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Chem 211 > Units 7,11 > Flashcards

Units 7,11 Flashcards

0
Q

Solute

A

Smallest quantity of solution, is dissolved

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1
Q

Solution

A

Homogeneous mixture of solute and solvent

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2
Q

Solvent

A

Greatest quantity of solution, does the dissolving

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3
Q

Solvation

A

Process of dissolving

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4
Q

Dissociation

A

Crystals of an ionic solid (salt) dissipate by action of water into the ions in which the compound is composed. NaCl—>Na+ + Cl-

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5
Q

The ___ ions of the salt are attracted to the positive H+ end of the water

A

Negative

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6
Q

Dissociation example
NaCl—->Na+ + Cl- (2 ions)

AlBr3—->Al+3 + 3Br- (4 ions)

A

Assume all salt is dissolved in water

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7
Q

Electrolytes

A

Solutes which form ions in water and will conduct electricity.

Ex: ionic salts

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8
Q

Non electrolytes

A

Do not conduct electricity because they do not form ions in solvent.

Ex: insoluble substances

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9
Q

Soluble

A

Ionic substances that form ions in solution

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10
Q

Insoluble

A

Substances that form precipitates or do not dissolve

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11
Q

Colligative properties depend

A

only on the number of solute particles, does matter what the solute is

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12
Q

Colligative-vapor pressure

A

Solutes lower the vapor pressure of a liquid solvent.

Vapor pressure-pressure of gas above its liquid in closed container

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13
Q

Colligative- boiling point elevation

A

Addition of solute ( like salt) to liquid results in elevation increase of normal boiling point

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14
Q

Boiling point is the temperature where vapor pressure is equal to

A

Atmospheric pressure

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15
Q

Colligative-Freezing point depression

A

Addition of solute to liquid which lowers the normal freezing point

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16
Q

Colligative-determining number of solute particles (n)

A

Non electrolyte n=1 (sugars)

Electrolyte n=number of ions after dissociation (salts)

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17
Q

The boiling point is ______ when the atmospheric pressure is higher

A

Higher

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18
Q

Critical temperature

A

Highest temperature possible to liquefy a gas at any pressure

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19
Q

Critical pressure

A

Pressure required to liquefy a gas at its critical temperature

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20
Q

Critical volume

A

Volume occupied by a mole of gas under its critical temperature and critical pressure

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21
Q

Water density

A

1g per mL or 1 g/cc

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22
Q

Concentration

A

Amount of solute dissolved in a measured amount of solvent

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23
Q

Dilute solutions

A

Low concentration of solute in large amount of solvent

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24
Concentrated solution
High concentration of solute in measured solvent
25
Saturated solution
Solute is in equilibrium with solvent
26
Triple point of water
All three phases can coexist
27
Most _____ compounds do not dissolve in water.they are also
Organic: decomposed by heat, slow reactions, joined by covalent bonds
28
Acetone, oil, waxes, rubber are examples of
Organic products
29
Metals, inert gases, pigments are examples of
Inorganic products
30
Prefixes of hydrocarbons: number of carbons 1-10
``` Meth Eth Prop But Pent Hex Hept Oct Non Dec ```
31
Hydrocarbon single double and triple bonds
Ane Ene Yne
32
Name this: | C-C-C assume H bonds all around
3 carbon = prop Single bonds=Ane Propane
33
Name this: | C---C-C
3 carbons=prop Triple bond=yne Propyne
34
Alkanes: formula
Single covalent bond CnH2n+2 Parrafin (wax) series
35
Alkenes
2 carbon atoms with double covalent bond. CnH2n Olefin series
36
Alkynes
2 C atoms with triple bond CnH2n-2 Acetylene series
37
Naming hydrocarbons
1) number longest continuous chain as parent chain 2) when numbering parent chain, start at end that results in lowest number 3) if alkyl group is present, indicate by number of C it's attached to and proper prefix 4) uses prefixes to indicate multiple alkyl groups 5) if diff chains name in alph order 6) straight chains can be named like n-octane
38
Alkyl halides
Include halogen. R-X. R= alkyl, X=halogen | Bromo, chloro
39
Alcohol groups
OH group, end in ol. Hydroxyl R-OH Middle or end of chain Sub OH for H, methane CH4 becomes methanol CH3OH
40
Al-deHydes
Double bonded O w/ single bonded H attached to terminal C position on parent chain. Ends in al Propanal
41
Ket-O-nes
Have double bonded O located anywhere on the chain but not on the ends (middle) End in one Butanone
42
Ester-ooate
Have double bonded O and single bonded O attached to same C in middle of chain. Named r to l and end in oate
43
CarbOXylIC ACIDS
Double bonded O and a hydroxyl group in a terminal position | End in oic acid
44
-Ethers-O
Single bonded O between 2 chains | Named alph
45
AmiNes
N in chain End in amine 1,2, or 3 chains Alph order
46
Amide-NO
Double bonded O and N group attached to C | Proteins
47
Amino acids
Contain amine and carboxylic acid
48
Isomers
Same chemical formula but different structure
49
Alka-di-enes
Contain 2 sets of double covalent bonds bt C atoms, must at least alternate. End in diene Butadiene
50
Cyclic
``` Ring of C. Prefix cyclo Cyclopropane CnH2n Not as stable ```
51
Aromatic-6
Alternating single and double bonds in 6 member C rings.
52
Reaction alkanes R+X2=
RX+HX | C-C+Cl2=C-C-Cl+HCl
53
Reactions Alkenes
Add things to double bond
54
Polymers
Repeating units of monomers
55
Intramolecular
W/in the compound Ionic-strongest, salts, opposite (electrostatic) covalent-shared e, H-H metallic-sea of electrons, Au
56
Intermolecular
Ion-dipole: ion and polar, strong but less than all intra Dipole-dipole: partial charges of polar. HCl and HCl. Weak H bond: H bonded to N, O, or F and another N,O,or F weak
57
Effervescence
Rapid release of gas (open a pop)
58
5 physical properties of liquid
``` One free surface Def volume No def shape Fluidity and diffusion Non compressible ```
59
CT of water
370 C
60
MP, FP, BP, sublimation point, condensing and evaporating
``` Mp, FP -solid and liquid in equilibrium BP-liquid and gas in equilibrium SP-solid and gas in equilibrium Condensing-gas to liquid Evaporating-liquid to gas ```
61
Hydrocarbon single O
Ether, alcohol
62
Hydrocarbon types 16
``` Alkane alkene alkyne Alkyl halides Alcohol Aldehydes Ketones Ester and ether Carboxylic acid Amine and amide Amino acid Alkadienes Cyclic Aromatic ```
63
Terminal hydrocarbons
Carboxylic | Aldehydes

Chem 211 (13 decks)

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