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Chemistry 101 > Exam 2 > Flashcards

Exam 2 Flashcards

(96 cards)

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1
Q

Coefficient

A

used to describe the quantity relationships between substances involved in a chemical equation

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2
Q

Mole ratio or mole bridge

A

Relationship between two component sin a balanced chemical equation

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3
Q

A+B —> C + D

How many grams of D made from Xg of A

A

Mass in g of A–>moles of a—>moles of D—->mass in g of D

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4
Q

how to find out if and how much of access there is

A

count out on dot diagram, must obey law of conservation by showing access

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5
Q

Theoretical yield

A

theoretical yield: stoichiometry

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6
Q

solution defintion

A

homogeneous mixture of 2+ solutions

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7
Q

2 different components of a solution

A

solvent- major component: water

Solute-minor component

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8
Q

aqueous solution

A

dissolved in water

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9
Q

color of CuSO4(s) vs color of CuSO4(aq)

A

blue-intensive

blue-extensive (depends on amount of waterCuSO4)

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10
Q

electrolyte

A

substance who’s solution (substance (aq)) contains ions and has the ability to conduct electricity

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11
Q

how to identify an electrolyte

A

look for ionic compounds (metal and non metal)

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12
Q

non elctrolyte

A

a substance who’s aqueous solution does not contain ions and therefore doesn’t conduct electrocution (coval

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13
Q

non elctrolyte

A

a substance who’s aqueous solution does not contain ions and therefore doesn’t conduct electrocution

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14
Q

how to identify a non electrolyte

A

covalent bond: 2 non metals

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15
Q

what happens to ions in a solution

A

solvent forms a cane around an ion because solvent (water) has partially polar ends and ions have charged ends

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16
Q

What happens in a solution with polyatomic ions

A

never break apart when in solution

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17
Q

what happens when you put a covalent compound in H2O

A
  1. solid dissolve in water: tend to have N,O, Halogen
  2. solids don’t dissolve (only C,H)
  3. Liquids that are Miscible: will mix
  4. Liquids that are immiscible (lots of C,H)
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18
Q

Miscible/immiscible

A

able to mix/unable to mix

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19
Q

electrolytes in Ionic compounds

A

Strong electrolytes: All, strong bases and salts, lots of ions in solution
Weak electrolyte: none, few ions in solution
Non electrolytes: none

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20
Q

electrolytes in Covalent compounds

A

Strong electrolytes: strong acids, lots of ions in solution
Weak electrolytes: weak acids, weak bases, few ions in solution
No electrolytes: almost all (every covalent molecule)

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21
Q

what certain types of molecules compounds don’t disassociate when mix with water

A

most important acid

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22
Q

Strong acids

A

strong electrolytes

  • only move one way through he reaction (one arrow)
  • completely dissociates
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23
Q

Weak acids

A

Weak electrolytes

  • moves both ways through equation, double arrow
  • partially disassociate
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24
Q

Strong acids

A
  1. HCl
  2. HBr
  3. HI
  4. HNO3
  5. H2SO4
  6. HClO4
  7. HClO3
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25
Weak acids
H and anything else lol
26
Solubility of NO3-,CLO4-,Na+,K+,NH$+
Soluable | no exceptions
27
Solubility of Cl- and I-
Soluble except with Ag+, Hg22+,Pb2+
28
Solubility of SO42-
Soluble except with Ca2+,Ba2+,Sr2+,Hg,2+,Pb2+,Ag+
29
CO32- and PO43- solubility
insoluble except with Group 1A and NH4+
30
OH- solubility
Insoluble except with Group 1A, Ca2+,Ba2+,Sr2+
31
S2- solubility
insoluble except with Group 1A, 2A, and NH4+
32
Strong acids vs strong bases in terms of compounds and dissacociation
Strong acids: Covalent compounds fully dissacociate | Strong bases: Ionic compounds and always include NH-
33
Are Molecular (covalent) compounds) with OH
Pb2+ and Ca2+
34
exchange reaction
reaction in which cation from one reactant and the anion from the other reactant form a product
35
Two ionic compounds as reactants making two ionic compouns
make aqueous solution of ionic reactants
36
common strong acids
``` Hydrochloric acid HCl Hydrobromic acid HBr Hydroiodic acid HI Chloric acid HClO3 Perchloric acid HClO4 Nitric acid HNO3 Sulfuric acid (first proton) H2SO4 ```
37
Strong bases
Group 1A metal hydroxides (LiOH,naOH,kOH,RbOH,CsOH) Heavy group 2A metal hydroxides (Ca(OH)2,Sr(OH)2,Ba(OH)2
38
Precipitation reactions
1. use reaction formulas to determine available ions 2. switch partners; propose products 3. check solubility rules 4. balance equation
39
Molecular equation
balanced reaction shown without charges | AgNO3(aq)+NaCl(aq)-->AgCl(s)+NaNO3(aq)
40
Complete ionic equations
balanced reactions shown with all aqueous solutions as ions | Ag+(aq) + NO3- (aq) +Na+ (aq) + Cl- (aq) --> AgCl(s) + Na+(aq) + NO2-(aq)
41
Net ionic equation
balanced equation that does not predicate in product formation (without spectator ions) Ag+(aq)+Cl-(aq)-->AgCL(s)
42
Spectator ions
The ions which do not change state
43
acids are
molecular compounds that ionize in water, produce H+ (hydrogen cation) proton donors 1. strong acid completely disassociates h+ grabbed by H2O 2. Weak acids partially disassociate H3O+ hydronium
44
Basics reacting with water
1. Ionic solids that dissolve in water, result of OH- in solution STRONG 2. Molecular compounds react with water, result of reaction is OH- in solution, WEAK
45
Note to remember about bases
1. NaOH(s) -->(in H2O) -->Na+(aq) + OH- (aq) | 2. NH3(l) -->in H2O
46
monoprotic acids
1 reactant:1 H+ mole ratio
47
Polyprotic
1 reactant: X H+ mole ratio
48
Strong acids
Only one way, will not see any reactions in solution
49
Weak acids
Both ways, see reactants and products in solution | -not all equally weak; more H+ you see the stronger the weak acid
50
Strong Base
mOH,m(OH)2 heavy metal
51
Weak bases
Look for "n" in molecular formulas
52
Neutralization reaction
exchange reaction between acid and base | *note: some will relate gas if base contains CO32- carbonate
53
Molarity (M)
describes solution concentrations
54
M=
Moles/Liters
55
Dilution
M1V1=M2V2 | -Number of moles removed from concentrated solution is equal to number of moles put into dilute solution
56
Solution stychiometry
1. in solution you will be given volume, go to moles and use the mole bridge 2. build a chemical reaction any time two different compounds are being discussed
57
Neutral pH
H+=OH-
58
Acid pH
H+>OH-
59
Basic pH
H+
60
[H+][OH-]=
1.0x10^-14
61
pH=
-Log[H+]
62
pH+pOH
14
63
pOH=
-log[OH-]
64
[OH-]=
10^-pOH
65
H+=
10^-pH
66
What is one of the most important properties of water
it has the ability to act as either an acid or a base
67
K>1
Reaction is product forward
68
K<1
Reaction is reaction forward
69
Kw=
1.0x10^-14
70
How to solve pH
1. identify acid or base 2. write what you expect 3. what I the dissacoication of the chemical being discussed?
71
Thermochemistry
energy chains accompanying chemical reactions
72
Energy
capacity to do work or to transfer heat
73
Work (w)
ability to move something
74
Heat (q)
cause a temp change - remove heat: object cools - add heat: object warms
75
Kinetic energy
energy of motion despite small size, atoms, and molecules have mass and motion. therefor they have kinetic energy
76
Ek=
1/2mv^2 unites of Jules (j)
77
potential energy
energy an objet has due to it's position relative to other objects
78
two types of potential energy
1. Gravitational potential E: macro scale items | 2. Elecrostatic potential E: Due to interactions between 2 charges particles
79
Ee1=
(KQ1Q2)/d Q1-charge 1 Q2-charge 2
80
relationship between attraction and distance between particles
Opposites attracts as the distance between decreases, the attraction increases
81
System
part you're interested in: a chemical reaction that'll take place (phase change or rxns)
82
surroundings
literally everything else in the universe
83
Three kinds of systems
1. open-energy and matter can be transferred (coffee cup w no top) 2. closed-Energy can be transferred matter not transfereed (cardboard cup with lid and sleeve) - -since matter not transferred just worry about energy 3. isolated-energy nor matter can't be transferred(yeti)
84
transferring heat
- cause temperature change - heat can be transferred from system to surrounding or from surrounding to system - if heat enters: endothermic - if heat leaves: exothermic
85
Transferring work
when force moves an object | -work can be preformed on or by system
86
first law of thermodynamics
-energy conserved -E can be transferred in and out of a system, but the total E of the universe is constant Euniverse=Esys+Esur
87
The internal energy, E, of a system
add up every component of all kinetic and potential E of every piece of mater in system - motion of molecules; interactions b/t molecules - in any given atom you have motions and interactions b/t nuclei and electrons
88
Change in E
Ef-Ei
89
state of function=
delta E
90
Delta E>0
system must gain energy from surroundings
91
Delta E<0 system
must lose heat to surroundings
92
what is so special about only having to quantify chang
Energy is both heat and work delta E=q+w
93
loss of E of battery
W/coil: energy lost only as heat | w/fan: energy lost w heat and work
94
Exothermic feels
warm to touch
95
endothermic feels
cold to touch
96
First law of thermodynamics
Reactants to products delta E<0 loss of E | Products to reactants delta E>0 gain of E

Chemistry 101 (4 decks)

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