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Chemistry > Oceans > Flashcards

Oceans Flashcards

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1
Q

What happens when a solute dissolves?

A

The solute and solvent bonds break, and new bonds are formed.

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2
Q

What determines if a substance dissolves in a solvent?

A

If the new bonds are weaker than the broken bonds, the substance won’t dissolve.

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3
Q

What are the types of solvents?

A

Polar (e.g., water) and non-polar (e.g., hexane).

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4
Q

Why do ionic substances dissolve in polar solvents?

A

The positive and negative ions form ion-dipole bonds with the solvent’s dipoles, breaking the ionic lattice.

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5
Q

What is solvation?

A

The process of ions being surrounded by solvent molecules.

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6
Q

What is hydration?

A

Solvation when the solvent is water.

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7
Q

Why do covalent substances dissolve in non-polar solvents?

A

Both have weak instantaneous dipole—induced dipole bonds, making them compatible.

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8
Q

Why don’t most covalent substances dissolve in polar solvents?

A

Hydrogen bonds in polar solvents (e.g., water) are stronger than the bonds formed with covalent substances.

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9
Q

What is lattice enthalpy (ΔLEHo)?

A

The enthalpy change when 1 mole of an ionic lattice forms from gaseous ions, always negative (exothermic).

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10
Q

What is hydration enthalpy (ΔhydHo)?

A

The enthalpy change when 1 mole of gaseous ions dissolve in water to form aqueous ions, always negative (exothermic).

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11
Q

What is the enthalpy change of solution (ΔsolHo)?

A

The enthalpy change when 1 mole of an ionic substance dissolves in enough solvent to form an infinite dilution.

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12
Q

How can the enthalpy change of solution be calculated?

A

Using a Hess cycle: ΔsolHo = −(lattice enthalpy) + sum of hydration enthalpies.

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13
Q

What factors affect lattice enthalpy?

A

Higher charge density increases electrostatic attraction, making lattice enthalpy more exothermic.

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14
Q

What factors affect hydration enthalpy?

A

Higher charge density makes water more attracted to ions, making hydration enthalpy more exothermic.

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15
Q

What is entropy (S)?

A

A measure of the number of possible arrangements of particles and energy quanta in a system.

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16
Q

What factors increase entropy?

A

Gases and liquids have higher entropy than solids, and higher energy or larger amounts of substances increase entropy.

17
Q

How is total entropy change calculated?

A

ΔtotS = ΔsysS + ΔsurrS, where ΔsysS = Sproducts − Sreactants, and ΔsurrS = −ΔH/T.

18
Q

What determines reaction feasibility?

A

A positive ΔtotS indicates feasibility, while a negative ΔtotS means the reaction isn’t feasible.

19
Q

What is the solubility product (Ksp)?

A

The equilibrium constant for the dissociation of a sparingly soluble salt into its ions in a saturated solution.

20
Q

How can a solubility product be determined experimentally?

A

Prepare a saturated solution, measure ion concentration using titration or colorimetry, and calculate Ksp.

21
Q

What is the Brønsted-Lowry definition of acids and bases?

A

Acids are proton donors (release H+), and bases are proton acceptors.

22
Q

What are conjugate acid-base pairs?

A

Pairs like HCl and Cl−, where one species donates or accepts a proton.

23
Q

What are strong acids?

A

Acids that completely dissociate in water, e.g., HCl.

24
Q

What are strong bases?

A

Bases that completely dissociate in water to form OH− ions.

25
Q

What are weak acids?

A

Acids that only slightly dissociate in water, forming few H+ ions, e.g., CH3COOH.

26
Q

How is Ka used for weak acids?

A

Ka = [H+]^2 / [HA], where [HA] is the concentration of the weak acid.

27
Q

How is pKa calculated?

A

pKa = −log10Ka, and a smaller pKa indicates a stronger acid.

28
Q

What is pH?

A

A measure of H+ concentration: pH = −log10[H+].

29
Q

What is Kw

A

and how is it used?

30
Q

What is a buffer solution?

A

A solution that resists pH changes when small amounts of acid or base are added.

31
Q

How do acidic buffers work?

A

Made of a weak acid and its salt, they adjust equilibrium to resist pH changes when H+ or OH− is added.

32
Q

What is the greenhouse effect?

A

Greenhouse gases absorb and re-emit IR radiation, trapping heat in the atmosphere.

33
Q

What causes the enhanced greenhouse effect?

A

Increased greenhouse gases due to human activity, intensifying heat retention.

34
Q

How do greenhouse gases trap heat?

A

They absorb IR, causing bond vibrations that transfer energy to other gas molecules, raising temperature.

Chemistry (8 decks)

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