Chapter 8 Flashcards

1
Q

What is the difference between trigonal planar and trigonal pyramidal

A

trigonal planar doesn’t have lone pairs on the central atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

what group tends to have trigonal planar arrangements

A

group 3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what group tend to have trigonal bipyramidal arrangements

A

group 5

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is the electron arrangement of a molecule with 4 e- pairs around the central atom

A

tetrahedral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is the electron arrangement
of a molecule with 3 e- pairs around the central atom

A

trigonal planar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is the electron arrangement
of a molecule with 2 e- pairs around the central atom

A

linear

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is the electron arrangement
of a molecule with 5 e- pairs around the central atom

A

trigonal bipyramidal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is the electron arrangement
of a molecule with 6 e- pairs around the central atom

A

octahedral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Geometric arrangement of a molecule with 2 sigma bonds and no lone pair

A

linear

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Why are double and triple bonds considered as one in the VSPER theory

A

Only sigma bonds are considered and there’s only on in each multiple pair; the other bonds are pi bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Geometric arrangement of a molecule with 3 sigma bonds and 0 lone pairs

A

trigonal planar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Geometric arrangement of a molecule with 2 sigma bonds and 1 lone pair

A

angular/bent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Geometric arrangement of a molecule with 4 sigma bonds and 0 lone pair

A

tetrahedral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Geometric arrangement of a molecule with 3 sigma bonds and 1 lone pair

A

trigonal pyramidal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Geometric arrangement of a molecule with 2 sigma bonds and 2 lone pairs

A

angular/bent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Geometric arrangement of a molecule with 5 sigma bonds and 0 lone pair

A

trigonal bipyramidal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Geometric arrangement of a molecule with 4 sigma bonds and 1 lone pair

A

irregular tetrahedral/see-saw

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Geometric arrangement of a molecule with 3 sigma bonds and 2 lone pair

A

T-shaped

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Geometric arrangement of a molecule with 2 sigma bonds and 3 lone pair

A

linear

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Geometric arrangement of a molecule with 6 sigma bonds and 0 lone pair

A

octahedral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Geometric arrangement of a molecule with 5 sigma bonds and 1 lone pair

A

square pyramidal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Geometric arrangement of a molecule with 4 sigma bonds and 2 lone pair

A

square planar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What is the bond angle between 2 e- pairs in a linear arrangement?

A

180 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What is the bond angle between 3 e- pairs in a trigonal planar arrangement?

A

120 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
What is the bond angle between 4 e- pairs in a tetrahedral arrangement?
109.5 degrees
26
What is the bond angle between 5 e- pairs in a trigonal bipyramidal arrangement?
90 degrees between the vertical and horizontal plane 120 degrees between the electrons in the horizontal plane
27
What is the bond angle between 6 e- pairs in an octahedral arrangement?
90 degrees between all pairs
28
What is the bond angle in a water molecule
104.5 degrees
29
how does the bond angle change in a molecule with lone pairs and why?
the angle of the respective electron arrangement reduces since lone pairs require more space
30
Define chemical bond
the strong attractive force between certain atoms in a substance
31
Whats the difference between an ionic and covalent bond
ionic bonds are formed by a transfer of e- in a cation and anion in a molecule. A covalent bond is formed by sharing a pair of e-
32
Define bonding pair
electron pair between two atoms, represented by one line
33
Define lone pair
electron pair that are nonbonding
34
What rule do atoms obey when forming bonds and why
atoms except hydrogen ten toward the octet rule to become more stable
35
Define polar covalent bond
unequal sharing of electrons between atoms in molecule=charge separation in bond charge oriented towards an electric field
36
Define electronegativity
measure of the ability of an atom to draw bonding electrons to itself
37
What characteristic is related to electronegativity
ionization energy and electron affinity
38
Define polar bond
covalent bond where bonding electrons spend more time near one atom than near the other atom
39
How does electronegativity increase and why
it increases from left to right and bottom to top
40
what elements are the most electronegative
F, O, N, and CL
41
What's the link between polarity and electronegativity? what does it represent
the difference between 2 atoms in a bond = measure of bond polarity large difference= ionic or polar bond small difference= nonpolar bond
42
Define Dipole moment
A molecule whose charge can be represented by center positive and center negative, where a net vector is present positive center is least electronegative while negative is most electronegative
43
what do vectors that cancel out mean
no net dipole moment
44
Are bonds more polar when parallel or perpendicular to the trend
Parallel
45
How does an anion compare to its parent atom and why?
Anion is bigger since e- is added
46
How does a cation compare to its parent atom and why?
Cation is smaller, since removal e-
47
What's an Isoelectronic series
Serie of ions or atoms containing the same number of electrons
48
How do you determine the central atom
least electronegative atom is central atom H\F are never central atoms
49
what are the exceptions to the octet rule
H has 1 e- pair C, O, N, F have 4 e- pairs Be has 2 e- pairs B, Al, Sn have 3 e- pairs
50
what conditions need to be respected when distributing the remaining electrons?
H is always surrounded by 2 electrons Be is always surrounded by 4 e- B is always surrounded by 6 e- C, O, N, F are always surrounded by 8 e- other atoms can have 8 or more e-
51
Why cant element of the second period expand their octet
they only have s and p orbitals= can't expand their electron configuration
52
What do we call more than one valid Lewis structure that can be written for a molecule
resonance structures
53
How can you obtain the hypothetical charge of an atom
with equation: F=V-B/2-L
54
How can a molecule be more stable
when all formal charges are similar
55
True or False the sum of the formal charges of all atoms in a given molecule/ion must equal to overall charge on that species.
true
56
Why can e- move around a molecule
they're delocalized
57
Are noble gases electronegative?
No
58
What does VSEPR stand for ?
Valence Shell Electron Pair Repulsion
59
what are the rules when assigning the formal charges
1) all FC must be similar to have a stable compound 2) the most electronegative electrons must have the most negative FC 3) the structure with the lowest FC in magnitude must be prioritized 4) the sum of all FC must equal the charge of the species 5) FC of an atom must be as close as possible to 0
60
what molecular arrangement give molecules no net dipole and why is that
linear/ trigonal planar/ tetrahedral all vectors cancel eachother out
61
how to achieve a stable compound
make sure that atleast one atom has a noble gas electronic configuration.
62
whats the trend is ion sizes
for metal: bigger down a group and smaller in a period for non metals: bigger both ways since add electrons
63
explain the localized electron model
electron pairs are localized on aparticular atom aka central atom
64