Unit 2 PacketName

Atoms, Ions and Compounds

Unit 2

Atoms, Ions, and Compounds

Chemistry: Unit 2 Outline: Atoms, Ions and Compounds

Assignment / WB Page Number / Score / Out of
Podcast 2.1 (CB 1-5) / Online / 
Worksheet A / pg 9 / 
Demo: Cathode Ray Tubes / In Class / 
Podcast 2.2 (CB 7-9) / Online / 

Worksheet B

/ Pg 10 / 
Lab: Vegium / Pg 4-6 / 20
Podcast 2.3 (CB 11-19) / Online / 
Worksheet C / Pg 11 / 
Lab: Chemical Names and Formulas Lab - SS / Pg 7-8 / 20
Podcast 2.4 (CB 21-23) / Online / 
Worksheet D / Pg 12-14 / 
Podcast 2.5 (CB 25) / Online / 
Worksheet E / Pg 15-19 / 
Podcast 2.6 (CB 27-29) / Online / 
Worksheet F / Pg 20 / 
Lab: Technology / In Class / 20
Worksheet G / Pg 21 / 
THL: Chemicals Everywhere / Pg 3 / 
Unit 2 Review / Pg 22-23 / 
Unit 2 Exam / In Class / 100

Chemicals, chemicals everywhere!

Throughout the course of this year, it will be essential for you to know how to name different chemicals as well as how to take chemical names and write correct formulas.

For today’s activity, you will walk around the classroom or laboratory to examine several common food labels Careful examination of food labels reveals a wide range of chemical ingredients. However, the food industry may not always use the standardized system of naming accepted by scientists around the world. Thus, you must be able to identify a correctly named chemical on food labels for this activity. Do not include any non-standard names in your data table. From the labels, fill in the following table. Do not repeat the same chemical more than once or use multiple chemicals from the same food item.

Number / Food item / Chemical name / Chemical formula
1
2
3 /
4
5 …
30

For homework:

Find five different food items in your house and write the item, chemical name, and standard chemical formula.

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.

Introduction

Isotopes 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.

Purpose

In 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 record
  3. Weigh each group of veggies and record
  4. Divide the total mass of each isotope group by the count of each group to get the average mass for one isotope
  5. 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 isotope
  7. Add the relative weights and of each isotope to get the “atomic mass” of the element vegium

Vegium LabName: ______

Period: _____

Data Table:

Isotope / Total number of each isotope / Mass of isotopes counted / Average mass of one piece of isotope / Percent
abundance (decimal) / Relative mass
Veggie 1
______
Veggie 2
______
Veggie 3
______

Total

/

X

/

X

/ 1.00 / Average Atomic Mass

Questions:

  1. Define isotope. Sub-atomically how do isotopes of an element differ? How are they the same?
  1. What are the three isotopes of vegium? What is the average mass of each?
  1. Compare your average atomic mass with a classmate. Are they exactly the same? Explain.
  1. 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?
  1. 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.

Chemical Names and Formula Lab

Purpose

To practice naming and formula writing of ionic compounds

To observe and describe visible properties of ionic compounds in solution

Procedure

  1. 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 provided
  3. 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
(Fe+3) / KI
(I1-) / NaOH
(OH1-) / Na2CO3
CO32- / Na3PO4
(PO43-)
AgNO3
(Ag1+)
Pb(NO3)2
(Pb2+) /
CuSO4
(Cu2+) /
MgSO4
(Mg2+) /

FeCl3
(Fe+3) /

Questions

  1. Write the formulas (with charges) and names of all the ions used in this investigation.
  1. When are Roman numerals used?
  1. What does a numerical subscript following an element in a chemical formula mean?
  1. What does a numerical subscript following a set of parentheses in a chemical formula mean?
  1. Write the rules for naming an ionic compound.
  1. Write the rules for writing the formula for an ionic compound.

WS A – 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. Would you expect two electrons to attract or repel each other?

3. Why is an atom electrically neutral?

4. How many protons are in the nuclei of the following atoms?

a. Phosphorus

b. Molybdenum

c. Aluminum

d. Cadmium

e. Chromium

f. Lead

5. Complete this table.

Atomic Number / Mass number / Number of protons / Number of neutrons / Number of electrons / Symbol of element
9 / 10
14 / 15
47 / 25
55 / 25

WS B – Isotopes and 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?

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 down into the nucleus, and those you would see looking our from the nucleus.

WS C –Ions and Molecules

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

a. Br-

b. Na+

c. As3_

d. Ca2+

e. Cu+

f. H-

2. Identify the number and kinds of atoms present in a molecule of each compound.

a. Ascorbic acid (citamin C) C6H8O6

b. Monosodium glutamate (MSG) C5H8O4Na

c. Sucrose (table sugar) C12H22O11

d. Trinitrotoluene (TNT) C7H5N3O6

e. 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. Lithium ion

d. Nitride ion

e. Copper(II) ion

f. 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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Atoms, Ions and Compounds

WS D – Writing and Naming Ionic Compounds

Part A

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Atoms, Ions and Compounds

Instructions: 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

  1. Sodium Chloride
  2. Strontium Sulfide
  3. Magnesium Fluoride
  4. Rubidium Iodide
  5. Cesium Sulfide
  6. Radium Oxide
  7. Barium Phosphide
  8. Aluminum Bromide
  9. Aluminum Sulfide
  10. Aluminum Nitride
  11. Barium Fluoride
  12. Lithium Oxide
  13. Sodium Iodide
  14. Beryllium chloride
  15. Strontium Nitride

Name the following Compounds

  1. NiCl2
  2. NiCl3
  3. CoCl2
  4. CrN
  5. Cr2O3
  6. AgCl
  7. Ag2O
  8. FeCl3
  9. FeCl2
  10. HgO
  11. HgF2
  12. CdS
  13. Cd3P2
  14. WF5
  15. W2O5

Write the formulas

  1. Iron II Bromide
  2. Copper I Oxide
  3. Copper II Oxide
  4. Zinc II Iodide
  5. Cobalt II Chloride
  6. Manganese IV Oxide
  7. Lead II Sulfide
  8. Lead IV Sulfide
  9. Tin II Nitride
  10. Tin IV Nitride
  11. Gold I Sulfide
  12. Tungsten V Iodide
  13. Zirconium IV Fluoride
  14. Scandium III Nitride
  15. Scandium III Bromide

Write the Names

  1. Cs2S
  2. SrBr2
  3. VCl2
  4. FeO
  5. Fe2O3
  6. BaBr2
  7. CaI2
  8. NiO
  9. Ni2O
  10. MgS

Write the formulas

  1. Platinum IV Sulfide
  2. Potassium Bromide
  3. Copper II Phosphide
  4. Tungsten V Iodide
  5. Potassium Selenide
  6. Cesium Nitride
  7. Chromium III Iodide
  8. Strontium Fluordie
  9. Iron II Phosphide
  10. Cobalt II Iodide

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WS E – Writing and Naming Ionic Compounds Part 2

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Name the following

  1. NaNO3
  2. Ba(CN)2
  3. Li2SO4
  4. K3PO4
  5. Cs(CH3COO) or Cs(C2H3O2)
  6. Mg(NO2)2
  7. CaCO3
  8. Sr3(PO4)2
  9. NaHCO3
  10. KOH

Write the formula

  1. Barium chlorate
  2. Magnesium acetate
  3. Barium Sulfate
  4. Potassium chlorite
  5. Sodium Nitrite
  6. Sodium hydroxide
  7. Magnesium hydroxide
  8. Calcium phosphate
  9. Aluminum phosphite
  10. Zinc sulfate

Name the following

  1. CuNO3
  2. Ni2SO4
  3. Cd(OH)2
  4. ZnSO3
  5. ScPO4
  6. Pb(CN)4
  7. Cr2(CO3)3
  8. Sn(CH3COO)4 or Sn(C2H3O2)4
  9. NH4NO3
  10. (NH4)2O

Write the formula

  1. Nickel II Nitrite
  2. Iron III chlorate
  3. Titanium IV sulfate
  4. Cadmium II hydroxide
  5. Lead II carbonate
  6. Lead IV carbonate
  7. Molybdenum IV hydroxide
  8. Silver I phosphate
  9. Gold I bicarbonate or Gold I hydrogen carbonate
  1. Tungsten V phosphite

Name the following:

  1. Co(NO3)2
  2. Ca(NO3)2
  3. Pt(HCO3)2
  4. PbSO4
  5. NH4CN
  6. (NH4)3PO4
  7. Li2SO3
  8. HgOH
  9. Hg(OH)2
  10. Bi2(SO4)3

Write the formula

  1. Potassium nitrate
  2. Iron II sulfate
  3. Iron III sulfate
  4. Nickel II hydrogen carbonate or bicarbonate
  1. Strontium phosphate
  2. Aluminum chlorate
  3. Copper I carbonate
  4. Lead II nitrate
  5. Lead IV nitrate
  6. Sodium acetate

Name the following:

  1. MgO
  2. Sr(NO3)2
  3. (NH4)2S
  4. Na3P
  5. Na3PO4
  6. Cu3P
  7. Cu3PO4
  8. Cd(OH)2
  9. BaCO3
  10. Cr2O3

Write the formula

  1. Silver I nitrate
  2. Sodium carbonate
  3. Cobalt II nitrite
  4. Ammonium hydroxide
  5. Chromium III cyanide
  6. Zinc II chlorite
  7. Scandium III nitrite
  8. Barium bicarbonate
  9. Lead II oxide
  10. Lead IV oxide

Name the following

  1. N2O5
  2. CO2
  3. C2O4
  4. P4O10
  5. CI4
  6. CCl4

Write the Formula

87.Carbon Tetrabromide

  1. diphosphorous pentaoxide
  2. sulfur hexafluoride
  3. Selenium disulfide
  4. Arsenic triiodide
  5. silicon tetrabromide
  6. Nitrogen triiodide
  7. Selenium pentaflouride

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WS F – Writing and Naming Covalent Compounds

Name These Covalent Compounds

  1. CO2
  2. CO
  3. SO2
  4. SO3
  5. N2O
  6. NO
  7. N2O3
  8. NO2
  9. N2O4
  10. N2O5
  11. PCl3
  12. PCl5
  13. NH3
  14. SCl6
  15. P2O5
  16. CCl4
  17. SiO2
  18. CS2
  19. OF2
  20. PBr3

WS G – Writing and Naming Acids

Name These Acids

  1. HNO3
  2. HCl
  3. H2CO4
  4. H2SO3
  5. HC2H3O2
  6. CH3COOH
  7. HBr
  8. HNO2
  9. H3PO4
  10. H2S
  11. H2CO3
  12. HClO4

Write the Formula for These Acids

  1. 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
  11. chloric acid
  12. chlorous acid

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
Dalton
Electron
Rutherford
Electron Shells

4.

Particle

/ Charge / Location in Atom
Proton
Neutral
Negative

5.

Atomic Number / Mass Number / Number of Protons / Number of Neutrons / Number of Electrons / Symbol of Element
10 / 12
18 / 20
51 / 25
58 / 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).

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.

9. Define “atomic mass unit”

Name or write the formula:

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Atoms, Ions and Compounds

  1. CaCl2
  2. BaF2
  3. BeO
  4. Na2S
  5. AlP
  6. Cesium Sulfide
  7. Radium Oxide
  8. Barium Phosphide
  9. Aluminum Bromide
  10. CoCl
  11. Cr2O3
  12. AgCl
  13. FeCl3
  14. FeCl2
  15. Iron II Bromide
  16. Copper I Oxide
  17. Copper II Oxide
  18. Zinc II Iodide
  19. Cobalt II Chloride
  20. Lead II Sulfide
  21. N2O4
  22. CO2
  23. ClF4
  24. diphosphorus pentoxide
  25. dinitrogen monixide
  26. carbon tetrafluoride
  27. HF
  28. HClO3
  29. H2SO3
  30. nitrous acid
  31. sulfuric acid
  32. hydrobromic acid
  33. ZnCO3
  34. K2SO4
  35. Cu(ClO3)2
  36. sodium sulfate
  37. iron III hydroxide
  38. magnesium phosphate

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