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?