Fundamentals Of Chemistry Flashcards
(278 cards)
1
Q
What is the study of matter and the ways in which different forms of matter combine with each other?
A
Chemistry
2
Q
Which period is referred to as the ‘Golden Age of Chemistry’ in the history of chemistry?
A
Muslim Period (600-1600 AD)
3
Q
Who is generally known as the father of chemistry?
A
Jabber Ibn Haiyan
4
Q
What is the primary goal of Muslim chemists during the 600-1600 AD period?
A
To find methods to prolong life, change basemetals into gold, and support religious/philosophical beliefs.
5
Q
True or False: Muslim chemists succeeded in changing base metals like lead into gold.
A
False
6
Q
Fill in the blank: Jabber Ibn Haiyan invented experimental methods like distillation, sublimation, filtration, and the extraction of ________.
A
metals
7
Q
What famous book did Al-Razi write, discussing various chemical processes?
A
Al-Asrar
8
Q
MCQ: Which of the following elements was discovered by Muslim chemists? A) Gold B) Arsenic C) Oxygen
A
B) Arsenic
9
Q
True or False: Al-Razi divided chemical compounds into four types and classified substances into living and non-living origins.
A
True
10
Q
What chemical substances did Jabber Ibn Haiyan prepare?
A
Hydrochloric acid, Nitric acid, White lead
11
Q
MCQ: Which method did Jabber Ibn Haiyan NOT invent? A) Filtration B) Sublimation C) Teleportation
A
C) Teleportation”Question
12
Q
Who is known as the Aristotle of the Muslim world?
A
Ibn-e-Sina
13
Q
Which scientist rejected the idea that base metals can be converted into gold?
A
Ibn-e-Sina
14
Q
True or False: Al-Beruni made significant contributions in the field of Chemistry and determined the densities of different substances.
A
True
15
Q
MCQ: Which field of chemistry deals with the study of substances and their chemical reactions that occur in living organisms? A) Biochemistry B) Environmental Chemistry C) Organic Chemistry
A
A) Biochemistry
16
Q
Fill in the blank: Al-Beruni made contributions in various fields, including Physics, Metaphysics, Mathematics, Geography, Astronomy, and ________.
A
History
17
Q
Which branch of chemistry focuses on the relationship between the physical properties of substances and the chemical changes in them?
A
Physical Chemistry
18
Q
MCQ: In which branch of chemistry do chemists study hydrocarbons and their derivatives? A) Organic Chemistry B) Inorganic Chemistry C) Nuclear Chemistry
A
A) Organic Chemistry
19
Q
True or False: Inorganic Chemistry deals with the study of hydrocarbons and their derivatives.
A
False
20
Q
Which branch of chemistry is concerned with the study of qualitative and quantitative analysis of matter?
A
Analytical Chemistry
21
Q
Fill in the blank: A chemist working on the preparation of industrial products such as cement, glass, and fertilizers is working in the field of ________ chemistry.
A
Industrial
22
Q
MCQ: Which branch of chemistry is concerned with the study of the nucleus and radiation emission or absorption? A) Nuclear Chemistry B) Biochemistry C) Environmental Chemistry
A
A) Nuclear Chemistry
23
Q
True or False: Environmental Chemistry focuses on the interaction of chemical substances with the environment and their impact on it.
A
True
24
Q
Which branch of chemistry is used to determine the amount of an impurity in drinking water?
A
Analytical Chemistry
25
MCQ: A chemist working to develop medicine for thyroid problems would be working in which branch of chemistry? A) Organic Chemistry B) Biochemistry C) Nuclear Chemistry
B) Biochemistry
26
True or False: Analytical Chemistry deals with the study of all elements and compounds, excluding hydrocarbons.
False"Question
27
What is the definition of matter?
Anything that has mass and occupies space.
28
True or False: A substance in pure form has exactly the same composition and properties regardless of its sources.
True
29
MCQ: Which of the following is an example of a pure substance? A) Air B) Water C) Salad
B) Water
30
Fill in the blank: The smallest particle of an element that can take part in a chemical reaction is called an ________.
atom
31
True or False: An element can be split into other simpler substances by ordinary physical or chemical processes.
False
32
MCQ: How many elements are naturally occurring? A) 118 B) 92 C) 150
B) 92
33
MCQ: Who proposed the system for representing elements with symbols in 1814? A) Dalton B) Berzelius C) Mendeleev
B) Berzelius
34
True or False: The symbols of elements are always represented by the first letter of their name in capital letters.
False
35
Fill in the blank: The theory of dual nature of matter, stating that matter has both properties of particles and waves, was put forward by ________.
de Broglie
36
MCQ: Which of the following is NOT a pure substance? A) Gold B) Air C) Oxygen
B) Air
37
MCQ: What is the fundamental unit of an element? A) Atom B) Molecule C) Compound
A) Atom
38
True or False: Atoms of a particular element are the same to each other but different from atoms of other elements.
True
39
Fill in the blank: An element is a pure substance that cannot be split into simpler substances by ordinary ________ or ________ processes.
physical, chemical
40
MCQ: Which of the following elements has the symbol 'C'? A) Carbon B) Calcium C) Chlorine
A) Carbon
41
True or False: All elements can be represented by symbols that are derived from their names, with some elements using the first two letters of their names.
True"Question
42
MCQ: Which element has the symbol 'Cu'? A) Copper B) Cobalt C) Calcium
A) Copper
43
True or False: The symbol for gold is 'Au' which comes from its Latin name 'Aurum'.
True
44
Fill in the blank: The element with the symbol 'Pb' is known as ________.
Lead
45
MCQ: Which of the following elements has the symbol 'Fe'? A) Iron B) Fluorine C) Francium
A) Iron
46
True or False: Potassium's symbol, 'K', comes from its Latin name 'Kalium'.
True
47
Fill in the blank: The symbol 'Na' for Sodium comes from its Latin name ________.
Natrium
48
MCQ: Which of the following elements has the symbol 'Ag'? A) Silver B) Aluminum C) Argon
A) Silver
49
True or False: Tungsten is represented by the symbol 'W' because of its Latin name 'Wolfram'.
True
50
MCQ: What is the name of the element with the symbol 'Sn'? A) Tin B) Titanium C) Sulfur
A) Tin
51
Fill in the blank: Gallium is a soft metal that can be cut with a knife, and its symbol is ________.
Ga
52
True or False: Gallium is a solid at room temperature but melts from the warmth of your hand.
True
53
MCQ: What is the atomic number of Gallium? A) 31 B) 32 C) 33
A) 31
54
MCQ: Water (H2O) is an example of a _________. A) Element B) Compound C) Mixture
B) Compound
55
True or False: The properties of a compound are the same as the elements that form it.
False
56
MCQ: What is the ratio of hydrogen atoms to oxygen atoms in water? A) 1:1 B) 2:1 C) 1:2
B) 2:1
57
Fill in the blank: Sodium chloride (NaCl) is an example of a _________.
Compound
58
MCQ: Which of the following is an example of a compound? A) Iron B) Water C) Air
B) Water
59
True or False: Compounds are mixtures of two or more elements chemically combined in a fixed ratio by mass.
True"Question
60
MCQ: What does a chemical formula represent in a compound? A) The name of the compound B) The elements present and their ratio C) The physical state of the compound
B) The elements present and their ratio
61
True or False: Changing the ratio of elements in a compound will always give a different compound.
True
62
Fill in the blank: The chemical formula of Sodium bicarbonate is ________.
NaHCO3 (baking soda)
63
MCQ: Which of the following is the chemical name for baking soda? A) Sodium bicarbonate B) Calcium hydroxide C) Magnesium oxide
A) Sodium bicarbonate
64
True or False: In a mixture, the components are chemically combined and cannot be separated by physical methods.
False
65
Fill in the blank: The chemical formula of table salt (NaCl) is composed of ________ and ________.
Sodium, Chlorine
66
MCQ: What is the chemical formula of methane? A) CH4 B) NaCl C) CaO
A) CH4
67
True or False: A mixture can be separated by physical methods, and its components retain their original properties.
True
68
Fill in the blank: In a homogeneous mixture, the composition is ________ throughout its mass.
Uniform
69
MCQ: Which of the following is an example of a homogeneous mixture? A) Sugar in water B) Sand in water C) Oil and water
A) Sugar in water
70
True or False: The components of a mixture are chemically bonded together.
False
71
Fill in the blank: The chemical name for bleach is _________.
Calcium hypochlorite {Ca(ClO)₂}
72
MCQ: Which of the following compounds is commonly used in the preparation of hydrogen peroxide? A) Sodium hydroxide B) Sodium chloride C) Hydrogen peroxide
C) Hydrogen peroxide
73
True or False: An alloy is a mixture of metals or metals with other elements.
True
74
Fill in the blank: The chemical formula for calcium carbonate is ________.
CaCO3
75
MCQ: Which of the following is a compound? A) Brass B) Water C) Air
B) Water
76
True or False: Mixtures consist of elements or compounds that are chemically combined in fixed proportions.
False"Question
77
MCQ: What type of mixture forms when sugar is dissolved in water? A) Heterogeneous B) Homogeneous C) Both
B) Homogeneous
78
True or False: In a heterogeneous mixture, the components are not uniformly distributed.
True
79
Fill in the blank: In a heterogeneous mixture of sand and water, the ________ particles are visible, while the ________ particles are not visible even under a microscope.
Sand, Sugar
80
MCQ: Which of the following is an example of a heterogeneous mixture? A) Sugar dissolved in water B) Sand mixed with water C) Salt in water
B) Sand mixed with water
81
True or False: The components of a homogeneous mixture can be physically separated.
False
82
Fill in the blank: A compound always has a ________ composition by mass.
Fixed
83
MCQ: What can be used to separate the components of a heterogeneous mixture? A) Physical methods B) Chemical reactions C) Both
A) Physical methods
84
True or False: The properties of the components in a mixture remain unchanged.
True
85
Fill in the blank: In a solution, the solute is dissolved in the ________.
Solvent
86
MCQ: Which of the following is a key characteristic of a homogeneous mixture? A) The components are easily distinguishable B) The composition is uniform C) The components can be seen
B) The composition is uniform
87
True or False: The components of a homogeneous mixture cannot be physically separated.
False
88
Fill in the blank: A mixture where the components retain their original properties is called a ________.
Homogeneous mixture
89
MCQ: Which of the following is a property of compounds? A) They have a fixed composition B) Their components retain individual properties C) They can be physically separated
A) They have a fixed composition
90
True or False: A compound is formed by the physical combination of its components.
False
91
Fill in the blank: In a heterogeneous mixture, the components are ________ distributed.
Unevenly
92
MCQ: When iron (Fe) and sulfur (S) are strongly heated, what do they form? A) Iron Sulphide B) Iron Oxide C) Iron Chloride
A) Iron Sulphide
93
True or False: Iron and sulfur can be separated by a magnet after they are strongly heated.
False
94
Fill in the blank: Iron and sulfur react to form a compound called ________.
Iron Sulphide
95
MCQ: What happens when iron (Fe) and sulfur (S) are mixed without heating? A) They form a compound B) They form a mixture C) They dissolve into each other
B) They form a mixture
96
True or False: Iron filings and sulfur can be separated with a magnet in a mixture.
True
97
Fill in the blank: The atomic number of an element is the number of ________ in its nucleus.
Protons
98
MCQ: What is the atomic number of Oxygen? A) 1 B) 6 C) 8
C) 8
99
True or False: Atoms of different elements have the same number of protons.
False
100
Fill in the blank: The atomic number of an element is equal to the number of ________ in an atom.
Protons ot Electrons
101
MCQ: Which element has an atomic number of 6? A) Hydrogen B) Carbon C) Oxygen
B) Carbon
102
True or False: The atomic number is a unique identifier for each element.
True
103
Fill in the blank: The number of neutrons in an atom varies and cannot be used to characterize the atom because it differs between atoms of the same element.
True
104
MCQ: The atomic number of Sodium (Na) is A) 6 B) 8 C) 11
C) 11
105
True or False: The atomic number of Hydrogen is 1.
True
106
Fill in the blank: The number of protons in an atom is also called its ________ number.
Atomic"Question
107
MCQ: The mass number of an atom is equal to the sum of which two subatomic particles? A) Protons and Electrons B) Protons and Neutrons C) Neutrons and Electrons
B) Protons and Neutrons
108
True or False: The mass number is the same as the atomic number of an element.
False
109
Fill in the blank: The number of neutrons in an atom can be calculated using the formula: Mass Number = ________ + Number of Neutrons.
Number of Protons
110
MCQ: What is the mass number of Carbon if it has 6 protons and 6 neutrons? A) 12 B) 6 C) 18
A) 12
111
True or False: The atomic number of an element is equal to the number of protons in its nucleus.
True
112
Fill in the blank: The number of neutrons in Carbon is calculated as: Mass Number - Atomic Number = ________.
6
113
MCQ: If an element has an atomic number of 8, how many protons does it have? A) 8 B) 16 C) 6
A) 8
114
True or False: The number of electrons in a neutral atom is equal to the number of protons.
True
115
Fill in the blank: The number of neutrons in an Oxygen atom with an atomic mass of 16 and atomic number 8 is ________.
8
116
MCQ: What is the atomic number of Oxygen? A) 6 B) 8 C) 12
B) 8
117
True or False: Isotopes of the same element have different atomic numbers but the same mass number.
False
118
Fill in the blank: Isotopes of an element have the same ________ but different mass numbers.
Atomic Number
119
MCQ: Which of the following is an isotope of Carbon? A) Carbon-12 B) Carbon-14 C) Both A and B
C) Both A and B
120
True or False: Isotopes of an element have the same number of protons but a different number of neutrons.
True
121
Fill in the blank: An atom of Lithium has three protons and four neutrons. Its atomic number is ________ and its atomic mass is ________.
3, 7
122
MCQ: If the atomic number of iron is 26 and its atomic mass is 56, how many neutrons does an iron atom have? A) 30 B) 26 C) 56
A) 30
123
True or False: An isotope of an element has the same number of protons but a different number of electrons.
False"Question
124
MCQ: What is the standard atom used for comparing atomic masses? A) Hydrogen B) Oxygen C) Carbon-12
C) Carbon-12
125
True or False: Atomic masses are expressed in grams or kilograms.
False
126
Fill in the blank: The relative atomic mass of an element is the mass of an atom of that element relative to the mass of the atom of ________.
Carbon-12
127
MCQ: 1 atomic mass unit (a.m.u.) is equal to the mass of 1/12th of the mass of which atom? A) Oxygen B) Carbon-12 C) Hydrogen
B) Carbon-12
128
True or False: The relative atomic mass is always a whole number.
False
129
Fill in the blank: The relative atomic mass of oxygen is ________ a.m.u.
15.8994
130
MCQ: Which of the following elements has an atomic mass of 24.3050 a.m.u.? A) Sodium B) Magnesium C) Silver
B) Magnesium
131
True or False: Average atomic mass is the weighted average of the atomic masses of naturally occurring isotopes of an element.
True
132
Fill in the blank: The average atomic mass of chlorine is calculated by taking into account its isotopes chlorine-35 and chlorine-37 and their ________ abundance.
Percentage
133
MCQ: What is the average atomic mass of chlorine? A) 37 a.m.u. B) 35.5 a.m.u. C) 32 a.m.u.
B) 35.5 a.m.u.
134
True or False: The relative atomic mass of an element can be a decimal due to the presence of isotopes.
True
135
Fill in the blank: The average atomic mass of chlorine is calculated as: Atomic mass of Cl-35 × its ________ abundance + Atomic mass of Cl-37 × its ________ abundance.
Percentage, Percentage
136
MCQ: What is the atomic mass of hydrogen? A) 1.0079 a.m.u. B) 15.8994 a.m.u. C) 22.9897 a.m.u.
A) 1.0079 a.m.u.
137
True or False: The atomic mass of an element is the same for all of its isotopes.
False
138
Fill in the blank: The atomic mass of silver is ________ a.m.u.
107.8082
139
MCQ: What does the atomic mass unit (a.m.u.) represent? A) The mass of an atom of hydrogen B) The mass of an atom of carbon-12 C) The mass of an atom of oxygen
B) The mass of an atom of carbon-12"Question
140
MCQ: What is the empirical formula of a compound? A) The actual formula showing the exact number of atoms B) The simplest formula showing the smallest whole number ratio of atoms C) A random formula with no meaning
B) The simplest formula showing the smallest whole number ratio of atoms
141
True or False: The molecular formula of a compound always shows the exact number of atoms of each element in the compound.
True
142
Fill in the blank: The molecular formula of a compound is derived from the empirical formula by multiplying it by a factor '____'.
n
143
MCQ: The molecular formula of glucose is A) C6H12O6 B) CH2O C) C5H10O5
A) C6H12O6
144
True or False: The empirical formula of benzene is C6H6.
False
145
Fill in the blank: The empirical formula of benzene is _____, while its molecular formula is C6H6.
CH
146
MCQ: The average atomic mass of chlorine can be calculated using the relative atomic masses of chlorine-35 and chlorine-37. If the abundances of these isotopes are 75% and 25%, respectively, what is the average atomic mass? A) 35.5 a.m.u. B) 36.5 a.m.u. C) 37.5 a.m.u.
A) 35.5 a.m.u.
147
True or False: The molecular formula of a compound always has the simplest ratio of elements.
False
148
Fill in the blank: The molecular formula of benzene is derived by multiplying the empirical formula CH by a factor of _______.
6
149
MCQ: What does the empirical formula represent? A) The actual number of atoms in the compound B) The smallest whole number ratio of atoms in the compound C) The chemical reaction of the compound
B) The smallest whole number ratio of atoms in the compound
150
True or False: The molecular formula of glucose (C6H12O6) is the same as its empirical formula.
False
151
Fill in the blank: To calculate the average atomic mass of gallium, the atomic masses of Ga-69 and Ga-71 must be multiplied by their respective __________ abundance.
Percentage
152
MCQ: The molecular formula of glucose is A) C6H12O6 B) CH2O C) C6H10O5
A) C6H12O6
153
True or False: The molecular formula of a compound is the exact representation of the number of atoms in one molecule of the compound.
True
154
MCQ: The empirical formula of glucose is A) C6H12O6 B) CH2O C) C12H24O12
B) CH2O"Question
155
MCQ: What is the molecular mass of ethane (C2H6)? A) 24 a.m.u. B) 30 a.m.u. C) 32 a.m.u.
B) 30 a.m.u.
156
True or False: The empirical formula of acetic acid is the same as its molecular formula.
False
157
Fill in the blank: The molecular mass is calculated by adding the relative atomic masses of all the atoms present in a ______ of a substance.
Molecule
158
MCQ: What is the formula mass of sodium chloride (NaCl)? A) 32.5 amu B) 58.5 amu C) 12 amu
B) 58.5 amu
159
True or False: Formula mass is the sum of the atomic masses of ions in a formula unit of an ionic compound.
True
160
Fill in the blank: The formula mass of NaCl is calculated by adding the atomic masses of one atom of sodium and one atom of chlorine, which are 23 amu and 35.5 amu, respectively, to give a total of ______ amu.
58.5 amu
161
MCQ: The molecular formula of ethane is A) CH4 B) C2H6 C) C3H8
B) C2H6
162
True or False: The formula unit is the smallest repeating unit of a compound that shows the ratio of atoms in an ionic compound.
True
163
Fill in the blank: The molecular mass of a compound is the sum of the relative atomic masses of all the atoms in one ______ of that compound.
Molecule
164
MCQ: The formula mass of Fe(NO3)2 is A) 180 amu B) 150 amu C) 120 amu
A) 180 amu
165
True or False: The molecular formula and the empirical formula of a compound are always the same.
False
166
Fill in the blank: The molecular formula of benzene is C6H6, and its empirical formula is ______.
CH
167
MCQ: Which of the following compounds has an empirical formula different from its molecular formula? A) Acetylene B) Benzene C) Glucose
B) Benzene
168
True or False: The molecular mass of a substance is the same as its formula mass for ionic compounds.
False
169
Fill in the blank: The formula mass of Fe(NO3)2 can be calculated by adding the atomic masses of iron (56 amu), nitrogen (14 amu), and oxygen (16 amu), giving a total of ______ amu.
180 amu"Question
170
MCQ: What is a molecular ion? A) A neutral atom B) A molecule that has lost or gained electrons C) An ionic compound
B) A molecule that has lost or gained electrons
171
True or False: Anionic molecular ions carry a negative charge.
True
172
Fill in the blank: A ______ is a molecule that has gained or lost electrons and has a charge.
Molecular ion
173
MCQ: Which of the following is an example of a cationic molecular ion? A) CH3+ B) CH3- C) H2O
A) CH3+
174
True or False: Free radicals have paired electrons in their outer shell.
False
175
Fill in the blank: Free radicals are atoms or groups of atoms with a ______ electron in their outer shell.
Unpaired
176
MCQ: What is formed when a chlorine molecule breaks into two atoms, each having an unpaired electron? A) Chlorine molecular ion B) Chlorine free radical C) Chlorine ion
B) Chlorine free radical
177
True or False: Free radicals are stable and exist independently in nature.
False
178
MCQ: What is an example of a polyatomic molecule? A) O2 B) H2O C) Ne
B) H2O
179
True or False: Monoatomic molecules consist of only one atom.
True
180
Fill in the blank: ______ molecules consist of three atoms and include substances like water (H2O).
Tri-atomic
181
MCQ: Which of the following is an example of a monoatomic molecule? A) Ne B) O2 C) H2O
A) Ne
182
Fill in the blank: A ______ molecule is formed by the chemical combination of many atoms, such as sulphuric acid (H2SO4).
Polyatomic
183
True or False: Hemoglobin is an example of a macromolecule.
True
184
MCQ: What type of molecule is made of only one atom? A) Polyatomic B) Diatomic C) Monoatomic
C) Monoatomic"Question
185
MCQ: What is a homoatomic molecule? A) A molecule made of atoms of different elements B) A molecule made of atoms of the same element C) A molecule made of ions
B) A molecule made of atoms of the same element
186
True or False: Oxygen (O2) is an example of a homoatomic molecule.
True
187
Fill in the blank: A ______ molecule consists of atoms of different elements.
Heteroatomic
188
MCQ: Which of the following is an example of a heteroatomic molecule? A) O2 B) CO2 C) Cl2
B) CO2
189
True or False: Water (H2O) is an example of a heteroatomic molecule.
True
190
MCQ: What does Avogadro's number represent? A) The mass of one mole of a substance B) The number of particles in one mole of a substance C) The volume of one mole of a substance
B) The number of particles in one mole of a substance
191
True or False: Avogadro's number is 6.023 × 10^23.
True
192
Fill in the blank: Avogadro's number is equal to ______ particles in one mole of any substance.
6.023 × 10^23
193
MCQ: How many atoms are in 1 mole of hydrogen? A) 6.023 × 10^23 B) 12 C) 1
A) 6.023 × 10^23
194
True or False: 12 grams of carbon equals 1 mole.
True
195
Fill in the blank: One mole of NaCl weighs ______ grams.
58.5
196
MCQ: If a computer counts at a speed of 10 million atoms per second, how long would it take to count one mole of atoms? A) 2 billion years B) 2 hours C) 2 minutes
A) 2 billion years
197
True or False: The mole is a counting unit used by chemists to measure the amount of a substance.
True
198
MCQ: How many molecules are in 1 mole of water? A) 6.023 × 10^23 B) 1 molecule C) 10 molecules
A) 6.023 × 10^23
199
Fill in the blank: If one mole of marbles were spread over the Earth, it would cover the surface with a ______ thick layer of marbles.
Three miles
200
True or False: The mole concept helps chemists count atoms, molecules, and ions in large quantities.
True"Question
201
MCQ: What is the unit used to represent the amount of substance in the mole concept? A) Grams B) Moles C) Atoms
B) Moles
202
True or False: A mole is defined as the amount of a substance that contains Avogadro's number of particles.
True
203
Fill in the blank: The mass of a substance when expressed in grams is called its ______ mass.
Molar
204
MCQ: Which of the following represents the mole of a substance? A) Mass in grams B) Number of atoms C) Volume in liters
A) Mass in grams
205
True or False: 12 grams of carbon is equal to 1 mole of carbon.
True
206
Fill in the blank: The molecular mass of water (H2O) is 18 g, which equals ______ mole(s) of water.
1 mole
207
MCQ: What is the gram atomic mass of oxygen? A) 16g B) 18g C) 12g
A) 16g
208
True or False: The gram formula mass of sodium chloride (NaCl) is 58.5g, which represents 1 mole of sodium chloride.
True
209
MCQ: What is the term used when the relative atomic mass of a substance is expressed in grams? A) Gram atomic mass B) Molecule mass C) Molarity
A) Gram atomic mass
210
True or False: The gram molecular mass of carbon dioxide (CO2) is 44.01g.
True
211
Fill in the blank: When the formula mass of an ionic compound is expressed in grams, it is called ______ mass.
Gram formula
212
MCQ: Which of the following compounds has a gram molecular mass of 98g? A) Water B) Sulfuric acid C) Carbon dioxide
B) Sulfuric acid
213
True or False: The gram molecular mass of water is 18g.
True
214
MCQ: The mass of one mole of sodium chloride (NaCl) is equal to: A) 12g B) 58.5g C) 18g
B) 58.5g
215
Fill in the blank: The gram molecular mass of water (H2O) is ______g.
18g
216
MCQ: What is the mole concept primarily used for in chemistry? A) To calculate the number of particles in a sample B) To measure the volume of gases C) To determine the color of substances
A) To calculate the number of particles in a sample"Question
217
MCQ: What is the formula mass of KCl? A) 58.5 amu B) 74.5 amu C) 39.5 amu
B) 74.5 amu
218
MCQ: What is the formula mass of Na2CO3? A) 106 amu B) 105 amu C) 104 amu
A) 106 amu
219
Fill in the blank: A ______ is formed when an atom gains or loses one or more electrons, resulting in a net charge.
Ion
220
True or False: A cation is a negatively charged ion formed when an atom gains electrons.
False
221
MCQ: Which of the following ions is a cation? A) Na+ B) Cl- C) O2-
A) Na+
222
True or False: An anion has more electrons than protons.
True
223
Fill in the blank: The positive charge on a cation results from the loss of ______.
Electrons
224
MCQ: Which of the following is an example of an anion? A) Na+ B) Cl- C) Fe3+
B) Cl-
225
True or False: The formula mass of NaCl is the sum of the atomic masses of Na and Cl.
True
226
Fill in the blank: The formula mass of KCl is calculated by adding the atomic mass of K (39.5 amu) and Cl (35.5 amu), which gives ______ amu.
74.5 amu
227
MCQ: Which of the following describes an anion? A) Loss of electrons B) Gain of electrons C) Equal protons and electrons
B) Gain of electrons
228
True or False: The number of protons in a cation is greater than the number of electrons.
True
229
Fill in the blank: A neutral atom has the same number of ______ and electrons.
Protons
230
MCQ: What happens when an atom loses an electron? A) It becomes a cation B) It becomes an anion C) It becomes neutral
A) It becomes a cation
231
True or False: Anions always have fewer electrons than protons.
False"Question
232
MCQ: What is the molar mass of CO2? A) 44 g/mol B) 12 g/mol C) 32 g/mol
A) 44 g/mol
233
True or False: 1 mole of CO2 is equal to 44 grams of CO2.
True
234
Fill in the blank: The molar mass of water (H2O) is ______ grams.
18 grams
235
MCQ: Avogadro's number represents the number of particles in: A) 1 mole of a substance B) 1 gram of a substance C) 1 liter of a substance
A) 1 mole of a substance
236
True or False: 1 mole of any substance contains 6.023 × 10^23 particles.
True
237
Fill in the blank: The formula to calculate the number of particles is: No. of particles = No. of moles x ______.
6.023 × 10^23
238
MCQ: How many particles are in 2 moles of water? A) 6.023 × 10^23 B) 12.046 × 10^23 C) 3.011 × 10^24
B) 12.046 × 10^23
239
True or False: To calculate the number of moles, you divide the mass of a substance by its molar mass.
True
240
Fill in the blank: To calculate the mass of a substance, the equation is: Mass = No. of moles x ______ mass.
Molar
241
MCQ: If you have 60g of CO2, how many moles of CO2 do you have? A) 1.36 moles B) 2.5 moles C) 1 mole
A) 1.36 moles
242
True or False: The relationship between moles and mass is: Mass (in grams) = No. of moles x Molar mass.
True
243
Fill in the blank: 1 mole of water (H2O) weighs ______ grams.
18 grams
244
MCQ: To calculate the number of moles of a substance, you divide its mass by: A) Avogadro's number B) Molar mass C) Volume
B) Molar mass
245
True or False: 6.023 × 10^23 is also called Avogadro's number and is used to convert moles to particles.
True
246
Fill in the blank: To find the number of moles, you divide the number of particles by ______.
6.023 × 10^23"Question
247
MCQ: How many moles of hydrogen are there in 8.9 x 10^3 hydrogen atoms? A) 1.48 moles B) 1 mole C) 6.023 x 10^23 moles
A) 1.48 moles
248
True or False: Avogadro's number is 6.023 x 10^23 particles per mole.
True
249
Fill in the blank: To calculate the number of moles from the number of atoms, use the formula: No. of moles = No. of atoms / ______.
Avogadro's number (6.023 x 10^23)
250
MCQ: How many moles are in 3.01 x 10^23 molecules of CO2? A) 1.48 moles B) 0.5 moles C) 1 mole
B) 0.5 moles
251
True or False: The number of molecules in 5 moles of glucose (C6H12O6) is 6.023 x 10^23.
False
252
Fill in the blank: The number of molecules in 5 moles of glucose can be calculated by: No. of molecules = No. of moles x ______.
6.023 x 10^23
253
MCQ: What is the molar mass of CO2? A) 12 g/mol B) 32 g/mol C) 44 g/mol
C) 44 g/mol
254
True or False: Mole-mass calculations are based on the relationship: Mass (in grams) = No. of moles x Molar mass.
True
255
Fill in the blank: The formula to calculate the mass of a substance is: Mass = No. of moles x ______.
Molar mass
256
MCQ: How many moles of water (H2O) are there in 60g of H2O? A) 1.0 mole B) 3.3 moles C) 2 moles
A) 1.0 mole
257
True or False: The number of particles in 1 mole of any substance is 6.023 x 10^23.
True
258
Fill in the blank: To calculate the number of particles in a substance, multiply the number of moles by ______.
6.023 x 10^23
259
MCQ: How many moles of CO2 are in 60g of CO2? A) 1.36 moles B) 2 moles C) 3.6 moles
A) 1.36 moles
260
True or False: 1 mole of water weighs 44 grams.
False
261
Fill in the blank: 1 mole of a substance contains 6.023 x 10^23 ______.
particles"Question
262
MCQ: Which one of the following groups comprises elements? A) Mercury, water, Ammonia B) Iodine, Tin, Iron C) Copper, Aluminum, Methane D) Coal, Smoke, Fog
B) Iodine, Tin, Iron
263
True or False: The average atomic mass is the weighted average of the atomic masses of the naturally occurring isotopes of an element.
True
264
Fill in the blank: A ______ is the shorthand method of representing a compound.
Chemical formula
265
MCQ: Which one of the following can be broken down into simpler substances? A) Ammonia B) Iron C) Oxygen D) Coal
A) Ammonia
266
True or False: The empirical formula shows the actual number of atoms present in a molecule of a compound.
False
267
Fill in the blank: The ______ formula shows the smallest whole number ratio of the atoms/ions present.
Empirical
268
MCQ: The gram molecular mass of HNO3 is: A) 60 B) 100 C) 98 D) 110
C) 98
269
True or False: A molecule is the smallest particle of a compound or element that can exist independently.
True
270
Fill in the blank: Molecules made up of different atoms are called ______ molecules.
Hetero-atomic
271
MCQ: Which of these molecules is not a compound? A) N2 B) NO C) CH4 D) H2O
A) N2
272
True or False: The molecular formula of a compound shows the actual number of atoms present in a molecule.
True
273
MCQ: Which one of the following is equal to two moles of water (H2O)? A) 1.084 x 10^23 molecules B) 6.022 x 10^23 molecules C) 1.204 x 10^24 molecules D) 1.806 x 10^24 molecules
C) 1.204 x 10^24 molecules
274
True or False: Avogadro's number is 6.023 x 10^23 atoms or molecules per mole.
True
275
Fill in the blank: A molecule formed from the same kind of atoms is called a ______ molecule.
Homo-atomic
276
MCQ: Hydrogen gas is: A) A monoatomic gas B) A mixture of hydrogen atoms C) A diatomic gas with each molecule made up of two atoms D) A diatomic atom made up of two molecules
C) A diatomic gas with each molecule made up of two atoms
277
True or False: A free radical is a species with an unpaired electron and is the result of homolytic fission of the bond.
True
278
MCQ: Which one of the following is an example of a triatomic molecule? A) A monoatomic gas B) O2 C) O3 D) NH3
C) O3
