Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry 01 > Cahpter 4 > Flashcards

Cahpter 4 Flashcards

(61 cards)

Start Studying
1
Q

What is a Aqueous Solution?

A

A solution in which the solvent is water.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is the shape of the water molecule?

A

An individual H2O molecule is bent or V-shaped, with an H-O-H angle of approx. 105 degrees. The O-H bonds are covalent bonds formed by electron sharing. between the oxygen and hydrogen atoms.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is a partial charge?

A

Less than one unit of charge.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is a polar molecule?

A

Unequal charge distribution of a molecule.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is hydration?

A

When the positive ends of the water molecules are attracted to the negatively charged anions and that the negative ends are attracted to the positively charged cations.

It is very important to recognize that when ionic substances (salts) dissolved in water, they break up into the individual cations and anions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Solubility

A

Polar and ionic substances are expected to be more soluble in water than nonpolar substances. Like dissolves like is a useful rule for predicting solubility.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

True of False A solution is a homogeneous mixture?

A

True

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is the difference between Solute and Solvent.

A

Solute is the substance and the solvent is generally water.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is the difference between Strong Electrolytes, Week Electrolytes, and Nonelectrolytes.

A

Strong electrolytes dissolve completely in water, week electrolytes dissolve somewhat and nonelectrolytes, not at all.

Strong electrolytes are substances that are completely ionized when they are dissolved in water.

Classes of strong electrolytes: Soluble salts, strong acids, and strong bases.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is electrical conductivity?

A

Ability of conduct an electric current? Strong electrolytes conduct the best.

The extent to which a solution can conduct an electric current depends directly on the number of ions present.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is a acid?

A

Arrhenius proposed that an acid is a substance that produces H+ ions (protons) when it is dissolved in water.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is a strong acid?

A

A strong acid is one that completely dissociates into its ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is a strong base?

A

Soluble ionic compounds containing the hydroxide ion OH-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is a weak acid?

A

Any acid that dissociates (ionizes) only to a slight extent in aqueous solutions is called a weak acid.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are nonelectrolytes?

A

Nonelectrolytes are substances that dissolve in water but do not produce any ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is molarity (M)?

A

M - molarity = moles of solute / liters of solution

also M x V = mol

Most commonly used expression of concentration.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is a standard solution?

A

A solution whose concentration is accurately known.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is dilution?

A

When water is added to achieve the molarity desired for a particular solution.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Question #1?

A

Moles of solute after dilution = moles of solute before dilution.

M1V1 = M2V2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What is a pipet?

A

Is a device for accurately measuring and transferring a given volume of solution. There are volumetric (or transfer) pipets and measuring pipets.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What are the Types of Solution Reactions?

A

Precipitation reactions
Acid-base reactions
Oxidation-reduction reactions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What is precipitation reaction?

A

When two solutions are mixed, an insoluble substance sometimes forms; that is, a solid forms and separates from the solution. Such a reaction is called a precipitation reaction and the solid that forms is called a precipitate.

A precipitation reactions also can be called a double displacement reaction.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Remember

A

In virtually every case, when a solid containing ions dissolves in water, the ions separate and move around independently.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What can help predict the products of a reaction?

A
  1. When ions form a solid compound, the compound must have a zero net charge.
  2. Most ionic materials contain only two types of ions: one type of cation and one type of anion.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
What does doing chemistry require?
Doing chemistry requires both understanding ideas and remembering key information.
26
What are the Simple Rules for the Solubility of Salts in Water?
1. Most nitrate (NO3-) salts are soluble. 2. Most salts containing the alkali metal ions (Li+, Na+, K+, Cs+, Rb+) and the ammonium ion (NH4+) are soluble. 3. Most chloride, bromide, and iodide salts are soluble. Notable exceptions are salts containing the ions Ag+, Pb++, and Hg2++ 4. Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, Hg2SO4 and CaSO4. 5. Most hydroxides are only slightly solble. THe important soluble hydroxides are NaOH and KOH. The compounds Ba(OH)2, Sr(OH)2, and Ca(OH)2 are marginally soluble. 6. Most sulfide (S--), carbonate (CO3--), chromate (CrO4--), and phosphate (PO4---) salts are only slightly soluble, except for those contain the cations in Rule 2.
27
What is the key to dealing with the chemistry of an aqueous solution?
First to focus on the actual components of the solution before any reaction occurs and then to figure out how these component will react with each other.
28
What are the three types of equations that are used to describe reactions in solution?
Formula equation Complete ionic equation Net ionic equation.
29
What is a formula equation?
Gives the overall reaction stoichiometry but not necessary the actual forms of the reactants and products in solution.
30
What is a complete ionic equation?
Represents as ions all reactants and products that are strong electrolytes.
31
What is a net ionic equation?
Includes only those solution components undergoing a change. Spectator ions are not included.
32
What are spectator ions?
Ions that do not participate directly in the reaction are called spectator ions.
33
What two points need special emphasis when solving solution reactions?
1. It is sometimes difficult to tell immediately what reaction will occur when two solutions are mixed. 2. To obtain the moles of reactants we must use the volume of the solution and its molarity.
34
Problem-Solving Solving Stoichiometry Problems for Reactions in Solution
1. Identify the species present in the combined solution, and determine what reaction occurs. 2. Write the balanced net ionic equation for the reaction. 3. Calculate the moles of reactants. 4. Determine which reactant is limiting. 5. Calculate the moles of product or products, as required. 6. Convert to grams or other units, as required.
35
Difference between an acid and a base?
An acid is a substance that produces H+ ions when dissolved in water, and a base is a substance produces OH- ions.
36
How did Johannes N. Bronsted and Thomas M. Lowry define acids and bases?
Acid is a proton donor Base is a proton acceptor.
37
OH-
OH- ion has such a strong affinity for protons that it can strip them form other molecules.
38
Second OH-
The hydroxide ion is such a strong base that for purposes of stoichiometric calculations it can be assumed to react completely with any weak acid that we will encounter. Of course, OH- ions also react completely with the H+ ions in solutions of strong acids.
39
Problem Solving Performing Calculations for Acid-Base Reactions
1. List the species present in the combined solution before any reaction occurs, and decide what reaction will occur. 2. Write the balanced net ionic equation for this reaction. 3. Calculate the moles of reactants. For reactions in solution, use the volumes of the original solutions and their molarities. 4. Determine the limiting reactant where appropriate. 5. Calculate the moles of the required reactant or product. 6. Convert to grams or volume (of solution) as required.
40
What is a neutralization reaction?
An acid-base reaction is often called a neutralization reaction. When just enough base is added to react exactly with the acid in a solution, we say the acid has been neutralized.
41
What is Volumetric Analysis?
Volumetric Analysis is a technique for determining the amount of a certain substance by doing a titration.
42
What is a titration?
A titration involves delivery (from a buret) of a measured volume of a solution of know concentration (the titrant) into a solution containing the substance being analyzed (the analyte)
43
What are the Requirements for a Successful Titration?
1. The exact reaction between titrant and analyte must be known (and rapid). 2. The stoichiometric (equivalence) point must be marked accurately. 3. The volume of titrant required to reach the stoichiometric point must be know accurately.
44
The analysis of complex solutions.
The first step in analysis of a complex solution is to write down the components and focus on the chemistry of each one. When a strong electrolyte is present, write it as separated ions. In doing problems involving titrations, you must first decide what reaction occurring. Sometimes this seems difficult because the titration solution contains several components. The key to success in doing solution reactions is to first write down all the components in the solution and focus on the chemistry of each one.
45
What are Oxidation-reduction reactions?
When one or more electrons are transferred.
46
What is another name for oxidation-reduction reactions?
Redox reactions.
47
Photosynthesis is what type of reaction?
oxidation-reduction reaction.
48
Most reactions used for energy production are what type of reactions?
oxidation-reduction reactions.
49
Combustion is what type of reaction?
oxidation-reduction reactions.
50
What are oxidation states?
The concept of oxidation states provides a way to keep track of electrons in oxidation-reduction reactions, particularly redox reactions involving covalent substances. Recall that electrons are shared by atoms in covalent bonds. The oxidation states of atoms in covalent compounds are obtained by arbitrarily assigning the electrons (which are actually shared) to particular atoms. We do this as sollows: For a covalent bond between two identical atoms, the electrons are split equally between the two. In cases where two different atoms are involved (and the electrons are thus shared unequally), the shared electrons are assigned completely to the atom that has the stronger attraction for electrons. Thus in water, oxygen has formally "taken" the electrons from two hydrogen atoms.
51
Define oxidation states.
The oxidation states of the atoms in a covalent compound as the imaginary charges the atoms would have if the shared electrons were divided equally between identical atoms bonded to each other or, for different atoms were all assigned to the atom in each bond that has the greater attraction for electrons. Of course, for ionic compounds containing monatomic ions, the oxidation states of the ions are equal to the ion charges.
52
Oxidation states are also know as?
Oxidation numbers.
53
What is the oxidation state for an electrically neutral compound?
The sum of the oxidation state must be zero for an electrically neutral compound.
54
Can the oxidation state be a noninteger?
Yes. A noninteger value for the oxidation state may seem strange because charge is expressed in whole numbers. However, although they are rare, noninteger oxidation states do occur because of the rather arbitrary way that electrons are divide up by the rules. For example, the rules assume that all the iron atoms are equal when in fact this compound can best be viewed as containing four O-- ions, two Fe+++ ions and one Fe++ ion per formula unit. i.e 8/3+
55
Helpful mnemonics.
OIL RIG = Oxidation Involves Loss, Reduction Involves Gain LEO says GER = Loss of Electrons, Oxidation; Gain of Electrons, Reduction.
56
Rules for Assigning Oxidation States
1. An atom in an element is zero. Element: 0 2. A monatomic ion is the same as its charge. Monatomic ion: charge of ion. 3. Fluorine is -1 in its compounds. Fluorine: -1 4. Oxygen is usually -2. Exception: peroxides (containing O2-- in which oxygen is -1 Oxygen: -2 5. Hydrogen is +1 in its covalent compounds. Hydrogen: +1
57
What is Oxidation?
Oxidation is an increase in oxidation state (a loss of electrons). Oxidizing agent - electron acceptor.
58
What is Reduction?
Reduction is a decrease in oxidation state (a gain of electrons). Reducing agent (electron donor)
59
Oxidized
Loses electrons Oxidation state increases Reducing agent
60
Reduced
Gains electrons Oxidation state decreases Oxidizing agent.
61
Problem Solving Balancing Oxidation - Reduction Reactions by Oxidation States
1. Write the unbalanced equation 2. Determine the oxidation sates of all atoms in the reactants and products. 3. Show electrons gained and lost using "tie lines" 4. Use coefficients to equalize the electrons gained and lost. 5. Balance the rest of the equation by inspection. 6. Add appropriate sates.

Chemistry 01 (3 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions