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Exam 1 Flashcards

1
Q

Conversion equation for F to C

A

(F-32) x .55 = C

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2
Q

Conversion equation for C to F

A

F = 1.8 (C) + 32

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3
Q

Conversion for inches to cm

A

1 inch = 2.54 cm

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4
Q

Kg to lbs conversion and lbs to kg

A 
1kg = 2.2 lbs
1lb = 0.454kg
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5
Q

Kelvin conversion (C to K and K to C)

A 
C = K -273
K = C + 273
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6
Q

Formula for concentration

A

Concentration = amount (mass) / volume

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7
Q

Formula for amount (mass)

A

Amount (mass) = concentration x volume

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8
Q

% concentration means ?

A

Grams / 100 ml

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9
Q

1:1,000 means?

A

1 gram / 1,000ml

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10
Q

What does an exponent of zero equal?

A

An exponent of 0 = 1

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11
Q

When powers are multiplied the exponents are?

A

Added

Ex. Ten to the third power times ten to the negative fourth power = ten to the negative one power.

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12
Q

When powers are divided, the exponents are ?

A

Subtracted

Ex. Cm cubed divided by cm cubed = cm squared

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13
Q

In scientific notation how many digits are to the left of the decimal place?

A

Just 1 digit is to the left of the decimal place.

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14
Q

11,000,000 expressed in scientific notation

A

1.1 x 10^7

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15
Q

0.0000000045 expressed in scientific notation?

A

4.5 x 10 ^-9

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16
Q

Water boils at?

Water freezes at?

A

212 F or 100 C - boils

32 F or 0 C - freezes

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17
Q

State what Charles law is and the formula.

A

Volume of a gas is directly proportional to the temperature (when pressure is constant).

(More basically stated) - The volume of a gas shrinks as it become cooler or expands as it heats up, easy to notice in a closed space such as a balloon.

V/T = k

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18
Q

What is Boyles law and what is the formula?

A

Volume and pressure are inversely proportional when temperature is constant.
(More basically stated) - describes how the pressure of a gas tends to increase when volume of a container decreases. (Becoming more compressed)

PV = k

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19
Q

What’s the constant in Charles law and what’s the constant in Boyles law?

A

The constant in Charles law is pressure

The constant in Boyles law is temperature

Constant is always represented as k

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20
Q

With Charles and Boyles law what always goes on the Y-axis?

A

VOLUME goes on the Y axis

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21
Q

Are zeroes significant in scientific notation?

A

All non zero digits in a number are significant

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22
Q

What is precision

A

Precision is the consistency and reproducibility of a test (reliability)

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23
Q

What is accuracy

A

Accuracy is the trueness of test measurements (validity)

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24
Q

Coldest possible temp. And can we reach it?

A

Absolute zero is the coldest possible temp. No we can not reach it.

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25
Where does the Kelvin scale begin?
At absolute zero
26
What does absolute zero =
0 K =absolute zero = -273.15 C
27
Formula for density and most common units.
Density = mass/volume | Grams/mL
28
Density of water
1.0 g/mL
29
What’s the equation for specific gravity ?
Specific gravity = density of object / density of water Specific gravity will equal density when the units of measure are grams/mL because the density of water is 1g/mL
30
What is an atom composed of?
Protons, neutrons, and electrons
31
Aluminum
Antiperspirants and antacids
32
Barium
Barium enema
33
Calcium
Blood clotting Excitation and contraction of muscles Found as a salt in bones and teeth
34
Carbon
Organic compounds | Activated charcoal
35
Chlorine
Disinfectant
36
Copper
Wilson’s disease (increased copper)
37
Fluorine
Strengthens teeth
38
Helium
Coolant in MRI instruments
39
Hydrogen
Most abundant atom! | Responsible for the body’s PH (which is a measure of H+ atoms)
40
Iodine
Topical antiseptic | Required for synthesis of thyroid hormones
41
Iron
Fe++ (ferrous) is good Fe+++ (bad) cannot carry oxygen Transport oxygen in Hb
42
Lithium
For bipolar disorder
43
Magnesium
calms down cells In bones Cofactor in the number of metabolic reactions.
44
Mercury
Used in BP cuffs and thermometers
45
Nitrogen
79% of Air Anesthetic gas, nitrous oxide A component of proteins and nucleic acids
46
Oxygen
21% of air Production of ATP Protectant in the ozone agains skin cancer O3 (ozone)
47
Phosphorus
Present in DNA, RNA, ATP
48
Potassium
Major cation in cells | Necessary for conduction of nerve impulses and contractions
49
Sulfur
Component of proteins particularly muscle proteins | Found in cytochrome oxidase
50
Sodium
Major positive ion found in extra cellular fluid Important for water balance, plasma osmolarity and volume Conduction of nerve impulses and muscle contractions
51
Silicon
Breast implants
52
Silver
Dental fillings
53
Titanium
Prosthetic implants
54
Zinc
``` Calamine lotion sun blocks (zinc oxide) ```
55
What is a cation | What is an anion
Cation is an ion that is positively charged because it has lost an electron Anion is an ion that is negatively charged because it has gained an electron (Remember electrons are (-) thus if you gain one you are more negative, if you lose one you are more positive.)
56
Atomic number
Equal to the number of protons Ex is carbon’s atomic number is 6 bc it has 6 protons. (Also tells the number of electrons)
57
Atomic weight (mass)
Average of the mass numbers of all isotopes in an element
58
Mass number
Mass number of an element is equal to the number of the protons plus number of neutrons. Electrons ignored bc they are weightless
59
Isotopes
Atoms with the same atomic number but with different atomic weights. They have the same number of protons and electrons but a different number of neutrons.
60
Radioisotope
Are heavier, unstable isotopes of an element that spontaneously decompose into more stable forms. Half life comes from radioisotopes, time required to lose half of the radioactivity
61
The same atomic number but different mass numbers (same Z, different A) describes what?
Isotopes
62
Same number of protons, different number of neutrons describes what?
Isotopes
63
What altered Dalton’s theory?
Modified after the discovery of isotopes
64
Rows on a periodic table are called? | Columns are called?
``` Rows = periods Columns = groups or families ```
65
Where is atomic number and atomic weight on the element on the period table?
Atomic number is above the number typically and atomic weight is a decimal number below the element.
66
Mixture vs compounds
No chemical bonding takes place Most mixtures can be separated by physical means Mixtures can be hetero or homo Compounds can not be separated by physical means All compounds are homo
67
Covalent bond
Sharing of electron pairs between atoms (equally sharing) Occurs between non metals sharing electrons Covalent = close on the periodic table
68
Ionic bonding
Complete transfer of electrons between atoms. Type of bond that generates two oppositely charged ions. Metal with non metal The metal loses an electron to becomes a positively charged cation The non metal gains an electron to become the negatively charged anion.
69
What holds ionic compounds together
Ionic bonds, or the attraction between atoms that have opposite charge. (Do to the complete transfer of an electron in order to bond)
70
In the solid state ionic compounds form what structure?
Crystalline lattices
71
Cations are attracted to all neighboring anions or just one?
ALL
72
Bonds are formed using electrons from what level or shell?
The outermost shell or level
73
Valance shell?
The outermost energy level containing chemically active electrons
74
Octet rule
All elements want their outermost shell full. The first level closest to the atom or element can contain 2 electrons and is satisfied with 2, but all other shells require 8 electrons to be full, this dictates which elements will share electrons with who. They are always looking to fill their valance shell, when filled they are stable.
75
Who has their outer shells filled as a single atom and are happy and not wanting to bond?
HELIUM AND NOBLE GASES
76
Polar molecule?
The larger atom the more electron cloud it takes, the smaller the atom the less electron cloud it gets. This creates unequal sharing and creates a polar molecule.
77
How many bonds do the following elements make?
Hydrogen forms single bonds Oxygen forms two bonds Nitrogen forms three bonds Carbon forms four bonds
78
Electrons shared equally between atoms produce?
Non polar molecules
79
Unequal sharing of electrons produces
Polar molecules
80
Dipole applies to what molecule
Polar molecule
81
Sodium chloride is an example of what kind of bond
Ionic bond
82
Water is an example of what kind of bond
Polar covalent bond
83
Carbon dioxide is an example of what kind of bond?
Non polar covalent bond
84
Hydrogen bonds?
Hydrogen bonds are weak attractions that form between partially charged atoms found in polar molecules. COMMON in water (a single water molecule is polar bond, but water to water is hydrogen bond)
85
Surfactant
Role of surfactant is to break down the hydrogen bonding of water inside the alveoli and reduce the tension and keep the alveoli open. Without surfactant the hydrogen bonds between water molecules in the lungs would cause the lungs to collapse in on themselves.
86
Why can a water strider walk on the top of a pond?
Because of the high surface tension of water. (Combined strength of the hydrogen bonds in water)
87
Most commonly used desiccant is?
Silica gel (SiO2)
88
METHEMOGLOBINEMIA
Altered state of Hgb in which the ferrous ions of hemoglobin are oxidized to the ferric state (ous = 2, ic = 3). Methemoglobin can not bind with oxygen because ferric iron inhibits oxygens binding capacity.
89
What can cause methemoglobinemia
Genetic or congenital Increased synthesis or decreased clearance issues Exposure to toxins
90
Treatment of MetHgb
Methylene blue

Chemistry (4 decks)

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