Final Flashcards
(64 cards)
1
Q
Acid ends in -ate
A
ending in -ic acid ex. chlorate -> chloric acid
2
Q
Acid ends in -ite
A
ending in -ous acid ex. chlorite -> chlorous acid
3
Q
Acid ends in -ide
A
ending in -ic acid prefix hydro- ex. chloride -> hydrochloric acid
4
Q
The one with the second fewest oxygens
A
ends in -ite
5
Q
The one with the second most oxygens
A
ends in -ate
6
Q
The one with the most oxygens
A
per_____ate
7
Q
The one with the least oxygens
A
hypo_____ite
8
Q
Cation
A
metal
9
Q
Anion
A
nonmetal
10
Q
Group 1A
A
Alkali Metals
11
Q
Group 2A
A
Alkaline earth metals
12
Q
Group 6A
A
Chalcogens
13
Q
Group 7A
A
Halogens
14
Q
Group 8A
A
Noble Gases
15
Q
Beta rays (charge)
A
negative
16
Q
Alpha rays (charge)
A
positive
17
Q
Gama rays (charge)
A
none
18
Q
Naming (order to name)
A
Cation first; Anion second
19
Q
Intensive properties
A
inside material ex. density, boiling point, color
20
Q
Extensive properties
A
depends on how much material there is ex. mass, volume, energy
21
Q
Combination reactions
A
Two or more reactants combine to form a single compound.
22
Q
Decomposition reactions
A
A single reactant breaks apart to form two or more substances.
23
Q
Combustion in Air
A
Hydrocarbon + Oxygen -> Carbon dioxide and Water.
24
Q
Formula Weight
A
is the sum of the atomic weights for the atoms in a chemical formula (once been reduced)
25
Molecular Weight
is the sum of the atomic weights of the atoms in a molecule
26
Percent Composition
(Number of atoms\*atomic weight)/(FW of compound)x100
27
Stoichiometric Calculations
28
Limiting Reactant
reactant present in the smallest stoichiometric amount.
29
Theoretical yield
the maximum amount of product that can be made.
– In other words, it's the amount of product possible as calculated through the stoichiometry problem.
30
Actual yield
amount one actually produces and measures
31
Percent Yield
32
Solutions
homogeneous mixtures of two or more pure substances.
33
Solvent
present in greatest abundance
34
Solutes
All other substances
35
Dissosciation
Whenanionic substance dissolves in water, the solvent pulls the individual ions from the crystal and solvates them
36
Electrolyte
substance that dissociates into ions when dissolved in water.
37
Nonelectrolyte
may dissolve in water, but it does not dissociate into ions when it does so.
38
Electrolytes & Nonelectrolytes
may dissolve in water, but it does not dissociate into ions when it does so.
39
Strong Electrolyte
dissociates completely when dissolved in water.
40
Weak Electrolyte
dissociates partially when dissolved in water.
41
Strong Acids
42
Strong Bases
43
Ionic equation
all strong electrolytes (strong acids, strong bases, and soluble ionic salts) are dissociated into their ions
44
Net Ionic Equation
To form the net ionic equation,cross out anything that does not change from the left side of the equation to the right:
45
Neutralization Reactions
Generally, when solutions of an acid and a base are combined, the products are a salt and water:
46
Oxidation number
* Elements in their elemental form have an oxidation number of 0.
* The oxidation number of a monatomic ion is the same as its charge.
* Nonmetals tend to have negative oxidation numbers, although some are positive in certain compounds or ions.
* Oxygen has an oxidation number of −2, except in the peroxide ion, in which it has an oxidation number of −1.
* Hydrogen is −1 when bonded to a metal, +1 when bonded to a nonmetal.
* Fluorine always has an oxidation number of −1.
* The other halogens have an oxidation number of −1 when they are negative; they can have positive oxidation numbers, however, most notably in oxyanions
* The sum of the oxidation numbers in a neutral compound is 0.
* The sum of the oxidation numbers in a polyatomic ion is the charge on the ion.
47
Dilution
The molarity of the new solution can be determined from the equation:
where Mc and Md are the molarity of the concentrated and dilute solutions, respectively, and Vc and Vd are the volumes of the two solutions.
48
Energy
the ability to do work or transfer heat
49
Work
organized transfer of energy (such as that used to cause an object that has mass to move)
50
Heat
Chaotic transfer of energy. flows from warmer objects to cooler objects
51
First Law of Thermodynamics
Energy is neither created nor destroyed
52
Internal Energy
the change in internal energy, ΔE, is the final energy of the system minus the initial energy of the system
Efinal - Einitial
53
Changes in Internal Energy (absorbes)
If ΔE \> 0, Efinal \> Einitial Therefore, the system absorbed energy from the surroundings.
This energy change is called ***_endergonic_***
54
Changes in Internal Energy (release)
If ΔE \< 0, Efinal \< Einitial Therefore, the system released energy to the surroundings.
– This energy change is called ***_exergonic_***.
55
ΔE, q, w, and Their Signs
56
endothermic
When heat is absorbed by the system from the surroundings...delta H is positive
57
Exothermic
When heat is released by the system into the surroundings....delta H is negative
58
State Functions
internal energy is a state function..q and w are not state functions
59
Enthalpy
the internal energy plus the product of pressure and volume:
H = E + PV
1. Enthalpy is an extensive property.
2. ΔH for a reaction in the forward direction is equal in size, but opposite in sign, to ΔH for the reverse reaction.
3. ΔH for a reaction depends on the state of the products and the state of the reactants (it is a state function)
60
Change in Enthalpy
61
Specific Heat
62
Hess's Law
“[i]f a reaction is carried out in a series of steps, ΔH for the overall reaction will be equal to the sum of the enthalpy changes for the individual steps.”
63
Calculation of Delta H
64
