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 . . . .
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Most Common Ions (40)
Aluminum will lose ___ electrons to form its most common ion.
Oxygen will gain ___ electrons to form its most common ion.
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Ion / Charge (200)
The CrO4 ion has a ___ charge.
The chromate ion has a ___ charge.
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Naming Ions (60)
Fill-in-the-blank
Chromate is . . .
Sulfite is . . .
Nitrate is . . .
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Naming Ions (60)
Fill-in-the-blank
ClO4- is . . .
NH4+ is . . .
C2H3O2- is . . .
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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 . . .
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Gas Evolved (25)
Na2S + H+
NaHCO3 + HCl
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Precipitate Formed (15)
AgNO3 + NaCl →
FeCl3 + LiOH →
Pb(C2H3O2)2 + KClO4 →
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Stoichiometry (50)
Click the Play button to animate the stoichiometric process.
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Atoms in Formula (30)
3 Co(C2H3O2)2 contains __ 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
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Activity Series (40)
Select the least active metal.
Sodium is more active than Zinc. True / False
The reaction Ca2+ + Cu° →
will / will not occur.
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Reaction Type (15)
2Li + F2 → 2LiF
AgNO3 (aq) + NaCl(aq) → AgCl(s) + NaNO3 (aq)
2H2O → 2H2 + O2
2AgNO3 + Mg° → Mg(NO3)2 + 2Ag°
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Oxidation Numbers (50) The oxidation number of Mn in MnO4- is . . .
The
oxidation number of Gold metal is . . .
The oxidation number of Cl- is . . .
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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
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Electronic Structure (90)
Group 3 elements have __ unpaired electrons.
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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 . . . .
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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.
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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 -
← and ↓ | → and ↑
Metals tend to have large / small ionization energies.
Anions are larger / smaller than the parent atom.
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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
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Formal Charges (40)
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Geometry (130)
A ______ molecular geometry has bond angles of 109.5°.
The flashing bond is a(n) π / σ / ω bond.
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Geometry (con't)
In the actual H2O molecule, the angle between the two bonding electron pairs (Blue Angle) is . . .
> 109.5° | < 109.5° | 109.5°
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Geometry (con't)
Molecules with T-shaped geometries have __ bonding domains.
The central atom in the molecule below is ____ hybridized.
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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.
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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.
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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, m is 0.10 m / 0.20 m / 0.30 m / 0.40 m . |
Colligative Properties (con't)
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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
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Kinetics (con't)
A + A → products
is a Uni- / Bi- / Ter- molecular reaction.
zero / first / second / third order in B.

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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
The reaction below is proceeding toward equilibrium.

? = x / 2x / -x / -2x
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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 . . .
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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
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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.
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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
CaCO3 (s) ⇌ Ca2+ (aq)
+ CO32- (aq)
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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 .
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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.
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Electrochemistry (130)
Oxidation occurs at the anode / cathode .
Oxidation is the
loss / gain of electrons.
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