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Chemistry 1220 > Exam 1 > Flashcards

Exam 1 Flashcards

ch 10, 11

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1
Q

What are the 3 main types of IMFs?

A

London forces, dipole-dipole, hydrogen bonding

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2
Q

Electrostatic attractions between + and - charges

A

Intermolecular Forces (IMFs)

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3
Q

All matter meets the requirements for attraction due to temporary dipoles
Stronger the more massive the particle/molecule and the greater its surface area

A

London Forces

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4
Q

Requires polar molecules with permanent dipoles

The more polar the molecule, the stronger this force is

A

Dipole-Dipole

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5
Q

Requires a grouping within the molecule of O–H, N–H, or F–H and available nonbonding/lone pair electrons on the other molecule
O–H is more electronegative than N–H

A

Hydrogen Bonding

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6
Q

Requires ions and polar (solvent) molecules

A

Ion-Dipole Forces

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7
Q

The ability of atoms in a molecule to attract bonding electrons to themselves

A

Electronegativity

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8
Q

Results from the relative positions of the actual bonds between atoms within the electronic geometry

A

Molecular Geometry

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9
Q

Extended networks of atoms held together by metallic bonding (Cu, Fe)

A

Metallic Solids

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10
Q

Extended networks of ions held together by ion-ion interactions (NaCl, MgO)

A

Ionic Solids

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11
Q

Extended network of atoms held together by covalent bonds (C, Si)

A

Covalent Network Solids

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12
Q

Ions are mobile in solution

A

Electrolytes

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13
Q

Homogeneous mixtures on a molecular level

A

Solutions

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14
Q

Component that determines the phase of the solution

-Usually present in the largest quantity

A

Solvent

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15
Q

Material(s) that is/are dissolved

A

Solute

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16
Q

(mass of component/total mass of sol’n)(100/1)

A

Mass Percent

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17
Q

moles of desired component/total moles

A

Mole Fraction

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18
Q

moles solute/L solution

A

Molarity

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19
Q

moles solute/kg solvent

A

Molality

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20
Q

The limit of solute that will dissolve in a solvent has been reached, no more added solute will dissolve

A

Saturated Solution

21
Q

Holds more solute than required for a saturated solution, these are unstable

A

Supersaturated Solution

22
Q

Occurs when industrial users take water from a river or lake, and return it (no matter how clean) at a higher temperature

A

Thermal Pollution

23
Q

(constant given for gas M/atm)(partial pressure of same gas above the solution atm)

A

Henry’s Law, solubility of gas in solution (M)

24
Q

Physical properties of solutions that depend only on the number of solute particles in solution, not on their nature (vapor pressure and freezing point depression, boiling point elevation, osmotic pressure)

A

Colligative Properties

25
Q

The pressure exerted by a vapor in equilibrium with the liquid phase

A

Vapor Pressure

26
Q

When we add a non-volatile solute to a solvent, we see a ?? of the vapor pressure, since we have effectively decreased the fraction of molecules in the entire sample with any “escaping ability”

A

lowering/depression

27
Q

(mole fraction)(vapor pressure of pure solvent solution at a given temp)

A

Vapor pressure of solution, Raoult’s Law

28
Q

Method: boil mixture, collect vapor, condense it

A

Distillation

29
Q

(boiling point elevation constant)(solute molality)

A

Boiling Point Elevation

30
Q

(freezing point depression constant for solvent)(molality)

A

Freezing Point Depression

31
Q

The net movement of water molecules from the less concentrated solution towards the more concentrated solution

A

Osmosis

32
Q

The pressure required to stop osmosis between a pure solvent and a solution

A

Osmotic Pressure

33
Q

(M)(0.0821Latmmol^-1K^-1)(temp in kelvins)

A

Osmotic Pressure

34
Q

The ratio of the actual value of a colligative property to the value calculated, assuming the substance to be a nonelectrolyte

A

Van’t Hoff Factor

35
Q

Suspensions of particles larger than individual ions or molecules, but too small to settle out by gravity (ie: snowglobe)

A

Colloids

36
Q

Colloidal suspensions can scatter rays of light

A

Tyndall Effect

37
Q

if plot of 1/[A] vs t, linear, slope=k

A

Second Order

38
Q

if plot of ln[A] vs t, linear, slope=-k

A

First Order

39
Q

if plot of [A] vs t, linear, slope=k

A

Zero Order

40
Q

The rate constant; it is the proportionality constant between reaction rate and reactant concentration

A

k

41
Q

A mathematical statement of the way in which rate changes with changing concentration of reactants

A

Rate Law

42
Q

Usual units for rate?

A

Ms^-1

43
Q

The order to determine rates of reactions, we need to be able to measure ?,as they are changing

A

concentrations

44
Q

The change in concentration of reactants or products with time

A

Reaction Rate

45
Q

What are the 4 factors that influence the rates of chemical reactions?

A
  1. Nature of the products and reactants
  2. Temperature
  3. Other agents and catalysts
  4. Concentration of the reactants
46
Q

Reaction rate depends on what 3 things?

A

Collision frequency, collision energy, collision orientation

47
Q

The constants Kb and Kf, related to freezing point depression and boiling point elevation, are properties of: a. solutions

b. solvents
c. solutes
d. solids

A

b. solvents

48
Q

Which does not favor solubility of a solid solute in a liquid solvent?

a. weak solute-solute interactions
b. strong solute-solvent interactions
c. increase in disorder of the system
d. covalent network bonding in solute
e. solution lower in energy that solute and solvent

A

d. covalent network bonding in solute

Chemistry 1220 (2 decks)

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