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Chemistry 300 > Chemistry 300 - Fall Term > Flashcards

Chemistry 300 - Fall Term Flashcards

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1
Q

SF rule for adding/subtracting?

A

Keep the fewest number of decimal points

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2
Q

SF rule for multiplying/dividing?

A

Keep the fewest number of significant figures

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3
Q

When there is a (blank), trailing zeros are significant

A

decimal point

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4
Q

When there is an imbalance between protons and electrons, the atom is called an

A

ion

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5
Q

Positive Ion (more protons than electrons; positive charge) is called a

A

Cation

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6
Q

Negative ion (more electrons than protons; negative charge) is called a

A

Anion

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7
Q

Carbonate

A

CO₃²⁻

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8
Q

Sulfate

A

SO₄²⁻

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9
Q

Acetate

A

CH₃COO⁻

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10
Q

Bicarbonate (or Hydrogen Carbonate)

A

HCO₃⁻

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11
Q

Hydroxide

A

OH⁻

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12
Q

Nitrate

A

NO₃⁻

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13
Q

Phosphate

A

PO₄³⁻

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14
Q

Ammonium

A

NH₄⁺

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15
Q

Hydrochloric

A

HCl

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16
Q

Nitric

A

HNO₃

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17
Q

Sulfuric

A

H₂SO₄

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18
Q

Acetic

A

CH₃COOH

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19
Q

Baking Soda

A

NaHCO₃

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20
Q

Glucose

A

C₆H₁₂O₆

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21
Q

Hydrogen Peroxide

A

H₂O₂

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22
Q

Sucrose (Table Sugar)

A

C₁₂H₂₂O₁₁

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23
Q

Ammonia

A

NH₃

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24
Q

Empirical Formula Song

A

Percent to mass, mass to mole, divide by small, multiply till whole

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25
Q

Molecular Formula =

A

(empirical formula)n

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26
Q

Mass MF =

A

(Mass EF) n

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27
Q

Ionic Bond =

A

Metal x Non-Metal

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28
Q

Covalent Bond =

A

Non-medal + Non-metal

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29
Q

Bond where u transfer

A

Ionic

30
Q

Type 1 ionic nomenclature is for metals where

A

we know the charge (only one possible charge)

31
Q

Bond where u share

A

Covalent

32
Q

Type 2 ionic nomenclature is for…

A

transition metals (which are special since they can have multiple possible charges) EXCEPT for zinc, silver

33
Q

Type 2 ionic nomenclature is for transition metals though there is an exception with which two metals which are type 1

A

zinc and silver

34
Q

type 3 ionic nomenclature =

A

metal cation (according to type 1 or type 2) and polyatomic anion

35
Q

Percent Water in a Hydrate formula

A

(mass H20/mass hydrate) x 100

36
Q

formula for finding x in a hydrate (x = molecules of water)

A

mol H20/mol anhydrous salt

37
Q

Which diatomic element is a gas at room temperature?

A

H₂ (Hydrogen)
N₂ (Nitrogen)
O₂ (Oxygen)
F₂ (Fluorine)
Cl₂ (Chlorine)

38
Q

Which diatomic element is a liquid at room temperature?

A

Br₂ (Bromine)

39
Q

Which diatomic element is a solid at room temperature?

A

I₂ (Iodine)

40
Q

What is the state of Hydrogen (H₂) at room temperature?

A

Gas

41
Q

What is the state of Nitrogen (N₂) at room temperature?

A

Gas

42
Q

What is the state of Oxygen (O₂) at room temperature?

A

Gas

43
Q

What is the state of Fluorine (F₂) at room temperature?

A

Gas

44
Q

What is the state of Chlorine (Cl₂) at room temperature?

A

Gas

45
Q

What is the state of Bromine (Br₂) at room temperature?

A

Liquid

46
Q

What is the state of Iodine (I₂) at room temperature?

A

Solid

47
Q

What does “solubility” mean?

A

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
Q

If something is soluble in water,

A

it can dissolve in water

49
Q

If something is insoluble in water

A

it cannot dissolve in water

50
Q

What does “aqueous (aq)” mean?

A

“Aqueous (aq)” means the substance is dissolved in water, forming a solution.

51
Q

What are the solubility rules for salts?

A

Salts with alkali metals (Group 1) are soluble.
Salts with ammonium (NH₄⁺) are soluble.
Salts with nitrates (NO₃⁻) are soluble.

52
Q

Are salts with alkali metals soluble in water?

A

Yes, they are always soluble

53
Q

Are salts with ammonium (NH₄⁺) soluble?

A

Yes

54
Q

Are salts with nitrate (NO₃⁻) soluble?

A

Yes

55
Q

Solute

A

The thing getting dissolved

56
Q

Solvent

A

The thing that is doing the dissolving

57
Q

Solvent + Solute =

A

Solution

58
Q

What happens when a solid dissolves in water?

A

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
Q

When does a solid become aqueous?

A

When it dissolves in water, it turns into an aqueous solution.

60
Q

Precipitate meaning

A

Something insoluble

61
Q

Ions are held together in the _____ phase but split up in ______

A

Ions are held together in the solid phase but split up in aqueous solution

62
Q

How do you identify alkali metals?

A

Alkali metals are in Group 1 of the periodic table, except for hydrogen

63
Q

what type of reaction is it when two aqueous solutions are mixed, but one is insoluble

A

precipitate reaction

64
Q

Ionic compound is built of

A

cation and anion

65
Q

Spectator ions

A

Not involved in the precipitate reaction

66
Q

Net ionic equation

A

the ions that create a precipitate reaction (aq) (aq) = (s)

67
Q

If a reaction does not yield a precipitate, then

A

no (real) reaction has occurred - all the ions just sit in solution, and none recombine to form solid products

68
Q

Describe how precipitate reactions work to like a five year old

A

good job! <3

69
Q

What is the mnemonic for solubility rules?

A

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
Q
A

Chemistry 300 (3 decks)

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