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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
Group VA
pnictogens
26
A __________________ consists of the simultaneous attraction of two nuclei for one or more pairs of electrons.
covalent bond
27
within each shell, electrons are paired into orbitals with each orbital holding _____ electrons
two
28
two kinds of bonding
1. ionic bonds 2. covalent bonds
29
Two group = ?
linear (180 degrees)
30
Group VIIIA
noble gas
31
The best Lewis structure puts a negative charge on the?
most electronegative atom
32
Joining two or more elements to forms compounds.
bonds
33
Elements in the same group have _____________________
similar properties
34
Group VIIA
halogens
35
Group VIA
chalcogens
36
A _____________ results when the bonding orbitals are parallel to each other and perpendicular to the axis connecting the two bonding nuclei
pi (π) bond
37
It is composed of negatively charged electrons
electron cloud
38
These hybrid orbitals are called ____________ because they are formed from one s orbital and three p orbitals
sp3 hybrid orbitals
39
Rows represent the ________
period
40
Columns represent ________
groups
41
Rule 1 in electron configuration
Aufbau principle
42
atoms will give up, accept, or share electrons in order to achieve a noble gas configuration
Octet Rule
43
A σ bond is formed by end-on overlap of?
two sp2 hybrid orbitals
44
shells are arranged in ____________ energy
increasing
45
Electrons have properties of both a particle and wave
Quantum mechanics
46
It is where most of the mass of the atom is contained
nucleus
47
> or < interaction between parallel orbitals ____ orbitals that point at each other
<
48
It is the probability of finding an electron at a given point in space
Ψ2
49
These are much more common in organic chemistry than ionic bonds.
covalent bonds
50
type of covalent bond: s-to-s, p-to-p, hybrid-to-hybrid, s-to-hybrid, etc.
sigma bond
51
Rule 3 in electron configuration
Hund's rule
52
Three group = ?
trigonal planar (120 degrees)
53
Through ____________, atoms attain a complete outer shell of valence electrons
bonding
54
A _________________ is formed by end-on overlap of two sp2hybrid orbitals.
σ bond
55
Group IIA
alkaline earth metals
56
These are used to form bonds.
orbitals
57
__________________ across a row of the periodic table as the size of the atom decreases
decreases
58
paired electrons within an orbital have ____________ spins
opposite
59
Gives the total energy of an electron at a given point in space (x,y,z).
Schrödinger wave equation (Ψ)
60
A ________________ bond results when the bonding orbitals point along the axis connecting the two bonding nuclei
sigma (σ)
61
Geometry is affected by?
bond length and bond angle
62
four groups = ?
tetrahedral (109.5 degrees)
63
A ___________ concentrates electron density on the axis that joins two nuclei.
σ bond
64
A maximum of two electrons may be placed in each orbital but only when the spins of the electrons are paired.
Pauli exclusion principle
65
It contains positively charged protons and uncharged neutrons
nucleus
66
To summarize, a C≡C bond consists of?
one sigma bond and two pi bonds
67
These orbitals are formed when 1 s orbital combines with 2 p orbitals
sp2 hybrid orbitals
68
examples of more than an octet
1. dimethyl sulfoxide 2. sulfuric acid 3. alendronic acid
69
this result from the sharing of electrons between two nuclei
covalent bonds
70
these are electrons in the outermost shell; electrons involved in bonding
Valence Electrons
71
formula of formal charge
number of valence electrons - number of electrons an atom "owns" (number of unshared electrons + 1/2 of the number of shared electrons)
72
The __________________ comprises most of the volume of the atom
electron cloud
73
Group IIA
triels
74
types of covalent bonds
1. sigma bond 2. pi bond
75
type of covalent bond: either standard atomic orbitals or hybrids
sigma bond
76
____ orbitals are not used to form the hybrid orbital
2p
77
It is the space where an electron spends ~95% of its time.
orbital
78
Determines the shape around any atom bonded to two other atoms.
Bond angle
79
Distance between the nuclei of two atoms joined by a covalent bond
bond length

Chem 31 (22 decks)

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