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A&P 1 > Unit 2 > Flashcards

Unit 2 Flashcards

1
Q

Atoms

A

Smallest unit of matter to retain characteristics of an element.

Diameter 10^-10m (0.1nm)

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2
Q

Elements

A

Substances with different chemical properties (e.g. Oxygen, Hydrogen, Carbon, Nitrogen)

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3
Q

Sub atomic particles

A

Smaller than an atom (protons, neutrons, electrons)

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4
Q

Proton

A
  1. Positive (+)
  2. In the Nucleus
  3. Mass of 1
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5
Q

Neutron

A
  1. Neutral (No charge)
  2. In the nucleus
  3. Mass of 1
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6
Q

Electrons

A
  1. Negative (-)
  2. Surrounding the nucleus in an electron cloud
  3. Low energy closer to the nucleus
  4. High energy further from nucleus
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7
Q

Atomic Mass Unit

A

1 AMU = 1 Dalton (Da)

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8
Q

Ion

A

Number of electrons and protons are different.

Cation = more protons
Anion = more electrons

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9
Q

Cation

A

More protons

E.g. Potassium charged +1 = 19P/18E

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10
Q

Anion

A

More electrons

E.g. Chloride charged -1 = 17P/18E

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11
Q

Photon

A
  1. Particle of light
  2. Excess energy as electrons rearrange/shed
  3. Visible light, UV, X-ray, Gamma Rays all made of photons
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12
Q

Visible light

A

Low Energy/Long wavelength

  1. Red - 700 nm
  2. Orange
  3. Yellow
  4. Green
  5. Blue
  6. Indigo
  7. Violet - 400 nm

High Energy/Short wavelength

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13
Q

Ultraviolet

A
  1. Enough energy to cause 1st degree burns/Sunburn
  2. Can cause scar tissue on cornea/lens
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14
Q

X-Rays

A
  1. Photons with high energy to penetrate living tissue
  2. Stopped by bone
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15
Q

Gamma Rays

A
  1. Radioisotope - High energy photons
  2. Used to destroy tissues that cannot be reached surgically
  3. Penetrate living tissue and cause damage to tissues
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16
Q

Wavelengths

A

Long - low energy/frequency
Short - high energy/frequency

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17
Q

Hydrogen

A

H

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18
Q

Helium

A

He

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19
Q

Lithium

A

Li

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20
Q

Beryllium

A

Be

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21
Q

Boron

A

B

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22
Q

Carbon

A

C

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23
Q

Nitrogen

A

N

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24
Q

Oxygen

A

O

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25
Flourine
F
26
Neon
Ne
27
Sodium
Na
28
Magnesium
Mg
29
Aluminum
Al
30
Silicon
Si
31
Phosphorus
P
32
Sulfur
S
33
Argon
Ar
34
Potassium
K
35
Calcium
Ca
36
Iron
Fe
37
Selenium
Se
38
Bromine
Br
39
Krypton
Kr
40
Iodine
I
41
Xenon
Xe
42
Chemical reactions
Breaking and forming of chemical bonds
43
Chemical bonds
The basis for all biological systems, formed by atoms giving, taking, and sharing electrons
44
Valance orbital
The upper most orbital
45
Covalent bond
Bond formed between two or more atoms sharing electrons
46
Chemistry
Interaction of electrons with the collision of atoms
47
Electromagnetic spectrum
Lowest energy 1. Radio 2. Microwaves 3. Infrared 4. Visible 5. Ultraviolet 6. Xray 7. Gamma Highest energy
48
Alpha particles
1. Helium nuclei 2. Low penetration 3. High energy transfer 4. Stopped by paper
49
Beta particles
1. Stopped by aluminum 2. Electron with a negative charge
50
Positrons
1. Antimatter electrons with a positive charge 2. PET
51
Electron capture
Electrons strikes a nucleus, emitting an xray (photon)
52
Gamma particles
1. Penetrates deeply through tissue 2. Release of a photon at a higher energy then x-ray 3. Gamma knife
53
Isotopes
When the number of neutrons adjust, but protons stay the same.
54
Radioisotopes
1. Isotopes that are unstable due to the different number of neutrons versus protons. 2. Used for nuclear medicine 3. Unstable equals radioactive 4. The more unstable the faster it will rearrange equals radioactive decay
55
Isotopes of hydrogen
Protium - 1P 0N 1E Deuterium- 1P 1N 1E Tritium - 1P 2N 1E (radioactive)
56
Atomic Number
Number of protons in an element
57
Atomic mass number
The number of protons and number of neutrons
58
The periodic table
1. Elements listed by order of atomic number 2. Each column is called a group and each group have similar chemical properties 3. Each row is called a period
59
Alkali metals
Group one H, Li, Na, K, Rb, Cs, Fr
60
Valence
The number of electrons lost, or the number of electrons gained to achieve a low energy stable state.
61
Electronegativity
Electron pulling capacity of an atom Most electronegative- F>O>Cl>N>Br>S Generally, increases moving towards the top right of the periodic table
62
Noble gases
2_He, 10_Ne, 18_Ar, 36_Kr, 54_Xe, 86_Rn 1. Inert/zero valance/shells filled completely 2. Do not participate in chem reactions
63
Neutral atom
The number of protons in the nucleus is equal to the number of electrons.
64
Alkaline Earth Metals
Group 2 Be, Mg, Ca
65
3 states of matter
1. Gas 2. Liquid 3. Solid
66
Gaseous State
1. Indefinite shape and volume 2. Highly Compressible 3. Wide spread particles, flying around hitting each other
67
Solid State
1. Definite shape and volume 2. Not Compressible 3. Tightly associated structured particles
68
Liquid State
1. Indefinite shape and definite volume 2. Not very Compressible 3. Particles interacting with each other
69
Kinetic Molecular Theory
The state of matter depends on the movement of molecules in relation to each other (kinesis)
70
Entropy
Random distribution of particles High entropy = High disorder and randomness Low entropy = Low disorder and high structure
71
Potential Energy
Energy that is stored, not yet able to do work. Like a coiled spring
72
Kinetic energy
Energy of movement
73
Type of energy in chemical bonds
Potential Energy
74
Endothermic reaction
Endergonic/anabolic 1. Absorbs energy 2. Chemical reactions that convert kinetic energy to potential 3. Start with less, end with more
75
Exothermic reaction
Catabolic/exergonic 1. Releases energy (gives off heat) 2. Converts potential energy to kinetic energy 3. Starts with more ends with less
76
Non-polar single bond
1. Equal sharing of electrons 2. Indicated by a single line 3. 🔺EN 0.0 - 0.5
77
Non-polar Double bond
1. sharing 4 of electrons 2. Indicated by a double line 3. 🔺EN 0.0 - 0.5
78
Non-polar triple bond
1. Sharing of 6 electrons 2. Indicated by a triple line 3. 🔺EN difference 0.0 - 0.5
79
Polar bond
1. Sharing of electrons but unequally 2. The nucleus that has higher EN will likely pull the electrons and have a partial negative delta 3. The nucleus that has the lower EN will have a partial positive delta 4. 🔺EN difference 0.5 - 1.7
80
Ionic bonds
1. Result from complete removal or addition of electrons 2. Highly EN atom just takes the electron and acquires a full valance charge (-) 3. Lower EN atom loses the electrons and acquires a positive valence charge (+) 4. These two attract to form the ionic bond 5.🔺EN difference 1.7 - 4.0
81
Hydrogen bond
1. (O, N, S) with Hydrogen atom 2. Attraction between the delta - and + 3. Weakest of all bonds
82
Bond strength
Strong to weak 1.Triple covalent 2.Double covalent 3.Single 4.Ionic 5.Hydrogen
83
Surface tension
1. Results from hydrogen bonds between water. 2. Water are molecules are strongly attracted to each other and pull together like an elastic sheet.
84
Surfacant
Biological soap that breaks hydrogen bonds
85
CH3COO-
Acetate - POLYATOMIC
86
HCO3-
Bicarbonate - POLYATOMIC
87
CO3^2-
Carbonate - POLYATOMIC
88
H2PO4-
Dihydrogen Phosphate - POLYATOMIC
89
OH-
Hydroxide - POLYATOMIC
90
HPO4^2-
Mono-hydrogen Phosphate - POLYATOMIC
91
NO3-
Nitrate - POLYATOMIC
92
NO2-
Nitrite - POLYATOMIC
93
O2^2-
Peroxide - POLYATOMIC
94
PO4^3-
Phosphate - POLYATOMIC
95
SO4^2-
Sulfate - POLYATOMIC
96
NH4+
Ammonium - POLYATOMIC
97
H3O+
Hydronium - POLYATOMIC
98
-OH
Hydroxyl - FUNCTIONAL GROUP
99
-SH
Sulfhydryl - FUNCTIONAL GROUP
100
-NH2
Amino - FUNCTIONAL GROUP
101
C6H6 R-C6H6
Phenyl - FUNCTIONAL GROUP Benzene Ring
102
R-COOH
Carboxyl - FUNCTIONAL GROUP
103
CH3-COOH
Acetic Acid - FUNCTIONAL GROUP (Methyl + Carboxyl)
104
R-CH3
Methyl - FUNCTIONAL GROUP
105
R1-CH2-R2
Methylene - FUNCTIONAL GROUP
106
R1-C-O-C-R2
Ether - FUNCTIONAL GROUP (Dimethyl Ether)
107
Orbitals
1. Electrons fill each layer before moving on. 2. All ⬆️ first then ⬇️ 3. 2-1s, 8-2s, 8-2p
108
Acids
Proton donors H+/H3O+
109
Base
Proton acceptors
110
Strong acids
Donate all protons - completely dissociate in water
111
Weak acids
Donate small amount of protons
112
Strong base
Accepts all protons - completely dissociate in water
113
Weak base
Accepts small amounts of protons
114
PH
Scale from 1-14 for how weak/strong an acid and base are. 1 Strong acid (10-1) 7 Neutrals (water) 14 Strong base (10-14) Scale is logarithmic (each unit is power of 10)
115
Buffer
1. Chemical that minimizes PH change. 2. H+(cation) or A- (anion) act as sponges for excess ions 3. When H+ or A- is present, the ion can donate or except hydrogen to keep the pH concentration nearly constant.
116
Osmolarity
Total concentration of all solutes in the solution (OSM/L)
117
Molarity
Number of moles of solute per liter of solution
118
Avogados #
1. 6.02x10^23 2. Equal to 1 Mole 3. There is 6.02×10^23 molecules in X grams of an element where X equals atomic mass of the element.
119
Suspension
Particles are size of cells and big enough to be separated, with a centrifuge.
120
Colloid
Molecules are big enough to scatter light
121
Solution
Small sized molecules surrounded by water, does not scatter light (clear)
122
Hypertonic
1. Particle concentration high/low water concentration outside the cell. 2. Low particle concentration/High water concentration inside the cell. 3. Water moves out of the cell
123
Isotonic
1. Balanced particle and water concentration inside and outside of the cell. 2. No net water movement
124
Hypotonic
1. Particle concentration low/high water concentration outside the cell. 2. High particle concentration/low water concentration inside the cell. 3. Water moves into the cell
125
Micelles
Clumps of protein molecules in a mixture
126
Stoichometry
Balanced chemical equation by the reactant and product
127
Monomers
Small, identical, or similar molecules
128
Polymers
Large molecule made up of smaller subunits
129
Dehydration synthesis
1. Used to join many different monomers into a polymer 2. Joined by removal of OH from one and H from another Monomer. Joined by covalent bond with O.
130
Hydrolysis
1. To break up a larger polymer into smaller pieces. 2. Adding OH to one monomer and H to another by the addition of a water molecule.

A&P 1 (4 decks)

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