Chapter 2 BIO Powerpoint Flashcards
(254 cards)
1
Q
All living and non living things are made of
A
Matter
2
Q
Matter
A
Anything that occupies space and has mass
3
Q
Types of matter
A
Liquid, solids and gas
4
Q
Difference between mass and weight
A
Mass is the amount of matter an object contains
Weight is the measure of the force of gravity on mass
Mass is the same everywhere
Weight varies
5
Q
What is energy
A
The capacity to do work
6
Q
What types of energy are there
A
Potential and kinetic
7
Q
What is potential energy
A
Stored or inactive energy
8
Q
Kinetic energy
A
Energy of motion
9
Q
Forms of energy
A
Chemical energy
Electrical energy
Mechanical
Radiant
10
Q
Chemical energy
A
The making or breaking of chemical bonds
11
Q
Electrical energy
A
The movement of charged particles
12
Q
Mechanical energy
A
Movement of matter
13
Q
Radiant energy
A
Light or other electromagnetic radiation
14
Q
Synthesis
A
Synthesis is a type of reaction where you’re taking something small and putting it into a bigger complex molecule
So you use energy to build it
It’s an anabolic reaction
15
Q
Decomposition is what kind of reaction
A
Catabolic reaction, where you’re taking something big and breaking it down.
Energy is always released
16
Q
Chemical reactions are
A
The formation, rearrangement or breaking of bonds
17
Q
Types of chemical reactions
A
Synthesis
Decomposition
18
Q
A+B -> C
A
Chemical reaction
A+B are reactants
C is the product
19
Q
In decomposition is released energy always used for another purpose?
A
No
20
Q
Glycogen into glucose molecules is an example of
A
Decomposition
Catabolic reaction
21
Q
Amino acids join to form a protein molecule what is this
A
Synthesis
Anabolic reaction
22
Q
Bonds contain
A
Energy
23
Q
When you break bonds you
A
Release energy
24
Q
When you break molecules and give off energy what also is created in your body
A
Heat
25
What do a majority of the reactions in the body contain
Synthesis (Anabolic) and decomposition (catabolic) reactions
26
Chemical exchange reactions
When synthesis and decomposition occur in the same reaction
27
AB + CD AD + CB Shows?
An exchange reaction
| Breaking down by taking A and putting together
28
ATP + Glucose Glucose-6 phosphate + ADP is?
Example of an exchange reaction
| ATP transfers it phosphate to form glucose phosphate
29
Solvent
Medium in which things are mixed
30
Solute
Various other components in mix
31
Colloids
```
Heterogeneous mixtures that appear translucent or milky
Smaller particles
Clumps of similar molecules
Scatter light
Particles do not settle out
```
32
Jell-o and cell cytoplasm are
Colloids
33
Suspensions
Heterogeneous mixture with larger often visible particles
| Particles settle out due to gravity if particles aren't in motion
34
Blood (red blood cells suspended in plasma) are
Suspensions
35
Mineral water is an example of what mixture and why
Solution
| Particles are very tiny do not settle out or scatter light
36
Gelatin is an example of what type of mixture and why
Solute particles are larger than in a solution and scatter light, do not settle out
37
Blood is an example of what mixture and why?
Suspension
| Are very large, settle out and may scatter light
38
Concentration is what
Amount of solute particles
39
What are
Mg/dl
Molarity- miles/liters
Ways to solve concentration of a solute in a solvent
40
Mole
Total atomic weight of a molecule
41
Strongest to weakest bonds
Covalent
Ionic
Hydrogen
Van der walls= hydrophobic
42
What bond shares electrons
Covalent
43
How many bonds can a covalent bond have
Single, double or triple
44
What does the valent shell do
Determine the properties of bonding for an atom
45
Which bonds have an unequal sharing depending on weight
Covalent
46
Types of covalent bonds
Non polar and polar
47
If electrons are shared equally what type of covalent bond is it?
Nonpolar
48
O=C=O is
Non polar covalent bond sharing between carbon and oxygen
| CO2
49
No polls created
Non polar bond
50
What bond creates polls show
Polar bonds
51
H2O is what kind of bond
Polar covalent
| Looks like an upside Mickey Mouse
52
Ionic bonds happen when
Electrons are separated and transferred from one atom to another forming positive and negative ions
53
Types of ionic bonds
Cations
| Anions
54
Cations are
The electron donor
Have a positive charge
Positive because they loose a negative
55
Anions are
Electron acceptor
| Have a negative charge
56
Why do ionic bonds occur
Because one atom has an extra electron
57
Oppositely charged ions do what
Attract each other
58
Na+ Cl- is what
An ionic bond
| Table salt
59
The atom that takes an electron becomes _____ and the atom that gives an electron becomes____
Negative
| Positive
60
Bonds in order of stability
| Greatest to least
Nonpolar covalent bonds
Polar covalent bonds
Ionic bonds
61
Ionic bonds do what with electrons
Completely transfer electrons
62
Polar covalent bonds do what with electrons
Unequally share electrons
63
Nonpolar covalent bonds do what with electrons
Equally share electrons
64
Ionic bond charge
Charged particles
65
Polar covalent bonds charge
Slight negative on one end of molecule
| Slight positive charge on the other end
66
Nonpolar covalent bonds charge
Charged balanced
67
Hydrogen bonds are
Easier to break
| Have weak attractions between different molecules which contain polar covalent bonds
68
Water contains what kind of bond
Covalently bound hydrogen
69
What gives water its tension
Covalently bound hydrogen bonds
70
Synthesis
Building - anabolic
| Consuming energy
71
Decomposition
Catabolic breaking bonds
| Releases energy
72
OIL RIG
Oxidation is lost
| Reduction is gained
73
what happens when an atom looses an electron
Becomes unstable and wants to bond
74
Unstable atom is
Free radical
75
Antioxidants
Combine with unstable atoms in body
| Blueberry Pom
76
Reactant losing electrons and positive hydrogen ions
Are electron donor
Oxidized
Energy is released
Decreased potential energy
77
Reactant gaining electrons and positive hydrogen ions are
Electron acceptor
It's positive charge is Reduced
Energy is absorbed
Increased in potential energy
78
Energy flows is chemical reactions
Exergonic
| Endergonic
79
Exergonic reaction
Release energy
Energy may be usable
Releases waste heat-exothermic
80
endergonic reaction
require energy-endothermic
81
Products have more potential energy in bonds than reactants
Endergonic reaction
82
Products have less energy in their chemical bonds than the reactants
Exergonic reactions
83
All chemical reactions are...
Theoretically reversible
84
When is it more difficult to reverse a reaction
When energy is released during reaction
| Energy must be added back to reverse the reaction
85
All chemical reactions tend toward
An equilibrium/homeostasis
86
When chemical reactants are in equilibrium
the rates of forward and reverse reactions are equal
| The products and reactants are in balanced proportions
87
What causes a proportionate shift in other components of the reaction
Change in energy
| Change in concentrations of reactants or products
88
Factors influencing rate of reactions
Molecular collisions
| Probability of collisions
89
Molecular collisions are required
For chemical reactions to occur
90
The probability of collisions is affected by
Temp
Particle size
concentration
catalyst
91
How does temp affect molecular collisions
Changes in kinetic energy
| Hotter particles move faster
92
How does particle size affect collisions
Smaller particles move faster
| Bigger particles move slower
93
How does concentration affect probability molecular collisions
Collisions are more likely to occur when more molecules are present
More molecules more collisions
Higher concentration faster reaction
94
Catalyst influence the probability of collisions
Bring reactants together more rapidly or in more favorable orientations for reactions to take place or both
Speeds up reactions
95
10 pizzas vs 1 pizza
Higher Concentration
| Smell travels faster
96
Catalyst is only used in the body every single time as an _____ in our body
Enzyme
97
What is a catalyst/enzyme
Speeds up a reaction
| By lowering the energy required for it to work
98
Enzyme
Lowers activation energy speeding up reactions
99
ASE is?
An enzyme in the body
100
All chemical reactions tend towards what kind of state
Equilibrium state
101
Reversibility of chemical reactions refers to
All chemical reactions are theoretically reversible
| All chemical reactions tend toward an equilibrium state
102
Inorganic compounds
Gases
Water
Pretty much smaller
103
Organic compounds
Anything with carbon atoms
| Except gases
104
What carbon atoms are inorganic compounds
Carbon monoxide
Carbon dioxide
Carbides
105
What type of compounds are h2o
O2
CO2
N2
Inorganic
106
What type of compounds are various ion
Inorganic
107
Ion
Charged particles
108
What happens when a cation or anion dissolve in our blood and disassociate
Electrolyte
109
Sodium chloride is an
Electrolyte
110
Na and Cl
Sodium chloride
Separate in a solvent like blood what is formed
An electrolyte
111
Properties of water
```
High heat capacity
High heat of vaporization (212 degrees)
Polarity
Reactivity
Lubrication and cushioning
```
112
Why does water have a high heat capacity
Because it takes a lot of kinetic energy in it to change its temp
113
What does waters high heat capacity contribute to?
Temperature stability
114
Water has special properties why?
Due to its ability to form hydrogen bonds
115
How is sweating a similar transition to gas phase
Because it takes energy away from the body
116
The change from liquid to gas phase of water requires?
Breaking many hydrogen bonds
117
What is a polar covalent
Water h2o
| Mickey Mouse
118
Waters Polarity/solvent properties
Polar covalent bond
Water is a good solvent
Water brings solute molecules into close proximity making reactions more likely
119
What is considered a universal solvent and neutral
Water
120
Reactivity of water
A lot of chemical reactions take place in water
| It is added or removed from molecules in breakdown or synthesis reactions
121
Lubrication and cushions of water
Water is found in serous and mucous fluids in body to help lubricate parts
Found in cerebrospinal fluid
And amniotic fluid
122
What special property is amniotic fluid and example of the
Lubrication and cushioning of water
123
What are ions
Salt
124
Ions are called
Electrolytes
125
Contain cations and anions
NaCl
Ca2CO3
Examples of salts
| Ionic compounds
126
What dissociate (ionize) into component ions when dissolved in water
Salts
127
Electrolytes are
Anything with a charge particle
128
What are Na and Cl separately
Ions
129
Ph scale measures
How many hydrogen ions are in some type of solution
130
[ ] what does this label
Concentration on ph scale
131
acids and bases are
Compounds which break their ionic bonds when dissolved in h2o
132
To break an ionic bond/compound
water molecules must be able to stabilize the ions that result from breaking the ionic bond
133
Why do ionic bonds break when dissolved in water
Polar water attracts polar molecules and ions. It pushes out non polar non charged substances.
Positive poles of water are attracted to anions and negative poles to cations
So the water molecules pull the ions.
134
Acids do what when dissolved in waye h2o
Donate a hydrogen to the solution (H+ Donor)
Separate to release hydrogen ions (h+) and anions (negatively charged ion)
135
```
HCl hydrochloric
H2CO3 carbonic
H2SO4 sulfuric
H3PO4 phosphoric
Are examples of?
```
Acids
136
Bases do what in a solution
Accept protons
(h+ acceptor)
Separate into hydroxyl ion or more cations (positively charged ion)
137
Anions
Negatively charged ion
138
Cation
Positively charge ion
139
Dissociate
Molecules or ionic compounds separating or splitting into smaller particles such as
Ions
Radicals
Atoms
140
What is measured in ph units
Concentration of hydrogen ions
141
Ph ranges from
0-14
142
Nuetral ph is
7 [h+]=[oh-]
| Concentration of hydrogen ions equals concentration of hydroxide ions
143
1 ph unit charge equals how much of a change in [h+] hydrogen concentration
10x
144
Below ph7 solutions are
| Why?
Acidic
| Have more h+ ions
145
Above ph7 solutions are
| Why
Basic
| Have more OH- ions
146
Ph number
the higher?
The lower?
Higher more basic
| Lower more acidic
147
Ph scale is measuring
How many hydrogen ions are in a solution
148
14 on ph scale
Basic
149
0 on ph scale
Acid
150
Structure and function are
Complimentary
151
Our body has to maintain an acid and base balance at
| Why?
7.35-7.45 ph maintained
| Important for internal homeostasis
152
What in our body is very sensitive to ph
Biochemical reactions
153
Biochemical reactions
Transformation of one molecule to another inside a cell.
| Mediated by enzymes
154
What 3 homeostatic mechanism do humans use to regulate acid base balance
Buffers
Respiratory system
Renal system
155
Buffer
Example Blood in our body
Anything that resists changes in pH despite things dissolving in it
Blood because of water is resisting the changes in ph in our bodies
156
Respiratory system and renal maintain ph
Due to excretion of excess ions maintain our ph
157
Organic compounds always contain
Hydrogen
carbon
oxygen
158
Organic compounds sometimes contain
Sulfur
nitrogen
phosphorus
159
Carbon can form how many covalent bonds
4
160
Why does carbon form 4 covalent bonds
Because it has four in its valence shell and needs four more to complete its octet
161
Carbon atoms can form chains with
Other carbons
162
What do polar organic compounds dissolve well in?
| Why
In water
Water surrounds polar site of organic compound molecules
Striping the molecule set from the solute turning it into a solvent
The individual particles of the solute (coco) separate from their neighbors and move between the spaces of the solvent particles
163
Covalent bond is
A chemical bond that shares electrons between atoms
164
Organic compound
Any compound composed of atoms (always containing C,H,O, sometimes S,N,P) held together by covalent (shared electron) bonds
165
ATP
| Adenosine triphosphate is an example of
Transfers energy in a cell
| When the covalent bonds in the organic compound (atp) are broken down and released
166
Are organic molecules large or small
Large
167
What do organic molecules make
Good structural components
168
subunits of organic molecules
```
Simple molecules=
Monomers
Monomers join together to form macromolecules
Macromolecules=
Polymers
```
169
Monomers are made up of
Simple molecules
170
Polymers are a series of
Monomers
171
Monomers join together to make up
Macromolecules
172
Monomers is a
Molecule that is able to bond in long chains
173
Polymers means
Many monomers
174
Polymers are sometimes known as
Macromolecules or large sized molecules
175
```
Molecules
Monomers
Macromolecules
Polymers
Are
```
Organic compounds
176
Four classes of polymers
Lipids
Carbohydrates
Proteins
Nucleic acids
177
Carbohydrates
```
Anything that's a
Sugar
Starch
Glycogen
Cellulose
Chitin
```
178
Sugar (saccharide)
Monosaccharide- Simple sugars, Make up Disaccharide. Which make up poly saccharide
179
Starch
Long chains of these organic compounds.
| Vegetables
180
Glycogen
Stored form of glucose (carb)
181
When you have too much glucose it's stored as
Glycogen
182
Quaternary structure
Two or more proteins aggregated together
183
Secondary structure
Alpha helix and Beta pleated Sheets
184
Fatty acids with more than one double bond between carbon atoms
Polysaturated
185
Fatty acids with one double bind between carbon atoms
Monosaturated
186
Fatty acids with all single bonds between carbon atoms
Saturated
187
Sex hormones come from
Steroids
188
What regulates inflammation
Eicosanoids
189
Major components of cell membranes
Phosolipids
190
Used for energy storage and insulation
Triglycerides
191
Fatty acids with all single bonds between carbon atoms
Saturated
192
96 percent of body weight is made up of how many elements
Four elements
193
Reactions where you release energy
Exergonic
194
Prostaglandins
Proteins
195
Ph is a concentration unit used to measure the concentration of
Hydrogen ions in a solution
196
Molecular chaperones aid in the desired folding of
Proteins
197
the function of micro RNA is to
Turn some genes on and other off, controlling genetic expressions
Transfer genetic code to the ribosome for protein synthesis
198
```
Sugar contains all the following except
Calcium
Hydrogen
Carbon
Oxygen
```
Calcium
199
And organic compound that has twice as many hydrogen atoms as oxygen atoms is most likely a
Carbohydrates
200
A release of energy
Catabolic reactions
201
Buffers tend to prevent dramatic changes in Ph when what are added to a solution
Proton donors or proton acceptor
202
Exergonic
Chemical reactions that release energy
203
Nucleotides
Building blocks of rna and DNA
204
Adenine
Guanine
Cytosine
Thymine
DNA
205
Adenine
Guanine
Cytosine
Uracil
RNA
206
Important cholesterol based molecule
Steroids
207
Dipoles
Orient themselves towards other dipole molecules
Water
Not electrically balanced
Play essential roles in chemical reactions
208
What bonds are found in inorganic compounds
Ionic
209
Elements are unique substances that cannot be broken down into simpler substances by ordinary chemical means
True
210
Glucose is an example of
Monosaccharides
211
How isotopes differ from each other
By the number of neutrons contained
212
Lipids and energy
Good source of stored energy
| Perferred source of energy for fueling cellular activity
213
Oxygen is in proteins and fats
True
214
The lower the ph level the lower the hydrogen ion concentration
True
215
Metabolism
Term used to describe all chemical reactions involved in maintaining living state of cells and the organism
Catabolism
Anabolism
216
Molecule
Group of atoms
| Smallest fundamental unit of a chemical compound
217
Compounds
Two or more elements
218
Element
Is a substance consisting of atoms that all have the same atomic number
Chemically the simplest substances and cannot be broken down
219
Water as an inorganic compound
Does not contain carbon atom in its molecules making it inorganic
220
Carbon is the universal element of
Organic compounds
221
How many monosaccharides does it take to make a poly
10s to 100s
222
Triglycerides
storage for of fats for energy
Non polar
Hydrophobic
223
Glycerol head and 3 fatty acid side chains
Triglycerides
224
Solid at room temp and only one bond between those carbon chains
Saturated fat
Lard
Butter
225
Unsaturated fatty acids
Double bond
| More fluid at room temp
226
Phospholipids
Modified triglycerides
227
2 fatty acids and a phosphate group attached to glycerol
Phospholipids
228
Polar head non polar tail
Hydrophoilic head
Hydrophobic tail
Phospholipids
229
Has polar and non polar regions
Amphipathic
230
Dipole
A molecule in which a concentration of positive electric charge is separated from a concentration of negative charge
231
Buffer
Constantly resisting the changes in ph
232
Steroid hormones and prostaglandins are examples of what kind of important polymers
Lipids
233
Polymers
Organic compounds
234
```
Glucose
Fructose
Galactose
Deoxyribose
Ribose
```
Monosaccharides
| Simple sugar
235
Sucrose
Maltose
Lactose
disaccharide
236
Dehydration
Water molecule removed during bond
237
Add water molecule to liberate the monosaccharides
Hydrolysis
238
```
4 rings of carbon atoms
Non polar
Fat soluble
Hydrophobic
Cholesterol derived
```
Steroid
239
Prostaglandins
Leukotrienes
Regulate blood clotting, inflammation
Immune reaction, labor
Eicosanoids
| Local hormones
240
Contains
| C, H, O, N, S
Proteins
241
12-18% body mass
Proteins
242
Amino acids are building block of
Proteins
243
How many amino acids to build a protein
20
244
Cholesterol, prostaglandins and leukotrines are
Lipids
245
Proteins are to help with.
Structural
246
Proteins found in
Skeletal muscle
247
Amino acids bormallly end in
INE
248
Bond that holds together amino acids
Peptide
249
C,H,O
| WHAT compound
Organic compounds
250
Bond that comes together by dehydration synthesis
Peptide
251
What denatures proteins
Tempature
| PH
252
Ends in ASE most of the time
Enzymes
253
Apoenzyme
Globular proteins that are organic catalyst
254
Tertiary structure
Three dimensional structure resulting from folding
