Which combination describes the PH 4 + ion?

Tetrahedral; sp 3 hybridization

Square Planar, sp 3 hybridization

Tetrahedral, sp 2 hybridization

Square Planar, sp 2 hybridization

Which equation represents enthalpy of hydration?

NaCl(s) → Na + (g) + Cl − (g)

NaCl(s) → Na + (aq) + Cl − (aq)

Which combination of Δ H θ and Δ S θ will result in a non-spontaneous reaction at all temperatures?

Δ H θ - Positive; Δ S θ - Negative

Δ H θ - Negative; Δ S θ - Positive

Δ H θ - Positive; Δ S θ - Positive

Δ H θ - Negative; Δ S θ - Negative

Which statement is correct for the overall reaction in a voltaic cell? 2AgNO 3 (aq) + Ni(s) → 2Ag(s) + Ni(NO 3 ) 2 (aq) E θ = +1.06 V

Ag has a more positive standard electrode potential value than Ni.

Electrons flow from Ag electrode to Ni electrode.

Ni is oxidized to Ni 2+ at the cathode (negative electrode).

Ag + is reduced to Ag at the anode (positive electrode).

Which is the first step in the CFC-catalysed destruction of ozone in UV light?

CCl 2 F 2 → •CClF 2 + Cl•

CCl 2 F 2 → CClF 2 + + Cl –

CCl 2 F 2 → CCl 2 F + + F –

CCl 2 F 2 → •CCl 2 F + F•

Which statement is correct?

Pi bonds are formed parallel to the axis between atoms.

Sigma bonds are formed only by the combination of s atomic orbitals.

Pi bonds can be formed in the absence of sigma bonds.

Pi bonds are formed only by the combination of hybrid orbitals.

Which is correct about reaction mechanisms?

Reactants in a fast step before the slow step are included in the rate expression.

A species that is zero order does not take part in the reaction.

A catalyst does not take part in the reaction.

Reactants in a fast step after the slow step are included in the rate expression.

Ammonia is a stronger ligand than water. Which is correct when concentrated aqueous ammonia solution is added to dilute aqueous copper(II) sulfate solution?

Ammonia replaces water as a ligand.

The d-orbitals in the copper ion split.

There is a smaller splitting of the d-orbitals.

The colour of the solution fades.

What is the correct explanation for the colour of [Cu(H 2 O) 6 ] 2+ ?

Light is absorbed when an electron moves to a d orbital of higher energy.

Light is released when an electron moves to a d orbital of higher energy.

Light is absorbed when electrons move from the ligands to the central metal ion.

Light is absorbed when electrons move between d and s orbitals.

Which best explains why transition metal complexes are coloured?

As electrons are promoted to higher energy levels, light of a certain colour is absorbed, and the complementary colour is observed.

As electrons return to lower energy levels, light of a certain colour is emitted, and the complementary colour is observed.

As electrons return to lower energy levels, light of a certain colour is emitted, so the complex appears to have the same colour.

As electrons are promoted to higher energy levels, light of a certain colour is absorbed, so the complex appears to have the same colour.

Which transition represents an enthalpy of hydration?

A. 2H 2 O (l) → H 3 O + (aq) + OH − (aq)

NaCl (s) → Na + (aq) + Cl − (aq)

Which mixture is a buffer solution?

50 cm 3 of 0.10 mol dm -3 NH 3 (aq) and 25 cm 3 of 0.10 mol dm -3 HCl (aq)

25 cm 3 of 0.10 mol dm -3 NH 3 (aq) and 50 cm 3 of 0.10 mol dm -3 HCl (aq)

25 cm 3 of 0.10 mol dm -3 NaOH (aq) and 25 cm 3 of 0.10 mol dm -3 HCl (aq)

50 cm 3 of 0.10 mol dm -3 NaOH (aq) and 25 cm 3 of 0.10 mol dm -3 HCl (aq)

Which statement about a first-order reaction is correct?

The reactant concentration decreases exponentially with time.

The reactant concentration decreases linearly with time.

The rate of reaction remains constant as the reaction proceeds.

The rate of reaction increases exponentially as the reaction proceeds.

Consider the rate expression: Rate = k[X][Y] Which change decreases the value of the rate constant, k?

Decrease in the reaction temperature

Increase in the reaction temperature

Increase in the concentration of X and Y

Decrease in the concentration of X and Y

Two half-cells are connected via a salt bridge to make a voltaic cell. Which statement about this cell is correct?

Ions flow through the salt bridge.

Oxidation occurs at the positive electrode (cathode).

It is also known as an electrolytic cell.

It requires a power supply to operate.

What should be changed to alter the rate of nucleophilic substitution of tertiary halogenoalkanes?

The concentration of the tertiary halogenoalkane

The concentration of the nucleophile

The first ionization energies (in kJ mol -1 ) of five successive elements in the periodic table are: 1314, 1681, 2081, 496 and 738 What could these elements be?

The last three elements of one period and the first two elements of the next period

The last two elements of one period and the first three elements of the next period

The last five elements of a period

The same quantity of electricity is passed through separate dilute aqueous solutions of sulfuric acid and copper(II) sulfate using platinum electrodes under the same conditions. Which statement is correct?

The same volume of oxygen is obtained in both cases.

The same volume of hydrogen is obtained in both cases.

The amount of copper deposited at the negative electrode in the copper(II) sulfate solution is half the amount of hydrogen gas formed at the negative electrode in the sulfuric acid solution.

The pH of both solutions increases as the electrolysis proceeds.

IB Chemistry Options

Quiz

•

Chemistry

•

University

•

Practice Problem

•

Hard

•

NGSS

HS-PS1-5, HS-PS1-4, HS-PS1-1

+6

Standards-aligned

Charles Martinez

FREE Resource

46 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Which statements are correct for ionic compounds?
I. Lattice energy increases as ionic radii increase.
II. Within the same group, the melting point of salts tends to decrease as the radius of the cation increases.
III. Solubility in water depends on the relative magnitude of the lattice energy compared to the hydration energy.

I and II only

I and III only

II and III only

What is the standard enthalpy of formation, in kJ mol^–1, of IF (g)?
IF₇ (g) + I₂ (s) → IF₅ (g) + 2IF (g) ΔH = –89 kJ
ΔH_f (IF₇) = –941 kJ mol^–1
ΔH_f (IF₅) = –840 kJ mol^–1

–190

–95

+6

+95

Which equation represents the lattice enthalpy of magnesium sulfide?

MgS (s) → Mg (g) + S (g)

MgS (s) → Mg⁺ (g) + S^– (g)

MgS (s) → Mg²⁺ (g) + S^2– (g)

MgS (s) → Mg (s) + S (s)

4.

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

The rate expression for the reaction X (g) + 2Y (g) → 3Z (g) is
rate = k[X]⁰ [Y]²
By which factor will the rate of reaction increase when the concentrations of X and Y are both increased by a factor of 3?

6

9

18

27

At 700 ºC, the equilibrium constant, K_c, for the reaction is 1.075 × 10⁸.
2H₂ (g) + S₂ (g) <- -> 2H₂S (g)
Which relationship is always correct for the equilibrium at this temperature?

[H₂S]² < [H₂]² [S₂]

S₂] = 2[H₂S]

[H₂S] < [S₂]

[H₂S]² > [H₂]²[S₂]

6.

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Which of the following will form a buffer solution if combined in appropriate molar ratios?

HCl and NaCl

NaOH and HCOONa

NH₄Cl and HCl

HCl and NH₃

7.

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

What is the product of the reaction between pentan-2-one and sodium borohydride, NaBH₄?

Pentan-1-ol

Pentan-2-ol

Pentanoic acid

Pentanal

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IB Chemistry Options

46 questions

What is the standard enthalpy of formation, in kJ mol^–1, of IF (g)?
IF₇ (g) + I₂ (s) → IF₅ (g) + 2IF (g) ΔH = –89 kJ
ΔH_f (IF₇) = –941 kJ mol^–1
ΔH_f (IF₅) = –840 kJ mol^–1

Which equation represents the lattice enthalpy of magnesium sulfide?

The rate expression for the reaction X (g) + 2Y (g) → 3Z (g) is
rate = k[X]⁰ [Y]²
By which factor will the rate of reaction increase when the concentrations of X and Y are both increased by a factor of 3?

At 700 ºC, the equilibrium constant, K_c, for the reaction is 1.075 × 10⁸.
2H₂ (g) + S₂ (g) <- -> 2H₂S (g)
Which relationship is always correct for the equilibrium at this temperature?

Which of the following will form a buffer solution if combined in appropriate molar ratios?

What is the product of the reaction between pentan-2-one and sodium borohydride, NaBH₄?

Which combination describes the PH₄⁺ ion?

Which species have resonance structures?
I. Ozone, O₃
II. Carbon dioxide, CO₂
III. Benzene, C₆H₆

Which equation represents enthalpy of hydration?

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IB Chemistry Options

46 questions

What is the standard enthalpy of formation, in kJ mol–1, of IF (g)?IF7 (g) + I2 (s) → IF5 (g) + 2IF (g) ΔH = –89 kJΔHf (IF7) = –941 kJ mol–1ΔHf (IF5) = –840 kJ mol–1

Which equation represents the lattice enthalpy of magnesium sulfide?

The rate expression for the reaction X (g) + 2Y (g) → 3Z (g) is rate = k[X]0 [Y]2By which factor will the rate of reaction increase when the concentrations of X and Y are both increased by a factor of 3?

At 700 ºC, the equilibrium constant, Kc, for the reaction is 1.075 × 108.2H2 (g) + S2 (g) <- -> 2H2S (g)Which relationship is always correct for the equilibrium at this temperature?

Which of the following will form a buffer solution if combined in appropriate molar ratios?

What is the product of the reaction between pentan-2-one and sodium borohydride, NaBH4?

Which combination describes the PH4+ ion?

Which species have resonance structures?I. Ozone, O3II. Carbon dioxide, CO2III. Benzene, C6H6

Which equation represents enthalpy of hydration?

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Similar Resources on Wayground

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Discover more resources for Chemistry

What is the standard enthalpy of formation, in kJ mol^–1, of IF (g)?
IF₇ (g) + I₂ (s) → IF₅ (g) + 2IF (g) ΔH = –89 kJ
ΔH_f (IF₇) = –941 kJ mol^–1
ΔH_f (IF₅) = –840 kJ mol^–1

The rate expression for the reaction X (g) + 2Y (g) → 3Z (g) is
rate = k[X]⁰ [Y]²
By which factor will the rate of reaction increase when the concentrations of X and Y are both increased by a factor of 3?

At 700 ºC, the equilibrium constant, K_c, for the reaction is 1.075 × 10⁸.
2H₂ (g) + S₂ (g) <- -> 2H₂S (g)
Which relationship is always correct for the equilibrium at this temperature?

What is the product of the reaction between pentan-2-one and sodium borohydride, NaBH₄?

Which combination describes the PH₄⁺ ion?

Which species have resonance structures?
I. Ozone, O₃
II. Carbon dioxide, CO₂
III. Benzene, C₆H₆