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SCIENCE 10
CHAPTER 2: Naming, formulas, &
propertiesNAME:______________________
DAY: _____ BLOCK: _____
W. P. Wagner 1
Understanding Matter – WHMIS symbols
Ionic Compounds
Students will:Explain, using the periodic table, how elements combine to form compounds, and follow IUPAC guidelines for naming ionic compounds and simple molecular compounds
predict formulas and write names for ionic compounds using a periodic table, a table of ions and IUPAC rules
Made up of positive ions (cations )METALS and negative ions (anions) NON-METALS Always have no net charge (i.e. are neutral) therefore, the ratio of cations to anions must be
such that the total positive charge and total negative charge are equal (lowest whole number ratio) e.g.
Always named according to the following format:
Types of ions and ionic compounds:
W. P. Wagner 2
METAL (+) NON (-)ide
MAIN GROUP ANIONS
MAIN GROUP CATIONS
MONATOMIC IONS
TRANSITION METAL CATIONS
POLYATOMIC ANIONS
POLYATOMIC CATIONS
POLYATOMIC IONS
IONS
BINARY IONIC COMPOUNDS
TERNARY IONIC COMPOUNDS
HYDRATES
I O N I C C O M P O U N D S
I BINARY IONIC COMPOUNDS: (Compounds composed of a metal and a non-metal)
Rules for naming:
1. Name the metallic ion first, followed by the non-metallic ion. (the non-metallic ion ends in "ide")
2. Ionic compounds always start with a metal or an ammonium ion.
Name the following ionic compounds:
Ag2S __________________ AlCl3 _________________
KCl ____________________ K2O ___________________
CaS ____________________ Al2O3__________________
CaF2____________________ AgCl ___________________
Mg3N2 __________________ Li2S ___________________
K2S ____________________ BaI2____________________
RbF _____________________ LiBr____________________
Na2O____________________ AlBr3___________________
BaO _____________________ MgS__ _________________
Sr3N2___________________ GaCl3___________________
Ag3P____________________ ScN____ _________________
CdS_____________________ InP______________________
BaI2____________________ BeS_____________________
Al2S3___________________ MgSe__________________
GeCl4___________________ Cs3N____________________
W. P. Wagner 3
Ionic compounds
- Formed when metals ions bind to non-metal ions; called an ___________________.- Called salts (just like table salt). When the positive and negative charges attract each other a
_____________ _____________ structure is formed. o Each crystal could contain thousands, millions or trillions of ions;
the number varies from crystal to crystal..
.- Formulas for ionic compounds tell you the _____________ of metal ions to non-metal ions.
o It is impractical to use a chemical formula showing the exact number of ions since the exact number varies from crystal to crystal. Instead we create a RATIO using subscript numbers
o For example the formula NaCl tells us that, for every sodium ion, there is one chloride ion. MgCl2 tells us that, for every magnesium ion, there are two chloride ions.
- To tell what the ratio is we rely on the knowledge that ionic compounds are formed from ions. o Since chloride ions have a charge of one negative, and calcium ions have a charge of
positive two, it takes two chloride ions to cancel the charge of one calcium ion.
o Since the aluminum ion has a charge of positive three, and the oxide ion has a charge of positive two the ratio of aluminium ions to oxide ions 2:3
Name Summary of Charge Formulamagnesium chloride MgCl2
sodium bromideNaF
silver sulfideK2O
cesium oxideAl2S3
calcium phosphideZnCl2
W. P. Wagner 4
Complete the following table by either writing the correct chemical formula or IUPAC name.
ChemicalFormula
Summary of ChargeName of Compound
eg. CaCl2 Ca2+ , Cl-, Cl- calcium chloride
1. potassium iodide
2. MgO3. aluminum chloride
4. NaBr5. CaO6. lithium nitride
7. Al2O3
8. barium chloride
9. sodium chloride
10. ZnO11. silver bromide
12. magnesium hydride
13. magnesium chloride
14. zinc chloride
15. Ag2S16. potassium chloride
17. CaF2
18. sodium sulphide
19. CaH2
20. zinc sulphide
W. P. Wagner 5
Writing formulas for Ionic Compounds 1. When given the name, write the symbol and charge for each ion.
2. Remember all compounds are electrically neutral.
3. Use subscripts to equalize the total number of positive and negative charges. (The formula shows the lowest ratio of positive to negative ions.)1
Example:
Aluminum oxide Al3+ O2- (3+)2 = 6+ (2-)3 = 6- Al2O3
Write formulas for the following:
l. aluminum oxide_________________ 14. barium chloride _______________
2. silver fluoride _________________ 15. scandium nitride ______________
3. potassium sulfide ______________ 16. gallium selenide ______________
4. calcium nitride ________________ 17. beryllium arsenide ____________
5. sodium phosphide_______________ 18. zinc sulfide __________________
6. aluminum fluoride ______________ 19. calcium iodide ________________
7. magnesium oxide _______________ 20. lithium bromide _______________
8. cesium nitride_________________ 21. sodium fluoride _______________
9. calcium hydride ________________ 22. strontium phosphide ___________
10. silver oxide __________________ 23. sodium sulfide ________________
11. calcium phosphide_____________ 24. gallium oxide_________________
12. zinc bromide__________________ 25. indium fluoride_______________
13. francium nitride_______________ 26. magnesium fluoride____________
1
W. P. Wagner 6
Composition of Chemical Compounds - The Stock System
The Stock System. Some ions can exist with different ion charges in different situations. For example, iron can exist as Fe3+ and Fe2+. To distinguish one from the other, Roman numerals are used in the name of compounds that are made with ions that can have different charges.
Fe3+ is called the iron (III) ion and Fe2+ is called the iron (II) ion.
Write the chemical formula for iron (II) oxide. ________, for iron (III) oxide. ________
Complete the following table using the Stock System for naming ionic compounds. Remember that all transition metals except for aluminum, zinc and silver require the Roman numeral to specify ion charge.
Chemical Formula
IUPAC Name Summary of Charges
1. Cu3N2 copper (II) nitride Cu2+, Cu2+, Cu2+, N3-, N3-
2. gold (I) chloride
3. Al2S3
4. tin (II) oxide
5. antimony (V) bromide
6. SbF3
7. CuCl
8. Fe2Se3
9. ZnCl2
10. aluminum sulphide
11. mercury (I) nitride
12. AlP
13. Ni2S3
14. VI5
15. cobalt (II) phosphide
16. chromium (II) hydride
17. silver telluride
W. P. Wagner 7
Composition of Chemical Compounds - Ternary Ionic Compounds
Ternary ionic compounds are usually compounds made from polyatomic ions. These polyatomic ions are identified on your periodic table in the box at the top of the page. Generally, if you don't recognize the name of a substance it is a polyatomic ion.
For example: If asked to write the formula for sodium sulphate. You can recognize the sodium part but sulphate may be a word you don't recognize. In that case check the box containing the polyatomic ions. Sulphate shows up as SO4
2-. This means it is a polyatomic ion with a charge of -2.
To write the formula for the compound sodium sulphate, you need two sodium ions and one sulphate ion. Na+ + Na+ + SO4
2- makes Na2SO4 and it has a neutral charge so you are done. Whenever you need multiple polyatomic ions, you must put parentheses around the polyatomic ion and add the subscript outside the parentheses.
E.g. Write the name of Mg(ClO)2 ____________________________________.
The following table that requires you to name some common polyatomic ions. Remember that complex ions are not molecules and cannot exist by themselves as they are on the periodic table or in this exercise.
Ion Name Formula Ion Name Formula
1. silicate 6. sulfite
2. ClO3- 7. NO3
-
3. NH4+ 8. hydrogen sulfide
4. dichromate 9. HPO42-
5. OH- 10. CH3 COO-
W. P. Wagner 8
Naming Compounds with Polyatomic IonsUse the table of polyatomic ions to complete the following exercise. Only those polyatomic ions listed on the periodic table are used in science 10.
International Formula Summary of Charges IUPAC English Name1. Na2CO3
2. (NH4)2CO3
3. FeSO4
4. lithium hydroxide
5. aluminum hydroxide
6. NaClO
7. potassium dichromate
8. LiC6H5COO9. NaNO2
10. ammonium sulphate
11. sodium hydrogen carbonate
12. Na3PO4
13. calcium dihydrogen
phosphate
14. PbCrO4
15. sodium hydrogen sulphate
16. KMnO4
17. aluminum silicate
18. Li2CO3
19. potassium cyanide
Naming Compounds with Polyatomic Ions and the Stock SystemComplete the following table using the stock system and polyatomic ions for naming compounds.
Chemical Formula
Summary of Charge Name of Compound
eg. Cu2SO3 Cu+, Cu+, SO32- copper(I) sulphite
1. uranium(IV) oxide
2. lead(IV) sulphate
3. Sn(HPO4)2
4. Al2O3
5. manganese(IV) iodate
6. Sb2S3
7. thallium(III) hydroxide
8. HgS
9. MoS3
10. polonium (II) thiosulphate
11. FeSO4
12. lead(IV) chlorate
13. Hg(NO3)2
14. ZnSe
15. V2O5
16. tin (II) borate
17. chromium (III) phosphate
18. TiO2
19. Ag2SO3
20. AuCl3
21. uranium(IV) cyanide
22. NiBr2
23. cobalt(II) hypochlorite
Composition of Chemical Compounds - Hydrated Compounds
Hydrated compounds are compounds that contain water as part of their structure. Some compounds are water seeking and are most stable when they are attached to many water molecules.
To name these substances we need to know the common prefixes so that the compounds can be described correctly.
The common substance, Epsom salts, is named magnesium sulphate heptahydrate and its formula is MgSO47H2O. If you remove the water by heating or by some other means, the compound can be used to soak up water as it gets back the water you have taken away. Anti-perspirants are made in this way.
Generally the chemical formula ends with __H2O - where the blank is the correct value for the number
of water molecules that are bonded to the ionic compound.
The IUPAC name can be written in two different ways. For the above example MgSO47H2O would be written either;
- using the prefix system as magnesium sulphate heptahydrate or- using the number system as magnesium sulphate-7-water.
***You must be able to read and write the names of hydrated compounds using either system.
Eg. – Cu(NO3)2 4 H2O tetrahydrate
copper (II) nitrate
Full Name: copper (II) nitrate tetrahydrate
1 - mono2 - di3 - tri4 - tetra5 - penta
6 - hexa7 - hepta8 - octa9 - nona10- deca
Naming Hydrated Compounds. Complete the following table.
Name of Hydrate Common Name, Use or Discrition Formula
e.g. copper(II) sulphate pentahydrate
blue vitriol, bluestone, copper plating, blue solid
CuSO45H2O(s)
1. Epsom salts, white solid explosives, matches
MgSO47H2O(s)
2. sodium carbonate decahydrate
washing soda, soda ash, water softener, white solid
3. white solid, fireproofing wood, disinfectants, parchment paper
MgCl26H2O(s)
4. barium chloride dihydrate
white solid, pigments, dyeing fabrics, tanning leather
5. white solid, photographic emulsions Cd(NO3)24H2O(s)
6. white solid, embalming material, fireproofing lumber, vulcanizing
ZnCl25H2O(s)
7. zinc sulphate heptahydrate
white solid, clarifying glue, preserving wood and skins
8. lithium chloride tetrahydrate
white solid, soldering aluminum in fireworks
9. photographic hypo, antichlor, white solid Na2S2O35H2O(s)
10 cobalt(II) chloride hexahydrate
pink solid, humidity and water indicator, foam stabilizer in beer
11 white solid, antiperspirant AlCl36H2O(s)
12 de-icer used on icy highways, added to cement mixtures to prevent freezing
CaCl22H2O(s)
13 barium hydroxide octahydrate
white solid, manufacture of glass, water softener
14 nickel(II) chloride hexahydrate
green solid, manufacture of glass, water softener
15 Glauber's salt (a medicine), white solid, drying agent
Na2SO410H2O(s)
Composition of Chemical Compounds - Solubility of Ionic Compounds
Students will: predict whether an ionic compound is relatively soluble in water, using a solubility chart
Ionic compounds are determined to have either high solubility or low solubility when placed into water. Since it is not possible for you to know which is which, a solubility chart is provided for you on the periodic table. The top row of ions on the Solubility Chart contains the high solubility (H) compounds; the bottom row contains the low solubility (L) compounds.
To determine the solubility of an ionic compound you first look for the anion on the chart (the non-metal ion). Once you find the anion, there are two choices for the cation in the compound. If it appears in the top box below the anion name, it has high solubility and is therefore said to be aqueous (aq). If it appears in the bottom box it has low solubility and the compound is a solid (s).
Ionic compounds are deemed to be high solubility (H) if large amounts of the solid will dissolve in water. Low solubility (L) substances dissolve only very slightly in water.
Predict whether the following Ionic Compounds are high solubility or low solubility.
IUPAC Name State of the Pure substance(s, l, or g)
Solubility H/L
State in a Water Environment (s or aq)
1. AgNO3 ( ) ( )2. NH4OH ( ) ( )3. PbS ( ) ( )
4. Ag2SO4 ( ) ( )5. CaCO3 ( ) ( )6. Mg(CH3COO)2 ( ) ( )7. Al2(SO4)3 ( ) ( )8. Na2S ( ) ( )9. Ca(OH)2 ( ) ( )
Composition of Compounds – Forming a Precipitate (optional)
The following ionic species (ions) were placed in an aqueous environment (in water). Describe what will happen when each pair of ions reacts to form an ionic compound. Write the chemical formula for the ionic compound, including the state in the aqueous environment, then indicate whether they are high or low solubility and whether a precipitate forms.
If a low solubility substance forms when the ions combine, the evidence will be the formation of a precipitate. You can tell when a precipitate forms because it becomes a solid (usually white and cloudy). In this case the chemical formula will be written with a (s).
High solubility substances that form will remain in solution (no cloudiness), are written as (aq).
Complete the table below by writing the name of the chemical formula including its state in a water environment, its solubility and whether a precipitate will form.
IONS Solubility?H/L
Precipitate? Chemical Formula & State
1. Ba2+ and SO42- BaSO4
2. Mg2+ and S2- MgS
3. Fe3+ and OH- Fe(OH)3
4. K+ and CO32- K2CO3
5. Sr2+ and OH- Sr(OH)2
6. Na+ and OH- NaOH-
7. NH4+ and PO4
3- (NH4)3PO4
8. Cu+ and Cl- CuCl-
Composition of Chemical Compounds - Naming of Acids Students will:
predict formulas and write names for common acids using a periodic table, a table of ions and IUPAC rules
Acids are a special kind of ionic compound. Acids are made up of positive and negative ions but the positive ion in this case is only the hydrogen ion (H+). Acids are unique also because they do not behave as acids until they are dissolved in water.
Acids have the following properties:
are solids, liquids or gases at SATP. (when they are not in a water environment) are highly soluble in water. form conducting solutions. turn indicators like blue litmus paper red and bromothymol blue solution yellow. react with metals such as zinc to produce hydrogen gas (H2(g)).
Acids naming appears to be complex at first but there are really only three different naming conventions for acids. As ionic compounds (not in water) they have different names than as acids when they are dissolved in water. This table illustrates the way the different acids are named.
Ionic Name Acid Name1. hydrogen ________ide
eg. hydrogen nitride becomeshydro_________ic acid hydronitric acid H3N(aq)
2. hydrogen ________ateeg. hydrogen nitrate becomes
_____________ic acid nitric acid HNO3(aq)
3. hydrogen ________ite eg. hydrogen nitrite becomes
_____________ous acid nitrous acid HNO2(aq)
More Acid Naming
Chemical Formula Name as an Ionic Name as an Acid
1. H2 SO4 (aq)
2. H3 PO4 (aq)
3. boric acid
4. carbonic acid
5. hydrogen fluoride
6. hydrosulphuric acid
7. chloric acid
8. H2 S (aq)
9. hydrogen nitrate
10. sulphurous acid
11. HNO3 (aq)
12. HCl (aq) hydrochloric acid
13. hydrogen nitrite
14. hydrogen benzoate
15. HCNq)
16. oxalic acid
17. HBr (aq)
18. HI (aq)
19. CH3 COOH(aq)
Distinguishing between ionics and acids. In the following table, indicate the state of the compound in a water environment as (s), (l) or (aq).
Acid/Ionic Chemical Formula Name of Compound1. Al(OH)3 (s)
2. aluminium sulphate3. H3 BO3 (aq)
4. sulphuric acid5. NH4 NO3 (aq) 6. potassium carbonate7. H2 SO4 (aq)
8. phosphoric acid9. Cu SO4 (aq)
10. hydroiodic acid11. lead (II) acetate12. H2 CO3 (aq) 13. hydrosulphuric acid14. sodium chlorate15. KI (aq)
16. KMnO4 (aq)
17. ammonium nitrate18. HNO2 (aq)
19. barium hydroxide20. hydrochloric acid21. Au( NO3 )3 (aq) 22. nitric acid23. HOOCCOOH ( )
24. aluminum phosphate25. tin (II) sulphate
Composition of Chemical Compounds - Molecular CompoundsStudents will:
predict formulas and write names for molecular compounds using a periodic table, a table of ions and IUPAC rules
Some molecular compounds must be memorized because there are no simple rules for naming them. Many molecular compounds can be named using the prefix system as with hydrates.
In molecular compounds, the prefixes refer to the subscript number. This is different than hydrates where the prefix referred to the coefficient (the number in front of the H2O). Note: The mono prefix is only used for the second element where necessary.
E.g. - CO is named carbon monoxide not monocarbon monoxide. - CO2 is named carbon dioxide.
The molecular compounds that must be remembered are:
1 - mono2 - di3 - tri4 - tetra5 - penta
6 - hexa7 – hepta8 – octa9 – nona10- deca
1. ammonia NH3(g)
2. glucose C6H12O6(s)
3. hydrogen peroxide H2O2(l)
4. sucrose C12H22O11(s)
5. methane CH4(g)
6. ethane C2H6(g)
7. propane C3H8(g)
8. methanol CH3OH(l)
9. ethanol C2H5OH(l)
10. ozone O3(g)
11. water H2O(l)
In addition to these molecular compounds, there are other polyatomic molecular compounds.
The Special Seven : N O F **These seven elements formdiatomic compounds when they
Cl individually written.
H Br Eg. H2(g), N2(g), O2(g), F2(g), Cl2(g), Br2(l), I2(s)
I
Two other polyatomic molecules are: sulphur, S8(s) and phosphorous, P4(s).
Eg. The formula for bromine is Br2(l).
The formula for hydrogen gas is H2(g).
Molecular Naming
Molecular Formula
(inc. SATP state)
IUPAC English Name
1. dinitrogen monoxide
2. nitrogen dioxide
3. dinitrogen trioxide
4. NO(g)
5. N2O4(g)
6. N2O5(g)
7. P2O5(s)
8. sulphur hexafluoride
9. sulphur trioxide
10. phosphorus trichloride
11. PCl5(s)
12. CH3OH(l)
13. O2F2(g)
14. CO(g)
15. NH3(g)
16. sucrose
17. C2H5OH(l)
Composition of Chemical Compounds – More Molecular Compounds
1. List the molecular prefixes from one to ten.
2. For which type of molecular substance are these prefixes used?
3. Why is memorisation required for the nomenclature of many molecular substances in this unit?
Molecular Formula (inc. SATP state) IUPAC English Name1. oxygen
2. P2O5(s)
3. hydrogen monochloride
4. NH3(g)
dinitrogen tetrahydride (liquid)
6. PCl5(g)
methane
8. NI3(l)
9. CH3OH( l )
10. sucrose
11. S4N2(s)
12. ethanol
13. CO( )
14. H2O2( )
15. SO3(g)
sulphur
17. propane
Science 10 – Naming Summary PURE SUBSTANCES S1C811.ds4
IONIC COMPOUNDSEmpirical evidence- Form white solids at room temperature.- Can be soluble in water to become (aq) ions.- If not soluble, form solids (s).- Form conducting solutions if soluble in water
Theoretical evidence- They transfer electrons to form + and - ions.- There is an attraction between + and - ions.- Cations - positively charged ions.- Anions - negatively charged ions.- Made of: a metal and a non-metal or
a metal and a polyatomic ion ortwo polyatomic ions.
Naming- Positive ion is named first then negative ion.- The negative ion ends in -ide.- Formula must be written so that the positive
and negative charges are balanced.Stock system- use Roman numerals after the name of any
transition metal to specify the ion charge. 3 exceptions are Al(s), Zn(s) & Ag(s).
Hydrates- are compounds with water molecules as part
of their structure. The hydrate part is named using standard prefixes.
ACIDSEmpirical evidence- Can be solid, liquid or gas in pure form.- Form conducting aqueous solutions.- Form solutions which turn blue litmus pink.- React with active metals and release H2(g).- They taste sour (like vinegar).
Theoretical evidence- the positive ion in acid formulas is the H+ ion.- they dissociate in water to form hydrogen ions (H+
(aq)).
Naming Acids1) hydrogen ____ide hydro_____ic acid2) hydrogen _____ate ______ic acid3) hydrogen _____ite _____ous acid- all acids are written as aqueous (aq).
Bases- Theoretically bases consist primarily of hydroxide (OH-) ions.- Empirically bases taste bitter, feel slippery and turn red litmus paper blue.
MOLECULAR COMPOUNDSEmpirical evidence- Can be solids, liquids and gases at SATP.- Form non-conducting solutions.- Most are not soluble in water.
Theoretical evidence- elements in molecular compounds share
electrons.- molecular compounds form covalent bonds.- Made of two or more non-metals.Naming The following molecular compounds including state and name must be memorized.H2O(l) water H2O2(1)hydrogen peroxideNH3(g) ammonia C12H22O11(s) sucroseCH4(g) methane C3H8(g) propaneCH3OH(l) methanol C2H5OH(l) ethanolC6H12O6(s) glucose O3(g) ozone
- Other molecular compounds are named using the prefix system (mono, di, tri, tetra, penta, hexa, hepta, octa, nona, and deca.)
Polyatomic Molecular Elements- elements that can only exist as two or more atoms of the same substance are:P4(s), S8(s), H2(g), Br2(l), Cl2(g),F2(g), I2(s), N2(g),O2(g)
Composition of Chemical Compounds - Naming Review 1
Complete the following table for the binary ionic compounds and those containing polyatomic ions.
Chemical Formula IUPAC Name Summary of Charges
1. MnCl2(s)
2. AlBr3(s)
3. zinc oxide
4. iron(II) fluoride
5. Ni2O3(s)
6. Cu2S(s)
7. cobalt(II) chloride
8. Al(NO3)3(s)
9. tin(II) chlorite
10. chromium(III) hydroxide
11. Fe2(SO4)3(s)
12. Cu(NO2)2(s)
13. iron(II) dichromate
14. Ag2SO3(s)
15. Ca(HCO3)2(s)
16. aluminum chlorate
17. nickel(III) oxalate
Composition of Chemical Compounds – Review of Naming 2
Predicted Formula
IUPAC Name Summary of Charges
1. K2SO4(s)
2. Ca(HS)2(s)
3. magnesium hypochlorite
4. tin(II) acetate5. chromium(II) sulphite6. iron(III) acetate7. Co(OH)2(s)
8. Cu2SO4(s)
9. Cr3N2(s)
10. Ni2(S2O3)3(s)
11. vanadium(V) silicate12. aluminum sulphate13. nickel(III) chlorate Ni3+, ClO3-, ClO3-, ClO3-,14. Cr(CN)2(s)
15. CuSO45H2O(s)
16. calcium chloride hexahydrate
17. Na2CO310H2O(s)
18. MgSO47H2O(s)
Composition of Chemical Compounds – Review of Naming 3 Complete the following table of ionic compounds.
Predicted Chemical
Formula
IUPAC English Name
1. SrCl2(s)
2. RbBr(s)
3. Na2O(s)
4. aluminum sulphide
5. magnesium iodide
6. TiO2(s)
7. Cu2O(s)
8. tin(II) sulphide
9. chromium(III) oxide
10. iron(II) sulphide
11. KC6H5COO(s)
12. Na2S2O3(s)
13. NH4HCO3(s)
14. ammonium sulphide
15. barium sulphite
16. magnesium hydroxide
17. FeSO47H2O(s)
18. LiCl4H2O(s)
19. sodium sulphate decahydrate
20. Au(NO3)3(s)
21. bismuth(III) sulphate
22. lead(II) acetate trihydrate
23. KMnO4(s)
Composition of Chemical Compounds – Naming Review 4
Predicted Chemical Formula IUPAC English Name
1. CrCl2
2. V2O5
3. Au2S
4. aluminum chloride
5. gallium sulphide
6. barium bromide
7. CaCl2
8. KI
9. Ag2O
10. calcium hydroxide
11. zinc carbonate
12. ammonium phosphate
13. NaCH3COO
14. K2SiO3
15. NH4HSO4
16. lead(II) oxide
17. nickel(II) sulphate
18. manganese(II) chloride
19. MgSO4H2O
20. BaCl24H2O
21. sodium thiosulphate pentahydrate
22. nickel(II) chloride hexahydrate
23. Sb2(SO4)3
24. calcium hydrogen carbonate
Composition of Chemical Compounds – Review of Naming 5 Classify each substance as ionic, molecular or acid. Predict the international chemical formula
(including state of matter at SATP) or the IUPAC English name. Communicate the solubility of the substance in a water environment using (aq) for high solubility and (s, l or g) for low solubility substances.
i,m,a, Chemical Formula Solubility IUPAC English Name
1. PbI2(s)
2. (l) ethanol
3. NaHS(s)
4. sulphurous acid
5. H2O2(l) (l)
6. titanium(IV) oxide
7. Co(NO3)26H2O(s)
8. H2S(g)
9. gallium sulphide
10. sulphuric acid
11. CH4(g) (g)
12. ammonium chromate
13. SO3(g) (g)
14. H2CO3(aq)
15 (g) dinitrogen tetraoxide gas
16. Al2(SO4)3(aq) aluminum sulfate
17. Na2SO3(s)
18. (g) ammonia
19. sodium thiosulphate
pentahydrate
20. (g) chlorine
Composition of Chemical Compounds – Naming Review 6
Complete the following table. Classify the substance as ionic, molecular or acid (i, m, or a) in the first column. Use the subscript to indicate the state of each substance (s, l, g or aq at room temp.)
Chemical Formula Name of Compound i, m or a
1. Al(OH)3( )
2. sodium sulphate
decahydrate
3. sodium nitrate hexahydrate
4. Al2(SO4)3( )
5. calcium chloride hexahydrate
6. NH4NO3( )
7. (g) phosphorous trihydride
8. N2O3(g)
9. (g) methane
10. H2SO4( )
11. H3PO4( )
12. boric acid
13. (NH4)2SO4( )
14. SnF2( )
15. carbonic acid
16. PbO2(s)
17. (s) silicon dioxide
18. NaClO( )
19. potassium permanganate
20. KNO3( )
Composition of Chemical Compounds – Naming Review 7
Chemical Formula Name of Compound i, m, or a21. K2CO32H2O( )
22. hydrofluoric acid23. H2S( g )
24. sodium hydroxide
25. NaHSO4( )
26. magnesium sulphate heptahydrate
27. Ca(OH)2( )
28. sodium thiosulphate
29. CaO( )
30. copper(II) sulphate pentahydrate
31. sulphur
32. B2H8(g)
33. KI( )
34. phosphorus
35. SO3(g)
36. sodium chlorate
37. Na2SiO3( )
38. methanol
39. chlorous acid
40. lead(II) sulphate
41. Ca(HCO3)2( )
42. (g) nitrogen trichloride
43. sodium hydrogen sulphite44. CS2(s)
45. H2S(aq)
46. water
47. aluminum phosphate
48. nitrous acid