Exam 1

Question 1

What are the 3 main types of IMFs?

Answer 1

London forces, dipole-dipole, hydrogen bonding

Question 2

Electrostatic attractions between + and - charges

Answer 2

Intermolecular Forces (IMFs)

Question 3

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

Answer 3

London Forces

Question 4

Requires polar molecules with permanent dipoles

The more polar the molecule, the stronger this force is

Answer 4

Dipole-Dipole

Question 5

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

Answer 5

Hydrogen Bonding

Question 6

Requires ions and polar (solvent) molecules

Answer 6

Ion-Dipole Forces

Question 7

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

Answer 7

Electronegativity

Question 8

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

Answer 8

Molecular Geometry

Question 9

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

Answer 9

Metallic Solids

Question 10

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

Answer 10

Ionic Solids

Question 11

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

Answer 11

Covalent Network Solids

Question 12

Ions are mobile in solution

Answer 12

Electrolytes

Question 13

Homogeneous mixtures on a molecular level

Answer 13

Solutions

Question 14

Component that determines the phase of the solution

-Usually present in the largest quantity

Answer 14

Solvent

Question 15

Material(s) that is/are dissolved

Answer 15

Solute

Question 16

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

Answer 16

Mass Percent

Question 17

moles of desired component/total moles

Answer 17

Mole Fraction

Question 18

moles solute/L solution

Answer 18

Molarity

Question 19

moles solute/kg solvent

Answer 19

Molality

Question 20

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

Answer 20

Saturated Solution

Question 21

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

Answer 21

Supersaturated Solution

Question 22

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

Answer 22

Thermal Pollution

Question 23

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

Answer 23

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

Question 24

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)

Answer 24

Colligative Properties

Question 25

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

Answer 25

Vapor Pressure

Question 26

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"

Answer 26

lowering/depression

Question 27

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

Answer 27

Vapor pressure of solution, Raoult's Law

Question 28

Method: boil mixture, collect vapor, condense it

Answer 28

Distillation

Question 29

(boiling point elevation constant)(solute molality)

Answer 29

Boiling Point Elevation

Question 30

(freezing point depression constant for solvent)(molality)

Answer 30

Freezing Point Depression

Question 31

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

Answer 31

Osmosis

Question 32

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

Answer 32

Osmotic Pressure

Question 33

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

Answer 33

Osmotic Pressure

Question 34

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

Answer 34

Van't Hoff Factor

Question 35

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

Answer 35

Colloids

Question 36

Colloidal suspensions can scatter rays of light

Answer 36

Tyndall Effect

Question 37

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

Answer 37

Second Order

Question 38

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

Answer 38

First Order

Question 39

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

Answer 39

Zero Order

Question 40

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

Answer 40

k

Question 41

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

Answer 41

Rate Law

Question 42

Usual units for rate?

Answer 42

Ms^-1

Question 43

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

Answer 43

concentrations

Question 44

The change in concentration of reactants or products with time

Answer 44

Reaction Rate

Question 45

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

Answer 45

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

Question 46

Reaction rate depends on what 3 things?

Answer 46

Collision frequency, collision energy, collision orientation

Question 47

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

Answer 47

b. solvents

Question 48

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

Answer 48

d. covalent network bonding in solute