CH.2 ATOMS, IONS, & MOLECULES Flashcards
1
Q
What is Matter?
A
Composed of Atoms, Takes up space/ made up of Mass
2
Q
What are the three forms Matter comes in:
A
Solid, Liquid, Gas
3
Q
Atom
A
Smallest Particles that exhibits the chemical properties of an element.
4
Q
What are the 6 Major Elements of the Human Body?
A
Carbon, Hydrogen, Oxygen, Nitrogen, Calcium, Phosphorus
5
Q
What are the 6 minor Elements of the Human Body
A
Sulfur(S), Potassium(K), Sodium(Na), Chlorine(Cl), Magnesium(Mg), Iron (Fe)
6
Q
What are the Subatomic Particles?
A
Protons: +, 1amu
Neutron: Neutral, 1amu
Electron: -, 0amu (1.66x10-27)
7
Q
What are Isotopes?
A
Different # of Neutrons, but same # for Protons and Electrons.
8
Q
What are Radioistopes?
A
Unstable forms of isotopes, bc their Nuclei contains on excess # of Neurons.
Ex: Gamma Rays
9
Q
How Do Radioisotopes become more stable?
A
By decaying or breaking down over time.
10
Q
What is a Physical Half-Life
A
How long it takes for half of a substance to break down/ decay.
11
Q
What is a biological Half-Life
A
The time for half a radioactive material to be elmintated from the body. (Also can include nonradioactive, like Hormones, or drugs)
12
Q
What is Chemical Stability?
A
Happens when there is a complete Valence shell
13
Q
What are Noble Gases?
A
Atoms that don’t typically interaction with other elements (Right side of Periodic Table)
14
Q
Octet Rule
A
-Needs to have all 8 electrons.
-Gains chemical stability either by gaining, losing, or sharing electrons.
15
Q
Chemical Compound
A
Stable connections between two or more elements combined in a fixed ratio.
Ex: Ionic or Molecular Compounds
16
Q
Ionic Compounds
A
Structures combined with two or more charged elements.
17
Q
Ion
A
An atom (Or a group of atoms) that have charges.
Ex: Na+, H+, Cl-
18
Q
What are the two types of Ions
A
Cation: +, loses an electron.
Anion: -, Gains an electron.
19
Q
Polyatomic Ion
A
Composed of one or more charged atom.
Ex: HCO-3 (Has charge and more than one atom)
20
Q
Ionic Bonds
A
Cations and Anions binding together.
Even though they lose or gain electrons, they still are electrostatically attracted to each other
Ex: NaCl (Table salt)
21
Q
What does it mean to be Oxidized?
A
Loses Electron
22
Q
What does it mean to be Reduced
A
Gains an Electron
23
Q
Covalent Bonds
A
- Shares Electron between two elements.
-Makes Molecules - Most common elements seen is CHON
24
Q
Molecular Compounds
A
Molecules composed of Two or more elements within a covalent bond.
Ex: CO2, H2O
25
Molecular Formula:
The number & types of atoms in an element composing a molecule:
Ex: H2CO3= Carbonic Acid
26
Structural Formula
-Is Complementary to Molecular Formula
-Shows the spacial arrangements of the molecule.
Ex: CO2-> O=C=O
27
Isomers
Molecules composed of the type elements and #, (Molecular Formula).
28
Examples of Isomers
Glucose, Galatose, (diff placement of OH), Frustose (Different shape)
29
When Do covalent bonds happen?
- To make molecules
-To make both atoms chemically stable
30
What are the three types of Covalent Bonds:
Single Covalent Bonds (Least Strong)
Double Covalent Bonds
Triple Covalent bonds (Most Strongest)
31
What is Carbon Skeleton Formation
Arrangement of Carbon Atoms
32
What are the three types of Carbon Chains in the Skeleton Formation
Straight Chain (Lipids)
Branched Chain
Ring Chain (Glucose)
33
What is Electronegativty
Measure of the ability of an atom to attract electrons.
Not only determined by the # of protons but the proximity of Valence E- shells to Nucleus.
34
What are Non-polar Covalent Bonds
Equal sharing of Electrons,
-C-H, C-C,
-Hydrophobic
Ex: Triglycerides, mostly composed of non-polar bonds.
35
What are Polar Covalent bonds
Unequal sharing of Electrons
- H2O
-Hydrophilic
-Glucose
36
How is Electronegativity determined by the Periodic Table?
From bottom to the top, Electronegativty strong on top.
More to the right is strongest
37
How does Partial charges connect with Electronegativity
More Electronegativity= Partial Negative Charge.
Less Electronegativity= Partial Positive charge.
38
Amphipathic Molecules
Contains both polar and Nonpolar bonds/ components.
-Like Phospholipids,
Heads: Hydrophilic
Tails: Hydrophobic
39
Non-Polar Molecules
Contains primary non-polar bonds.
One Exception: If a molecule containing a polar bond that extends in opposite ways= Non-polar because the partial charges cancel each other.
Ex: Tryglycerides.
40
Polar Molecules
Contains primarly Polar bonds.
Ex: Glucose, Water
41
Intermolecular Attractions
- In between Molecules
-Weak Chemical Attraction to other molecules.
*Can involve non-polar molecules when for a brief second that have unequal electron attraction.
Ex: Water to Water
42
Hydrogen Bonds
Forms Between polar molecules
Weak Attraction between partial negative and positive.
43
Hydrophobic Interaction
Non-polar molecules are put into Polar Molecules
44
Intramolecular Attractions:
-Happens Within the molecule.
Like H-O-H= H2O
45
Organic Molecules
Molecules that contain Carbon, which are (or have been) components of living organisms.
Ex: Glucose, Protein, Tryglycerides.
46
Inorganic Molecules
All Other types of molecules.
Ex: Water, Salts (Sodium Chloride, Acids (Hydrochloric Acid) & Bases (Sodium Hydroxide.
47
What is Water
-Is composed of two Hydrogen Atoms & A Oxygen Atom.
-Universal Solvent.
48
What are the Four Major Roles of Water
-Transport Nutrients (Blood)
-Lubricates: (Serous Fluid between Heart Sac)
Cushions: the sudden movements is absorbed by water based Fluids (Cerebrospinal Spiral)
Excretes Wastes: Urine
49
What is Cohesion?
Attraction between Water to Water Molecules
50
What is Adhesion?
Attraction between Water Molecules and other substances. (Like a leaf and Water)
51
Surface Tension
Inward pulling of cohesive forces at the surface of water.
52
What is High Specific Heat for Water
-Amount of energy needed to break the Hydrogen bonds of water/ increase the temp to 1 gram to 1 C
53
What is Temperature?
Measured by the amount of Kinetic Energy or random movement of particles.
54
How does the Human Body temp stay constant (With the help of water and High Specific Heat)?
-Heat energy causes the Hydrogen Bond to break.
-The kinetic energy increases as the bonds break.
55
What is Heat of Vaporization
-Energy required for molecules to change from liquid to gasous form.
-Break all the hydrogen bonds to free the molecules (Turns into Vapor).
Ex: Sweating to Cool Down.
56
What is a Solvent
Liquid that dissolves the Solute into a solution.
Ex: Water
57
What is a Solute
The substance that is getting dissolved but the Solvent.
58
What are Substances that DO Dissolve in Water?
-Polar Molecules & Ions
- Electrolytes: Dissolve and Dissociate.
Ex: NaCl- (Table Salt)
-Non-Electrolytes: Only Dissolves
Ex: Glucose.
59
What are the Substances that Do NOT dissolve in Water?
-Non-polar Molecules
Hydrophobic Exclusion: Water sticks together but forces Non-polar molecules out.
- Ex: Oil & Water.
60
What are substances that Partially dissolve in Water?
-Amphipathic Molecules.
- Ex: Phospholipids
61
What is the Neutral Solvent & Why is it?
-Water because it spontaously dissociates to forms ions.
-The hydrogen bonds of one H2O breaks, releasing a H+ and the other H2O molecule accepts it.
62
When the Water dissociates and lets the H+ move freely out, where does it go?
Another water molecule accepts it.
-Dissociation Reaction:
H2O+H2O= H3O+ +OH-
OR
H2O = H+ + OH-
63
Equal Numbers of postively charged H+ and negatively charged OH-, is formed from Water dissociation.
64
What is an Acid
- Proton Donor
-#1-#6
- A substance that dissociates in water to produce more H+ and less OH-
Ex: Orange
65
Strong Acid
-A substance that has a greater extent to dissociate, and produce H+
(1-3)
- Hydrochloric Acid (HCl)
66
Weak Acid
A substance that doesn't dissociate as well and produces less H+
Ex: Carbonic Acid (H2CO3)
67
What is the equation for Acids
Substance A (Acid in Water) = (H+) + Anion
68
What is an Acidic Solution
Formed with the addition of Acid to water
69
What is a Base?
-Proton Acceptor
- Produces OH-, and uses H+ when it is present in solution.
(8-14)
70
What is the Base's Equation?
Substance B +H+= B-H
71
What are Strong Bases?
A substance that has a greater extent to bind to more H+ and produce it into OH-.
Ex: Sodium Hydroxide (NaOH)
72
What are Weak Bases?
A substance that binds to less H+, and produces more OH-
Ex: Bicarbonate (HCO3-)
73
What is a Base Solution
The addition of a base into the solution of water.
74
What is pH?
The measure of the amount of H+ in a substance.
- Is represented in a 10-fold like 10-1
75
What is a Buffer?
-It is a molecule or two or more different molecules that regulates the pH balance in the body.
-If pH increases/ more basic: Add more H+
-If pH decreases/ more acidic: Add OH-.
Ex: Bicarbonate (HCO3-) accepts H+ as an acid to the blood
76
What are mixtures?
Formed from combing or mixing two or more substances.
Ex: Sugar Water
77
What are two defining features of Mixtures
- It doesn't chemically change the substances that are mixed.
-Substances in the mixed can be physically separated either by Evaporation or filtering.
78
What are the Four Categories of Water Mixtures?
Suspensions, Colloids, Solutions, Emulsion.
79
What is Suspension
-Larger Particles
When the substance is not in motion, it settles down back into place.
-Appears in a opaque, cloudy, scatters when revealed to light.
-Ex: Whole Blood
80
What is Colloid?
-The Mixture composed of smaller particles than Suspension.
-Stays mixed in motion but separated.
Appear Milky or opaque, scatters in light.
Ex: Blood Plasma, Gelatin.
81
What is a solution
-Contains Smaller particles, and stays mixed when not in motion.
Ex: Soda
82
Emulsion
- Composed of water and Non-polar molecules.
-Doesn't stay mixed when in motion.
Just Hydrophobic Exclusion.
Ex: Oil & Water
83
What is the Expression of Solution Concentration?
It is the amount of solute dissolved in a solution determines the solubility of a solution.
84
What are the Four types of Solution Concentration
Mass/ Volume
Mass Volume Percent
Molarity
Molality
85
Mass/ Volume
-Mcg of Solute/ dL Of solution.
-mg of Solute/ dL Of Solution
Ex: Normal Blood Concentration of Iron is within 40-50 mcg/dL.
86
Mass/Volume percent
-Grams of Solute/ 100 mL.
Ex: 0.9% NaCl is 0.9 grams of NaCl per 100 mL
87
Molarity
-Moles of Solute/ L solution.
-Less accurate but more used
Ex: 1M glucose/ 1L water.
88
Molality
-Moles of Solute/ kg of Solvent.
- More accurate but used less.
Ex: 1M glucose/ 1 kg water
89
Which one is more influenced by Temperature
- Molarity.
Temperature increases, Molarity decreases because of the volume.
90
What is a Osmole?
Whether a substance dissolves & dissociate when placed in a solution.
-Term used to extent a solution is able to alter water movement through osmosis.
Ex: When glucose in a solution= 1osmole.
91
What is Osmolarity
of particles/ L of water.
92
Osmolality
of particles in a 1kg of water
-More accurately reflects osmotic movement of water in body but difficult to measure.
93
Moles
The mass in grams that is equal to either the amu or the molecular mass of a compound.
-Ex: Carbon= 12.01 amu= 12.01 grams
94
Molecular Mass:
By multiplying to amu and the # of atoms per Element. The add all the numbers together
95
What are Hydrocarbons? And where are they mostly seen in?
-Composed of molecules with single carbon atom or Carbon skeleton.
- C-C or C-H.
-Ex: Methane Gas (CH4)
96
What are Functional Groups?
Two or more atoms that when present together on a molecule, always exhibits the same specific Characteristics.
97
What are the four functional groups?
Hydroxyl, Carboxyl, Amine, & Phosphate
98
What is Hydroxyl?
--OH
-Polar
-Forms Hydrogen Bonds
-Increases molecules' solubility in water.
Seen in All Macromolecules.
99
What is Carboxyl?
-C=O
-OH
-Polar
-Forms Hydrogen bonds
-Increases molecules solubility in water.
Acts a an Acid
-Seen in Proteins and Lipids
100
Amine
-H-N-H
-Polar
-Forms Hydrogen Bonds
-Increases molecules solubility in water.
Acts as a base
-Seen in Protein and Nucleic Acids.
101
What is the structure of Phosphate? Function? And what macromolecules is it seen in?
O-P-O=O-O
-Polar
-Forms Hydrogen bonds
Forms Phosphodiester bonds.
-Acts as a Acid
-Seen in Nucleic Acids, Phospholipids, ATP
102
What are Polymers?
Made up of Monomers through the process of Dehydration Synthesis.
Ex: Proteins, Carbohydrates, Nucleic Acids.
103
What is Dehydration Synthesis
Monomer(OH-) + Monomer(H)= Polymer (With H2O)
104
What is Hydrolysis?
Polymer becoming Monomers and destroying H2O
105
What are Lipids?
Fats, that store energy, insulation.
-Hydrophobic
-Is not a polymer (Because they are formed from repeated monomers)
106
What are Tryglycerides?
-Formed from dehydration Synthesis
-Long Term storage for energy in Adipose CT.
-Structural Support, Cushioning.
107
What is the Compositions of Tryglycerides?
Composed of three fatty Acids, and Glycerol.
108
What is Saturated Fatty Acids:
-No double bonds
-Stays solid in room temp
109
What is Unsaturated Fatty Acids?
-1 double bonds
-Liquid in room temp
110
What are Polyunsaturated Fats?
-Composed of 2 or more double bonds.
111
What is the Process of making and destroying Polymers Called, for Lipids.
Lipogenesis: Dehydration Synthesis of the Fatty Acids & Glycerol to Tryglycerides.
Lipolysis: Hydrolysis from Tryglycerides to Fatty Acids & Glycerol.
112
What is a Phospholipid& What is its composition?
-In the Cell membrane
-Composed of Two fatty Acids, Phosphate group, Glycerol, and a few Organic Molecules.
-Is Amphipathic
113
What are Steroids?
-Composed of Hydrocarbons with Four Rings (Branched Chain).
Ex: Cholestrol, Hormones (Testosterone, Estrogen)
114
Eicosanoids
-Composed of 20- carbon fatty acids
Ex: Prostaglandins, (Used to help with the inflammatory in Immune system, and Nervous System).
115
What are Glycolipids?
Carbohydrates linked with Lipids.
116
What is Carbohydrates General Chemical Formula?
(CH2O)n
n= # of carbon atoms that are in one molecule, 3-7
117
What are Monosaccharides, Disaccharides, and Polysaccharides?
Mono + Mono = Dimer (Disaccharide) + Disaccharide = Polysaccharide.
118
Give me examples of Monosaccharides Hexose
-Galatose & Fructose.
6-Carbon
119
Give me examples of Monosaccharides/ Pentose
Ribose & Deoxyribose
-5 Carbon
120
Give me examples of Dissaccharides.
Lactose (Milk sugar), Maltose (Malt Sugar), Sucrose (table Sugars).
- A monomer with glucose.
121
What is Glycogen?
-Seen in Liver in Skeletal Muscle tissue absorb the excess glucose the bind the Glucose monomers
122
What is the Process of making and destroying Polymers Called, for Carbohydrates
Glycogenesis: Using Glucose to make Glycogen.
Glycogenolysis: Break glycogen to create glucose.
123
Glycosaminoglycans (GAGs)
-Large carbohydrate molecules w/ Amine groups.
- Attached to a protein Proteoglycans.
124
What are Nucleotides composed of?
Sugar (Pentose Sugar), Phosphate group, Nitrogenous Base.
125
Types of Nitrogenous Base
Single Ring (Pyrimidines)
Double Ring (Purines)
126
Names of the Pyrimidines?
Cytosine, Uracil, Thymine
127
Names of Purines?
Guanine & Adenine
128
What Specific Covalent bond links together the monomers within DNA & RNA?
-Phosphodiester.
129
DNA: Number of Strand, Sugar, Nitrogenous Base
2, Deoxyribose, Thymine.
130
RNA: Number of Strand, Sugar, Nitrogenous Base
1, Ribose, Uracil
131
What is Adenosine Triphosphate? What is the Nitrogenous base, Sugar, & P group
ATP, Nitrogenous base: Adenine, Ribose sugar, Three phosphate.
132
What are the other two Dinucleotides
Nicotinamide Adenine Dinucleotide (NAD+) &
Flavin Adenine Dinucleotide (FAD)
133
What are Protein composed?
-Polymer
-Composed of one or more Amino Acids Monomers.
-We have 20 AA
134
What are Proteins Functions:
-Catalyzes Reactions (Enzyme)
-Structural Support (Cytoskeleton)
-Body Movement (Myosin)
-Transports in Blood (Plasma)
-Membrane Transport
-Protection (Antibodies)
135
Oligopeptide
-A strand of a small # of AA (3-20).
- Smaller than Polypeptide.
136
Polypeptide
-Larger strand of AA
137
Glycoproteins
Proteins w/ Carbohydrates attached.
Ex: Determines ABO blood type
138
Four Categories of Amino Acids
Non-polar, Polar, Charged Ions, AA W/ Special Functions.
139
What do Non-Polar Amino Acids contain? & Who do they tend to group with?
Contains: R-group with either Hydrogen (Glycine) or Hydrocarbons (Alanine, Valine, Leucine, Isoleucine, Phenylalanine, Trytophan).
-Tend to group w/ hydrophobic or Non-polar AA.
140
Polar Amino Acids
-Contains: R groups w/elements in addition to Carbon & Hydrogen (ONS)
-(Serene, Threonine, Asparagine, Glutamine, Tyrosine).
-Other polar AA
141
What are Charged Amino Acids composed of?
Negative Charged R group: Glutamate & Aspartate.
Positive: Histidine, Lysine, Arginine.
Electrostatic Interation.
142
Electrostatic Interaction
An Ionic Bonds can form between both charges.
143
*AA w/ Special Function
-Proline Cysteine & Methionine.
- Proline: R group attaches the Amine group, forming a ring. Hydrophilic & Increases the solubility of protein in Water.
- Cysteine (Disulfide Bonds): Stabilizes the folding of a protein, Form by the Sulfhydryl (-S-H)
-Methionine: First AA positioned where a protein is synthesized & may OR may not be removed.
144
The Complex structures in Protein are dependent on what type of Attraction?
Intramolecular Attraction between AA in Linear Sequence for proper folding & maintaining of a protein's conformation.
145
What are Chaperones?
Assisting of protein folding by specialized proteins.
146
What are the Four Protein Formation Structures?
Primary, Secondary, Tertiary, and Quaternary Structure.
147
What is Primary Structure?
Linear Sequence of AA joined by peptide bonds.
-Is forced into its initial shape as Hydrophobic exclusion "tucks" AA w/ non-polar R groups.
-Hydrogen bonds form between the polar R groups (between Amine & Carboxylic)
-Ionic Bonds form between an AA w/ A Anion R group.
-Disfulfide bonds form between Sulfhydryl (-S-H) groups of two cysteine AA.
148
What is the Secondary Structure
Structural patterns start to form within the protein. (created Hydrogen bonds).
- Alpha Helix (Coil), and beta sheet (Zig Zag).
149
What is the Tertiary Structure?
Final 3-D shape of a protein.
-Globular Protein (Fold into compact, spherical shape like enzymes)
-Fibrous Proteins: Extend linear molecules (Like Cytoskeleton)
150
What is the Quaternary Structure?
Molecule composed of two or more separate proteins.
Ex: Hemoglobin.
151
What is Protein Conformation?
Protein that forms/folds into it's 3D shape
152
What is a Prosthetic Group?
- Nonprotein structure covalently bonded to the protein.
- Normal Function of a proteins may require this.
Ex: Lipid heme group in Hemoglobin protein.
153
What is Denaturation and What part of the Protein structure does it disrupt?
-When the protein loses its shape causing it to lose its function
-Happens in the Tertiary Structure
154
What are the 2 Factors that causes Denaturation in Proteins?
Changes in pH & Increase in temperature
155
What are the details of how changes in pH causes denaturation?
Changes in pH: Alters the H+ concentration which interferes with the Electrostatic Interaction (Ionic Bonds).
-Increase pH= Decrease H+: Disrupts the H+ that was participating in E.T
-Decrease pH= Increase H+: Excess H+ binds to negatively charged R groups, then loses it's negative Charge that helped the E.T
156
What are the details of how increase in temperature denatures the Protein?
- Weakens the intramolecular interactions that hold the protein in it's 3D shape.
