1 NAME:__________________________________________________ BLOCK:________ SCIENCE 9: CHEMISTRY UNIT I. ATOMIC STRUCTURE B D A E SKILLS 1. I can name the subatomic particles, identify their locations in the atom, relative masses and charges 2. I can calculate the number of subatomic particles given atomic mass &/or atomic number &/or number of neutrons 3. I can describe and define isotopes and write their symbols II. PERIODIC TABLE B D A E 4. I can describe how the modern periodic table is arranged including identifying: metals, non-metals & transition metals and family names 5. I can describe the properties of metals, non-metals and metalloids III. BOHR MODELS B D A E 6. I can draw Bohr models for the first 20 elements 7. I can identify an element’s period & family from a Bohr diagram and predict the # of e- shells and # of valence e- based on its position on the table 8. I can draw Bohr Models for both positive and negative ions 9. I can predict which elements are isoelectronic with which ions IV. BONDING B D A E 10. I can differentiate between ionic and covalent bonds 11. I can draw ionic bonds using Bohr Models 12. I can draw covalent bonds using Bohr Models V. IONIC NOMENCLATURE B D A E I can write formulae and name compounds between: 13. Metals & non-metals 14. Multivalent metals & non-metals 15. Polyatomic ions 16. Non-Metals & other Non-Metals (covalent compounds) 17. All Mixed Together Nomenclature VI. LAB– BAG OF CHANGE B D A E 18. I can safely conduct the experiment and make observations and correctly answer the lab questions 19. I can write a conclusion based on my experiment % Chemistry Exam Result
B D A E SKILLS 1. I can name the subatomic particles, identify their locations in the atom, relative
masses and charges
2. I can calculate the number of subatomic particles given atomic mass &/or atomic number &/or number of neutrons
3. I can describe and define isotopes and write their symbols
II. PERIODIC TABLE
B D A E 4. I can describe how the modern periodic table is arranged including identifying: metals,
non-metals & transition metals and family names
5. I can describe the properties of metals, non-metals and metalloids
III. BOHR MODELS B D A E
6. I can draw Bohr models for the first 20 elements
7. I can identify an element’s period & family from a Bohr diagram and predict the # of e- shells and # of valence e- based on its position on the table
8. I can draw Bohr Models for both positive and negative ions
9. I can predict which elements are isoelectronic with which ions
IV. BONDING B D A E 10. I can differentiate between ionic and covalent bonds
11. I can draw ionic bonds using Bohr Models
12. I can draw covalent bonds using Bohr Models
V. IONIC NOMENCLATURE
B D A E I can write formulae and name compounds between:
13. Metals & non-metals
14. Multivalent metals & non-metals
15. Polyatomic ions
16. Non-Metals & other Non-Metals (covalent compounds)
17. All Mixed Together Nomenclature
VI. LAB– BAG OF CHANGE
B D A E
18. I can safely conduct the experiment and make observations and correctly answer the lab questions
19. I can write a conclusion based on my experiment
% Chemistry Exam Result
2
To Do List This is a list of the activities in this unit. You can check off the activities as you complete them.
√ ACTIVITY FINISH BY DATE
Read the introductory information on the atom in the BC Science 9 text pp.32 & 33
Complete the worksheet: The Atom
Complete the “Build an Atom simulation Part One: Atoms ”with the accompanying worksheet
Complete the “Build an Atom simulation Part Two: Symbols” with the accompanying worksheet
Read the online tutorial(s) on Isotopes
Complete the package worksheet on isotopes
Complete the “Build an Atom simulation Part Three: Isotopes” with the accompanying worksheet
Complete quiz on The Atom (skills #1,2, & 3)
Review the online and textbook information about the periodic table and fill in the notes requested on the blank periodic table
Complete the worksheet Periodic Table of the Elements – Practice
Complete the worksheet REVIEW: The Periodic Table
Listen and participate in a whole-class discussion of the periodic table
Complete quiz on The Periodic Table (skills #4 & 5)
Read the online document about how to draw Bohr Models
Practice by drawing the Bohr models on the Bohr Diagram Template sheet
Complete the questions that follow the diagram practice (Bohr Assignment)
Read the on-line document about how Atoms become Ions. See also BC Science 9 p. 67
Practice worksheet: Atoms and Ions
Read the on-line document about isoelectronic atoms and complete the accompanying questions
Read about Ionic and Covalent Bonds online and in the text on pp. 77 & 78
Make notes comparing and contrasting Ionic and Covalent Bonds
Try the reading check questions on p.79 of BCScience9 (also available online)
With some classmates, answer the true and false questions about bonding contained in the online document, discuss your answers, then check your answers on the bulletin board.
Read the on-line document about drawing ionic bonds and complete the accompanying questions
Complete the worksheet: Drawing Ionic Bonds using Bohr Models
Complete quiz on Bonding (skills #10, 11, & 12)
Listen to your teacher explain how to name/write formulae between metals and non-metals. Work along on the worksheet: Ionic Bonding: A. METAL + NON-METAL
Practice using the laminated worksheets 1(A) and 1(B) using a personal whiteboard OR print yourself a worksheet answer sheet to work on
3
Complete quiz on metal + non-metal nomenclature (skill #13)
Listen to your teacher explain how to name/write formulae between transition metals and non-metals. Work along on the worksheet: Ionic Bonding: B. TRANSITION METAL + NON-METAL
Practice using the laminated worksheets 2(A) and 2(B) using a personal whiteboard
Complete quiz on transition metal + non-metal nomenclature (skill #14)
Listen to your teacher explain how to name/write formulae using polyatomic ions. Work along on the worksheet: Ionic Bonding: C. POLYATOMIC IONS
Practice using the laminated worksheets 3(A) and 3(B) using a personal whiteboard
Complete quiz on polyatomic ion nomenclature (skill #15)
Practice using the laminated worksheets 4(A) and 4(B) where the different types of compounds are combined in one worksheet.
Listen to your teacher explain how to name/write formulae for covalent compounds (two non-metals together). Work along on the worksheet: D. COVALENT COMPOUNDS
Practice using the laminated worksheets 5(A) and 5(B) using a personal whiteboard
Complete quiz on Covalent Nomenclature (skill #16)
Re-do worksheets 4(A) and 4(B) using a personal whiteboard.
Do the “all mixed up” worksheets (available on the website) which have both ionic and covalent compounds mixed together. Practice until you feel confident and you can work very quickly.
Complete quiz on “All Mixed Together” Nomenclature (skill #17)
Read the lab “bag of change” in the textbook on p.17 Obtain a lab worksheet, look it over to become familiar with it, then find a buddy or two
with whom to work and complete the lab. If there are no lab sets available at that moment, see below and come back to the lab later.
Find a study group to work with and come up with a plan to prepare for your Chemistry Unit Test
CHEMISTRY UNIT SUMMATIVE TEST (recall: no re-writes on a Unit Test!)
Beginning Developing Accomplished Exemplary
Does not demonstrate a basic understanding of concepts.
Demonstrates a basic understanding of concepts.
Demonstrates a solid understanding of concepts.
Demonstrates a complete and deep understanding of concepts.
LEVEL Beginning Developing Accomplished Exemplary
LETTER GRADE I/F C-/C C+/B-/B/B+ A-/A/A+
PERCENTAGE 0 30 45 55 60 65 70 75 80 85 90 95 100
% % of Unit
My estimate based on quizzes and assignments:
Mark Assigned by my teacher: 70
My Chemistry Exam mark 30
4
The Atom ( BC Science 9 pp.32&33)
Particle Location in
Atom
Electric Charge Relative Mass*
Symbol
Electron
Proton
Neutron
Definitions:
1. Atomic mass
2. Atomic number
3. Isotope
Use the diagram of an atom to answer the following questions:
1. Label the parts of the atom. Include the following labels: proton, electron, neutron,
energy shell, nucleus.
2. What element is represented by this diagram? How do you know?
3. What is the electric charge of this nucleus? What is the electric charge of this atom?
4. What is the mass of this atom? Does the mass number match the atomic mass on the
periodic table? If not, why not?
5
5. How could you figure out how many neutrons are in a particular atom if you only know
the atomic number and the mass number?
6. Using a periodic table, look up titanium.
(a) What is its atomic number?
(b) How many protons does a titanium atom have?
(c) How many electrons does it have?
7. Give the mass number of each of the following atoms:
(a) beryllium with 5 neutrons (c) gallium with 39 neutrons
(b) titanium with 26 neutrons (d) iron with 30 neutrons
8. Calcium-40 has ____protons, _____neutrons, and ____electrons
Tin -119 has ____protons, _____neutrons, and ____electrons
Carbon-13 has ____protons, _____neutrons, and ____electrons
9. An element has 8 protons and 9 neutrons.
(a) what element is it? ____________________
(b) What is its mass number?______
10. An element has 36 electrons and 46 neutrons.
(a) what element is it? ____________________
(b) How many protons are in on atom of this atom? _____
(c) What is its mass number?______
6
BUILD AN ATOM simulation
PART I: ATOMS Build an Atom simulation (http://phet.colorado.edu/en/simulation/build-an-atom)
1. Explore the Build an Atom simulation with your group. As you explore, talk about what you
found.
2. (a) List two things your group observed in the simulation.
(b) What particle(s) are found in the center of the atom?
3. Play until you discover which particle(s) determine(s) the name of the element you build. What
did you discover?
4. What is the name of the following atoms?
An atom with 3 protons: _______________________
An atom with 2 protons: _______________________
An atom with 4 protons: _______________________
5. What is the name of the following atoms?
An atom with 3 protons and two neutrons: _______________________
An atom with 3 protons and four neturons: _______________________
What can you conclude about the effect of adding neutrons to an atom?
6. Play with the simulation to discover which particles affect the charge of an atom or ion.
Fill in the blanks below to show your results:
a. Neutral atoms have the same number of protons and electrons.
b. Positive ions have ________________________________ protons than electrons.
c. Negative ions have _______________________________ protons than electrons.
7. (a) Develop a relationship (in the form of a single sentence or equation) that can predict the
charge based on the number and types of particle.
(b) What happens to make a neutral atom turn into a negative ion?
8. Play with the simulation to discover what affects the mass number of your atom or ion.
What is a rule for determining the mass number of an atom or ion?
9. Practice applying your understanding by playing 1st and 2nd levels on the game screen.
PART II: SYMBOLS 1. Using the Symbol readout box, figure out which particles affect each component of the atomic symbol.
a) In the atomic symbol below, label each letter (a, b, c, and d) with:
the particle(s) used to determine the letter, and
how the value of each letter is determined.
2. Create a definition (using a complete sentence) for each of these items based on your labels from the atomic symbol above.
a) Element Symbol
b) Charge
c) Atomic Number
d) Mass Number
3. Practice applying your understanding by playing the 3rd and 4th game levels. Play until you can get all the questions correct on the 4th level.
4. In addition to atomic symbol, we can represent atoms by name and mass number. a) Complete the table below:
Symbol Name
Carbon-12
b) Each representation (Symbol and Name) in the table above provides information about the atom. Describe the similarities and differences between the Symbol and Name representations.
The atom: https://www.youtube.com/watch?v=FSyAehMdpyI&list=PL8dPuuaLjXtPHzzYuWy6fYEaX9mQQ8oGr&index=1
ISOTOPES If we added a neutron to the nucleus of an atom, we would change the mass of the atom, but NOT the charge, or the atomic number.
Define ISOTOPE in your notebook
The Complete Nuclear Symbol To write a complete nuclear symbol, the mass number is placed at the upper left (superscript) of the chemical symbol and the atomic number is placed at the lower left (subscript) of the symbol. The complete nuclear symbol for helium−4 is drawn below.
Notation Complete Nuclear Symbol Atomic diagram
Protium: one proton, no neutrons
Hydrogen-1
Deuterium: one proton, one neutron
Tritium: one proton, three neutrons
Watch this video: https://www.youtube.com/watch?v=EboWeWmh5Pg
? How come the periodic table lists chlorine with a mass of 35.5 amu?
We can’t have 0.5 of a proton or 0.5 of a neutron!
The half amu is not from the mass of electrons (0.5 amu ≅ 900 electrons!)
Calculating Average Mass
(% abundance)(atomic mass) + (% abundance)(atomic mass) = Average atomic mass
a) Which particles affect the stability of the nucleus?
b) Which particles do not affect the stability of the nucleus?
2. What are the names of the stable forms of oxygen? a) Oxygen-____
b) Oxygen-____
c) List all of the things that are the same about these atoms (ignore the electrons).
d) List all of the things that are different about these atoms (ignore the electrons).
3. The atoms in the previous question are isotopes of each other. Based on this information, list the requirements for two atoms to be isotopes of each other.
4. Test your understanding of isotopes by examining the relationships between the pairs of atoms
listed below:
Atom 1 Atom 2 Relationship between atom 1 and atom 2
(check all that apply)
Isotopes Same Atom, Not Isotopes of Each Other Different Element
Carbon-12
Isotopes Same Atom, Not Isotopes of Each Other Different Element
Argon-40 Argon-41 Isotopes Same Atom, Not Isotopes of Each Other Different Element
Boron-10 Isotopes Same Atom, Not Isotopes of Each Other Different Element
An atom with 13 protons and 13
neutrons
An atom with 14 protons and 13 neutrons
Isotopes Same Atom, Not Isotopes of Each Other Different Element
6
12C 6
13C
6
12C
5
11B
10
5. The periodic table has a great deal of information about every atom. Using your periodic table, answer the following questions:
a) What is the atomic number of chlorine (Cl)? _____
b) What is the atomic number of tungsten (W)? _____
c) How many protons are there in any Cl atom?_____
d) How many protons are there in any Te atom? _____
e) Can you tell from the periodic table exactly how many neutrons are in an atom?
6. Complete the following table:
Name Symbol Atomic number
Mass Number
Number of neutrons
Number of Electrons
Charge
hydrogen-2 2H 1 2 1 1 0
3H
sodium-22 22Na+ 10
12 24 12
12 25 13
46Ti-2
107Ag
19F-1
carbon-12 6
carbon-13 6
carbon-14 6
carbon-12 7
carbon-12 5
4He
8 8 10
argon-40 18 18
70Ga
70Ga+3
4 9 2
7 8 8
7. To test your knowledge of isotopes, draw arrows between all pairs of atoms in the table above that
are isotopes of each other.
BLANK PERIODIC TABLE
11
DO NOT fill in the names or symbols of elements on this periodic table. The purpose of the blank table is for
you to consolidate notes about the periodic table onto one sheet of paper.
Below is a list of things you can put on your blank table. You may want to colour code the items and use a
legend, write the terms in the appropriate spaces, add notes of your own, use arrows to show trends…use
your imagination!
Metal Alkali Metal Metalloid Period
Liquid metal Non-Metal Alkaline Earth Metal Halogen
Family of One Atomic mass Transition Metal Noble Gases
Family Liquid element Atomic number Period
Try to fit ALL your notes about atoms and the periodic table onto this one sheet now your study
sheet!
Using The Periodic Table
The left-hand column in the chart below contains statements about various elements. Write the name and symbol for the element to which each statement refers.
Description of Element Name of Element Symbol
It is the only gas in group 1.
This inert gas is in period 3.
There is no heavier member of group 2.
This element is the lightest of the halogens.
Group 16 contains this reactive non-metal gas.
The atomic mass of this metal is about 56.
Period 6 contains this group 2 metal.
This is the only liquid halogen.
This metallic element is liquid at room temperature.
Photosynthesis produces this element.
This is the lightest element in period 2.
12
13
Periodic Table of Elements - Practice
Directions: Use the periodic table to fill in the below chart.
Element Symbol
Atomic
Number # of protons
# of
electrons
Atomic
Mass
Rounded
Atomic
Mass
# of Neutrons (show
work) Period
1 Oxygen O 8 8 8 15.999 16 16 - 8 = 8 2
2 Helium
3 Carbon
4 Aluminum
5 Calcium
6 Sodium
7 Potassium
8 Nitrogen
9 Silicon
10 Iron
11 Hydrogen
14
REVIEW: The Periodic Table
Directions: Answer the questions with the proper information using your notes, textbook, the world-
wide interwebs and/or the periodic table.
1. Define “family:
2. What is a period?
3. What is the symbol for the following elements.
a. Magnesium ______ b. Potassium _____ c. Iron ______ d. Copper _____
4. What are the names of the following elements.
a. C _________________________ b. Cl _________________________
c. Au _________________________ d. Sr _________________________
5. In what period are the following elements found?
a. He ______ b. Ge ______ c. Rb ______ d. I ______
6. In what group (family name) are the following elements found?
a. Sulfur _____________________________ b. Ca _____________________________
c. Iodine _____________________________ d. Fe _____________________________
7. List one atom from each of the following "collections:
a. Halogen ______________ b. Halogen ______________
c. Alkali metal ______________ d. Boron family ______________
e. Lanthanide series ______________ f. Alkaline Earth metal ______________
g. Transition metal ______________ h. Nobel gas ______________
8. What is the atomic mass of mercury? __________
9. What is the atomic symbol for silver? __________
10. Ni is the symbol for what element? __________
11. What element has the atomic number 17? __________
15
12. List the symbols for two transition metals. __________
13. Cu, Ag, and Au are all in what group # __________
14. Name two noble gases __________
15. Give the symbol for two halogens. __________
16. What is the symbol for element with atomic number 74? __________
17. What is the atomic mass of copper? __________
18. What is the last element in period 4? __________
19. What is the atomic number of:
a. Calcium _____ Iron _____ Gold _____ Uranium _____
20. What is the Atomic mass of:
b. Calcium _____ Iron _____ Gold _____ Uranium _____
21. How many protons do the following have?
a. Calcium _____ Iron _____ Gold _____ Uranium _____
22. How many electrons do the following have?
a. Calcium _____ Iron _____ Gold _____ Uranium _____
23. Does mercury have more protons and electrons than tin? _________
24. Is mercury a heavier element than tin? _________
25. Does potassium have more electrons than neon? _________
Read the on-line document about Bohr Models
Take notes in your notebook before moving on to do the worksheets.
16
Bohr Diagram Template
H
HYDROGEN
He
HELIUM
Li
LITHIUM
Be
BERYLLIUM
B
BORON
C
CARBON
N
NITROGEN
O
OXYGEN
F
FLUORINE
Ne
NEON
Na
SODIUM
Mg
MAGNESIUM
Al
ALUMINUM
Si
SILICON
P
PHOSPHORUS
S
SULFUR
Cl
CHLORINE
Ar
ARGON
17
BOHR ASSIGNMENT:
Answer the following questions:
1. In what ways are the Bohr model diagrams for the alkali metals similar?
2. Examine the rows of the periodic table. As the rows increase, what happens to the number of electron
shells?
3. How many electrons are there in the outer shell of a sulfur(S) atom?
4. How many electron shells would you expect to find in a sulfur atom?
5. Identify the elements whose Bohr model diagrams are shown below. Write the symbols of the elements
in the spaces provided
6. Examine the Bohr model diagrams below. Highlight the atoms that are stable.
(a) (b) (c) (d) (e)
Why did you choose the one(s) you did?
7. The following Bohr model diagram represents an oxygen atom. Examine the diagram, then answer the
following questions.
(a) why is this not a stable electron arrangement?
(b) what would make this atom stable?
(c) use a different coloured pen to adjust the diagram so that it
shows a stable electron arrangement
18
[
Atom 1 Atom 2 Atom 3 Atom 4
ATOM ELEMENT MASS
NUMBER
PERIOD HOW DO YOU KNOW WHAT PERIOD THE ELEMENT
IS FOUND IN BY LOOKING AT THE BOHR MODEL?
FAMILY STABLE OR
UNSTABLE?
1
2
3
4
RE-DRAW STABLE BOHR DIAGRAMS FOR ANY ATOMS THAT WERE UNSTABLE (AND WRITE THEIR SYMBOL)
Go to our website and read on-line and watch the video about Atoms and Ions
Worksheet: ATOMS AND IONS
1. Use the words from the list to fill in the blanks in the paragraph below.
attract, charge, electron, ionic bond, negative, negatively charged, opposite, positive, positively charged, transferred (a) When an atom gains or loses a(n) ________________, an ion is formed. All ions have a(n) ________________.
(b) Metals tend to form ________________ ions. Non-metals tend to form __________ ions.
(c) When a metal atom reacts with a non-metal atom, one or more electrons are ________________, which results in the formation
of ions. One of these ions will be ________________ and one will be ________________. Because of these ______________ charges, the ions
________________ each other, forming a(n) _________.
2. (a) Draw a model Bohr diagram for lithium in the space provided.
(b) What process or change would turn this lithium atom into an ion?
(c) Would the ion that it forms be positively or negatively charged? Explain.
3. (a) Draw a Bohr model diagram for fluorine in the space provided.
(b) What process or change would turn this fluorine atom into an ion?
(c) Would this ion be positively charged or negatively charged? Explain.
Boron atom Boron ion
Atomic number: Atomic number:
Mass number: Mass number:
Protons: Protons:
Neutrons: Neutrons:
Electrons: Electrons:
Boron atom Boron ion Cation/Anion: Ion symbol:
Nitrogen atom Nitrogen ion
Atomic number: Atomic number:
Mass number: Mass number:
Protons: Protons:
Neutrons: Neutrons:
Electrons: Electrons:
Nitrogen atom Nitrogen ion Cation/Anion: Ion symbol:
20
LAB ACTIVITY: IONS AND ATOMS L
Ionic compounds form when a metal reacts with a non-metal. The reaction creates oppositely charged ions that are chemically different from the original atoms. Some elements are very reactive and form ionic compounds with a variety of elements. Chlorine is an example of a reactive element.
As an element (atom), it is a yellowish-green gas that is extremely corrosive.
It was used as a weapon by both sides of the First World War causing many deaths and casualties, yet the chloride ion is an essential part of nutrition.
It is found as a safe and stable part of many important compounds.
The properties of an element’s atoms are quite different from the properties of an element’s
ions.
In this Investigation, you will compare the properties of an atom and its ion.
Copper (II) chloride is corrosive and poisonous. Take care to avoid drips and wipe up all spills promptly. If any solution splashed on skin or in eyes, flush immediately with plenty of cold water and inform your teacher
Question: Are the properties of an ion different than the properties of an element?
Hypothesis: If aluminum metal is reacted with copper (II) chloride, it will become an aluminum ion, Al3+ and the copper ion, Cu2+, will become copper metal (atoms).
Experimental Design:
In this experiment, you will react an ionic compound with a metal.
You will use your observations of the reaction to compare some of the properties of the metal
ions.
21
Materials:
Safety goggles Copper (II) chloride (CuCl2) 3 x 250-mL beakers Water Graduated cylinder Aluminum foil
Stirring Rod Ring Stand Ring Clamp Funnel Filter Paper
Procedure:
1. Read the Procedure, and create a table to record your observations. 2. Put on your safety goggles.
3. Your teacher will supply you with a beaker that contains approximately 1.0 g of copper
(II) chloride. Observe and record the properties of this compound.
4. Add approximately 100 mL of water and stir until the copper (II) chloride is completely dissolved. Observe and record the properties of the copper (II) chloride solution.
5. Observe and record the properties of the aluminum metal foil.
6. Crumple a foil square and place it in the copper (II) chloride solution and immediately
begin to watch for any changes to the solution or the square of aluminum. Record your observations.
7. Use the stirring rod to ensure that all the foil is submerged. Continue to add small
scraps of foil until the blue-green colour disappears from the solution.
8. Set up the ring stand with the funnel and filter paper, as demonstrated by your teacher.
9. Swirl the solution gently, and then pour it into the funnel, pouring along the stirring rod
as shown in Figure 1. Touch the stirring rod to the spout of the beaker so that the liquid flows down the rod and into the filter cone.
10. When all the solution has been poured, add some water to rinse out the remaining
solids.
11. Allow the filter paper to dry a little by putting it on top of several layers of paper towel. Pour any remaining solutions into the waste container designated by your teacher. Rinse the beaker, stirring rod, and funnel. Return the equipment to your lab basket ready for the next class (or put it away if you are the last block)
12. Observe the solid on the filter paper. Record your observations.
22
Analysis
1. What ions are present in a solution of copper (II) chloride? What colour do you think the copper (II) ions are? Explain.
2. What are the properties of aluminum that confirm it is a metal?
3. What observations convinced you that a chemical reaction was occurring between
the aluminum foil and the copper (II) chloride solution?
4. What happened to the aluminum atoms in the foil? Explain.
5. What happened to the copper (II) ions in the solution? Explain.
6. What happened to the chloride ions in the solution? Explain.
7. Are the ions of a metal very different from the atoms of a metal? Give some
important differences in the properties you observed. 8. Did the Investigation verify the prediction? Why or why not?
9. Some metal ions are serious pollutant if they get into rivers, lakes or oceans. Do you think this method would be a reasonable way to remove copper ions from waste water? Why or why not?
23
NOMENCLATURE - Summary Notes
1. METAL + NON-METAL
metal written first (more electropositive or left-most)
non-metal written second (more electronegative or right-most)
name of the second (non-metal) element modified to end in "ide"
numbers are reduced to the lowest ratio
Zn2+ S2- ZnS Examples: zinc and sulfur …………zinc sulfide
Br- Na+ NaBr
bromine and sodium …..sodium bromide
2. TRANSITION METAL (With More Than One Combining Capacity) + NON-METAL
roman numerals after the metal to indicate the oxidation number.
Same rules as for metal + non-metal (reduce, “ide” ending)
Examples:
Fe2+ with Cl-1 iron (II) chloride Cu+1 with Cl-1 copper (I) chloride
Fe3+ with Cl-1 iron (III) chloride Cu2+ with Cl-1 copper (II) chloride
3. POLYATOMIC IONS
names of ions are capitalized, but names of compounds are not
common polyatomic ions are listed on a table to which you may refer during all homework,
quizzes and tests.
You are not required to memorize the names and formulae, but it is strongly recommended
that you memorize the list of common polyatomic ions below. (failure to do so could cost you a
great deal of valuable time)
Carbonate CO32- Chromate CrO4
2- Phosphate PO43- Ammonium NH4
+
Sulphite SO32- Dichromate Cr2O7
2- Hydroxide OH- Nitrate NO3-
Sulphate SO42- Permanganate MnO4
- Acetate CH3COO- Bisulphate HSO4-
4. HYDROGEN
Some areas of common confusion concerning hydrogen are listed below:
