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IB Chem 11 > Unit Test 1 > Flashcards

Unit Test 1 Flashcards

1
Q

Accuracy

A

How closely a measured value agrees with the True(Reference) value.

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2
Q

Precision

A

How closely measurements agree with each other - more DPs more precise

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3
Q

How to fix Random Errors?

A

More Trials/Increase Sample Size/More Precise Device

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4
Q

How to Average Values with Uncerts.

A

Avg of Measurements + Avg of Uncerts.

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5
Q

Giga/Mega/Kilo/Deci/Centi/Milli/Micro/Nano

A

9/6/3/-1/-2/-3/-6/-9

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6
Q

Discrete Data

A

Points can be joined - plotted as bar chart

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7
Q

Continuous Data

A

Best fit line can connect data

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8
Q

Coefficient R

A

+1/Perfect Positive Linear
0/No Linear Trend
-1/Perfect Negative Linear

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9
Q

Error Propaagation

A

Slope Uncert.

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10
Q

Tangent

A

Drawn as Large as possible to minimize uncert.

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11
Q

Interpolation

A

Assume Pattern applies between points

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12
Q

Extrapolation

A

Extend Trend Beyond Measurement Range

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13
Q

Matter

A

Mass and Volume

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14
Q

Pure Substances

A

Element or Compound - (Ionic or Molecular)

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15
Q

Mixtures

A

Solutions(Steel and Brass) or Suspensions(Blood) or Mechanical

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16
Q

Extensive Property

A

Depends on Amount - Mass, Volume

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17
Q

Intensive Property

A

Depends of Nature - Density, Melting Point

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18
Q

Distillation

A

For liquid-liquid Solutions - Based on Melting Point
Gas Distilled called Distillate

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19
Q

Solvent Extraction

A

Separating Solid-Solid or Liquid-Liquid mixtures - different solubilities

20
Q

Gravity Seperation

A

Based on Density - Centrifuge

21
Q

Paper/Column Chromatography

A

Pen-Ink Colour Separation
1. Stationary Phase
2. Mobile Phase
3. Developing Solvent

22
Q

Rule for Naming Hydrates

A

Name as Normal - add (prefix) hydrate

23
Q

Rule for Naming Acids

A

Binary Acids: Hydro___ic Acid
Polyatomic Ions: ate-ic ite-ous

24
Q

Laws for Chemical Reactions

A

Law of Conservation of Mass/Energy/Electrical Charge/Atoms

25
Q

Neutralization Reaction

A

Hx + mOH -> H20 + mx

26
Q

Combustion

A

CxHyOz + O2 -> CO2 + H2O

27
Q

Carbonate Reactions

A

Hx + mCO3 -> H2O + CO2 + mx

28
Q

Activity Series Gas

A

F
Cl
Br
I
(As Listed)

29
Q

Empirical Formula (Provides Ratio) Procedure

A
  1. % to grams
  2. grams to moles
  3. divide by smallest
30
Q

Percentage Composition Procedure

A

Molar Mass/Total Molar Mass

31
Q

Molecular Formula Procedure

A

Empirical Formula First
1. Obtain Multiplier - Molar Mass of Compound/Empirical Molar Mass

32
Q

How to obtain Density from Molarity?

A

Density = Molarity times Molar Mass

33
Q

Molarity Procedure

A

Total Moles/Total Volume (L)

34
Q

Dilution Procedure

A

m1v2 = m2v2

35
Q

Charles’s Law

A

Volume is proportional to Temperature

36
Q

Gay-Lussac’s Law

A

Pressure is proportional to Temperature

37
Q

Combined Gas Law

A

P1V1/T1 = P2V2/T2

38
Q

Ideal Gas Law Conditions

A

Pressure - Pa
Volume - m^3
Temperature - Kelvins
R - Gas Constant - 8.31

*K = C + 273.15
1 atm = 101.325kPa
1 bar = 100kPa

*kPa(dm^3) = Pa(m^3)

39
Q

STP Conditions

A

Temperature - 273K - 0C
Pressure - 100 kPa - 1 bar

40
Q

Ideal Gas Law vs Combined Gas Law?

A

Combined Gas Law - Changing Conditions
Ideal Gas Law - Same Gas, Solving for Unknown

41
Q

Limiting/Excess Procedure

A

*Get How much excess left - use reagent side stoich

Use all given with stoich to convert to specified/chosen product - least product produced is LIMITING

42
Q

Percentage Yield

A

Actual(Experiment)/Theory

43
Q

Percent Purity

A

Pure Amount/Total Amount

44
Q

Titration Setup

A

Base (Titrant) on top (In Burette with high precision - 2 dp)
Acid with Indicator on bottom

45
Q

What is a Primary Standard and what to do with it?

A

Chemicals that are stable, pure, and non-hygroscopic (does not absorb water)

  1. Titrate the Titrant
  2. Use known Molarity for Actual Titration

IB Chem 11 (2 decks)

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