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Chem > Chapter 4; Molecular Geometry, Polarity, And Intermolecular Forces Of Attraction > Flashcards

Chapter 4; Molecular Geometry, Polarity, And Intermolecular Forces Of Attraction Flashcards

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1
Q

what is electron geometry

A

relative position of the groups of electrons on the central atom

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2
Q

what groups does the electron geometry include

A

single bond
double bond
a triple bond
a nonbonding pair

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3
Q

what is molecular geometry

A

relative position of the atoms in a molecule; determine by the electron geometry

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4
Q

what does the VSEPR theory predict about groups of electrons

A

predicts that groups of electrons on the central atom are oriented to maximize distance between them

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5
Q

depending on the number of groups of electrons what are main three names

A

two groups; linear
three groups; trigonal planar
four groups; tetrahedral

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6
Q

what are the angles for a linear, trigonal planar, and tetrahedral group

A

linear - 180
trigonal planar - 120
tetrahedral - 109.5

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7
Q

what is molecular geometry determined by

A

based on the number of bonding versus nonbonding groups on the central atom

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8
Q

what is the electron and molecular geometry for 2 electron groups

A

electron - linear
molecular - linear

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9
Q

what is the electron and molecular geometry for 3 electron groups

A

electron - trigonal planar
molecular - trigonal or bent (2 bonding and 1 nonbonding group)

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10
Q

what is the electron and molecular geometry for 4 electron groups

A

electron - tetrahedral
molecular - tetrahedral, trigonal pyramidal (3 bonding and 1 nonbonding groups), or bent (2 bonding and 2 nonbonding groups)

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11
Q

how to find a molecular bond angle

A

angle (0 - 360)

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12
Q

what is molecular polarity

A
  • determines how molecules interact with each other at the molecular level
  • molecular level interactions determine their macroscopic properties
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13
Q

what is a covalent bond

A

two atoms sharing valence electrons

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14
Q

is sharing valence electrons always equal in covalent bonds

A

no; one atoms may attract the electrons in a bond more closely towards it nucleus

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15
Q

what is electronegativity

A

ability of an atom, when part of a covalent bond, to draw electrons towards its nucleus

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16
Q

as the atomic # increases what happens to the protons and electrons

A

atomic # increases = more protons in atoms = attract electrons

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17
Q

what does negativity attract.
what does positive attract

A

negative attracts positive
positive attracts negative

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18
Q

in the periodic table which ways does electronegativity increase in the periodic table

A

down to up
left to right

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19
Q

when increasing electronegativity do the atoms get smaller or bigger

A

smaller
as go down a group it adds energy levels, so the electron cloud gets bigger = further away the less get pulled to nucleus

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20
Q

what determines if a bond is polar or non polar

A

electronegativity differences

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21
Q

in an electron density diagram that shows polar and non polar molecules, what color is high density

A

red

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22
Q

in an electron density diagram that shows polar and no polar molecules what color is low density

A

blue

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23
Q

in an electron density diagram that shows polar and non polar molecules, what color is neutral

A

green to yellow

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24
Q

atom with a greater electron density has a partial negative charge

A

s^-

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25
Q

atom with a lesser electron density has a partial positive charge

A

s^+

26
Q

what is a dipole

A

separation of partial charges

27
Q

what type of covalent bonds are used with dipoles

A

polar bonds

28
Q

what are some facts about non polar bonds regarding electronegativity

A
  • form between atoms of similar electronegativity
  • even electron distribution
  • no partial charges or dipoles
29
Q

if there is a electronegativity difference of 0.5 and less (x<0.5) what does this make it

A

non polar covalent bond

30
Q

if there is an electronegativity difference of greater than 0.5 and less than 2.0 (0.5<x>2.0), what does this make it</x>

A

polar covalent bond

31
Q

if there is an electronegativity difference of greater than 2.0 (x>2.0), what does this make it

A

ionic bond

32
Q

can entire molecules be polar and non polar

A

yes

33
Q

how can entire molecules be polar or nonpolar

A

polar molecules have overall charge separation
non polar molecule have even distribution of electros
- side note; polar and non polar molecules have very different physical and chemical properties

34
Q

a non polar molecule can be a molecular with all […] bonds, or a molecule with […] geometry and […] polar bonds/bond dipoles

A

non polar
symmetrical
identical

35
Q

non polar molecules with non polar bonds

A

hydrocarbon compounds
diatomic elements

36
Q

non polar molecules with polar bonds

A
  • identical polar bonds in symmetrical molecules
  • bond dipoles cancel
  • three symmetrical shapes; linear, trigonal planar and tetrahedral
37
Q

a molecule is non polar if
1. all the bonds are […] or
2. the […] geometry is […] (the central atom has no nonbonding electrons) AND all the bonds are […}

A

nonpolar
molecular
symmetrical

38
Q

a polar molecule can be
- a molecule with one […] bond
- a molecule with […] molecular geometry and more than […] polar bond
- a molecule with […] molecular geometry and nonidentical polar bonds

A

polar
nonsymmetrical
one
symmetrical

39
Q

what is a covalent bond

A

result of intramolecular forces of attraction

40
Q

what are intermolecular forces of attraction

A

attractions between molecules in liquid and solid states

41
Q

intermolecular bonds are weaker than

A

covalent bonds

42
Q

intermolecular and intermolecular forces of attraction determine […] properties of a compound; […],[…],[…]

A

physical
boiling point
melting point
solubility

43
Q

do polar molecules have permanent or temporary dipoles

A

permanent

44
Q

do non polar molecules have permanent or temporary dimples

A

can form temporary

45
Q

intermolecular forces of attraction form between a […] charge on one molecule and the […] partial charge on another

A

partial
opposite

46
Q

what is the order of the types of intermolecular forces of attraction from weakest to strongest

A

dispersion forces (or London forces)
dipole - dipole forces
hydrogen bonding

47
Q

dispersion forces - or London forces are…

A
  • common to all compounds and elements
  • also called London forces
  • weakest intermolecular force of attraction and * only one available for non polar compounds *
48
Q

how does a dispersion force form

A

electrons in a non polar compound may shift, forming a temporary dipole
- temporary dimple induces another temporary dipole in a nearby molecule
- weak attraction between temporary dipole and induced dipole = dispersion force

49
Q

compounds with larger molecules have […] dispersion forces than compounds with smaller molecules

A

stronger
propane (C3H8) > methane (CH4)
(more opportunities for electrons to shift)

50
Q

elements with larger atoms have […] dispersion forces than elements with smaller molecules

A

Iodine (I2) > fluorine (F2)

51
Q

dispersion forces are (core concept)

A
  • the only forces of attraction in elements and non polar compounds
  • dispersion forces result from induced temporary dipoles
52
Q

what are dipole dipole forces

A
  • form between oppositely charged ends of polar molecules
  • form between permanent dipoles
  • are stronger than dispersion forces
53
Q

dipole dipole intermolecular forces …

A
  • exist between polar molecules that have a permanent dipole
  • they are stronger than dispersion forces
54
Q

hydrogen bonding forces are dipole dipole forces between molecules with […] bond dipoles, which are

A

H-F
H-O
H-N
form between the partial positive pole of one molecule (H) and partial negative pole of another (F, O, N)

55
Q

how to depict a hydrogen bonding force

A

use dotted line between H (one molecule) and N,O, or F (another molecule) or dashes
e.g. H-F …. H-F
there is donor and receptor

56
Q

how to determine the strongest intermolecular force of attraction

A

are polar molecules present
no - dispersion force
yes = are H-O H-N or H-F bonds present
no - dipole dipole forces
yes - hydrogen bonding forces
side note;
in a molecule with hydrogen bonding forces can also have dispersion forces

57
Q

what are the intermolecular forces of molecules that are bonded to H such as F, O, N

A

hydrogen bonding

58
Q

what are the intermolecular forces of attraction of molecules that are polar

A
  • dipole dipole
  • London dispersion forces
59
Q

what are the intermolecular forces of attraction in molecules that are non polar
side note; molecules that contain only C and H are non polar

A

London dispersion forces

60
Q
A

Chem (10 decks)

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