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Chemistry > Exam 1 > Flashcards

Exam 1 Flashcards

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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
Q

Where does the Kelvin scale begin?

A

At absolute zero

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26
Q

What does absolute zero =

A

0 K =absolute zero = -273.15 C

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27
Q

Formula for density and most common units.

A

Density = mass/volume

Grams/mL

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28
Q

Density of water

A

1.0 g/mL

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29
Q

What’s the equation for specific gravity ?

A

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

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30
Q

What is an atom composed of?

A

Protons, neutrons, and electrons

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31
Q

Aluminum

A

Antiperspirants and antacids

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32
Q

Barium

A

Barium enema

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33
Q

Calcium

A

Blood clotting
Excitation and contraction of muscles
Found as a salt in bones and teeth

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34
Q

Carbon

A

Organic compounds

Activated charcoal

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35
Q

Chlorine

A

Disinfectant

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36
Q

Copper

A

Wilson’s disease (increased copper)

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37
Q

Fluorine

A

Strengthens teeth

38
Q

Helium

A

Coolant in MRI instruments

39
Q

Hydrogen

A

Most abundant atom!

Responsible for the body’s PH (which is a measure of H+ atoms)

40
Q

Iodine

A

Topical antiseptic

Required for synthesis of thyroid hormones

41
Q

Iron

A

Fe++ (ferrous) is good
Fe+++ (bad) cannot carry oxygen
Transport oxygen in Hb

42
Q

Lithium

A

For bipolar disorder

43
Q

Magnesium

A

calms down cells
In bones
Cofactor in the number of metabolic reactions.

44
Q

Mercury

A

Used in BP cuffs and thermometers

45
Q

Nitrogen

A

79% of Air
Anesthetic gas, nitrous oxide
A component of proteins and nucleic acids

46
Q

Oxygen

A

21% of air
Production of ATP
Protectant in the ozone agains skin cancer O3 (ozone)

47
Q

Phosphorus

A

Present in DNA, RNA, ATP

48
Q

Potassium

A

Major cation in cells

Necessary for conduction of nerve impulses and contractions

49
Q

Sulfur

A

Component of proteins particularly muscle proteins

Found in cytochrome oxidase

50
Q

Sodium

A

Major positive ion found in extra cellular fluid
Important for water balance, plasma osmolarity and volume
Conduction of nerve impulses and muscle contractions

51
Q

Silicon

A

Breast implants

52
Q

Silver

A

Dental fillings

53
Q

Titanium

A

Prosthetic implants

54
Q

Zinc

A 
Calamine lotion 
sun blocks (zinc oxide)
55
Q

What is a cation

What is an anion

A

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
Q

Atomic number

A

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
Q

Atomic weight (mass)

A

Average of the mass numbers of all isotopes in an element

58
Q

Mass number

A

Mass number of an element is equal to the number of the protons plus number of neutrons.

Electrons ignored bc they are weightless

59
Q

Isotopes

A

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
Q

Radioisotope

A

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
Q

The same atomic number but different mass numbers (same Z, different A) describes what?

A

Isotopes

62
Q

Same number of protons, different number of neutrons describes what?

A

Isotopes

63
Q

What altered Dalton’s theory?

A

Modified after the discovery of isotopes

64
Q

Rows on a periodic table are called?

Columns are called?

A 
Rows = periods
Columns = groups or families
65
Q

Where is atomic number and atomic weight on the element on the period table?

A

Atomic number is above the number typically and atomic weight is a decimal number below the element.

66
Q

Mixture vs compounds

A

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
Q

Covalent bond

A

Sharing of electron pairs between atoms (equally sharing)
Occurs between non metals sharing electrons

Covalent = close on the periodic table

68
Q

Ionic bonding

A

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
Q

What holds ionic compounds together

A

Ionic bonds, or the attraction between atoms that have opposite charge. (Do to the complete transfer of an electron in order to bond)

70
Q

In the solid state ionic compounds form what structure?

A

Crystalline lattices

71
Q

Cations are attracted to all neighboring anions or just one?

A

ALL

72
Q

Bonds are formed using electrons from what level or shell?

A

The outermost shell or level

73
Q

Valance shell?

A

The outermost energy level containing chemically active electrons

74
Q

Octet rule

A

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
Q

Who has their outer shells filled as a single atom and are happy and not wanting to bond?

A

HELIUM AND NOBLE GASES

76
Q

Polar molecule?

A

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
Q

How many bonds do the following elements make?

A

Hydrogen forms single bonds
Oxygen forms two bonds
Nitrogen forms three bonds
Carbon forms four bonds

78
Q

Electrons shared equally between atoms produce?

A

Non polar molecules

79
Q

Unequal sharing of electrons produces

A

Polar molecules

80
Q

Dipole applies to what molecule

A

Polar molecule

81
Q

Sodium chloride is an example of what kind of bond

A

Ionic bond

82
Q

Water is an example of what kind of bond

A

Polar covalent bond

83
Q

Carbon dioxide is an example of what kind of bond?

A

Non polar covalent bond

84
Q

Hydrogen bonds?

A

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
Q

Surfactant

A

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
Q

Why can a water strider walk on the top of a pond?

A

Because of the high surface tension of water. (Combined strength of the hydrogen bonds in water)

87
Q

Most commonly used desiccant is?

A

Silica gel (SiO2)

88
Q

METHEMOGLOBINEMIA

A

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
Q

What can cause methemoglobinemia

A

Genetic or congenital
Increased synthesis or decreased clearance issues
Exposure to toxins

90
Q

Treatment of MetHgb

A

Methylene blue

Chemistry (4 decks)

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