What experimental evidence did Thompson have for … · Web viewName the following: Co(NO 3) 2...

Unit 2 Packet NameAtoms, Ions and Compounds

Unit 2Atoms, Ions, and Compounds

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Chemistry: Unit 2 Outline: Atoms, Ions and Compounds

Assignment Can only be done in class? √

Unit 2 Vocabulary (Can be done over the course of the unit)Podcast 2.1: History of the AtomWorksheet 2.1Demo: Cathode Ray Tubes YesPodcast 2.2 Counting Sub-Atomic ParticlesWorksheet 2.2Podcast 2.3: Isotopes and Average Atomic MassWorksheet 2.3Lab: Vegium YesPodcast 2.4: Introduction to the Periodic TableWorksheet 2.4Podcast 2.5: Intro to BondingWorksheet 2.5Types of Bonding Labette YesPodcast 2.6: Ionic Charge and PolyionsWorksheet 2.6Lab: Chemical Names and Formulas Lab - SS YesPodcast 2.7: Naming Ionic (Binary Compounds)Worksheet 2.7 (Long)Podcast 2.8: Naming Ionic (With Polyions—Long)Podcast 2.9: Naming Molecular CompoundsWorksheet 2.9Podcast 2.10: Naming AcidsWorksheet 2.10Unit 2 ReviewUnit 2 Exam Yes

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Unit 2 Vocabulary: Atoms Ions and Compounds

AtomElectronsCathode RayProtons NeutronsnucleusAtomic Number Mass NumberIsotope atomic massatomic mass unitmoleculemolecular compoundsionic compoundsmolecular compoundsionic compoundsmonatomic ionionscationanions.chemical formulamolecular formulaformula unit.polyatomic ions.binary compound.

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Vegium (isotope lab)

Objectives - Determine the average weights of each isotope of the fictitious element vegium. - Determine the relative abundances of isotopes of vegium. - Calculate from experimental data the atomic mass of vegium.

IntroductionIsotopes are atoms of the same atomic number which have different atomic masses

because they have different numbers of neutrons. The atomic mass of an element is calculated by finding the weighted average of the masses of the isotopes of that element. The weighted average takes into account both the mass and relative abundance of each isotope as it occurs in nature. Relative abundance and mass of small atomic particles are measured in the laboratory by an instrument called a mass spectrometer. The mass spectrometer separates particles by mass and measures the mass and relative abundance of each. From this data a weighted average is calculated to determine the atomic mass of the element.

PurposeIn this lab you will carry out experiments and perform the necessary calculations to

determine the atomic mass of the fictitious element vegium. The three different isotopes are represented by different kinds of dried vegetables. As in real elements, these isotopes are collections of particles having different masses. Your job will be to obtain a sample of vegium and determine the relative abundance of each isotope and the mass of each type of particle. From these data, you will calculate the weighted average mass, or atomic mass, of vegium. Unlike real isotopes, the individual isotopic particles of vegium differ slightly in mass, so you will determine the average mass of each type of isotopic particle. Then you can calculate the weighted average mass, or “atomic mass”, of vegium.

Procedure

Carry out the following steps and record your results in your data table.

1. Separate the sample of vegium into piles of each of the three isotopes (types of vegetables)

2. Count the number of veggies in each group and record3. Weigh each group of veggies and record4. Divide the total mass of each isotope group by the count of each group to get the average

mass for one isotope5. To get percent abundance, divide the number of each isotope by the total number of

isotopes counted (record percent abundance as a decimal Ex: 53% = 0.53)6. Multiply the decimal abundance by the average mass of each isotope to get the relative

weight of each isotope7. Add the relative weights and of each isotope to get the “atomic mass” of the element

vegium

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Vegium Lab Name: ______________

Period: _____Data Table:Isotope Total

number of each isotope

Mass of isotopes counted

Average mass of one piece of isotope

Percentabundance (decimal)

Relative mass

Veggie 1

________

Veggie 2

________

Veggie 3

________

Total X X 1.00Average

Atomic Mass

Questions:1. Define isotope. Sub-atomically how do isotopes of an element differ? How are they the

same?

2. What are the three isotopes of vegium? What is the average mass of each?

3. Refer to the periodic table. Why are the average atomic mass of H (#1) thru Bi (#83) generally not whole numbers? Why are Pu (#94) thru Und (#110) whole numbers?

4. This is a good analogy of the relative abundances of different isotopes of the same element. What is wrong with this analogy? Think about the isotopes used here and how they are different in from the isotopes of elements found in nature.

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Types of Bonding Lab

At the lab station there are several different chemicals that are both elements and compounds. Fill in the table below:

Name of Chemical Formula Type of bonding (Ionic, Covalent, Metallic)

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Chemical Names and Formula Lab

PurposeTo practice naming and formula writing of ionic compoundsTo observe and describe visible properties of ionic compounds in solution

Procedure1. Carefully place the drops in the center of the squares on the reaction grid. Place the plastic “flimsy” over

(not in) the surface.2. Record your observation in the square provided3. Write down the formula of the chemical that was made. Use the Ion and the charge to determine the

formula of the observed compound.4. Write the name of the compound formed

FeCl3

(Cl-)KI(I1-)

NaOH(OH1-)

Na2CO3

(CO32-)

Na3PO4

(PO43-)

AgNO3

(Ag1+)

Pb(NO3)2

(Pb2+)

CuSO4

(Cu2+)

MgSO4

(Mg2+)

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Do not mix these combos


FeCl3

(Fe+3)

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Questions

1. When are Roman numerals used?

2. What does a numerical subscript following an element in a chemical formula mean?

3. What does a numerical subscript following a set of parentheses in a chemical formula mean?

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WS 2.1: History of the Atomic Theory – Atomic Theory and Atomic Structure

1. What experimental evidence did Thompson have for each statement?a. Electrons have a negative charge

b. Atoms of all elements contain electrons

2. Describe how small atoms are.

3. List three atoms and their atomic number and atomic mass.

WS 2.2: Counting Sub Atomic Particles1. Would you expect two electrons to attract or repel each other? Explain

2. Why is an atom electrically neutral?

3. Complete this table.Atomic Number

Mass number

Number of protons

Number of neutrons

Number of electrons

Symbol of element

9 1014 15

47 2555 25

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WS 2.3: Isotopes and Average Atomic Mass

1. Name two ways that isotopes of an element differ.

2. What data must you know about the isotopes of an element to calculate the atomic mass of the element?

3. The four isotopes of lead are shown below, each with its percent by mass abundance and the composition of its nucleus. Using these data, calculate the approximate atomic mass of lead.

4. Lithium has two naturally occurring isotopes. Lithium-6 has an atomic mass of 6.015 amu; lithium-7 has an atomic mass of 7.016 amu. The atomic mass of lithium is 6.941 amu. What is the percentage of naturally occurring lithium-7? (Make Li-6’s percent abundance x and Li-7’s percent abundance 1-x)

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82p122n1.37%

82p124n26.26%

82p125n20.82%

82p126n51.55%


5. What is the atomic mass of an element, and how does it differ from the mass number?

6. Imagine you are standing on top of a boron-11 nucleus. Describe the numbers and kinds of subatomic particles you would see looking down into the nucleus, and those you would see looking out from the nucleus.

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WS 2.5: Introduction to Bonding

1. For each of the following compounds list them either as ionic, metallic, or covalentCompound Ionic, Metallic, CovalentAg2OO2

NH3

AgFeNaClFe2(SO4)3

W2(CO3)5

NH4Cl

WS 2.6: Ionic Charge and Polyions

1. State the number of electrons either lost or gained in forming each ion.a. Br-

b. Na+

c. As3-

d. Ca2+

e. Cu+

2. Identify the number and kinds of atoms present in a molecule of each compound.a. Ascorbic acid (vitamin C) C6H8O6

b. Monosodium glutamate (MSG) C5H8O4Na

c. Sucrose (table sugar) C12H22O11

d. Ammonium nitrate (fertilizer) NH4NO3

3. Write the symbol for each ion. Be sure to include the charge.a. Oxide ion

b. Lead(II) ion

c. Nitride ion

d. Copper(II) ion

e. Fluoride ion

4. Criticize this statement: “the ionic charge of any metal can be determined from the position of the element in the periodic table.”

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WS 2.7: Writing and Naming Ionic Compounds

Part AInstructions: name the following

1. CaCl2

2. AlCl3

3. BaF2

4. BeO

5. Na2S

6. AlP

7. Na3P

8. Cs2S

9. Mg3P2

10. CsF

11. AlBr3

12. Ca2C

13. K2O

14. Cs2O

15. SrI2

Write the formulas

16. Sodium Chloride

17. Strontium Sulfide

18. Magnesium Fluoride

19. Rubidium Iodide

20. Cesium Sulfide

21. Radium Oxide

22. Barium Phosphide

23. Aluminum Bromide

24. Aluminum Sulfide

25. Aluminum Nitride

26. Barium Fluoride

27. Lithium Oxide

28. Sodium Iodide

29. Beryllium chloride

30. Strontium Nitride

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Name the following Compounds

31. NiCl2

32. NiCl3

33. CoCl2

34. CrN

35. Cr2O3

36. Ag2O

37. FeCl3

38. FeCl2

39. HgO

40. CdS

41. Cd3P2

42. WF5

43. W2O5

Write the formulas

44. Iron II Bromide

45. Copper I Oxide

46. Copper II Oxide

47. Zinc II Iodide

48. Lead IV Sulfide

49. Tin II Nitride

50. Tin IV Nitride

51. Gold I Sulfide

52. Tungsten V Iodide

53. Zirconium IV Fluoride

54. Scandium III Nitride

55. Scandium III Bromide

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Write the Names

56. Cs2S

57. SrBr2

58. VCl2

59. FeO

60. Fe2O3

61. NiO

62. Ni2O

63. MgS

Write the formulas

64. Platinum IV Sulfide

65. Potassium Bromide

66. Copper II Phosphide

67. Chromium III Iodide

68. Strontium Fluordie

69. Iron II Phosphide

70. Cobalt II Iodide

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WS 2.8 – Writing and Naming Ionic Compounds With PolyionsName the following

1. NaNO3

2. Ba(CN)2

3. Li2SO4

4. K3PO4

5. Cs(C2H3O2)

6. Mg(NO2)2

7. CaCO3

8. Sr3(PO4)2

9. NaHCO3

10. KOH

Write the formula

11. Barium chlorate

12. Magnesium acetate

13. Barium Sulfate

14. Potassium chlorite

15. Sodium hydroxide

16. Magnesium hydroxide

17. Calcium phosphate

18. Aluminum phosphite

Name the following

19. Ni2SO4

20. Cd(OH)2

21. ZnSO3

22. ScPO4

23. Pb(CN)4

24. Cr2(CO3)3

25. Sn(CH3COO)4

26. NH4NO3

27. (NH4)2O

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Write the formula

28. Nickel II Nitrite

29. Iron III chlorate

30. Titanium IV sulfate

31. Lead II carbonate

32. Lead IV carbonate

33. Silver I phosphate

34. Tungsten V phosphite

Name the following:

35. Co(NO3)2

36. Ca(NO3)2

37. PbSO4

38. NH4CN

39. (NH4)3PO4

40. Hg(OH)2

41. Bi2(SO4)3

Write the formula

42. Potassium nitrate

43. Iron II sulfate

44. Iron III sulfate

45. Strontium phosphate

46. Aluminum chlorate

47. Copper I carbonate

48. Lead II nitrate

49. Lead IV nitrate

50. Sodium acetate

Name the following:

51. MgO

52. Sr(NO3)2

53. (NH4)2S

54. Na3P

55. Cu3P

56. Cu3PO4

57. Cd(OH)2

58. BaCO3

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Write the formula

59. Silver I nitrate

60. Sodium carbonate

61. Cobalt II nitrite

62. Ammonium sulfide

63. Ammonium phosphate

64. Ammonium hydroxide

65. Iron III chloride

66. Magnesium oxide

67. Potassium perchlorate

68. Zinc II chlorite

69. Scandium III nitrite

70. Barium bicarbonate

71. Lead II oxide

72. Lead II hydroxide

73. Lead IV oxide

74. Lead IV hydroxide

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WS 2.8: Naming Molecular

Compounds

1. N2O5

2. CO2

3. C2O4

4. P4O10

5. CI4

6. CCl4

Write the Formula

7. Carbon Tetrabromide

8. sulfur hexafluoride

9. Selenium disulfide

10. Arsenic triiodide

11. silicon tetrabromide

12. Nitrogen triiodide

13. Selenium pentaflouride

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WS 2.10 – Writing and Naming Acids

Name These Acids1. HNO3

2. HCl

3. H2CO3

4. HC2H3O2

5. CH3COOH

6. HBr

7. HNO2

8. H3PO4

9. H2S

10. HClO4

Write the Formula for These Acids1. sulfuric acid

2. nitric acid

3. hydrochloric acid

4. acetic acid

5. hydrofluoric acid

6. phosphorous acid

7. carbonic acid

8. nitrous acid

9. phosphoric acid

10. hydrosulfuric acid

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Unit 2 Review

Chemistry

1. How are the properties of a compound related to the properties of the elements from which it is made?.

2. What is the smallest particle of an element that still retains the properties of the element?

3.Name of Scientist Discovery/Contribution Atomic Model

DaltonElectron

RutherfordElectron Shells

4.Particle Charge Location in Atom

ProtonNeutral

Negative

5.Atomic Number

Mass Number

Number of Protons

Number of Neutrons

Number of Electrons

Symbol of Element

10 1218 20

51 2558 27

6. Isotopes of an element have the same number of ____________ but a different number of ___________.

7. Describe the relationship between elements in the same family (column).

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8. The element copper has two isotopes: copper-63 and copper-65. The relative abundance and atomic masses are 69.2% for mass = 62.93 amu, and 30.8% for mass = 64.93 amu. Calculate the average atomic mass of copper.

8. Define “atomic mass unit”

Name or write the formula:

71. CaCl2

72. BaF2

73. BeO

74. Na2S

75. AlP

76. Cesium Sulfide

77. Radium Oxide

78. Barium Phosphide

79. Aluminum Bromide

80. CoCl

81. Cr2O3

82. AgCl

83. FeCl3

84. FeCl2

85. Iron II Bromide

86. Copper I Oxide

87. Copper II Oxide

88. Zinc II Iodide

89. Cobalt II Chloride

90. Lead II Sulfide

91. N2O4

92. CO2

93. ClF4

94. diphosphorus pentoxide

95. dinitrogen monixide

96. carbon tetrafluoride

97. HF

98. HClO3

99. H2SO3

100. nitrous acid

101. sulfuric acid

102. hydrobromic acid

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What experimental evidence did Thompson have for … · Web viewName the following: Co(NO 3) 2...

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