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Biophysical & Physical > Lecture 2 > Flashcards

Lecture 2 Flashcards

1
Q

Chemistry is the study of

A

Matter and changes it undergoes

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2
Q

Physics is the study of

A

Motion, matter and energy interactions

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3
Q

Inorganic compounds contain all elements except

A

Carbon

Ionic and molecular compounds

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4
Q

Organic compounds contain

A

Carbon

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5
Q

Analytic chemistry studies

A

The percent composition of a sample

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6
Q

Atoms

A

Basic building blocks of matter
Smallest particle of an element
Composed of protons, neutrons, and electrons

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7
Q

An element is defined by its number of

A

Protons

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8
Q

Protons have a mass of

A

1 amu= 1.66 c 10^-27

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9
Q

Ions are

A

Atoms that have gain or lost electrons from their natural composition
Positive (cation) negative (anion)

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10
Q

O2 is is both

A

Molecule and element

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11
Q

Chemical properties are

A

Characteristics that describe the chemical reactivity of a substance. Result in formation of different compounds

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12
Q

Physical properties are

A

Do not describe the chemical reactivity of substance. A substance can display physical properties without a change in composition

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13
Q

Atomic number (Z) of an element is

A

The number of protons in the nucleus

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14
Q

The mass number (A) of an atom is

A

The sun of the proton (or atomic number) and the neutron number (N)

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15
Q

Atomic mass or atomic weight is the

A

Average mass of an atom in a natural sample of the element

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16
Q

Atomic number is equal to

A

The number of protons ( atomic number of carbon is 6)

Tells number of electrons

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17
Q

Mass number of an element is equal

A

To the number of protons plus number of neutrons

Electrons are ignored because they are weightless

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18
Q

Atomic weight is the average

A

Of the mass numbers of all isotopes of an element

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19
Q

Isotope are

A

Atoms with the same atomic numbers but with different atomic weights. Same number of protons (and electrons) but a diff is not be number of neutrons

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20
Q

Radioisotopes are

A

Heavier, unstable isotopes of an element that spontaneously decompose into more stable forms
- half live

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21
Q

Half live is

A

Time required to lose 1/2 of radioactivity

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22
Q

Carbon dating

A

Determines age of fossils by using half life

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23
Q

Who discovered isotopes

A

JJ Thompson

At 22 amu

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24
Q

Isotopes have the same atomic number but different

A 
Mass numbers (same Z, different A)
Same number of protons but different number of neutrons
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25
Dalton’s theory
Proposed 3 hypotheses to explain laws of conservation of mass and definite proportions
26
Dalton’s 3 laws
1. Each element is compost of tiny indivisible particles called atoms 2. Chemical combination is simply the binding of a definite, small whole number of atoms of each of the combing elements in a fixed ratio to make 2 molecule to form a compound. 3 no atoms are gained, lost, or changed in identity during a chemical reaction; they are just rearranged to produce a new substance
27
What are daltons 2 theory’s
1. Law of conservation of mass- no detectable change in the total mass occurs during a chemical reaction. 2. Law of definite proportions- different samples of a pure compound always contain the same elements in the same proportion by mass. (Water is always 11.2% hydrogen and 88.8% oxygen
28
Who constructed the periodic table
Dmitri Mendeleev 1834-1907, he emphasized that chemical and physical properties are repeated in predictable way
29
The rows in a periodic table are called
Period and increase by atomic number
30
The columns in a periodic table are called
Groups or families, elements within a family have similar chemical and physical property
31
Periodic law is
The properties of elements are periodic functions of their atomic numbers
32
Metals are
Shiny, lustrous Malleable, ductile Electrical and thermal conductor Left side of periodic table
33
Non metals are
Variable Brittle Non conductor (except graphite) Located on right side of periodic table
34
Metalloids (semimetals) are
Shiny, lustrous Variable Poor conductors Located on the stair step of the periodic table
35
Covalent bonds is a
Group of aroma chemically bonded together into a discreet unit Covalent=close on the periodic table
36
Methemoglobinemia
A form of hemoglobin that has been oxidized, changing from ferrous to ferric which cannot bind to oxygen which as a result cannot carry oxygen to tissues
37
Common element aluminum
Antiperspirant (aluminum chloride) and antacids (aluminum hydroxide)
38
Common elements of barium
``` Radio opaque Barium enema (BaSO4) ```
39
Common elements for calcium
``` Excitation and contraction o f muscles Blood clothing (factor IV) ```
40
Common elements of Carbon
Organic compounds | Activated charcoal to absorb toxic material
41
Common elements for chlorine
Disinfectant as sodium hypochlorite (NaOCl) Clorox
42
Common elements of copper
Wilson’s disease (increased copper)
43
Common elements of fluorine
Strengthens teeth | Present in inhalation anesthetics (isoflurane, enflurane)
44
Common elements for helium
Coolant in MRI instruments
45
Common elements for hydrogen
Most abundant atom | Responsible for body pH
46
Common elements for iodine
Topical antiseptic | Requires for synthesis of thyroid hormones
47
Common elements for iron
Fe++ ferrous and Fe +++ ferric Transport O2 in Hb Methemoglobinemia tx iv methylene blue
48
Common elements for lithium
Bipolar disorder
49
Common elements for magnesium
Mag sulfate
50
Common elements for mercury
Used in sphygmomanometers, thermometers
51
Common elements of nitrogen
``` 80% of air Nitrous oxide (N2O) anesthetic gas ```
52
Common elements for oxygen
20% of air Production of ATP O3 ozone protects skin cancer
53
Common elements of phosphorous
Present in DNA, RNA, and ATP
54
Common elements of potassium
Most abundant intracellular ion | Muscle contraction, nerve conduction
55
Common elements of sodium
Most abundant extra cellular ion | Determines plasma osmolarity and volume
56
Common elements of silicon
Breast implants
57
Common elements of silver
Dental fillings
58
Common elements of silver
Found in cytochrome oxidase
59
Common elements of titanium
Prosthetic implants
60
Common elements of zinc
Calamine lotion and sun blocks (zinc oxide)
61
Ionic compounds are held together by
Ionic bonds - attraction of oppositely charged ions
62
In a solid state, ionic compounds form
Crystalline lattices Cations are attracted to all neighboring anions not just one Thus there is no discrete ionic “molecule”
63
Chemical bond is an
Energy relationship between the electrons of the reacting atoms Bonds are formed using the electrons in the outermost energy level
64
Valence shell is
Outermost energy level containing chemically active electrons
65
Octet rule (rule of 8)
Except for the first shell which is full with 2 electrons, atoms interact in a manner to have 8 electrons in their valence shell
66
What are 3 types of chemical bonds
Ionic Covalent Hydrogen
67
Ionic bonds are
Chemical bonds that form between two atoms that transfer one or more electrons from one atom to the other Form crystals instead of molecules NaCl is a crystal- large structures of cations and anions held together by ionic bonds
68
Anion is an
Electron acceptor carrying a net negative charge due to an extra electron
69
Cation is an
Electron donor carrying a net positive charge due to the loss of an electron
70
Covalent bonds are
Bonds that form when electrons are shared between 2 atoms | Can be doubled or tripled bonds
71
Hydrogen bonds are
Weak attractions that form between partially charged atoms found in polar molecule Common in dipoles such as water Responsible for surface tension in water Hydrogen bonds tend to collapse the lunch
72
Ions are
An atom with a charge, cannot cross cell membrane Cations - positive, formed by loss of electron, metals Anion- negative, form from gain of electron, nonmetals
73
How can we get ions to cross cell membrane?
Check pH, has to be non ionic to cross
74
Desiccant is
The anhydrous form of a component d that has a strong tendency to form a hydrate, and is used to scavenge the last traces of wager from a system. Most common is silica gel (SiO2) Addition of water to a desiccant is a reversible process so saturated desiccants can be used as moisturizers
75
Moles is an
Amount of substance that contains exactly as many particles as 12.00 grams of carbon This number is called Avogadro’s number Particles could mean molecules, atoms, ions, or electrons
76
Molecular mass is
The sun if they masses of the component atoms
77
Avogadro’s number
6.02 x 10^23

Biophysical & Physical (2 decks)

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