MCQ in General Chemistry Part 3 | ECE Board Exam

This is the Multiples Choice Questions Part 3 of the Series in General Chemistry as one of the General Engineering and Applied Sciences (GEAS) topics. In Preparation for the ECE Board Exam make sure to expose yourself and familiarize yourself with each and every question compiled here taken from various sources including past Board Questions in General Engineering and Applied Sciences (GEAS) field.

Continue Practice Exam Test Questions Part 3 of the Series

⇐ MCQ in General Chemistry Part 2 | ECE Board Exam

Choose the letter of the best answer in each question.

101. What is the most abundant element in the atmosphere?

A. Oxygen

B. Nitrogen

C. Helium

D. Inert gases

102. What is the only gas in Group VIA in the periodic table?

A. Argon

B. Krypton

C. Oxygen

D. Helium

103. What is the second most abundant element in the atmosphere?

A. Hydrogen

B. Helium

C. Oxygen

D. Nitrogen

104. What element is used in advertising signs?

A. Neon

B. Helium

C. Sodium

D. Xenon

105. What principle states about the fundamental limitation that, for a particle as small as the electron, one cannot know exactly where it is and at the same time know its energy how it is moving?

A. Autbau principle

B. Uncertainty principle

C. Pauli exclusion principle

D. Kinetic molecular theory

106. Who discovered the uncertainty principle?

A. Werner Karl Heisenberg principle

B. Louie de Broglie

C. Albert Einstein

D. John Newlands

107. What principle states that the electrons fill the orbitals, one at a time, starting with the lowest orbital then proceeding to the one with higher energy?

A. Autbau principle

B. Uncertainty principle

C. Pauli exclusion principle

D. Kinetic molecular theory

108. What principle states that no two electrons in the same atom can have the same set of four quantum numbers?

A. Autbau principle

B. Uncertainty principle

C. Pauli exclusion principle

D. Kinetic molecular theory

109. What describes how the electrons and distributed among the orbitals?

A. Electronegativity of the element

B. Electron configuration of an atom

C. Energy state of the atom

D. Pauli exclusion principle

110. The _______ of the atom describes the atom as having a nucleus at the center around which electrons move?

A. spin number

B. quantum mechanical model

C. quantum number

D. azimuthal number

111. What are the main energy levels where the valence electrons belong called?

A. Valence shells

B. Azimuthal shells

C. Spin shells

D. Quantum shells

112. The elements of groups IA, IIA, IIIA, IVA, VA, VIA, VIIA and VIIIA are called main group elements or

A. transition

B. representatives

C. inner transitions

D. metals or nonmetals

113. For the representative elements, the number of valence electrons is the same as the _____.

A. number of electrons

B. number of neutrons

C. the rightmost digit of the group number of the element

D. number of electrons less the number of neutrons

114. For transition elements, the number of valence electron is the same as _______.

A. the group number

B. the rightmost digit of the group number of the element

C. the number of electrons less the number of neutrons

D. the number of electrons less the number of protons

115. The size of the atom is dependent on which of the following:

A. the size of the nucleus

B. the region of space occupied by its electrons

C. the number of protons and neutrons

D. all of the choices above

116. What happens to the atomic size of the elements in a group when you go from top to bottom of the group?

A. It remains the same

B. It increases

C. It decreases

D. It become zero

117. Who first predicted the Bose-Einstein condensate (BEC) in 1924?

A. Albert Einstein

B. Satyendra Nath Bose

C. Carl Wieman

D. Wollgang Ketterie

118. The ionization energy is _________ to the atomic size of atom.

A. directly proportional

B. inversely proportional

C. equal to

D. not related

119. What refers to the measure of the atom’s tendency to attract an additional electron?

A. Period number

B. Electron affinity

C. Ionization energy

D. Electronegativity

120. The process of gaining or losing an electron results to the formation of a charged atom or molecule called _______.

A. ion

B. cation

C. anion

D. crystal

121. Aside from liquid, gas and solid, there are two other states of matter.

A. Plasma and Quark

B. Quartz and Plasma

C. Quartz and Quasar

D. Plasma and Bose-Einstein condensate

122. Who first identified plasma in 1879?

A. William Crookes

B. Irving Langmuir

C. Albert Einstein

D. Eric Cornell

123. Who coined the term “plasma” in 1928?

A. William Crookes

B. Irving Langmuir

C. Albert Einstein

D. Eric Cornell

124. What is made of gas atoms that have been cooled to near absolute zero at which temperature the atoms slow down, combine and forms a single entity known called a super atom?

A. Ionized gas

B. Bose-Einstein condensate (BEC)

C. Plasma

D. Quark

125. The fifth state of matter, the BEC (Bose-Einstein condensate) was first created in what year?

A. 1992

B. 1993

C. 1994

D. 1995

126. What is a high-energy, electrically charged gas produced by heating the gas until the electrons in the outer orbitals of the atoms separate, leaving the atoms with a positive charge?

A. Quartz

B. Quark

C. BEC

D. Plasma

127. Water has bigger density when it is in what state?

A. Liquid

B. Gas

C. Solid

D. Vapor

128. What is the temperature of water in solid state at 1 atm?

A. 4°C

B. 25°C

C. 0°C

D. 5°C

129. The density of water is the largest at what temperature?

A. 2°C

B. 1°C

C. 3°C

D. 4°C

130. What element has a very high melting point and ideal for filaments of light bulbs?

A. Barium

B. Aluminum

C. Tungsten

D. Titanium

131. Metals can be drawn into wires. This illustrates what property of metals?

A. Malleability

B. Ductility

C. Rigidity

D. Plasticity

132. Steel is the widely used construction material because of its high tensile strength. It is a combination of what element?

A. Iron and carbon

B. Iron and aluminum

C. Lead and carbon

D. Lead and aluminum

133. What refers to the electrostatic attraction that holds together the oppositely charged ions, the cations and anions, in the solid compound?

A. Electronic bond

B. Metallic bond

C. Covalent bond

D. Ionic bond

134. What states that atoms tend to gain, lose or share electrons until they are surrounded by eight valence electrons?

A. Figure of 8 rule

B. Octet rule

C. Ionic rule

D. Lewis rule

135. What indicates the number of valence electrons to the atom represented by dots scattered on four sides of the atomic symbol?

A. Electron dot structure

B. Lewis structure

C. Crystalline structure

D. Electron dot structure or Lewis structure

136. What is formed by sharing of electrons between atom?

A. Covalent bond

B. Ionic bond

C. Metallic bond

D. Electronic band

137. What is the distance between the nuclei of two bonded atoms called?

A. Bond length

B. Molecular length

C. Atomic distance

D. Atomic radius

138. The overall shape of a molecule is described by which two properties?

A. Bond distance and bond size

B. Bond distance and bond angle

C. Bond radius and bond angle

D. Bond angle and bond size

139. What is an angle made by the lines joining the nuclei of the atoms in the molecule?

A. Atomic angle

B. Bond angle

C. Molecular angle

D. Ionic angle

140. “The best arrangement of a given number of shared and unshared electrons is the one that minimizes the repulsion among them”. This is known as ___________.

A. valence bond theory

B. electron group theory

C. molecular polarity theory

D. valence-shell electron-pair repulsion theory

141. “A covalent bond is formed by the overlap of atomic orbitals.” This statement is the basic idea of which theory?

A. Valence bond theory

B. Energy group theory

C. Molecular polarity theory

D. Valence-shell electron-pair repulsion (VSPER) theory

142. What refers to the ability of an atom in a molecule to attract shared electrons?

A. Electronegativity

B. Electron affinity

C. Ionization energy

D. Periodic number

143. What type of bond occurs when the difference in electronegativity is greater than or equal to 2?

A. Ionic

B. Nonpolar covalent

C. Polar covalent

D. Either nonpolar covalent or polar covalent

144. Nonpolar covalent bond occurs if the difference in electronegativity ranges from:

A. 0.00 to 0.40

B. 0.50 to 1.90

C. 1.90 to 2.00

D. 2.00 and up

145. When can we say that a molecule is polar?

A. When the centers of positive and negative charge do not coincide

B. When the centers of positive and negative charge coincide

C. When there is no positive nor negative charge

D. When there is only one charge, either negative or negative

146. What is the sum of the masses of the atoms in the molecule of the substance called?

A. Atomic mass

B. Molecular mass

C. Formula mass

D. Atomic weight

147. What refers to the number of atoms in exactly 12 grams of carbon-12?

A. Avogadro’s number

B. Mole

C. Molar mass

D. amu

148. Which one is the Avogado’s number?

A. 6.20 x 10^23

B. 6.62 x 10^23

C. 6.32 x 10^23

D. 6.22 x 10^23

149. What is defined as the amount of substance that contains 6.02 x 10²³ particles of that substance?

A. Mole

B. Molar mass

C. Atomic mass

D. amu

150. What refers to the mass in grams of one mole of a substance?

A. Molar mass

B. Molecular mass

C. Atomic mass

D. Atomic weight

Complete List of MCQs in General Engineering and Applied Science per topic