Studied by 1 person
B. Chemistry
The science that studies the composition, structure, properties, and changes of matter.
a. Biology
b. Chemistry
c. Math
d. Physics
C. Rocks
2. Which of the following is not phases of matter?
a. Gas
b. Liquid
c. Rocks
d. Solid
C. Plasma
3. An electrically conducting medium with equal numbers of positively and negatively charged particles, produced when atoms in a gas become ionized.
a. Gas
b. Liquid
c. Plasma
d. Solid
C. Melting
4. The process of changing a solid into a liquid when heat is applied.
a. Condensation
c. Melting
b. Deposition
d. Sublimation
D. Vaporation
5. The conversion of a substance from the liquid or solid phase into the gaseous phase.
a. Condensation
b. Deposition
c. Freezing
d. Vaporization
D. Sublimation
6. The conversion of a substance from the solid to the gaseous state without becoming a liquid.
a. Condensation
b. Deposition
c. Melting
d. Sublimation
D. Materials Engineering
7. Understanding the properties of different materials and their interactions.
a. Chemical Engineering
c. Environmental Engineering
b. Electrical Engineering
d. Materials Engineering
C. Environmental Engineering
8. Developing methods to minimize environmental impact.
a. Chemical Engineering
b. Electrical Engineering
c. Environmental Engineering
d. Materials Engineering
A. Chemical Engineering
9. Designing processes for large-scale chemical production.
a Chemical Engineering
c. Environmental Engineering
b. Electrical Engineering
d. Materials Engineering
A. Atoms
10. The basic unit of a chemical element.
a. Atoms
b. Compounds
c. Modures
d. Molecules
D. Molecules
11. Two or more atoms bonded together.
a. Aloms
b. Compounds
c. Mixtures
d. Moleculers
C. Mixtures
12. A combination of two or more substances that are not chemically combined.
a. Atoms
b. Compounds
c. Mixtures
d. Molecules
D. Neurons
13. What is not the main subatomic particles of an atom?
a. Electrons
b. Neutrons
c. Protons
d. Neurons
B. Inorganic chemistry
14. The field of science concerned with the composition, properties, and structure of chemical elements and compounds that contain little or no carbon.
a. Biochemistry
b. Inorganic Chemistry
c. Organic Chemistry
d. Nuclear Chemistry
B. 213 g/mol
15. Calculate the molar mass of Al(NO₂), (Aluminum Nitrate).
a. 212 g/mol
b. 213 g/mol
c. 214 g/mol
d. 215 g/mol
D. Titanium
16. Which of the following is NOT an Alkaline Earth Metal?
a. Calcium
b. Magnesium
c. Strontium
d. Titanium
A. Chemical Reaction
18. A process in which one or more substances are converted to one or more different substances.
a. Chemical Reaction
b. Physical Reaction
c. Nuclear Reaction
d. Thermodynamic Reaction
D. Sodium
17. Which of the following is NOT an Alkali Metal?
a. Lithium
b. Potassium
c. Rubidium
d. Sodium
C. Single replacement reaction
19. A reaction where one element replaces another in a compound.
a. Chemical Reaction
b. Decomposition Reaction
c. Single Replacement Reaction
d. Thermodynamic Reaction
B. Combustion reaction
20. A reaction where a substance combines with oxygen, releasing energy as light and heat.
a. Chemical Reaction
b. Combustion Reaction
c. Decomposition Reaction
d. Single Replacement Reaction
A. Inertness
21. The noble gases are known for being chemically inert due to their complete electron shells, making them very stable and unlikely to react.
a. Inertness
b. Insedoess.
c. Inverness
d. Inxedness
D. Fr
22. The symbol of the rarest naturally occurring element on Earth.
a. F
b. Fe
C. FI
d. Fr
A. Calorimeter
23. A device used to measure the heat of chemical reactions or physical changes.
a. Calorimeter
b. Calirometer
c. Caligropher
d. Calcumeter
C. Electrochemistry
24. The branch of chemistry that deals with the relationship between electrical energy and chemical reactions.
a. Ancient Chemistry
b. Classical Chemistry
c. Electrochemistry
d. Quantum Chemistry
C. Redox reaction
25. A reaction that involves a change in the oxidation state of one or more elements.
a. Chemical Reaction
b. Compound Reaction
c. Redox Reaction
d. Synthesis Reaction
C. +6
26. What is the oxidation state of sulfur in H₂SO₄?
a.+4
b. +5
c. +6
d. +7
C. -3
27. What is the oxidation state of nitrogen in NH?
a. -1
b. -2
c.-3
d. 0
A. Zinc oxidized, copper reduced
28. In the reaction: Zn CuSO.ZnSO, Cu, identify the oxidized and reduced elements.
a Zinc oxidized, copper reduced
b. Zinc reduced, copper oxidized
c. Both oxidized
d. Both reduced
B. +5
29. Determine the oxidation state of chlorine in KCIO
a. +3
b. +5
c. +7
d. +4
A. Hydrogen oxidized, oxygen reduced
30. In the reaction: 2H₂O, 2H₂O, determine the species oxidized and reduced.
a. Hydrogen oxidized, oxygen reduced
b. Oxygen oxidized, hydrogen reduced
c. Both oxidized
d. Both reduced
B. +5
31. What is the oxidation state of phosphorus in H₃PO₄?
a. +3
b. +5
c. +7
d. +4
b. Chlorine
32. In the reaction Fe Cl, ECI,, identify the oxidizing agent.
a. Iron
b. Chlorine
C. FeCl
d. None
D. +7
33. Calculate the oxidation state of manganese in KMnO
a. +3
b.+4
c. +5
d. +7
C. -4
34. What is the oxidation state of carbon in CH,?
a. -2
b. -3
c. -4
d. 0
A. Magnesium
35. In the redox reaction: 2Mg+0,2MgO, which element is oxidized?
a. Magnesium
b. Oxygen
c. Both
d. Neither
B. +4
36. What is the oxidation state of sulfur in SO₂?
a. +2
b.+4
c. +6
d. 0
A. Aluminum
37. What is the reducing agent in the reaction 2AI+3CI2→2AICI3?
a. Aluminum
b. Chlorine
c. AlCl2
d. None
C. +5
38. What is the oxidation state of nitrogen in HNO,?
a +3
b.+4
c. +5
d +6
B. Silver (Ag)
39. In the redox reaction: Cu+ 2AgNO3→ 2Ag+ Cu(NO2)2 which element is reduced?
a. Copper
b. Silver
c. Nitrate
d. Both
C. +6
40. Determine the oxidation state of chromium in K
a. +3
b. +4
c. +6
d. +7
B. Chlorine
41. In the reaction H2+Cl2 → 2HCl which species is reduced?
a. Hydrogen
c. Both
b. Chlorine
d. None
A. -1
42. What is the oxidation state of oxygen in H2O2?
a. -1
b. -2
c. 0
d. 1
A. Potassium
43. In the reaction: 2K + Br2 -> 2KBr, identify the reducing agent.
a. Potassium
b. Bromine
c. KBr
d. None
D. Mixed oxidation states
44. Calculate the oxidation state of sulfur in Na2S2O3
a. +2
b. +4
c. 5
d. Mixed oxidation states
A. Iron
45. In the redox reaction: 4Fe + 3O2 -> 2Fe2O3, which element is oxidized?
a. Iron
b. Oxygen
c. Both
d. Neither
A. +2
46. What is the oxidation state of sulfur in Na2S2O3?
a. 2
b. +4
c. +6
d -2
B. Oxygen
47. In the reaction: 2H2O2→ 2H2O+O2 which element is reduced?
a. Hydrogen
b. Oxygen
c. Water
d. None
C. +3
48. What is the oxidation state of chromium in Cr2 O3?
a.+6
b +4
c. +3
d. +2
C. Carbon monoxide
49. In the reaction: Fe2O2 + 3CO -> 2Fe + 3CO2 which species is the reducing agent?
a. Fe2O2
b.CO2
c. Carbon monoxide (CO)
d. Iron (Fe)
C. +5
50. What is the oxidation state of nitrogen in N2O3?
a. +1
b. +3
c +5
d. -3
C. Alpha decay
51. This particle is composed of 2 protons and 2 neutrons and is emitted during alpha decay.
a. Beta particle
b. Gamma ray
c. Alpha particle
d. Proton
D. Strong nuclear force
52. The force that holds protons and neutrons together within the nucleus of an atom.
a Electromagnetic force
b Gravitational force
c. Weak nuclear force
d. Strong nuclear force
B. Nuclear fusion
53. The process of combining two lighter nuclei to form a heavier nucleus, releasing energy.
a. Nuclear fission
b. Nuclear fusion
c. Radioactive decay
d. Beta decay
A. Isotopes
54. Atoms of the same element that have different numbers of neutrons.
a. Isotopes
c. lons
b. Molecules
d. Nuclei
B. Fission energy
55. The energy released when a single nucleus undergoes fission, often measured in MeV.
a lonization energy
b. Fission energy
c. Kinetic energy
d. Binding energy
C. Beta minus decay
56. This process involves the emission of an electron when a neutron converts into a proton within the nucleus.
a. Gamma decay
b. Alpha decay
c. Beta-minus (p") decay
d. Positron emission
C. Neutron
57. The subatomic particle that has no charge and is found within the nucleus alongside protons.
a Proton
b. Electron
c. Neutron
d. Positron
C. Gamma radiation
58. This type of radiation involves the release of a high-energy photon from an excited nucleus.
a. Alpha radiation
b. Beta radiation
c. Gamma radiation
d. X-ray radiation
c. Ernest Rutherford
59. The scientist who proposed the model of the atom with a dense, positively charged nucleus.
a. Niels Bohr
b. J.J. Thomson
c. Ernest Rutherford
d. Marie Curie
C. Carbon -14
60. A radioactive isotope commonly used in carbon dating to determine the age of archaeological finds.
Carbon-12
c. Carbon-14
b. Carbon-13
d. Carbon-16
A. Nuclear fission
61. The type of reaction used in nuclear power plants to generate electricity by splitting large nuclei
a. Nuclear fusion
b. Nuclear fission
c. Radioactive decay
d. Neutron capture
C. Gamma radiation
62. The form of radiation that has the highest penetration power and can pass through most materials.
a. Alpha radiation
b. Beta radiation
c. Gamma radiation
d. Neutron radiation
C. Radioactive decay
63. The process in which an unstable nucleus emits radiation to become more stable.
a. Nuclear fusion
b. Fission
c. Radioactive decay
d. Ionization
B. Mass number
64. The name for the total number of protons and neutrons in the nucleus of an atom.
a. Atomic number
b. Mass number
c. Nucleon number
d. Isotopic number
B. Radioisotopes
65. The name given to isotopes that spontaneously emit radiation to stabilize their nuclei.
a. Stable isotopes
b. Radioisotopes
c. Neutral isotopes
d. Fission products
C. Carbon
66. The element whose isotopes include C-12, C-13, and C-14.
a. Hydrogen
b. Oxygen
c. Carbon
d. Nitrogen
A. Radiation
67. The term for the particles and energy emitted by radioactive substances.
a. Radiation
b. Alpha particles
c. Gamma rays
d. Neutrons
D. Bacquerel(Bq)
68. A unit used to measure radioactive decay, equivalent to one disintegration per second.
a Joule
b. Hertz
c. Curie
d. Becquerel (Bq)
B. Fission
69. A nuclear reaction in which an atom's nucleus splits into two or more smaller nuclei, releasing energy.
a. Nuclear fusion
b. Fission
c. Radioactive decay
d. Alp
ha decay
B. Positron
70. The particle released during beta-plus decay, which has the same mass as an electron but a positive charge.
a. Proton
b. Positron
c. Neutrino
d. Antineutrino
C. 12.5 grams
71. A radioactive isotope has a half-life of 10 days. If you start with a 100-gram sample, how much remains after 30 days?
a. 25 grams
c. 12.5 grams
b. 50 grams
d. 6.25 grams
A. 6hours
72. A 40-gram sample of a radioactive isotope decays to 5 grams in 24 hours. What is the half-life of the isotope?
a. 6 hours
c. 12 hours
b. & hours
d. 15 hours
C. 3 hours
73. A 64-gram sample of a radioactive substance decays to 8 grams in 9 hours. What is the half- life of the substance?
a. 1.5 hours
c. 3 hours
b. 2 hours
d. 4.5 hours
b. 60 minutes
74. The half-life of a radioactive isotope is 20 minutes. How long will it take for a 200-gram sample to decay to 25 grams?
a. 40 minutes
b. 60 minutes
c. 80 minutes
d. 100 minutes
a. 10 grams
75. A sample of a radioactive isotope has a mass of 80 grams and a half-life of 12 hours. How much will remain after 36 hours?
a. 10 grams
c. 15 grams
b. 20 grams
d. 5 grams
b. 1 to 100 nanometers
76. What is the size range that defines nanomaterials?
a. 1 to 100 micrometers
c. 10 to 200 nanometers
b. 1 to 100 nanometers
d. 0.1 to 1 micrometer
c. Larger size than bulk materials
77. Which of the following is NOT a characteristic of nanomaterials?
a. Exceptional strength
b. Quantum effects
c. Larger size than bulk materials
d. Unique optical properties
c. Drug delivery systems
78. Which of the following is a key application of nanomaterials in medicine?
a. Water filtration
c. Drug delivery systems
b. Solar energy
d. Cement production
c. Enhanced scattering and emission of light
79. Nanomaterials can exhibit which of the following optical properties?
a. Increased scattering of light
b. Decreased absorption of light
c. Enhanced scattering and emission of light
b. Magnetization only in the presence of an external field
80. What is superparamagnetism in nanomaterials?
a. Permanent magnetization
b. Magnetization only in the presence of an external field
c. Magnetic repulsion
d. No magnetic properties
b. Graphene
81. Which of the following materials is a carbon nanomaterial?
a. MCM-41
b. Graphene
b. The combination of nanomaterials with other materials
82. What are nanocomposites?
a. Single-element materials
b. The combination of nanomaterials with other materials
c. Only metal-based nanomaterials
d. Materials without any nanoscale features
b. Liposomes
83. Which organic nanomaterial is commonly used in drug delivery systems?
a. Carbon nanotubes
b. Liposomes
c. Titanium dioxide nanoparticles
d. Graphene
b. Optical properties, including UV absorption
85. Which of the following is a characteristic of metal oxide nanoparticles?
a. High electrical conductivity
b. Optical properties, including UV absorption
c. Magnetic properties
d. Solubility in water
c. Titanium dioxide nanoparticles
84. Which of the following is an inorganic nanomaterial?
a. Dendrimers
b. Liposomes
c. Titanium dioxide nanoparticles
d. Graphene
b. Marine Litter
86. What is a possible type of water pollutant?
a. Contamination
b. Marine Litter
c. Magnetic properties
d. Solubility in water
a. Aquifer
87. What is the name of the underground body of rock or sediment that hoids water?
a. Aquifer
b. Water Table
c. Well
d. None of the above
c. Both A or B
88. What are the possible consequences of discharging untreated sewage near drinking water sources?
a. Disruption of surrounding ecosystems
b. Outbreak of human diseases such as cholera
c. Both A or B
d. None of the Above
c. They can have harmful effects when ingested by humans, such as mental degradation and even cancer
89. Why is dumping heavy metals such as lead, mercury, and cadmium in water prohibited?
a. The metals alter marine DNA, making fish metallic and inedible
b. The heaviness of the metals causes earthquakes
c. They can have harmful effects when ingested by humans, such as mental degradation and even cancer
d. None of the Above
a. Poor or neglected water systems
90. Why do large portions of the human population still lack access to clean and safe drinking water?
a. Poor or neglected water systems
b. They don't deserve clean water
c. Corruption in government policies
d. None of the Above
a. Environmental Chemistry
91. Which branch of chemistry deals with the biochemical and chemical phenomena that occur naturally in the environment?
a. Environmental Chemistry
b. Water Chemistry
c. Sanitary Chemistry
d. None of the Above
c. Precipitation
92. In which phase of the water cycle does water vapor condense into water droplets and fall back to Earth's surface?
a. Condensation
b. Evaporation
c. Precipitation
d. Sublimation
c. Water purification methods
93. What is a possible method for treating water pollutants?
a. Proper waste disposal
b. Improving sewage systems
c. Water purification methods
d. None of the Above
B. Monomer
94. What is the basic repeating unit of polymer?
a. Crystal Lattice
b. Monomer
c. Micelle
d. Unit Cell
C. Cold drying
95. Which method is not used for purifying natural polymer?
a. Air Drying
b. Freeze Drying
c. Cold Drying
d. Oven Drying
B. Rigidity
96. Which property makes cross-linked polymers suitable for thermosetting plastics?
a. Elasticity
b. Rigidity
c. Transparency
d. Conductivity
C. Reduces packing efficiency, resulting in lower density and increased flexibility.
97. Which of the following best describes how branching affects the properties of polymers?
A. Increases density and crystallinity by allowing tight packing of chains.
B. Decreases flexibility and makes the polymer more brittle.
C. Reduces packing efficiency, resulting in lower density and increased flexibility.
D. Creates a rigid, heat-resistant structure with high thermal stability.
C. Loosely packed and disordered structure.
98. Which of the following is not a characteristic of a crystalline region in polymers?
A Highly ordered and tightly packed structure.
B. Forms a 3d lattice with a repeating unit.
C. Loosely packed and disordered structure.
D. Contributes to the strength and rigidity of the polymer.
b. Adhesive and protective coatings
99. What is the role of polymers like epoxy resins in industrial applications?
a. Elasticity
b. Adhesive and protective coatings
c. Conducting Electricity
d. Biodegradability
a. Petroleum Oil
100. Where do synthetic polymers come from?
a. Petroleum Oil
c. Kerosene Oil
b. Synthetic Oil
d. Conventional Oil
Note 
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