TALIGAMAN NATIONAL HIGH SCHOOLButuan City

SCIENCE IIITHIRD PERIODICAL EXAMINATION

(S.Y. 2011-2012)

NAME: __________________________________ YR.&SEC. ______________ SCORE: ____

Encircle the letter that best corresponds to your answer.

1. Which is a gas in liquid solution?a. alcohol in water b. carbonated drink c. air d. brass

2. Which of the following is not a solution?a. sugar dissolved in water c. mayonnaiseb. amalgram d. oxygen dissolved in water

3. The salt that is dissolved in water to make a solution is called ___________a. sediment b. tincture c. solute d. solvent

4. In which of the following solvents will table salt readily dissolve?a. alcohol b. kerosene c. oil d. water

5. In the preparation of some candied fruits, sliced fruits are cooked in a solution of sugar in water. Upon cooling, sugar crystallized on the surface of the fruit pieces. What type of sugar solution was used?a. dilute b. saturated c. unsaturated d. supersaturated

6. What should you do to dissolve more solid solute in a saturated liquid solution?a. Stir the solution. c. Apply heat to the solution.b.Reduce the pressure on the solution. d. Remove some solvent from the solution

7. The rate of dissolution of a particular substance is affected by_____________a. stirring b. liquid solutes c. size of particles d. all of the stated

8. The amount of substance that dissolves in another substance is affected by _____________a. nature of substance b. temperature c. pressure d. stirring

9. Ice cream vendors use rock salt to prolong the coldness due to ice cubes. What colligative property is being shown?

a. boiling point elevation c. freezing point lowering b. vapor pressure lowering d. osmotic pressure

10.What is the common name for colloids with liquid as dispersion medium and solid as the dispersed phase.a. sol b. emulsion c. gel d. aerosol

11.Which demonstrates the adsorptive property of colloids?a. cloud seeding c. using charcoal to remove unpleasant odorsb. adding egg yolk in preparing mayonnaise d. using a kidney machine in dialysis

12.Which describes the process of dialysis in purifying colloids?a. separating ions through a semi-permeable membraneb. movement of charged colloidal particles towards the electrodesc. clustering of very small particles into colloidal sized. breaking very large particles into colloidal size

13.Which statement best describes a metallic bond?a. It is the attraction between molecules for each other.b. It is the sharing of electrons between atoms.c. It is the transfer of electrons from one atom to another.d. It is the attraction provided by mobile electrons for a network of positive ions.

14.When you cut an electric copper wire, what force of attraction is broken?a. covalent bond b. ionic bond c. metallic bond d. hydrogen bond

15.Which of the following pairs of elements will form an ionic bond?a. Cl and Br b. H and Cl c. Na and Cl d. C and Cl

16.Which of the following shows the highest tendency to form an ionic bond?a. metal and a nonmetal c. two nonmetalsb. noble gas elements d. two metal elements

17. A pair of elements has an electronegativity difference of 0.28. What type of bond between atoms are formed?a. nonpolar covalent bond c. ionic bondb. polar covalend bond d. hydrogen bond

18.Which of the molecules below is held by polar covalent bonds?a. Cl – Cl b. Si – Si c. O = O d. C – Cl

19.Which formula indicates the actual number of atoms of the element in a molecule of a compound?a. empirical formula c. molecular formulab. structural formula d. simplest formula

20.Which of the following is the simplest form or the empirical formula of Benzene (C6H6)?a. CH b. C2H2 c. C3H3 d. CH2

21.Which of the following formula is correctly written?a. ZnCl b. HgCl c. NH4SO4 d. H2S

22.The following statements are true for Polar Covalent bonds except one. What statement describes the Nonpolar covalent bond?

a. It can be formed by atoms of different elementsb. It is when the molecules are electrically uniform c. It is when the molecules resulted from unsymmetrical shape.d. It can be formed when the central atom is bonded to different substituent atoms

23.Which of the following intermolecular force that resulted from the attraction of electrons of an atom to the nucleus of a nearby atom?a. London dispersion force c. hydrogen bondb. dipole – dipole force d. ion-dipole attraction

24. The chemical formula of water is H2O. What holds the molecules of water together?a. hydrogen bond b. ionic bond c. metallic bond d. covalent bond

25.Which of the following is the weakest bond?a. hydrogen bond c. polar covalent bondb. dipole interaction d. ionic bond

26.Which one of the following involves a change of phase?a. changing water into steam c. filtering sand from sand and waterb. mixing vinegar with water d. grinding coffee beans into powder

27.Which of the following changes will not produce a new substance?a. burning of wood c. rusting of iron nailb. melting of butter d. decaying of garbage

28.The following processes involves a chemical change, which one does not?a. generation of gas from manure c. digestion of foodb. distillation of water d. fermentation of coconut water into vinegar

29.Which of the following is true of different substances having an equal number of moles?

a.They have equal masses. c. They have the same amount of energy.b. They have equal volume per unit mass. d. They have equal number of particles.

30.How many H2O molecules are contained in one mole of water?a. 6.02 x 1023 b. 60.23 x 1023 c. 6.02 x 1022 d. 6.02 x 1020

31.Which of the following represents a mole of a substance?Atomic mass: Ca = 40 amu F = 19 amu H = 1 amu

Ne = 20 amu O = 16 amu Li = 6.94 amu

a. 80.0 g calcium atoms c. 44.9 g of lithium fluoride saltb. 1.00 g of hydrogen molecules d. d. 20.0 g of neon atoms

32.Carbonic acids has the formula H2CO3. The molar masses of the components elements are:H = 1 g/mole; C = 12 g/mole; O = 16 g/mole

What is the molar mass of H2CO3?a. 50 g/mole c. 10 g/moleb. 62 g/mole d. 40 g/mole

33.Which of the following laws states that the total mass of the reactants is equal to the total mass of the product?a. Law of definite composition c. Law of conservation of massb. Law of conservation of energy d. Law of inertia

34.Dalton’s Atomic Theory explains the laws of chemical changes. Which of Dalton’s assumptions explains the Law of Conservation of Mass?

a. An atom is the smallest particle of an element.b. In ordinary chemical reactions, no new atoms are created and no old ones are destroyed.c. Atoms of a given element have the same properties of size, shape and mass.d. Atoms combine in ratios of small whole numbers.

35. In the reaction: A + B C, 10 g of A reacted with B to produce 25 g of C. The mass of B that reacted is 15g, Which law is being illustrated?a. Dalton’s Law c. Law of Multiple Proportionb. Law of Conservation of Mass d. Law of Definite Composition

For items 36-38:In a mixture of 20g of Sodium chloride (NaCl) and 180g of water (H2O), given the formula:

% by mass of solute = mass of solute x 100 mass of the solution

36. What is the total mass of the solution?a. 20g b. 180g c. 200g d. 160g

37.What is the percentage by mass composition of Sodium chloride (NaCl)?a. 10% b. 20% c. 90% d. 80%

38. What is the percentage by mass composition of water (H2O) in item 36?a. 10% b. 20% c. 90% d. 80%

39. Powdered copper when heated in an atmosphere of oxygen produces copper(II) oxide according to the chemical equation:

2 Cu + O2 2 CuO

What is the mass of copper (II) oxide that forms when all reactants combined?a. The same as the mass of copper that combines with oxygen.b. Twice the mass of oxygen that combines with copper.c. The sum of the masses of copper and oxygen that combined.d. The sum of twice the mass of copper and the mass of oxygen that combined.

40.Which reaction below is not a combination reaction?a. 2 Na + Cl2 2 NaClb. 2 H2 + O2 2 H2O

c. 4 Fe + 3 O2 2 Fe2O3

d. CaCO3 CaO + CO2

41.What type of reaction is shown by the equation below?Zn + 2 NaOH H2 + Na2ZnO2

a. combination c. single displacementb. decomposotion d. double replacement

42.Given these two chemical reactions:I. 2 KNO3 2 KNO2 + O2

II. Fe + S FeS

What type of chemical reactions are I and II?a. I – combination reaction c. I – double displacement reaction II – decomposition reaction II – displacement reaction

b. I – displacement reaction d. I – decomposition reaction II – double displacement reaction II – combination reaction

43.What products form when potassium nitrate decomposes?a. Potassium nitrate and oxygen c. Potassium, oxygen and nitrogenb. Potassium nitrite and oxygen d. Potassium oxide and nitrogen

44.What is the chemical formula of the compound formed when Mg reacts with S?a. MgS2 c. MgSb. Mg2 d. Mg2S3

45. What is the correct formula of iron(III) sulfate?a. FeS c. Fe2(SO4)3

b. Fe3(SO4)2 d. FeSO4

46.How many atoms of C are present in a compound with a chemical formula K4[Fe(CN)6]2?a. 4 b. 6 c. 12 d. 48

47.The following equation are not correctly balance except one, What chemical equation below is correctly balanced?a. H2 + O2 H2O c. Mg + 2 HCl MgCl2b. SO2 + O2 SO3 d. Zn + 2 H2SO4 ZnSO4 + 2H2

48.Which of the following equations describes the complete balanced decomposition of potassium chlorate?

a. 2 KClO3 2 KCl + 2 O2 c. 2 KClO2 2 KCl + 4 O2

b. 2 KClO3 2 KCl + 3 O2 d. 2 KClO 2 KCl + O2

49.Which is the correct coefficient of oxygen in the equation C3H8 + O2 3 CO2 + 4 H2Oa. 3 b. 4 c. 5 d. 6

50.Which of the following is not correctly balanced?a. NaCl + AgNO3 NaNO3 + AgCl c. N2 + H2 NH3

b. 4 Fe + 3O2 2 Fe2O3 d.2 Na + 2 H2O 2 NaOH + H2

GOOD LUCK!!!

Prepared by: Rosevil Famorcan Dangate

TALIGAMAN NATIONAL HIGH SCHOOLButuan City

SCIENCE III

THIRD PERIODICAL EXAMINATION(S.Y. 2011-2012)

ANSWER KEY

1.B 11.C 21.D 31.D 41.C2.C 12.A 22.B 32.B 42.D3.C 13.D 23.A 33.C 43.B4.D 14.C 24.A 34.B 44.C5.C 15.C 25.B 35.B 45.C6.C 16.A 26.A 36.C 46.C7.B 17.A 27.B 37.A 47.D8.D 18.D 28.B 38.C 48.B9.C 19.C 29.D 39.C 49.C10.A 20.A 30.A 40.D 50.C

_________________________________________________________________________________________________

TALIGAMAN NATIONAL HIGH SCHOOLButuan City

SCIENCE IIITHIRD PERIODICAL EXAMINATION

(S.Y. 2011-2012)ANSWER KEY

1.B 11.C 21.D 31.D 41.C2.C 12.A 22.B 32.B 42.D3.C 13.D 23.A 33.C 43.B4.D 14.C 24.A 34.B 44.C5.C 15.C 25.B 35.B 45.C6.C 16.A 26.A 36.C 46.C7.B 17.A 27.B 37.A 47.D8.D 18.D 28.B 38.C 48.B9.C 19.C 29.D 39.C 49.C10.A 20.A 30.A 40.D 50.C

TALIGAMAN NATIONAL HIGH SCHOOLButuan City

SCIENCE IIITHIRD PERIODICAL EXAMINATION

(S.Y. 2011-2012)

NAME: __________________________________ YR.&SEC. ______________ SCORE: ____

Encircle the letter that best corresponds to your answer.

2. Which is a gas in liquid solution?a. alcohol in water b. carbonated drink c. air d. brass

24.Which of the following is not a solution?a. sugar dissolved in water c. mayonnaiseb. amalgram d. oxygen dissolved in water

25.The salt that is dissolved in water to make a solution is called ___________a. sediment b. tincture c. solute d. solvent

26. In which of the following solvents will table salt readily dissolve?a. alcohol b. kerosene c. oil d. water

27. In the preparation of some candied fruits, sliced fruits are cooked in a solution of sugar in water. Upon cooling, sugar crystallized on the surface of the fruit pieces. What type of sugar solution was used?a. dilute b. saturated c. unsaturated d. supersaturated

28.What should you do to dissolve more solid solute in a saturated liquid solution?a. Stir the solution. c. Apply heat to the solution.b.Reduce the pressure on the solution. d. Remove some solvent from the solution

29.The rate of dissolution of a particular substance is affected by_____________a. stirring b. liquid solutes c. size of particles d. all of the stated

30.The amount of substance that dissolves in another substance is affected by _____________a. nature of substance b. temperature c. pressure d. stirring

31. Ice cream vendors use rock salt to prolong the coldness due to ice cubes. What colligative property is being shown?

a. boiling point elevation c. freezing point lowering b. vapor pressure lowering d. osmotic pressure

32.What is the common name for colloids with liquid as dispersion medium and solid as the dispersed phase.a. sol b. emulsion c. gel d. aerosol

33.Which demonstrates the adsorptive property of colloids?a. cloud seeding c. using charcoal to remove unpleasant odorsb. adding egg yolk in preparing mayonnaise d. using a kidney machine in dialysis

34.Which describes the process of dialysis in purifying colloids?a. separating ions through a semi-permeable membraneb. movement of charged colloidal particles towards the electrodesc. clustering of very small particles into colloidal sized. breaking very large particles into colloidal size

35.Which statement best describes a metallic bond?a. It is the attraction between molecules for each other.b. It is the sharing of electrons between atoms.c. It is the transfer of electrons from one atom to another.d. It is the attraction provided by mobile electrons for a network of positive ions.

36.When you cut an electric copper wire, what force of attraction is broken?a. covalent bond b. ionic bond c. metallic bond d. hydrogen bond

37.Which of the following pairs of elements will form an ionic bond?a. Cl and Br b. H and Cl c. Na and Cl d. C and Cl

38.Which of the following shows the highest tendency to form an ionic bond?a. metal and a nonmetal c. two nonmetalsb. noble gas elements d. two metal elements

39. A pair of elements has an electronegativity difference of 0.28. What type of bond between atoms are formed?a. nonpolar covalent bond c. ionic bondb. polar covalend bond d. hydrogen bond

40.Which of the molecules below is held by polar covalent bonds?a. Cl – Cl b. Si – Si c. O = O d. C – Cl

41.Which formula indicates the actual number of atoms of the element in a molecule of a compound?a. empirical formula c. molecular formulab. structural formula d. simplest formula

42.Which of the following is the simplest form or the empirical formula of Benzene (C6H6)?a. CH b. C2H2 c. C3H3 d. CH2

43.Which of the following formula is correctly written?a. ZnCl b. HgCl c. NH4SO4 d. H2S

44.The following statements are true for Polar Covalent bonds except one. What statement describes the Nonpolar covalent bond?

a. It can be formed by atoms of different elementsb. It is when the molecules are electrically uniform c. It is when the molecules resulted from unsymmetrical shape.d. It can be formed when the central atom is bonded to different substituent atoms

45.Which of the following intermolecular force that resulted from the attraction of electrons of an atom to the nucleus of a nearby atom?a. London dispersion force c. hydrogen bondb. dipole – dipole force d. ion-dipole attraction

24. The chemical formula of water is H2O. What holds the molecules of water together?a. hydrogen bond b. ionic bond c. metallic bond d. covalent bond

36.Which of the following is the weakest bond?a. hydrogen bond c. polar covalent bondb. dipole interaction d. ionic bond

37.Which one of the following involves a change of phase?a. changing water into steam c. filtering sand from sand and waterb. mixing vinegar with water d. grinding coffee beans into powder

38.Which of the following changes will not produce a new substance?a. burning of wood c. rusting of iron nailb. melting of butter d. decaying of garbage

39.The following processes involves a chemical change, which one does not?a. generation of gas from manure c. digestion of foodb. distillation of water d. fermentation of coconut water into vinegar

40.Which of the following is true of different substances having an equal number of moles?

a.They have equal masses. c. They have the same amount of energy.b. They have equal volume per unit mass. d. They have equal number of particles.

41.How many H2O molecules are contained in one mole of water?a. 6.02 x 1023 b. 60.23 x 1023 c. 6.02 x 1022 d. 6.02 x 1020

42.Which of the following represents a mole of a substance?Atomic mass: Ca = 40 amu F = 19 amu H = 1 amu

Ne = 20 amu O = 16 amu Li = 6.94 amu

a. 80.0 g calcium atoms c. 44.9 g of lithium fluoride saltb. 1.00 g of hydrogen molecules d. d. 20.0 g of neon atoms

43.Carbonic acids has the formula H2CO3. The molar masses of the components elements are:H = 1 g/mole; C = 12 g/mole; O = 16 g/mole

What is the molar mass of H2CO3?a. 50 g/mole c. 10 g/moleb. 62 g/mole d. 40 g/mole

44.Which of the following laws states that the total mass of the reactants is equal to the total mass of the product?a. Law of definite composition c. Law of conservation of massb. Law of conservation of energy d. Law of inertia

45.Dalton’s Atomic Theory explains the laws of chemical changes. Which of Dalton’s assumptions explains the Law of Conservation of Mass?

a. An atom is the smallest particle of an element.b. In ordinary chemical reactions, no new atoms are created and no old ones are destroyed.c. Atoms of a given element have the same properties of size, shape and mass.d. Atoms combine in ratios of small whole numbers.

46. In the reaction: A + B C, 10 g of A reacted with B to produce 25 g of C. The mass of B that reacted is 15g, Which law is being illustrated?a. Dalton’s Law c. Law of Multiple Proportionb. Law of Conservation of Mass d. Law of Definite Composition

For items 36-38:In a mixture of 20g of Sodium chloride (NaCl) and 180g of water (H2O), given the formula:

% by mass of solute = mass of solute x 100 mass of the solution

51. What is the total mass of the solution?a. 20g b. 180g c. 200g d. 160g

52.What is the percentage by mass composition of Sodium chloride (NaCl)?a. 10% b. 20% c. 90% d. 80%

53. What is the percentage by mass composition of water (H2O) in item 36?a. 10% b. 20% c. 90% d. 80%

54. Powdered copper when heated in an atmosphere of oxygen produces copper(II) oxide according to the chemical equation:

2 Cu + O2 2 CuO

What is the mass of copper (II) oxide that forms when all reactants combined?a. The same as the mass of copper that combines with oxygen.b. Twice the mass of oxygen that combines with copper.c. The sum of the masses of copper and oxygen that combined.d. The sum of twice the mass of copper and the mass of oxygen that combined.

55.Which reaction below is not a combination reaction?a. 2 Na + Cl2 2 NaClb. 2 H2 + O2 2 H2O

c. 4 Fe + 3 O2 2 Fe2O3

d. CaCO3 CaO + CO2

56.What type of reaction is shown by the equation below?Zn + 2 NaOH H2 + Na2ZnO2

a. combination c. single displacementb. decomposotion d. double replacement

57.Given these two chemical reactions:I. 2 KNO3 2 KNO2 + O2

II. Fe + S FeS

What type of chemical reactions are I and II?c. I – combination reaction c. I – double displacement reaction II – decomposition reaction II – displacement reaction

d. I – displacement reaction d. I – decomposition reaction II – double displacement reaction II – combination reaction

58.What products form when potassium nitrate decomposes?a. Potassium nitrate and oxygen c. Potassium, oxygen and nitrogenb. Potassium nitrite and oxygen d. Potassium oxide and nitrogen

59.What is the chemical formula of the compound formed when Mg reacts with S?a. MgS2 c. MgSb. Mg2 d. Mg2S3

60. What is the correct formula of iron(III) sulfate?a. FeS c. Fe2(SO4)3

b. Fe3(SO4)2 d. FeSO4

61.How many atoms of C are present in a compound with a chemical formula K4[Fe(CN)6]2?a. 4 b. 6 c. 12 d. 48

62.The following equation are not correctly balance except one, What chemical equation below is correctly balanced?a. H2 + O2 H2O c. Mg + 2 HCl MgCl2b. SO2 + O2 SO3 d. Zn + 2 H2SO4 ZnSO4 + 2H2

63.Which of the following equations describes the complete balanced decomposition of potassium chlorate?

a. 2 KClO3 2 KCl + 2 O2 c. 2 KClO2 2 KCl + 4 O2

b. 2 KClO3 2 KCl + 3 O2 d. 2 KClO 2 KCl + O2

64.Which is the correct coefficient of oxygen in the equation C3H8 + O2 3 CO2 + 4 H2Oa. 3 b. 4 c. 5 d. 6

65.Which of the following is not correctly balanced?a. NaCl + AgNO3 NaNO3 + AgCl c. N2 + H2 NH3

b. 4 Fe + 3O2 2 Fe2O3 d.2 Na + 2 H2O 2 NaOH + H2

GOOD LUCK!!!

Prepared by: Rosevil Famorcan Dangate