Chemistry 5 Notes

What are the 3 states of matter?

What is the easiest to study? How do you breathe?

Gas

1

What is pressure? _______ per unit _____

Molecules in the gaseous state collide with objects, exerting force (_______) on them

Units of gas pressure Pounds per square inch (____)

______, _____

atmospheres (____)

Pascal (__) SI unit

2

Original Barometer Measures ___________ pressures One end of the tube is ______ Height in the tube is relative to

the __________ on the mercury reservoir and to _________

Manometer Measures _________ pressure One end of the tube is ________

into the system to be studied

Current barometers and manometers are _________

What happens the pressure if the volume is increased?

http://z.about.com/d/weather/1/0/-/1/-/-/Barometer.gif3

Increase in pressure _________ in volume __________ temperature, mols

If two systems are at the same temperature with the same number of moles, k will be the same

Example: Crushing an empty water bottle, Balloon

Note: Untrue at extreme temperatures, pressures, volumes

4

Increase temperature ___________ volume ____________ pressure, mols

If two systems have the same pressure and mols, then k is the same

Example: Take a balloon from warm outdoors to cool indoors

Note: Untrue for extreme temperatures, volumes and pressures

Wait What about negative temperatures?

5

When using gas laws, __ and __ will not work Cant have a __________ volume and cant divide by

_______

When using gas laws, __ will work Do gases exist at absolute zero?

6

Increase temperature ___________ pressure ___________ volume, mols

If two systems have the same volume and number of mols, then k is the same

Example: Opening a 2L of cold drink

Note: Untrue for extreme values of temperature, pressure and volume

7

Increase in volume ____________ in mols _____________ temperature, pressure

If two systems have the same temperature and pressure, then k is the same

Note: Untrue for extreme temperatures, volumes, and pressures

Four Laws Is there a simpler way?

8

Ideal Gas Constant 0.08206 (Latm)/(molK) 8.31447 J/(molK) 8.3145 (kPadm3)/(molK)

Example: A balloon sitting outside (pressure = 1atm) on a chilly

day (temperature = 10C) contains 0.097 mols of nitrogen gas. What is its volume?

Note: K = C + 273.15

nRTPV

9

A gas exerts a pressure of 0.892atm on a 5.00L container at 15C. How many moles are in the container?

A 16.0g sample of methane gas (CH4) has a volume of 5.0L at 27C. What is the pressure?

What is the temperature of a 350mL flask containing 0.012mols of gas at 0.96atm?

A 25.0mL sample of a gas is sealed in a 22C flask. The flask is placed in a 0C ice bath. What is the new volume of gas if the pressure is constant?

Need more practice? Try problems 12.12-12.36 and 12.43-12.52

10

What is diffusion (in terms of gases)? The _____________, due to random motion, of a gas

into a space or the ________ of one gas with another

Hence the strange smell fills the room!

What is effusion? The escape of a gas through a ____________

____________ material ___________ contain gases it has to be ________

Hence throwing something producing gas in a trash can with a lid cannot contain the smell they can escape!

11

STP Standard Temperature and Pressure Ideal gas law works well

Standard Molar Volume The volume of _____ mol of ___________ at STP It would be precise if all gases were ideal

What else can be found from the Ideal Gas Law?

12

If number of grams of sample is known, then can find molecular weight

Example: What is the molecular weight of a gas if a 0.495g sample occupies 127mL at 98C and 754 torr?

Note: The molecular weight calculated here can be used in conjunction with percent composition information in order to find the molecular formula

13

Using the ideal gas law, can calculate the density of a gas at a given temperature and pressure

Example: What is the density of N2 gas at 1.00 atm and 100C?

14

Number of moles of each type of molecule is additive, so pressure of each type of molecule is additive

Example: The partial pressures of the atmospheric gases N2, Ar,

CO2 and other trace gases are 0.7808atm, 0.0093atm, 0.00038atm, and 0.00002atm, respectively. If the air pressure in the room is 1atm, what is the partial pressure of O2?

...321 PPPPTotal

15

The fraction of molecules that are a certain component Note: The sum of all the mole fractions should equal 1

Can be related to partial pressure using the ideal gas law

Note: All liquids have a characteristic vapor pressure The amount of liquid that will vaporize at a given

temperature A partial pressure if gas is collected over a liquid

16

What is the molecular weight of a gas if a 1.580g sample occupies 1L at 273K and 760 torr?

What is the density of O2 gas at 0.96 atm and 60.C? Two flasks are attached with a valve. The 2.4L side is

filled with CO2 to 4.3atm. The 3.6L side is filled with N2 to 6.9atm. The valve is opened and the gases mix. What is the volume of the system? What are the partial pressures of each gas? What is the mole fraction of CO2?

O2 gas is collected over water at 20C and 754 torr. The total volume of gas collected was 500mL. How many mols of O2 were collected? Note: Vapor pressure of water at 20C is 17.54 torr

Need more practice? Try problems 12.37-12.42, 12.53-12.71

2211 VPVP ...321 PPPPTotal nRTPV

x17

Volumes of gases are additive

Reactions follow mol ratios

Example: 37.2g of Al(s) is placed in a balloon with excess water and NaOH. By how much will the volume of the balloon increase when the Al has finished reacting assuming H2 is an ideal gas?

H2(g) + Cl2(g) 2HCl(g)

2NaOH(aq) + 2Al(s) + 6H2O(l) 2Na[Al(OH)4](aq) + 3H2(g)

Try problems 12.72-12.84 18

Kinetic Molecular Theory Gases are made of ___________ (atoms or molecules) in

constant _____________ The _______ of the motion (kinetic energy) is determined

by the _____________ Molecules ________ and can _________ kinetic energy, but

the _______ kinetic energy remains the _____ Gas particles have ____________ Gas particles do ___________ or ________ each other Gas ___________ is caused by the ___________ of the

particles with the container it is in

If this is Kinetic-Molecular ________, whats your proof?

19

Boyles Law

Constant temperature same ___________ of molecules

Halving the volume __________ the surface area of the vessel and ____________ the distance traveled by molecules

More molecules _________ with the exterior of the vessel

Pressure depends on _________ with the walls of the vessel, then the pressure would __________ due to the _________ volume

kPV

http://3.bp.blogspot.com/_hfAYZzG11r8/SRj1eLqgMCI/AAAAAAAAAZw/ce4I1jM-XYI/s1600-h/Boyle_1.gif

20

Daltons Law

Gas molecules do ________ or _______ each other, so they collide independent of the type of molecules in the vessel

Each molecule __________ with the exterior of the vessel as if ___________ molecules are there

Each gas exerts the same amount of __________, giving a total pressure equal to the ____ of the ________ pressures

...321 PPPPTotal

http://spinner.cofc.edu/~martine/111LectWeek7.htm21

Charles law

____________ the temperature _________ the average KE of each of the molecules, ___________ the velocity (and momentum) of each of the molecules

Increased energy of the _________ on the exteriorof the vessel pushes the walls ________, __________ the total volume of the vessel

kT

V

http://boomeria.org/chemtextbook/fig18-6.jpg22

What is KE equal to?

So, if _____________ is known, the average ______ of molecules is known? Yes, but how do you change from ___ to __? Start with pressure

Force is proportional to momentum (=mass*velocity) Rate is proportional to molecular speed (v) and number

of molecules in the volume (N/V) So,

2

2

1mvKE TKE

or

23

It can be shown that on average (average velocity), the molecules collide 1/3 of the time, therefore

Knowing that the number of molecules (N) equals number of mols (n) times Avogadros number (NA) and the ideal gas law

Knowing KE=mv2/2, then

Knowing NA*m is molecular weight (M) and defining vrms as , then

v 2

24

Example: What is the root-mean-square speed of N2 molecules in

m/s at 25C?

Try this! What is the root-mean-square speed of O2 molecules in

m/s at 20C? The root-mean-square speed of some molecules was

found to be 1.425x103 m/s at 23C. What is the molecular weight? What molecule/atom is it?

Why is there such few molecules of H2 and He on earth when they are the most abundant molecules in the universe?

M

RTvrms

3

2

2

11s

mkgJ

mol

gM

Need more practice? Try problems 12.85-12.92 25

Kinetic Molecular Theory Gases are made of particles (atoms or molecules) in

constant motion The speed of the motion (kinetic energy) is

determined by the temperature Molecules collide and can change kinetic energy,

but the total kinetic energy remains the same Gas pressure is caused by the collisions of the

particles with the container it is in

All true?

26

If every gas were perfectly ideal, then

nRTPV 1RT

PVThen, For one mole

http://itl.chem.ufl.edu/2045/lectures/lec_e.html27

Attempt to account for non-ideality of gases

Two corrections Gas particles do have _________, especially seen at high _________ Each mole of gas takes up approximately __ (a constant for each gas) of

space (L/mol), so the volume of empty space is reduced by ___ Gas particles do ________, especially seen at low ____________ and

high _______________ Molecules deviate from a straight line, ___________ the collisions with

the walls The pressure measured is ________ than the pressure of an ideal gas The constant __ is a measure of the ______________ between molecules

(larger _, more ___________ attracted)

Constants are experimentally found

nRTnbVV

anP

2

2

28

Example What is the pressure of 2.00 moles of H2 in 250mL

vessel at 20C if H2 acts as an ideal gas? As a van der Waals gas? (a=0.244 L2atm/mol2; b=0.0266 L/mol)

Try this! You want to store 165g of CO2 gas in a 12.5L tank

at 25C. Calculate the pressure the gas would having using the ideal gas law and the van derWaals equation (a = 3.59 atmL2/mol2; b = 0.0427 L/mol).

Which molecule would have a higher value for a, NH3 or H2? b?

Need more practice? Try problems 12.93-12.101

x29

Where do you see acids and bases? ______________ (ammonia, sulfuric acid, sodium

hydroxide, sodium hypochlorite, boric acid, phosphoric acid)

_____________ (sulfuric acid)

_____________ (hydrochloric acid, carbonic acid)

_____________ (ammonia, sulfuric acid, nitric acid, phosphoric acid)

_______ (carbonic acid, sodium carbonate, uric acid)

____________ (carbonic acid, phosphoric acid, citric acid)

30

Acids ________ taste Change the ______ of indicators Nonoxidizing acids react with metals to produce

_________________ React with some salts to form a weaker acid and a

different _____ Conduct _______________

Bases _________ taste Slimy or slippery (_______ are slightly basic) Change the _______ of indicators (different _______ than

acids) React with acids to form __________ Conduct ______________

31

Gay-Lussacs thoughts Acids and bases should be defined by their ________

with _______________

Concluded that an acid and a base _________ each other

Arrhenius Theory Acids a substance that contains hydrogen and

produces ___ (_________) in aqueous solutions

Base a substance that contains the ___ group and produces _________ ions (____) in aqueous solutions

H+ + OH- H2O

32

Acids are found in aqueous solutions

What happens to H+ in water?

Forms the hydronium ion, ________ Hydrated hydrogen ions

Protons, hydrogen ions, hydronium ions, acid are all interchangeable terms

33

Arrhenius definitions work every time, right? Acids work great!

What about _________?

What is the formula for _____________?

Is it an acid or a base?

Brnsted-Lowry Theory Acid a substance that is a ________________

Base a substance that is a ________________

34

Anytime a _________ moves from one molecule to the other, it is an ___________ reaction

Conjugate Acid-Base Pairs From the Acid to the Base: The acid has ______ an H+ in

the formation of its conjugate base (both a hydrogen and a positive charge)

From the Base to the Acid: The base has ________ an H+in the formation of its conjugate acid

HF + H2O F- + H3O

+

35

Why was there a double arrow in the last reaction? The reaction goes _____________________

Do all acids and bases act that way?

Strength of Acids Strong acids completely dissociate in water

Weak acids _________________ in water Equilibrium lies (far) to the left

Strength of Bases Strong bases completely dissociate and

are soluble in water

Weak bases __________________ in water Equilibrium lies (far) to the left

36

HSO4- + H3O

+H2SO4H2O

SO42- + H3O

+H2O

See Table 10-2

37

Name the conjugate base for the following acids. Note which are amphiprotic. H2SO4 CH3COOH HClO4 HNO3 HCN

Name the conjugate acid for the following bases. Note which are amphiprotic. NH3 OH-

PO43-

HSO4-

NH2-

Which is a stronger electrolyte, a strong acid or a weak acid? Why?

Need more practice?Consider problems 10.1-10.29 38

What is the other half of the following equilibrium?

Water self-ionizes Which side is more favored? Why?

Is water amphiprotic?

H2O + H2O

39

Binary Acids Strong Acids: HCl, HBr, HI Weak Acid: HF Why? Things to consider: The ease of breaking the HF _______

The _________ of the resulting _____ in solution

Bond strengths:

The HF bond is strongest Difference in electronegativity: HF ____; HCl ____; HBr

____; HI _____

Wait that would mean HF is _______, so it should dissociate and be the strongest acid in water

Since each ion is ________, it causes the water molecules to be more _________, which is energetically ____________

HF>>HCl>HBr>HI

40

Out of HF, HCl, HBr, and HI HF is the weakest. What is the strongest?

In dilute water solutions, HCl, HBr, and HI ___________ ionize Water is basic enough to ___ differentiate between the acids Water is considered to be a ________________ for these acids All are completely ionized, so all are _______ in acid strength

Acids ____________ than H3O+ ______________ with water to form

H3O+ and their conjugate base

In anhydrous acetic acid, (or other solutions less basic than water) HCl __ HBr __ HI in acid strength

Pattern is the same for group 6A hydrides H2O ___ H2S __ H2Se __ H2Te

Consider Table 10-2 41

Any acids _________ than H3O+ will completely react in

water to form H3O+ and its conjugate base

All of the ______________ are stronger than H3O+

The ______________ is the one that exists in solution Any base __________ than OH- will react in water to

form OH- and its conjugate acid All of the bases with an __________ completely dissociate

_____________ bases than water Bases without _________ (NH2

-) are stronger bases than OH-

and acquire an additional ___ from ________ Remember: Bases have to ___________ into water to be

considered a strong base

Note: Other solvents can be leveling solvents, but must be ____________ and are defined using ________ acidic and basic forms

x42

Ternary Acids acids containing __________ different elements

Many are __________ compounds of nonmetals Ionize to produce ___ (not _____, like in compounds

of metals) Example: HNO3 is written with the H first to

emphasize it is an _______, but could be written as HONO2 due to its ____________ The O-nonmetal bond is more _________

than in O-metal bonds giving a _____________ bond for O-nonmetal

Makes the _____ bond the _____ point, causing ___ to ionize rather than _____

http://en.wikipedia.org/wiki/File:Nitric-acid-3D-balls-B.png43

What is the Lewis Dot Structure of H2SO4? HSO4-?

SO42-?

Do all polyprotic acids completely dissociate?

Most polyprotic acids are _________ than H3O+ in their most

acidic form Removing an additional positive charge from a positive ion

is more _________ than a positive charge from a neutral acid

http://commons.wikimedia.org/wiki/File:Sulfuric-acid-2D.png

HSO4- + H3O

+H2SO4H2O

SO42- + H3O

+H2O

44

What is the Lewis Dot Structure for H2SO3? HSO3-?

SO32-?

Which is a stronger acid, H2SO4 or H2SO3? Why? _________ more electronegative oxygen atoms causing the

hydrogen bonds to be more _______________

Typically, acids in the same periodic table group increase in strength as the electronegativity _________ H2SeO4 __ H2SO4

Try this! - Which is the stronger acid? HNO3 or HNO2? HClO or HClO2?

http://upload.wikimedia.org/wikipedia/commons/c/c5/Sulfurous-acid-2D.png


Strong acids and bases Completely ____________ in water Acid is stronger than H3O

+, base is stronger than OH-

(and can be dissolved in water)

Any strong acid strong base reaction will have the same net ionic equation Consider HCl and NaOH What happens to HCl in water? NaOH?

Then what reacts?

What is the total ionic equation?

46

What is the net ionic reaction of a weak acid and a strong base that form soluble salts and water? Consider the reaction of HCN and NaOH What is the overall reaction?

What happens to HCN in water? NaOH?

What is the total ionic equation?

What is the net ionic equation?

What is a general way of denoting a weak monoprotic acid reaction with a strong base?

47

Try this! What is the overall reaction, total ionic reaction, and net ionic

reaction for the neutralization of HClO2 and LiOH? What is the overall reaction, total ionic reaction, and net ionic

reaction for the neutralization of KOH with HClO4? Predict the acid-base reaction that would form the following salts NaCl KNO3 BaCl2 CaSO4

Predict the general net ionic equation for A strong acid strong base reaction producing an insoluble salt A weak acid strong base reaction producing an insoluble salt A weak base - strong acid reaction producing a soluble salt A weak acid weak base reaction producing a soluble salt Note: there are no common examples of a weak base reacting with

either a weak or strong acid producing insoluble salts


When all the H+ and OH- have reacted, there has been complete ________________

Normal salts contain no __________ H or OH groups (complete neutralization) Examples: NaCl, KNO3

Acidic salts less than stoichiometricamounts of base used with a ___________ acid, products are water and an acidic salt

H2SO4 + NaOH

H2SO4 + 2NaOH

49

Basic Salts less than stoichiometric amounts of acid used with a _______________ bases

Note: Acidic Salts are considered acidic Because they contain another ____________ and can

neutralize __________ Not because they are _______ (___)

Note: Basic Salts are considered basic Because they contain another ____________ group and

can neutralize _________ Not because they are _______ (___)

Ca(OH)2 + HCl

Ca(OH)2 + 2HCl

Consider problems 10.57-10.66x

50

Most comprehensive Acid any species that can accept or share an __________

______ Atoms not having a ___________

Base any species that can donate or share an __________ ______ In theory, any species with a _____________ can act as a Lewis base

Neutralization coordinate covalent bond (or dative) formation, a bond in which ______ electrons are furnished by _____ atom or ion (Lewis ______) Includes all the ______________ acids and bases as the proton is

bonded using ________ electrons from the _________ Example: BCl3 + NH3

Try this! Which of the following are Lewis Acids? Lewis Bases? AlCl3, NH3, SnCl4, PBr3


Which is the best theory to use? ____ Arrhenius acids and bases are Brnsted-Lowry

acids and bases, but ________ Brnsted-Lowry acids and bases are Arrhenius

___ Brnsted-Lowry acids and bases are Lewis acids and bases, but ________ Lewis acids are Brnsted-Lowry acids and bases

The vast majority of Lewis acids that _______ Brnsted-Lowry acids and bases are most important in ___________ solvents

In _______ solvated solutions (or other protic solvents), Arrhenius or Brnsted-Lowry definition works _______

52

Every neutralization reaction has a ______________

Reaction ratio relative number of ______ of reactants and products in a reaction Ratio between moles of ________ and moles of ______

For complete neutralization, the product must be a ___________________ All ___________ H and OH groups must have __________

Example: What are the products of the complete neutralization of H2SO4 and NaOH? Mole ratio?

Try this! What are the products of the complete neutralization of each of the following? Mole ratio? H3PO4 and LiOH HCl and KOH HBr and Ca(OH)2

53

The mole ratio indicates how many ______ of acid needed to _______ with the base

In what form do acids and bases usually come in? Solid (______ ________) Aqueous (________ _______)

What is molarity?

Example: 150mL of 0.12M HCl is mixed with 150mL of 0.15M NaOH. What solutes exist in the solution? What are their concentrations?

Try this! 200mL of 0.60M H3PO4 is mixed with 300mL of 0.9M Ca(OH)2. What solutes exist in the solution? What are their concentrations?


The process of reacting an acid or a base of known concentration (____________) and volume with a base or an acid of unknown concentration where the volume is added slowly until the ___________________ is reached Typically use a ______ to measure volumes

___________________ where the mols of acid and base are stoichiometrically equal

Indicators are selected to change _______ at or near the equivalence point Indicator a substance that has different forms having

different _______ based on the ___ concentration, intensely __________ (little must be added to the reaction)

____________ where the indicator changes colors

55

A solution with known concentration, has been _______________

Standardization process by which one determines the _________ concentration of a solution by titration against a ______ standard, the solution is then a __________ standard

Primary standard Must _________ with or _______ the components of the atmosphere

(H2O, O2, CO2, etc) Must react with ______________ reaction High _______ High ___________ (minimize errors in weighing) _________ in solvent of interest Readily available and _____________ Environmentally _____________ Examples: Oxalic Acid, Sodium Carbonate, KHP (Potassium

hydrogen phthalate)

56

Example: Consider the standardization of HCl with Na2CO3. If the volume HCl needed to neutralize 0.2130g of Na2CO3 is 43.21mL, what is the concentration of HCl? What is the molar ratio?

How many mols of Na2CO3 was neutralized?

How many mols of HCl were in the solution?

What is the molarity of HCl?

2NaCl + CO2 + H2O2HCl + Na2CO3

57

23.42 mL of the secondary standard solution of HCl found in the previous problem was used to titrate 25.00mL of an unknown concentration of KOH. What is the concentration of the KOH? What is the molar ratio?

How many mols of HCl was neutralized?

How many mols of KOH were in the solution?

What is the molarity of KOH?

KCl + H2OHCl + KOH

58

30.00mL of 2.424M HCl is reacted with an unknown concentration of LiOH three times. The volume of LiOH used is 15.32mL, 15.28mL, and 15.29mL, respectively. What is the concentration of LiOH?

What is the concentration of NaOH if 43.96mL, 43.97mL and 43.99mL were required to reach the equivalence point with 20.00mL of 3.6513M HNO3?

The volumes of H2SO4 used in the three titration trials were 23.43mL, 23.41mL, and 23.44mL. If 25.00mL of 1.3287M NaOHwas used, what is the concentration of H2SO4?

A student had just finished their titration experiment using 35.00mL of 2.157M HCl as a standard and found that the concentration of their NaOH was 2.074M. As they were cleaning up, water spilled all over the volumes of NaOH used, making them unreadable. What was the average value of the volumes? If two of the volumes were found to be 36.40mL and the other 36.41mL,

what was the third volume?


Using a primary or secondary standard, the ______________ can be found

Example: An impure sample of KHP was titrated against standardized 0.1932M Ca(OH)2. The titration required 16.51mL of the base to reach the end point upon reaction with 1.452g of KHP. What is the percent purity of the sample of KHP (KC8H5O4)?

Ca(KP)2 + 2H2OCa(OH)2 + 2KHP

60

A molecule has resonance when ____________ Lewis formulas with the same atomic arrangements can be drawn to describe the bonding What are the Lewis structures for CO3

2-? How would the bonds be appropriately denoted on a single Lewis structure?

What about SO2?

NO2-?

61

Steps to balance a redox reaction Determine which atoms change _____________ (there should be

_______ than one!) Write _________ for all atoms that change oxidation state (be sure

to balance the atoms on each _____________) Balance the ___________ lost with the __________ gained across the

half-reactions Place the ____________ on the overall reaction (be sure to always

keep those proportions) Balance the remaining atoms If the reaction is in acid, Balance O with _____ (make sure to add to the correct side) Balance H with ____ (make sure to add to the correct side)

If the reaction is in base, Balance as if in acid Neutralize the ___ by adding the same number of ___ as ___ to each side Cancel out _______ molecules if necessary

62

Balance the following redox reactions

H3PO4 + NOP4 + NO32-

acid

Cu2+ + H2O + SO2Cu + H+ + SO4

2-

Cr3+ + I2 + H2OCr2O72- + H+ + I-

IO3- + Cl- + H+ClO3

- + H2O + I2


Combining titration calculation with a balanced redox reaction __________ the redox reaction

Complete the calculation as a _____________________

Example: The following reaction happens in acidic conditions. What is the concentration of H2O2 if it takes 13.53mL of 0.2582 MnO4

-

to react with 20.00mL?

Mn2+ + O2H2O2 + MnO4-

64

What volume of 0.1897M KMnO4 would be required to oxidize 25.00mL of 0.1482M KI? (Products include Mn2+ + I2)

What volume of 5.0M nitrate ion solution would be required to react with 35mL of 0.75M sulfide ion solution?

35.32mL of the I2 solution is required to titrate a sample containing As2O3. Calculate the mass of As2O3 in the sample.

Need more practice?Consider problems 11.62-11.71

NO + SNO3- + S2- acid

H3AsO4 + HIAs2O3 + H2O + I2

65

Exam 5 Measuring pressures Boyles Law, Charles Law, Gay-Lussacs Law, Avogadros Law, Daltons Law Temperature Scale Ideal Gas Law Diffusion, Effusion STP, Standard Molar Volume Molecular Weight/Density of gases Mole Fraction Reactions involving gases Kinetic Molecular Theory, problems thereof Experimental evidence of Kinetic Molecular Theory Kinetic Energy of Molecules, Root Mean Square Velocity of molecules Van der Waals gases Properties of Acids and Bases Arrhenius, Bronsted-Lowry, Lewis Acids and Bases Conjugate Acid-Base Pairs Strength of Acids and Bases (Binary and Ternary) Amphiprotic Acids Leveling Effect Acid-Base Reactions in Water (titrations, standardization) Acidic and Basic Salts Percent purity Resonance Redox reactions, redox titrations

66

Cumulative Reading volumes, lengths, etc.

Significant Figures

Scientific Notation

Unit Conversion

Accuracy vs. Precision

Specific Heat

Density

Radioactive particles, Fusion vs. Fission, Atomic Symbols

Naming Ionic and Binary Covalent Compounds

Moles

Molecular/Formula Weight

Balancing Reactions

Mass Relationships/Limiting Reagents

Percent Composition

Molarity, Dilutions

Reaction Types

Quantum Numbers

Orbital Box Diagram

Electron Configuration

Effective Charge

Atomic Spectra

Lewis Dot Structures

Periodic Trends

Bond Types, polarity of bonds

Electronic Geometry, Molecular Shape, Bond Angles

Molecular Orbital Diagrams (homonuclear, heteronuclear)

Bond order

Balancing redox reactions in water, acid, base

and the information for Exam 5

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Chemistry 5 Notes