Science Grade 10 (4th Quarter)
1.
Boyle's Law
volume & pressure of gases at constant temperature
2.
Boyle's Law formula
V1P1 = V2P2
3.
stated by Robert
Boyle during 16th
century
volume of a fixed amount of gas is inversely proportional to its pressure at
constant temperature
4.
Boyle's Law
pressure increases = volume decreases
5.
Gas particles
have a very weak intermolecular force of attraction, hence they move as far
as possible from each other
6.
Charles' Law formula V1/T1 = V2/T2
7.
Charles' Law
volume & temperature at constant pressure
8.
By Jacques Charles
at constant pressure, the volume of a fixed amount of gas is directly proportional to the Kelvin (K) temperature
9.
Gay-Lussac's Law for- P1/T1 = P2/T2
mula
10. Gay-Lussac's Law
temperature & pressure at constant volume
11. By Joseph
Louis Gay-Lussac
(1746-1823)
the pressure of the gas is directly proportional to its temperature
12. Combined Gas Laws
formula
P1V1/T1 = P2V2/T2 -> V1P1T2 = V2P2T1
13. Combined Gas Law
temperature, pressure, and volume at constant number of moles
14. Combined Gas Law
increase in pressure = expansion of volume
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Science Grade 10 (4th Quarter)
15. Lorenzo Romano
Amedeo Carlo Avogadro
contributes in shedding light on reaction stoichiometry
16. Lorenzo Romano
Amedeo Carlo Avogadro
explaining why compounds react in definite ratios and how gas volume
relates to its amount
17. Lorenzo Romano
Amedeo Carlo Avogadro
the number of molecules is named after him
18. by Lorenzo Romano
Amedeo Carlo Avogadro
gas volume is directly proportional to the number of moles at a given
temperature and pressure
19. Lorenzo Romano
Amedeo Carlo Avogadro
in 1881, "Equal volume of all gases, kept at the same pressure and temperature, contain the same number of molecules"
20. Ideal Gas Law formula PV = nRT
21. Ideal Gas Law
the pressure,volume, temperature, and number of moles of a gas
22. Ideal Gas Law
volume of a gas is directly proportional to the number of moles
23. Phlogiston Theory
by George Ernst Stahl, stated that when a material burns, it releases a
substance known as phlogiston
24. Antoine Lavoisier
debunked the phlogiston theory as he discovered that instead of releasing
(Theory of Oxidation) a substance (phlogiston) a material accurately burns as it reacts (uses) with
oxygen
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Grade 10 4th Quarter Science
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25. COMBINATION REAC- two/more reactants form a single product. The general formula for this
TION
reaction is: A + B ’AB
26. DECOMPOSITION RE- a single reactant breaks down into simpler ones. (2 or more products). This
ACTION
is the reverse of combination reaction. The general formula for this reaction
is: AB ’A + B
27. SINGLE DISPLACEone element replaces another element from a compound. The general
MENT (Replacement) formula for this reaction is:
A + BC ’AC + B
REACTION
28. DOUBLE DISPLACEMENT REACTION
(Metathesis)
the positive ions (cations) and negative ions (anions) of ditterent compounds switch places, froming two entirely ditterent compounds. The general formula for this reaction is:
AB + CD ’AD + CB
29. COMBUSTION (Burn- oxygen combines with a hydrocarbon to form water and carbon dioxide
ing) REACTION
30. ACID-BASE REACTION reaction between an acid and a base producing salt and water
HCI + NaOH ’NaCl + H2O
31. Law of Conservation
of Mass
for balancing chemical reactions and states that mass is conserved in a
chemical
32. Law of Conservation
of Mass
total mass of reactants = total mass of products
33. Biomolecule
any molecule that is produced by a living organism, including large macromolecules such as proteins, polysachharides, lipids and nucleic acids
34. Monomer
small molecule that joins with other similar molecules to make a polymer,
repeating units of a polymer
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35. Polymer
large organic molecule consisting of small repeating units called monomers
36. Carbohydrates
major source of energy for the body consist of carbon, hydrogen, and
oxygen. They include simple sugars, starch, and cellulose.
37. Monosaccharides
simplest form of sugar, consisting of one sugar molecule
38. Monosaccharides ex- glucose (dextrose) and fructose
amples
39. Polar hydroxyl groups soluble in water due to
40. Glucose
is crucial for cellular energy; excess glucose stored as glycogen
41. Disaccharides
consist of two monosaccharides that are chemically combined
42. Disaccharides exam- sucrose
ple
43. Condensation and
Hydrolysis
Breakdown of glucose to sucrose involves two reactions
44. Condensation reaction
between two monosaccharides, losing a water molecule
45. Hydrolysis reaction
the bond between monosaccharides is broken with the addition of a water
molecule
46. Polysaccharides
made up of many smaller units and are polymers containing monosaccharide monomers
47. Polysaccharides examples
starch, glycogen, and cellulose
48. Starch
chief storage form in plants; important in human nutrition
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49. Glycogen
Storage form in animals; highly branched for rapid energy release
50. Cellulose
Structural component in plants; not digestible by humans
51. Amylose
coiled structure
52. Amylopectin
branched
53. Lipids
store energy for later use, found in hormones and cell membranes
54. Structural types of
Lipids:
fatty acids, triglycerides, steroids and waxes
55. Lipids
Insoluble in water, soluble in nonpolar solvents
56. Proteins
are polymers of amino acids, found in hair, nails, connective tissues. composed of CHONS
57. Proteins
Second most common molecules in the human body (10-20% of cell mass)
58. Amino acids
building blocks of proteins, 20 in human protein, 9 essential (not synthesized by the body), 11 nonessential (can be synthesized)
59. Nucleic Acids types
Deoxyribonucleic acid (DNA) and Ribonucleic acid (RNA)
60. Deoxyribonucleic acid polymers that are made up of nucleotides
(DNA) and Ribonucleic acid (RNA)
61. Nucleotides
are molecules that are composed of three parts: a five carbon sugar, a
nitrogen-containing base, and a phosphate group
62. Collision Theory
Explains how collisions between reactant molecules lead to chemical reactions
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63. Conditions for effective collision
Reactant molecules must possess minimum kinetic energy (activation energy). Reactant molecules must be in correct orientation during collision.
64. Svante Arrhenius
(1888)
proposed the concept of activation energy
65. Energy Diagrams
Used to analyze energy changes in a reaction
66. Activation energy
Energy needed to initiate a reaction. Forms an activated complex at the
energy peak
67. Acrivation complex
located at the energy peak
68. Energy barrier
Reactant energy must surpass an
69. surface area of reac- The rate of chemical reaction is attected by the following factors:
tants, concentration
of reactants, temperature and presence of
catalyst
70. Catalysts
Substances that accelerate reaction rates without being consumed
71. Enzymes
are proteins acting as catalysts in biological reactions (e.g., Photosynthesis,
Cellular Respiration)
72. Food storage
Utilized by society for preserving food
73. Lower temperature
decreases the rate of food breakdown and bacterial growth
74. bigger surface area
Smaller particles have
75. Concentration
measures the number of particles in a given volume
76. Fermentation
Conversion of sugars to organic acids
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77. Irradiation
Food exposed to radiation like gamma rays
78. Oxidation
Oxygen reacts with other substances
79. Acid Rain
Produced by reaction of water vapor with gas emissions from vehicles,
thermal power plants, and coal mining industries
80. Acid Rain
is caused by the reaction of various pollutants such as CO2, CO, SO2, NO2,
and NO from sources like automobiles, thermal power plants, and coal
mining industries, with water vapor in the air, resulting in the production
of acids
81. faster rate of reaction Higher concentration leads to
82. possible effective col- Higher concentration means greater number of
lisions among molecules
83. Avogadro's Law formula
V1n2 = V2n1
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