Topic # 8 Descriptive Chemistry of reactions and Chemical ...



Name:_________________________ Period: _______ iPad # _____

Descriptive Chemistry,

Formula Writing

and Nomenclature

Homework ___________

Exam Date:

Free Response ~ ___________

Multiple Choice ~ ___________

Textbook:

Read Chapter 9 ~ Chemical Names & Formulas pages 262 - 297

Read Chapter 11 ~ Chemical Reactions pages 345- 368

Descriptive Chemistry of reactions and Chemical Formulas Student Outline

Descriptive chemistry involves the rules for writing formulas of compounds and writing different types of chemical reactions. Balancing equations is introduced and studied more in the topic of mole concept. Dalton first described that elements within a compound occur in specific ratios that do not change.

Chemical Equation-

Parts of a chemical equation

1. reactants

• products

• yield sign

• double arrows

• arrow up at end of an equation^

• arrow down at the end of equation

• ( over the arrows

• heat in kilojoules at the beginning of the reaction(with the reactants) means endothermic

• heat in kilojoules at the end of the reaction( with the products) means exothermic

• significance of coefficients in balancing equations

• (s) = solid, (l) liquid, (g) gas, (aq) aqueous (homogeneous mixture with water /solution/hydrated)

• catalyst in a reaction

Chemical Equations

• Chemical equation – combinations of elements and compounds and symbols that reflect a chemical reaction taking place

• Coefficients tell the # of formula units

Parts of a chemical Equation

1. Reactants

2. Products

3. Yields

4. Coefficient (formula units)

5. Change in (()

6.

|TYPE OF REACTION |DESCRIPTION AND GENERAL REACTION |

| |Atoms of elements combine to form a compound |

| | |

|Synthesis |4 Fe + 3 O2 ( 2 Fe2O3 |

| |Compound is broken down into its component elements or simpler compounds|

| | |

| | |

|Decomposition |2 HgO ( 2 Hg + O2 |

| |A single element reacts with a compound to take the place of an element |

| |of similar character. This replacement results in the formation of a new|

| |compound and a new free element. |

|Single Replacement | |

| |Cu + 2 AgNO3 ( Cu(NO3)2 + 2Ag |

| |Two compounds react to produce two new compounds (elements switch |

| |places) |

|Double Replacement | |

| |AgCl + KNO3 ( AgNO3 + KCl |

Assigning Oxidation States:

1. 1st element in a compound (the one on the left which is typically a metal or the element that is MORE likely to lose e-) usually assumes a POSITIVE oxidation state.

Exceptions:

• (OH)-1 … oxygen = -2 and hydrogen = +1

• NH3 & (NH4)+1 … nitrogen = -3 and hydrogen = +1

• Organic compounds: CH4 … C= -4 and hydrogen = +1

• Oxygen is ALMOST ALWAYS = -2 Except: 1. OF2 …O= +2 and F = -1 (F has a greater electronegativity)

2. Peroxides: H2O2 ….H = +1 and O -1

3. Na2O2… Na= +1 and O = -1

2. if there is more than one oxidation choice

a. stock system: assigning roman numerals for the oxidation state… (example +1 = I….+4= IV…..

+7= VII) ( the roman numeral IS the oxidation # … not the CHOICE

b. ** Old latin/ standard system – using suffix to designated the higher or lower of 2 oxidation choices.

“ous” = lower choice…. “ic” = higher choice.

Prefixes include: Iron = Ferr… Lead = Plumb…Copper= cupr

Examples: Fe+2 ferrous; Fe+3 ferric; Example: Cu+1=cuprous; Cu+2=cupric

c. complicated assignments – the need to figure out the correct choice using other information in the formula. When assigning oxidation states … you can assume the overall charge of the compound = 0 … unless designated with an ion charge ( + or -)

3. If there are more than 2 elements in a compound … non binary compounds … must use 1st last middle rule to identify oxidation states. Check for polyatomic ions on reference table E * be careful of SHARED OXIDATION CHARGES *

4. Assigning oxidation states to ions … such as polyatomic ions… overall charge of the ion is always noted.

5. Free elements or diatomic molecules .. can exist alone .. uncombined always have an oxidation state of 0

Diatomic molecules: elements that always occur in pairs when not in a chemical compound

** REMEMBER~ BrINClHOF

6. Be careful of Dimercury … chart E …+2

Naming Chemical Compounds

1. Ionic Compounds:

binary compounds – metal written first with “ide” ending on the nonmetal

exceptions: cyanide, hydroxide

A. ternary compounds – metal(+) and polyatomic(-)second name ends in “ate” or “ite”. Use chart E.

OR polyatomic ion(+) and nonmetal(-)second name ends in “ide”

C. transition elements with multiple oxidation states – use the stock system including a Roman numeral designating

the oxidation state of the first element.

D. Standard system can be used with “ic” or “ous” endings

2. Covalent compounds

A. Stock system used with roman numerals designates the oxidation state of the first element

a. CO2 carbon IV oxide

B. Standard system used with prefixes denoting number of atoms for that element NOT the oxidation state; used more commonly with covalent compounds

a. CO2 carbon dioxide (Prefixes: mono = 1 di = 2 tri = 3 tetra = 4 penta = 5)

Writing Chemical Formulas

1. Ionic Compounds:

a. Binary – criss cross method

b. Ternary – criss cross method; use parenthesis around polyatomic ions if subscript is more than one:

c. Stock System – criss cross method (All types reduce subscripts to empirical formula)

2. Covalent Compounds:

a. Binary (prefix) – no criss crossing

b. Binary (stock system) – criss cross method (All types reduce to empirical formula)

VOCABULARY

Chemical Equation

reactants

products

yields

double arrows

( over the arrows

exothermic

endothermic

precipitate

coefficients

Synthesis

Decomposition

Single Replacement

Double Replacement

Valence Electrons

Oxidation States

Chemical symbol

Chemical Formula

Molecular Formula

Empirical Formula

Binary Compound

Ternary Compound

stock system

standard system

ion charge

oxidation states.

Free elements

diatomic molecule

Descriptive Chemistry and Chemical Formulas Homework

Assigning oxidation states

A. Give the correct/most probable oxidation state that each element or polyatomic ion will assume when in a compound

|Element/ion |Oxidation state |Element/ion |Oxidation state |

|1. Calcium |+2 |7. sulfide |-2 |

|2. Fluoride |-1 |8. aluminum |+3 |

|3. Sodium |+1 |9. Chloride |-1 |

|4. Zinc |+2 |10. Krypton |0 OR +2 |

|5. Copper I |+1 |11. Strontium |+2 |

|6. Cobalt III |+3 |12. Sulfite |-2 |

Textbook Page 269

#6 a) K+1 cation, poatssium ion b) O-2 anion, oxygen ion c) Br-1, anion, bromine ion

d) Sn+2, cation, Tin ion e) Be+2, cation, beryllium ion f) Co+3, cation, cobalt(III) ion

#7 a) NH4+1 b) Cr+2 c) (CrO4)-2 d) (NO3)-1

Textbook Page 298

#57 a) -2 b) +1 c) -1 d) +3

#58 a) +2 b) +2 c) +3 d) +1

Pearson SuccessNet Online

Chapter 11 Directed Virtual Lab:

Identification of Cations in Solution

B. For each of the molecular formulas give the correct empirical formula

|Molecular Formula |Empirical Formula |

|1. N2O4 |NO2 |

|2. C6H8O6 |C3H4O3 |

|3. C2H6 |CH3 |

|4. CH4 |CH4 |

|5. Hg2I2 |HgI |

|6. C8H18 |C4H9 |

C. Complete the chart below

|Chemical Formula |Moles of atoms in one formula unit |Number of formula units represented |Total moles of atoms represented |

|1. Ag2CO3 |2 + 1 + 3 = 6 |1 |6 |

|2. 2Fe(NO3)2 |1 + 2 + 6 = 9 |2 |18 |

|3. 4AlBr3 |1 + 3 = 4 |4 |16 |

|4. 6Ba(PO4)2 |1 + 2 + 8 = 11 |6 |66 |

|5. 3CH3COOH |1 + 3 + 1 + 2 + 1 = 8 |3 |24 |

Writing chemical formulas and naming compounds

For each of the following give the oxidation state of each element based on the chemical formula and

write the correct IUPAC name for that compound.

|Compounds |oxidation state |oxidation state last |IUPAC Name of compound |

|(IONIC) |first element |element | |

|1. Fe2O3 |+3 |-2 |Iron (III) Oxide |

|2. CoF2 |+2 |-1 |Cobalt (II) Flouride |

|3. NiS |+2 |-2 |Nickel (II) Sulfide |

|4. MnF3 |+3 |-1 |Manganese (III) Flouride |

Pearson SuccessNet Online

Directed Virtual Lab: Ionic Naming Activity

Textbook page 273

#10 a) BaS b) Li2O c) Ca3N2 d) CuI2

#11 a) NaI b) SnCl2 c) K2S d) CaI2

Textbook page 275

#12 a) Zinc Sulfide b) Potassium Chloride c) Barium Oxide d) Copper (II) Bromide

Textbook page 298

#62 zero, compounds are neutral

Pearson SuccessNet Online

Chapter 9 Concepts in Action: Your Ionic Kitchen

|Compounds |oxidation |oxidation state|IUPAC |standard (PREFIX) name |

|(COVALENT) |state first |last element |Stock System Name | |

| |element | | | |

|5. N2O |+1 |-2 |Nitrogen(I) Oxide |Dinitrogen oxide |

|6. N2O3 |+3 |-2 |Nitrogen(III) Oxide |Dinitrogen trioxide |

|7. CO2 |+4 |-2 |Carbon (IV) oxide |Carbon Dioxide |

|8. CCl4 |+4 |-1 |Carbon (IV) Chloride |Carbon Tetrachloride |

|9. SO3 |+6 |-2 |Sulfur (VI) oxide |Sulfur Trioxide |

|10. CS2 |+4 |-2 |Carbon (IV) Sulfide |Carbon Disulfide |

Textbook page 283

#32 a) Carbon (IV) Sulfide OR Carbon Disulfide b) Dichlorine Heptaoxide

c) CBr4 d) P2O3

#35 a) molecular (N-metal & N-metal) b) ionic (metal & N-metal)

c) ionic (metal & N-metal) d) molecular (N-metal & N-metal)

Textbook page 298

#70 a) tri b) mono c) di

d) hexa e) penta f) tetra

Textbook page 294

#54 a) Sn(OH)2 b) BaF2

c) I4O9 d) Fe2(C2O4)3

|Polyatomic |oxidation state first |oxidation state last |Name of polyatomic ion |

|ion |element |element |(use Table E) |

|11. SO3-2 |+4 |-2 |Sulfite |

|12. NO3-1 |+5 |-2 |Nitrate |

|13. ClO2-1 |+3 |-2 |Chlorite |

|14. ClO4-1 |+7 |-2 |perchlorate |

| 15. OH-1 |-2 |+1 |Hydroxide |

|16. NH4+1 |-3 |+1 |ammonium |

|Ternary |oxidation state |oxidation state last |oxidation state middle|IUPAC Name of compound |

|compounds |first element |element |element | |

|17. Al(ClO)3 |+3 |-2 |+1 |Aluminum Hypochlorite |

|18. NH4Cl |-3 |-1 |+1 |Ammonium Chloride |

|19. Ca(MnO4)2 |+2 |-2 |+7 |Calcium Permanganate |

|20. CuSO4 |+2 |-2 |+6 |Copper (II) Sulfate |

|21. Ba(CN)2 |+2 |-3 |+2 |Barium Cyanide |

|22. Fe(NO3)3 |+3 |-2 |+5 |Iron ( III) Nitrate |

Textbook Page 277

# 14 a) (NH4)2 SO3 b) Ca3(PO4)2

# 15 a) Li(HSO4) b) Cr(NO2)3

Textbook Page 279

#23 a) Cr(NO2)3 b) NaClO4

c) Mg(HCO3)2 d) Ca(C2H3O2)2

Textbook page 299

#80 a) KmnO4 b) Ca(HCO3)2 c) Cl2O7

d) Si3N4 e) Na((H2PO4) f) PBr5

#81 a) MgS b) Na3PO3 c) Ba(OH)2

d) Cu(NO3)2 e) K2SO3 f) CaCO3

g) NaBr h) Fe2(SO4)3

#83 a) Lithium Perchlorate b) Chlorine (II) Oxide or dichlorine monoxide c) Mercury (II) Fluoride

d) Calcium Oxide e) Barium Phosphate f) Iodine

g) Strontium Sulfate h) Copper ( II) Acetate i) Silicon (IV) Chloride OR Silicon Tetrachloride

#84 a) magnesium permanagante b) beryllium nitrate c) potassium carbonate

d) dinitrogen tetrahydride e) Lithium Hydroxide f) Barium Flouride

g) phosphorous trioiodide h) zinc oxide i) hydrogen phosphate

Textbook page 303

#1 B

#2 D

#3 D

#4 B

#7 D

#8 C

#9 A

#10 B

Textbook page 294

#50 Dalton stated that elements combine in definite ratios and proportions

#52

Chemical reactions

Textbook page 349

#1 solid sodium added to water produce hydrogen gas and aqueous sodium hydroxide

#2 S(s) + O2(g) ( SO2(g)

Textbook page 359

#12 HBr(g)

#13 2HI(g) ( H2(g) + I2(g)

#14 3Mg(s) + N2(g) ( Mg3N2(s)

Textbook page 361

#15 a Fe(s) + Pb(NO3)2(aq) ( Fe(NO3)2(aq) + Pb(s)

#15 b Cl2(aq) + 2NaI(aq) ( 2NaCl(aq) + I2(aq)

Textbook page 363

#16 a 3NaOH(aq) + Fe(NO3)2(aq) ( Fe(OH)2(s) + 3NaNO3(aq)

#16 c FeS(s) + 2HCl(aq) ( FeCl(s) + H2S(g)

Textbook page 377

#34 a Reactants: Na & H2O

Products: H2 & NaOH

#34 b Reactants: CO2 & H2O

Products: O2 + C6H12O6

Textbook page 381

#7 D

#8 Decomposition

#9 H2O, NH3, CO2

Pearson SuccessNet Online

Chapter 11 Concepts in Action: A Balanced Equation for Fire

-----------------------

Copper Chlorine

A 32.10g = .5/.5 = 1 17.90g = .5/.5 = 1

63.5 35.5

B 23.64 = .37/.37 = 1 26.37 = .74/.37 = 2

63.5 35.5

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