Chem Final Sem 2 Flashcards
1
Q
Oxidation numbers, what are they?
A
+ or - charge on atom or group of atoms
2
Q
Give two examples of an element or polyatomic ion with its oxidation number
A
Na+,
3
Q
List the prefixes in order from 1 through 9
A
1- Mono
2- Di
3- Tri
4- Tetra
5- Penta
6- Hexa
7- Hepta
8- Octa
9- Nona
3
Q
Greek prefixes – what do they tell us?
A
The number of whatever the item is
4
Q
Compound naming: you should be able to use your Ion Chart and be able to name binary ionic
compounds!
SbN
A
Antimony (III) Nitride
5
Q
What does binary mean
A
2 parts
6
Q
What does ionic mean
A
Atom loses electron to other when they bond
7
Q
What is cation and which part of formula do you see it
A
Positive ion, in very front
8
Q
LiH which is cation
A
Li
9
Q
Formula for sodium benzoate
A
Na2C7H6O2
10
Q
Formula for magnesium acetate
A
Mg(C2H3O2)2
11
Q
Formula for Iron (III) chloride and Iron (II) chloride
A
Iron (III) chloride- FeCl3
Iron (II) chloride- FeCl2
12
Q
What’s the difference between Iron (III) and Iron (II)
A
+2 vs +3 charge (oxidation #)
13
Q
What is stock system of naming compounds and give examples
A
Iron (II) oxide
Antimony(III) Phosphide
14
Q
Why is it important to balance the + and - charges of ions in a formula
A
Balances to 0 which is neutral and less likely to react
15
Q
Water can and does attach itself to the crystalline structure of a molecule. What is the water called?
A
Hydrate
16
Q
What do we call a compound that has no water in the molecule?
A
Anhydrous
17
Q
What is the name for MgSO4 * 3H2O
A
Magnesium sulfate Trihydrate
18
Q
Chemical formula for calcium fluoride
A
CaF2
19
Q
Chemical formula for silicon disulfide?
A
SiS2
20
Q
What is the reactant or reactants and product or products in 4Fe + 3O2 —-> 2Fe2O3
A
Reactant: 4Fe + 3O2
Products: 2Fe2O3
21
Q
Define reactant and product in any chemical equation.
A
Reactant- what starts at beginning (ingredients)
Product- what you get at the end
22
Q
What are coefficients and subscripts
A
Coefficients- How many of that atom or molecule is in equation
Subscript- How many atoms or group of atoms there are
23
Q
Coefficients and subscript for 3H2 + O2 —-> 3H2O
A
Coefficients- 3
Subscripts- 2
24
What part of any equation can we change to balance all the atoms of each element on both sides of the equation?
Coefficients only
25
Why do we need to balance every atom of every element on both sides of reaction
Law of mass conservation: you can't have matter disappear in universe like that
26
NaCl(s)
(s) means
Solid was produced
27
NaCl(aq)
(aq) means
Aquaeous; dissolved in water=solution
28
N2(g)
(g) means
Gas was produced
29
What does -----> mean
Yields or this will result in
30
What does (triangle sign) above arrow mean
Heat was added to get reaction going
31
When you see an element above arrow, it means it's catalyst. What do they do
Speeds up reaction while its unchanged
32
Synthesis reaction
Make something by combining reactants
2H2 + O2 ----> 2H2O
33
Decomposition reaction
Break down something
CaCl2 ---> Ca + Cl2
34
Single replacement reaction
Cations swap places
Mg + CuSO4 ---> Cu + MgSO4
35
Double replacement reaction
Cations swap places but no cation is left alone
AgNO3 + NaCl ---> AgCl + NaNO3
36
What do net ionic equations show*
Ions that actually react
37
What are spectator ions*
Appears in both reactants and products; it doesn't react with other ions
38
Describe what is a mole, what is number value of mole
Its a number
6.022 x 10^23 of anything
39
Mole is also known as __________________
Avogandro's number
40
What is Avogandro's number based on
12.01 grams per mole of Carbon-12
41
2 examples of mole used in chem
1 mole of Hydrogen atoms weigh 1.01 g
42
One mole of CO2 contains ___ moles of carbon atoms and ____ moles of oxygen atoms
1, 2
43
Molar mass is typically expressed in which unit?
Grams/mole
44
What type of formula best represents the arrangement of bonds in a molecule?
Structural formula
45
What is the molar mass of carbon monoxide?
28 g
46
Where can you find the information needed to change grams of a substance to moles?
Periodic table show you the grams per mole of an element.
47
Limiting reactant
Reactant thats used up 1st before other reactants in reaction
Prevents more product from forming
48
Excess reactant
Any leftover reactants when reaction is finished
49
Empirical formula
Simplest form of a formula . Numbers cannot be divided even lower.
P10H14 no P5H7 yes
50
Molecular formula
Shows all the elements and how many of each element in the formula
C2H6O
51
Structural formula
Number and types of atoms involved. How these atoms are put together
52
Yield
How much product are you getting at the end
53
Actual yield
Physically measured amount of of product at end of reaction
54
Theoretical yield
Max amnt of product made that is calculated on paper from a given amnt of reactant
55
Percent yield
Percentage of theoretical yield that was actually produced
56
The most important indicator of efficiency for a chemical manufacturing company is its ____________ yield
Percent
57
Solute vs solvent
Solute: Dissolved substances in solution
Colvent: Major part of solution, does dissolving
58
What makes up most of solution
Solvent
59
Example of liquid, solid, and gas solution
Liquid: Coffee
Solid: Staples
Gas: Atmosphere
60
Properties of solutions
Solutes can't be filtered out of solution
Solutes don't settle out of solution
Solutions are uniform
Solutions are not chemically combined
Solutions can vary in their concentration
61
How does water dissolve NaCl
Solvation
62
Solutions can occur in solids, liquids, and gases. Y/N
Yes
63
Can you have more than one solute in solution
Yes
Ex: Soda
64
Characteristics of acid and base
Acid: Sour, electrolyte, react with metals to product H+ gas and salt, pH below 7
Base: Bitter, feels slippery, some are electrolytes, pH above 7
65
Electrolyte
Substance that ionizes to conduct electricity in solution
66
pH means what
Power of hydrogen
67
pOH means what
Power of hydroxide
68
What is pH and pOH scale based on
Ionization constant of water
69
What does pH scale tell you
How acidic or basic/alkaline a substance is
70
What does pOH scale tell you
Hydroxide ion concentration
71
pH = 7 tells what
Neutral solition
72
pH < 7 vs pH > 7
pH < 7 = acid
pH > 7 = base
73
pOH < 7 vs pOH > 7
pOH < 7 = Base
pOH > 7 = Acid
74
Strong vs weak acid
Strong: Give up protons easily, ionize completely, dissolves well
Weak: Don't dissociate (separate) completely into ions, dissolve poorly in water
75
Strong vs weak base
Strong: Accept proton readily, dissolves well
Weak: Weak proton acceptors, doesn't dissolve well
76
Neutralization, whats the idea
Acid and base neutralize each other as they are opposites
77
Acid + base -------> ____________ + __________
Salt, water
78
If you look at a glass of water, are 100% of water in there H2O
No
79
Conjugate acid
Formed when proton is transformed to the base
Base gains H+ ----> Conj acid
80
Conjugate base
Everything that remained of acid molecule after a proton is lost
Acid loses H+ ----> Conj base
81
Bases and acids are they the same or are they ___________________
Opposites
82
Oh my lady gaga you spilled base on your arm! How do you respond to neutralize it?
Add acid on it
83
Titrations
Controlled neutralization reactions that are used to determine unknown concentration of solution
84
Equivalence point
Equal moles of acid and base
85
End point
Color changes at pH 7
86
MaVa = MbVb tells what
Equation used to solve for unknown molarity concentrations
87
Buffer
Solutions that resist changes in pH. Most effective at regulating slight pH changes
88
Bronsted-Lowry acid and base
Acid donates proton (deprotonation)
Base accepts proton (protonation)
89
What does REDOX mean
Oxidation reduction reaction
90
Reduction; give half equation ex
Atom gains electron/s
Ex: Na ---> Na+ + 1e-
91
Oxidation; give half equation ex
Atom loses electron's
Ex: Na+ + 1e- ---> Na
92
What is being lost or gained in any REDOX reaction
Electrons
93
Oxidation agents
Atoms that would cause another atom to lose electrons
94
Reduction agents
Atoms that would cause another atom to gain electrons
95
Weak electrolyte vs strong electrolyte, which is better electrical conductor
Strong bc they allow more electrons to conduct
96
Spontaneous
No energy needed to get reaction going
Ex: Voltaic/galvanic battery, vinegar reacting w/baking soda
97
Nonspontaneous
You need energy to get the reaction going
Ex: Recharging a battery by running electricity and causing chemical reaction to go backwards to charge battery
98
Anode
Attracts anions; is positive; oxidation
99
Cathode
Attracts cations; negative; reduction
100
RED CAT
Reduction cathode- gains electrons from anode
101
AN OX
Oxidation anode- Electrons leave to go to cathode
102
Zinc anode
Provides electrons to go through circuit, power up what is hooked up and goes on to cathode
As it loses electrons, zinc begins to disintegrate
103
Copper cathode
Where all electrons go to accumulate on copper electrode due to electrons attracting copper ions
104
Salt bridge, why do we need it for battery to work
Electrochemical cells
Needed to assure neutrality of both compartments
105
Voltaic cell aka galvanic cell
Cell that provides electricity to power devices like phone
106
Intermolecular forces types, rate from strongest to weakest
Hydrogen bonding
Dipole-dipole
London (Dispersion) forces
107
Intermolecular force that exist btwn only nonpolar molecules (ex: oil) would be
London dispersion forces only
108
Why does water have a high boiling point? Why does it exist as a liquid at room temperature
Hydrogen bonds make water have higher boiling
109
Of all states of matter: Solid liquid gas and plasma, would you expect it to be the heaviest
Solid is heaviest except water due to how many molecules form when frozen
110
Evaporation vs vaporization
Both involving changing liquid to gas <--- alike
Evaporation is off the surface and below the boiling point.
Vaporization is the surface and happening in the inside of a liquid
111
Which is it, evaporation or vaporization would you expect to occur at the boiling point?
Both can happen there but vaporization is the main one because it is a total change.
112
What is the binding forces in crystals forming a crystal lattice , like NaCl, or sugar?
(Attractions between molecules)
113
How can we cause a crystal lattice to melt?
Add thermal energy. (Heat)
114
Why do crystal lattices melt?
Adding thermal energy overcomes the crystal lattice and the solid begins to melt.
