Data BookletSC

IENC

E

Table of Contents

1

2

2

3

3

4

4

6

8

9

9

10

12

12

Miscellaneous Kinematics and Dynamics Formulas Gravitational and Electrical Fields Electricity Waves Electrochemistry Thermodynamics Periodic Chart of the Elements and Ions Nuclear Chemistry Organic Chemistry Solutions Acids and Bases Genetics Scoring Guides

2

Miscellaneous

Data and Formulas solar constant = 1353 watts/m2

% efficiency = outputinput × 100

% error = valueltheoretica

valueltheoreticavaluealexperiment − × 100

magnification = power ofocular lens ×

power ofobjective lens

speed of light = c = 3.00 × 108 m/s

1 light year = 9.47 × 1015 m

1 AU = astronomical unit

1 AU = 1.50 × 1011 m

slope = riserun =

x

y

∆∆

= 12

12

xx

yy

−−

Some Non-SI Units Used with SI

Quantity Unit Name Symbol Definition

Time minute hour day year

min h d a

1 min = 60 s 1 h = 3 600 s 1 d = 86 400 s 1 a = 31 557 600 s

Area hectare ha 1 ha = 1 hm2 = 10 000 m2

Volume litre L 1 L = 1000 cm3 Mass metric ton

or tonne t 1 t = 1 000 kg

= 1 Mg Pressure standard

atmosphere atm 1 atm = 101.325 kPa

A System of Prefixes

Prefix Symbol Factor by Which Base Unit is Multiplied

exa E 1 000 000 000 000 000 000 = 1018 peta P 1 000 000 000 000 000 = 1015 tera T 1 000 000 000 000 = 1012 giga G 1 000 000 000 = 109

*mega M 1 000 000 = 106 *kilo k 1000 = 103 hecto h 100 = 102 deca da 10 = 101 deci d 0.1 = 10–1 centi c 0.01 = 10–2

*milli m 0.001 = 10–3 *micro µ 0.000 001 = 10–6 nano n 0.000 000 001 = 10–9 pico p 0.000 000 000 001 = 10–12 femto f 0.000 000 000 000 001 = 10–15 atto a 0.000 000 000 000 000 001 = 10–18

*most commonly used

3

Kinematics and Dynamics Formulas

t

dv =

t

vva if −

=

amF =net

W = Fd

P = Wt

Fc = mv2

r

2i 2

1tatvd +=

tvv

d

+

=2

fi

vmp =

amt

p =∆∆

′+′=+ 22112211 vmvmvmvm

Ep = mgh

Ek = 12 mv2

v = velocity (m/s)

v = speed (m/s)

d = displacement (m)

d = distance (m)

t = time elapsed (s)

a = acceleration (m/s2)

F = force (kg•m/s2 or N)

m = mass (kg)

W = work (N•m or J)

P = power (J/s or W)

Fc = magnitude of centripetal force (N)

r = radius (m)

p = momentum (kg•m/s)

Ep = gravitational potential energy (J)

g = magnitude of acceleration due to gravity (9.81 m/s2)

h = height (m)

Ek = kinetic energy (J)

Gravitational and Electrical Fields

Fg = Gm1m2

r2

gmF =g

g = Gm1

r2

Fe = kq1q2

r2

qF

E e=

d

V

r

kqE ==

21

Fg = magnitude of force due to gravity (N)

m = mass (kg)

G = gravitational constant = 6.67 × 10–11 N•m2/kg2

r = centre-to-centre distance (m)

g = acceleration due to gravity = 9.81 m/s2 or 9.81 N/kg

Fe = magnitude of force between two electrostatic charges (N)

k = Coulomb’s law constant = 8.99 × 109 N•m2/C2

q = electrostatic charge in coulombs (C)

E = electric field strength (N/C) or (V/m)

Related values:

Mass of Earth = 5.97 × 1024 kg Radius of Earth = 6.37 × 106 m

Mass of Sun = 1.99 × 1030 kg Elementary charge = 1.60 × 10–19 C (charge of a proton or electron)

4

Electricity Formulas For resistances connected in series RT = R1 + R2 + R3 + ... Rn

For resistances connected in parallel 1

RT =

1R1

+ 1R2

+ 1R3

+ ... 1Rn

P = IV = I2R = V2

R

V = IR

E = Pt Transformers

Np

Ns =

Vp

Vs =

Is

Ip

R = resistance in ohms (Ω)

P = power (watts)

I = current in amperes (A)

V = voltage in volts (V)

E = energy (J)

t = time in seconds (s)

N = number of turns

p = primary

s = secondary

Output Voltage × Primary Turns = Input Voltage × Secondary Turns Output Current × Secondary Turns = Input Current × Primary Turns

Related values: 1 kW•h = 3.60 × 106 J

Waves Wave Formula v = ƒλ v = speed of wave (m/s) ƒ = frequency (/s or Hz) λ = wavelength (m) Electromagnetic Spectrum

103 105 107 109 1011 1013 1015 1017 1019 1021 1023

104 102 1 10−2 10−4 10−6 10−8 10−10 10−12 10−14

Longwave (Radio) Shortwave

Wavelength (metres)

Frequency (Hertz)

X-Rays

Gamma rays

TV

Micro-wave

400 nm700 nm

O

Vis

(Visible light)

Y G B I VR

UVIR

Note: Speed of EMR = 3.00 × 108 m/s

5

Electrochemistry Activity Series (for 1.0 mol/L solution at 25°C)

Reduction Half-Reaction

Met

al i

ons

get

mor

e st

able

Au3+(aq)

Ag+(aq)

Hg2+(aq)

Cu2+(aq)

2H+(aq)

Pb2+(aq)

Sn2+(aq)

Ni2+(aq)

Cd2+(aq)

Fe2+(aq)

Cr2+(aq)

Zn2+(aq)

Al3+(aq)

Mg2+(aq)

Na+(aq)

Ca2+(aq)

Li+(aq)

+ + + + + + + + + + + + + + + + +

3e–

2e–

e–

2e–

2e–

2e–

2e–

2e–

2e–

2e–

2e–

2e–

3e–

2e–

e–

2e–

e–

→ → → → → → → → → → → → → → → → →

Au(s) Ag(s) Hg(l) Cu(s) H2(g) Pb(s)

Sn(s) Ni(s) Cd(s) Fe(s) Cr(s) Zn(s) Al(s) Mg(s) Na(s) Ca(s) Li(s)

Metal atom

s get more stable

Thermodynamics Heat Capacities of Some Common Compounds

Compound Specific Heat Capacity (J/g°C) or kJ/kg°C Water (liquid) 4.19 Methanol 2.55 Ethanol 2.46 Hexane 2.26 Water (solid) 2.01 Water (gas) 2.01 Toluene 1.80 Sulphuric acid 1.13

Heats of Fusion of Various Substances

Substances Heat of Fusion (J/g) or kJ/kg Water 333 Sulphuric acid 163 Hexane 152 Ethanol 109 Methanol 100 Toluene 72

Heats Of Vaporization Of Various Substances

Substances Heat of Vaporization (J/g) or kJ/kg Water 2260 Methanol 1076 Ethanol 855 Sulphuric acid 510 Toluene 363 Hexane 335

Pa5+

protactinium (V)

Pa4+

protactinium (IV)

Ion charge

Stock name (IUPAC)

Symbol of ion

Am3+

americium (III) Am4+

americium (IV)

Eu3+

europium (III) Eu2+

europium (II)

Pt4+

platinum (IV) Pt2+

platinum (II)

Pd2+

palladium (II) Pd4+

palladium (IV)

Ni2+

nickel (II) Ni3+

nickel (III)

28

nickel58.71

Ni

46

palladium106.40

Pd

78

platinum195.09

Pt

64

gadolinium157.25

Gd

96 curium(247.07)

Cm

Cm3+

curium

Gd3+

gadolinium

Au3+

gold (III) Au+

gold (I)

Ag+

silver

Cu2+

copper (II) Cu+

copper (I)

29

copper63.55

Cu

47

silver107.87

Ag

79

gold196.97

Au

65

terbium158.93

Tb

97 berkelium(247.07)

Bk

Bk3+

berkelium (III) Bk4+

berkelium (IV)

Tb3+

terbium

Hg2+

mercury (II) Hg+

mercury (I)

Cd2+

cadmium

Zn2+

zinc

30

zinc65.38

Zn

48

cadmium112.41

Cd

80

mercury200.59

Hg

66

dysprosium162.50

Dy

98 californium(242.06)

Cf

Cf3+

californium

Dy3+

dysprosium

TI+ thallium (I) TI3+

thallium (III)

In3+

indium

Ga3+

gallium

Al3+

aluminium

5

boron10.81

B

13

aluminum26.98

Al

31

gallium69.72

Ga

49

indium114.82

In

81

thallium204.37

Tl

67

holmium164.93

Ho

99 einsteinium(252.08)

Es

Es3+

einsteinium

Ho3+

holmium

Pb2+

lead (II) Pb4+

lead (IV)

Sn4+

tin (IV) Sn2+

tin (II)

Ge4+

germanium

6

carbon12.01

C

14

silicon28.09

Si

32

germanium72.59

Ge

50

tin118.69

Sn

82

lead207.19

Pb

68

erbium167.26

Er

100 fermium(257.10)

Fm

Fm3+

fermium

Er3+

erbium

Bi3+

bismuth (III) Bi5+

bismuth (V)

Sb3+

antimony (III) Sb5+

antimony (V)

As3–

arsenide

P3–

phosphide

N3–

nitride

7

nitrogen14.01

N

15

phosphorus30.97

P

33

arsenic74.92

As

51

antimony121.75

Sb

83

bismuth208.98

Bi

69

thulium168.93

Tm

101 mendelevium(258.10)

Md

Md2+

mendelevium (II) Md3+

mendelevium (III)

Tm3+

thulium

Po2+

polonium (II) Po4+

polonium (IV)

Te2–

telluride

Se2–

selenide

S2–

sulphide

O2–

oxide

8

oxygen16.00

O

16

sulphur32.06

S

34

selenium78.96

Se

52

tellurium127.60

Te

84

polonium(208.98)

Po

70

ytterbium173.04

Yb

102 nobelium(259.10)

No

No2+

nobelium (II) No3+

nobelium (III)

Yb3+

ytterbium (III) Yb2+

ytterbium (II)

At– astatide

I–

iodide

Br–

bromide

Cl– chloride

F–

fluoride

H–

hydride

9

fluorine19.00

F

17

chlorine35.45

Cl

35

bromine79.90

Br

53

iodine126.90

I

85

astatine(209.98)

At

71

lutetium174.97

Lu

103 lawrencium(260.11)

Lr

Lr3+

lawrencium

Lu2+

lutetium

2 helium4.00

He1 hydrogen1.01

H

10

neon20.17

Ne

18 argon39.95

Ar

36 krypton83.80

Kr

Xe

86 radon(222)

Rn

Cs+

cesium

Rb+

rubidium

K+

potassium

Na+

sodium

Li+ lithium

H+

hydrogen

1

hydrogen1.01

H

3

lithium6.94

Li

11

sodium22.99

Na

19

potassium39.10

K

37

rubidium85.47

Rb

55

cesium132.91

Cs

87

francium(223.02)

Fr

Ba2+

barium

Sr2+

strontium

Ca2+

calcium

Mg2+

magnesium

Be2+

beryllium

Y3+

yttrium

Sc3+

scandium

57

lanthanum138.91

La

89

actinium(277.03)

Ac

Ac3+

actinium

La3+

lanthanum

Hf4+

hafnium

Zr4+

zirconium

Ti4+

titanium (IV) Ti3+

titanium (III)

22

titanium47.90

Ti

40

zirconium91.22

Zr

72

hafnium178.49

Hf

104 unnilquadium(266.11)

Unq

58

cerium140.12

Ce

90

thorium(232.04)

Th

Th4+

thorium

Ce3+

cerium

Ta5+

tantalum

Nb5+

niobium (V) Nb3+

niobium (III)

V5+

vanadium (V) V4+

vanadium (IV)

23

vanadium50.94

V

41

niobium92.91

Nb

73

tantalum180.95

Ta

105 unnilpentium(262.11)

Unp

59

praseodymium140.91

Pr

91

protactinium(231.04)

Pa

Pa5+

protactinium (V) Pa4+

protactinium (IV)

Pr3+

praseodymium

W6+

tungsten

Mo6+

molybdenum

Cr3+

chromium (III) Cr2+

chromium (II)

24

chromium52.00

Cr

42

molybdenum95.94

Mo

74

tungsten183.85

W

106 unnilhexium(263.12)

Unh

60

neodymium144.24

Nd

92

uranium238.03

U

U6+

uranium (VI) U4+

uranium (IV)

Nd3+

neodymium

Re7+

rhenium

Tc7+

technetium

Mn2+

manganese (II) Mn4+

manganese (IV)

25

manganese54.94

Mn

43

technetium(98.91)

Tc

75

rhenium186.21

Re

107 unnilseptium(262.12)

Uns

61 promethium(144.91)

Pm

93

neptunium(237.05)

Np

Np5+

neptunium

Pm3+

promethium

Os4+

osmium

Ru3+

ruthenium (III) Ru4+

ruthenium (IV)

Fe3+

iron (III) Fe2+

iron (II)

26

iron55.85

Fe

44

ruthenium101.07

Ru

76

osmium190.20

Os

108 unniloctium(265)

Uno

62

samarium150.35

Sm

94

plutonium(244.06)

Pu

Pu4+

plutonium (IV) Pu6+

plutonium (VI)

Sm3+

samarium (III) Sm2+

samarium (II)

Ir4+

iridium

Rh3+

rhodium

Co2+

cobalt (II) Co3+

cobalt (III)

27

cobalt58.93

Co

45

rhodium102.91

Rh

77

iridium192.22

Ir

109 unnilennium(266)

Une

63 europium151.96

Eu

95

americium(243.06)

Am

Fr+

francium

Ra2+

radium

18

VIIIA or O

17

VIIA

16

VIA

15

VA

14

IVA

13

IIIA

12

IIB

11

IB

7

VIIB

6

VIB

5

VB

4

IVB

3

IIIB

2

IIA

1

IA

109

VIIIB

8

Periodic Chart of the Elements and Ions

Table of Polyatomic Ions and Elementsacetate

ammonium

benzoate

borate

carbonate

hydrogen carbonate

chlorate

hypochlorite

chromate

dichromate

cyanide

hydroxide

nitrate

nitrite

permanganate

phosphate

hydrogen phosphate

dihydrogen phosphate

silicate

sulphate

CH3COO–

NH4+

C6H5COO–

BO33–

CO32–

HCO3–

CIO3–

CIO–

CrO42–

Cr2O72–

CN–

OH–

NO3–

NO2–

MnO4–

PO43–

HPO42–

H2PO4–

SiO32–

SO42–

sulphite

hydrogen sulphide

hydrogen sulphate

hydrogen sulphite

SO32–

HS –

HSO4–

HSO3–

astatine

bromine

chlorine

fluorine

hydrogen

At2

Br2

Cl2

F2

H2

iodine

nitrogen

oxygen

phosphorus

sulphur

I2

N2

O2

P4

S8

Note: The legend at the right denotes the physical state of the elements at 101.325 kPa and 298.15 K (25ºC)

LiquidSolid

Legend for the elements

91

protactinium231.04

Pa Symbol of the elementAtomic number

Name of the elementAtomic mass

Key

Based on 126 C

Most stable or common ion is listed above dotted line( ) Indicates mass of the most stable isotope

4

beryllium9.01

Be

12

magnesium24.31

Mg

20

calcium40.08

Ca

38

strontium87.62

Sr

56

barium137.33

Ba

88

radium(226.03)

Ra

21

scandium44.96

Sc

39

yttrium88.91

Y

57-71

89-103

Seldom forms ionsGas

C carbon

B boron

Si silicon

54 xenon131.30

Ar argon

He helium

Xe xenon

Rn radon

Ne neon

Kr krypton

6 7

ElementsPolyatomic ions

8

Standard Heats of Formation at 298.15 K (25°C)

Name Formula H°f(kJ/mol)

ammonia benzene butane calcium carbonate

NH3(g) C6H6(l) C4H10(g) CaCO3(s)

– 46.1 +49.0

–126.5 –1206.9

calcium hydroxide carbon dioxide carbon monoxide

Ca(OH)2(s) CO2(g) CO(g)

–986.1 –393.5 –110.5

ethane ethanoic acid (acetic acid) ethanol ethene (ethylene) ethyne (acetylene)

C2H6(g) CH3COOH(l) C2H5OH(l) C2H4(g) C2H2(g)

–84.7 – 484.5 –277.1 +52.3

+226.7

glucose hydrogen sulphide

C6H12O6(s) H2S(g)

–1273.1 –20.6

methanal (formaldehyde) methane

CH2O(g) CH4(g)

–115.9 –74.8

methanol octane

CH3OH(l) C8H18(l)

–239.0 –250.0

pentane propane sucrose

C5H12(l) C3H8(g) C12H22O11(s)

–146.4 –103.8 –2225.5

sulphur dioxide sulphur trioxide (vapor) water (liquid) water (vapor)

SO2(g) SO3(g) H2O(l) H2O(g)

–296.8 –395.7 –285.8 –241.8

Note: ∆Hof for elements is zero

Energy Formulas

Q = mc∆t

∆Hfus = Qm

∆Hvap = Qm

∆H = ∑H°f (products) – ∑H°

f (reactants)

∆E = ∆mc2 (c = 3.00 × 108 m/s)

Q = quantity of heat energy (kJ)

m = mass (kg)

c = specific heat capacity (kJ/kg°C)

∆t = change in temperature (°C)

∆Hfus = heat of fusion (kJ/kg)

∆Hvap = heat of vaporization (kJ/kg)

∆H = change in heat (kJ)

°fH = standard heat of formation (kJ/mol)

∑ = the sum of

∆E = change in energy (J)

9

Nuclear Chemistry

Masses of Selected Nuclides and Subatomic Particles

Nuclide or Particle Mass (10–3 kg/mol)

Nuclide or Particle Mass (10–3 kg/mol)

electron 01− e 0.000 549 sulphur–31 31

16 S 30.970 77

positron 01+ e 0.000 549 potassium– 4 0 40

19 K 39.953 57

proton 11 H 1.007 28 rubidium–90 90

37 Rb 89.894 27

neutron 10 n 1.008 67 krypton–92 92

36 Kr 91.906 01

deuterium 21 H 2.013 55 strontium–95 95

38 Sr 94.898 47

helium–3 32 He 3.014 93 ruthenium–107 107

44 Ru 106.885 98

tritium 31 H 3.015 50 barium–141 141

56 Ba 140.883 40

alpha particle (helium nucleus)

42 He 4.001 50 cesium–144 144

55 Cs 143.901 18

beryllium–7 74 Be 7.014 70 lanthanum–146 146

57 La 145.894 14

beryllium–8 84 Be 8.003 11 lead–206 206

82 Pb 205.929 5

boron–8 85 B 8.021 86 lead–208 208

82 Pb 207.931 6

nitrogen–13 137 N 13.001 90 polonium–210 210

84 Po 209.936 8

nitrogen–14 147 N 13.999 231 polonium–218 218

84 Po 217.962 8

carbon–14 146 C 13.999 95 radon–222 222

86 Rn 221.970 3

oxygen–15 158 O 14.998 67 radium–226 226

88 Ra 225.977 1

fluorine–17 179 F 16.997 15 thorium–230 230

90 Th 229.983 7

neon–20 2010 Ne 19.986 95 uranium–235 235

92 U 234.993 4

phosphorus–31 3115 P 30.965 53 plutonium–239 239

94 Pu 239.000 6

Elements For Radioactive Dating

Radioisotope Approximate Half-life (a) Decay Product

146 C (carbon–14) 5.73 × 103 14

7 N (nitrogen–14)

4019 K (potassium–40) 1.28 × 109 40

18 Ar (argon–40)

8737 Rb (rubidium–87) 4.86 × 1010 87

38 Sr (strontium–87)

23592 U (uranium–235) 7.13 × 108 207

82 Pb (lead–207)

23892 U (uranium–238) 4.51 × 109 206

82 Pb (lead–206)

10

Organic Chemistry Homologous Series of Alkanes (state at room temperature and pressure)

Name Chemical Formula methane ethane propane butane pentane hexane heptane octane nonane decane

CH4(g) C2H6(g) C3H8(g) C4H10(g) C5H12(l) C6H14(l) C7H16(l) C8H18(l) C9H20(l) C10H22(l)

Prefixes for Molecular Compounds 1 = mono- 6 = hexa- 2 = di- 7 = hepta- 3 = tri- 8 = octa- 4 = tetra- 9 = ennea- (nona-) 5 = penta- 10 = deca-

Functional Groups

alcohol

aldehyde

carboxylic acid

ketone

ester

halide

polymers

R— O – H

R— C O

H

R— C O

O – H

R— C

O

– R′

R— C O

O – R′

R — Q

- - - ( x – y )n- - -

R is usually a carbon groupQ stands for a halogenx-y is a monomer unit

=–

=–

=–

=

Organic Functional Groups

Solutions Solubility of Some Common Ionic Compounds in Water at 298.15 K (25°C) Ion

Group 1 NH4

+

H+(H3O+)

ClO3–

NO3–

ClO4–

CH3COO–

Cl– Br–

I–

SO4

2–

S2–

OH–

PO43–

SO32–

CO32–

Solubility greater than or equal to 0.1 mol/L (very soluble)

all all most most most Group 1 Group 2

NH4+

Group 1

NH4+

Sr2+

Ba2+

Tl+

Group 1

NH4+

Solubility less than 0.1 mol/L (slightly soluble)

none none Ag+

Ag+

Pb2+

Hg+

Cu+

Tl+

Ca2+

Sr2+

Ba2+

Ra2+

Pb2+

Ag+

most most most

11

Stoichiometry and Solution Formulas

n = mM

C = nV

C1V1 = C2V2

nr = ng × coefficientrcoefficientg

C = concentration (mol/L)

m = mass (g)

M = molar mass (g/mol)

n = number of moles (mol)

V = volume (L)

r = required substance

g = given substance

Ways of Expressing Concentration

Moles per Litre (mol/L)

Parts per Million (ppm)

Percent Mass/Volume (% m/V)

Percent by Volume (% V/V)

solutionL

solutemol 610

solutiong

soluteg×

solutionmL

soluteg × 100

solutionmL

solutemL× 100

Colour Chart of Common Aqueous Ions

Ion Symbol Colour

chromate chromium(III) chromium(II) cobalt(II) copper(I) copper(II) dichromate iron(II) iron(III) manganese(II) permanganate

CrO42–

Cr3+ Cr2+ Co2+ Cu+ Cu2+ Cr2O7

2– Fe2+ Fe3+ Mn2+ MnO4

–

yellow green blue pink green blue orange pale green pale yellow pale pink purple

Acids and Bases Acid Formulas pH = –log10[H3O+

(aq)] [H3O+(aq)] = antilog10[–pH]

IUPAC Rules for Naming Acids

Example Ionic Name Acid Name Formula Ionic Name Acid Name

hydrogen --ide hydro--ic acid HCl(aq) hydrogen chloride hydrochloric acid

hydrogen --ate --ic acid H3PO4(aq) hydrogen phosphate phosphoric acid

hydrogen --ite --ous acid H3PO3(aq) hydrogen phosphite phosphorous acid

12

Relative Strengths of Acids and Bases at 0.10 mol/L and 298.15 K (25°C) Acid Name Acid Formula Conjugate Base Formula

hydrochloric acid

sulphuric acid

nitric acid

HCl(aq)

H2SO4(aq)

HNO3(aq)

Cl–(aq)

HSO4–

(aq)

NO3–

(aq)

hydronium ion H3O+(aq) H2O(l)

oxalic acid

sulphurous acid (SO2 + H2O)

hydrogen sulphate ion

phosphoric acid

orange IV

nitrous acid

hydrofluoric acid

methanoic acid

methyl orange

benzoic acid

ethanoic (acetic) acid

carbonic acid (CO2 + H2O)

bromothymol blue

hydrosulphuric acid

phenolphthalein

boric acid

ammonium ion

hydrogen carbonate ion

indigo carmine

HOOCCOOH(aq)

H2SO3(aq)

HSO4–

(aq)

H3PO4(aq)

HOr(aq)

HNO2(aq)

HF(aq)

HCOOH(aq)

HMo(aq)

C6H5COOH(aq)

CH3COOH(aq)

H2CO3(aq)

HBb(aq)

H2S(aq)

HPh(aq)

H3BO3(aq)

NH4+

(aq)

HCO3–

(aq)

HIc(aq)

HOOCCOO–(aq)

HSO3–

(aq)

SO42–

(aq)

H2PO4–

(aq)

Or–(aq)

NO2–

(aq)

F–(aq)

HCOO–(aq)

Mo–(aq)

C6H5COO–(aq)

CH3COO–(aq)

HCO3–

(aq)

Bb–(aq)

HS–(aq)

Ph–(aq)

H2BO3–

(aq)

NH3(aq)

CO32–

(aq)

Ic–(aq)

water (55.5 mol/L) H2O(l) OH–(aq)

Acid-Base Indicators at 298.15 K (25°C)

Indicator

Abbreviation

pH Range

Colour Change As pH Increases

methyl violet thymol blue thymol blue orange IV methyl orange bromocresol green litmus methyl red chlorophenol red bromothymol blue phenol red phenolphthalein thymolphthalein alizarin yellow R indigo carmine 1,3,5–trinitrobenzene

HMv H2Tb HTb– HOr HMo HBg HLt HMr HCh HBb HPr HPh HTh HAy HIc HNb

0.0 – 1.6 1.2 – 2.8 8.0 – 9.6 1.4 – 2.8 3.2 – 4.4 3.8 – 5.4 4.5 – 8.3 4.8 – 6.0 5.2 – 6.8 6.0 – 7.6 6.6 – 8.0 8.2 – 10.0 9.4 – 10.6 10.1 – 12.0 11.4 – 13.0 12.0 – 14.0

yellow to blue red to yellow yellow to blue red to yellow red to yellow yellow to blue red to blue red to yellow yellow to red yellow to blue yellow to red colorless to pink colorless to blue yellow to red blue to yellow colorless to orange

13

Genetics

Scoring Guides

Scoring Guide for Knowledge

Score Scoring Descriptions

4

Standard of

Excellence

The response is well organized and addresses all the major points of the question. Relevant scientific, technological, and/or societal concepts and examples are identified and interrelationships are explicit. The descriptions and/or explanations of these concepts are correct, well organized, and reflect thorough understanding and logical consistency of thought. The student uses complete sentences that make effective use of scientific vocabulary. When appropriate, suitable metaphors, similes, diagrams, and/or sketches are used to illustrate descriptions and/or explanations.

3

The response is organized and addresses most of the major points of the question. Relevant scientific, technological, and/or societal concepts and examples are identified and interrelationships are evident. The descriptions and/or explanations of these concepts are organized and reflect correct understanding. The student uses complete sentences that employ correct scientific vocabulary. When appropriate, suitable diagrams or sketches are used.

2

Acceptable Standard

The response addresses most major points. Relevant scientific, technological, and/or societal concepts and examples are identified, and interrelationships are shown. The descriptions and/or explanations of concepts may be disorganized but demonstrate correct understanding. The student uses complete sentences but is inconsistent in the use of appropriate scientific vocabulary, diagrams and sketches.

1

The response addresses few major points. Concepts are identified, but interrelationships are not evident. The student superficially describes concepts in sentences but organizational skills, scientific vocabulary, diagrams and sketches are minimal.

0 The response does not address any of the major points of the question at an appropriate level for a 30-level course.

Pedigree Chart Abbreviations for Nitrogen Bases Nitrogen Base Abbreviation

Adenine A

Cytosine C

Guanine G

Thymine T

Uracil U

Male

I

II

1 2 3

Female

Mating

Affectedindividuals

Offspring listed in birthorder. Roman numeralssymbolize generations.Arabic numberssymbolize birth orderwithin generation.

14

Scoring Guide for Skills

Score Scoring Descriptions 4

Standard of

Excellence

The problem is thoroughly understood. An appropriate and practical design is presented. The data are accurately and completely analyzed. Accurate interpretations and conclusions are made, based on an analysis of the data. The evaluation of the overall study is based on a thorough understanding of the principles of scientific inquiry.

3

The problem is well understood. An appropriate and somewhat practical design is presented. The data are completely analyzed. Interpretations and conclusions are made, based on an analysis of the data. The evaluation of the overall study is based on a correct understanding of the principles of scientific inquiry.

2

Acceptable Standard

The problem is understood. The design is generally appropriate, or a practical procedure with some omissions or errors is presented. The data are partially analyzed. Interpretations and conclusions are generally based on an analysis of the data. The evaluation of the overall study is based on a generally correct understanding of the principles of scientific inquiry.

1

The problem is poorly understood. The design is incomplete, or an impractical procedure with major omissions or errors is presented. The data are incorrectly analyzed. Interpretations and conclusions are incorrect or are not based on an analysis of the data. The evaluation of the overall study is based on a superficial understanding of the principles of scientific inquiry.

0 The response does not address any of the major points of the question at an appropriate level for a 30-level course.

Scoring Guide for STS

Score Scoring Descriptions 4

Standard of

Excellence

The design and function of the technological device are clearly explained. The interrelationships among science, technology, and society are thoroughly understood. Risks and benefits are thoroughly evaluated. Insightful and convincing arguments are used to support a decision or judgement, and a range of viewpoints is considered.

3

The design and function of the technological device are explained. The interrelationships among science, technology, and society are understood. Risks and benefits are evaluated. Clear and logical arguments are used to support a decision or judgement, and alternative points of view are considered.

2

Acceptable Standard

The design and function of the technological device are described. The interrelationships among science, technology, and society are generally understood. Risks and benefits are listed. Logical arguments are used to support a decision or judgement, and polar points of view are considered.

1

The design and function of the technological device are incorrectly described. The interrelationships among science, technology, and society are poorly understood. Few risks and benefits are listed. Poorly formed arguments are used to support a decision or judgement, and only one point of view is considered.

0 The response does not address any of the major points of the question at an appropriate level for a 30-level course.