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Chapter 2 BIO Powerpoint Flashcards

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Biology 101 flashcards
1
Q

All living and non living things are made of

A

Matter

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2
Q

Matter

A

Anything that occupies space and has mass

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3
Q

Types of matter

A

Liquid, solids and gas

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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

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5
Q

What is energy

A

The capacity to do work

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6
Q

What types of energy are there

A

Potential and kinetic

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7
Q

What is potential energy

A

Stored or inactive energy

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8
Q

Kinetic energy

A

Energy of motion

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9
Q

Forms of energy

A

Chemical energy
Electrical energy
Mechanical
Radiant

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10
Q

Chemical energy

A

The making or breaking of chemical bonds

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11
Q

Electrical energy

A

The movement of charged particles

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12
Q

Mechanical energy

A

Movement of matter

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13
Q

Radiant energy

A

Light or other electromagnetic radiation

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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

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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

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16
Q

Chemical reactions are

A

The formation, rearrangement or breaking of bonds

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17
Q

Types of chemical reactions

A

Synthesis

Decomposition

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18
Q

A+B -> C

A

Chemical reaction
A+B are reactants
C is the product

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19
Q

In decomposition is released energy always used for another purpose?

A

No

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20
Q

Glycogen into glucose molecules is an example of

A

Decomposition

Catabolic reaction

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21
Q

Amino acids join to form a protein molecule what is this

A

Synthesis

Anabolic reaction

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22
Q

Bonds contain

A

Energy

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23
Q

When you break bonds you

A

Release energy

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24
Q

When you break molecules and give off energy what also is created in your body

A

Heat

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25
Q

What do a majority of the reactions in the body contain

A

Synthesis (Anabolic) and decomposition (catabolic) reactions

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26
Q

Chemical exchange reactions

A

When synthesis and decomposition occur in the same reaction

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27
Q

AB + CD AD + CB Shows?

A

An exchange reaction

Breaking down by taking A and putting together

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28
Q

ATP + Glucose Glucose-6 phosphate + ADP is?

A

Example of an exchange reaction

ATP transfers it phosphate to form glucose phosphate

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29
Q

Solvent

A

Medium in which things are mixed

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30
Q

Solute

A

Various other components in mix

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31
Q

Colloids

A 
Heterogeneous mixtures that appear translucent or milky 
Smaller particles 
Clumps of similar molecules 
Scatter light 
Particles do not settle out
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32
Q

Jell-o and cell cytoplasm are

A

Colloids

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33
Q

Suspensions

A

Heterogeneous mixture with larger often visible particles

Particles settle out due to gravity if particles aren’t in motion

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34
Q

Blood (red blood cells suspended in plasma) are

A

Suspensions

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35
Q

Mineral water is an example of what mixture and why

A

Solution

Particles are very tiny do not settle out or scatter light

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36
Q

Gelatin is an example of what type of mixture and why

A

Solute particles are larger than in a solution and scatter light, do not settle out

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37
Q

Blood is an example of what mixture and why?

A

Suspension

Are very large, settle out and may scatter light

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38
Q

Concentration is what

A

Amount of solute particles

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39
Q

What are
Mg/dl
Molarity- miles/liters

A

Ways to solve concentration of a solute in a solvent

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40
Q

Mole

A

Total atomic weight of a molecule

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41
Q

Strongest to weakest bonds

A

Covalent
Ionic
Hydrogen
Van der walls= hydrophobic

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42
Q

What bond shares electrons

A

Covalent

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43
Q

How many bonds can a covalent bond have

A

Single, double or triple

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44
Q

What does the valent shell do

A

Determine the properties of bonding for an atom

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45
Q

Which bonds have an unequal sharing depending on weight

A

Covalent

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46
Q

Types of covalent bonds

A

Non polar and polar

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47
Q

If electrons are shared equally what type of covalent bond is it?

A

Nonpolar

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48
Q

O=C=O is

A

Non polar covalent bond sharing between carbon and oxygen

CO2

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49
Q

No polls created

A

Non polar bond

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50
Q

What bond creates polls show

A

Polar bonds

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51
Q

H2O is what kind of bond

A

Polar covalent

Looks like an upside Mickey Mouse

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52
Q

Ionic bonds happen when

A

Electrons are separated and transferred from one atom to another forming positive and negative ions

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53
Q

Types of ionic bonds

A

Cations

Anions

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54
Q

Cations are

A

The electron donor
Have a positive charge
Positive because they loose a negative

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55
Q

Anions are

A

Electron acceptor

Have a negative charge

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56
Q

Why do ionic bonds occur

A

Because one atom has an extra electron

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57
Q

Oppositely charged ions do what

A

Attract each other

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58
Q

Na+ Cl- is what

A

An ionic bond

Table salt

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59
Q

The atom that takes an electron becomes _____ and the atom that gives an electron becomes____

A

Negative

Positive

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60
Q

Bonds in order of stability

Greatest to least

A

Nonpolar covalent bonds
Polar covalent bonds
Ionic bonds

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61
Q

Ionic bonds do what with electrons

A

Completely transfer electrons

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62
Q

Polar covalent bonds do what with electrons

A

Unequally share electrons

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63
Q

Nonpolar covalent bonds do what with electrons

A

Equally share electrons

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64
Q

Ionic bond charge

A

Charged particles

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65
Q

Polar covalent bonds charge

A

Slight negative on one end of molecule

Slight positive charge on the other end

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66
Q

Nonpolar covalent bonds charge

A

Charged balanced

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67
Q

Hydrogen bonds are

A

Easier to break

Have weak attractions between different molecules which contain polar covalent bonds

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68
Q

Water contains what kind of bond

A

Covalently bound hydrogen

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69
Q

What gives water its tension

A

Covalently bound hydrogen bonds

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70
Q

Synthesis

A

Building - anabolic

Consuming energy

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71
Q

Decomposition

A

Catabolic breaking bonds

Releases energy

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72
Q

OIL RIG

A

Oxidation is lost

Reduction is gained

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73
Q

what happens when an atom looses an electron

A

Becomes unstable and wants to bond

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74
Q

Unstable atom is

A

Free radical

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75
Q

Antioxidants

A

Combine with unstable atoms in body

Blueberry Pom

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76
Q

Reactant losing electrons and positive hydrogen ions

A

Are electron donor
Oxidized
Energy is released
Decreased potential energy

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77
Q

Reactant gaining electrons and positive hydrogen ions are

A

Electron acceptor
It’s positive charge is Reduced
Energy is absorbed
Increased in potential energy

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78
Q

Energy flows is chemical reactions

A

Exergonic

Endergonic

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79
Q

Exergonic reaction

A

Release energy
Energy may be usable
Releases waste heat-exothermic

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80
Q

endergonic reaction

A

require energy-endothermic

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81
Q

Products have more potential energy in bonds than reactants

A

Endergonic reaction

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82
Q

Products have less energy in their chemical bonds than the reactants

A

Exergonic reactions

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83
Q

All chemical reactions are…

A

Theoretically reversible

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84
Q

When is it more difficult to reverse a reaction

A

When energy is released during reaction

Energy must be added back to reverse the reaction

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85
Q

All chemical reactions tend toward

A

An equilibrium/homeostasis

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86
Q

When chemical reactants are in equilibrium

A

the rates of forward and reverse reactions are equal

The products and reactants are in balanced proportions

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87
Q

What causes a proportionate shift in other components of the reaction

A

Change in energy

Change in concentrations of reactants or products

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88
Q

Factors influencing rate of reactions

A

Molecular collisions

Probability of collisions

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89
Q

Molecular collisions are required

A

For chemical reactions to occur

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90
Q

The probability of collisions is affected by

A

Temp
Particle size
concentration
catalyst

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91
Q

How does temp affect molecular collisions

A

Changes in kinetic energy

Hotter particles move faster

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92
Q

How does particle size affect collisions

A

Smaller particles move faster

Bigger particles move slower

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93
Q

How does concentration affect probability molecular collisions

A

Collisions are more likely to occur when more molecules are present

More molecules more collisions
Higher concentration faster reaction

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94
Q

Catalyst influence the probability of collisions

A

Bring reactants together more rapidly or in more favorable orientations for reactions to take place or both

Speeds up reactions

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95
Q

10 pizzas vs 1 pizza

A

Higher Concentration

Smell travels faster

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96
Q

Catalyst is only used in the body every single time as an _____ in our body

A

Enzyme

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97
Q

What is a catalyst/enzyme

A

Speeds up a reaction

By lowering the energy required for it to work

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98
Q

Enzyme

A

Lowers activation energy speeding up reactions

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99
Q

ASE is?

A

An enzyme in the body

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100
Q

All chemical reactions tend towards what kind of state

A

Equilibrium state

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101
Q

Reversibility of chemical reactions refers to

A

All chemical reactions are theoretically reversible

All chemical reactions tend toward an equilibrium state

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102
Q

Inorganic compounds

A

Gases
Water
Pretty much smaller

103
Q

Organic compounds

A

Anything with carbon atoms

Except gases

104
Q

What carbon atoms are inorganic compounds

A

Carbon monoxide
Carbon dioxide
Carbides

105
Q

What type of compounds are h2o
O2
CO2
N2

A

Inorganic

106
Q

What type of compounds are various ion

A

Inorganic

107
Q

Ion

A

Charged particles

108
Q

What happens when a cation or anion dissolve in our blood and disassociate

A

Electrolyte

109
Q

Sodium chloride is an

A

Electrolyte

110
Q

Na and Cl
Sodium chloride
Separate in a solvent like blood what is formed

A

An electrolyte

111
Q

Properties of water

A 
High heat capacity 
High heat of vaporization (212 degrees)
Polarity 
Reactivity 
Lubrication and cushioning
112
Q

Why does water have a high heat capacity

A

Because it takes a lot of kinetic energy in it to change its temp

113
Q

What does waters high heat capacity contribute to?

A

Temperature stability

114
Q

Water has special properties why?

A

Due to its ability to form hydrogen bonds

115
Q

How is sweating a similar transition to gas phase

A

Because it takes energy away from the body

116
Q

The change from liquid to gas phase of water requires?

A

Breaking many hydrogen bonds

117
Q

What is a polar covalent

A

Water h2o

Mickey Mouse

118
Q

Waters Polarity/solvent properties

A

Polar covalent bond
Water is a good solvent
Water brings solute molecules into close proximity making reactions more likely

119
Q

What is considered a universal solvent and neutral

A

Water

120
Q

Reactivity of water

A

A lot of chemical reactions take place in water

It is added or removed from molecules in breakdown or synthesis reactions

121
Q

Lubrication and cushions of water

A

Water is found in serous and mucous fluids in body to help lubricate parts
Found in cerebrospinal fluid
And amniotic fluid

122
Q

What special property is amniotic fluid and example of the

A

Lubrication and cushioning of water

123
Q

What are ions

A

Salt

124
Q

Ions are called

A

Electrolytes

125
Q

Contain cations and anions
NaCl
Ca2CO3

A

Examples of salts

Ionic compounds

126
Q

What dissociate (ionize) into component ions when dissolved in water

A

Salts

127
Q

Electrolytes are

A

Anything with a charge particle

128
Q

What are Na and Cl separately

A

Ions

129
Q

Ph scale measures

A

How many hydrogen ions are in some type of solution

130
Q

[ ] what does this label

A

Concentration on ph scale

131
Q

acids and bases are

A

Compounds which break their ionic bonds when dissolved in h2o

132
Q

To break an ionic bond/compound

A

water molecules must be able to stabilize the ions that result from breaking the ionic bond

133
Q

Why do ionic bonds break when dissolved in water

A

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
Q

Acids do what when dissolved in waye h2o

A

Donate a hydrogen to the solution (H+ Donor)

Separate to release hydrogen ions (h+) and anions (negatively charged ion)

135
Q 
HCl hydrochloric 
H2CO3 carbonic 
H2SO4 sulfuric 
H3PO4 phosphoric 
Are examples of?
A

Acids

136
Q

Bases do what in a solution

A

Accept protons
(h+ acceptor)
Separate into hydroxyl ion or more cations (positively charged ion)

137
Q

Anions

A

Negatively charged ion

138
Q

Cation

A

Positively charge ion

139
Q

Dissociate

A

Molecules or ionic compounds separating or splitting into smaller particles such as
Ions
Radicals
Atoms

140
Q

What is measured in ph units

A

Concentration of hydrogen ions

141
Q

Ph ranges from

A

0-14

142
Q

Nuetral ph is

A

7 [h+]=[oh-]

Concentration of hydrogen ions equals concentration of hydroxide ions

143
Q

1 ph unit charge equals how much of a change in [h+] hydrogen concentration

A

10x

144
Q

Below ph7 solutions are

Why?

A

Acidic

Have more h+ ions

145
Q

Above ph7 solutions are

Why

A

Basic

Have more OH- ions

146
Q

Ph number
the higher?
The lower?

A

Higher more basic

Lower more acidic

147
Q

Ph scale is measuring

A

How many hydrogen ions are in a solution

148
Q

14 on ph scale

A

Basic

149
Q

0 on ph scale

A

Acid

150
Q

Structure and function are

A

Complimentary

151
Q

Our body has to maintain an acid and base balance at

Why?

A

7.35-7.45 ph maintained

Important for internal homeostasis

152
Q

What in our body is very sensitive to ph

A

Biochemical reactions

153
Q

Biochemical reactions

A

Transformation of one molecule to another inside a cell.

Mediated by enzymes

154
Q

What 3 homeostatic mechanism do humans use to regulate acid base balance

A

Buffers
Respiratory system
Renal system

155
Q

Buffer

A

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
Q

Respiratory system and renal maintain ph

A

Due to excretion of excess ions maintain our ph

157
Q

Organic compounds always contain

A

Hydrogen
carbon
oxygen

158
Q

Organic compounds sometimes contain

A

Sulfur
nitrogen
phosphorus

159
Q

Carbon can form how many covalent bonds

A

4

160
Q

Why does carbon form 4 covalent bonds

A

Because it has four in its valence shell and needs four more to complete its octet

161
Q

Carbon atoms can form chains with

A

Other carbons

162
Q

What do polar organic compounds dissolve well in?

Why

A

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
Q

Covalent bond is

A

A chemical bond that shares electrons between atoms

164
Q

Organic compound

A

Any compound composed of atoms (always containing C,H,O, sometimes S,N,P) held together by covalent (shared electron) bonds

165
Q

ATP

Adenosine triphosphate is an example of

A

Transfers energy in a cell

When the covalent bonds in the organic compound (atp) are broken down and released

166
Q

Are organic molecules large or small

A

Large

167
Q

What do organic molecules make

A

Good structural components

168
Q

subunits of organic molecules

A 
Simple molecules=
Monomers 
Monomers join together to form macromolecules
Macromolecules= 
Polymers
169
Q

Monomers are made up of

A

Simple molecules

170
Q

Polymers are a series of

A

Monomers

171
Q

Monomers join together to make up

A

Macromolecules

172
Q

Monomers is a

A

Molecule that is able to bond in long chains

173
Q

Polymers means

A

Many monomers

174
Q

Polymers are sometimes known as

A

Macromolecules or large sized molecules

175
Q 
Molecules
Monomers
Macromolecules
Polymers 
Are
A

Organic compounds

176
Q

Four classes of polymers

A

Lipids
Carbohydrates
Proteins
Nucleic acids

177
Q

Carbohydrates

A 
Anything that's a 
Sugar
Starch 
Glycogen 
Cellulose 
Chitin
178
Q

Sugar (saccharide)

A

Monosaccharide- Simple sugars, Make up Disaccharide. Which make up poly saccharide

179
Q

Starch

A

Long chains of these organic compounds.

Vegetables

180
Q

Glycogen

A

Stored form of glucose (carb)

181
Q

When you have too much glucose it’s stored as

A

Glycogen

182
Q

Quaternary structure

A

Two or more proteins aggregated together

183
Q

Secondary structure

A

Alpha helix and Beta pleated Sheets

184
Q

Fatty acids with more than one double bond between carbon atoms

A

Polysaturated

185
Q

Fatty acids with one double bind between carbon atoms

A

Monosaturated

186
Q

Fatty acids with all single bonds between carbon atoms

A

Saturated

187
Q

Sex hormones come from

A

Steroids

188
Q

What regulates inflammation

A

Eicosanoids

189
Q

Major components of cell membranes

A

Phosolipids

190
Q

Used for energy storage and insulation

A

Triglycerides

191
Q

Fatty acids with all single bonds between carbon atoms

A

Saturated

192
Q

96 percent of body weight is made up of how many elements

A

Four elements

193
Q

Reactions where you release energy

A

Exergonic

194
Q

Prostaglandins

A

Proteins

195
Q

Ph is a concentration unit used to measure the concentration of

A

Hydrogen ions in a solution

196
Q

Molecular chaperones aid in the desired folding of

A

Proteins

197
Q

the function of micro RNA is to

A

Turn some genes on and other off, controlling genetic expressions

Transfer genetic code to the ribosome for protein synthesis

198
Q 
Sugar contains all the following except 
Calcium
Hydrogen
Carbon
Oxygen
A

Calcium

199
Q

And organic compound that has twice as many hydrogen atoms as oxygen atoms is most likely a

A

Carbohydrates

200
Q

A release of energy

A

Catabolic reactions

201
Q

Buffers tend to prevent dramatic changes in Ph when what are added to a solution

A

Proton donors or proton acceptor

202
Q

Exergonic

A

Chemical reactions that release energy

203
Q

Nucleotides

A

Building blocks of rna and DNA

204
Q

Adenine
Guanine
Cytosine
Thymine

A

DNA

205
Q

Adenine
Guanine
Cytosine
Uracil

A

RNA

206
Q

Important cholesterol based molecule

A

Steroids

207
Q

Dipoles

A

Orient themselves towards other dipole molecules
Water
Not electrically balanced
Play essential roles in chemical reactions

208
Q

What bonds are found in inorganic compounds

A

Ionic

209
Q

Elements are unique substances that cannot be broken down into simpler substances by ordinary chemical means

A

True

210
Q

Glucose is an example of

A

Monosaccharides

211
Q

How isotopes differ from each other

A

By the number of neutrons contained

212
Q

Lipids and energy

A

Good source of stored energy

Perferred source of energy for fueling cellular activity

213
Q

Oxygen is in proteins and fats

A

True

214
Q

The lower the ph level the lower the hydrogen ion concentration

A

True

215
Q

Metabolism

A

Term used to describe all chemical reactions involved in maintaining living state of cells and the organism

Catabolism
Anabolism

216
Q

Molecule

A

Group of atoms

Smallest fundamental unit of a chemical compound

217
Q

Compounds

A

Two or more elements

218
Q

Element

A

Is a substance consisting of atoms that all have the same atomic number
Chemically the simplest substances and cannot be broken down

219
Q

Water as an inorganic compound

A

Does not contain carbon atom in its molecules making it inorganic

220
Q

Carbon is the universal element of

A

Organic compounds

221
Q

How many monosaccharides does it take to make a poly

A

10s to 100s

222
Q

Triglycerides

A

storage for of fats for energy
Non polar
Hydrophobic

223
Q

Glycerol head and 3 fatty acid side chains

A

Triglycerides

224
Q

Solid at room temp and only one bond between those carbon chains

A

Saturated fat
Lard
Butter

225
Q

Unsaturated fatty acids

A

Double bond

More fluid at room temp

226
Q

Phospholipids

A

Modified triglycerides

227
Q

2 fatty acids and a phosphate group attached to glycerol

A

Phospholipids

228
Q

Polar head non polar tail
Hydrophoilic head
Hydrophobic tail

A

Phospholipids

229
Q

Has polar and non polar regions

A

Amphipathic

230
Q

Dipole

A

A molecule in which a concentration of positive electric charge is separated from a concentration of negative charge

231
Q

Buffer

A

Constantly resisting the changes in ph

232
Q

Steroid hormones and prostaglandins are examples of what kind of important polymers

A

Lipids

233
Q

Polymers

A

Organic compounds

234
Q 
Glucose
Fructose 
Galactose 
Deoxyribose 
Ribose
A

Monosaccharides

Simple sugar

235
Q

Sucrose
Maltose
Lactose

A

disaccharide

236
Q

Dehydration

A

Water molecule removed during bond

237
Q

Add water molecule to liberate the monosaccharides

A

Hydrolysis

238
Q 
4 rings of carbon atoms 
Non polar 
Fat soluble 
Hydrophobic 
Cholesterol derived
A

Steroid

239
Q

Prostaglandins
Leukotrienes
Regulate blood clotting, inflammation
Immune reaction, labor

A

Eicosanoids

Local hormones

240
Q

Contains

C, H, O, N, S

A

Proteins

241
Q

12-18% body mass

A

Proteins

242
Q

Amino acids are building block of

A

Proteins

243
Q

How many amino acids to build a protein

A

20

244
Q

Cholesterol, prostaglandins and leukotrines are

A

Lipids

245
Q

Proteins are to help with.

A

Structural

246
Q

Proteins found in

A

Skeletal muscle

247
Q

Amino acids bormallly end in

A

INE

248
Q

Bond that holds together amino acids

A

Peptide

249
Q

C,H,O

WHAT compound

A

Organic compounds

250
Q

Bond that comes together by dehydration synthesis

A

Peptide

251
Q

What denatures proteins

A

Tempature

PH

252
Q

Ends in ASE most of the time

A

Enzymes

253
Q

Apoenzyme

A

Globular proteins that are organic catalyst

254
Q

Tertiary structure

A

Three dimensional structure resulting from folding

Bio (22 decks)

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