Vocab, Unit 2 Flashcards
1
Q
Atom
A
“The smallest unit of matter which retain the properties and characteristics of the element.”
2
Q
Element
A
A substance which cannot be split into simpler substances by chemical means.
3
Q
What are the first four ingredients(elements) of a human?
A
- Oxygen (65%)
- Carbon (18.5%)
- Hydrogen (9.5%)
- Nitrogen (3.2%)
4
Q
Molecules
A
“two or more atoms sharing electrons joined by a chemical bond”
5
Q
What is a subscript?
A
“It is the number of each type of atom in a molecule”
6
Q
Compound
A
Composed of two or more elements
7
Q
Table salt
A
NaCL
8
Q
Common mineral in the Great Salt Lake
A
CaCL(sub)2
9
Q
What are the 3 states of matter?
A
- Solid
- Liquid
- Gas
10
Q
Solids
A
“are substance in which the particles are tightly associated with each other. They have shape and definite volume and are not compressible.”
11
Q
Liquids
A
“contain particles that are interacting with one another, but much more weakly. It has an indefinite shape, but a definite volume. Liquids are not very compressible. The atoms are colliding with each other but still have some interaction”
12
Q
Gases
A
“have widely spaced particles that are flying around, banging off of each other. The particles don’t interact much beyond these collisions. They have an indefinite shape and volume and are very compressible.”
13
Q
Potential engery
A
“is stored energy that is not yet able to do work.”
14
Q
Kinetic energy
A
Its potential energy that is usable - “energy of movement”
15
Q
Endergonic
A
“reactions that store energy” Energy can be stored in chemical bonds.
16
Q
Exergonic
A
A reaction that releases energy.
17
Q
Catabolic reactions, (catabolism)
A
“Chemical reactions that break down complex organic compounds into simple ones, with the net release of energy.”
18
Q
Anabolic Reactions (Anabolism)
A
“Synthetic, energy requiring reactions whereby small molecules are built up into larger ones.”
19
Q
Heat
A
often a byproduct of work, and is utilized by the body to maintain temperature
20
Q
Work
A
energy put to good use
21
Q
Entropy
A
As particles move, they bounce around and become disorganized. Entropy is moving from order to disorder.
22
Q
Diffusion
A
“If there is no barrier, substances always move from where they are at high concentration to where they are at low concentration.”
23
Q
Thermodynamics - High to low movement
A
Energy is always moved from high to low. You can heat a baby bottle in a microwave but to cool it you have to put it in an ice bath and the heat is moved to the ice.
24
Q
Specific heat
A
“the amount of energy it takes to raise a gram of substance one degree of temperature”
25
High specific heat
"Difficult to heat up, but once heated they stay hot for a long time"
26
Low specific heat
"They get hot fast, and cool off fast"
27
What is the specific heat of water?
1.000 - it has a high specific heat
28
What is the specific heat of Ice?
0.492
29
What is the specific heat of Gold?
0.0312
30
What is the specific heat of Lead?
0.0305 - it has a low specific heat
31
Conversion of food Calorie to metric calories?
1 food Calorie = 1000 metric calories.
| C's are capitalized to remind about the abbreviation
32
Calorie
"Its a measure of specific heat. A calorie is the amount of energy it takes to raise one gram (one ml) of water one degree Centigrade. The official SI unit is a Joule.
33
Food calorie
If there is 18 calories (food) of sugar in a drink, then that is 18000 calories and could raise 1 liter of water 18 degrees Centigrade.
34
Who created the periodic table?
Mendeleev in 1869
35
Atomic number
The number of protons in a nucleus
36
Periodic table: Metals are found where?
They are located on the left 2/3 of the table.
37
Periodic table: non metals are found where?
They are located on the far right side of the table. Triangle type shape.
38
Hydrogen - metal or not?
It is technically a metal, but is generally not called one.
39
What is the most common noble gas?
Argon. It is found naturally in the atmosphere and is simply Ar.
40
What is a metalloid?
A element that shares both metal and non-metal properties.
41
What is a noble gas?
1. They are in the far right column of the periodic table.
2. They do not combine with any other element or themselves.
3. They are not in the body.
4. They have complete outer shells.
42
List the three subatomic particles or elementary particles
1. Electron
2. Proton
3. Neutron
43
Electron
1. The smallest of the particles
2. Carries a negative charge
3. They do not travel in an orbit.
44
Particles of an Atom
Electrons are equal to protons
45
Particles of an Ion
Has unequal numbers of protons and electrons. Either short or a gain of electrons.
This is indicated by a superscript by the number following the element. ( Ca^2+ )
46
Neutron
1. Located in the nucleus of the atom
2. Has a neutral charge
3. They have mass
4. Only really found in nuclear situations
(? Formed by radioisotopes?, pg 74 SG)
47
Proton
1. Located in the nucleus of the atom
2. Has a positive charge
3. They have mass
4. Only really found in nuclear situations
5. The number of protons determines what element it is.
48
What does a MRI work off of?
"The magnetic properties of hydrogen nuclei"
49
Positron
These are like electrons, except they carry a positive charge. They are used in positron-emission tomography (PET)
50
What is Positron-emission tomography?
It is a nuclear medical imaging technique. Frequently used with the neurological problems, cancer, and heart disease. It shows functional processes of the body, and places of higher levels of activity show up as yellow. These often correspond to area's of disease.
51
Particles of an Isotope
1. These vary in number of neutrons
2. They are usually stable
3. Identical chemical properties of the element
4. They have a different mass (superscript before the symbol 1^H)
52
Atomic number
The number of protons in the nucleus.
53
Atomic Mass
1. This number is located at the bottom of the each square in the periodic table
2. Its also known as atomic weight, and is an average of all of its naturally occurring isotopes.
54
What is the atomic mass unit? (amu)
It is measured in daltons
55
Mass number
Is the sum of protons and neutrons
56
Where is the atomic number located?
At the top of each square in the periodic table
57
What is the name of the only element that does not occur on earth?
Technetium
Atomic number 43
It is artificially produced and not found on earth
Is used for medical treatments
58
Write two ways to express Technetium with a mass number of 99.
99^Tc or technetium-99
| it has 43 protons as indicated by the atomic number, and 56 neutrons
59
Electron Shell
are energy states that electrons occupy. The outer most shell determines the chemical properties of the element and is loosely associated with the nucleus.
60
What are the first four electron shells?
1s
2s
2p
3s
61
What is heavy water?
It is an isotope of hydrogen plus an oxygen atom. It is represented as D(sub 2)O.
62
Half-life
"the time required for one half the atoms of a given amount of a radioactive substance to disintegrate"
63
Nuclear fission
"The process in which the nucleus of radioisotopes comes apart." (The free dictionary)
64
Radioisotopes
A natural or artificially produced radioactive isotope of an element. (some combinations of protons and neutrons are unstable)
65
Decay
"To fall apart"
66
Affects of radiation exposure?
1. It interacts with human tissues and triggers chemical reactions that create free radicals and can with enough exposure, damage DNA.
2. Long term, low levels - increased occurrences of cancer.
3. Acute exposure - radiation burns, radiation sickness.
67
Beta particle
"are electrons expelled at high energy from radioactive atoms.
68
Gamma particle
Also known as an x-ray, it "is a high-energy packet of light energy(photon) Photons of lower energy lights are visible light."
69
Photons
Visible light. It is a particle and a wave. They have zero mass but a measurable momentum.
Examples of photons are "x-rays, gamma rays, ultraviolet, visible light, ect" (these are at different momentum (energy) and different wavelengths.)
70
Alpha particle
"2 protons and 2 neutrons bond together in a particle identical to a helium nucleus"
Produced by alpha decay, they are a dangerous form of radiation. (wiki)
71
Photon properties
Photons wave that has both electrical and magnetic properties - thus they are electromagnetic waves.
72
Wavelength
"Is the distance between the peak of each wave crest. Higher energy equals more vibration equals shorter wavelength"
73
Gamma ray
High energy, short wave length
74
What is beyond violet?
Beyond our eye sight is ultraviolet, x-ray, and last gamma rays.
75
Radio wave
"the lowest energy and longest wavelength
76
Visible light spectrum
"Red is the lowest energy/longest wave length, then orange, yellow, green, blue, indigo, and violet. The mnemonic for this sequence is ROY G. BIV"
77
Bones on an x-ray
x-rays can penetrate tissue but not bones, so bones appear white on an x-ray
78
Ion
An electrically charged atom by either the loss or gain of an electron.
79
Cation
A positively charged ion which is created by the loss of an electron(s) (it has more protons thus the positive charge) More protons than electrons.
80
Anion
A negatively charged ion which is created by the gain of an electron(s) (it has more electrons thus than protons)
81
Transition metals
They are located in the center of the periodic table and are not governed by simply filling electron shells. They are complicated. So Iron (a transition metal) can give a way two or three electrons.
82
Ferrous Ion
This is a transition metal that is important part of the molecule hemoglobin, because the ferrous ion (Fe^+2) binds with oxygen (O^-2).
83
Ferric ion
This is a transition metal that has given away three electrons (Fe^+3)
84
What are 4 electrolytes usually measured in the body?
Sodium (Na^+) Most common
Potassium (k^+)
Chloride (Cl^-) Common
Bicarbonate (HCOsub3^-) Common
85
Electrolytes
ions that are dissolved in the tissues of the body
86
Free radicals
Electrons like to hang out in pairs. When a molecule has an unpaired electron it is called a free radical. These are dangerous to biological systems and are believed to be a cause of cancer. They are created through normal cell function.
87
When writing a molecule what comes first?
The cation, then the anion. Generally speaking, if its symbol is on the left side of the periodic table, then its on the left side of the formula for the compound.`
88
Free radical scavengers
Lycopenes, omega-3, fatty acids, and vitamins C and E are thought to reduce the amount of free radicals in cells and prevent disease. (works in test tubes, humans? debatable)
89
Superoxide
O sub 2 ^ -
| The minus sign indicates an extra electron. It is a free radical molecule,
90
Polyatomic Ions or ionic compounds
* Elements that like to travel together in charged groups. Example: Sodium bicarbonate.
* When Polyatomic anions are looking to take electrons, they do so as a group.
* two polyatomic ions can combine
91
Hydroxyl group
when an -OH group is found in a molecule. Examples are alcohols and sugars
92
What does a superscript dot behind OH^. mean?
That its a free radical (unpaired electron) and polyatomic.
93
What is a name for the hydroxide ion?
Hydroxyl
94
How is the number of electrons indicated?
This is done by having the number of electrons subscripted in front of the element.
Examples:
^17 Cl (needs one more electron to be stable)
^19 K (wants to give one electron away)
95
C^+4
| What is the superscript +4
Its a valance. It usually indicates the number of electrons to be given or taken.
Taken to form anions are expressed as a negative number
Given to form cations are expressed as a positive number.
96
What is the valance of Nitrogen?
It can fill its outer shell ether by adding 3 electrons (-3) or by shedding 5 electrons (+5)
97
Valance Shell
The outer shell of electrons
98
Covalent bond
When two atoms share electrons. This is indicated by a single - between them. Such as H - H
99
Group number
Is the roman numeral at the top of each column of the periodic table. The number portion is mostly the same as the electrons in the outer shell.
100
What is the valance for lA?
+1
101
What is the valance for llA?
+2
102
What is the valance for lllA?
+3
103
What is the valance for lVA?
+4 -4
104
What is the valance for VA?
+5 -3
105
What is the valance for VlA?
-2
106
What is the valance for VllA?
-1
107
What is the valance for iron?
it is +2 or +3
| It is the only one you need to know from the center (transition metals) of the periodic table.
108
Covalent double bond and triple bonds
When two atoms share two electrons equally. this is indicated by a double line.
Example: O=O
Triple is the same except with an extra line, and they share three electrons.
109
Polar covalent bond or polar bond
When sharing electrons not all share equally. So if the electron being shared is drawn more to one than the other, it creates a slight negative charge on the greedy side, and a slight positive charge on the bullied side. Hsub2O is an example of polar covalent bonds.
110
What 3 elements frequently form polar covalent bonds?
Oxygen
Nitrogen
Sulfur
111
Ionic Bonds
* Mostly formed between metals and non-metals.
* They are attracted to opposite charges(thus between two ions) but do not actually share electron.
* Salt (NaCl) is an example of an ionic bond.
* They are easily disrupted in water
112
Why does salt dissolve in water?
Because salt is held together by ionic bonds and the polar covalent bonds have charges that disrupt the ionic bonds. Think about it.
113
Electronegativity
"Electronegativity is the power of an atom when in a molecule to attract electrons to itself", pg 89. SG
They are electron thieves.
It creates a dipole where there is a more positive charge towards one end, and a more negative towards the other.
114
What sign indicates electronegativity
The sigma, a cursive looking g with a + or -
115
What three elements are electron thieves biologically speaking?
(high electronegativity number)
Oxygen
Nitrogen
Sulfur
116
What is a partial ionic bond?
A hydrogen bond.
117
Hydrogen bond
Electronegative atoms such as Oxygen, Sulfur, and Nitrogen are involved with atoms of less electronegativity such as Hydrogen, and it creates a dipole. Thus the molecule is slightly negative at one end is attracted to another end of a molecule that is slightly positive.
118
List the bonds from strongest to weakest
Covalent - triple, double, single
ionic
hydrogen
119
Examples of covalent bonds
Gases dissolved in blood?
| Biologically important molecules such as protein primary sequence, single strands of DNA and RNA
120
Examples of ionic bonding
Teeth and bones
| Dissolved ions in electrolytes
121
Examples of hydrogen bonds
Holds protein structures
Holds two strands of DNA together
It keeps ketchup in a bottle
122
What is a title for water?
Near-Universal Solvent, because it readily forms hydrogen bonds between molecules.
123
Why does ice float?
Because water does not allow its molecules to rotate and pack as tightly as liquid water.
124
How else can H(sub2)O be written?
HOH
125
Surface Tension
"is a property that results from the cohesion of molecules to each other." Water with its hydrogen bond is a good example. This is only with Hydrogen bonds.
126
Surfactant
They interfere with hydrogen bonds. They create a hydration shell around themselves. Example is soap. One end likes grease, and the other end water.
127
Surfactant and your lungs
"Specialized cells in your lungs secrete surfactant to keep the lungs from collapsing due to surface tension" NICU babies can not produce this yet.
128
Capillary action
Surface tension + attraction between glass and water = capillary action
Thus why water climbs the wall of a glass container.
129
Solution
It is a combination of solvent and solute
130
Solvent
It dissolves another substance. There is usually more solvent than solute.
In the human body, the solvent is almost always water.
131
Solute
The substance being dissolved.
132
What is a mole?
It is a SI unit, for this class used to explain solute in a solution. Thus moles per liter (mol/L)
A mole is
6.02x10^20
133
What is Avogadro's number?
It is a mole - 6.02x10^20
This number is important because "One mole of a substance is equal to the same number of grams as the atomic mass" pg 97 SG
134
How are moles expressed in correlation to the body?
They are often used as millimoles per liter, or mmol/L
135
Colloids
"Is a substance microscopically dispersed throughout another substance" Wikipedia
Its particles are large enough to scatter light, thus they are translucent or opaque.
Particles remain dispersed even over long periods of time.
136
Size
| Colloids vrs Solutions
Solutions the dissolved particle is the size of an atom or molecule
Colloid, the particles are more like 200 times the size of an atom.
137
List the 3 types of mixtures?
1. Colloid
2. Solution
3. Suspension
138
Emulsion
"A Colloid where all components are liquid"
| Example is milk
139
Suspension
A mixture of larger particles than a colloid that will eventually settle to the bottom.
140
Blood in relation to mixtures
Colloid - The plasma is a colloid of proteins in a solution of salt in water.
Suspension - the cells are suspended in the plasma.
141
Acid
"Is a substance that dissociates into one or more hydrogen ions (cation) and one or more anions."
Example: Carbonic acid (Hsub2COsub3) which is critical in the maintenance of blood PH.
SG, pg 101
142
Base
"Is a substance that dissolves in water, releasing cations and OH- as an anion (negative ion).
143
Salt
"A salt is a substance which dissolves in water and releases ion. Neither ion is H+ or OH-."
144
Dissociate - in relation to bases and acids
They separate into ions and become surrounded by water molecules.
145
Explain the PH scale
It ranges from 0 to 14 with neutral being at 7. It is scale is based on the concentration of H+ ions in in moles per liter. Thus more H+ ions means its more acidic and less, more basic.
146
How is a base or acid considered to be strong or weak?
According to how much OH- ions or H+ ions are given off.
147
Buffer
"The chemical compounds that can convert strong acids or bases into weak ones by removing or adding protons (H+)" Text
"acts as a sponge to hold and inactivate H+ and/or OH-" SG
148
What is one of the most important buffers in the human body?
carbonic acid-bicarbonate buffer system and sodium phosphate is an important one too.
149
Acid on the PH scale
Has a PH number between 0-6.99
| More H+ than OH-
150
Base on the PH scale
Has a PH number between 7.01-14
| More OH- than H+
151
Neutral on the PH scale
Has equal amounts of H+ and OH-
| PH number of 7
152
Acids in the human body
Gastric juice, vaginal fluid, urine (most of the time) and saliva.
153
Bases in the human body
Urine (only rarely based on diet), blood semen cerebrospinal fluid, pancreatic juices and bile.
154
Another word for base solotions?
Alkaline solutions
155
What buffer regulates the PH of the blood?
Carbonic acid - bicarbonate buffer system
156
What is the PH of a healthy individuals blood?
7.4
| Normal range is 7.35 - 7.45
