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Химия на английском. Модуль 1

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Министерство образования и науки Российской Федерации Федеральное агентство по образованию Южно-Уральский государственный университет Кафедра аналитической химии

Ш143.21-9 Д182

Е.И. Данилина

ХИМИЯ НА АНГЛИЙСКОМ ЯЗЫКЕ

Модуль 1 БАЗОВЫЕ ХИМИЧЕСКИЕ ПОНЯТИЯ

Учебное пособие

Челябинск Издательство ЮУрГУ

2009

УДК 54(075.8) ББК Ш143.21-923 Д182

Одобрено учебно-методической комиссией химического факультета

Рецензенты:

Балыкин В.П., Бояльская Т.А.

Д182 Данилина, Е.И.

Химия на английском языке. Модуль 1. Базовые химические понятия: учебное пособие. – Челябинск: Изд-во ЮУрГУ, 2008. – 37 с.

Учебное пособие составлено на английском языке по материалам американских и английских учебников по химии для колледжей и университетов и предназначено для практических занятий и самостоятельной работы студентов. В учебном пособии предложены вопросы и задачи, охватывающие круг базовых химических понятий и соответствующие школьному курсу химии. В приложениях приведены необходимые справочные материалы для численного решения задач и их устного чтения: Периодическая таблица, транскрипция названий элементов и соединений по правилам ИЮПАК.

Пособие предназначено для студентов 1 курса химического факультета.

УДК 54(075.8) ББК Ш143.21-923

© Издательство ЮУрГУ, 2009

2

 

 

CONTENTS

 

1.

Formulas and Names of Elements and Compounds..........................................

4

2.

Atomic and Molecular Mass. Mole Concept......................................................

9

3.

Calculating the Percentage by Mass.................................................................

14

4.

Concentration of Solutions...............................................................................

18

5.

Balancing Chemical Equations.........................................................................

21

6.

Calculations Based on Chemical Equations......................................................

25

References.............................................................................................................

 

30

Appendix 1.

Periodic Table of Chemical Elements..............................................

31

Appendix 2.

Elements and Electronegative Components.....................................

33

Appendix 3.

Acids and Anions..............................................................................

36

3

1. FORMULAS AND NAMES OF ELEMENTS AND COMPOUNDS

1.1. What is the chemical symbol for each of the following elements?

a) iron;

b) silver;

c) phosphorus;

d) calcium:

e) mercury;

f) nickel.

1.2. What are the symbols for the following elements?

a) magnesium;

b) manganese:

c) cobalt:

d) argon:

e) silicon;

f) beryllium.

1.3. What is the name of each of the following element?

a) K;

b) Al;

c) C;

d) N;

e) Ne;

f) Na;

g) O;

h) Os;

i) He.

1.4. Give the names of the elements for which the symbols are…

a) H;

b) Rb;

c) Ba;

d) Sr;

e) S;

f) Xe;

g) F;

h) Cl;

i) Bi.

1.5. What are the empirical formulas of each of the following?

a) N2O4;

 

b) C6H12O6;

 

 

 

 

 

 

 

c) C8H8;

 

d) CH3COOH.

 

 

 

 

 

 

 

1.6. The structural formula for glucose is

H

C O

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

H

 

 

 

 

 

 

CH2OH

 

 

 

 

 

C

 

OH

 

 

 

 

 

 

 

 

 

 

 

 

 

 

HO

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

H

 

 

O H

C

 

H

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

H

 

 

 

 

 

H

 

 

 

 

 

 

H

 

 

 

C

 

OH

 

 

 

 

 

 

 

 

 

 

 

OH

 

 

 

H

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

C

 

H

OH

 

 

 

OH

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

CH2OH

 

H

OH

 

 

 

What are the molecular and empirical formulas of glucose?

1.7. Choose the elements that form monoatomic anions from the following list; name the elements and the anions:

Zn, H, Al, S, K, Hg, F, Ag, I, Sb, Cu, V, P, Cl, Na, Si, He, Cs, Br, Cr, N, Fe, Pb, Cd, C, W, Ne, Zr.

4

1.8. How are the cations named in compounds? (Pay attention to Roman numerals.)

+1

+2

+3

+4

 

Mg2+

 

 

Li+

Ca2+

 

 

Na+

Ba2+

Al3+

 

K+

Zn2+

Bi3+

Pb4+

Ag+

Ni2+

Cr3+

Sn4+

Cu+

Fe2+

Fe3+

 

Hg+

Cu2+

Co3+

 

NH4+

Hg2+

 

 

 

Pb2+

 

 

 

Sn2+

 

 

 

Co2+

 

 

1.9. What are the symbols of the following monoatomic anions?

 

 

–1

–2

 

–3

 

bromide

 

 

 

 

chloride

oxide

 

nitride

 

fluoride

peroxide

 

phosphide

 

 

hydride

sulfide

 

 

 

 

iodide

 

 

 

1.10. Name the following compounds:

 

a) MgCl2;

b) AlBr3;

c) Li3N;

 

d) CaO;

e) CaS;

f) Al2O3.

 

1.11. Name the following compounds:

 

a) CrCl3;

b) CuO;

c) Mn2O3;

 

d) SnO2;

e) Hg2Cl2;

f) PbS;

 

g) FeCl3;

h) PbI2;

i) Pb3O4.

 

1.12. Write the formulas of the following compounds:

 

a) calcium chloride;

b) zinc sulfide;

 

c) strontium fluoride;

d) magnesium oxide;

 

e) silver bromide;

f) barium chloride;

 

g) mercury(I) iodide;

h) tin(IV) chloride.

 

1.13. Write the chemical formulas for the following compounds:

 

a) sodium oxide;

b) barium sulfide;

 

c) magnesium nitride;

d) silver iodide;

 

e) calcium carbide;

f) iron(III) chloride.

 

5

1.14. Write the formulas of the following compounds:

a) magnesium bromide;

b) aluminum carbide;

c) copper(I) chloride;

d) barium iodide;

e) silver nitride;

f) zinc fluoride.

1.15. Supply the missing information about the following compounds:

a) SnF2;

 

e) iron(III) sulfide;

b) FeS;

 

f) tin(IV) chloride;

c) PbO2;

 

g) lead(II) oxide;

d) CuBr2;

 

h) chromium(III) chloride.

1.16. Name the following compounds;

a) ICl3;

b) BrF3;

c) AsCl3;

d) SF4;

e) PCl3;

f) SO3.

1.17. Write correct chemical formulas for the following: a) chlorine dioxide; b) silicon tetrafluoride; c) diboron tetrabromide; d) tricarbon disulfide;

e)iodine pentafluoride; f) tetraphosphorus trisulfide.

1.18.Write the chemical formula of each of the following compounds:

a) dinitrogen tetroxide;

b) sulfur hexafluoride;

b) bromine trifluoride;

c) tetraphosphorus decoxide;

d) sulfur dioxide;

e) phosphorus pentachloride.

1.19. Give the name of the following compounds:

a) KCl;

b) Na2S;

c) NaI;

d) SO3;

e) P4O6;

f) N2O3.

1.20. Write down the names for the following polyatomic anions:

–1

–2

–3

–4

OH–

 

 

 

NO3–

SO42–

 

 

MnO4–

CO32–

PO43–

SiO44–

ClO3–

CrO42–

Fe(CN)63–

Fe(CN)64–

HCO3–

Cr2O72–

 

 

CH3COO–

C2O42–

 

 

IO3–

SO32–

 

 

CN–

S2O32–

 

 

6

1.21. Write the correct formula of compounds formed between the following ions, name them:

a) Al3+ and O2–;

b) Mg2+ and N3–;

c) Pb2+ and O2–;

d) NH4+ and CN–;

e) NH4+ and SO42–;

f) Al3+ and SO42–;

g) Fe3+ and OH–;

h) Fe2+ and OH–.

1.22. Write the chemical formulas for the following compounds:

a) magnesium nitrate;

b) silver nitrate;

c) ammonium chromate; d) potassium phosphate;

e) nickel(II) chlorate;

f) copper(I) bromide;

g) zinc phosphate;

h) chromium(III) sulfate;

i) calcium carbonate;

j) potassium permanganate;

k) lead(II) acetate;

l) aluminum hydroxide.

1.23. Write correct formulas for the following compounds:

a) iron(III) sulfide;

b) mercury(I) acetate;

c) ammonium nitrate;

d) calcium bicarbonate;

e) lead(II) chromate;

f) potassium permanganate.

1.24. Write the correct formula of the compounds formed between the corresponding cations and anions, name them:

 

 

 

 

 

 

 

 

 

 

Ions

Cl–

 

O2–

PO43–

SiO32–

OH–

NO3–

SO42–

S2–

Na+

 

 

 

 

 

 

 

 

 

Ca2+

 

 

 

 

 

 

 

 

 

Al3+

 

 

 

 

 

 

 

 

 

1.25. Give the names of the following compounds:

 

 

a) CuSO4;

 

b) Mg3(PO4)2;

 

 

c) BaCrO4;

 

d) K2Cr2O7;

 

 

e) S2Cl2;

 

f) SCl6;

 

 

g) SnBr4;

 

h) Cl2O7;

 

 

i) MgSO4·7H2O;

j) CaSO4·2H2O.

 

1.26. Name the compounds which contain polyatomic ions:

 

 

a) NaNO3;

 

b) SrCO3;

 

 

c) Ca3(PO4)3;

d) KClO3;

 

 

e) Al2(SO4)3;

f) K2Cr2O7.

 

1.27. Write the correct names for the following salts:

 

 

a) CuI;

 

b) CuI2;

 

 

c) SnCl2;

 

d) SnCl4;

 

 

e) CoSO4;

 

f) Co2(SO4)3.

 

7

1.28. Write the correct formulas of the compounds formed between the corresponding cations and anions:

 

 

Oxide

Iodide

 

Phosphate

 

Permanganate

Sodium

 

 

 

 

 

 

 

Silver

 

 

 

 

 

 

 

Zinc

 

 

 

 

 

 

 

Ammonium

 

 

 

 

 

 

 

Copper(I)

 

 

 

 

 

 

 

Iron(II)

 

 

 

 

 

 

 

Iron(III)

 

 

 

 

 

 

 

Lead(IV)

 

 

 

 

 

 

 

 

 

Sulfide

Hydroxide

 

Chromate

 

Carbonate

Sodium

 

 

 

 

 

 

 

Silver

 

 

 

 

 

 

 

Zinc

 

 

 

 

 

 

 

Ammonium

 

 

 

 

 

 

 

Copper(I)

 

 

 

 

 

 

 

Iron(II)

 

 

 

 

 

 

 

Iron(III)

 

 

 

 

 

 

 

Lead(IV)

 

 

 

 

 

 

 

1.29. Supply the missing information for each of the following:

 

a) PbCrO4;

b) dihydrogen monoxide;

 

c) (NH4)2Cr2O7;

d) sodium thiosulfate;

 

 

 

e) MgCl2.6H2O;

f) potassium ferricyanide;

 

g) P4O6;

h) sodium sulfate decahydrate;

 

i) CBr4;

j) phosphorus tribromide.

 

1.30. Supply the missing information for the following compounds:

 

a) KMnO4;

b) sodium nitrate;

 

 

 

c) FePO4;

d) silver phosphate;

 

 

 

e) FeSO4.7H2O;

f) cobalt(II) sulfate;

 

 

 

g) Si2F6;

h) lead(IV) acetate;

 

 

 

i) Cl2O;

j) potassium carbonate.

 

 

 

1.31. Supply the missing information for the following:

 

a) (NH4)2SO4;

b) sodium chromate;

 

 

 

c) NaOH;

d) calcium cyanide;

 

 

 

e) Cu3(PO4)2;

f) potassium chlorate;

 

 

 

g) Al2(CO3)3;

h) potassium oxalate;

 

 

 

i) Pb(IO3)2;

j) chromium(III) nitrate.

 

 

 

 

8

 

 

 

 

2.ATOMIC AND MOLECULAR MASS. MOLE CONCEPT

2.1.The ratio of the mass of oxygen to carbon atom is 1.3329. What is the mass of the oxygen atom?

2.2.The ratio of the mass of bromine atom to carbon is 6.650. What is the mass of the bromine atom?

2.3.Calculate the number of moles in each of the following:

a)3.01x1022 N2 molecules;

b)4.82x1024 iron atoms.

2.4.Perform the following interconversions of mole and partical number:

a)6.02x1022 Fe atoms = ? mol Fe atoms;

b)2 mol O2 molecules = ? O2 molecules;

c)1.2x1025 H2O molecules = ? mol H2O molecules;

d)0.25 mol H+ ions = ? H+ ions.

2.5.How many years does it take to evaporate all the molecules in one millimole of water, if six billion (6x109) water molecules evaporate in each second?

2.6.Answer these questions for 0.25 mol of Al2O3. Find:

a)the number of molecules it contains;

b)the mole number of each kind of atom it contains;

c)the total number of atoms it contains.

2.7.Answer these questions for 2.4x1024 SO3 molecules. Find:

a)its mole number;

b)the number of moles of S and O atoms it contains;

c)the total number of atoms it contains.

2.8.Answer these questions for 26 g of chromium. Calculate:

a)the mole number of atoms it contains;

b)the number of atoms it contains;

c)the mass of a single chromium atom (pay attention to the differences between atomic mass and the actual mass of an atom).

2.9.How many grams of each of the constituent elements are contained in one mole

of: a) CH4; b) Fe2O3; c) Ca3P2? How many atoms of each element are contained in the same amount of compound?

2.10.Calculate the number of grams in a mole of each of the following common substances: a) calcite, CaCO3;

b)quartz, SiO2;

9

c)cane sugar, C12H22011;

d)gypsum, CaSO4.2H2O;

e)white lead, Pb(OH)2.

2.11. Calculate the molar mass of each of these compounds:

a) CO2;

b) Ca3(PO4)2;

c) CuSO4·5H2O;

d) Fe(NH4)2(SO4)2 ·6H2O.

2.12. Calculate the molar mass of the following compounds:

a) N2O5;

b) H2SO4;

c) Al(OH)3;

d) KAl(SO4)2·12H2O;

e) Fe4[Fe(CN)6]3.

2.13.What is the mass of 1.00 mole of each of the following nitrogen compounds: N2O; NO; NO2; NH3; N2H4; HN3?

2.14.Determine the molar mass for:

a) LiOH; b) H2SO4; c) O2;

d)S8; e) Ca3SO4; f) K4[Fe(CN)6].

2.15.Perform the following conversions:

a)3.2 g Cu = ? mol Cu;

b)0.2 mol Ag = ? g Ag;

c)3.01x1022 Fe atoms = ? mol Fe atom = ? g Fe;

d)1 silver atom = ? g;

e)6.4 g S atom = ? mol S atom = ? S atoms.

2.16.List the following species in order of increasing mass:

a)1 mol C atom;

b)1 g of C;

c)1 carbon atom;

d)3.01x1023 C atoms.

2.17.Which one of the following is the heaviest?

a)3.02x1023 Mg atoms;

b)0.2 mol S atom;

c)10.8 g of Ag;

d)1 mol Li.

2.18.How many moles of atoms are contained in:

a) 32.7 g Zn;

b) 7.09 g C1;

c) 95.4 g Cu;

d) 4.31 g Fe;

e) 0.378 g S?

 

2.19. Calculate, how many moles are represented by:

a) 24.5 g H2SO4;

b) 4.00 g O2.

10

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