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chemistry 190 > Chapter 7 > Flashcards

Chapter 7 Flashcards

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AP® Chemistry flashcards Periodic Table flashcards
1
Q

VSPER

A

says electrons want to get as far away from each other in a 3D space

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2
Q

Axn

A

A is central atom, x is # of electron pairs, n positive whole numbers

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3
Q

highly symmetric molecule

A

every angle is the same

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4
Q

electron domain geometry

A

describes only the positions of bonding pairs.

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5
Q

molecular geometry

A

describes positions of all electron pairs.

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6
Q

5 electron domain geometries

A 
linear, 2 terminal atoms
trigonal planar, three terminal atoms
tetrahedral: 4 terminal atoms
trigonal bipyramidal: 5 terminal atoms
octahedral: 6 terminal atoms
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7
Q

which electron-domain geometry does not exhibit high symmetry

A

trigonal bipyramidal

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8
Q

angle in linear electron domain

A

180

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9
Q

angle in trigonal planar geometry

A

120

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10
Q

angle in tetrahedral geometry

A

109.5

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11
Q

angles in trigonal bipyramidal geometry

A

90 (b/w top and middle) and 120 (b/w 2 middle atoms)

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12
Q

angle in octahedral geometry

A

octahedral

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13
Q

2 bonded pairs molecular geometry

A

linear

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14
Q

2 BP 1 LP mol. geometry

A

bent

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15
Q

2 BP 1 LP mol. geo.

A

bent

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16
Q

2 BP 3 LP molecular geo.

A

linear

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17
Q

3 BP molecular geometry

A

trigonal planar

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18
Q

3 BP 1 LP mol. geometry

A

trigonal pyramidal

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19
Q

3 BP 2 LP mol. geometry

A

t-shaped

20
Q

4 BP mol. geometry

A

tetrahedral

21
Q

4 BP 1 LP mol. geometry

A

seesaw

22
Q

4 BP 2 LP mol. geometry

A

square planar

23
Q

5 BP mol. geometry

A

trigonal bipyramidal

24
Q

5 BP 1 LP mol. geometry

A

square pyramidal

25
Q

6 BP mol. geometry

A

octahedral

26
Q

why are multiple bonds counted as single pairs?

A

there is only 1 sigma bond in a 2 or 3 pair.

27
Q

sigma bond

A

formed by head-on-head overlap. represent single bonds. Only one in double and triple bonds.

28
Q

pi bonds

A

formed by side-to-side overlap. 1 in double bonds and 2 in triple bonds

29
Q

polarity criteria

A
  1. must have polar bonds

2. the overall dipole is the vector sum of individual dipoles (so if they cancel, they are not polar)

30
Q

molecules that are usually polar

A

non-symmetric molecules and when there is the presence of at least one lone pair.

31
Q

types of intermolecular forces

A

dispersion, dipole-dipole, hydrogen bonding, ion-dipole interaction

32
Q

ion-dipole interaction

A

happens when there is an ion and a polar substance

33
Q

dispersion forces

A

happen in everything

34
Q

hydrogen bonding

A

occur when H is paired with a highly electronegative element (N, O, F) that has at least one lone pair.

35
Q

dipole-dipole

A

occurs when a polar molecule interacts with another polar molecule

36
Q

what causes nitrogen (a non-polar gas) to become liquid when temp. drops

A

dispersion forces, heavier things are harder to turn into a gas

37
Q

low boiling point corresponds with what kind of dipole moments?

A

low dipole moments, and weak attractions

38
Q

valence bond theory

A

atoms share electrons when an atomic orbital on one atom overlaps with an atomic orbital on another. It balances electron attraction with repulsion from protons.

39
Q

according to valence bond theory, how many bonds would you expect an oxygen atom to form

A

2

40
Q

problems with valence bond theory

A

simple diatomic molecules are the only things that can be explained by VB theory. (# of orbitals and degrees do not match p)

41
Q

hybridization

A

using atomic orbitals in a combination to form hybrid orbitals that have correct geometry to explain bonding in larger molecules.

42
Q

tetrahedral (4 bonds) electron domain hybridization

A

sp3

43
Q

trigonal planar (3 bonds) electron domain hybridization

A

sp2

44
Q

linear (2 bonds) electron domain hybridization

A

sp

45
Q

trigonal bipyramidal (5 bonds) electron domain hybridization

A

sp3d

46
Q

octahedral (6 bonds) electron domain hybridization

A

sp3d2

47
Q

is it possible to hybridize just part of the atomic orbitals

A

yes

chemistry 190 (5 decks)

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