Naming and Writing Formulas - NLESDschool.nlesd.ca/~glennlegge/FOV1-00045D53/FOV1-00045D54/Review1… · Molecular compounds are composed of two or more ... chromium (III) oxide r

Review Chemistry 2202 Name:

Naming and Writing Formulas

1. Identify the following as ionic (i) or molecular (m):

Compound LiBr Na2O CF4 Fe2O3 SO2 N2O4 SiO2 PBr3 PbO2 Cu3P2

i or m

2. Write the formulas for the following compounds in the space provided:

a) carbon dioxide k) nitrogen monoxide

b) silicon dioxide l) tetraphosphorus decoxide

c) water m) silicon carbide

d) carbon disulfide n) hydrogen peroxide

e) ammonia o) diphosphorus pentabromide

f) carbon tetrachloride p) arsenic tribromide

g) carbon q) carbon monoxide

h) oxygen r) sulfur dioxide

i) fluorine s) neon

j) diphosphorus trioxide t) dinitrogen tetroxide

3. Write the names for the following compounds, in the space provided:

a) CBr4 k) N2O

b) I2 l) H2O2

c) PF3 m) Br2

d) N2O4 n) Ar

e) CO o) P4

f) NH3 p) ClO2

g) H2O2 q) SiCl2

h) SCl6 r) BH3

i) SO3 s) C2S4

j) P4O6 t) OF2


4. Complete the table below:

Formula Name Name Formula

a) P4O6 k) iodine trifluoride

b) S2F10 l) chlorine dioxide

c) N2O4 m) ammonia

d) ICl5 n) boron trifluoride

e) SF6 o) diboron hexahydride

f) S8 p) phosphorous trihydride

g) S4N2 q) phosphorus pentachloride

h) H2O2 r) carbon disulfide

i) N2O3 s) sulfur trioxide

j) NH3 t) diarsenic trioxide

Prefixes indicate the number of each atom when naming _____________ compounds Molecular compounds are composed of two or more _________________.


a) CaCl2 k) potassium iodide

b) MgO l) aluminum chloride

c) NaBr m) lithium nitride

d) Al2O3 n) barium chloride

e) CaO o) magnesium hydride

f) ZnO p) magnesium chloride

g) Ag2S q) sodium sulfide

h) CaF2 r) zinc sulfide

i) CaH2 s) potassium chloride

j) K2S t) silver bromide



a) Li2O k) zinc iodide

b) CaS l) silver chloride

c) KF m) magnesium nitride

d) Mg2S3 n) barium phosphide

e) CaO o) calcium nitride

f) AlP p) magnesium chloride

g) ZnO q) lithium oxide

h) SrCl2 r) barium iodide

i) MgH2 s) cesium sulfide

j) Li3N t) magnesium bromide

7. Identify the type of ions found in each compound below.

Key: S –only simple ions P –polyatomic ion(s) present M –multi-valent metal ions

Compound CoCl3 Na2O MnCl4 NH4NO3 SrCO3 PbO K2SO4 CoCO3

S, M, and/or P

8. Write names or formulas for each compound using the correct charge for each cation.

a) uranium (IV) oxide k) SnO2

b) lead (IV) sulfide l) Sb2S3

c) manganese (IV) oxide m) HgS

d) iron (III) oxide n) PdS2

e) copper (II) sulfide o) FeS

f) lead (IV) oxide p) HgO

g) tin (II) fluoride q) V2O5

h) chromium (III) oxide r) TiO2

i) uranium (VI) bromide s) AuF3

j) cobalt chloride t) NiBr2


9. Place the symbol for each ion in the space provided. Then write the correct chemical formula and name for the ionic compound. Be sure to balance the charges.

Remember polyatomic ions end in -ite, and -ate, except for cyanide, hydroxide and ammonium.

The first one is completed for you.

Cation Anion Formula

a) aluminum Al 3+ chloride Cl - AlCl3

b) calcium sulfite

c) sodium phosphate

d) copper(II) nitrate

e) chromium(II) nitride

f) silver chromate

g) nickel(III) iodide

h) barium nitride

i) sodium carbonate

j) zinc acetate

k) magnesium hydroxide

l) iron(III) nitrite

m) mercury(I) oxide

n) copper(II) chlorate

o) potassium bromate

p) aluminum hydrogen carbonate

q) lead(II) hydrogen sulfate

r) beryllium iodide

s) mercury(II) nitride

t) ammonium oxide

u) strontium sulfite

v) copper(II) hydrogen sulfate


10. Provide the name or chemical formula of each compound.

Formula Name Name Formula

1. Li2CO3 16. potassium hydroxide

2. K2SO4 17. lithium phosphate

3. Al(OH)3 18. iron (III) hydroxide

4. Fe(ClO)3 19. sodium bicarbonate

5. H2SO4 20. calcium chlorate

6. Ca(HCO3)2 21. hydrogen borate

7. Pb3(PO4)2 22. magnesium silicate

8. Zn(CH3COO)2 23. ammonium nitrate

9. Cu(NO3)2 24. sodium hypochlorite

10. Cu(NO2)2 25. potassium nitrate

11. K2S2O3 26. sodium benzoate

12. CaCO3 27. potassium thiocyanate

13. Na2Cr2O7 28. calcium cyanide

14. NaCN 29. chromium (III) nitrite

15. KH2PO4 30. iron (II) chlorite

11. Provide the name or formula for each hydrate below:

1. copper (II) sulfate pentahydrate

2. MgSO4 • 7 H2O

3. potassium carbonate octahydrate

4. MgCl2 • 6 H2O

5. barium chloride dihydrate

6. Cd(NO3)2 • 4 H2O

7. lithium bromide trihydrate

8. Na2S2O3 • 5 H2O

9. cobalt (II) chloride hexahydrate

10. AlCl3 • 6 H2O

11. zinc sulfate nonahydrate

12. CaCl2 • H2O

13. barium hydroxide monohydrate

14. Na2SO4 • 10 H2O

15. magnesium silicate pentahydrate


Acids: - acids are hydrogen compounds that have been dissolved in water - composed of non-metals(m) - may be solids, liquids or gases or room temperature (m) - dissolve in water to form conducting solutions (i)

Rules for naming acids: Rule 1 hydrogen _____ide becomes hydro_____ic acid

Acid Formula ionic name acid name

HCl(aq) hydrogen chloride hydrochloric acid

HBr(aq)

HCN(aq)

HF(aq)

Rule 2 hydrogen _____ate becomes _____ic acid

HClO3(aq) hydrogen chlorate chloric acid

HNO3(aq)

H2CO3(aq)

H2CrO4(aq)

Rule 3 hydrogen _____ite becomes _____ous acid

HNO2(aq) hydrogen nitrite nitrous acid

HClO2(aq)

HClO(aq)

H2SO3(aq)

*Two exceptions to naming acid rules are acids which have sulf or phosph as roots. Syllables are added to theses acid names to make them sound better. Thus,

H2SO4(aq) is sulfuric acid and H3PO4(aq) is phosphoric acid.


To write formulas, first write the ionic name and then use charges to write the formula. Rule 1 hydrogen _____ide becomes hydro_____ic acid

HCl(aq) hydrogen chloride hydrochloric acid

hydroiodic acid

hydrosulfuric acid

hydroselenic acid

Rule 2 hydrogen _____ate becomes _____ic acid

HClO3(aq) hydrogen chlorate chloric acid

dichromic acid

sulfuric acid

acetic acid

Rule 3 hydrogen _____ite becomes _____ous acid

HNO2(aq) hydrogen nitrite nitrous acid

iodous acid

phosphorous acid

bromous acid

12. Write the name for each acid below:

HNO3(aq) HNO2(aq)

H2SO4(aq) HBr(aq)

H2CrO4(aq) H3PO4(aq)

13. Write the formula for each acid below:

permanganic acid hydrosulfuric acid

sulfurous acid hydrochloric acid

carbonic acid chlorous acid



Formula Acid Name Formula Acid Name

a) H3BO3 (aq) k) HClO4 (aq)

b) hydrochloric acid l) hypochlorous acid

c) CH3COOH(aq) m) H2S (aq)

d) H2SO4 (aq) n) hydrofluoric acid

e) H2SO3 (aq) o) HCN (aq)

f) oxalic acid p) nitrous acid

g) phosphoric acid q) benzoic acid

h) sulfuric acid r) H2SiO3 (aq)

i) H2CO3 (aq) s) thiosulfuric acid

j) nitric acid t) chromic acid

15. Identify the type of compound and use the appropriate rules to complete the table below:

i, m

Formula Name i, m

Name Formula

or a or a

OF2 tetracarbon octahydride

HNO3(aq) molybdenum(III) oxide

Zn3P2 lead(IV) nitrate dihydrate

FeCl2 magnesium perchlorate

CaCO3 beryllium oxide

HBr(aq) bromic acid

HClO2(aq) hydroiodic acid

P3H5 sulfurous acid

SrCl2 cobalt(II) phosphate

S3H5 ammonia

H2O2

lithium permanganate

tetrahydrate

Ca(OH)2 carbon disulfide

AuP boron trihydride


Balance the following chemical equations and identify the reaction type

1 H2O(l) H2(g) + O2(g)

2 N2(g) + H2(g) NH3(g)

3 H2SO4(aq) + NaOH(aq) HOH(l) + Na2SO4(aq)

4 Al(s) + Cu(NO3)2(aq) Cu(s) + Al(NO3)3(aq)

5 Cl2(g) + KBr(aq) Br2(l) + KCl(aq)

6 Pb(NO3)2(aq) + NaI(aq) PbI2(s) + NaNO3(aq)

7 NaOH(aq) + Al2(SO4)3(aq) Al(OH)3(s) + Na2SO4(aq)

8 P4(s) + O2(g) P4O10(s)

9 CH3OH(l) + O2(g) CO2(g) + H2O(g)

10 NO2(g) + H2O(l) HNO3(aq) + NO(g)


Balance the following chemical equations and identify the reaction type Reaction Type

1. H2 + O2 ➞ H2O _____________________

2. S8 + O2 ➞ SO3 _____________________

3. HgO ➞ Hg + O2 _____________________

4. Zn + HCl ➞ ZnCl2 + H2 _____________________

5. Na + H2O ➞ NaOH + H2 _____________________

6. Si2H3 + O2 ➞ SiO2 + H2O _____________________

7. Al(OH)3 + H2SO4 ➞ Al2(SO4)3 + H2O _____________________

8. Fe2(SO4)3 + KOH ➞ K2SO4 + Fe(OH)3 _____________________

9. C7H6 + O2 ➞ CO2 + H2O _____________________

10. Fe2O3 + H2 ➞ Fe + H2O _____________________

11. C7H16 + O2 ➞ CO2 + H2O _____________________

12. SiO2 + HF ➞ SiF4 + H2O _____________________

13. Al2(SO4)3 + Ca(OH)2 ➞ Al(OH)3 + CaSO4_____________________

14. FeCl3 + NH4OH ➞ Fe(OH)3 + NH4Cl _____________________

15. C3H8 + O2 ➞ CO2 + H2O _____________________

16. Al + HCl ➞ AlCl3 + H2 _____________________

17. PCl5 ➞ P4 + Cl2 _____________________

18. H2S ➞ H2 + S8 _____________________

19. Mg + N2 ➞ Mg3N2 _____________________

20. Si2S4 ➞ Si + S8 _____________________


SYNTHESIS and DECOMPOSITION REACTIONS Complete the following questions in the spaces provided.

1. Lithium metal is reacted with nitrogen to produce lithium nitride

Word equation: +

Chemical equation: +

2. Copper (I) oxide is decomposed into its elements

Word equation: +


3. A silver spoon tarnishes when exposed to sulfur (S8).

Word equation: +


4. Pieces of magnesium produce flashes of light when burned in the presence of oxygen

Word equation: +


5. Cobalt(III) fluoride results when cobalt reacts with fluorine

Word equation: +



6. Using heat, sodium bicarbonate is decomposed to produce carbon dioxide and water. (decomposition but not simple)

Word equation: +


7. Phosphorus trifluoride is made from the reaction of phosphorus (P 4) with fluorine.

Word equation: +


8. Shock sensitive nitrogen triiodide is made from nitrogen gas and iodine.

Word equation: +


9. Sulfur dioxide from burning fossil fuels combines with rain water to produce sulfurous acid (acid rain)

Word equation: +


10. Sulfur dioxide forms when solid sulfur burns in oxygen gas.

Word equation: +


12


SINGLE REPLACEMENT

1. Magnesium is reacted with a solution of silver nitrate.

Word equation: + ➔

Chemical equation: + ➔

2. Aluminum is reacted with iron (III) oxide.



3. Copper reacts with a solution of silver sulfate.



+

+

+

+

+

+

4. Iron reacts with hydrochloric acid to produce a gas and one other compound.

Word equation: + ➔ +


+

5. Sentence:


Chemical equation: Br2 (l) + KI(aq) ➔ +


6. Aluminum reacts with sulfuric acid


Chemical equation: + ➔ +

7. Potassium reacts with water (HOH).



8. Zinc metal reacts with lead (II) nitrate solution



9. Sentence:


Chemical equation: K(s) + ZnBr2 (aq) ➔ +

10. Sentence:


Chemical equation: + ➔ Ag(s) + Pb(CH3COO)2(aq)


DOUBLE REPLACEMENT

1. A solution of aluminum chloride is reacted with a solution of potassium hydroxide.



2. A solution of barium chloride is mixed with a solution of silver nitrate.



3. A solution of barium hydroxide is neutralized by carbonic acid



4. A calcium hydroxide solution is neutralized by nitric acid.



5. Sentence:

Word equation: Lead (II) nitrate + Sodium Iodide ➔ +



6. Sentence:

Word equation: + ➔ Cobalt (II) hydroxide + Sodium chloride


7. Lead (II) nitrate is mixed with sodium acetate



8. Phosphoric acid is neutralized by a solution of potassium hydroxide.



9. Sentence:


Chemical equation: CaCO3(s) +HCl (aq) ➔ +

10. Sentence:


Chemical equation: + ➔ Al2S3(s) + Ca(OH)2 (aq)


COMBUSTION

1. Propane ( C3H8 ) burns in a barbecue.



2. Kerosene ( C11H22 ) burns in a lamp.



3. The combustion of gasoline ( C8H18 ) occurs in a lawn mower Word equation: + ➔ +


4. Candlewax ( C25H52 ) provides some heat and light as it burns Word equation: + ➔ +


5. The combustion of methanol ( CH3OH ) is used to keep food trays warm Word equation: + ➔ +


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Naming and Writing Formulas - NLESDschool.nlesd.ca/~glennlegge/FOV1-00045D53/FOV1-00045D54/Review1… · Molecular compounds are composed of two or more ... chromium (III) oxide r