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AP Chemistry > Ch 1, 2, 3 Review > Flashcards

Ch 1, 2, 3 Review Flashcards

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1
Q

Subscripts in Chemical Formulas

A

tell number of atoms of an element in a compound

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2
Q

Coefficients in Chemical Formulas

A

tell number of molecules of the compound

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3
Q

Law of Multiple Proportions

A

when two elements form multiple compounds, you can find the ratio of each compounds’ masses and there will be a common whole number ratio between those ratios

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4
Q

Isotopes and number of protons

A

The number of protons in an element never changes; given carbon-26, we know that there are 12 carbon protons and therefore there are 14 neutrons in this isotope

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5
Q

Ionic vs Molecular Compounds

A

Ionic is between metal and nonmetal; a Molecular is between two nonmetals, aka Covalent

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6
Q

Covalent Compounds

A

formed by two nonmetals sharing electrons

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7
Q

Naming Ionic Compounds

A

metals with nonmetals; metal name + (IV) if a transition metal + nonmetal name + -ide

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8
Q

Naming Covalent Compounds

A

nonmetals with nonmetals; prefix based on number + first nonmetal (-ion charge) + prefix based on number + other nonmetal + -ide

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9
Q

Prefixes for naming covalent compounds

A

mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca

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10
Q

Naming acids

A

When there is no oxygen involved: Hydro + root+ -ic
When there is oxygen: root of polyatomic + -ic/-ous
-ate becomes -ic, -ite becomes -ous

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11
Q

Calculating Number of Atoms or Molecules

A

multiply moles by Avogadros number

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12
Q

Percent Composition in a Compound

A

Molar Mass of Element looking for/ Total Molar Mass of Compound

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13
Q

How to calculate empirical formula from percent composition

A

Assume you have 100gs of solution and convert percents into masses. Convert masses to moles using the molar mass. Divide all moles by the lowest mole quantity to get the ratio.

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14
Q

Combustion Analysis: Empirical

A

Take product mass and convert to moles. Convert to moles of reactant (if looking for C moles, use CO2 as the product you focus on). Convert to mass. Repeat for all reactants. Using conservation of mass, solve for unknown mass. Find lowest moles and divide to get a common ratio.

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15
Q

Formula Weights vs Molar Mass vs Molecular Weight

A

same number, different units. in amu. the formula weight of a compound is it’s molar mass just in amu instead of g/mol; formula weight is for ionic compounds, molecular weight is for molecular compounds

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16
Q

Mass of n moles of an element

A

n*the element’s molar mass

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17
Q

Percent Error

A

abs(actual-theoretical)/theoretical

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18
Q

prefix hypo

A

means that it’s a polyatomic ion and it has one fewer oxygen than the -ite form of the ion.

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19
Q

prefix per

A

means that it’s polyatomic ion and it has one more oxygen than the -ate form of the ion

20
Q

Avogadro’s Number

A

6.022e23

21
Q

W

A

Tungsten

22
Q

Sb

A

Antimony

23
Q

Zr

A

Zirconium

24
Q

Pu

A

Plutonium

25
Q

Pt

A

Platinum

26
Q

Mercury (I)

A

Hg2

Charge: +1

27
Q

Mercury (II)

A

Hg2

Charge: +2

28
Q

Acetate

A

C2H3O2

Charge: -1

29
Q

Nitrate

A

NO3

Charge: -1

30
Q

Carbonate

A

CO3

Charge: -2

31
Q

Hydrogen Carbonate

A

HCO3

Charge: -1

32
Q

Dichromate

A

Cr2O7

Charge: -2

33
Q

Chromate

A

Cr2O4

Charge:-2

34
Q

Oxalate

A

C2O4

Charge: -2

35
Q

Peroxide

A

O2

Charge: -2

36
Q

Charges on the periodic table

A

+1,+2,+3 …, -3, -2, -1

37
Q

Copper Charge

A

+1, +2

38
Q

Gold Charge

A

+1, +3

39
Q

Silver Charge

A

+1

40
Q

Thallium Charge

A

+1, NOT +3

41
Q

Cobalt Charge

A

+2, +3

42
Q

Iron Charge

A

+2, +3

43
Q

Lead Charge

A

+2, +4

44
Q

Manganese Charge

A

+2, +4

45
Q

Nickel Charge

A

+2, +3

46
Q

Bismuth Charge

A

+3

47
Q

Chromium Charge

A

+3

AP Chemistry (8 decks)

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