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CHEM 120 > Module 1 > Flashcards

Module 1 Flashcards

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1
Q

IUPAC

A

International Union of Pure and Applied Chemistry. The world’s head on everything regarding chemistry formatting ex. naming, units, values, etc. International Federation. Makes sure chemistry is universal.

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2
Q

CAS

A

Chemical Abstract Services. A database containing information about elements’ properities.

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3
Q

Alkali Metals

A

Group 1

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4
Q

Alkaline Earth Metals

A

Group 2

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5
Q

Transition Metals

A

Groups 3 - 12

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6
Q

Halogens

A

Group 17

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7
Q

Noble Gases

A

Group 18

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8
Q

Lanthanoids

A

Top row of the bottom two rows.

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9
Q

Actinoids

A

Bottom row of the bottom two rows.

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10
Q

Synthesis

A

A + B —> C OR A + B —> C + D

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11
Q

Decomposition

A

A —> B + C

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12
Q

Single Displacement

A

AB + C —> BC + A

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13
Q

Double Displacement

A

AB + CD —> AC + BD

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14
Q

Combustion

A

CxHy + O2 —> CO2 + H2O

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15
Q

Acid-Base

A

Acid + Base —> Salt + Water

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16
Q

Solution

A

A homogeneous mixture in which one or more solutes are dissolved in a solvent.

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17
Q

Aqueous Solutions

A

Have water as the solvent.

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18
Q

Ionic Compounds

A

Consist in positive and negative ions in a crystal lattice. Ions are bonded by ionic bonds. Ex. NaCl.

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19
Q

Molecular Compounds

A

Stable, neutral molecules held by covalent bonds. Ex. H2O, CCl4, CO2.

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20
Q

Precipitation Reactions

A

The ions in the solution form a solid, ie. a precipitate.

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21
Q

Gravimetric/Gravitational Analysis

A

The amount of substance in a sample is concluded by the mass of the precipitate that is formed, ie. how much product was formed.

22
Q

Solubility Guidelines for Ionic Compounds Rule 1

A

Salts of alkali metals, group 1, are soluble. Ex. NaCl, KNO3.

23
Q

Solubility Guidelines for Ionic Compounds Rule 2

A

Ammonium, NH4+, salts are soluble. Ex. NH4Cl, (NH4)2SO4.

24
Q

Solubility Guidelines for Ionic Compounds Rule 3

A

Nitrates, NO3-, are soluble. Ex. AgNO3, Zn(NO3)2.

25
Q

Solubility Guidelines for Ionic Compounds Rule 4

A

Chlorides, Cl-, bromides, Br-, and iodides, I-, are soluble except when paired with lead, Pb^2+, mercury, Hg+ and Hg2^2+, and silver, Ag+. Ex. ZnCl2 is soluble but PbCl2 is not soluble.

26
Q

Solubility Guidelines for Ionic Compounds Rule 5

A

Sulfates, SO4^2-, are soluble except when paired with calcium, Ca^2+, strontium, Sr^2+, barium, Ba^2+, silver, Ag2+, mercury, Hg2+ and Hg^2+, and lead, Pb^2+. Ex. Na2SO4 is soluble but CaSO4 is not.

27
Q

Solubility Guidelines for Ionic Compounds Rule 6

A

Carbonates, CO3^2-, phosphates, PO4^3-, and sulfides, S^2-, are insoluble expect when paired with:
i) alkalis (Rule 1)
ii) ammonium (Rule 2)

28
Q

Solubility Guidelines for Ionic Compounds Rule 7

A

Hydroxides, OH-, are insoluble/slightly soluble expect when paired with alkalis (Rule 1). Note: the hydroxides of group 2, alkaline earth metals, are slightly soluble.

29
Q

Full Molecular Equation

A

The full balanced chemical equation.

30
Q

Net Ionic Equation

A

The balanced chemical equation not including the spectator ions.

31
Q

Brønsted-Lowry Acid-Base

A

The acid is a proton (H+) donor and the base is a proton (H+) acceptor. The proton is transferred from the acid to the base.

32
Q

Protonated

A

An acid produces H3O+ ions when dissolved in water.

33
Q

De-protonated

A

A base produces OH- ions when dissolved in water.

34
Q

Strong Acids

A

Completely ionizes in water.

35
Q

Strong Bases

A

Completely ionizes in water.

36
Q

Common Strong Acids

A

HCl - hydrochloric acid
HBr - hydrobromic acid
HI - hydroiodic acid
HClO4 - perchloric acid
HBrO4 - perbromic acid
HIO4 - periodic acid
HNO3 - nitric acid
H2SO4 - sulfuric acid

37
Q

Common Strong Bases

A

Group 1 + 2 hydroxides
Hydride, H-, ions
Oxide, O^2-, ions

38
Q

Diprotic

A

Ionizes twice. Ex. H2SO4.

39
Q

Mole (mol)

A

The SI unit for the amount of substance.

40
Q

Avogadro’s Number

A

1 mol = 6.022 x 10^23 particles

41
Q

Molar Mass (Mr)

A

The mass in g of 1.0 mol of a substance.

42
Q

Molecular Formula

A

Mr molecular = x(Mr empirical)

43
Q

Theoretical Yield

A

The maximum amount of products that can be produced.

44
Q

Limiting Reactant/Reagent

A

The species that limits the amount of product that can form (the one that “runs out” first).

45
Q

% Yield

A

% Yield = (actual yield/theoretical yield) x 100%

46
Q

Consecutive Reactions

A

A series of reactions that occur sequentially. The products from one reaction are consumed as reactants in a subsequent reaction. Can add the reactions together to obtain the overall reaction.

47
Q

Simultaneous Reactions

A

Reactions that are independent and occur at the same time. Are used in the analysis of chemical mixtures. Can’t add together.

48
Q

Intermediate

A

A species produced in one step and consumed in a subsequent step. Never appears in the overall equation. May need to be multiplied by a coefficient to cancel it out.

49
Q

Green Chemistry

A

An approach to chemistry that is intentionally focused on not only the efficient use of atoms (and energy) but also chemical methods that reduce or eliminate reagents, products, solvents, by-products, wastes, etc. that are hazardous to human health or the environment.

50
Q

% Atom Economy

A

(stoichiometric mass of the desired product/sum of the stoichiometric mass of the reactants) x 100%

51
Q

Stoichiometric Mass

A

stoichiometric coefficients x molar mass

52
Q

E-factor (Environmental Factor)

A

mass of waste produce (minus water)/mass of product obtained

CHEM 120 (7 decks)

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