VISTA RIDGE CHEMISTRY **THIS WEBSITE IS NO ...vistaridgechemistry.weebly.com/uploads/4/9/6/4/49648… · Web viewPodcast 5.1 Ionic vs Covalent Read p. 187 – 193; Questions 3-11

Name:___________________________Period:__________________________

Chemistry Unit 5 – Forming CompoundsChemistry Daily Journal

Today’s Date

What do I need to accomplish today?

What do I need to finish up at home?

Objective □ Learning Opportunities Suggested Due Date

Date Completed

5.1 Compare and Contrast Ionic Compounds and Covalent Compounds

□ Podcast 5.1 Ionic vs Covalent□ Read p. 187 – 193; Questions 3-11 p. 193,

Read p. 213-216; Questions 1-5 p.216□ Types of Chemical Bonds and

Counting Atoms

11/14/14

5.2 Chemical Formulas of Binary Ionic Compounds

The Naming Card can be printed in FULL COLOR from the Vista Ridge Chemistry website!

□ Podcast 5.2 Bonding Basics (complete Bonding Basics Worksheet Sections A and B)

□ Read p.194-199 and p. 260-266; Questions 12 and 13 p. 196, 14-20 p. 199 and 14-19 p. 266

□ POGIL Chemical Formulas□ Forming Ionic Compounds Lab□ Criss-Cross Charges□ Writing and Naming Ionic

Compounds□ Naming Ionic Compounds

11/18/14

5.3 Chemical Formulas with Multivalent Metals: Stock Naming and Classical Naming

□ Podcast 5.3 Multivalent Metals in Ionic Compounds

□ Writing Formulas from Names□ Read 253-258; Questions 4-9 p. 258, and 14-

19 p. 266□ Cat Food Take Home Lab□ Naming Compounds Moodle Quiz

11/20/14

5.7 Metallic Bonding □ Podcast 5.7 Metallic Bonding□ Read p. 201-203□ The Alchemists Dream: Penny Lab*

MUST pass Naming Quiz to be

11/21/14

eligible for the Penny Lab

Podcast 5.1: Ionic vs Covalent CompoundsForming Ionic Compounds

• Ionic bonds form when electrons are __________________ from one atom to another, forming ions.

• Bond represents the ________________ of a positively- charged particle and a negatively-charged particle

Orderly Arrangement of Atoms

•

•

•

•

••••

• •Properties of Ionic Compounds

• Usually ___________ at room temperature

• Have _________ melting points >300 oC• ____________ an electric current when melted or

dissolved in water• Highly ________________ in water• Ions arranged in regular repeating pattern called a ____________

structure• Made of ________ ___________ (not true molecules)

Covalent/Molecular Compounds• Covalent bonds form by the _____________ of electrons• Atoms can form single, double, or even triple bonds to satisfy the

_____________ ________ for each atom (except Hydrogen)Molecular Structures (Sketch)Water Ammonia Carbon Dioxide Methane (CH4)

Hematite Fe

Properties of Covalent Compounds• Can be solids, liquids, or gases• Tend to have ______________melting points (<300 oC) and boiling

points• Not always soluble in water• _____________ conductors of electricity

Metallic Bonding• Metals have closely-packed cations with a ________ of ____________

_______________ freely moving around them.• Metallic bonds form due to the ____________ of free-floating

valence electrons for the positively-charged metal ions

Crystal Structure of Metals Allow for Close-Packing of CationsProperties of Metals

• __________ conductors of heat and electricity• ________________ – can be drawn into wires• ________________ – can be hammered or forced into shapes• Crystallize in characteristic patterns• _____________ enhance natural properties of individual metals to

make their traits more desirableDetermining the Type of Compound

• A ___________ and a _______________ form Ionic bonds• ________________ alone form Covalent bonds• ________________ alone form Metallic bonds

Examples:1. KNO3

2. Fe2O3

3. CO2

4. NO2

5. Cu2S6. CH4

7. C6H12O6

8. Bronze (alloy of copper and tin)

Number of Atoms in a FormulaDetermine the number if atoms in the following chemical formulas.

1. NaCl 2. H2SO4 3. KNO3 4. CaCl2 5. C2H6 6. Ba(OH)2 7. NH4Br 8. Ca3(PO4)2 9. Al2(SO4)2 10.Mg(NO3)2 11.Cu(NO3)2 12.KMnO4 13. H2O2 14.H3PO4 15.(NH4)3PO4 16.Fe2O3 17.NaC2H3O2 18.Mg(C2H3O2)2 19.Hg2Cl2 20.K2SO3

Types of Chemical BondsIdentify the following compounds as ionic (metal and nonmetal), covalent (nonmetal and nonmetal) or both (compound containing both).

1. CaCl2 2. CO2 3. H2O 4. BaSO4 5. K2O 6. NaF 7. Na2CO3 8. CH4 9. SO3 10.LiBr 11.MgO 12.NH4Cl 13.HCl 14.KI 15.NaOH 16.NO2 17.AlPO4 18.FeCl3 19.P3O5

6

Bonding BasicsSection A: Complete the chart using a periodic table to help you.

Element Atomic Symbol

Total # of Electrons

# of Valence Electrons

# of Electrons Gained or Lost

Oxidation Number

Chlorine

Potassium

Magnesium

Fluorine

Aluminum

Sodium

Nitrogen

Oxygen

Hydrogen

Carbon

Iodine

Answer these questions:

An atom that gains one or more electrons will have a ____________________ charge.

An atom that loses one or more electrons will have a ____________________ charge.

An atom that gains or loses one or more electrons is called an ____________. A positive ion is called a ______________ and a negative ion is called an

_______________.

Section B: What is an ionic bond?

Atoms will transfer one or more ______________________ to another to form the bond.

Each atom is left with a ______________________ outer shell. An ionic bond forms between a _______________ ion with a positive charge

and a __________________ ion with a negative charge.

7

Example B1: Sodium + Chlorine Example B2: Magnesium + Iodine

Example B3: Potassium + Iodine Example B4: Sodium + Oxygen

Example B5: Calcium + Chlorine Example B6: Aluminum + Chlorine

Section C: What is a covalent bond? Atoms ______________________ one or more electrons with each other to form the

bond. Each atom is left with a ______________________ outer shell. A covalent bond forms between two ______________________.

Example C1: Hydrogen + Hydrogen Example C2: 2 Hydrogen + Oxygen

Example C3: Chlorine + Chlorine Example C4: Oxygen + Oxygen

Example C5: Carbon + 2 Oxygen Example C6: Carbon + 4 Hydrogen

8

Challenge: What are some other ionic or covalent bonds that can be formed by the elements you see? Write the chemical formula for the compound and its name on a separate piece of paper and attach to this page.

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Podcast 5.3: Naming Ionic Compounds Ions and Formulas: By predicting formation of __________, you can determine the __________________ of compoundsExample: what compound would form from Ca + O?

Step 1 –

Step 2 –

Step 3 –

Examplesa) Al,Br

b) K,S

c) Zn,O

d) Mg,N

e) C,Cl

f) Cu,O

Naming Ionic Compounds: Rules for naming1. Names end in ______________. Example: sodium chloride2. Metal (__________________ ion) comes first

- not chlorine sodide 3. Do not capitalize unless starting a sentence

Examples: Give formulas & names:

Ca + I

O + Mg

Na + S

Transition Metals: Standard NamingChange anion ending to ____________ The charge of the metal is indicated in parenthesis using ________________ ________________

Ex: Cu1+ is _______________ , Cu2+ is _________________11

3. Numbers refer to __________________ not to number of atoms

Examples: Write Names and Formulas for the Following Compounds

a) Cu2++Cl-

b) Zn2+ + Cl-

c) Co2++Cl-

d) Hg+S (do both charges)

Transition Metals: Classical Names1. Change anion ending to -ide 2. The metal is named with it’s Latin or English root and ends in _______ or

______ to denote chargea. “ic“ is higher than – “ous”b. (because i am more important than u) c. Example: Cu1+ is ____________, Cu2+ is______________

Now You Try! Give formulas and Latin names for:

a) Cu2+ + Cl- b) Co2+ + Cl-

Naming with Polyatomic Ions: Groups of atoms can also have a charge__________________ ions are groups of atoms that interact as a single unit. Examples: OH1-, (SO4)2-, Ba3(PO4)2=

Examples: Name the Following Compounds with Polyatomic Ionsa) Ca(OH)2

b) CuSO4

c) NH4NO3

d) Co2(CO3)3

Writing Formulas from Names1. Identify the ions and __________________ involved.2. _____________ - ______________ the charges to write the formula3. Use parenthesis around polyatomic ions

Examples1. sodium chlorate 4. ferrous oxide

2. iron (III) hydroxide 5. silver nitrate

3. barium fluoride 6. ammonium chloride

Examples: Write the formulas of the following compounds1. Ferric oxide

2. Chromous sulfide

3. Aluminum sulfite

4. Copper (I) hypochlorite12

5. Copper (II) hydroxide

6. Potassium bromide

7. Plumbic cyanide

8. Manganese (II) nitrite

9. Manganic phosphide

10. Calcium chlorite

Writing and Naming Ionic CompoundsFill in each column with the appropriate information. For the

“Compound Name” you may choose to do stock naming or classical naming. But just so you know we will be using stock naming most

of the time.

This would be a really good chance for you to get to know your ion card really well.

Compound Made Of…

Positive Ion

Negative Ion

Chemical Formula

Compound Name

Number of

Atoms

1 Ca and Cl

2 Ni (II) and SO4

3 Cu (I) and CO3

4 Mg and Cl

5 Sn (II) and SO4

6 NH4 and PO4

7 Al and NO3

8 Ca and SO3

9 Fe (II) and CO3

10 Ca and OH

1 Li2SO4

13

112 SrCO3

13 NH4F

14 Cr2O3

15 Fe3(PO4)2

Compound Made Of…

Positive Ion

Negative Ion

Chemical Formula

Compound Name

Number of

Atoms16 Ca(NO3)2

17 SnCl4

18 CuCO3

19 BaBr2

20 SnSO3

21

Ammonium nitrate

22

Lithium phosphate

23

Sodium bicarbonate

24

Lead (II) phosphate

25

Magnesium hydroxide

26 Silver sulfide

27 Barium acetate

14

28

Manganese (II) fluoride

29 Chromic nitrate

30 Ferric sulfate

15

Making Ionic Compounds Lab

SO4-2 C2H3O2

-1 NO2-1 C2O4

-2

Al+3

Name

NH4+1

Name

Ba+2

Name

K+1

Name

PurposeTo study the formation of ionic compounds and derive the formula of the ionic compounds formed.

Materials Reaction well plate Solution A (Fe3+ ion – Fe(OH)3) Solution B (Ag+ ion – AgNO3 ) Solution C (Pb2+ ion – Pb(NO3)2)

Solution X (CO32- ion – Na2 (CO3) )

Solution Y (OH- ion – NaOH) Solution Z (PO4

3- ion- Na3(PO4) )

PRE-LAB: In the chart below, write the correct formula for each of the following ionic compounds using the Criss-Cross Method.

Procedure1. Label three columns A, B, and C in your well plate2. Add 5 drops (0.5 mL) of solutions A, B, and C to their respective wells.3. Add 5 drops of solution X to one well of A, B, and C. Observe each for the formation

of a solid and briefly describe each reaction on the chart on the next page.4. Repeat Step 3 using solutions Y and Z.

Data Table

Cation Anion CO32- OH- PO4

3-

16

Fe3+

Description

Formula

Name

Ag+1

Description

Formula

Name

Pb2+

Description

Formula

Name

Analysis and Conclusions1. Can mixing a cation and anion lead to the formation of a precipitate, which is an

insoluble ionic compound (one that does not dissolve in water)? Describe what you think is happening.

2. Do you think mixing together a solution of ANY cation with a solution of ANY anion will ALWAYS lead to the formation of a precipitate? Why or why not?

3. How does this lab relate to what we are doing in class?

17

Name

18

19

Name: Date: Period:

If Your Cat Took Chemistry, Would She Eat This Stuff? The following are the listed ingredients for Puss'n'Boots Pounce ( Shrimp Flavor) Treats for Cats:Flour, liver, dried whole egg, glycerin, pregelatinized wheat flour, shrimp by-products, wheat gluten, torula dried yeast, calcium sulfate, cheese meal, phosphoric acid, animal fat (preserved with butylated hydroxyanisole, otherwise known as BHA), potassium chloride, salt, potassium sorbate ( a preservative), wheat middlings, color, choline chloride, calcium carbonate, ferrous sulfate, vitamin E supplement, zinc oxide, BHA ( again!), cupric oxide, cobalt carbonate, manganous oxide, vitamin A supplement, potassium iodide, D-calcium pantothenate, vitamin B-12 supplement, vitamin D-3 supplement, water sufficient for processing.The purpose of this activity is to practice writing formulas for simple inorganic compounds whose names are found on labels of products in the supermarket, drugstore or at home. On your naming card there is a list of ions. You are to read product labels to find compounds formed from the ions on the list. You must have a positive and negative ion for each compound. For each compound, the following information will be required:

Name of compound as it appears on the labelFormulaName of the product in which it is found.

1. Name of compound as it appears on the label -

Formula -

Name of the product in which it is found. –


Formula -



Formula -



Formula -



Formula -



Formula -



Formula -



Formula -

Name of the product in which it is found. -


Formula -



Formula -

Name of the product in which it is found.20

Example:Name of the compound as it appears on the label: Potassium ChlorideFormula: KClName of the product in which it is found: Pounce

Alchemist’s DreamPrelab Questions - Answer in complete sentences!Read section 7.3 (201-203) to answer the following questions.

1) What are metals made up of?

2) Describe the valence electrons in metals

3) Define a metallic bond. Use the info in the text, not the glossary. Include how these bonds are held together.

4) What are some properties of metals? Explain each property.

5) How are metal atoms arranged in metallic compounds?

6) What is an alloy?

7) What is the first example of an alloy given in the book? What is it made of?

8) Why are alloys important?

9) Name and describe (what they are made of) at least three other alloys.Data Table

ConditionAppearance Tape Penny Here

Untreated penny

Penny treated with solution

Penny treated with solution and heated in

flame

21

Post-Lab Analysis: Now that you have completed the lab, answer the following questions based upon your results and your new knowledge.

1) a. Compare the color of the three coins—untreated (the control), heated in solution only, and heated in solution and in the flame.

b. Do the treated coins appear to be composed of metals other than copper? If so, explain.

2) What is the silver color composed of (what metal(s))? Would you consider this a coating or an alloy? Explain.

3) What is the gold color composed of (what metal(s))? Would you consider this a coating or an alloy? Explain.

4) If someone claimed that a precious metal was produced in the activity, how would you decide whether the claim was correct? (Hint: think about different physical and chemical properties of metals)

5) Identify at least two practical (real life…outside of the classroom) uses for metallic changes similar to those you observe in this activity.

6) a. What happened to the copper atoms originally present in the treated pennies? (Give an answer for both treated pennies)

b. Do you think the treated pennies could be converted back to ordinary coins? Explain why or why not for both treated pennies.

22

c. Based on your answer in question 4b, was the change that happened to the treated pennies a physical or chemical change? (I know, we’re going way back to the beginning of the semester, but time to start reviewing for the final! )

23

Name: ________________________Per: _____ Date: _______________

Atoms, Compounds, and Ions1 2

3

4 5

6 7

8 9

10

11

12 13 14

15 16 17

18

19 20

21

ACROSS DOWN4 A positively charged atom. 1 Positively charged subatomic particle.5 The number of neutrons in sodium. 2 Outer most electron shell.6 A solution of known composition used as a 3 The element that does not have a neutron. comparison. (Reference Solution) 7 The chemical name of Fe2(SO4)3.9 The number of electrons in the second energy level. 8 A bond formed when electrons are transferred.10 An ion consisting of a group of atoms. 11 The chemical name of ZnO.12 A test that identifies the contents, not the amount, 13 The basic unit of matter. of a substance or mixture. 14 Orbits the nucleus and has a negative charge.17 Charged atoms. 15 A negatively charged atom.18 Where the protons and neutrons exist. 16 Calculated by subtracting the atomic number 19 The chemical formula for potassium hypochlorite. from the atomic mass.20 A test that confirms the presence of something. (Confirming)21 A bond formed when electrons are shared.

Unit 5 Review – Ionic Compounds 24

1. What is a valence electron?

2. Write the Lewis (electron) dot structure for:a. Al

b. S

c. Li

3. What is the ionization equation for:a. Aluminum

b. Barium

c. Oxygen

d. Chlorine

4. Describe the composition (make up) of an ionic compound, molecular compound, and metallic compound.

5. How many atoms are in:a. Li2CO3 ___________b. C6H12O6 ___________c. Cu3(PO4)2 ___________d. (NH4)3PO3 ___________

6. Naming Practice Give the correct formula for each of the following compounds.a. Sodium oxide ________________________________________

b. Potassium fluoride ________________________________________

c. Iron (II) sulfide ________________________________________

d. Iron (III) chloride ________________________________________

e. Calcium sulfate ________________________________________

f. Ammonium bromide ________________________________________

g. Copper (II) phosphate ________________________________________

h. Lead (II) hydroxide________________________________________

i. Potassium iodide ________________________________________

j. Sodium chloride ________________________________________

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7. Name the following compounds (Stock AND Classical where applicable):

a. Na2O ________________________________________

b. KF ________________________________________

c. FeS ________________________________________

d. FeCl3 ________________________________________

e. CaSO4 ________________________________________

f. NH4Br ________________________________________

g. Cu3(PO4)2 ________________________________________

h. Pb(OH)2 ________________________________________

i. NaHCO3 ________________________________________

j. AgNO3 ________________________________________

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VISTA RIDGE CHEMISTRY **THIS WEBSITE IS NO ...vistaridgechemistry.weebly.com/uploads/4/9/6/4/49648… · Web viewPodcast 5.1 Ionic vs Covalent Read p. 187 – 193; Questions 3-11

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