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Bioscience > Chemistry CH 1 & 2 > Flashcards

Chemistry CH 1 & 2 Flashcards

1
Q

Charles Law describes?

A

At a constant pressure, when you have a known mass of gas, the volume of the gas is directly proportionately to the temperature.

  • Heat goes up, then vol goes up
  • Heat goes down, then vol goes down
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2
Q

What is the formula for Charles Law?

A

V1/T=V2/T2

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3
Q

F to C

A

C= (F-32) x 5/9
Or
C= (F-32)/1.8

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4
Q

C to F

A

F= 9/5C + 32

or

F = 1.8C + 32

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5
Q

Log (a x b) =

A

Log (a) + Log (b)

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6
Q

Log (a/b) =

A

Log (a) - Log (b)

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7
Q

Lob (a^b) =

A

b x Log (a)

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8
Q

Any quantity (except zero) raised to the zero will equal?

A

1

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9
Q

Any quantity (except zero) to the -1 power is equal to?

A

The reciprocal of the quantity
2^ -1 = 1/2^1

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10
Q

When powers are multiplied, the exponents will be added or subtracted?

A

added

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11
Q

When powers are divided, the exponents will be added or subtracted?

A

subtracted

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12
Q

What is the mantissa?

A

the scientific notation where there is only one number to the left of the decimal.

1.5 x 10^3

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13
Q

What is the formula for slope intercept?

A

y = mx + b

y= vertical axis (dependent variable)
x= horizontal axis (independent variable)
m= slope line
b = intercept (the value of the function where it crosses the y-axis)

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14
Q

What is the formula to find the slope (m)

A

m = (y2-y1)/(x2-x1)

note: the slope of a line (m) depicts the change in the dependent variable (y) as the independent variable (x) is changed

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15
Q

What are significant figures?

A

Digits in a measured value that have a physical meaning and can be reproducibly determined

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16
Q

Exact numbers are?

A

Numbers not obtained using measuring devices. easily countable, no question as to the value

ex. 12 cm = 1 ft
12 ducks

These measurements have an infinite number of significant figures

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17
Q

What are the 4 rules when dealing with significant figures?

A
  • Nonzero digits are always significant
  • Captive zeros are always significant
  • Leading zeros (despite the decimal place) are never significant
  • Trailing zeros are only significant when the number contains a decimal point (ex: 1.50 vs 100; 1.50 has 3 sigfigs and 100 has 1 sigfig)
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18
Q

How many sigfigs do you keep when adding or subtracting?

A

Keep the smaller number of decimal places

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19
Q

How many sigfigs do you keep when multiplying or dividing?

A

Keep the smaller number of sigfigs

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20
Q

Define accuracy

A

The agreement between experimental data and the true value.

In other words, how close a measurement is to the true/accepted value

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21
Q

Define precision

A

The agreement between replicate measurements.

In other words, how close measurements of the same item are to each other

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22
Q

Can accuracy be improved?

A

Accuracy can be improved by making replicate measurements and taking the average of those measurements

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23
Q

Can precision be improved?

A

Repeated measures do not improve precision.

Precision can be quantified by standard deviation. The smaller the SD the greater the precision

The SD is the square root of the data set’s variance

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24
Q

giga is

A

1 x 10^9

G

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25
Q

mega is

A

1 x 10^6

M

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26
Q

kilo is

A

1 x 10^3

k

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27
Q

deci is

A

1 x 10^-1

d

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28
Q

centi is

A

1 x 10^-2

c

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29
Q

mili is

A

1 x 10^-3

m

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30
Q

micro is

A

1 x 10^-6

u

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31
Q

nano is

A

1 x 10^-9

n

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32
Q

1in = ? cm

A

2.54cm

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33
Q

1mi = ? km

A

1.609 km

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34
Q

1mi = ? ft

A

5,280 ft

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35
Q

1 lb = ? kg

A

0.454 kg

Correctly stated as 1 lb = 4.45 N

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36
Q

1 lb = ? N

A

4.45 N

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37
Q

1 lb = ? oz

A

16 oz

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38
Q

1 oz = ? g

A

28.35 g

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39
Q

1 grain = ? mg

A

64.80 mg

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40
Q

1 L = ? dm^3

A

1 dm^3

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41
Q

1 gal = ? L

A

3.79 L

42
Q

1mL (cc) = ? cm^3

A

1 cm^3

43
Q

Kelvin temperature scale begins at?

A

absolute zero (coldest)

no temp lower than 0k
notice, no reported degrees

44
Q

On a celsius scale how do you calculate for kelvin?

A

K = C + 273.15

45
Q

What is Density?

A

Density is the ratio of the mass of an object to its volume

d = mass/volume = m/v

46
Q

What is specific gravity?

A

The ratio between (density of an object / density of water)

Specific gravity only equals density when the units of measure are g/mL because the density of water is 1g/mL.

No units used in specific gravity because it is a RATIO

47
Q

What is the density of water?

A

1.0 g/mL or 1.0g/cm^3
1000kg/m^3
8.33 lb/gal

48
Q

What is matter?

A

Anything that has a mass and occupies space; doesn’t have to be visible

49
Q

How many atoms to form an element

A

a single atom

50
Q

How many atoms to form a compound

A

two or more atoms

51
Q

What are atoms comprised of

A

Protons, neutrons, and electrons

52
Q

What is the SI units for atoms

A

atomic mass units (amu)

53
Q

1 amu = ? kg

A

1.66 x 10^-27 kg

54
Q

1 mol = ? amu

A

1 amu

55
Q

What are ions?

A

Ions are atoms or a group of atoms bonded together that have a net electrical charge

This charge can be obtained by adding or removing electrons

56
Q

Charge or cations

A

protons > #electrons

(+) charge

57
Q

Charge for anions

A

protons < #electrons

(-) charge

58
Q

Define molecules (molecular compound)

A

Group of atoms chemically bonded together into a discrete unit by covalent bonds

Contains ONLY NON-METALS
Electrically NEUTRAL

59
Q

Define Ionic Compounds

A

Contains (+) charged ions and (-) charged ions

Contains METALS & NON-METALS

Ionic compounds are NOT molecules

60
Q

What is the difference between physical property and chemical property?

A

Physical property can be observed or measured without chemical change (ex color)

Chemical property describes the chemical changes the material tends to undergo (ex gases are flammable)

61
Q

Define a pure substance

A

Materials that cannot be physically separated into simpler components

Ex: Elements are pure substances

62
Q

T or F
Substances are compounds only

A

False

Substances can be either a compound or an element

If substances are a compound, then can be chemically separated into its elemental components. Elements are pure substances and cannot be further separated

63
Q

What makes up a mixture

A

Comprised of 2 or more pure substances

Can be resolved into simpler components through physical processes

64
Q

Homogenous mixtures are

A

uniform in chemical and physical properties

65
Q

Heterogenous mixture

A

Exhibits distinct phase boundaries between its components
Ex: emesis

66
Q

Define phase boundary

A

A demarcation where the chemical and/or physical properties of the sample change

67
Q

The mass of an atom is the sum of what

A

Protons and Neutrons

Represented as an integer

68
Q

1 neutron = ? amu

A

1.0087 amu

or 1.6749 x 10^-27 kg

69
Q

1 proton = ? amu

A

1.0073 amu

or 1.6726 x 10^-27 kg

70
Q

Elements are always

A

Electrically neutral

Therefore, each atom must have an equal # of (+) protons and (-) electrons

71
Q

Define Isotopes

A

Have the same atomic number but different mass number.

In other words, same # protons but different # neutrons

72
Q

What does Dalton’s Atomic Theory include?

A

1) Elements are composed of tiny atoms
2) Compounds are formed by bonding of atoms in a fixed ratio
3) Chemical rxns do not create, destroy, or change atoms; they recombine into a new substance

73
Q

What are the 3 laws used in Dalton’s Atomic Theory?

A

1) Law of Conservation of Mass - no detectable change in the total mass occurs during a chemical rxn

2) Law of Definite Proportions - Different samples of a pure compound always contain the same elements in the same proportion by mass

3) Law of Multiple Proportions - some elements can combine to give more than one compound

74
Q

What are polyatomic ions?

A

Polyatomic ions are considered ionic compounds as well.

They contain 2 or more non-metals plus a metal with an electrical charge (either + or -)

75
Q

How would you name a molecular substance?

A
  • Name each element
  • Indicate how many of each is present with a prefix multiplier (mono, di, try, tetra, etc…)
  • Add the suffix “-ide” to the last element name

Ex: N2S3 -> Dintrogen trisulfide

76
Q

mono is

A

1

77
Q

di is

A

2

78
Q

tri is

A

3

79
Q

tetra is

A

4

80
Q

penta is

A

5

81
Q

hexa is

A

6

82
Q

hepta is

A

7

83
Q

octa is

A

8

84
Q

If a transitional metal forms more than one cation, how do you name it?

A

You need to name the metal, then indicate the charge on the cation with roman numerals in parentheses

ex. Fe3+ - iron (III) cation

85
Q

How do you name monatomic anions?

A

Add the suffix “-ide” to the stem name

ex:
Cl- —> Chloride ion
S2- —> Sulfide ion
P3- —> Phosphide ion

86
Q

How do you name monatomic cations?

A

Add cation or ion at the end of the name

*note, there are no simple cations with charges of +4

Ex: Cu 1+ —> Copper cation or Copper ion

87
Q

How do you name polyatomic ions?

A

Some ions like SO4^2- and SO3^2- differ only in a single atom. In these cases, the larger # is given the suffix “-ate” while the smaller # is given the suffix “-ite”

SO4^2- would be sulfate ion
SO3^2- would be sulfite ion

88
Q

How do you name a hydrate ion?

A

name the ion then add “hydrate” at the end

Ex: CuSO4 * 5H2O - Copper (II) sulfate pentahydrate

89
Q

What is an electrolyte

A

A substance that dissolves in water to give a solution that conducts electricity

90
Q

What is Avogadro’s Number?

A

Conversion factor between particles and moles

6.02 x 10^23 particles/mol

91
Q

What is a mole

A

Quantity of material, analogous to a dozen. It is an amount of a substance that contains exactly as many particles as there are in exactly 12g of Carbon-12.

92
Q

What does particle mean?

A

It could mean molecules, atoms, ions, or electrons

93
Q

1m = ? cm

A

100 cm

94
Q

1s = ?ms

A

1000ms

95
Q

Molecular formula for ammonia

A

NH3

96
Q

Ionic formula for ammonium

A

NH4+

97
Q

Molecular formula for Methane

A

CH4

98
Q

Molecular formula for propane

A

C3H8

99
Q

Molecular formula for nitrous oxide

A

N2O

100
Q

1 cm^3 = ? m

A

0.01 m
Or
10^-2

101
Q

1micrometer (um) = ? nanometers (nm)

A

1,000nm

Bioscience (5 decks)

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