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General Chemistry > Chapter 8 > Flashcards

Chapter 8 Flashcards

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1
Q

What is the difference between trigonal planar and trigonal pyramidal

A

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

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2
Q

what group tends to have trigonal planar arrangements

A

group 3

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3
Q

what group tend to have trigonal bipyramidal arrangements

A

group 5

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4
Q

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

A

tetrahedral

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5
Q

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

A

trigonal planar

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6
Q

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

A

linear

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7
Q

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

A

trigonal bipyramidal

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8
Q

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

A

octahedral

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9
Q

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

A

linear

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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

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11
Q

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

A

trigonal planar

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12
Q

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

A

angular/bent

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13
Q

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

A

tetrahedral

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14
Q

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

A

trigonal pyramidal

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15
Q

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

A

angular/bent

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16
Q

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

A

trigonal bipyramidal

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17
Q

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

A

irregular tetrahedral/see-saw

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18
Q

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

A

T-shaped

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19
Q

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

A

linear

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20
Q

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

A

octahedral

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21
Q

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

A

square pyramidal

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22
Q

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

A

square planar

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23
Q

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

A

180 degrees

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24
Q

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

A

120 degrees

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25
Q

What is the bond angle between 4 e- pairs in a tetrahedral arrangement?

A

109.5 degrees

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26
Q

What is the bond angle between 5 e- pairs in a trigonal bipyramidal arrangement?

A

90 degrees between the vertical and horizontal plane
120 degrees between the electrons in the horizontal plane

27
Q

What is the bond angle between 6 e- pairs in an octahedral arrangement?

A

90 degrees between all pairs

28
Q

What is the bond angle in a water molecule

A

104.5 degrees

29
Q

how does the bond angle change in a molecule with lone pairs and why?

A

the angle of the respective electron arrangement reduces since lone pairs require more space

30
Q

Define chemical bond

A

the strong attractive force between certain atoms in a substance

31
Q

Whats the difference between an ionic and covalent bond

A

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
Q

Define bonding pair

A

electron pair between two atoms, represented by one line

33
Q

Define lone pair

A

electron pair that are nonbonding

34
Q

What rule do atoms obey when forming bonds and why

A

atoms except hydrogen ten toward the octet rule to become more stable

35
Q

Define polar covalent bond

A

unequal sharing of electrons between atoms in molecule=charge separation in bond charge
oriented towards an electric field

36
Q

Define electronegativity

A

measure of the ability of an atom to draw bonding electrons to itself

37
Q

What characteristic is related to electronegativity

A

ionization energy and electron affinity

38
Q

Define polar bond

A

covalent bond where bonding electrons spend more time near one atom than near the other atom

39
Q

How does electronegativity increase and why

A

it increases from left to right and bottom to top

40
Q

what elements are the most electronegative

A

F, O, N, and CL

41
Q

What’s the link between polarity and electronegativity? what does it represent

A

the difference between 2 atoms in a bond = measure of bond polarity
large difference= ionic or polar bond
small difference= nonpolar bond

42
Q

Define Dipole moment

A

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
Q

what do vectors that cancel out mean

A

no net dipole moment

44
Q

Are bonds more polar when parallel or perpendicular to the trend

A

Parallel

45
Q

How does an anion compare to its parent atom and why?

A

Anion is bigger since e- is added

46
Q

How does a cation compare to its parent atom and why?

A

Cation is smaller, since removal e-

47
Q

What’s an Isoelectronic series

A

Serie of ions or atoms containing the same number of electrons

48
Q

How do you determine the central atom

A

least electronegative atom is central atom
H\F are never central atoms

49
Q

what are the exceptions to the octet rule

A

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
Q

what conditions need to be respected when distributing the remaining electrons?

A

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
Q

Why cant element of the second period expand their octet

A

they only have s and p orbitals= can’t expand their electron configuration

52
Q

What do we call more than one valid Lewis structure that can be written for a molecule

A

resonance structures

53
Q

How can you obtain the hypothetical charge of an atom

A

with equation: F=V-B/2-L

54
Q

How can a molecule be more stable

A

when all formal charges are similar

55
Q

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.

A

true

56
Q

Why can e- move around a molecule

A

they’re delocalized

57
Q

Are noble gases electronegative?

A

No

58
Q

What does VSEPR stand for ?

A

Valence Shell Electron Pair Repulsion

59
Q

what are the rules when assigning the formal charges

A

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
Q

what molecular arrangement give molecules no net dipole and why is that

A

linear/ trigonal planar/ tetrahedral
all vectors cancel eachother out

61
Q

how to achieve a stable compound

A

make sure that atleast one atom has a noble gas electronic configuration.

62
Q

whats the trend is ion sizes

A

for metal: bigger down a group and smaller in a period
for non metals: bigger both ways since add electrons

63
Q

explain the localized electron model

A

electron pairs are localized on aparticular atom aka central atom

64
Q
A

General Chemistry (9 decks)

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