right to left and up to down

A

atomic size increases

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15
Q

electrons are arranged in __________ at various distances from the nucleus

A

“shells”

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16
Q

Group IVA

A

tetrels

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17
Q

Group IA

A

alkali metals

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18
Q

The charge assigned to individual atoms in a Lewis structures

A

Formal charge

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19
Q

It is the joining of two atoms in a stable arrangement.

A

bonding

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20
Q

trend: down to up and left to right

A

electronegativity and ionization energy increases

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21
Q

This result from the transfer of electrons from one element to another.

A

ionic bonds

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22
Q

the most stable arrangement keeps the groups as far away as possible from the others to minimize repulsions.

A

Valence-shell Electron-pair Repulsion(VSEPR)Theory

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23
Q

These orbitals are formed when 1 s orbital combines with 1 p orbital

A

sp hybrid orbitals

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24
Q

Orbitals are filled so that those
of lowest energy are filled first

A

Aufbau principle

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25
Q

Group VA

A

pnictogens

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26
Q

A __________________ consists of the simultaneous attraction of two nuclei for one or more pairs of electrons.

A

covalent bond

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27
Q

within each shell, electrons are paired into orbitals with each orbital holding _____ electrons

A

two

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28
Q

two kinds of bonding

A
  1. ionic bonds
  2. covalent bonds
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29
Q

Two group = ?

A

linear (180 degrees)

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30
Q

Group VIIIA

A

noble gas

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31
Q

The best Lewis structure puts a negative charge on the?

A

most electronegative atom

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32
Q

Joining two or more elements to forms compounds.

A

bonds

33
Q

Elements in the same group have _____________________

A

similar properties

34
Q

Group VIIA

A

halogens

35
Q

Group VIA

A

chalcogens

36
Q

A _____________ results when the bonding orbitals are parallel to each other and perpendicular to the axis connecting the two bonding nuclei

A

pi (π) bond

37
Q

It is composed of negatively charged electrons

A

electron cloud

38
Q

These hybrid orbitals are called ____________ because they are formed from one s orbital and three p orbitals

A

sp3 hybrid orbitals

39
Q

Rows represent the ________

A

period

40
Q

Columns represent ________

A

groups

41
Q

Rule 1 in electron configuration

A

Aufbau principle

42
Q

atoms will give up, accept, or share electrons in order to achieve a noble gas configuration

A

Octet Rule

43
Q

A σ bond is formed by end-on overlap of?

A

two sp2 hybrid orbitals

44
Q

shells are arranged in ____________ energy

A

increasing

45
Q

Electrons have properties of both a particle and wave

A

Quantum mechanics

46
Q

It is where most of the mass of the atom is contained

A

nucleus

47
Q

> or <
interaction between parallel orbitals ____ orbitals that point at each other

A

<

48
Q

It is the probability of finding an electron at a given point in space

A

Ψ2

49
Q

These are much more common in organic chemistry than ionic bonds.

A

covalent bonds

50
Q

type of covalent bond: s-to-s, p-to-p, hybrid-to-hybrid, s-to-hybrid, etc.

A

sigma bond

51
Q

Rule 3 in electron configuration

A

Hund’s rule

52
Q

Three group = ?

A

trigonal planar (120 degrees)

53
Q

Through ____________, atoms attain a complete outer shell of valence electrons

A

bonding

54
Q

A _________________ is formed by end-on overlap of two sp2hybrid orbitals.

A

σ bond

55
Q

Group IIA

A

alkaline earth metals

56
Q

These are used to form bonds.

A

orbitals

57
Q

__________________ across a row of the periodic table as the size of the atom decreases

A

decreases

58
Q

paired electrons within an orbital have ____________ spins

A

opposite

59
Q

Gives the total energy of an electron at a given point in space (x,y,z).

A

Schrödinger wave equation (Ψ)

60
Q

A ________________ bond results when the bonding orbitals point along the axis connecting the two bonding nuclei

A

sigma (σ)

61
Q

Geometry is affected by?

A

bond length and bond angle

62
Q

four groups = ?

A

tetrahedral (109.5 degrees)

63
Q

A ___________ concentrates electron density on the axis that joins two nuclei.

A

σ bond

64
Q

A maximum of two electrons may be placed in each orbital but only when the spins of the electrons are paired.

A

Pauli exclusion principle

65
Q

It contains positively charged protons and uncharged neutrons

A

nucleus

66
Q

To summarize, a C≡C bond consists of?

A

one sigma bond and two pi bonds

67
Q

These orbitals are formed when 1 s orbital combines with 2 p orbitals

A

sp2 hybrid orbitals

68
Q

examples of more than an octet

A
  1. dimethyl sulfoxide
  2. sulfuric acid
  3. alendronic acid
69
Q

this result from the sharing of electrons between two nuclei

A

covalent bonds

70
Q

these are electrons in the outermost shell; electrons involved in bonding

A

Valence Electrons

71
Q

formula of formal charge

A

number of valence electrons - number of electrons an atom “owns” (number of unshared electrons + 1/2 of the number of shared electrons)

72
Q

The __________________ comprises most of the volume of the atom

A

electron cloud

73
Q

Group IIA

A

triels

74
Q

types of covalent bonds

A
  1. sigma bond
  2. pi bond
75
Q

type of covalent bond: either standard atomic orbitals or hybrids

A

sigma bond

76
Q

____ orbitals are not used to form the hybrid orbital

A

2p

77
Q

It is the space where an electron spends ~95% of its time.

A

orbital

78
Q

Determines the shape around any atom bonded to two other atoms.

A

Bond angle

79
Q

Distance between the nuclei of two atoms joined by a covalent bond

A

bond length

Chem 31 (12 decks)

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