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Chem > Ch 10,11 > Flashcards

Ch 10,11 Flashcards

0
Q

Order of intermolecular forces from lowest to highest

A

London dispersion
Dipole dipole
Hydrogen bonding between H and N,F, and O
Ionic

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1
Q

Definition of Electronegativity

A

Tendency to attract the electrons in a bond.
Pauling
Fluorine is most electronegative

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2
Q

Nonpolar Definition

Polar Definition

A
  • Cancel to zero
  • Doesn’t cancel

Opposite signs attract. Same signs repel. It will turn away until the positive end touches the negative end.

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3
Q

Intramolecular force

Intermolecular force

A

-

-Between molecules

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4
Q

Boiling Points

A

Increase as you go down the periodic table.

Stronger forces have higher boiling points.

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5
Q

Freezing points

A

Aka

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6
Q

Crystalline solids

A

When water crystallize into I’ve they pack into a crystal, honeycomb shaped structure.

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7
Q

Weak force can liquefy noble gases

A

.

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8
Q

Amorphous Solids

A

Atoms aren’t arranged in 3d array.

Ex. Glass plastics rubber

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9
Q

Crystalline

A

Lattice

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10
Q

Three types of cubic atoms

A

Simple 1 atom
Body centered 2 atoms
Face centered 4 atoms Ex. Cu

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11
Q

Waves curve at the same place to

If they don’t curve in the same place to

A

They become constructive, additive.

They become destructive.

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12
Q

Bragg Construction Equation

A

N(wavelength)= 2d(sin theta)

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13
Q

What is the Coordination number?

A

The number of atoms am atom touches

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14
Q

What type of atom has the higher coordination number?

A

Closest packing

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15
Q

Body
Face
Edge
Corner

A

1 atoms mass worth
1/2
1/4
1/8

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16
Q

X ray diffraction

A

.

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17
Q

Vapor Pressure

A

If the h20 molecules posses enough energy they will cut through the surface to the vapor.
H2o molecules are attracted everywhere but the top.

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18
Q

Exothermic

Endothermic

A

Produces heat it has a negative delta h

Produces her it has a positive delta h

19
Q

Rate of evaporation

Rate of condensation

A

Proportional to surface area

Changes. Depends on particles

20
Q

Equilibrium

A

At equilibrium the rate of condensation equals the rate of evaporation. After that there is no more change

21
Q

Equilibrium of vapor pressure

A

0 degrees ice is 4.6 pressure

100 degress 760 hg pressure

22
Q

How do you tell which molecule has a higher or lower vapor pressure

A

Stronger forces a molecule has, the harder it is to pull apart delta h increases

23
Q

Is vapor pressure a linear or exponential relationship?

A

Exponential. It curves
Temp increases pressure increases.
Delta h increases pressure decreases.
RT gets bigger delta g gets smaller making it less negative

24
Q

Clausius claperyon equation

A

Ln(p1/p2)= delta h/r (1/t2-1/t1)

25
Q

What is an example of a phase change? What stays the same during this change?

A

Ice to water.

Temperature

26
Q

Know the phase change diagram and formulas

A

.

27
Q

Solution definition

A

Something dissolved in something else

28
Q

Concentration diagram

A

.

29
Q

Molar solubility

Gram solubility

A

Mol solute/ l solution

Grams solute/ 100 g solution

30
Q

Molarity formula

A

Moles of solute/ liters of solution

31
Q

Molality formula

A

Moles of solute/ kg solvent (mass)

32
Q

Mass percent formula

A

Mass solute/ mass solution x 100

33
Q

Mass fraction

A

.

34
Q

Mole fraction formula (chi)

A

Moles solute/ moles total

35
Q

Collegiate properties

A

.

36
Q

Boiling point elevation equation

Freezing point depression equation

A

Delta t = kb m

Delta t= kf m

37
Q

Osmotic pressure

A

Net flow into the more concentrate solution. Raising the level

38
Q

Normality equation

A

Equivalence/ liter of solution

39
Q

MM = nEM

A

.

40
Q

Solution energetics

A

.

41
Q

Vapor pressure of solution equation

A

Delta p= chi solvent + pure solvent

Psolv= chi solv x pure solvent

42
Q

Molar mass equation

A

Mass(g) / n(moles)

43
Q

Raoults law

A

P= XaPa + XbPb

44
Q

Osmotic pressure equation

A

Pi = MRT

45
Q

Types of crystalline solids

A

Ionic
Molecular
Atomic (metallic and nonmetal) also group a

Chem (5 decks)

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