Chemistry Exam 2

Front 1

Strong Acids

Back 1

HNO3 (nitric acid),
HClO4 (perchloric acid),
HCl (hydrochloric acid),
HBr (hydrobromic acid),
HI (hydroiodic acid),
H2SO4 (sulfuric acid).

Front 2

Types of Reactions:

Back 2

Precipitate
Neutralization
Combination
Decomposition
Redox

Front 3

Precipitate Reactions

Back 3

Solubility Rules on exam
two (aq) solutions combine to form a solid and an (aq) solution.
Total Ionic Equation
Net Ionic Equation

Front 4

Neutralization Reactions

Back 4

Acid- Base Reactions
hydronium ions (responsible for acidity) neutralize the hydroxide ions (responsible for basicity) to form water (a neutral compound).
Net ionic equation: H+(aq) + OH-(aq) → H2O(l)

Front 5

Combination Reactions

Back 5

two reacting elements combine to form a single product

Front 6

Decomposition Reactions

Back 6

A single reactant decomposes to form 2 or more products

Front 7

Redox Reactions

Back 7

combination reaction that involves oxidation and reduction

Front 8

Oxidation

Back 8

Loss of electrons; oxidation number increases from low number to higher number. Ex: ON goes from -2 to 0

Front 9

Reduction

Back 9

Gain of electrons; oxidation number decreases from high number to lower number. Ex: ON goes from 0 to -2

Front 10

Rules for Oxidation numbers

Back 10

Rule #1: All elements are assigned an oxidation number of zero.
Rule #2: Elements in groups IA and IIA are assigned oxidation numbers of +1 and +2, respectively.
Rule #3: In a binary ionic compound, the ON for the nonmetal is group# minus 8; for example, in KCl, the ON for chlorine is 7-8 = -1.
Rule #4: The ON for oxygen in most of its compounds is -2 (exceptions are peroxides, ON of oxygen is -1).
Rule #5: The sum of the oxidation numbers of all elements is equal to zero in a neutral compound.

Front 11

Activity Series

Back 11

spontaneity of single replacement reactions can be predicted using the activity series; Items higher on the activity series will react with those below it on the activity series.

Front 12

Diatomic Gases

Back 12

BrINClHOF
Bromine, Nitrogen, Chlorine, Hydrogen, Oxygen, Fluorine

Front 13

Boyle's Law

Back 13

VOLUME AND PRESSURE
V is inversely related to P, therefore:
V1P1=V2P2

Front 14

Charles's Law

Back 14

VOLUME AND TEMPERATURE (K)
V is directly proportional to T therefore:
V1/T1=V2/T2

Front 15

Avogadro's Law

Back 15

VOLUME AND AMOUNT OF GAS(n)
V is directly proportional to n therefore:
V1/n1=V2/n2

Front 16

Ideal Gas Equation

Back 16

PV=nRT

Front 17

Dalton's Law of Partial Pressure

Back 17

total pressure is the sum of the partial pressures of the components of the mixture;
Pt =P1 +P2 +P3 +.............

Front 18

Standard Temperature and Pressure (STP)

Back 18

0 degrees Celcius and 1 atm;
273 K and 1 atm
for 1 mol of any ideal gas at STP, V=22.4 L

Front 19

Application of Ideal Gas Law with Density

Back 19

Density = mass/volume
number of mol= mass/ Molar Mass so:
mass/volume=PM/RT

Front 20

Kinetic Molecular Theory:

Back 20

Postulates:
1)Gas particles in constant, random, straight-line motion except during collisions
2)colliding molecules exchange energy but do not lose any through friction (total KE is constant)
3)Particle volume << container volume; particles considered as point masses

Front 21

Average Kinetic Energy of a Particle

Back 21

Ek = (3/2) (R/Na)T (temperature is related to average energy of molecular motion). Note: Na is Avogadro’s number

Front 22

Root-mean-square velocity

Back 22

urms = (3RT/M)1/2; R = 8.314 J/mol.K and M, molar mass is in kg/mol

Front 23

Effusion

Back 23

process by which a gas escapes through a tiny hole into an evacuated space
rate:1/square root of M
Rate of effusion (diffusion) is inversely proportional to square root of MM (molar mass)
Time of effusion (diffusion) is directly proportional to square root of MM

Front 24

Diffusion

Back 24

the movement of a gas through space or of one gas through another

Front 25

Graham's Law

Back 25

(r1/r2) = (M2/M1)1/2
rate of effusion of gas 1 over the rate of effusion of gas 2 is equal to the square root of the molar mass of gas 2 over the molar mass of gas 1

Front 26

Mean Free Path

Back 26

average distance traveled between collisions at a given T and P

Front 27

Collision Frequency

Back 27

(#collisions/second) = speed/mean free path

Front 28

Van der Waal's Equation

Back 28

Deviations from ideal behavior of gas are observed at high P and low T;
(P + n2a/V2)(V - nb) = nRT
a: relates to particle complexity and strength of intermolecular attractions
b: molecular volume

Front 29

Thermodynamics

Back 29

study of heat and its transformations

Front 30

Thermochemistry

Back 30

study of heat changes in chemical reactions

Front 31

State Function

Back 31

depends only on initial and final states and is independent of the pathway (E is a state function).

Front 32

System and Surroundings

Back 32

System, part of the universe that is being studied
Surroundings, everything else relevant to the system

Front 33

Open vs Closed vs Isolated System

Back 33

Open system: exchanges MASS and ENERGY (usually as heat) with its surroundings
Closed system: allows transfer of ENERGY (heat) but NOT MASS
Isolated system: does NOT allow transfer of either MASS or ENERGY

Front 34

First Law of Thermodynamics

Back 34

Euniverse = Esystem + Esurroundings = 0
Total energy of the universe is constant

Front 35

Heat and work

Back 35

When energy is transferred from one object to another, it appears as heat and/or work.
E = q (heat) + w (work); q and w are not state functions

Front 36

Heat and Work (Signs)

Back 36

If heat is added to the system from the surroundings, q is positive.
If heat is added to the surroundings from the system, q is negative.
If work is done on the system by the surroundings, w is positive.
If work is done on the surroundings by the system, w is negative.

Front 37

Units of Work and Heat

Back 37

Work (joules)= force x distance=
kg m2/s2