Chem exam 4 Flashcards

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
Things that make something more polar
-Mainly Larger electronegativity difference -How much dipoles don't cancel out
26
Coulombs law permanent dipoles
-Larger electronegativity, stronger -Closer distance, less strong
27
Coulombs law instantaneous dipoles
-Larger molecules, bigger dipoles, stronger attraction -Closer molecules, stronger (smaller molecules can be closer together)
28
Dipole induced dipole
-Polar permanent dipole with non polar molecule
29
Miscible
-Forming a homogenous solution -Like with like -More polar with non polar= less miscible
30
Vaporization
-Liquid to gas -Endothermic
31
Condensation
-Gas to Liquid -Exothermic
32
Melting
Solid to liquid -Endothermic
33
Freezing
-Liquid to solid -Exothermic
34
Larger delta H
-Stronger interactions
35
C-C bond
350kJ
36
acetone
C3H6O
37
Methanol
CH3OH
38
Ethanol
C2H6O
39
Heating curve of water
1. Ice warming 2. Ice melting to liquid 3. Liquid water warming 4. Liquid water vaporizing 5. steam warming
40
J for water and ice
Water: 4.184 J Ice: 2.09 J