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CHEM1011 > Terms and Rules > Flashcards

Terms and Rules Flashcards

1
Q

Sig fig rule for multiplication and division

A

The answer cannot be more precise than the measurement with the fewest significant figures.

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2
Q

Sig fig rule for adding and subtracting

A

The answer must have the same decimal places as the least precise measurement or the least amount of decimal places.

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3
Q

Quadratic Equation

A

ax^2 + bx + c = 0

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4
Q

Linear Equation

A

y = mx + b

y, x = variables

m = slope

b = y-intercept

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5
Q

Quadratic Formula

A

x = [-b +/- sqrt((b^2)-4ac)]/2a

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6
Q

Logarithm (Base-10)

A

Base-10 Logarithm of a number z is the power (x) to which 10 must be raised to equal z

b^x = a <-> logba

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7
Q

Antilog

A

Used to find the # corresponding to a certain logarithm

To calculate, raise the power of x to the base

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8
Q

Natural Logarithm

A

When the base of the logarithm is e and abbreviated as ln

e^lnx = x <-> ln e^x = x

Note: The inverse of the exponential function

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9
Q

Exponential Function

A

f(x) = e^x

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10
Q

Product Rule for Natural Logarithms

A

ln(xy) = ln(x) + ln(y)

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11
Q

Quotient Rule for Natural Logarithms

A

ln(x/y) = ln(x) - ln(y)

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12
Q

Power Rule for Natural Logarithms

A

ln(x^a) = aln(x)

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13
Q

Relationship between log and ln?

A

ln(x)
= ln(10^log(x))
= log(x)ln(10)
= 2.303log(x)

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14
Q

Hydrated Salts

A

When salts are formed from solution, water gets caught in their newly formed lattice structure creating hydrated salts

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15
Q

How to name hydrated salts

A

Add the prefix for number of water molecules to “hydrate”

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

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16
Q

Naming Polyatomic Compounds and Ions

A

Parent ion - Suffix “-ate”

Add O - Add prefix “per-“

Remove one O - Suffix changes to “-ite”

Remove two O - Add prefix “hypo-“

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17
Q

Naming Transition Metal Ionic Compounds (Group 3-12)

A

Add “-ide” suffix to non-metal

Use roman numerals to specify the charge of the metal

Old Rules:

Lowest charge metal suffix “-ous”
Highest charge metal suffix “-ic”

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18
Q

Oxidation States

A

The hypothetical charge of an atom if all its bonds to other atoms were fully ionic. The charge may be positive, negative or zero.

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19
Q

Rules for Naming Ionic Compounds (Salts)

A

Name the metal first

Name the non-metal and add the suffix “-ide”

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20
Q

Prefix for 1 Atom (Molecular/Inorg)

A

Mono-

Note: Not used on the first element in a compound

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21
Q

Prefix for 2 Atoms (Molecular/Inorg)

A

Di-

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22
Q

Prefix for 3 Atoms (Molecular/Inorg)

A

Tri-

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23
Q

Prefix for 4 Atoms (Molecular/Inorg)

A

Tetra-

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24
Q

Prefix for 5 Atoms (Molecular/Inorg)

A

Penta-

25
Q

Prefix for 6 Atoms (Molecular/Inorg)

A

Hexa-

26
Q

Prefix for 7 Atoms (Molecular/Inorg)

A

Hepta-

27
Q

Prefix for 8 Atoms (Molecular/Inorg)

A

Octa-

28
Q

Prefix for 9 Atoms (Molecular/Inorg)

A

Nona-

29
Q

Prefix for 10 Atoms (Molecular/Inorg)

A

Deca-

30
Q

Prefix for Naming Diatomic Molecules

A

“Di-“

31
Q

Ionic Compound

A

Metal cation (+)
+ Non-metal Anion(-)

Electrostatic interaction (attraction or repulsion between objects with opposite or identical charges) cause the charges to balance

32
Q

Molecular Compound

A

Two or more non-metal elements bonded together

33
Q

Does group 16 or gain e-? Overall charge?

A

Gain 2e-

Overall charge 2-

34
Q

Does group 17 or gain e-? Overall charge?

A

Gain 1e-

Overall charge 1-

35
Q

Which group doesn’t usually gain or lose e-?

A

Group 18
Noble Gases

36
Q

Does group 13 lose or gain e-? What is their overall charge?

A

Lose 3e-

Overall charge 3+

37
Q

Does group 2 lose or gain e-? What is their overall charge?

A

Alkaline Earth Metals

Lose 2e-

Overall charge 2+

38
Q

What is the overall charge of compounds containing nitrogen and phosphorus?

A

Gain 3e-

Form nitrides and phosphides

Over -3 charge

Note: Group 14 and 15 may lose or gain e-

39
Q

Does group 1 lose or gain e-? What is their overall charge?

A

Alkali Metals

Lose 1e-

1+ charge

40
Q

Anions

A

Gain e-

Become negatively charged

41
Q

Cations

A

Lose e-

Become positively charged

42
Q

Halogens (Group 17)

A

F - Fluorine
Cl - Chlorine
Br - Bromine
I - Iodine
At - Astatine

43
Q

Noble Gases (Group 18)

A

Ne - Neon
Ar - Argon
Kr - Krypton
Xe - Xenon
Rn - Radon

44
Q

Alkaline Earth Metals (Group 2)

A

Be - Beryllium
Mg - Magnesium
Ca - Calcium
Sr - Strontium
Ba - Barium
Ra - Radium

45
Q

Alkali Metals (Group 1)

A

Li - Lithium
Na - Sodium
K - Potassium
Rb - Rubidium
Cs - Cesium
Fr - Francium

46
Q

RSD

A

Relative Standard Deviation

The deviation of a set of numbers disseminated around the mean

47
Q

Relative Standard Deviation

A

RSD = s/x = stardard deviation/mean

Note: Expressed as a percent or parts per thousand (ppt)

48
Q

Formula for Standard Deviation

A

s = sqrt[(1/N-1)((x1-x)^2+(x2-x)^2+…+(xN-X_^2)]

x = average
xN = measurement in a set
N = # of measurements in a set

49
Q

Standard Deviation

A

The measure of the amount of variation of a random variable expected about its mean.

50
Q

Formula for Average or Mean

A

x = 1/N (x1 + x2+…+xN)

51
Q

Precision

A

This is how close a collection of measurements are to each other.

52
Q

Accuracy

A

This is how close a measurement is to the actual value.

53
Q

Real Numbers

A

A number that can be used to measure a one-dimensional quantity. They include rational and irrational numbers.

54
Q

Irrational Numbers

A

A real number that cannot be expressed as a ratio of integers

Ex. Pi, sqrt(2), e

55
Q

Rational Numbers

A

A number that can be expressed as a fraction where the numerator and denominator are integers and the denominator cannot be zero.

56
Q

Integer

A

A whole number that is positive, negative, or zero.

57
Q

Naming Rules for Inorganic Aqueous Acids

A

Anion ends in “-ate”, the acid is named “-ic acid” as the suffix

Anion end in “-ite”, the acid is named “-ous acid” as the suffix

Anion ends in “-ide”, the acid is named “hydro-…-ic acid”

*HClO3 > ClO3^- chlorate ion > chloric acid

HClO2 > ClO2^- chlorite ion > chlorous acid

HF > hydrogen fluoride > hydrofluoric acid*

58
Q

Isomers

A

They are molecules or polyatomic ions with identical molecular formula – that is, the same number of atoms of each element – but distinct arrangements of atoms in space.

CHEM1011 (3 decks)

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