Sample TRQ Questions (General Chemistry)
There are more than 4000 General Chemistry TRQ questions . . .
the number in parentheses denotes the number of TRQ questions in each category.

Conversion Factors (100)
1 Å = _____ m

Symbol → Name(118)
The element with the symbol Ag is . . .

Name → Symbol (118)
The symbol for Astatine is . . .

Significant Figures (50)
0.0120 contains _____ significant figures.

Prefixes (40)
The prefix atto is . . . .

Numbers / Measurements / Units (40)
Which is larger . . .  0.000123 / 0.00123 / 1.23E-5 

Density has units of . . . .

Atoms (100)
An atom with 13 protons and 11 electrons has a ___ charge.

An anion has more protons than electrons.  True / False 

Naming Acids (20)
H2SO3 is . . .

H2CO3 is . . .

Naming Molecular Compounds (50)
P4S10 is . . . .

CO is . . . .

Most Common Ions (40)
Aluminum will lose ___ electrons to form its most common ion.

Magnesium will gain ___ electrons to form its most common ion.

Ion / Charge (200)
The CrO4 ion has a ___ charge.

The chromate ion has a ___ charge.

Naming Ions (60)
Fill-in-the-blank
Chromate is . . .

Sulfite is . . .

Nitrate is . . .

Naming Ions (60)
Fill-in-the-blank
ClO4-  is . . .

NH4+  is . . .

C2H3O2- is . . .

Naming Ionic Compounds (315)
Fill-in-the-blank

Name → Formula

Aluminum perchlorate is . . .

Iron(III) carbonate is . . .

Naming Ionic Compounds (315)
Fill-in-the-blank

Formula → Name

Hg2Cl2 is . . .

Ni(ClO3)2 is . . .

Gas Evolved (25)
Na2S + H+

NaHCO3 + HCl

Precipitate Formed (15)
AgNO3 + NaCl →

FeCl3 + LiOH →

Pb(C2H3O2)2 + KClO4

Stoichiometry (50)
Click the Play button to animate the stoichiometric process.

Atoms in Formula (30)
3 Co(C2H3O2)2contains __ Oxygen atoms.

CuSO4•5H2O contains __ Oxygen atoms.

Electrolytes (30)
Which of the following is a strong electrolyte?
 H2O / NaCl / HC2H3O2 

Which of the following is a non-electrolyte?
 C6H12O6 / NaCl / HC2H3O2 

Activity Series (40)
Select the least active metal.

Sodium is more active than Zinc. True / False 

The reaction Ca2+ + Cu° →
 will / will not  occur.

Reaction Type (15)
2Li + F2 → 2LiF

AgNO3 + NaCl →

Oxidation Numbers (50)
The oxidation number of Mn in MnO4- is . . .

The oxidation number of Gold metal is . . .

The oxidation number of Cl- is . . .

Solubility Rules (310)
Zinc(II) hydroxide is
 soluble / insoluble .

The insoluble hydroxide is
 Fe3+ / Na+ / NH4+  

Thermochemistry (130)
The 1st Law of Thermodynamics states . . .

-
ΔH is
 Endothermic / Exothermic 

ΔHf O(g) is  0 / not 0 

Gas → Liquid, Entropy will
  / /stay the same 

Electronic Structure (90)
Group 3 elements have __ unpaired electrons.

Valence Electrons (20)
Oxygen (1s22s22p4) has ___ valence electrons.

Oxygen (1s22s22p4) has ___ unpaired electrons.

Quantum Numbers (50)
For l = 3 there are
__ possible ml values.

The l quantum number of an f subshell is . . .

n = 2, l = 0 specifies the __ orbital.

Aufbau Principle (10)
The subshell just below the 5d is . . .

Electromagnetic Radiation (20)



Highest energy . . .
 Blue light / Yellow light 

Longest wavelength . . .
 Radio waves / microwaves 

Periodic Table (80)
Inner transition metals are located at the  Top / Bottom / Right / Left  of the Periodic Table.

Periodic Table (con't)
Na+ and Ar are isoelectronic.
 True / False 

An allotrope of O3 is . . .  O / O2 / O4 / Ne 

Periodic trend for increasing atomic radii . . .

Metals tend to have  large / small  ionization energies.

Anions are  larger / smaller  than the parent atom.

Bonding (50)
Ionic bonding occurs between . . .

A double bond is  stronger / weaker  than a single bond.

The octet rule states that atoms . . .

The bonds in CaCl2 are  ionic / covalent / polar .

Resonance structures are . . .
 imaginary | real 

Formal Charges (40)

Geometry (130)
A ______ molecular geometry has bond angles of 109.5°.

The flashing bond is a(n)  π / σ / ω  bond.

Geometry (con't)
In the actual H2O molecule, the angle between the two bonding electron pairs (Green Angle) is . . .
 > 109.5° | < 109.5° | 109.5° 

Geometry (con't)
Molecules with T-shaped geometries have __ bonding domains.

The central atom in the molecule below is ____ hybridized.

Geometry (con't)
The direction of the dipole moment in the molecule shown is . . .
← | → | |


A molecule with square planar geometry has a central atom that is ____ hybridized.

Gases (120)
The units for P in PV=nRT when R is 0.08206 . . .

An increase in P will cause V to  increase / decrease .

Is H2O a gas at standard conditions?

A gas becomes "more ideal" at  low / high  pressures.

Gases (con't)
In the manometer below the gas pressure is  greater / less  than atmospheric pressure.

Intermolecular Forces (120)
Large intermolecular forces cause a substance to have  high / low  vapor pressure.

Sublimation . . .  endothermic / exothermic 

A liquid's vapor pressure increases as the temperature  increases / decreases .

In osmosis, the  solvent / solute  move across the semi-permeable membrane.

Solutions (50)
C6H12 will best dissolve in  C8H14 / H2O / Hg(l).

An -O- or _OH group causes that part of the molecule to be hydro  philic / phobic .

Liquids that do not dissolve significantly in one another are  miscible / immiscible / hydrophobic .

The ΔS during the solution of a solid in a liquid is  positive / negative / zero .

Colligative Properties (50)
ΔTf =  KbM / KbXsolute / Kbm 

The presence of ion pairs in a solution will cause a  lower / higher  boiling point elevation than expected.

For an aqueous 0.10 m Calcium nitrate solution, the molality used in the
ΔTb = Kbm equation is  0.10 m / 0.20 m / 0.30 m / 0.40 m .

Colligative Properties (con't)

Kinetics (125)
10.0 g Sr-90 will decay leaving 5.00 g Sr-90 after  1 / 2 / 3 / 4  half-lives.

C is  Reactant / Transition State / Intermediate / Ea 

Kinetics (con't)
A + A → products
is a  Uni- / Bi- / Ter-   molecular reaction.

This reaction is  zero / first / second / third   order in B.

Chemical Equilibrium (125)
If N2 (g) + O2 (g) ⇌ 2NO(g) is at equilibrium, increasing N2 will cause O2 to  increase / decrease / stay the same .

A catalyst shifts the equilibrium to the right.  True / False 

Is Kc = Kp for CO2 (g) ⇌ C(s) + O2 (g)
 Yes / No / Unable to determine .

In osmosis, the  solvent / solute  move across the semi-permeable membrane.

Chemical Equilibrium (con't)
In the reaction below,
Keq =  3 / 6 / 18 / 36 

In the reaction above,
Q =  1 / 2 / 4 / 8 

What is "?" if the reaction is proceeding toward equilibrium?
? =  x / 2x / -x / -2x 

Identifying Acids / Bases (50)

 Strong acid / Weak acid /
Strong base / Weak base /
Neutral Compound
 

HC2H3O2 is a . . .
NH4Cl is a . . .
HCl is a . . .
NaCN is a . . .
NaH is a . . .
NaBr is a . . .
Na2O is a . . .
NH3 is a . . .
HClO is a . . .

Acid / Base Equilibria (140)
pOH = log[OH-]  True / False 

pH = 4
 acidic / basic / neutral 

CN- + H2O ⇌ HCN +         

A student mixes 10.0 mL 1.0M HCl
and 20 mL water
The new concentration of HCl is
 3.0M / 1.50M / 0.50M / 0.33M 

The pH of a solution whose
[OH-] = 1 × 10-5 M
 5 / -5 / 9 / -9 

Acid / Base Equilibria (con't)
What is the conjugate base of H2PO4-?

Cl-  does / does not  react with water.

The pH  increases / decreases / does not change  when ClO- is added to water.

The pH  increases / decreases / does not change  when Al3+ is added to water.

Aqueous Equilibrium (100)
NaOH is added to a HC2H3O2 / C2H3O2- buffer. The [HC2H3O2] will  increase / decrease / stay the same .

Which buffer has the largest [H+]?
 Buffer 1: : 1 M in both HF and NaF
 Buffer 2: : 0.1 M in both HF and NaF

Environmental Chemistry (100)
N2 + hv → 2 N is
 photodissociation / photoionization 

Carboxyhemoglobin is formed when
 CO(g) / CO2 (g) / CO32-(aq)  binds to hemoglobin.

Absorbs ultraviolet radiation . . .
 troposphere / mesosphere / stratosphere / thermosphere .

Thermodynamics (60)
A "+ΔS" indicates that the system has become more  ordered / disordered 

A spontaneous reaction has a  positive / negative  ΔG.

The standard molar free energies, ΔG, of elements at 298 K  is / is not  zero.

ΔG = ΔH  + / -  TΔS.

Electrochemistry (130)
Oxidation occurs at the anode / cathode .

Oxidation is the  loss / gain  of electrons.