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Chem unit 4 > Unit 1 > Flashcards

Unit 1 Flashcards

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1
Q

What is one of the most important substances on Earth?

A

Water

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2
Q

What is a key property of water that makes it a common solvent?

A

Can dissolve many different substances

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3
Q

What type of molecule is water due to its unequal charge distribution?

A

Polar molecule

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4
Q

What is a solute?

A

Substance being dissolved in a solution.

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5
Q

What is a solvent?

A

Liquid water that dissolves the solute.

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6
Q

What is an electrolyte?

A

Substance that can conduct electricity when dissolved in water.

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7
Q

Define strong electrolytes.

A

Electrolytes that are completely ionized in water and conduct current very efficiently.

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8
Q

What characterizes weak electrolytes?

A

They conduct only a small current due to a small degree of ionization in water.

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9
Q

What are nonelectrolytes?

A

Substances that dissolve in water but do not produce any ions, resulting in no electrical conductivity.

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10
Q

Fill in the blank: A substance that comes apart to form ions is said to _______.

A

ionize

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11
Q

True or False: Strong electrolytes produce no ions in solution.

A

False

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12
Q

What happens to insoluble substances in water?

A

They require too much energy to break apart.

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13
Q

What happens to a light bulb when a strong electrolyte is dissolved in water?

A

The bulb shines brightly.

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14
Q

What happens to a light bulb when a weak electrolyte is dissolved in water?

A

The bulb glows dimly.

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15
Q

What happens to a light bulb when a nonelectrolyte is dissolved in water?

A

The bulb remains unlit.

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16
Q

What is essential to know about chemical reactions of solutions?

A

The nature of the reaction, the amounts of chemicals present in the solutions, concentration, and molarity.

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17
Q

Define molarity.

A

Molarity = moles of solute / liters of solution.

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18
Q

Fill in the blank: Molarity is calculated by dividing _______ by liters of solution.

A

moles of solute

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19
Q

True or False: Concentration is not important in the context of chemical reactions of solutions.

A

False

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20
Q

What does molarity measure in a solution?

A

The concentration of solute in moles per liter.

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21
Q

List the key factors we must know for chemical reactions of solutions.

A
  • The nature of the reaction
  • The amounts of chemicals present in the solutions
  • Concentration
  • Molarity
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22
Q

What is the dissociation equation for the compound CaCl2 in solution?

A

CaCl2 → Ca2+ + 2Cl-

This equation shows how calcium chloride dissociates into calcium ions and chloride ions in solution.

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23
Q

What is the concentration of Ca2+ ions in a 0.25 M CaCl2 solution?

A

0.25 M

The concentration of Ca2+ ions is equal to the concentration of the CaCl2 solution since each formula unit produces one Ca2+ ion.

24
Q

What is the concentration of Cl- ions in a 0.25 M CaCl2 solution?

A

0.50 M

Each formula unit of CaCl2 produces two Cl- ions, resulting in a concentration that is double that of CaCl2.

25
Q

What is the definition of dilution?

A

The process of adding water to a concentrated solution to achieve the desired molarity

Dilution is commonly used in laboratories to prepare solutions of lower concentrations.

26
Q

Does dilution with water alter the number of moles of solute present?

A

No

The number of moles remains constant before and after dilution.

27
Q

What is the relationship between moles of solute before and after dilution?

A

Moles of solute before dilution = moles of solute after dilution

This principle is fundamental to the concept of dilution in chemistry.

28
Q

What is the dilution equation?

A

M1V1 = M2V2

M1 and V1 refer to the molarity and volume of the concentrated solution, while M2 and V2 refer to the molarity and volume of the diluted solution.

29
Q

Fill in the blank: The concentration of Ca2+ ions in a 0.25 M CaCl2 solution is _______.

A

0.25 M

This reflects the stoichiometry of the dissociation of CaCl2.

30
Q

Fill in the blank: The concentration of Cl- ions in a 0.25 M CaCl2 solution is _______.

A

0.50 M

This is because each mole of CaCl2 yields two moles of Cl- ions.

31
Q

What is a Precipitation Reaction?

A

A double displacement reaction in which a solid forms and separates from the solution.

This occurs when ionic compounds dissolve in water, leading to the formation of precipitate.

32
Q

What is the solid that forms in a Precipitation Reaction called?

A

Precipitate

The precipitate is the solid that separates from the solution during the reaction.

33
Q

What are the three main types of chemical reactions?

A
  • Precipitation Reactions
  • Acid-Base Reactions
  • Oxidation-Reduction Reactions

These types categorize chemical reactions based on the processes that occur during them.

34
Q

What is a precipitate?

A

A solid that forms from a solution.

35
Q

What does soluble mean?

A

Dissolves in solution; indicated by (aq) in reaction equations.

36
Q

What does insoluble mean?

A

Does not dissolve in solution; indicated by (s) in reaction equations.

37
Q

True or False: Insoluble and slightly soluble are often used interchangeably.

A

True.

38
Q

Fill in the blank: Soluble substances are typically associated with _______ in reaction equations.

A

(aq)

39
Q

Fill in the blank: Insoluble substances are typically associated with _______ in reaction equations.

A

(s)

40
Q

What are the solubility rules for alkali metals?

A

Alkali metals are soluble.

41
Q

What is the difference between soluble and insoluble substances?

A

Soluble substances dissolve in solution, while insoluble substances do not.

42
Q

What is a Formula Equation?

A

A representation of a chemical reaction showing reactants and products as compounds

43
Q

What is a Molecular Equation?

A

An equation that shows the complete formulas of the reactants and products

44
Q

What do solubility rules help determine?

A

Which compounds are aqueous and which are solids

45
Q

Given the reaction AgNO3(aq) + NaCl(aq) → ?, what is the product?

A

AgCl(s) + NaNO3(aq)

46
Q

What is a Complete Ionic Equation?

A

An equation where all strong electrolytes are represented as ions

47
Q

In the Complete Ionic Equation for the reaction AgNO3(aq) + NaCl(aq), what are the reactants in ionic form?

A

Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq)

48
Q

What is the solid product formed in the reaction between AgNO3 and NaCl?

A

AgCl(s)

49
Q

Fill in the blank: Strong electrolytes in a Complete Ionic Equation are represented as _______.

A

ions

50
Q

True or False: In a Molecular Equation, reactants are shown as individual ions.

A

False

51
Q

What is a net ionic equation?

A

Includes only those solution components that actually react

Shows only components undergoing a change.

52
Q

In the net ionic equation As (aq) + CI (aq) → AgC (s), what are spectator ions?

A

Ions that do not participate directly in the reaction

Examples include Na* and NOg.

53
Q

What does the Bronsted-Lowry definition state about acids?

A

Acid is a proton donor.

54
Q

What does the Bronsted-Lowry definition state about bases?

A

Base is a proton acceptor.

55
Q

Fill in the blank: In a strong acid and base reaction, the equation is ______ + OH (aq) → H2 (l).

A

[strong acid]

Chem unit 4 (1 decks)

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