Unit 2 Packet
Atoms, Ions and Compounds
Name
Unit 2
Atoms, Ions, and Compounds
Page 1 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
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 Atom
Worksheet 2.1
Demo: Cathode Ray Tubes
Podcast 2.2 Counting Sub-Atomic Particles
Worksheet 2.2
Podcast 2.3: Isotopes and Average Atomic Mass
Worksheet 2.3
Lab: Vegium
Podcast 2.4: Introduction to the Periodic Table
Worksheet 2.4
Podcast 2.5: Intro to Bonding
Worksheet 2.5
Types of Bonding Labette
Podcast 2.6: Ionic Charge and Polyions
Worksheet 2.6
Lab: Chemical Names and Formulas Lab - SS
Podcast 2.7: Naming Ionic (Binary Compounds)
Worksheet 2.7 (Long)
Podcast 2.8: Naming Ionic (With Polyions—Long)
Podcast 2.9: Naming Molecular Compounds
Worksheet 2.9
Podcast 2.10: Naming Acids
Worksheet 2.10
Unit 2 Review
Unit 2 Exam
Page 2 of 23
Yes
Yes
Yes
Yes
Yes
√
Unit 2 Packet
Atoms, Ions and Compounds
Name
Unit 2 Vocabulary: Atoms Ions and Compounds
Atom
Electrons
Cathode Ray
Protons
Neutrons
nucleus
Atomic Number
Mass Number
Isotope
atomic mass
atomic mass unit
molecule
molecular compounds
ionic compounds
molecular compounds
ionic compounds
monatomic ion
ions
cation
anions.
chemical formula
molecular formula
formula unit.
polyatomic ions.
binary compound.
Page 3 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
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
Page 4 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
Vegium Lab
Data Table:
Isotope
Name: ______________
Period: _____
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?
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.
Page 5 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
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)
Page 6 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
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
(Cl-)
KI
(I1-)
NaOH
(OH1-)
AgNO3
(Ag1+)
Pb(NO3)2
(Pb2+)
CuSO4
(Cu2+)
MgSO4
(Mg2+)
Do not mix
these
combos
FeCl3
(Fe+3)
Page 7 of 23
Na2CO3
(CO32-)
Na3PO4
(PO43-)
Unit 2 Packet
Atoms, Ions and Compounds
Name
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?
Page 8 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
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 Particles
1. 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
9
Mass
number
Number of
protons
14
47
55
Number of
neutrons
10
15
25
25
Page 9 of 23
Number of
electrons
Symbol of
element
Unit 2 Packet
Atoms, Ions and Compounds
Name
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.
82p
122n
1.37%
82p
124n
26.26%
82p
125n
20.82%
82p
126n
51.55%
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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Unit 2 Packet
Atoms, Ions and Compounds
Name
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.
Page 11 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
WS 2.5: Introduction to Bonding
1. For each of the following compounds list them either as ionic, metallic, or covalent
Compound Ionic, Metallic, Covalent
Ag2O
O2
NH3
Ag
Fe
NaCl
Fe2(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. Brb. Na+
c. As3d. 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.”
Page 12 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
WS 2.7: Writing and Naming Ionic Compounds
Part A
Instructions: name the following
1. CaCl2
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
2. AlCl3
3. BaF2
4. BeO
5. Na2S
6. AlP
7. Na3P
8. Cs2S
9. Mg3P2
10.
11.
12.
13.
14.
15.
CsF
AlBr3
Ca2C
K2O
Cs2O
SrI2
Page 13 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
Name the following Compounds
Write the formulas
31.
NiCl2
44.
Iron II Bromide
32.
NiCl3
45.
Copper I Oxide
33.
CoCl2
46.
Copper II Oxide
34.
CrN
47.
Zinc II Iodide
35.
Cr2O3
48.
Lead IV Sulfide
36.
Ag2O
49.
Tin II Nitride
37.
FeCl3
50.
Tin IV Nitride
38.
FeCl2
51.
Gold I Sulfide
39.
HgO
52.
Tungsten V Iodide
40.
CdS
53.
Zirconium IV Fluoride
41.
Cd3P2
54.
Scandium III Nitride
42.
WF5
55.
Scandium III Bromide
43.
W2O5
Page 14 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Write the Names
Name
Write the formulas
56.
Cs2S
64.
Platinum IV Sulfide
57.
SrBr2
65.
Potassium Bromide
58.
VCl2
66.
Copper II Phosphide
59.
FeO
67.
Chromium III Iodide
60.
Fe2O3
68.
Strontium Fluordie
61.
NiO
69.
Iron II Phosphide
62.
Ni2O
70.
Cobalt II Iodide
63.
MgS
Page 15 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
WS 2.8 – Writing and Naming Ionic Compounds With Polyions
Name the following
1. NaNO3
2. Ba(CN)2
17.
Calcium phosphate
18.
Aluminum phosphite
Name the following
3. Li2SO4
19.
Ni2SO4
4. K3PO4
20.
Cd(OH)2
5. Cs(C2H3O2)
21.
ZnSO3
6. Mg(NO2)2
22.
ScPO4
7. CaCO3
23.
Pb(CN)4
8. Sr3(PO4)2
24.
Cr2(CO3)3
9. NaHCO3
25.
Sn(CH3COO)4
10.
26.
NH4NO3
27.
(NH4)2O
KOH
Write the formula
11.
Barium chlorate
12.
Magnesium acetate
13.
Barium Sulfate
14.
Potassium chlorite
15.
Sodium hydroxide
16.
Magnesium hydroxide
Page 16 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
Write the formula
44.
Iron III sulfate
28.
Nickel II Nitrite
45.
Strontium phosphate
29.
Iron III chlorate
46.
Aluminum chlorate
30.
Titanium IV sulfate
47.
Copper I carbonate
31.
Lead II carbonate
48.
Lead II nitrate
32.
Lead IV carbonate
49.
Lead IV nitrate
33.
Silver I phosphate
50.
Sodium acetate
34.
Tungsten V phosphite
Name the following:
Name the following:
51.
MgO
35.
Co(NO3)2
52.
Sr(NO3)2
36.
Ca(NO3)2
53.
(NH4)2S
37.
PbSO4
54.
Na3P
38.
NH4CN
55.
Cu3P
39.
(NH4)3PO4
56.
Cu3PO4
40.
Hg(OH)2
57.
Cd(OH)2
41.
Bi2(SO4)3
58.
BaCO3
Write the formula
42.
Potassium nitrate
43.
Iron II sulfate
Page 17 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
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
Page 18 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
WS 2.8: Naming Molecular
Write the Formula
Compounds
7. Carbon Tetrabromide
1. N2O5
8. sulfur hexafluoride
2. CO2
9. Selenium disulfide
3. C2O4
10.
Arsenic triiodide
4. P4O10
11.
silicon tetrabromide
5. CI4
12.
Nitrogen triiodide
6. CCl4
13.
Selenium pentaflouride
Page 19 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
WS 2.10 – Writing and Naming Acids
Name These Acids
1. HNO3
2. HCl
3. H2CO3
4. HC2H3O2
5. CH3COOH
6. HBr
7. HNO2
8. H3PO4
9. H2S
10. 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
Page 20 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
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
Dalton
Discovery/Contribution
Atomic Model
Electron
Rutherford
Electron Shells
4.
Particle
Charge
Location in Atom
Proton
Neutral
Negative
5.
Atomic
Number
10
Mass
Number
Number of
Protons
18
51
58
Number of
Neutrons
12
20
25
Number of
Electrons
Symbol of
Element
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).
Page 21 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
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
89. Cobalt II Chloride
72. BaF2
90. Lead II Sulfide
73. BeO
91. N2O4
74. Na2S
92. CO2
75. AlP
93. ClF4
76. Cesium Sulfide
94. diphosphorus pentoxide
77. Radium Oxide
95. dinitrogen monixide
78. Barium Phosphide
96. carbon tetrafluoride
79. Aluminum Bromide
97. HF
80. CoCl
98. HClO3
81. Cr2O3
99. H2SO3
82. AgCl
100.
nitrous acid
83. FeCl3
101.
sulfuric acid
84. FeCl2
102.
hydrobromic acid
85. Iron II Bromide
86. Copper I Oxide
87. Copper II Oxide
88. Zinc II Iodide
Page 22 of 23
Unit 2 Packet
Atoms, Ions and Compounds
Name
Page 23 of 23