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chem 20 > Unit 2: Matter as Solutions (PART A) > Flashcards

Unit 2: Matter as Solutions (PART A) Flashcards

topic 1-6 - solutions and mixtures - dissociation, ionization, dissolving - net ionic equations - energy changes/solubility - saturation

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1
Q

matter

A
  • anything that has mass/volume (ex. solids, liquids, gases)
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2
Q

pure substance

A
  • matter that has a definite composition (ex. elements, compounds)
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3
Q

element

A
  • can’t be chemically broken down into simpler substances (ex. gold, hydrogen)
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4
Q

compound

A
  • 2+ elements that are chemically combined and can be broken down into simpler substances (ex. water, salt)
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5
Q

mixture

A
  • combinations of matter that can be separated physically and don’t have a definite composition (ex. salt water)
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5
Q

homogeneous

A
  • (solution) components are not visible
  • composition looks the same (ex. sugar water)
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6
Q

heterogeneous

A
  • (mechanical mixture) components are visible
  • composition looks different (ex. oil and water)
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7
Q

solvent

A
  • usually a liquid
  • a substance that a solute is dissolved to form a solution (ex. sugar water = water)
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8
Q

solute

A
  • a substance that’s dissolved in a solvent (ex. sugar water = sugar)
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9
Q

alloy

A
  • a solid solution of metals (bronze = copper + tin)
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10
Q

amalgam

A
  • solutions of mercury in other metals
  • liquid in a solid
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11
Q

colloid

A
  • a heterogeneous mixture that looks like a solution
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12
Q

non-electrolyte

A
  • substances that don’t conduct electric current when dissolved in water (ex. glucose)
  • conductivity probe = no dissolved ions
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13
Q

electrolyte

A
  • substances that do conduct an electric current when dissolved in water (ex. salt)
  • conductivity probe = dissolved ions
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14
Q

acidic

A
  • a solution with a pH < 7
  • blue litmus = red; red litmus = red
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15
Q

basic

A
  • a solution with a pH > 7
  • red litmus = blue; blue litmus = blue
16
Q

neutral

A
  • a solution with a pH = 7
  • red litmus = red; blue litmus = blue
17
Q

solvation

A
  • when a solution is formed, the solvent pulls solute particles apart and surrounds them (or solvates)
17
Q

dissociation

A
  • when an ionic compound dissolves in water, existing ions separate
18
Q

ionization

A
  • when a molecular compound dissolves in water, new ions form
  • specifically hydrogen ions
19
Q

dissolving

A
  • when a compound separates from each other in a solution
  • only a state change
20
Q

solubility

A
  • the concentration of a saturated solution at a specified temperature
21
Q

miscibility

A
  • the ability of two or more substances to mix completely with each other in the same phase, usually liquids or gases
22
Q

insoluble ionic compounds

A
  • don’t dissociate in water to a full extent and the compound remains intact overall
23
Q

soluble ionic compounds

A
  • dissociate in water to produce ions in water
24
Q

Arrhenius Theory

A

acids: a molecular compound that ionizes in water to produce hydrogen ions (ex. HCl)
bases: an ionic compound that dissociates in water to produce hydroxide ions (ex. NAOH)

25
Q

insoluble molecular compounds

A
  • molecules don’t separate
  • no state change
26
Q

soluble molecular compounds

A
  • molecules separate (aq)
  • ONLY state change
27
Q

endothermic

A
  • absorbs more energy than released
  • higher enthalpy of chemical system
  • temperature decrease
28
Q

exothermic

A
  • releases more energy than absorbed
  • lower enthalpy of chemical system
  • temperature increase
29
Q

saturated solution

A
  • a solution that contains that max. amount of dissolved solute at a given temperature than undissolved solute
30
Q

unsaturated solution

A
  • a solution that’s not saturated and can dissolve more solute at given temperature
31
Q

supersaturated solution

A
  • a solution that contains more dissolvled solute than its solubility at a given temperature
  • when disturbed by seed crystal –> becomes saturated and excess solute precipitates

chem 20 (4 decks)

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