Atoms, Elements and Compounds Student Pages:

Chemistry dictionary reference pages0001Chemistry dictionary reference pages0002Chemistry dictionary reference pages0003Chemistry dictionary reference pages0004Science Experiment Lab ReportAnother Chemical ReactionIon GizmoSubatomic Particle GizmoCW Models of Atom CombinationsElements MatchingDiffusion Experiment0001Diffusion Experiment0002Diffusion Experiment0003Lesson on Naming CompoundsNaming Compounds WorksheetChemical Bonding Terms matching quizPhysical and Chemical Change WorksheetModels of Acids and Bases0001Models of Acids and Bases0002

SCIENCE EXPERIMENT WORKSHEET

Name: _______________________________________Grade: ______________________

Project Title: _____________________________________________________________

Statement of the problem (Ask a Testable Question):_____________________________

_________________________________________________________________________

Hypothesis (Prediction: what I think will happen): ________________________________

_________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

Plan the Experiment (Rough Draft): __________________________________________

_________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

Equipment and materials (List the Materials): __________________________________

_________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

Procedure (What I plan to do): _______________________________________________

_________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

Record Data and Observations: _____________________________________________

_________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

Interpret Data and Observations: _________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

Conclusion (What I found out by doing this experiment): ___________________________

_________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

Apply Findings (How can the results of the experiment be used): ____________________

_________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

_________________________________________________________________________

Attach notes, measurements, photos, tables or graphs to this sheet.

Ion Gizmo Name _____________________ Pd _____

Electron Dot Diagrams

Before you begin, answer the following questions.

1. What is a valence electron?

2. How do you determine the total number of electrons in the electron cloud of an atom?

3. How do you determine the number of valence electrons that an atom has?

4. How many total electrons does a carbon atom have?

5. How many valence electrons does a carbon atom have?

I. Create an atom that contains 4 protons, 5 neutrons and 4 electrons. Check Show electron dot diagram.

1. What element is this?

2. What is its atomic number?

3. What is its mass number?

4. What is the net charge of the atom? The net charge can be found in the top left of the symbol.

II. Now take away two of the electrons to have an ion with 4 protons, 5 neutrons, and 2 electrons?

1. What is the charge on a proton?

2. What is the charge on an electron?

3. What is the charge on the ion? (Look at the top right of the element notation)

4. Describe the relationship between the number of protons and electrons in the ion that was formed when the two electrons were removed.

5. Why did the ion formed have the charge that it received?

III. Create an atom that contains 9 protons, 10 neutrons and 9 electrons.

1. What element is this?

2. What is its atomic number?

3. What is its mass number?

4. What is the net charge of the atom? The net charge can be found in the top left of the symbol.

IV. Now add one electron to have an ion with 9 protons, 10 neutrons, and 10 electrons?

1. What is the charge on a proton?

2. What is the charge on an electron?

3. What is the charge on the ion? (Look at the top right of the element notation)

4. Describe the relationship between the number of protons and electrons in the ion that was formed when the electron was added.

5. Why did the ion formed have the charge that it received?

V. Create a neutral neon atom with 10 protons, 10 neutrons, and 10 electrons?

1. What is the charge on the atom?

2. Why is the charge neutral?

3. Draw the atom from the gizmo (not the dot structure the “actual” picture of the atom?

VI. Create a neutral oxygen atom with 8 protons, 8 neutrons, and 8 electrons.

1. What is the charge on the atom?

2. Draw the atom from the gizmo.

3. Since the noble gases are stable (VERY unreactive), oxygen would like to look like one in terms of the number and arrangement of its electrons. What would the atom of oxygen have to do to its electrons in order to look like neon?

4. Now do this and draw the new ion formed. What is the charge on the ion?

5. Why does the ion have the charge that it does?

6. Since all elements in group 16 have the same number of valence electrons, then they all behave the same way in order to look like the noble gases. Therefore, what would an atom in group 16 have to do to look like a noble gas?

VII. Create a neutral fluorine atom with 9 protons, 10 neutrons, and 9 electrons.

1. What is the charge on the atom?

2. Draw the atom from the gizmo.

3. Since the noble gases are stable (VERY unreactive), fluorine would like to look like one in terms of the number and arrangement of its electrons. What would the atom of fluorine have to do to its electrons in order to look like neon?

4. Now do this and draw the new ion formed. What is the charge on the ion?

5. Why does the ion have the charge that it does?

6. Since all elements in group 17 have the same number of valence electrons, then they all behave the same way in order to look like the noble gases. Therefore, what would an atom in group 17 have to do to look like a noble gas and what would be the resulting charge?

VIII.Create a neutral sodium atom with 11 protons, 12 neutrons, and 11 electrons.

1. What is the charge on the atom?

2. Draw the atom from the gizmo.

3. Since the noble gases are stable (VERY unreactive), sodium would like to look like one in terms of the number and arrangement of its electrons. What would the atom of sodium have to do to its electrons in order to look like neon?

4. Now do this and draw the new ion formed. What is the charge on the ion?

5. Why does the ion have the charge that it does?

6. Since all elements in group 1 have the same number of valence electrons, then they all behave the same way in order to look like the noble gases. Therefore, what would an atom in group 1 have to do to look like a noble gas and what would be the resulting charge?

IX. Create a neutral magnesium atom with 12 protons, 12 neutrons, and 12 electrons.

1. What is the charge on the atom?

2. Draw the atom from the gizmo.

3. Since the noble gases are stable (VERY unreactive), magnesium would like to look like one in terms of the number and arrangement of its electrons. What would the atom of magnesium have to do to its electrons in order to look like neon?

4. Now do this and draw the new ion formed. What is the charge on the ion?

5. Why does the ion have the charge that it does?

6. Since all elements in group 2 have the same number of valence electrons, then they all behave the same way in order to look like the noble gases. Therefore, what would an atom in group 2 have to do to look like a noble gas and what would be the resulting charge?

Subatomic Particle Gizmo (2.1) Name _________________________ Pd ___

Some of the greatest breakthroughs in understanding the structure of the atom were provided by J. J. Thompson during his time at the renowned Cavendish Laboratory in Cambridge, England. Thompson had a reputation for being rather clumsy with his hands, and he always needed to have assistants to set up equipment for him. Nevertheless, he was a brilliant experimental physicist. Work conducted under his watchful eye led to the first discovery of a subatomic particle, the electron.

Once you log in, find the “Element Builder” Gizmo and select “Launch Gizmo.”

Location of Subatomic Particles

1. In this Gizmotm, subatomic particles (protons, neutrons and electrons) can be added to an atom or removed from it by clicking the arrows next to each supply of particles. Remove any protons (the program will not let you remove the last proton), neutrons, or electrons that are currently in the atom by clicking the left arrows. You can also highlight the number with the cursor and change the numbers manually. Below is what the screen should look like when you begin. The center of the atom is the nucleus and the area around the nucleus is the electron cloud.

a. Using the right arrows, add 1 proton, 2 neutrons, and 2 electrons to the atom so that there are 2 of each of the three particles located in the atom. Fill in the following chart.

Particle Location

ProtonNeutronElectron

Identity of the Atom

2. Place a check in the “Show element name” box, which is in the top right portion of the gizmo. Manipulate the number of protons to achieve the number of protons in the data table. Do not worry about the number of neutrons or electrons. Experiment with adding one and removing one proton to and from the atom. Fill in the following table. Once you have the identity of the element, look at the periodic table and write down the atomic number for the element, this is the integer located above the name of the element.

Number of protons Name of element Atomic Number from Periodic Table

231

a. Does changing the number of protons change the identity of the element you have built?

b. What is the relationship between the number of protons and the atomic number for an element?

3. Now you will do the same thing as step 2 except you will be changing the number of neutrons. Make sure that you begin with 2 each for the protons, neutrons, and electrons. Add one neutron to the atom to place 3 neutrons in the atom. Record the name of the element and look at the periodic table to find the atomic number. Next, take 2 neutrons away (a total of 1 should now be in the atom.) Again record the name of the atom and the atomic number from the periodic table.

Number of neutrons Name of element Atomic Number from Periodic Table

231

a. Does changing the number of neutrons change the identity of the element you have built?

b. Does changing the number of neutrons change the affect the atomic number?

4. Make sure that you have 2 each for the protons, neutrons, and electrons. Add one electron to the atom to place 3 electrons in the atom. Record the name of the element and look at the periodic table to find the atomic number. Next, take 2 electrons away (a total of 1 should now be in the atom.) Again record the name of the atom and the atomic number from the periodic table.

Number of electrons Name of element Atomic Number from Periodic Table

231

a. Does changing the number of electrons change the identity of the element you have built?

KEY FACT: Now looking at questions 2a, 3a, and 4a, which subatomic particle is responsible for the identity of an atom?

Mass of an atom

5. Build an atom again with exactly 2 protons, 2 neutrons, and 2 electrons. Check “Show element symbol.” Be sure “isotope” is not selected. Make adjustments to the atom to attain the number of protons, neutrons, and electrons as shown in the data table. Then finish filling in the table. The number to the upper left of the symbol indicates the mass of the atom. (See where the pointer is pointing in the screen shot.)

Number of protons Number of neutrons

Number of electrons

Identity of atom (give name)

Mass of atom

2 2 23 2 22 3 22 2 3

a. Does the proton affect the mass of an atom? You MUST justify your answer.

b. Does the neutron affect the mass of an atom? You MUST justify your answer.

c. Does the electron affect the mass of an atom? You MUST justify your answer.

d. Looking at the atom in the Gizmo, where is most of the mass of an atom concentrated? Explain.

5. Which 2 subatomic particles affect the mass of an atom?

KEY FACT: Write a mathematical formula to show the relationship between the number of protons, the number of neutrons, and the mass number for an atom.

SUMMARY: Based on this gizmo, the number of protons equals the _______________

______________ from the periodic table. The number of protons determines the

_______________ of an atom. The ____________ and _______________ determines the mass

of an atom. The protons and neutrons are located in the ________________ of an atom and

electrons are in the ________________ ______________.

How many protons are in the nucleus of an atom of Carbon (C)?

What is the formula for finding the mass number of an atom?

If an atom of C has 7 neutrons in the nucleus, then it would have a mass number of ______. (see previous 2 questions)

How many electrons would be found in the nucleus?

Elements: MatchingUse the following words:

_____ H 1)Cobalt

_____ B 2)Carbon

_____ O 3)Strontium

_____ Na 4)Sulfur

_____ Si 5)Tin

_____ Cl 6)Argon

_____ Fe 7)Boron

_____ Cu 8)Oxygen

_____ Kr 9)Nitrogen

_____ Au 10)Potassium

_____ K 11)Silicon

_____ He 12)Silver

_____ C 13)Gold

_____ F 17)Bromine

_____ Mg 18)Calcium

_____ P 19)Fluorine

_____ Ar 20)Lithium

_____ Co 21)Mercury

_____ Zn 22)Krypton

_____ Sr 23)Helium

_____ Hg 24)Hydrogen

_____ Ag 25)Neon

_____ Li 26)Nickel

_____ N 27)Zinc

_____ Ne 28)Aluminum

_____ Al 29)Lead

_____ S 14)Iodine

_____ Ca 15)Phosphorous

_____ Ni 16)Chlorine

_____ Br 30)Copper

_____ Sn 31)Magnesium

_____ Pb 32)Iron

_____ I 33)Sodium

Lesson on Naming Compounds:

Types of CompoundsIonic compounds are compounds composed of ions, charged particles that form when an atom (or group of atoms, in the case of polyatomic ions) gains or loses electrons.

• A cation is a positively charged ion• An anion is a negatively charged ion.

Covalent or molecular compounds form when elements share electrons in a covalent bond to form molecules. Molecular compounds are electrically neutral.Ionic compounds are (usually) formed when a metal reacts with a nonmetal (or a polyatomic ion). Covalent compounds are formed when two nonmetals react with each other. Since hydrogen is a nonmetal, binary compounds containing hydrogen are also usually covalent compounds.

• Metal + Nonmetal —> ionic compound (usually)• Metal + Polyatomic ion —> ionic compound (usually)• Nonmetal + Nonmetal —> covalent compound (usually)• Hydrogen + Nonmetal —> covalent compound (usually)

Naming Chemical Compounds – Some Notes1. Some nonmetals form a series of polyatomic ions with oxygen (all having the

same charge): ClO-, hypochlorite; ClO2-, chlorite; ClO3-, chlorate; ClO4-, perchlorate.

a. The -ate forms (formula and charge) must be memorized. In some cases, the -ate form has three oxygens, and in some cases four oxygens. The charge is the same for the entire series.

b. The -ite form has one less oxygen that the -ate form.c. The hypo- stem -ite form has two less oxygens than the -ate form.d. The per- stem -ate form has one more oxygen than the -ate form.e. The -ide form is the monatomic anion

2. The cation is written first, followed by the monatomic or polyatomic anion.3. The subscripts in the formula must produce an electrically neutral formula unit.

(That is, the total amount of positive charge must equal the total amount of negative charge.)

4. The subscripts should be the smallest set of whole numbers possible.5. If there is only one of a polyatomic ion in the formula, do not place parentheses

around it; e.g., NaNO3, not Na(NO3). If there is more than one of a polyatomic ion in the formula, put the ion in parentheses, and place the subscript after the parentheses; e.g., Ca(OH)2, Ba3(PO4)2, etc.

Remember the Prime Directive in writing formulas:Ca(OH)2 is not the same as CaOH2 !

Examples

Cation Anion FormulaNa+ Cl- NaCl Ca2+ Br- CaBr2 Na+ S2- Na2S Mg2+ O2- MgO Fe3+ O2- Fe2O3 Na+ SO42- Na2SO4

1. Binary Ionic Compounds Containing a Metal and a Nonmetal. A binary compound is a compound formed from two different elements. There may or may not be more than one of each element. A diatomic compound (or diatomic molecule) contains two atoms, which may or may not be the same.Metals combine with nonmetals to give ionic compounds. When naming binary ionic compounds, name the cation first (specifying the charge, if necessary), then the nonmetal anion (element stem + -ide).

4. Binary Covalent Compounds Between Two Nonmetals.Two nonmetals combine to form a covalent or molecular compound (i.e., one that is held together by covalent bonds which result from the sharing of electrons).In many cases, two elements can combine in several different ways to make completely different compounds. (This cannot happen with ionic compounds, except in the cases of metals that can form more than one charge.) For instance, carbon can share electrons with one oxygen to make CO (carbon monoxide), or with two oxygens to make CO2 (carbon dioxide). For this reason, it is necessary to specify how many of each element is present within the compound.

• The formula is written with the more electropositive element (the one further to the left on the periodic table) placed first, then the more electronegative element (the one further to the right on the periodic table).

[Important exception: when the compound contains oxygen and a halogen, the halogen is placed first. If both elements are in the same group, the one with the higher period number is named first.]

• The first element in the formula is given the neutral element name, and the second one is named by replacing the ending of the neutral element name with -ide. A prefix is used in front of each element name to indicate how many atoms of that element are present:

1 mono-2 di-3 tri-4 tetra-5 penta-6 hexa-7 hepta-8 octa-9 nona-10 deca-

• If there is only one of the first element in the formula, the mono- prefix is dropped.

Examples

SO2 sulfur dioxideSO3 sulfur trioxideN2O dinitrogen monoxideNO nitrogen monoxideNO2 nitrogen dioxideN2O4 dinitrogen tetroxideN2O5 dinitrogen pentoxide

Nonmetals may combine in a variety of ratios, so it is important that the name of a molecular compound indicates how many atoms of each type of element are present in the compound. This is accomplished using prefixes. If there is only one atom of the first element, no prefix is used. It is customary to prefix the name of one atom of the second element with mono-. For example, CO is named carbon monoxide rather than carbon oxide. Examples of Covalent Compound NamesSO2 - sulfur dioxideSF6 - sulfur hexafluorideCCl4 - carbon tetrachlorideNI3 - nitrogen triiodide Writing the Formula from the NameYou can write the formula for a covalent compound from its name by writing the symbols for the first and second element and translating the prefixes into subscripts. For example, xenon hexafluoride would be written XF6. It is common for students to confuse

ionic compounds and covalent compounds and then have trouble trying to write formulae from the compounds names. You aren't balancing charges of covalent compounds; if the compound does not contain a metal, don't try to balance this!

For IONIC Compounds follow these instructions:

Suppose we wish to write the formula for the compound that forms between aluminum and chlorine. To write the formula, we must first determine the oxidation numbers of the ions that would be formed. We will revisit the concept of oxidation numbers later, but for now, all you need to know is that the oxidation number for an atom in an ionic compound is equal to the charge of the ion it produces.

Then, we determine the simplest whole numbers with which to multiply these charges so they will balance (add to zero) since ionic compounds are neutral. In this case, we would multiply the by and the by .

You should note that we could multiply the by and the by to get and , respectively. These values will also balance, but this is not acceptable because empirical formulas, by definition, must have the lowest whole number multipliers. Once we have the lowest whole number multipliers, those multipliers become the subscripts for the symbols. The formula for this compound would be .

Here’s the process for writing the formula for the compound formed between aluminum and sulfur.

Therefore, the formula for this compound would be .

Another method used to write formulas is called the criss-cross method. It is a quick method, but it often produces errors if the user doesn’t pay attention to the results. The example below demonstrates the criss-cross method for writing the formula of a compound formed from aluminum and oxygen. In the criss-cross method, the oxidation numbers are placed over the symbols for the elements just as before.

In this method, the oxidation numbers are then criss-crossed and used as the subscripts for the other atom (ignoring sign).

This produces the correct formula for the compound. Here’s an example of a criss-cross error:

If you used the original method of finding the lowest multipliers to balance the charges, you would get the correct formula , but the criss-cross method produces the incorrect formula . If you use the criss-cross method to generate an ionic formula, it is essential that you check to make sure that the subscripts correspond to the lowest whole number ratio of the atoms involved. Note that this only applies to ionic compounds. When we learn about covalent compounds in the chapter “Covalent Bonds and Formulas,” you will see that the formula describes a different molecule than

, so it would not be reduced to its simplest ratio.

Naming Ionic Compounds Practice Worksheet

Name the following ionic compounds:

1) NH4Cl _____________________________________

2) Fe(NO3)3 _____________________________________

3) TiBr3 _____________________________________

4) Cu3P _____________________________________

5) SnSe2 _____________________________________

6) GaAs _____________________________________

7) Pb(SO4)2 _____________________________________

8) Be(HCO3)2 _____________________________________

9) Mn2(SO3)3 _____________________________________

10) Al(CN)3 _____________________________________

Write the formulas for the following compounds:

11) chromium (VI) phosphate ____________________________________

12) vanadium (IV) carbonate ____________________________________

13) tin (II) nitrite _____________________________________

14) cobalt (III) oxide _____________________________________

15) titanium (II) acetate _____________________________________

16) vanadium (V) sulfide _____________________________________

17) chromium (III) hydroxide _____________________________________

18) lithium iodide_____________________________________

19) lead (II) nitride _____________________________________

20 silver bromide _____________________________________

Lots of Ionic Naming Practice Problems

Name the following ionic compounds:

1) NaBr __________________________________

2) Sc(OH)3 __________________________________

3) V2(SO4)3 __________________________________

4) NH4F __________________________________

5) CaCO3 __________________________________

6) NiPO4 __________________________________

7) Li2SO3 __________________________________

8) Zn3P2 __________________________________

9) Sr(C2H3O2)2 __________________________________

10) Cu2O __________________________________

11) Ag3PO4 __________________________________

12) YClO3 __________________________________

13) SnS2 __________________________________

14) Ti(CN)4 __________________________________

15) KMnO4 __________________________________

16) Pb3N2 __________________________________

17) CoCO3 __________________________________

18) CdSO3 __________________________________

19) Cu(NO2)2 __________________________________

20) Fe(HCO3)2 __________________________________

Write the formulas for the following ionic compounds:

21) lithium acetate __________________________________

22) iron (II) phosphate __________________________________

23) titanium (II) selenide __________________________________

24) calcium bromide __________________________________

25) gallium chloride __________________________________

26) sodium hydride __________________________________

27) beryllium hydroxide __________________________________

28) zinc carbonate __________________________________

29) manganese (VII) arsenide __________________________________

30) copper (II) chlorate __________________________________

31) cobalt (III) chromate __________________________________

32) ammonium oxide __________________________________

33) potassium hydroxide __________________________________

34) lead (IV) sulfate __________________________________

35) silver cyanide __________________________________

36) vanadium (V) nitride __________________________________

37) strontium acetate __________________________________

38) molybdenum sulfate __________________________________

39) platinum (II) sulfide __________________________________

40) ammonium sulfate __________________________________

Mixed Ionic/Covalent Compound Naming

For each of the following questions, determine whether the compound is ionic or covalent and name it appropriately.

1) Na2CO3 _________________________________________

2) P2O5 _________________________________________

3) NH3 _________________________________________

4) FeSO4 _________________________________________

5) SiO2 _________________________________________

6) GaCl3 _________________________________________

7) CoBr2 _________________________________________

8) B2H4 _________________________________________

9) CO _________________________________________

10) P4 _________________________________________

For each of the following questions, determine whether the compound is ionic or covalent and write the appropriate formula for it.

11) dinitrogen trioxide _________________________________________

12) nitrogen _________________________________________

13) methane _________________________________________

14) lithium acetate _________________________________________

15) phosphorus trifluoride _______________________________________

16) vanadium (V) oxide _________________________________________

17) aluminum hydroxide ________________________________________

18) zinc sulfide _________________________________________

19) silicon tetrafluoride _________________________________________

20) silver phosphate _________________________________________

(Still) More Naming Practice

Write the names of the following chemical compounds:

1) BBr3 ______________________________________

2) CaSO4 ______________________________________

3) C2Br6 ______________________________________

4) Cr(CO3)3 ______________________________________

5) Ag3P ______________________________________

6) IO2 ______________________________________

7) VO2 ______________________________________

8) PbS ______________________________________

9) CH4 ______________________________________

10) N2O3 ______________________________________

Write the formulas of the following chemical compounds:

11) tetraphosphorus triselenide ____________________________________

12) potassium acetate ______________________________________

13) iron (II) phosphide ______________________________________

14) disilicon hexabromide ______________________________________

15) titanium (IV) nitrate ______________________________________

16) diselenium diiodide ______________________________________

17) copper (I) phosphate ______________________________________

18) gallium oxide ______________________________________

19) tetrasulfur dinitride ______________________________________

20) phosphorus ______________________________________

Review– Naming Chemical Compounds

The following are a good mix of naming and formula writing problems to help you get some practice.

Name the following chemical compounds:

1) NaBr ______________________________________________

2) Ca(C2H3O2)2 ______________________________________________

3) P2O5 ______________________________________________

4) Ti(SO4)2 ______________________________________________

5) FePO4 ______________________________________________

6) K3N ______________________________________________

7) SO2 ______________________________________________

8) CuOH ______________________________________________

9) Zn(NO2)2 ______________________________________________

10) V2S3 ______________________________________________

Write the formulas for the following chemical compounds:

11) silicon dioxide ______________________________________________

12) nickel (III) sulfide _____________________________________________

13) manganese (II) phosphate _____________________________________

14) silver acetate ______________________________________________

15) diboron tetrabromide _________________________________________

16) magnesium sulfate heptahydrate ________________________________

17) potassium carbonate _________________________________________

18) ammonium oxide ____________________________________________

19) tin (IV) selenide ______________________________________________

20) carbon tetrachloride __________________________________________

Solutions for the Naming Ionic Compounds Practice Worksheet

1) ammonium chloride2) iron (III) nitrate3) titanium (III) bromide4) copper (I) phosphide5) tin (IV) selenide6) gallium arsenide7) lead (IV) sulfate8) beryllium bicarbonate9) manganese (III) sulfite10) aluminum cyanide

11) Cr(PO4)212) V(CO3)213) Sn(NO2)214) Co2O315) Ti(C2H3O2)216) V2S517) Cr(OH)318) LiI19) Pb3N220) AgBr

Ionic Naming Practice Problems - Solutions

1) NaBr sodium bromide2) Sc(OH)3 scandium hydroxide3) V2(SO4)3 vanadium (III) sulfate4) NH4F ammonium fluoride5) CaCO3 calcium carbonate6) NiPO4 nickel (III) phosphate7) Li2SO3 lithium sulfite8) Zn3P2 zinc phosphide9) Sr(C2H3O2)2 strontium acetate 10) Cu2O copper (I) oxide11) Ag3PO4 silver phosphate12) YClO3 yttrium chlorate13) SnS2 tin (IV) sulfide14) Ti(CN)4 titanium (IV) cyanide

15) KMnO4 potassium permanganate16) Pb3N2 lead (II) nitride17) CoCO3 cobalt (II) carbonate18) CdSO3 cadmium sulfite19) Cu(NO2)2 copper (I) nitrite20) Fe(HCO3)2 iron (II) bicarbonate21) lithium acetate LiC2H3O222) iron (II) phosphate Fe3(PO4)223) titanium (II) selenide TiSe24) calcium bromide CaBr225) gallium chloride GaCl326) sodium hydride NaH27) beryllium hydroxide Be(OH)228) zinc carbonate ZnCO329) manganese (VII) arsenide Mn3As730) copper (II) chlorate Cu(ClO3)231) cobalt (III) chromate Co2(CrO4)332) ammonium oxide (NH4)2O33) potassium hydroxide KOH34) lead (IV) sulfate Pb(SO4)235) silver cyanide AgCN36) vanadium (V) nitride V3N537) strontium acetate Sr(C2H3O2)238) molybdenum sulfate Mo(SO4)339) platinum (II) sulfide PtS40) ammonium sulfate (NH4)2SO4

Ionic/Covalent Compound Naming Solutions

1) Na2CO3 sodium carbonate2) P2O5 diphosphorus pentoxide3) NH3 ammonia4) FeSO4 iron (II) sulfate5) SiO2 silicon dioxide6) GaCl3 gallium chloride7) CoBr2 cobalt (II) bromide8) B2H4 diboron tetrahydride9) CO carbon monoxide10) P4 phosphorus

11) dinitrogen trioxide N2O312) nitrogen N213) methane CH414) lithium acetate LiC2H3O215) phosphorus trifluoride PF316) vanadium (V) oxide V2O517) aluminum hydroxide Al(OH)318) zinc sulfide ZnS19) silicon tetrafluoride SiF420) silver phosphate Ag3PO4

(Still) More Naming Practice - Answers

1) BBr3 boron tribromide2) CaSO4 calcium sulfate3) C2Br6 dicarbon hexabromide4) Cr(CO3)3 chromium (VI) carbonate

5) Ag3P silver phosphide6) IO2 iodine dioxide7) VO2 vanadium (IV) oxide8) PbS lead (II) sulfide9) CH4 methane10) N2O3 dinitrogen trioxide

Write the formulas of the following chemical compounds:11) tetraphosphorus triselenide P4Se3

12) potassium acetate KC2H3O2

13) iron (II) phosphide Fe3P2

14) disilicon hexabromide Si2Br6

15) titanium (IV) nitrate Ti(NO3)4

16) diselenium diiodide Se2I2

17) copper (I) phosphate Cu3PO4

18) gallium oxide Ga2O3

19) tetrasulfur dinitride S4N2

20) phosphorus P4

Answers – Naming Chemical Compounds

1) NaBr sodium bromide

2) Ca(C2H3O2)2 calcium acetate

3) P2O5 diphosphorus pentoxide

4) Ti(SO4)2 titanium(IV) sulfate

5) FePO4 iron(III) phosphate

6) K3N potassium nitride

7) SO2 sulfur dioxide

8) CuOH copper(I) hydroxide

9) Zn(NO2)2 zinc nitrite

10) V2S3 vanadium(III) sulfide

Write the formulas for the following chemical compounds:11) silicon dioxide SiO2

12) nickel (III) sulfide Ni2S3

13) manganese (II) phosphate Mn3(PO4)2

14) silver acetate AgC2H3O2

15) diboron tetrabromide B2Br4

16) magnesium sulfate heptahydrate MgSO4.7H2O

17) potassium carbonate K2CO3

18) ammonium oxide (NH4)2O

19) tin (IV) selenide SnSe2

20) carbon tetrachloride CCl4

Chemical Bonding Terms:

Physical and Chemical Change Worksheet True or False. If false, correct the underlined portion of the statement so that it is true. 1. A physical change is a change of matter from one form to another without a change in chemical properties. TRUE2. A physical change is a change that occurs when a substance changes composition by forming one or more new substances. FALSE-CHEMICAL CHANGE3. Color change is evidence that a chemical change may have occurred. TRUE4. Fizzing or foaming is evidence that a chemical change may have occurred. TRUE5. Production of light is evidence that a physical change may have occurred. FALSE- CHEMICAL CHANGE6. Production of heat or light is evidence that a chemical change may have occurred. TRUE7. A change in odor is evidence that a physical change may have occurred. FALSE- CHEMICAL CHANGE

8. Chemical changes can be reversed by physical changes. FALSE- CHEMICAL CHANGES CANNOT BE REVERSED

Identify each of the following as either a

Physical change (P) or a chemical change (C). 1. You cut your hair. P 2. Making a peanut, pretzel

and cereal mixture. P 3. Baking soda reacts with

vinegar and forms a gas. C

4. A piece of metal is bent in half. P

5. An aspirin is crushed into fine powder. P

6. Copper turns green when exposed to the environment. C

7. Two clear liquids are mixed and a yellow color forms. C

8. Baking cookies. C 9. Diamonds are used to

scratch glass. P10. A tree burns to form

ashes. C 11. A piece of paper is

crumpled up. P12. Water freezes to form ice.

P 13. Food spoiling. C 14. A candle burning. C 15. A candle melting. P

A Thought Experiment A sealed flask of a clear, colorless liquid is left sitting on an interior sunny windowsill. After about an hour, there are droplets of a clear liquid on the glass above the solution, which has turned yellow. After two hours, the solution is dark brown with clear, colorless droplets of liquid on the glass. After sitting on the windowsill for a week, the walls of the flask have a silvery lining and both the solution and the droplets are clear and colorless. 6. Which of the following is

not an indication that a chemical reaction has occurred?

(a) formation of liquid droplets above the solution (b) the solution color changing from clear to yellow (c) the solution color changing from brown to clear (d) formation of a silvery metallic foil on the walls of the flask

7. The formation of the silvery lining is an example of which of the following indicators of chemical change?

(a) evolution of a gas (b) distinct color change (c) precipitate formation (d) temperature change

1. (Short answer) There is only one reaction taking place in the flask. What is one possible reason for all of the color changes?

The reaction is taking place over time (in stages) as the temperature changes due to location and duration.

2. (Short answer) An observant chemistry student is enjoying a glass

of iced tea during lunch (not in the lab!), and she notices that the color of her drink changes as the ice in the glass melts. Is a chemical reaction occurring? Why or why not?

No, a physical change is occurring as the tea is separating from the water. This is happening as the ice in the glass is melting. Change of state is a physical change.