Science 8 3rd Q RUQA Past Paper PDF

REGIONAL UNIFIED QUARTERLY ASSESSMENT (RUQA) SY 2024-2025 THIRD Quarter – Grade 8 (Science) ----------------------------------------------------------------------------------------------------------- GENERAL INSTRUCTIONS: Do not write an...

REGIONAL UNIFIED QUARTERLY ASSESSMENT (RUQA) SY 2024-2025 THIRD Quarter – Grade 8 (Science) ----------------------------------------------------------------------------------------------------------- GENERAL INSTRUCTIONS: Do not write anything on this test paper. After carefully reading all the questions, reflect on all your answers in a separate ANSWER SHEET. Shade the circle that corresponds to your chosen answer. For questions 1-3, refer to the figure and statements below. Figure 1. There are three (3) main phases of matter namely; solid, liquid, and gas. In molecular level, each phase varies accordingly to its molecular spacing, movement and attraction. Figure 1 above illustrates the said properties between molecules among the phases of matter. www.SciChem.com 1. Which of the following describes the particles of the solids? I. Particles are locked into place and are not compressible. II. Particles have lots of free space between them and are compressible. III. Particles flow easily and assume the shape and volume of the container. IV. Particles have unnoticeable space between them and are not capable of flowing. a. I and II b. II and III c. III and IV d. I and IV 2. Which among the phases of matter is dependent on container in order to acquire its shape? a. liquid b. solid c. liquid & gas d. liquid & soli 3. The spacing structure affects the movement of molecules of matter and when there is heat transfer, molecules will move and vibrate. What is your prediction on the movement of gas molecules? a. Gas molecules will be stationary. b. Gas molecules will move but almost negligible. c. Gas molecules will move but at a very limited distance. d. Gas molecules will move freely in space at high speed. 4. Which of the following statements best explain why solids have definite shape and volume while gases don’t have this property? a. Because the particles of solid are in close contact with one another and are loosely arranged, held by a very weak molecular attraction while gas particles are in close contact with one another and held by a weak molecular force b. Because the particles of solid are packed tightly together, often in an orderly arrangement and held by a strong molecular force while gas particles are  much farther apart and are loosely arranged with negligible attraction between each particle. c. Because the particles of solid are in close contact with one another, the arrangement is not rigid and held by a weak molecular force while the particles of gas are much farther apart and are loosely arranged with negligible attraction between each particle. d. Because the particles of solids are packed tightly together, often in an orderly arrangement and held by a strong molecular force while particles of gases are in close contact with one another and the arrangement is not rigid and it is held by a weak molecular force. 5. How does the arrangement of particles relate to the forces of attraction? a. The closer the particles to each other, the weaker the force of attraction between them. b. The closer the particles to each other, the stronger the force of attraction between them. c. The farther the particles to each other, the weaker the force of attraction between them. d. Either closer or farther the particles to each other, the force of attraction stays the same. 6. How does increasing the temperature affect the arrangement of particles in different phases of matter? a. Increasing the temperature causes particles to transition from solid to liquid to gas phases. b. Increasing the temperature causes particles to become more spread out in solids, liquids, and gases. c. Increasing the temperature has no effect on the arrangement of particles in solids, liquids, and gases. d. Increasing the temperature leads to particles becoming more tightly packed in solids, liquids, and gases. For questions 7-10, Refer to the Information below The number of protons, neutrons, and electrons in an atom can be determined from a set of simple rules. First, the number of protons in the nucleus of the atom is equal to the atomic number (Z). Second, the number of electrons in a neutral atom is equal to the number of protons. Third, the mass number of the atom (M) is equal to the sum of the number of protons and neutrons in the nucleus. Lastly, the number of neutrons is equal to the difference between the mass number of the atom (M) and the atomic number (Z) Isotope Element Name Atomic Mass # of p+ # of e # of n o charge No. No. B-11 Boron 5 11 5 5 6 0 N-14 Nitrogen 7 14 7 7 7 0 Ne-20 Neon 10 20 10 10 10 0 7. What does the atomic number of an atom represent? a. Electrons only b. Neutrons c. Protons D. No.Of protons and or electrons 8. How many neutrons are there in the element Boron? a. 0 b. 5 c. 6 d. 7 9. How do you calculate the number of electrons in a neutral atom? I. The number of electrons is equal to the number of protons. II. Subtract the number of protons from the number of neutrons. III. Subtract the number of protons from the atomic mass number. IV. Subtract the number of neutrons from the atomic mass number. a. I only b. I and III c. I and II d. II and IV 10. Based on the table presented, which of the following describes the mass number of an atom? I. It is equal to the number of protons in the nucleus. II. Has the same number as of electrons. III. It is equal to the sum of the number of protons and neutrons in the nucleus. IV. It is equal to the atomic number of the atom. a. I only b. III only c. I and III d. II and IV 11. The atomic number of an atom is 8, and its atomic mass number is How many protons, neutrons, and electrons are present in this atom? a. Protons: 8, Neutrons: 8, Electrons: 8 b. Protons: 8, Neutrons: 8, Electrons: 16 c. Protons: 16, Neutrons: 8, Electrons: 8 d. Protons: 8, Neutrons: 16, Electrons: 8 12. Which statement compares the masses of two subatomic particles? a. The mass of a proton is greater than the mass of a neutron. b. The mass of a proton is greater than the mass of an electron. c. The mass of an electron is greater than the mass of a proton. d. The mass of an electron is greater than the mass of a neutron. 13. Which of the following BEST explains the correlation between the number of electrons in a neutral atom and the number of protons? a. They are inversely proportional which means the greater the number of electrons the lesser the number of protons. b. They are directly proportional meaning if the number of electrons increases the number of protons will also increase. c. There is no correlation, they have no relationship at all meaning they are independent of each other. d. The number of electrons is always double the number of protons, meaning the number of electrons is two times higher than the number of protons. 14. Which two factors are influenced by the group number of an element? a. Reactivity and atomic mass b. Periodicity and chemical properties  c. Atomic radius and valence electrons d. Ionization energy and electronegativity 15. How do atomic radius trends impact ionization energy and electronegativity? a. Higher atomic radius leads to lower ionization energy and higher electronegativity. b. Lower atomic radius leads to higher ionization energy and lower electronegativity. c. Atomic radius has no impact on ionization energy or electronegativity. d. Atomic radius affects ionization energy but not electronegativity. For questions 16-21 Refer to the Information below The development of the periodic table could be traced back in 1817 to the work of Johann Dobereiner, a German scientist who formed triads of elements with similar properties like triad of calcium, barium and strontium. In 1863, John Newlands, an English chemist proposed the Law of Octaves. He based his classification of elements on the fact of similar properties could be noted for every eight element when they are arranged in order of increasing atomic masses. Around 1869 two scientists determined away to put the elements in order. Lothar Meyer and Dmitri Mendeleev both came up with the periodic table that showed how elements should be grouped according to increasing atomic mass. In 1914 Mosely, an English physicist arranged the element according to increasing atomic number. As more information was gathered about existing and newly discovered elements, irregularities were discovered. Some newly identified elements had properties that did not match those of the groups already included in the periodic table. To fit into the right groups, the positions of a few elements had to be rearranged. There were even elements that had to be placed in the table as a new group. The table was thus revised. J.J. Thomson's discovery of electrons and the shift to arranging elements by atomic number refined the table. Today, the periodic table is organized by the periodic law, emphasizing similarities in outer electron configurations within columns, grouping elements with similar traits. 16. Who formed the triads of elements? a. Dmitri Mendeleev b. Johann Dobereiner c. John Newlands d. Lothar Meyer 17. What is the current basis for organizing the periodic table? a. Periodic law b. Atomic number c. Atomic mass d. Electron configuration 18. Sequence the development of modern periodic table of elements. I. elements are arranged according to increasing atomic number by Mosely II. elements are arranged with similar properties based on triads by Johann Dobereiner III. elements are arranged with similar properties based on octaves according to John Newlands IV. elements are arranged according to increasing atomic number according to Lothar Meyer and Dmitri Mendeleev  a. I, III, II, and IV b. II, I, III, and IV c. II, III, IV, and I d. I, II, III, and IV 19. How did Mendeleev's prediction of undiscovered elements connect with J.J. Thomson's discoveries? a. Both were focused on electron configurations. b. Predicted elements were based on atomic number. c. Undiscovered elements were organized by atomic mass. d. Thomson's discoveries confirmed Mendeleev's predictions. 20. Compare the arrangement of elements of Henry Mosely with Lothar Meyer and Dmitri Mendeleev. Which of the statements is correct? a. Mosely arranged the elements according to increasing atomic mass whereas Lothar Meyer and Demetri Mendeleev arranged the elements according to increasing atomic number. b. Mosely arranged the elements according to increasing mass whereas Lothar Meyer and Demetri Mendeleev arranged the elements according to increasing properties. c. Mosely arranged the elements according to increasing atomic number whereas Lothar Meyer and Demetri Mendeleev arranged according to increasing properties. d. Mosely arranged the elements according to the same properties and increasing atomic number whereas Lothar Meyer and Dmitri Mendeleev arranged according to increasing atomic masses. 21. What does the periodicity concept of the periodic table reveal? a. Atomic mass of elements c. Valence electrons of elements b. Physical states of elements d. Chemical properties of elements For questions 22-23, please refer to the periodic table below The periodic table's periodicity concept reveals patterns in elements' chemical behavior. Group number determines valence electrons, influencing chemical properties. Atomic radius trends affect ionization energy and electronegativity, varying across periods and groups. Metals (left) lose electrons, non-metals (right) gain, impacting reactivity. Similar group behavior aids predictions in chemical reactions. These trends guide applications in materials, medicine, and environmental science. 22. Which of the following is a non- metal? a. Ba b. Pb c. Fe d. Se 23. Which group contains the most element? a. metal b. non metal c. metalloid d. semi metal 24. What does the periodicity concept of the periodic table reveal? a. Atomic mass of elements b. Physical states of elements c. Valence electrons of elements d. Chemical properties of elements 25. As the elements of Group 16 are considered in order from top to bottom, the atomic radius of each successive element increases. This increase is primarily due to an increase in a. atomic number. b. mass number. c. the number of protons occupying the nucleus. d. the number of occupied electron energy levels. 26. Which two factors are influenced by the group number of an element? a. Reactivity and atomic mass b. Periodicity and chemical properties c. Atomic radius and valence electrons d. Ionization energy and electronegativity 27. Which of the following sets is a set of all metals? a. S, Li, C c. K, Li, Na b. He, Be, Ne d. Ca, Cr, C For questions 28-30, Refer to the Information below Periodic trends are observable patterns in the properties of an element that are dependent on its position in the Periodic Table. These trends have allowed scientists in the past to predict certain characteristics of unknown elements Major periodic trends include: electronegativity, ionization energy, electron affinity, atomic radius , metallic and nonmetallic character. Electronegativity is the tendency of an atom to attract electron. Ionization energy is an energy required when an atom removes electron from an isolated atom. Electron Affinity is the tendency of an atom to gain an electron and act as an oxidizing agent (electron acceptor).Atomic radius is the total distance from an atom's nucleus to the outermost orbital of electron. Metallic character is the tendency of an element to lose electrons and form positive ions or cations while non-metallic character is the tendency of an element to accept electrons and form negative ions or anions. The diagram below shows the trends in the periodic table.Periodic trends is shown in figure 5 below 28. What happens to the ionization energy of the element as it moves across the period? a. decreases b. increases c. increases then decreases d. nothing happened 29. Which periodic trends are directly related? a. Ionization energy, electron affinity and atomic radius b. Ionization energy, metallic property and atomic radius c. Ionization energy, electron affinity and metallic property d. Ionization energy, electron affinity and nonmetallic property 30. Based on the observable trends in the Periodic Table what generalization can you make with respect to the properties of elements in the periodic table in relation to the number of its valence electrons? a. Atoms with smaller radius have less valence electrons and tend to attract more thus, it requires higher ionization energy and lower electronegativity. b. Atoms with smaller atomic radius have more valence electron tends to remove its electron thus require lower ionization energy and higher electronegativity. c. Atoms with bigger radius have more valence electrons and prefer to accept more thus require lower ionization energy in removing its electron and higher electronegativity. d. Atoms with bigger radius have less valence electron and preferred to give than attract more thus, require higher ionization energy needed in removing its electron and lower electronegativity. 31. An element has an atomic number equal to 84 and a mass number of 210. Which of the following will correctly describe the element in terms of the number and type of particles present? a. 84 protons and 84 neutrons b. 84 protons and 210 neutrons c. 84 protons and 126 neutrons d. 84 protons and 126 electron 32. What information is necessary to determine the atomic mass of the element chlorine? a. the atomic mass of each artificially produced isotope of chlorine, only b. the relative abundance of each naturally occurring isotope of chlorine, only c. the atomic mass and the relative abundance of each naturally occurring isotope of chlorine d. the atomic mass and the relative abundance of each naturally occurring and artificially produced isotope of chlorine 33. Each diagram below represents the nucleus of a different atom. Which diagrams represent nuclei of the same element? a. D and E, only b. D, E, and Q c. Q and R, only d. Q, R, and E 34. Which of the group 1 elements listed below requires the greatest amount of energy to remove the most loosely held electron from an atom? a. Lithium b. Sodium c. Rubidium d. Potassium 35. During a flame test, ions of a specific metal are heated in the flame of a gas burner. A characteristic color of light is emitted by these ions in the flame when the electrons a. gain energy as they return to lower energy levels b. gain energy as they move to higher energy levels c. emit energy as they return to lower energy levels d. emit energy as they move to higher energy levels 36. Which best describes isotopes? a. Same number of neutrons, different number of electrons b. Same number of neutrons, different number of protons c. Same number of protons, different number of electrons d. Same number of protons, different number of neutrons 37. If there were five positive charges (+5) and three negative charges (–3) in a body, what would be the overall charge of the body? a. +3 b. –2 c. +2 d. –3 38. An atom of oxygen has an atomic number of 8 and a mass number of 16. How many neutrons does it have? a. 6 b. 7 c. 8 d. 16 39. Determine the protons and electrons in the Calcium atom. (Atomic number is 20) a.20; 20 b. 20; 10 c. 40; 20 d. 20; 40 40. An atom of an element is electrically neutral because of the number of protons is equal to the number of _____________. a. electrons b. neutrons c. nucleons d. nucleus 41. Which two particles would be attracted to each other? a. protons and neutrons b. electrons and protons c. electrons and neutrons d. All particles are attracted to each other. 42. How many protons, neutrons and electrons are in the neutral atom of Cl 35 17 ? a. 17 protons, 15 neutrons and 17 electrons b. 17 protons, 17 neutrons and 17 electrons c. 17 protons, 17 neutrons and 18 electrons d. 17 protons, 18 neutrons and 17 electrons 43. Which of the following statements CORRECTLY describes atoms, ions and isotopes? I. A neutral atom has an equal number of protons, neutrons and electrons. II. Atoms are the smallest particles of matter that retain the characteristics of an element. III. Isotopes are atoms of the same element with an unequal number of neutrons in the nucleus.  IV. Ions are atoms with unequal numbers of protons and electrons and are formed when an atom loses or gains electrons. a. I, II and III b. II, III and IV c. I, III and IV d. I, II, III and IV For No. 44-46. Refer to the passage give. Consider the lithium ion shown in the notation below. Information on the subatomic particles may be derived from this shorthand. The base is the element’s symbol. The left subscript denotes the atomic number, therefore the number of protons may be known. The superscript at the left denotes the mass number wherein the number of neutrons may be derived. On the other hand, the superscript at the right denotes the charge wherein the number of electrons may be determined. When there is no superscript at the right, it means that the charge is zero (0). 44. How many protons are there in the lithium ion? a. 3 b. 4 c. 5 d. 6 45. How many neutrons are there in this lithium ion? a. 3 b. 4 c. 5 d. 6 46. How many electrons are there in the lithium ion? a. 3 b. 4 c. 5 d. 6 47. How many protons, electrons, and neutrons are present in Boron a. 5, 5, 5 b. 5, 6, 5 c. 5, 5, 6 d. 5, 6, 6 For Nos. 48-50. Refer to the illustration below. Below is a representation of Rutherford’s gold foil experiment. The paths of the alpha particles are represented with arrows. Use the diagram to answer the following questions. 48. According to Rutherford’s experiment, the atom is composed largely of _________. a. empty space b. alpha particles c. a charged nucleus d. cannot be determined 49. Which term is used for the vertical columns of the periodic table? a. group b. line c. rows d. Table 50. Elements in the same group have the same number of ________. a. protons b. neutrons c. electrons d. valence electrons _________________________________________________________________________ Congratulations! You completed the test! ________________________________________________________________________