Chemistry Diagnostic Exam: Quiz! Trivia

Which statement describes a chemical change?    

• Alcohol evaporates.

• Water vapor forms snowflakes.

• Table salt (NaCl) is crushed into powder.

• Glucose (C6H12O6) and oxygen produce CO2 and H2O.

What is the number of electrons in a completely filled second shell of an atom? 

• 32

• 2

• 18

• 8

Which atom attains a stable valence electron configuration by bonding with another atom? 

• Neon

• Radon

• Hydrogen

• Helium

A mixture of sand and table salt can be separated by filtration because the substances in the mixture differ in 

• Solubility in water

• Freezing point

• Density at STP

• Boiling point

An ion that consists of 7 protons, 6 neutrons, and 10 electrons has a net charge of 

• 4−

• 3−

• 3+

• 4+

Which quantity is equal to 50 kilojoules?    

• 0.05 J

• 5000 J

• 500 J

• 50 000 J

In the wave-mechanical model of the atom, an orbital is the most probable location of 

• A proton

• A positron

• A neutron

• An electron

Which Lewis electron-dot diagram represents a molecule having a nonpolar covalent bond? 

What is the number of electrons in an atom that has 3 protons and 4 neutrons? 

• 1

• 7

• 3

• 4

Which particle has the least mass?

• Alpha particle

• Beta particle

• Neutron

• Proton

Which element has the lowest electronegativity value? 

• F

• Fr

• Cl

• Cr

In a propanal molecule, an oxygen atom is bonded with a carbon atom.  What is the total number of pairs of electrons shared between these atoms?

• 1

• 2

• 3

• 4

When dissolved in water, an Arrhenius base yields

• Hydrogen ions

• Hydronium ions

• Hydroxide ions

• Oxide ions

Which element is paired with an excited-state electron configuration for an atom of the element? 

• Ca: 2-8-8-2

• Na: 2-8-2

• K: 2-6-8-3

• F: 2-8

Given the balanced equation representing a nuclear reaction:  Which phrase identifies and describes this reaction? 

• Fission, mass converted to energy

• Fission, energy converted to mass

• Fusion, mass converted to energy

• Fusion, energy converted to mass

The elements in Group 2 are classified as    

• Metals

• Metalloids

• Nonmetals

• Noble gases

Which sample of CO2 has a definite shape and a definite volume? 

• CO2 (aq)

• CO2 (g)

• CO2 (l)

• CO2 (s)

At standard pressure, CH4 boils at 112 K and H2O boils at 373 K. What accounts for the higher boiling point of H2O at standard pressure? 

• Covalent bonding

• Ionic bonding

• Hydrogen bonding

• Metallic bonding

Some solid KNO3 remains at the bottom of a stoppered flask containing a saturated KNO3(aq) solution at 22°C. Which statement explains why the contents of the flask are at equilibrium? 

• The rate of dissolving is equal to the rate of crystallization.

• The rate of dissolving is greater than the rate of crystallization.

• The concentration of the solid is equal to the concentration of the solution.

• The concentration of the solid is greater than the concentration of the solution.

Systems in nature tend to undergo changes toward 

• Lower energy and lower entropy

• Lower energy and higher entropy

• Higher energy and lower entropy

• Higher entropy and higher entropy

Which statement describes the distribution of charge in an atom? 

• A neutral nucleus is surrounded by one or more negatively charged electrons.

• A neutral nucleus is surrounded by one or more positively charged electrons.

• A positively charged nucleus is surrounded by one or more negatively charged electrons.

• A positively charged nucleus is surrounded by one or more positively charged electrons.

• Mass number, only

• Atomic number, only

• Both mass number and atomic number

• Neither mass number nor atomic number

Given the equation and potential energy diagram representing a reaction:  If each interval on the axis labeled “Potential Energy (kJ/mol)” represents 10. kJ/mol, what is the heat of reaction? 

• +60. kJ/mol

• +20. kJ/mol

• +30. kJ/mol

• +40. kJ/mol

Functional groups are used to classify    

• Organic compounds

• Inorganic compounds

• Heterogeneous mixtures

• Homogeneous mixtures

The elements on the Periodic Table are arranged in order of increasing 

• Atomic mass

• Atomic number

• Molar mass

• Oxidation number

What is the total number of valence electrons in a germanium atom in the ground state? 

• 22

• 2

• 32

• 4

Based on Reference Table J, which two reactants react spontaneously? 

• Mg(s) + ZnCl2(aq)

• Cu(s) + FeSO4(aq)

• Pb(s) + ZnCl2(aq)

• Co(s) + NaCl(aq)

As a result of the gold foil experiment, it was concluded that an atom.

• Contains protons, neutrons, and electrons

• Contains a small, dense nucleus

• Has positrons and orbitals

• Is a hard, indivisible sphere

Given the equation representing a reversible reaction:  According to one acid-base theory, the reactant that donates an H+ ion in the forward reaction is 

• NH3(g)

• H2O(l)

• NH4+(aq)

• OH (aq)

Which sample of matter is classified as a substance? 

• Air

• Ammonia

• Milk

• Seawater

An ionic bond can be formed when one or more electrons are 

• Equally shared by two atoms

• Unequally shared by two atoms

• Transferred from the nucleus of one atom to the nucleus of another atom

• Transferred from the valence shell of one atom to the valence shell of another atom

What occurs in order to break the bond in a Cl2 molecule? 

• Energy is absorbed.

• Energy is released.

• The molecule creates energy.

• The molecule destroys energy.

Which statement describes the particles of an ideal gas according to the kinetic molecular theory? 

• The gas particles are arranged in a regular geometric pattern.

• The gas particles are in random, constant, straight-line motion.

• The gas particles are separated by very small distances, relative to their sizes.

• The gas particles are strongly attracted to each other.

Given the balanced equations representing two chemical reactions:      Cl2 + 2NaBr → 2NaCl + Br2      2NaCl → 2Na + Cl2 Which types of chemical reactions are represented by these equations? 

• Single replacement and decomposition

• Single replacement and double replacement

• Synthesis and decomposition

• Synthesis and double replacement

At 25°C, gas in a rigid cylinder with a movable piston has a volume of 145 mL and a pressure of 125 kPa. Then the gas is compressed to a volume of 80. mL. What is the new pressure of the gas if the temperature is held at 25°C? 

• 69 kPa

• 93 kPa

• 160 kPa

• 230 kPa

A 2400.-gram sample of an aqueous solution contains 0.012 gram of NH3. What is the concentration of NH3 in the solution, expressed as parts per million? 

• 5.0 ppm

• 15 ppm

• 20. ppm

• 50. ppm

A solution consists of 0.50 mole of CaCl2 dissolved in 100. grams of H2O at 25°C. Compared to the boiling point and freezing point of 100. grams of H2O at standard pressure, the solution at standard pressure has 

• A lower boiling point and a lower freezing point

• A lower boiling point and a higher freezing point

• A higher boiling point and a lower freezing point

• A higher boiling point and a higher freezing point

Which formula represents the product of the addition reaction between ethene and chlorine, Cl2? 

A sealed, rigid 1.0-liter cylinder contains He gas at STP. An identical sealed cylinder contains Ne gas at STP. These two cylinders contain the same number of 

• Atoms

• Electrons

• Ions

• Protons

Which class of compounds contains at least one element from Group 17 of the Periodic Table?

• Aldehyde

• Amine

• Ester

• Halide

Which equation represents a change that results in an increase in disorder? 

• I2 (s) → I2 (g)

• CO2 (g) → CO2 (s)

• 2Na (s) + Cl2 (g) → 2NaCl (s)

• 2H2 (g) + O2 (g) → 2H2O (l)

When a voltaic cell operates, ions move through the 

• Anode

• Cathode

• Salt bridge

• External circuit

Which atom in the ground state has an outermost electron with the most energy? 

• Cs

• K

• Li

• Na

Which list includes elements with the most similar chemical properties? 

• Br, Ga, Hg

• Cr, Pb, Xe

• O, S, Se

• N, O, F

At which temperature is the vapor pressure of ethanol equal to 80. kPa? 

• 48°C

• 73°C

• 80.°C

• 101°C

Given the balanced ionic equation representing a reaction:  Which half-reaction represents the reduction that occurs? 

Which pair represents two forms of an element in the same phase at STP but with different structures and different properties? 

• I2(s) and I2(g)

• O2(g) and O3(g)

• H2(g) and Hg(g)

• H2O(s) and H2O(l)

Which compound is formed from its elements by an exothermic reaction at 298 K and 101.3 kPa? 

• C2H4 (g)

• HI (g)

• H2O (g)

• NO2 (g)