Choose the compound below that should has the largest lattice energy.

Which of the following compounds illustrates sp³ hybridization?

What is the correct electron configuration of the potassium cation?

Which of the following molecules have a trigonal bipyramidal geometry?

BrF₅ SF₄ PCl₅

In assembling a Lewis Dot diagram of diagram of CF₂Cl₂ , there are ____ total electrons to use in the model.

What is the net ionic equation for the reaction between aqueous sodium hydroxide (NaOH)

and aqueous nitric acid (HNO₃)?

Determine the initial volume needed to generate 2.50 L of 1.50 M HNO₃from 2.50 M HNO₃ by dilution

9.

Determine the simplest formula of the compound which has the composition 51.4 % C, 8.6 %

H, and 40.0 % N by mass

Which of the following compounds is soluble in water?

In the calibration of a calorimeter, an electrical resistance heater supplies 100.0 J of heat and

a temperature increase of 0.850°C is observed. Then, 0.214 g of a particular fuel is burned in

this same calorimeter and the temperature increases by 4.23°C. Calculate the energy density

of this fuel, which is the amount of energy liberated per gram of fuel burned.

Explain why the following is not a formation reaction.

4Na(s) + O₂(g)→2Na₂O(s)

Calculate ΔE for the system in which 16 J of work is done on a gas by the surroundings and

the gas releases 51 J of heat?

For the reaction, how much energy is needed to generate 20 moles of NO(g)?

N₂(g)+O₂ (g) →2 NO(g) ∆H = 180.5 kJ

Using these two equations,

C _(graphite) + PbO_(s) → Pb(s) + CO(g) ∆H°= 106.8 kJ

2C_(graphite) + O₂(g) →2CO(g) ∆H°= -221.0 kJ

find the standard enthalpy change for the formation of 1 mol PbO(s) from lead metal and oxygen gas.

Pb(s) + ½ O₂ (g) → PbO ∆H°= ?

A particular orbital has n = 3 and l = 1. What must this orbital be?

Write the ground state electron configuration for titanium

How many valence electrons are in gallium?

Which of the following represents invalid set of quantum numbers?

Hund's rule states that the most stable arrangement of electrons (for a ground state electron configuration)

If a hydrogen atom undergoes a transition from n = 1 (E = 4.17 × 10^-19J) to n = 3 (E = 8.62 × 10^-19J), what is the wavelength of the photo absorbed?

In the first 10.0 s of the reaction, the concentration of B decreased from 0.50 M to 0.35 M.

What is the rate of the reaction in this time interval?

In the first 10.0 s of the reaction, the concentration of B decreased from 0.50 M to 0.35 M.

2A + 3B → 2C + D

If the initial concentration of the reactant in a first-order reaction A → products is 0.64 mol/L

and the half-life is 30.0 s, how long would it take for the concentration of the reactant to drop

to 0.020 mol/L?

Consider the elementary step: 2A → C. What type of elementary step is this?

If a reaction is first order with respect to [B], tripling the concentration of [B] will result in:

The decomposition of N₂O₅ in solution of carbon tetrachloride is a first-order reaction:

2 N₂O₅ → 4 NO₂ + O₂

The rate constant at a given temperature is found to be 5.25 × 10^-4s^-1 . If the initial

concentration of N₂O₅ is 0.200 M, what is its concentration after exactly 5 minutes have passed?

Consider the reaction: 2A + B → C, and a kinetics study on this reaction yielded:

[A] mol·L ^-1 [B] mol·L ^-1 Rate = mol·L^-1·s^-1

0.100 0.200 5.03 × 10^-3

0.050 0.200 1.27 × 10^-3

0.050 0.100 1.25 × 10^-3

What is the value of the rate constant?

Which of the following relationships are true for gases?

i) The volume of a gas is directly proportional to its pressure (at constant temperature).

ii) The pressure of a gas is inversely proportional to its temperature in kelvins (at constant volume).

iii) The number of moles of a gas is directly proportional to its volume (at constant pressure and temperature)

A mixture of He and O₂ is placed in a 4.00 L flask at 32° C. The partial pressure of the He is

3.0 atm and the partial pressure of the O₂

is 2.0 atm. What is the mole fraction of O₂ ?

At constant temperature, 14.0 L of O

at 2.70 atm is compressed to 1.75 L. What is the final pressure of O₂?

What volume of O₂, measured at 91.2 °C and 743 mm Hg, will be produced by the decomposition of 3.25 g KClO₃ ? (R = 0.08206 L·atm/mol·K)

2 KClO₃ (s) → 2 KCl(s) + 3 O₂ (g)

Which of the followings are not generally true of gases?

32.

1) Gas particles do not collide with each other.

2) Gases expand to fill the volume of a container.

3) Gases have lower densities than solids or liquids.

4) Lighter gas particles tend to move faster at the same temperature.

5) At a fixed temperature, as pressure increases, average speed increases.

The ideal gas law begins to break down:

1) at high temperatures

2) at low temperatures

3) at high pressures

4) at low pressures

5) at low volume

Which of the following represent(s) a chemical change?

1)rusting of an iron bridge.

2)melting of ice.

3)burning of a wooden stick.

4)boiling of water.

5)dissolving of sugar in water.

Which of the following properties of a metal are chemical properties?

1) It is hard

2)It rusts in air

3)Its density is 5.5 g/cm

4)It reacts with a base

5)It is a good electrical conductor

Assuming the numbers given are measurements, carry out the indicated arithmetic operation

and give the answer with the correct number of significant figures.

2.36 × 10 + 5.4 × 10³

Oxygen boils at −297.3 °F. What is this temperature in Kelvin?

Without doing a calculation, predict which of the following shows a decrease in entropy?

The sign of ∆H_rxn and ∆S_rxn for several reactions are given. In which case is the reaction nonspontaneous at all temperatures?

Select the correct statement that corresponds to the second law of thermodynamics.

When magnesium sulfite decomposes, the solid transforms into magnesium oxide and sulfur dioxide.

MgSO₃ (s) → MgO(s) + SO₂ (g)

At what temperature will this reaction be spontaneous according to Gibb's Energy?

ΔG_f°in kJ/mol for: MgSO₃ (s) = −1172, MgO(s) = −569.6, SO₂(g) = −300.2

ΔH_f° in kJ/mol for: MgSO₃ (s) = −1068, MgO(s) = −601.8, SO₂(g) = −296.8

S° in J/mol K for: MgSO₃ (s) = 121, MgO(s) = 27, SO₂ (g) = 248.1

If a 5.0 L flask holds 0.125 moles of nitrogen at STP, what happens to the entropy of the

system upon heating the gas to 75 °C?

The randomness of a system may be described as its:

How many protons, neutrons, and electrons are in the

14 C atom?

Give the name of the following compound: N₂O₃

An element has two naturally occurring isotopes with the following masses and natural

abundances:

Isotope Mass (amu) Abundances (%)

W 68.9257 60.12

X 70.9249 39.88

What is the identity of the element above?

The correct formula for iron(II) chloride is:

Alkaline earth metal cations carry a charge of what?

Choose the substance that corresponds to an n-type semiconductor

What's the packing efficiency of the body-centered cubic structure?

The isotopes of carbon are

Which type(s) of intermolecular forces need to be overcome to convert acetone [(CH₃)₂CO]

from liquids to gases?

i. dispersion;

ii. dipole-dipole;

iii) H-bonding

Predict the order of vapor pressure for the following compounds.

i. FCH₂ CH₂F;

ii. FCH ₂ CH₂OH;

iii) HOCH₂CH₂OH

Which of the following substances represents an excellent conductor of electricity?

A mixture of 10.0 g of NO and 14.0 g of NO₂ results in the production of 8.52 g of N₂O_3.

What is the percentage yield?

NO(g) + NO₂(g) → N₂O₃(l)

A 20.00 mL sample of nitric acid, HNO₃ , requires 0.432 g of barium hydroxide, Ba(OH)

for titration to the equivalence point. What is the concentration of the nitric acid?

2 HNO₃ (aq) + Ba(OH)₂(aq) → Ba(NO₃)(aq) + 2 H₂O(l)

The combustion of methane (CH₄) produces carbon dioxide (CO₂) and steam (H₂O).

All of the following statements concerning this reaction are correct EXCEPT

When Al(OH) ₃ reacts with sulfuric acid, the following reaction occurs:

2 Al(OH)₃ + 3 H₂SO₄ → Al₂(SO₄) + 6 H₂O

If 0.45 × 10³g of Al(OH)₃ is combined with 880 g of H₂SO₄, how much aluminum sulfate can form?