Chemistry 300 - Fall Term Flashcards
1
Q
SF rule for adding/subtracting?
A
Keep the fewest number of decimal points
2
Q
SF rule for multiplying/dividing?
A
Keep the fewest number of significant figures
3
Q
When there is a (blank), trailing zeros are significant
A
decimal point
4
Q
When there is an imbalance between protons and electrons, the atom is called an
A
ion
5
Q
Positive Ion (more protons than electrons; positive charge) is called a
A
Cation
6
Q
Negative ion (more electrons than protons; negative charge) is called a
A
Anion
7
Q
Carbonate
A
CO₃²⁻
8
Q
Sulfate
A
SO₄²⁻
9
Q
Acetate
A
CH₃COO⁻
10
Q
Bicarbonate (or Hydrogen Carbonate)
A
HCO₃⁻
11
Q
Hydroxide
A
OH⁻
12
Q
Nitrate
A
NO₃⁻
13
Q
Phosphate
A
PO₄³⁻
14
Q
Ammonium
A
NH₄⁺
15
Q
Hydrochloric
A
HCl
16
Q
Nitric
A
HNO₃
17
Q
Sulfuric
A
H₂SO₄
18
Q
Acetic
A
CH₃COOH
19
Q
Baking Soda
A
NaHCO₃
20
Q
Glucose
A
C₆H₁₂O₆
21
Q
Hydrogen Peroxide
A
H₂O₂
22
Q
Sucrose (Table Sugar)
A
C₁₂H₂₂O₁₁
23
Q
Ammonia
A
NH₃
24
Q
Empirical Formula Song
A
Percent to mass, mass to mole, divide by small, multiply till whole
25
Molecular Formula =
(empirical formula)n
26
Mass MF =
(Mass EF) n
27
Ionic Bond =
Metal x Non-Metal
28
Covalent Bond =
Non-medal + Non-metal
29
Bond where u transfer
Ionic
30
Type 1 ionic nomenclature is for metals where
we know the charge (only one possible charge)
31
Bond where u share
Covalent
32
Type 2 ionic nomenclature is for...
transition metals (which are special since they can have multiple possible charges) EXCEPT for zinc, silver
33
Type 2 ionic nomenclature is for transition metals though there is an exception with which two metals which are type 1
zinc and silver
34
type 3 ionic nomenclature =
metal cation (according to type 1 or type 2) and polyatomic anion
35
Percent Water in a Hydrate formula
(mass H20/mass hydrate) x 100
36
formula for finding x in a hydrate (x = molecules of water)
mol H20/mol anhydrous salt
37
Which diatomic element is a gas at room temperature?
H₂ (Hydrogen)
N₂ (Nitrogen)
O₂ (Oxygen)
F₂ (Fluorine)
Cl₂ (Chlorine)
38
Which diatomic element is a liquid at room temperature?
Br₂ (Bromine)
39
Which diatomic element is a solid at room temperature?
I₂ (Iodine)
40
What is the state of Hydrogen (H₂) at room temperature?
Gas
41
What is the state of Nitrogen (N₂) at room temperature?
Gas
42
What is the state of Oxygen (O₂) at room temperature?
Gas
43
What is the state of Fluorine (F₂) at room temperature?
Gas
44
What is the state of Chlorine (Cl₂) at room temperature?
Gas
45
What is the state of Bromine (Br₂) at room temperature?
Liquid
46
What is the state of Iodine (I₂) at room temperature?
Solid
47
What does "solubility" mean?
Solubility is how much of a substance can dissolve in a liquid (like water) to form a solution. If something is soluble, it can dissolve. If it's non-soluble, it can't dissolve.
48
If something is soluble in water,
it can dissolve in water
49
If something is insoluble in water
it cannot dissolve in water
50
What does "aqueous (aq)" mean?
"Aqueous (aq)" means the substance is dissolved in water, forming a solution.
51
What are the solubility rules for salts?
Salts with alkali metals (Group 1) are soluble.
Salts with ammonium (NH₄⁺) are soluble.
Salts with nitrates (NO₃⁻) are soluble.
52
Are salts with alkali metals soluble in water?
Yes, they are always soluble
53
Are salts with ammonium (NH₄⁺) soluble?
Yes
54
Are salts with nitrate (NO₃⁻) soluble?
Yes
55
Solute
The thing getting dissolved
56
Solvent
The thing that is doing the dissolving
57
Solvent + Solute =
Solution
58
What happens when a solid dissolves in water?
When a solid (like NaCl) is added to water, it dissolves. The solid breaks apart into its individual particles (ions, molecules), and those particles become evenly spread throughout the water, forming an aqueous solution.
59
When does a solid become aqueous?
When it dissolves in water, it turns into an aqueous solution.
60
Precipitate meaning
Something insoluble
61
Ions are held together in the _____ phase but split up in ______
Ions are held together in the solid phase but split up in aqueous solution
62
How do you identify alkali metals?
Alkali metals are in Group 1 of the periodic table, except for hydrogen
63
what type of reaction is it when two aqueous solutions are mixed, but one is insoluble
precipitate reaction
64
Ionic compound is built of
cation and anion
65
Spectator ions
Not involved in the precipitate reaction
66
Net ionic equation
the ions that create a precipitate reaction (aq) (aq) = (s)
67
If a reaction does not yield a precipitate, then
no (real) reaction has occurred - all the ions just sit in solution, and none recombine to form solid products
68
Describe how precipitate reactions work to like a five year old
good job! <3
69
What is the mnemonic for solubility rules?
NAG SAG:
N: Nitrates (NO3-)
A: Acetates (C2H3O2-)
G: Group 1 Metals
S: Sulfates (SO42-)
A: Ammonium (NH4+)
G: Group 17 Halides
Exceptions:
PMS for sulfates and halides:
Lead (Pb2+)
Mercury (Hg22+)
Silver (Ag+)
Castro Bear:
Calcium (Ca2+)
Strontium (Sr2+)
Barium (Ba2+)
70
