Chemistry Trivia Questions for Students
190 trivia questions with answers, students. Multiple-choice trivia with answers, sorted by topic and level. Reveal the answers below, pick one at random, or present them full-screen.
- 1.
Which of the following is true for all bases?
- AOnly strong bases create solutions in which OH- ions are present.
- BOnly strong bases are good conductors when dissolved in solution.
- CFor weak bases, the concentration of the OH-ions exceeds the concentration of the base in the solution.
- DAll bases donate OH- ions into solution.
Answer: Only strong bases are good conductors when dissolved in solution. - 2.
Cerium(III) sulfate, Ce2(SO4)2, is less soluble in hot water than it is in cold. Which of the following conclusions may be related to this?
- AThe heat of solution of cerium(III) sulfate is exothermic.
- BThe heat of solution for cerium(III) sulfate is endothermic.
- CThe hydration energies of cerium ions and sulfate ions are very low.
- DThe solution is not an ideal solution.
Answer: The heat of solution of cerium(III) sulfate is exothermic. - 3.
The electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 signifies the ground state of the element
- ACo
- BTi
- CV
- DCa
Answer: Ca - 4.
Silver metal, often amalgamated with mercury, is used to reduce substances to a desired oxidation state. If the silver metal amalgam cannot be used because of concerns about mercury, which of the following would be a reasonable and safe substitute?
- AH+(aq)
- BNa(s)
- CCa2+(aq)
- DMg(s)
Answer: Mg(s) - 5.
Which would be the easiest way to burn an iron nail?
- AGrind the nail into very small, dust-sized particles, and spray them into a flame
- BUse the method in (A), but use an oxyacetylene torch to reach a higher temperature.
- CHold an iron nail with crucible tongs, and heat strongly in the flame of a Bunsen burner.
- DDissolve the nail in acid to make the oxide.
Answer: Grind the nail into very small, dust-sized particles, and spray them into a flame - 6.
A sample of a compound known to consist of only carbon, hydrogen, and oxygen is found to have a total mass of 29.05 g. If the mass of the carbon is 18.02 g and the mass of the hydrogen is 3.03 g, what is the empirical formula of the compound?
- AC2H6O3
- BC2H4O
- CC3H6O
- DC3H8O2
Answer: C3H6O - 7.
The relationship between the vapor pressure of a liquid and the heat of vaporization is expressed in the
- AGibbs free energy equation
- BRydberg equation
- CClausius-Clapeyron equation
- DArrhenius equation
Answer: Clausius-Clapeyron equation - 8.
Consider the Lewis structures for the following molecules: CO2, CO32-, NO2-, and NO3-. Which molecule would have the shortest bonds?
- ACO2
- BCO32-
- CNO2-
- DNO3-
Answer: CO2 - 9.
How many electrons, neutrons, and protons are in an atom of 52Cr?
- A24 electrons, 28 protons, 24 neutrons
- B24 electrons, 24 protons, 28 neutrons
- C24 electrons, 24 protons, 24 neutrons
- D27 electrons, 27 protons, 24 neutrons
Answer: 24 electrons, 24 protons, 28 neutrons - 10.
Of the following, the most important experimental information used to deduce the structure of the atom was
- Athe specific heat capacity
- Bthe emission spectrum of the elements, particularly hydrogen
- Cthe density of each element
- Dthe X-rays emitted from each element
Answer: the emission spectrum of the elements, particularly hydrogen - 11.
What is the general relationship between temperature and entropy for diatomic gases?
- AIt depends on the specific gas and the strength of the intermolecular forces between individual molecules.
- BThey are completely independent of each other; temperature has no effect on entropy.
- CThere is an inverse relationship, because at higher temperatures substances are more likely to be in a gaseous state.
- DThere is a direct relationship, because at higher temperatures there is an increase in energy dispersal.
Answer: There is a direct relationship, because at higher temperatures there is an increase in energy dispersal. - 12.
Which of the following is expected to have two or more resonance structures?
- APF5
- BH2O
- CSO3
- DCCl2F2
Answer: SO3 - 13.
Which of the following indicates that a reaction is spontaneous?
- Athe value of ΔG° is greater than zero
- Bthe value of Keq is less than one
- Cat equilibrium there are more products than reactants
- Dthe value of ΔS° is greater than zero
Answer: at equilibrium there are more products than reactants - 14.
Which of the following is not a good measure of relative intermolecular attractive forces?
- AVapor pressures
- BHeat of fusion
- CBoiling points
- DHeat of vaporization
Answer: Heat of fusion - 15.
The oxidation number of chlorine in the perchlorate ion, ClO4–, is
- A2
- B-1
- C7
- D-3
Answer: 7 - 16.
Argon can be liquefied at low temperature because of
- Athe very low temperature
- Binstantaneous and induced dipoles
- Cdipole-dipole attractive forces
- Dhydrogen bonding
Answer: instantaneous and induced dipoles - 17.
The units for R, the ideal gas law equation constant, may be
- AL atm mol-1 K-1
- Bvolt coulomb mol-1 K-1
- C(A), (B), and (C)
- DJ mol-1 K-1
Answer: (A), (B), and (C) - 18.
Most transition metals share a common oxidation state of +2. Which of the following best explains why?
- ATransition metals tend to gain electrons when reacting with other elements.
- BTransition metals will lose their outermost s-block electrons when forming bonds.
- CTransition metals have unstable configurations and are very reactive.
- DTransition metals all have a minimum of two unpaired electrons.
Answer: Transition metals will lose their outermost s-block electrons when forming bonds. - 19.
London dispersion forces are caused by
- Athe uneven electron-to-proton ratio found on individual atoms of a molecule
- Btemporary dipoles created by the position of electrons around the nuclei in a molecule
- Cthe electronegativity differences between the different atoms in a molecule
- Dthe three-dimensional intermolecular bonding present in all covalent substances
Answer: temporary dipoles created by the position of electrons around the nuclei in a molecule - 20.
How many electrons, neutrons, and protons are in an atom of Cr?
- A24 electrons, 28 protons, 24 neutrons
- B24 electrons, 24 protons, 24 neutrons
- C27 electrons, 27 protons, 24 neutrons
- Dmore information is needed to answer this question
Answer: more information is needed to answer this question - 21.
Which of the following is expected to be a polar molecule?
- ASi(CH3)4
- BBF3
- CPCl4F
- DCO2
Answer: PCl4F - 22.
The reaction of Br2(g) with Cl2(g) to form BrCl(g) has an equilibrium constant of 15.0 at a certain temperature. If 10.0 grams of BrCl is initially present in a 15.0-liter reaction vessel, what will the concentration of BrCl be at equilibrium?
- A3.8 × 10^-3 mol/L
- B5.77 × 10^-3 mol/L
- C9.9 × 10^-4 M
- D1.97 × 10^-3 M
Answer: 3.8 × 10^-3 mol/L - 23.
What is the pH of a solution made by dissolving 0.0300 mol of sodium ethanoate in enough water to make 50 mL of solution (Ka for ethanoic acid is 1.8 × 10^-5)?
- A11.02
- B9.26
- C4.74
- D7
Answer: 9.26 - 24.
Which of the following substances has an asymmetrical molecular structure?
- APCl5
- BCO2
- CBF3
- DSF4
Answer: SF4 - 25.
The collision theory of reaction rates does not include
- Athe energy of each collision
- Bthe number of collisions per second
- Cthe orientation of each collision
- Dthe transition state
Answer: the transition state - 26.
The units for the rate of a chemical reaction are
- AL2 mol-2 s-1
- Bit depends on the particular reaction
- CL mol-1 s-1
- Dmol L-1 s-1
Answer: mol L-1 s-1 - 27.
Consider the Lewis structures for the following molecules: CO2, CO32-, NO2-, and NO3-. Which molecule or molecules exhibit sp2 hybridization around the central atom?
- ACO2 and CO32-
- BCO32-, NO2- and NO3-
- CCO32- and NO3-
- DNO2- and NO3-
Answer: CO32-, NO2- and NO3- - 28.
The Pauli exclusion principle states that
- Ano two electrons can have the same four quantum numbers
- Bno two electrons can occupy separate orbitals
- Cno two electrons can pair up if there is an empty orbital available
- Dno two electrons with the same spin can occupy an orbital
Answer: no two electrons can have the same four quantum numbers - 29.
An element in its ground state
- Ahas all of its electrons in the lowest possible energy levels
- Bis an element as found in nature
- Cis an element that is unreactive and found free in nature
- Dhas all of its electrons paired
Answer: has all of its electrons in the lowest possible energy levels - 30.
The name for CH3CHBrCHClCH2CH3 is
- A2,3-bromochloropentane
- Bdibromotrichloropentane
- C2-bromo, 3-chloropentane
- Ddibromotrichloropropane
Answer: 2-bromo, 3-chloropentane - 31.
A metal is reacted with HCl to produce hydrogen gas. If 0.0623 gram of metal produces 28.3 mL of hydrogen at STP, the mass of the metal that reacts with one mole of hydrochloric acid is
- A49.3 g
- B493 g
- C24.7 g
- D98.6 g
Answer: 24.7 g - 32.
Which would be the easiest way to burn a copper penny?
- AUse the method in (A), but use an oxyacetylene torch to reach a higher temperature.
- BDissolve the copper penny in acid, precipitate the hydroxide, and heat in a Bunsen burner flame to make the oxide.
- CHold the copper penny with crucible tongs, and heat strongly in the flame of a Bunsen burner.
- DGrind the copper penny into very small, dust-sized particles, and spray the particles into a Bunsen burner flame.
Answer: Grind the copper penny into very small, dust-sized particles, and spray the particles into a Bunsen burner flame. - 33.
When collecting a gas over water, it is important to
- Await until the barometer reads 760
- Bcorrect for the vapor pressure of water
- Cset the temperature at 0°C
- Dbe sure the gas does not burn
Answer: correct for the vapor pressure of water - 34.
The ideal gas law is successful for most gases because
- Avolumes are small
- Broom temperature is high
- Cgases are dimers
- Dgas particles do not interact significantly
Answer: gas particles do not interact significantly - 35.
Which net ionic equation below represents a possible reaction that takes place when a strip of magnesium metal is oxidized by a solution of chromium (III) nitrate?
- AMg(s) + Cr3+ → Mg2+ + Cr(s)
- B3Mg(s) + 2Cr(NO3)3(aq) → 3Mg2+(aq) + 2Cr(s) + NO3-(aq)
- CMg(s) + Cr(NO3)3(aq) → Mg2+(aq) + Cr3+(aq) + 3NO3-(aq)
- D3Mg(s) + 2Cr3+ → 3Mg2+ + 2Cr(s)
Answer: 3Mg(s) + 2Cr3+ → 3Mg2+ + 2Cr(s) - 36.
Which of the following is a balanced chemical reaction?
- ANa2SO4 + Ba(NO3)2 → BaSO4 + NaSO4
- B5 FeCl2 + 8 HCl + KMnO4 → 5 FeCl3 + MnCl2 + 4 H2O + KCl
- CAl(NO3)3 + 3 KOH → Al(OH)3 + KNO3
- DAgNO3 + K2CrO4 → Ag2CrO4 + 2 KNO3
Answer: 5 FeCl2 + 8 HCl + KMnO4 → 5 FeCl3 + MnCl2 + 4 H2O + KCl - 37.
What is the work involved if a gas in a 2.0-liter container at 2.4 atmospheres pressure is allowed to expand against a pressure of 0.80 atmosphere?
- A-9.62 L atm
- B-4.8 L atm
- C-3.2 L atm
- D+14.4 L atm
Answer: -3.2 L atm - 38.
Chlorine is often used to oxidize other substances. It makes a good bleach because it can oxidize many colored compounds. If chlorine is not available, what other substance can be used for oxidizing substances?
- AKMnO4
- BAl
- CZn
- DH2S
Answer: KMnO4 - 39.
Examining data obtained from mass spectrometry supports which of the following?
- AIonization energy trends within the periodic table
- BThe common oxidation states of elements
- CThe existence of isotopes
- DAtomic size trends within the periodic table
Answer: The existence of isotopes - 40.
According to the kinetic-molecular theory of gases,
- Athe average kinetic energy of a gas particle is directly related to the Kelvin temperature
- Bthe atoms or molecules of an ideal gas have no volume
- C(A), (B), and (C) are part of the theory
- Dideal gas particles do not attract or repel each other
Answer: (A), (B), and (C) are part of the theory - 41.
When the dichromate ion is reacted, one of its most common products is Cr3+. What is the oxidation state (oxidation number) of chromium in the dichromate ion? Does reduction or oxidation occur when dichromate forms Cr3+?
- A6+, reduction
- B3+, reduction
- C6+, oxidation
- D12+, reduction
Answer: 6+, reduction - 42.
Using fundamental trends in electronegativity and bond strength, which of the following should be the strongest acid?
- AHBr
- BH2S
- CH2O
- DHI
Answer: HI - 43.
From the solubility rules, which of the following is true?
- AAll ammonium-containing compounds are soluble
- BAll chlorides, bromides, and iodides are soluble
- CAll sulfates are soluble
- DAll hydroxides are soluble
Answer: All ammonium-containing compounds are soluble - 44.
The symbol for antimony is
- AFe
- BSb
- CW
- DAn
Answer: Sb - 45.
Dissolving one mole of each of the oxoacids HNO2, HClO4, H2CO3, and H3PO4 in 2.0 L of distilled water results in solutions with different pH values. Arrange these acid solutions from the one with the highest pH to the one with the lowest pH.
- AHNO2 > HClO4 > H2CO3 > H3PO4
- BHClO4 > HNO2 > H2CO3 > H3PO4
- CH2CO3 > HNO2 > HClO4 > H3PO4
- DH2CO3 > H3PO4 > HNO2 > HClO4
Answer: H2CO3 > H3PO4 > HNO2 > HClO4 - 46.
Which of the following should be named using Roman numerals after the cation?
- AAlBr3
- BCaCl2
- CCuCl2
- DK2Cr2O7
Answer: CuCl2 - 47.
Which of the following molecules is expected to have the highest normal boiling point?
- ACH3CH2CH2CH3
- BCH3CH2CH2CH2Cl
- CCH3CH2CH2CH2OH
- DCH3CH2CH2CH2Br
Answer: CH3CH2CH2CH2OH - 48.
Which of the following is considered a metalloid?
- ACr
- BS
- CMn
- DSi
Answer: Si - 49.
Which of the following pair of liquids is expected to be immiscible?
- AH2O and CH3OH
- BC10H22 and CH2CH2CH2OH
- CCH3CH2NH2 and CH3CH2CH2OH
- DC6H6 and C5H12
Answer: C10H22 and CH2CH2CH2OH - 50.
You cannot prepare a buffer by
- Amixing a solution of a strong base with a strong acid
- Bmixing a solution of a weak acid with its conjugate base
- Cmixing a solution of a weak base with a strong acid
- Dmixing a solution of a weak acid with a strong base
Answer: mixing a solution of a strong base with a strong acid
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