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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
Q

Flourine

A

F

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26
Q

Neon

A

Ne

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27
Q

Sodium

A

Na

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28
Q

Magnesium

A

Mg

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29
Q

Aluminum

A

Al

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30
Q

Silicon

A

Si

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31
Q

Phosphorus

A

P

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32
Q

Sulfur

A

S

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33
Q

Argon

A

Ar

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34
Q

Potassium

A

K

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35
Q

Calcium

A

Ca

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36
Q

Iron

A

Fe

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37
Q

Selenium

A

Se

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38
Q

Bromine

A

Br

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39
Q

Krypton

A

Kr

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40
Q

Iodine

A

I

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41
Q

Xenon

A

Xe

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42
Q

Chemical reactions

A

Breaking and forming of chemical bonds

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43
Q

Chemical bonds

A

The basis for all biological systems, formed by atoms giving, taking, and sharing electrons

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44
Q

Valance orbital

A

The upper most orbital

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45
Q

Covalent bond

A

Bond formed between two or more atoms sharing electrons

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46
Q

Chemistry

A

Interaction of electrons with the collision of atoms

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47
Q

Electromagnetic spectrum

A

Lowest energy
1. Radio
2. Microwaves
3. Infrared
4. Visible
5. Ultraviolet
6. Xray
7. Gamma
Highest energy

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48
Q

Alpha particles

A
  1. Helium nuclei
  2. Low penetration
  3. High energy transfer
  4. Stopped by paper
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49
Q

Beta particles

A
  1. Stopped by aluminum
  2. Electron with a negative charge
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50
Q

Positrons

A
  1. Antimatter electrons with a positive charge
  2. PET
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51
Q

Electron capture

A

Electrons strikes a nucleus, emitting an xray (photon)

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52
Q

Gamma particles

A
  1. Penetrates deeply through tissue
  2. Release of a photon at a higher energy then x-ray
  3. Gamma knife
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53
Q

Isotopes

A

When the number of neutrons adjust, but protons stay the same.

54
Q

Radioisotopes

A
  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
Q

Isotopes of hydrogen

A

Protium - 1P 0N 1E
Deuterium- 1P 1N 1E
Tritium - 1P 2N 1E (radioactive)

56
Q

Atomic Number

A

Number of protons in an element

57
Q

Atomic mass number

A

The number of protons and number of neutrons

58
Q

The periodic table

A
  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
Q

Alkali metals

A

Group one
H, Li, Na, K, Rb, Cs, Fr

60
Q

Valence

A

The number of electrons lost, or the number of electrons gained to achieve a low energy stable state.

61
Q

Electronegativity

A

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
Q

Noble gases

A

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
Q

Neutral atom

A

The number of protons in the nucleus is equal to the number of electrons.

64
Q

Alkaline Earth Metals

A

Group 2 Be, Mg, Ca

65
Q

3 states of matter

A
  1. Gas
  2. Liquid
  3. Solid
66
Q

Gaseous State

A
  1. Indefinite shape and volume
  2. Highly Compressible
  3. Wide spread particles, flying around hitting each other
67
Q

Solid State

A
  1. Definite shape and volume
  2. Not Compressible
  3. Tightly associated structured particles
68
Q

Liquid State

A
  1. Indefinite shape and definite volume
  2. Not very Compressible
  3. Particles interacting with each other
69
Q

Kinetic Molecular Theory

A

The state of matter depends on the movement of molecules in relation to each other (kinesis)

70
Q

Entropy

A

Random distribution of particles

High entropy = High disorder and randomness

Low entropy = Low disorder and high structure

71
Q

Potential Energy

A

Energy that is stored, not yet able to do work. Like a coiled spring

72
Q

Kinetic energy

A

Energy of movement

73
Q

Type of energy in chemical bonds

A

Potential Energy

74
Q

Endothermic reaction

A

Endergonic/anabolic

  1. Absorbs energy
  2. Chemical reactions that convert kinetic energy to potential
  3. Start with less, end with more
75
Q

Exothermic reaction

A

Catabolic/exergonic

  1. Releases energy (gives off heat)
  2. Converts potential energy to kinetic energy
  3. Starts with more ends with less
76
Q

Non-polar single bond

A
  1. Equal sharing of electrons
  2. Indicated by a single line
  3. 🔺EN 0.0 - 0.5
77
Q

Non-polar Double bond

A
  1. sharing 4 of electrons
  2. Indicated by a double line
  3. 🔺EN 0.0 - 0.5
78
Q

Non-polar triple bond

A
  1. Sharing of 6 electrons
  2. Indicated by a triple line
  3. 🔺EN difference 0.0 - 0.5
79
Q

Polar bond

A
  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
Q

Ionic bonds

A
  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
Q

Hydrogen bond

A
  1. (O, N, S) with Hydrogen atom
  2. Attraction between the delta - and +
  3. Weakest of all bonds
82
Q

Bond strength

A

Strong to weak

1.Triple covalent
2.Double covalent
3.Single
4.Ionic
5.Hydrogen

83
Q

Surface tension

A
  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
Q

Surfacant

A

Biological soap that breaks hydrogen bonds

85
Q

CH3COO-

A

Acetate - POLYATOMIC

86
Q

HCO3-

A

Bicarbonate - POLYATOMIC

87
Q

CO3^2-

A

Carbonate - POLYATOMIC

88
Q

H2PO4-

A

Dihydrogen Phosphate - POLYATOMIC

89
Q

OH-

A

Hydroxide - POLYATOMIC

90
Q

HPO4^2-

A

Mono-hydrogen Phosphate - POLYATOMIC

91
Q

NO3-

A

Nitrate - POLYATOMIC

92
Q

NO2-

A

Nitrite - POLYATOMIC

93
Q

O2^2-

A

Peroxide - POLYATOMIC

94
Q

PO4^3-

A

Phosphate - POLYATOMIC

95
Q

SO4^2-

A

Sulfate - POLYATOMIC

96
Q

NH4+

A

Ammonium - POLYATOMIC

97
Q

H3O+

A

Hydronium - POLYATOMIC

98
Q

-OH

A

Hydroxyl - FUNCTIONAL GROUP

99
Q

-SH

A

Sulfhydryl - FUNCTIONAL GROUP

100
Q

-NH2

A

Amino - FUNCTIONAL GROUP

101
Q

C6H6

R-C6H6

A

Phenyl - FUNCTIONAL GROUP

Benzene Ring

102
Q

R-COOH

A

Carboxyl - FUNCTIONAL GROUP

103
Q

CH3-COOH

A

Acetic Acid - FUNCTIONAL GROUP
(Methyl + Carboxyl)

104
Q

R-CH3

A

Methyl - FUNCTIONAL GROUP

105
Q

R1-CH2-R2

A

Methylene - FUNCTIONAL GROUP

106
Q

R1-C-O-C-R2

A

Ether - FUNCTIONAL GROUP
(Dimethyl Ether)

107
Q

Orbitals

A
  1. Electrons fill each layer before moving on.
  2. All ⬆️ first then ⬇️
  3. 2-1s, 8-2s, 8-2p
108
Q

Acids

A

Proton donors
H+/H3O+

109
Q

Base

A

Proton acceptors

110
Q

Strong acids

A

Donate all protons - completely dissociate in water

111
Q

Weak acids

A

Donate small amount of protons

112
Q

Strong base

A

Accepts all protons - completely dissociate in water

113
Q

Weak base

A

Accepts small amounts of protons

114
Q

PH

A

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
Q

Buffer

A
  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
Q

Osmolarity

A

Total concentration of all solutes in the solution (OSM/L)

117
Q

Molarity

A

Number of moles of solute per liter of solution

118
Q

Avogados #

A
  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
Q

Suspension

A

Particles are size of cells and big enough to be separated, with a centrifuge.

120
Q

Colloid

A

Molecules are big enough to scatter light

121
Q

Solution

A

Small sized molecules surrounded by water, does not scatter light (clear)

122
Q

Hypertonic

A
  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
Q

Isotonic

A
  1. Balanced particle and water concentration inside and outside of the cell.
  2. No net water movement
124
Q

Hypotonic

A
  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
Q

Micelles

A

Clumps of protein molecules in a mixture

126
Q

Stoichometry

A

Balanced chemical equation by the reactant and product

127
Q

Monomers

A

Small, identical, or similar molecules

128
Q

Polymers

A

Large molecule made up of smaller subunits

129
Q

Dehydration synthesis

A
  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
Q

Hydrolysis

A
  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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