Guided Reader

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Name:_______________________________________ Date:_____________ Chapter 4

Guided Reader- Honors Chemistry

Directions: Please answer the questions to the guided reading activity as you read chapter 4 of your textbook. A word of advice: write page numbers by your answers so you can reference them later.

1.

Solutions in which water is the _______________ are called aqueous solutions.

2.

Water is the _________ for most chemical reactions that take place within and around us.

3.

What is the difference between a solvent and a solute?

4.

Ionizing aqueous solutions are called ____________. Whereas solutions that do not form ions are called__________________.

5.

When an ionic solid ____________, it breaks apart into its ions in solution.

6.

Describe why water is a very effective solvent for ionic compounds.

7.

What dissolved species are present in a solution of lithium carbonate?

8.

What dissolved species are present in a solution of methanol (CH

3

OH)?

9.

________________ exist completely as ions in solution.

10.

________________ exist as mostly molecules with few ions in solution.

11.

The balance produced when a weak electrolyte is in solution is ______________________.

12.

What is a precipitate?

13.

The amount of a substance that can be dissolved in a given quantity of solvent at that temperature is its _____________.

14.

Is sodium nitrate soluble or insoluble?

15.

Is Iron (III) carbonate soluble or insoluble?

16.

A double replacement reaction is also known as an ___________ reaction or a __________ reaction.

17.

The balanced chemical equations we came to know in chapter 3 are _____________ equations.

18.

When strong electrolyes are written as ions in a chemical equation, it is known as a

_________________________________.

19.

_______________ appear as both reactants and products.

20.

When a complete ionic equation is written without spectator ions, it is called a

________________________.

21.

If every ion in a complete ionic equation is a spectator ion, then _____________________.

22.

_________ increase the number of H

+

ions.

23.

_________ accept H

+

ions.

24.

Carbonic acid is monoprotic/diprotic (CIRLCE ONE).

25.

A strong acid or base is also a strong ___________.

26.

Likewise, a weak acid or base is also weak ____________.

27.

List the strong acids.

28.

List the strong bases.

29.

Ionic compounds are always __________ electrolytes.

30.

Molecular compounds that are not acids or ammonia are ______________.

31.

Ammonia is a weak ________.

32.

The reaction of an acid and a base produces __________ and _________.

33.

Thus the net ionic equation for the reaction in #32 is always

34. What gas is produced from the reaction of hydrochloric acid and sodium bicarbonate?

35. Loss of electrons is _____________.

36. Gaining electrons is _____________.

37. The oxidation number on an atom in elemental form is ____.

38. Monatomic ions have oxidation numbers equal to their _________.

39. Oxygen’s oxidation number is always _____, except when it is a peroxide (O

2

2-

) and has an oxidation number of ____.

40. Hydrogen is +1 when it is with a __________ and -1 when it is with a ________.

41. All halogen except for fluorine have positive oxidation numbers when combined with _______.

42.

The sum of oxidation numbers of a neutral compound is equal to _______ .

43.

The sum of oxidation numbers in a polyatomic ion is equal to ____________.

44.

Oxidation of metals by acids and salts is an example of a single/double replacement. (CIRCLE 1)

45.

Whenever a substance is reduced, some other substance must be ________.

46.

What is an activity series?

47.

_______________ and ______________________ are called the active metals.

48.

______________________ are called the noble metals.

49.

Any metal on the activity series can be oxidized by the ions of elements __________.

50.

Can nickel metal be oxidized by ions of iron?

51.

Only the metals above hydrogen in the series are able to react with _______ to form _______.

52.

The amount of solute dissolved in a given quantity of solvent or solution is _______________.

53.

Fill in below:

Molarity =

54.

Calculate the molarity of a solution made from 45.2g sodium nitrate in enough water to form 225 mL of solution.

55.

A 2.0 M solution of Na

2

SO

4

is ___M in Na

+

ions and ____M in SO

4

2-

ions.

56.

Dimensional analysis tells us that molarity x volume= __________.

57.

Because matter cannot be created nor destroyed, in dilutions the number of ________ stays the same.

58.

M

1

V

1

= _________

59.

Fill in the stoichiometric figure below:

60.

What is a titration?

61.

A reagent solution of known concentration is called a ____________________.

62.

Stoichiometrically equivalent quantities are brought together at the _____________________.

63.

What is an indicator?

64.

What does the color change indicate in a titration?

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