AP Chemistry: Chapter 1-2 Notes Outline Friday, September 10 -TEST

Objectives:

  • Memorize key ions and atoms symbols and their charges
  • Be able to name ionic compounds
  • Be able to name hydrates
  • Be able to name acids
  • Be able to name molecular compounds
  • Be able to name and write formulas for coordination compounds
  • Be able to name organic compounds
  • Balance chemical equations
  • Be able to count and use significant figures in calculations
  • Be able to convert measurements using dimensional analysis
  • Know accuracy and precision
  • Be able to calculate standard deviation and percent error

Memorize Key ions and atoms:

You must score a 93% to receive credit. See memory sheet for these items. Retakes will be given immediately during your study hall on Thursday.

Naming Ionic Compounds (metal and nonmetal compounds)

Rules

1.  Name the cation

2.  Use Roman Numerals if the metal is a transition metal (Exceptions: Zn, Ag) or Pb and Sn

3.  Name the Anion ending in ide unless it is a polyatomic ion

Examples: From Formula to Name

  1. CsF 6. CuBr
  2. AlCl3 7. CoI2
  3. LiH 8. Na2SO4
  4. Fe2O3 9. Fe(NO3)3
  5. PbCl2 10. KMnO4

Examples: From Name to Formula (you must know the charges on the ions!)

  1. Vanadium (V) fluoride 6. Thallium (III) perchlorate
  2. Gallium oxide 7. Barium hydrogen carbonate
  3. Titanium (IV) nitrate 8. Rubidium sulfide
  4. Magnesium nitride 9. Sodium thiosulfate
  5. Iron (II) phosphate 10. Strontium chloride

Naming Hydrates – a compound that contains water molecules weakly bound in its crystal

Rules:

1.  Name the anhydrous compound (like above)

2.  Then a prefix for the number of water molecules followed by the word hydrate.

Examples

1.  CuSO4•5H2O 3. Sodium carbonate decahydrate

2.  MgSO4•7H2O 4. Sodium thiosulfate pentahydrate

Naming Acids

Rules: Always check the anion of the acid

1.  If the anion ends in ide change to hydo______ic acid

2.  If the anion ends in ate change to ______ic acid

3.  If the anion ends in ite change to ______ous acid

4.  If the anion is per____ate change to per_____ic acid

Examples

1. H2S(aq) 5. sulfurous acid

2. H3PO4(aq) 6. hydrobromic acid

3. HNO2(aq) 7. perbromic acid

4. HClO4(aq) 8. carbonic acid

Naming Molecular Compounds (two nonmetals)

Rules: Use prefixes for these compounds

1.  Prefix of the first element (mono is optional)

2.  Name the first element

3.  Prefix of the second element

4.  Name of the last element ending in ide

Examples: From Formula to Name

1. PCl5

2. PCl3

3. SF6

4. SO3

5. CO2

Examples: From Name to Formula

1. Dinitrogen monoxide 2. Sulfur dioxide 3. Carbon tetrachloride


Naming Coordination Compounds K4[Fe(CN)6]

Rules:

1.  The name of the cation precedes the name of the anion. (two words)

[Co(NH3)6]Cl3

2.  The name of the complex consists of two parts written together as one word. Ligands are named first, and then the metal atom is named second.

[Ru(NH3)5Cl]2

3.  Naming the ligands. Ligand – a molecule or anion bond to a metal through coordination of its lone pairs.

a.  Neutral ligands are given the name of the molecule. There are several exceptions, which are given in the table.

b.  Anionic ligands end in o.

c.  The prefixes used to denote the number of ligands is the same as the prefixes used in molecular compounds. (see chart above).

4.  The complete metal name consists of the name of the metal, followed by –ate if the complex is an anion, followed by the oxidation number of the metal (roman numeral).

5.  Examples:

  1. Na[AgCl2]
  2. Pt(NH3)2Cl2
  3. CrF63-
  4. Ag(CN)2-
  5. [Cr(H2O)4Cl2]+
  6. Hexaamminenickel (II) bromide
  7. Sodium tetrachlorooxomolybdate (IV)
  8. Tetraamminecarbonatocobalt (III) sulfate
  9. Potassium diaquatetrabromovanadate (III)

Naming Organic Compounds

Alkanes -

Rules:

1.  Add the suffix –ane to the Greek root for the number of carbon atoms in the compound.

General Formula: Greek roots # of C

Examples:

1.  CH4 5. butane

2.  C2H6 6. octane

3.  C7H16 7. propane

4.  C10H22 8. pentane

Adding an akyl group: When alkane groups appear as a

branch on the normal alkane.

When naming the compound with a branch, the longest

chain of carbon atoms are counted starting at the end

closest to the branch.

CH3

|

Example: CH3-CH2-CH-CH2-CH2-CH3

Try these:

1. CH3CHCH2CH2CH3 2. CH3─CH─CH─CH3

| │ │

CH3 CH3 CH3

CH3 CH2─CH3

│ │

3. CH3─C─CH2─CH3 4. CH3─CH2─CH─CH2─CH2─CH3

│

CH3

5. 4-ethyl-3,5-dimethyl nonane 6. 3,3-dimethyloctane 7. 4-ethyl-3-methylheptane

Alkenes-

General Formula:

Rules: 1. Find the longest chain containing the double bond. Use the prefixes + the suffix ene.

2.  The carbon atoms are numbered from the end nearest the double bond.

3.  The position of the double bond must be given as a number written in front of the stem name.

Examples:

1. CH3CH═CHCHCH2CH3 2. CH3CH2CH2CH2CHCH═CHCH3 3. 2,5-dimethyl-2-heptene

│

CH2CH2CH2CH2CH3

4. CH3C═CHCHCH3 5. CH3CH2CH2CHCH2CH2CH3 6. CH2═CHCHCH2CH3

│ │ │ │

CH3 CH2CH3 CH CH3

║

CH2

Alkynes-

General Formula:

Rules: : 1. Find the longest chain containing the triple bond. Use the prefixes + the suffix yne.

2.  The carbon atoms are numbered from the end nearest the triple bond.

3.  The position of the triple bond must be given as a number written in front of the stem name.

Examples:

1. CH3C≡CH 2. CH≡CCHCH3 3. CH3CHC≡CH

│ │

CH2CH3 CH3

Balance chemical equations

Balance the following:

__C6H12O6 + __O2 ® __CO2 + __H2O

__H2 + __O2 ® __H2O

__H2 + __N2 ® __NH3

__NO + __O2 ® __NO2

__NH3 + __O2 ® __NO + __H2O

Significant Figures:

Why significant figures?

Rules for counting significant figures

1.  All nonzero numbers count

2.  Captive zeros count

3.  Leading zeros don’t count

4.  Trailing zeros count if there is a decimal

5.  Trailing zeros don’t count if there is no decimal

Examples of counting significant figures:

1. 0.00105 g 2. 0.050080 g

3. 8.050 x 10-3 s 4. 1.008

EXACT NUMBERS: exact numbers have infinite significant figures, and therefore, are not counted when doing calculations.

Examples:
Rules for calculating with significant figures:

1.  Addition and Subtraction: You are only as good as your least accurate place value

2.  Multiplication and Division: You are only as good as your least accurate number of significant figures

Examples of calculations involving significant figures

1.  12.11 + 18.0 + 1.013 = 3. 1.05 x 10-3 6.135 =

2. 4.56 x 1.4 = 4. 21-13.8 =

Accuracy and Precision

Accuracy-

Precision-

Solving for standard deviation:

1.  Make a list of your data by pressing STAT then EDIT and enter the data into L1 (list 1)

2. Calculate the statistics

a. STAT CALC

b. 1 – Var Stats (1) and ENTER

c. ENTER again. Sx is the standard deviation.

Example: Commercial Tylenol contains approximately 500 mg of acetaminophen. A batch of tablets must contain between 450 – 550 mg of acetaminophen per tablet. Suppose a chemical analysis gave the following results for a batch of tablets: 428 mg, 479 mg, 442 mg, and 435 mg. Calculate the standard deviation.
Convert with Dimensional Analysis

The principle is that you are multiplying several fractions tog tether, but each is the same measurement so that you are essentially multiplying by 1.

Dimensional Analysis Rules:

1.  All numbers must be written as fractions—this includes numbers that are given—so 6.7 grams is

2.  All subsequent multipliers are written such that the units must cancel: For example: . Notice how the grams cancel

3.  All numbers on the top of a series of fractions are multiplied and all numbers on the bottom of a series of fractions are divided. For example:

. In your calculator you would:

143.55*0.264*4*2/1000=.

Example 1: One Dimensional Problems – a pencil is 7.00 inches long. What is the length in cm?

Example 2 : Working with multiple dimensions—Convert 55 miles per hour into meters per second.

Example 3: Complex Problems

- 1 -