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chem and bio > Chem exam 4 > Flashcards

Chem exam 4 Flashcards

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1
Q

N atoms

A

Will always have a lone pari if it has 3 bonds

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2
Q

Sigma bonds

A

Head on
Single: 1
Double: 1
Triple: 1

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3
Q

Pi bonds

A

Overlapping of P orbitals
Single: 0
Double: 1
Triple: 2

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4
Q

Hybridization orbitals

A

Sp: 2 electron domain
Sp2: 3 electron domains
Sp3: 4 electron domains
Sp3d: 5 electron domains
Sp3d2: 6 electron domains

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5
Q

Valence bond theory

A

-Valence electrons reside in quantum mechanical atomic orbitals. They can be S P D F or hybridized combinations of these
-A chemical bond results from the overlap of these 2 half filled orbitals and spin pairing
-The geometry of the overlapping orbitals determines the shape of the molecule

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6
Q

Melting points

A

Stronger= higher

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7
Q

Boiling points

A

Stronger= higher

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8
Q

Vapor pressure

A

Stronger=lower

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9
Q

Viscosity

A

Stronger= higher

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10
Q

Surface tension

A

Stronger = higher

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11
Q

Boiling point physical phase

A

If boiled before 295 = gas

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12
Q

Boiling point definition

A

Temperature at which the liquids vapor pressure equals the external pressure

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13
Q

Bond polarity

A

Caused by differences in electronegativity of elements

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14
Q

Molecule polarity

A

requires bond dipoles, but also has geometric considerations

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15
Q

Dipole moment

A

-Bigger electrongativety difference =bigger dipole moment
-Farther apart = bigger dipole moment
-Tells how big the difference is

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16
Q

Net dipole moment

A

-Overall dipole moment of a molecule
-Sum of individual bond dipoles
-Vector

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17
Q

Dipole-Dipole interactions

A

-Polar
-Permanent dipole moment
-Asymmetric
-Stronger when molecules are closer and bigger difference in electronegativity

18
Q

Dispersion interactions

A

-Instant non permanent
-in everything
-constant motion
-can be temporarily asymmetric
-creates instantaneous dipole moment
-Bigger molecules = stronger dispersion forces ( more e = larger charges)

19
Q

Ion dipole forces

A

-ions and a polar molecule interacting
-Full charge atoms
-Ion dipole must compete with ion-ion to get salts to dissolve

20
Q

Hydrogen Bonding

A

-Lone pairs
-On O, N, F sometimes Cl
-H atom
-Bonded to another electronegative atom

21
Q

H bond acceptor

A

Lone pairs are connected

22
Q

H bond donor

A

The one with H

23
Q

Covalent naming

A

1- mono
2- di
3- tri
4- tetra
5- penta
6- hexa
7- hepta
8- octa
9- nona
10- deca

24
Q

How many moles of (element) are in ___ moles of (compound)

A

Atoms of element * moles they want

25
Q

Things that make something more polar

A

-Mainly Larger electronegativity difference
-How much dipoles don’t cancel out

26
Q

Coulombs law permanent dipoles

A

-Larger electronegativity, stronger
-Closer distance, less strong

27
Q

Coulombs law instantaneous dipoles

A

-Larger molecules, bigger dipoles, stronger attraction
-Closer molecules, stronger (smaller molecules can be closer together)

28
Q

Dipole induced dipole

A

-Polar permanent dipole with non polar molecule

29
Q

Miscible

A

-Forming a homogenous solution
-Like with like
-More polar with non polar= less miscible

30
Q

Vaporization

A

-Liquid to gas
-Endothermic

31
Q

Condensation

A

-Gas to Liquid
-Exothermic

32
Q

Melting

A

Solid to liquid
-Endothermic

33
Q

Freezing

A

-Liquid to solid
-Exothermic

34
Q

Larger delta H

A

-Stronger interactions

35
Q

C-C bond

A

350kJ

36
Q

acetone

A

C3H6O

37
Q

Methanol

A

CH3OH

38
Q

Ethanol

A

C2H6O

39
Q

Heating curve of water

A
  1. Ice warming
  2. Ice melting to liquid
  3. Liquid water warming
  4. Liquid water vaporizing
  5. steam warming
40
Q

J for water and ice

A

Water: 4.184 J
Ice: 2.09 J

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