ATOMIC MASS
43. Define atomic mass.
44. The theory of atomic mass could well explain the law of -----------------.
45. Scientists could measure the atomic mass of an atom. True or False?
46. What are relative atomic masses?
47. How were relative atomic masses determined?
48. Expand 'amu'.
49. What was initially taken by scientists as the atomic mass unit?
50. Why was oxygen selected for this purpose? Give the two reasons.
51. In 1961, what was universally accepted the amu?
52. Define atomic mass unit.
53. Explain the theory of amu using the illustration of the fruit seller selling watermelon using a standard weight.
54. Define relative atomic mass.
55. Table 3.2 - Learn the atomic masses of the given elements.
HOW DO ATOMS EXIST?
56. Atoms of most elements are not able to exist dependently / independently.
57. Atoms form ----------- and --------------.
58. Molecules or ions ------------------------------------ to form matter.
WHAT IS A MOLECULE?
59. A molecule is a group of --------------- that are ------------- together.
60. Define molecule.
61. Atoms of the ------------------- or of ------------ can join together to form molecules.
MOLECULES OF ELEMENTS
62. The molecules of an element are constituted by the same / different type of actions.
63. Molecules of many elements are made up of -------------------- of that element.
64. What is a diatomic molecule? Give example.
65. What is the difference in molecules of most of the non-metals. Explain with an example.
66. What is atomicity?
67. Explain the structure of atoms in metals and some particular elements.
68. Table 3.3. Learn the atomicity of the given elements.
MOLECULES OF COMPOUNDS
69. Atoms of different elements join together in ---------------- to form molecules of compunds.
70. Table 3.4. Be familiar with the molecules of some given compunds.
71. Find out the ratio by number of atoms for water.
WHAT IS AN ION?
72. What are known as ions?
73. An ion is a ------------- particle and can be -------------- or ------------------ charged.
74. A negatively charged ion is called --------------.
75. A positively charged ion is called ----------------.
76. Explain anion and cation giving examples.
77. Ions may consist of ----------------- or -------------------- that have a net charge on them.
78. What is a polyatomic ion?
79. Table 3.5. Be familiar with the given ionic compunds.
WRITING CHEMICAL FORMULAE
80. What is a chemical formula?
81. To write the chemical formulae for different compunds we need to learn the -------------- and ---------------------- of the elements.
82. Define valency.
83. How can be valency used?
84. ------------------ can be considered as hands or arms of that atom.
85. Learn the illustration of octopus to have a better understanding of the valency and chemical formulae.
86. Table 3.6. Be familiar with the names and symbols of some ions.
87. What are the rules you have to follow while writing chemical formulae?
88. The valencies or charges on the ion must ---------------.
89. In a chemical formula, what should be written first? Why? Explain with an example.
90. What do you know of the brackets in a chemical formula?
FORMULAE OF SIMPLE COMPOUNDS
91. What are binary compunds?
92. Learn how to write the chemical formulae through the illustrations given in page 38 and 39.
MOLECULAR MASS AND MOLE CONCEPT
93. What is molecular mass?
94. Molecular mass is expressed in ------------------ units.
95. Learn how to calculate the relative molecular mass of different compunds.
FORMULA UNIT MASS
96. What is formula unit mass of a substance?
97. Formula unit mass is calculated in the same manner as molecular mass is calculated. True or False?
98. Calculate the formula unit mass of Sodium Chloride.
MOLE CONCEPT
99. What was the necessity to introduce the new unit mole?
100. What is mole?
101. The number of particles present in 1 mole of any substance is fixed with a value of --------------.
102. What is called the Avogadro Constant or Avogadro number?
103. The name Avogadro honours the Italian Scientist --------------.
104. The mass of 1 mole of a particular substance is fixed. True or False?
105. How is the molar mass calculated? Give an example.
106. Molar mass of atoms is also known as ------------------------.
107. The atomic mass of hydrogen is 1 u. The gram atomic mass of hydrogen = ---------------.
108. Why is mole the counting unit of the chemists?
109. The word mole is derived from Latin and it means ------------- or ---------------------.
110. Learn the illustrations given in page 41 and 42.
43. Define atomic mass.
44. The theory of atomic mass could well explain the law of -----------------.
45. Scientists could measure the atomic mass of an atom. True or False?
46. What are relative atomic masses?
47. How were relative atomic masses determined?
48. Expand 'amu'.
49. What was initially taken by scientists as the atomic mass unit?
50. Why was oxygen selected for this purpose? Give the two reasons.
51. In 1961, what was universally accepted the amu?
52. Define atomic mass unit.
53. Explain the theory of amu using the illustration of the fruit seller selling watermelon using a standard weight.
54. Define relative atomic mass.
55. Table 3.2 - Learn the atomic masses of the given elements.
HOW DO ATOMS EXIST?
56. Atoms of most elements are not able to exist dependently / independently.
57. Atoms form ----------- and --------------.
58. Molecules or ions ------------------------------------ to form matter.
WHAT IS A MOLECULE?
59. A molecule is a group of --------------- that are ------------- together.
60. Define molecule.
61. Atoms of the ------------------- or of ------------ can join together to form molecules.
MOLECULES OF ELEMENTS
62. The molecules of an element are constituted by the same / different type of actions.
63. Molecules of many elements are made up of -------------------- of that element.
64. What is a diatomic molecule? Give example.
65. What is the difference in molecules of most of the non-metals. Explain with an example.
66. What is atomicity?
67. Explain the structure of atoms in metals and some particular elements.
68. Table 3.3. Learn the atomicity of the given elements.
MOLECULES OF COMPOUNDS
69. Atoms of different elements join together in ---------------- to form molecules of compunds.
70. Table 3.4. Be familiar with the molecules of some given compunds.
71. Find out the ratio by number of atoms for water.
WHAT IS AN ION?
72. What are known as ions?
73. An ion is a ------------- particle and can be -------------- or ------------------ charged.
74. A negatively charged ion is called --------------.
75. A positively charged ion is called ----------------.
76. Explain anion and cation giving examples.
77. Ions may consist of ----------------- or -------------------- that have a net charge on them.
78. What is a polyatomic ion?
79. Table 3.5. Be familiar with the given ionic compunds.
WRITING CHEMICAL FORMULAE
80. What is a chemical formula?
81. To write the chemical formulae for different compunds we need to learn the -------------- and ---------------------- of the elements.
82. Define valency.
83. How can be valency used?
84. ------------------ can be considered as hands or arms of that atom.
85. Learn the illustration of octopus to have a better understanding of the valency and chemical formulae.
86. Table 3.6. Be familiar with the names and symbols of some ions.
87. What are the rules you have to follow while writing chemical formulae?
88. The valencies or charges on the ion must ---------------.
89. In a chemical formula, what should be written first? Why? Explain with an example.
90. What do you know of the brackets in a chemical formula?
FORMULAE OF SIMPLE COMPOUNDS
91. What are binary compunds?
92. Learn how to write the chemical formulae through the illustrations given in page 38 and 39.
MOLECULAR MASS AND MOLE CONCEPT
93. What is molecular mass?
94. Molecular mass is expressed in ------------------ units.
95. Learn how to calculate the relative molecular mass of different compunds.
FORMULA UNIT MASS
96. What is formula unit mass of a substance?
97. Formula unit mass is calculated in the same manner as molecular mass is calculated. True or False?
98. Calculate the formula unit mass of Sodium Chloride.
MOLE CONCEPT
99. What was the necessity to introduce the new unit mole?
100. What is mole?
101. The number of particles present in 1 mole of any substance is fixed with a value of --------------.
102. What is called the Avogadro Constant or Avogadro number?
103. The name Avogadro honours the Italian Scientist --------------.
104. The mass of 1 mole of a particular substance is fixed. True or False?
105. How is the molar mass calculated? Give an example.
106. Molar mass of atoms is also known as ------------------------.
107. The atomic mass of hydrogen is 1 u. The gram atomic mass of hydrogen = ---------------.
108. Why is mole the counting unit of the chemists?
109. The word mole is derived from Latin and it means ------------- or ---------------------.
110. Learn the illustrations given in page 41 and 42.
No comments:
Post a Comment