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Bio Med > Vocab, Unit 2 > Flashcards

Vocab, Unit 2 Flashcards

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Biology 101 flashcards
1
Q

Atom

A

“The smallest unit of matter which retain the properties and characteristics of the element.”

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2
Q

Element

A

A substance which cannot be split into simpler substances by chemical means.

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3
Q

What are the first four ingredients(elements) of a human?

A
  1. Oxygen (65%)
  2. Carbon (18.5%)
  3. Hydrogen (9.5%)
  4. Nitrogen (3.2%)
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4
Q

Molecules

A

“two or more atoms sharing electrons joined by a chemical bond”

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5
Q

What is a subscript?

A

“It is the number of each type of atom in a molecule”

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6
Q

Compound

A

Composed of two or more elements

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7
Q

Table salt

A

NaCL

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8
Q

Common mineral in the Great Salt Lake

A

CaCL(sub)2

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9
Q

What are the 3 states of matter?

A
  1. Solid
  2. Liquid
  3. Gas
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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.”

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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”

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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.”

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13
Q

Potential engery

A

“is stored energy that is not yet able to do work.”

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14
Q

Kinetic energy

A

Its potential energy that is usable - “energy of movement”

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15
Q

Endergonic

A

“reactions that store energy” Energy can be stored in chemical bonds.

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16
Q

Exergonic

A

A reaction that releases energy.

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17
Q

Catabolic reactions, (catabolism)

A

“Chemical reactions that break down complex organic compounds into simple ones, with the net release of energy.”

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18
Q

Anabolic Reactions (Anabolism)

A

“Synthetic, energy requiring reactions whereby small molecules are built up into larger ones.”

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19
Q

Heat

A

often a byproduct of work, and is utilized by the body to maintain temperature

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20
Q

Work

A

energy put to good use

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21
Q

Entropy

A

As particles move, they bounce around and become disorganized. Entropy is moving from order to disorder.

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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.”

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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.

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24
Q

Specific heat

A

“the amount of energy it takes to raise a gram of substance one degree of temperature”

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25
Q

High specific heat

A

“Difficult to heat up, but once heated they stay hot for a long time”

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26
Q

Low specific heat

A

“They get hot fast, and cool off fast”

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27
Q

What is the specific heat of water?

A

1.000 - it has a high specific heat

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28
Q

What is the specific heat of Ice?

A

0.492

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29
Q

What is the specific heat of Gold?

A

0.0312

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30
Q

What is the specific heat of Lead?

A

0.0305 - it has a low specific heat

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31
Q

Conversion of food Calorie to metric calories?

A

1 food Calorie = 1000 metric calories.

C’s are capitalized to remind about the abbreviation

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32
Q

Calorie

A

“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.

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33
Q

Food calorie

A

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.

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34
Q

Who created the periodic table?

A

Mendeleev in 1869

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35
Q

Atomic number

A

The number of protons in a nucleus

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36
Q

Periodic table: Metals are found where?

A

They are located on the left 2/3 of the table.

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37
Q

Periodic table: non metals are found where?

A

They are located on the far right side of the table. Triangle type shape.

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38
Q

Hydrogen - metal or not?

A

It is technically a metal, but is generally not called one.

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39
Q

What is the most common noble gas?

A

Argon. It is found naturally in the atmosphere and is simply Ar.

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40
Q

What is a metalloid?

A

A element that shares both metal and non-metal properties.

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41
Q

What is a noble gas?

A
  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.
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42
Q

List the three subatomic particles or elementary particles

A
  1. Electron
  2. Proton
  3. Neutron
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43
Q

Electron

A
  1. The smallest of the particles
  2. Carries a negative charge
  3. They do not travel in an orbit.
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44
Q

Particles of an Atom

A

Electrons are equal to protons

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45
Q

Particles of an Ion

A

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+ )

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46
Q

Neutron

A
  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)
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47
Q

Proton

A
  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.
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48
Q

What does a MRI work off of?

A

“The magnetic properties of hydrogen nuclei”

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49
Q

Positron

A

These are like electrons, except they carry a positive charge. They are used in positron-emission tomography (PET)

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50
Q

What is Positron-emission tomography?

A

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.

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51
Q

Particles of an Isotope

A
  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)
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52
Q

Atomic number

A

The number of protons in the nucleus.

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53
Q

Atomic Mass

A
  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.
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54
Q

What is the atomic mass unit? (amu)

A

It is measured in daltons

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55
Q

Mass number

A

Is the sum of protons and neutrons

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56
Q

Where is the atomic number located?

A

At the top of each square in the periodic table

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57
Q

What is the name of the only element that does not occur on earth?

A

Technetium
Atomic number 43
It is artificially produced and not found on earth
Is used for medical treatments

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58
Q

Write two ways to express Technetium with a mass number of 99.

A

99^Tc or technetium-99

it has 43 protons as indicated by the atomic number, and 56 neutrons

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59
Q

Electron Shell

A

are energy states that electrons occupy. The outer most shell determines the chemical properties of the element and is loosely associated with the nucleus.

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60
Q

What are the first four electron shells?

A

1s
2s
2p
3s

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61
Q

What is heavy water?

A

It is an isotope of hydrogen plus an oxygen atom. It is represented as D(sub 2)O.

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62
Q

Half-life

A

“the time required for one half the atoms of a given amount of a radioactive substance to disintegrate”

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63
Q

Nuclear fission

A

“The process in which the nucleus of radioisotopes comes apart.” (The free dictionary)

64
Q

Radioisotopes

A

A natural or artificially produced radioactive isotope of an element. (some combinations of protons and neutrons are unstable)

65
Q

Decay

A

“To fall apart”

66
Q

Affects of radiation exposure?

A
  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
Q

Beta particle

A

“are electrons expelled at high energy from radioactive atoms.

68
Q

Gamma particle

A

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
Q

Photons

A

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
Q

Alpha particle

A

“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
Q

Photon properties

A

Photons wave that has both electrical and magnetic properties - thus they are electromagnetic waves.

72
Q

Wavelength

A

“Is the distance between the peak of each wave crest. Higher energy equals more vibration equals shorter wavelength”

73
Q

Gamma ray

A

High energy, short wave length

74
Q

What is beyond violet?

A

Beyond our eye sight is ultraviolet, x-ray, and last gamma rays.

75
Q

Radio wave

A

“the lowest energy and longest wavelength

76
Q

Visible light spectrum

A

“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
Q

Bones on an x-ray

A

x-rays can penetrate tissue but not bones, so bones appear white on an x-ray

78
Q

Ion

A

An electrically charged atom by either the loss or gain of an electron.

79
Q

Cation

A

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
Q

Anion

A

A negatively charged ion which is created by the gain of an electron(s) (it has more electrons thus than protons)

81
Q

Transition metals

A

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
Q

Ferrous Ion

A

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
Q

Ferric ion

A

This is a transition metal that has given away three electrons (Fe^+3)

84
Q

What are 4 electrolytes usually measured in the body?

A

Sodium (Na^+) Most common
Potassium (k^+)
Chloride (Cl^-) Common
Bicarbonate (HCOsub3^-) Common

85
Q

Electrolytes

A

ions that are dissolved in the tissues of the body

86
Q

Free radicals

A

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
Q

When writing a molecule what comes first?

A

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
Q

Free radical scavengers

A

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
Q

Superoxide

A

O sub 2 ^ -

The minus sign indicates an extra electron. It is a free radical molecule,

90
Q

Polyatomic Ions or ionic compounds

A
  • 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
Q

Hydroxyl group

A

when an -OH group is found in a molecule. Examples are alcohols and sugars

92
Q

What does a superscript dot behind OH^. mean?

A

That its a free radical (unpaired electron) and polyatomic.

93
Q

What is a name for the hydroxide ion?

A

Hydroxyl

94
Q

How is the number of electrons indicated?

A

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
Q

C^+4

What is the superscript +4

A

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
Q

What is the valance of Nitrogen?

A

It can fill its outer shell ether by adding 3 electrons (-3) or by shedding 5 electrons (+5)

97
Q

Valance Shell

A

The outer shell of electrons

98
Q

Covalent bond

A

When two atoms share electrons. This is indicated by a single - between them. Such as H - H

99
Q

Group number

A

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
Q

What is the valance for lA?

A

+1

101
Q

What is the valance for llA?

A

+2

102
Q

What is the valance for lllA?

A

+3

103
Q

What is the valance for lVA?

A

+4 -4

104
Q

What is the valance for VA?

A

+5 -3

105
Q

What is the valance for VlA?

A

-2

106
Q

What is the valance for VllA?

A

-1

107
Q

What is the valance for iron?

A

it is +2 or +3

It is the only one you need to know from the center (transition metals) of the periodic table.

108
Q

Covalent double bond and triple bonds

A

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
Q

Polar covalent bond or polar bond

A

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
Q

What 3 elements frequently form polar covalent bonds?

A

Oxygen
Nitrogen
Sulfur

111
Q

Ionic Bonds

A
  • 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
Q

Why does salt dissolve in water?

A

Because salt is held together by ionic bonds and the polar covalent bonds have charges that disrupt the ionic bonds. Think about it.

113
Q

Electronegativity

A

“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
Q

What sign indicates electronegativity

A

The sigma, a cursive looking g with a + or -

115
Q

What three elements are electron thieves biologically speaking?
(high electronegativity number)

A

Oxygen
Nitrogen
Sulfur

116
Q

What is a partial ionic bond?

A

A hydrogen bond.

117
Q

Hydrogen bond

A

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
Q

List the bonds from strongest to weakest

A

Covalent - triple, double, single
ionic
hydrogen

119
Q

Examples of covalent bonds

A

Gases dissolved in blood?

Biologically important molecules such as protein primary sequence, single strands of DNA and RNA

120
Q

Examples of ionic bonding

A

Teeth and bones

Dissolved ions in electrolytes

121
Q

Examples of hydrogen bonds

A

Holds protein structures
Holds two strands of DNA together
It keeps ketchup in a bottle

122
Q

What is a title for water?

A

Near-Universal Solvent, because it readily forms hydrogen bonds between molecules.

123
Q

Why does ice float?

A

Because water does not allow its molecules to rotate and pack as tightly as liquid water.

124
Q

How else can H(sub2)O be written?

A

HOH

125
Q

Surface Tension

A

“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
Q

Surfactant

A

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
Q

Surfactant and your lungs

A

“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
Q

Capillary action

A

Surface tension + attraction between glass and water = capillary action

Thus why water climbs the wall of a glass container.

129
Q

Solution

A

It is a combination of solvent and solute

130
Q

Solvent

A

It dissolves another substance. There is usually more solvent than solute.

In the human body, the solvent is almost always water.

131
Q

Solute

A

The substance being dissolved.

132
Q

What is a mole?

A

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
Q

What is Avogadro’s number?

A

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
Q

How are moles expressed in correlation to the body?

A

They are often used as millimoles per liter, or mmol/L

135
Q

Colloids

A

“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
Q

Size

Colloids vrs Solutions

A

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
Q

List the 3 types of mixtures?

A
  1. Colloid
  2. Solution
  3. Suspension
138
Q

Emulsion

A

“A Colloid where all components are liquid”

Example is milk

139
Q

Suspension

A

A mixture of larger particles than a colloid that will eventually settle to the bottom.

140
Q

Blood in relation to mixtures

A

Colloid - The plasma is a colloid of proteins in a solution of salt in water.

Suspension - the cells are suspended in the plasma.

141
Q

Acid

A

“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
Q

Base

A

“Is a substance that dissolves in water, releasing cations and OH- as an anion (negative ion).

143
Q

Salt

A

“A salt is a substance which dissolves in water and releases ion. Neither ion is H+ or OH-.”

144
Q

Dissociate - in relation to bases and acids

A

They separate into ions and become surrounded by water molecules.

145
Q

Explain the PH scale

A

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
Q

How is a base or acid considered to be strong or weak?

A

According to how much OH- ions or H+ ions are given off.

147
Q

Buffer

A

“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
Q

What is one of the most important buffers in the human body?

A

carbonic acid-bicarbonate buffer system and sodium phosphate is an important one too.

149
Q

Acid on the PH scale

A

Has a PH number between 0-6.99

More H+ than OH-

150
Q

Base on the PH scale

A

Has a PH number between 7.01-14

More OH- than H+

151
Q

Neutral on the PH scale

A

Has equal amounts of H+ and OH-

PH number of 7

152
Q

Acids in the human body

A

Gastric juice, vaginal fluid, urine (most of the time) and saliva.

153
Q

Bases in the human body

A

Urine (only rarely based on diet), blood semen cerebrospinal fluid, pancreatic juices and bile.

154
Q

Another word for base solotions?

A

Alkaline solutions

155
Q

What buffer regulates the PH of the blood?

A

Carbonic acid - bicarbonate buffer system

156
Q

What is the PH of a healthy individuals blood?

A

7.4

Normal range is 7.35 - 7.45

Bio Med (5 decks)

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