Chapter One: Review Flashcards
(222 cards)
1
Q
Solvent
A
Is the substance that other substances (solute) are dissolved in. Usually a liquid, sometimes a gas.
2
Q
A liquid (the solvent) and its dissolved solutes.
A
Solution
3
Q
Solution has a higher solute concentration than the other solution. NET water moves towards this.
A
Hypertonic Solution
4
Q
Hypotonic solution
A
Solution has lower solute concentration than the other solution. NET water moves away
5
Q
Solutions have equal solute concentrations NO NET movement of water.
A
Isotonic solution
6
Q
Compound that dissociates into one or more hydrogen ions and one or more anions.
- donates H+ or produces H+
- HCl yields H+ + cl- ( in water)
A
Acid
7
Q
Molecule that binds with hydrogen ions when dissolved in water or produces OH- ions
- accepts H+ or produces OH-
A
Bases
8
Q
What is a logarithmic scale used for concentration of hydrogen ions in a solution.
A
pH scale
9
Q
pH value= 7
A
Neutral solution
10
Q
pH value greater than or equal to 7
A
Basic solutions
11
Q
pH value less than or equal to 7
A
Acid solutions
12
Q
Acidic solutions
A
Add H+ to the molecules
13
Q
Basic solutions
A
Take off H+ from the molecule
14
Q
Pure matter (substances) that cannot be separated into simpler matter (substances) by ordinary laboratory processes.
A
Elements
15
Q
Elements are the building blocks of ______ = anything that occupies space has mass.
A
Matter
16
Q
Represents the name of an element, consists of one to two letters and start with a capital letter.
A
Chemical Symbols
17
Q
C is ______ (element)
A
Carbon
18
Q
Nitrogen symbol is
A
N
19
Q
Fluorine symbol is
A
F
20
Q
Cobalts symbol is
A
Co
21
Q
Smallest unit of life
A
Atoms
22
Q
A substance that is dissolved in a liquid (solvent) to form a solution.
A
Solute
23
Q
Subatomic particle with a positive (+) charge
A
Proton
24
Q
Subatomic particle with a negative charge
A
Electron
25
Subatomic particle that is neutral
Neutron
26
Valence electrons
Electrons in the outer most shell
27
Outer most shells are stable when they are considered "_______" usually this is 8 electrons.
Full
28
Liters to measure ______________.
Volume
29
Grams to measure _____________.
Weight
30
Meters to measure ____________.
Length
31
L represents
Liters
32
g represents
Grams
33
m represents
Meters
34
milli is a prefix used to represent 1,000X _____________ than the base unit.
Smaller
35
There are how many 1,000mm in ___________m.
1
36
The average size of a bacteria is _____________. But the more practical way to say it is 1um
0.000001m (1 X 10^-6m)
37
Our cells are primarily made up of _______ and other different dissolved substances such as glucose, NaCl and O2
Water
38
Glucose is dissolved in water of the cell to form part of the the. In this example the glucose is an example of the __________ and the water is an example of the ___________.
Cytosol
Solute
Solvent
39
The most common solvent in a cell is.
Water
40
Not all solutes will dissolve in every solvent; solutes will only dissolve if they have __________ properties to the solvent.
Similar
41
Likes dissolve _________
Likes
42
Solutes dissolve in solvents that have similar ___________
Properties
43
Hydrophilic means __________ loving, solutes that will dissolve in hydrophilic solvents.
Water
44
Hydrophobic, water ___________; solutes will dissolve in hydrophobic solvents.
Hating
45
When there are more solutes on the outside of the cell then you have a ______________ solution. Water will want to leave the cell.
Hypertonic
46
When there are more solutes inside the cell than out of the cell you have a _________ solution. Water will want to move into the cell.
Hypotonic
47
When there are the same amount of solutes on the inside as there are on the outside is considered to be ___________. There is no net water movement.
Isotonic
48
The cell wall is an added layer of _______ and it can limit the amount of water that can be taken up.
Protection
49
Solutions and molecules can be (3)
Acidic
Neutral
Basic
50
Structure =
Function
51
Changing the pH can change the cells __________ and there for its function.
Shape
52
Acidic solution shave lots of _________ ions. The more acidic a solution is the more hydrogen ions there are in the solution.
Hydrogen
53
When a hydrogen ion is added to a molecule that is neutral it will add an overall ______ charge to the molecule; if the molecule already has a positive charge it will add to it causing it to have two positive _________ charges.
Positive
Positive
54
If the molecule has a negative charge then it will cause it to be ________ and so on.
Neutral
55
In a solution you have a smaller substance that is called the __________ that dissolves in a larger substance called the solvent.
Example: In our cells, water is our solvent and sugars,salts and proteins are the solutes that get dissolved in water.
Solute
56
The solute is the __________ substance (dissolves)
Smaller
57
The solvent is the ___________ substance
Larger
58
The property of the solute and solvent determines if the solute will _______. Solvents and solutes that are both hydrophilic or both hydrophobic are _________ likely to dissolve.
Dissolve
More
59
When you categorize the solution based on the number of solutes you have three possible types of solution. List and give an example of each.
Hypotonic solution: where there are more solutes in the cell.
Hypertonic solution: where there are more solutes on the outside of the cell.
Isotonic solution: where there are = number of solutes on the inside and outside of the cell.
60
You can describe the pH of a solution based on the number of H+ __________.
Ions
61
When there are a lot of H+ and the pHis less then 7 you have a _____________ solution and if you drop a molecule in the solution H ions are likely to _________ to your molecule. If you are lacking in H ions and your pH is over _________ you have an Alkaline solution, and if you drop a molecule in the solution H ions are likely to come off your molecule.
Acidic
Add
7
62
The periodic table organizes the ___________ based on a few properties such as ___________ and how many valance electrons they have.
Elements
Size
63
In human cells _______%of the cell is made up of C, H, O, and N.
________% of the cell is made up of Ca, P, K, S, Na, Cl, and Mg. Human cells also have a trace of other elements such as copper, zinc, iron, and iodine.
96%
4%
64
C represents what on the periodic table. 96%
Carbon
65
H represents what on the periodic table.96%
Hydrogen
66
Ca represents what on the periodic table.
Calcium
67
P represents what on the periodic table.
Phosphorus
68
K represents what on the periodic table.
Potassium
69
S represents what on the periodic table.
Sulfur
70
Na represents what on the periodic table.
Sodium
71
Cl represents what on the periodic table.
Chlorine
72
My represents what on the periodic table.
Magnesium
73
Cu represents what on the periodic table.
Copper
74
Zn represents what on the periodic table.
Zinc
75
Se represents what on the periodic table.
Selenium
76
I represents what on the periodic table.
Iodine
77
What does Mn represent on the periodic table.
Manganese
78
Co represents what on the Periodic table.
Cobalt
79
Fe represents what on the periodic table.
Iron
80
Mo represents what on the periodic table.
Molybdenum
81
F represents what on the periodic table.
Fluorine
82
Li represents what on the periodic table.
Lithium
83
Sr represents what on the periodic table.
Strontium
84
Al represent on the periodic table.
Aluminum
85
Si represents what on the periodic table.
Silicon
86
Pb represents what on the periodic table.
Lead
87
V represents what on the periodic table.
Vanadium
88
As represents what on the periodic table.
Arsenic
89
Br represents what on the periodic table.
Bromine
90
Cr represents what on the periodic table.
Chromium
91
Ag represents what on the periodic table.
Silver
92
Au represents what on the periodic table.
Gold
93
The proton which is a positive charge lives in the ____________ of the atom in the nucleus.
Center
94
The second subatomic particle is the _______ and it has a negative charge. The electrons orbit around the nucleus in orbital shells.
Electron
95
The third subatomic particle is called the __________ and lives in the center of the atom in the nucleus with the proton. Overall the electrons are on the outside roaring around the nuclear core.
Neutron
96
The smallest unit of matter/ molecule is mad up of 3 subatomic particles called _________,__________,_________.
Proton (+)
neutrons (neutral)
Electrons (-)
97
Electrons rotate around the ___________ of an atom. The more electrons an atom has the more _________ that these electrons will fill.
Nucleus
Shells
98
When atoms do not have ________electrons in their outermost electron shell they will try to achieve this by either gaming or losing electrons.
8
99
Oxygen has 6 electrons In its outer shell and has 2 unfilled spaces. Bc it requires less energy for oxygen to gain 2 electrons than to lose 6 it will ________.
Gain
100
Calcium on the other hand is more likely to lose ________electrons than gain 6.
2
101
Some elements are more likely to share electrons instead of Carbon has _______valance electrons and it's likely to share electrons instead of giving them up or gaining.
4
102
When atoms share electrons they will form ___________ bonds
Covalent
103
__________are the smallest unit of matter.
Atoms
104
Atoms are made up of 3 subatomic parts.
Neutrons
Protons
Electrons
105
If it takes up space its ___________.
Matter
106
Neutrons and protons are housed in the _______ of the atom and electrons rotate around the nucleus.
Middle
107
The electrons rotating farthest from the nucleus are called ___________ electrons.
Valance
108
____________ bond = an interaction between atoms in which electrons are either shared or transferred in such ways as to fill their valance shells.
Chemical
109
What are the 5 types of chemical bonds.
Covalent bonds
Ionic bonds
Hydrogen bonds
Hydrophobic interactions
Hydrophilic interactions
110
_____________ bonds are a stable bond.
Covalent
111
Covalent bonds are very important to producing _______ we find in our cells such as nucleic acids, proteins, carbohydrates, and lipids.
Macromolecules
112
A nucleic acid is an example of a macromolecule that is in charge of storing and transferring our cells information are made up of units called __________.
Nucleotides
113
The abbreviation for adenine triphosphate is.
ATP
114
The abbreviation for guanine triphosphate is.
GTP
115
What is the abbreviation for cytosine triphosphate.
CTP
116
Nucleotides are linked by what type of bonds?
Covalent
117
__________ is the sharing of of a pair of the electrons by two atoms.
Covalent
118
Atoms are important in nucleic acids, proteins, carbohydrates, and lipids which are all found in _____________molecules
Macro
119
Covalent bonds are stable. True or False
True
120
Some covalent bonds that we will become familiar with are.
C and H
C and O
C and N
C and P
O and O
O and H
H and H
121
Compounds that have carbon and __________ in them are called organic compounds.
Hydrogen
122
Which of the following compounds is not an organic compound.
Glucose C6H12O6
Table salt NaCl
Water H20
NaCl table salt
123
What is the most common molecule found in cells? The make up lipids including phospholipids and triglycerides.
Hydrocarbons
124
Hydrocarbons can have multiple _________ in the molecules. Hydrocarbons can also be attached to other atoms such as nitrogen and oxygen.
Carbons
125
Hydrocarbons can be in a ___________ line, __________ or in a ring.
Straight line
Branched
126
Hydrocarbons can also form more than just a single ___________. Carbons can also form double bonds or even triple bonds. When carbons have as many H as they can possible hold there are considered to be _____________.
Bond
Saturated
127
When there are double or triple bonds the carbons do not have their maximum number of hydrogens and they are considered to be ______________
Unsaturated
128
Carbon has ________ unpaired outer electrons.
4
129
The simplest hydrocarbon is ___________ (methane)
CH4
130
More complexed hydrocarbons involve _________or more carbon atoms.
2
131
Hydrocarbons can be linear or ___________
Branched
132
When talking about hydrocarbons what 3 types of bonds can be formed.
Single
Double
Triple
133
Not all covalent bonds are treated ____________
Equally
134
There are two types of covalent bonds what are they?
Polar covalent bonds and nonpolar covalent bonds
135
Some atoms are greedy and want there fronts more than the others. Theses atoms will NOT share their electrons ________ and will make _________ covalent bonds.
Equally
Polar
136
When two atoms want to the electrons similarity they will ________ their electrons equally and thy will form a nonpolar covalent bond.
Share
137
A non polar covalent bond is when oxygen and _________ share electrons.
Hydrogen
138
_________ is the attraction of an atoms nucleus has for its electrons.
Electronegativity
139
The greater the electronegativity, the _________ the pull the atom has for its electrons.
Higher
140
The electronegativity is determined by one of the other subatomic particles that the atom has called the __________.
Proton
141
When an atom has a larger electronegativity than the other it will want to the electrons in a covalent bond to send more time around it and will make the sharing of the electrons _________ and produce the polar covalent bond.
Unequal
142
What are the common non polar covalent bonds that I need to know this semester. For example one common non polar covalent bond would be C and H.
C and H
C and C
H and H
O and O
143
C-O, C-N, N-H, and P-O are all examples of ________ covalent bonds found in a cell.
Polar
144
An example of a compound with polar covalent bonds is ________. Water has 2 polar covalent bonds, since O is more electronegative than hydrogen, and when the electrons are more attracted to it the oxygen will acquire a partial positive charge.
Water
145
The greater the pull on atoms nucleus exerts on its electrons the _______ an atoms electronegativity is.
Higher
146
The more protons present in an atoms nucleus the more pull it has on the electrons. True or False
True
147
________ polar covalent bonds = type of chemical bond in which there is = sharing of electrons between atoms with ______ electronegativity
Non polar covalent bonds
Similar
148
_______ covalent bonds is the type of bond in which there is an = sharing of electrons between atoms with ________ electronegativities
Polar covalent
Different
149
A chemical bond involves the _______ or transferring of ________.
Sharing
Electrons
150
For an atom to gain or lose an electron they must undergo a reaction called ______ or oxidation. Whether or not the atom will give up or gain electrons depends on the electronegativity __________.
Reduction
Difference
151
If the difference in electronegativity is larger than 1.8 the atoms will undergo a transfer of electrons and the amount of the valance electrons will determine if the atom will lose electrons or gain electrons to make their valance shell happy. True or False
True
152
If the electronegativity difference is large enough and there are _____ electrons or less the atom usually loses its electrons and undergoes an oxidation _________
3
Reaction
153
If the electronegativity is difference is large enough and there are ______ or more electrons than atom will gain electrons and undergo a reduction _______
5
Reaction
154
When a atom loses an electron it will acquire a _______ charge for as many electrons as it loses.
Where's if the atom gains electrons it will acquire a ________ charge for every electron it gains.
The two ways to Remember these is.
LEO the lion goes GER
Lose of Electrons Oxidation, Gain of Electron Reduction.
OIL RIG
O for oxidation is loss and R is for reduction is gain
If one atom undergoes an oxidation reaction another atom had to undergo a ___________reaction.
Positive
Negative
Reduction
155
Not all molecules change their charge during oxidation and reduction reactions and therefore are tricky to identify as oxidation reduction reactions. True or false
True
156
During ___________ reactions the number of oxygen and carbon bonds increases or the number of hydrogen carbon bonds decreases.
Oxidation
157
During ___________ reactions the number of oxygen carbon bonds decrease and the number of carbon hydrogen bonds increase.
Reduction
158
_________ bond occurs when two atoms have opposite formal charges. They will make another chemical bond called an ionic bond.
Ionic
159
An ionic bond is the ____ attraction between ions of opposite charges.
A positively charged ion is called a _________
A negatively charged ion is called a _________
Electrical
Cation
Anion
160
How can ionic bonds be broken?
Put a molecule into a acidic solution H+ ions can add to molecules. If the molecule is placed in an alkaline solution H+ can be ______
Change in pH
Removed
161
In our cells ionic bonds are important in ________ production and nucleic acid and protein interactions.
Protein
162
________ bond is the electrical attraction between a partially positive charged hydrogen atom and a partially negatively charged O or N atom
Hydrogen bond
163
What are the requirements for hydrogen bonding?
H donor has to be attached to an N or an O
H acceptor typically is O dabble bonded to C, NH2 or OH
SO IN OTHER WORDS YOU NEED AN HYDROGEON ACCEPTOR AND DONNOR
164
Hydrogen bonds are broken how?
Increased heat and pH
A small increase in temperature can also break the bond
165
Hydrogen bonds are symbolized by.
A dotted line
166
Hydrogen bonds are important in building macromolecules in the cell. Hydrogen bonds also help protein and nucleic acids form their over all 3D shape. True or False.
True
167
Like ionic bonds hydrogen bonds can be broke by a change in _______
pH
168
If the molecules in a hydrogen bond move to fast because of the added temperature they will not stay aligned and the bonds will break.
What is an example of how our bodies use the above statement.
This is one way that our human bodies fight infections, by raising our temperature to break the hydrogen bonds.
169
Hydrophilic interactions and hydrophobic interactions are a type of bonding. True or false
True
170
Polar molecules are those with molecules with polar covalent bonds are water ____________, meaning they are attracted to water. Polar molecules will also participate in hydrophilic interactions.
Loving
171
Nonpolar molecules, those with molecules that are nonpolar covalent bonds are water _________,meaning they are not attracted to water. Nonpolar molecules will participate in hydrophobic interactions.
Hating
172
It is important to differentiate between talking about a property of a molecule that is hydrophilic and when talking about a bond.
If you are talking about a bond you must state the word _____________ after saying hydrophilic or hydrophobic.
For example: when you say hydrophilic if you mean the property of the molecule and you would say hydrophobic interactions of you were talking about the interaction between the two molecules
Interactions
173
We have molecules in cells that on one side will have nonpolar bonds and be hydrophobic and on the other side will have polar bonds and be hydrophilic.
An example of this is a cellular-relevant molecule type are the phospholipids. These have both a hydrophobic side and a hydrophilic side to them. So in other words they can do both hydrophobic __________ along with hydrophilic ________________
Interactions
Interactions
174
What are the 5 types of bonding?
Hydrogen bonding
Ionic bonding
Covalent bonding (polar and non-polar)
Hydrophobic interactions
Hydrophilic interactions
175
When electrons are shared you have a ___________ bond.
Covalent
176
There are two types of covalent bonding what are they?
Polar covalent bonds
Non-polar covalent bonds
177
When an atom has a formal charge it has an __________ to the opposite formal charge and can form an ionic bond.
Attraction
178
Hydrophobic interactions between hydrophobic molecules and have ____________interactions between ____________ molecules.
Hydrophilic
Hydrophilic
179
Functional groups:
Alcohol / hydroxyl
-OH
180
functional group:
___________ is the carbon of the carbonyl group (C double bonded to O) is attached to 2 carbon atoms.
Ketone
181
__________ acids contain the carboxyl group which is attached to the hydroxyl group.
Carboxylic
182
Groups make up ____________ groups
Functional
183
_____________ groups are reactive parts of larger molecules.
Functional
184
Functional groups can be just as small as a ______________ group.
Hydroxyl
185
Functional groups are more reactive therefore they are at the center of how and why molecules interact together. True or False?
True
186
Functional groups that contain oxygen in them.
When oxygen is covalently bonded to a carbon to make a C-O bond or to make a H-O bond they create a _____________ covalent bond.
Oxygen is more electronegative than either the C or H so it gets a partial negative charge and the H or C get a partial positive charge.
The uneven sharing of the electrons create a more__________ environment and thus creates the functional group.
Polar
Reactive
187
Functional group:
An alcohol/ hydroxyl group is an _________ group
OH
188
Functional group:
Ketone is a _________bonded carbon in a row with the middle carbon being dibble bonded to an oxygen.
3
189
Functional group:
A carboxylic is a ____________ group attached to a carbonyl group.
Carboxylic acids are ________.
The hydroxyl group can have a hydrogen or it can lose its hydrogen and gain a negative charge.
Hydroxyl
Ionizable
190
Some of the oxygen containing functional groups can participate in ___________ bonding.
Remember you need a hydrogen donor that includes a hydrogen covalently attached to O or N and a H acceptor which includes the N or the O covalently bonded to a H or the O that is covalently bonded to the C.
Hydrogen
191
Functional group:
_____________are the three atoms in a row, a C , O and then another C
This group must be in this order all the time C, O, C. hint community of Christ
Hint: a person that works in the commons is named this.
Esters
192
Esters are another example of a complex functional group. The combination of a carboxyl group with an _________. You must have the basic ether to make an ester but one of the carbons on either side of the ________ is a carboxyl carbon meaning it has a _________ bonded oxygen.
Ether
Oxygen
Double
193
The phosphoester is a _________ on the ester. With the phosphoester you have a ________ instead of a carbon in the carbonyl carbon.
Spin
P
194
Functional group:
Phosphate has a ______________ atom surrounded by oxygens. Three of the ___________have just 1 single bond to the oxygen, whereas the last one makes a dubbed bond to the phosphorus atom.
All of the single bonded oxygens are ionizable and can have a H or have lost their H and have a negative charge.
Phosphorus
Oxygens
195
Functional group:
The first N-containing functional group is the amine.
The amine is a nitrogen that makes _________ bonds to 3 different atoms where at least on of the atoms is a carbon.
3
196
There are three types of amines what are they? Hint 1,2,3
Primary amine- has 1 carbon attached to it
Secondary amine- has 2 carbons attached to it
Tertiary amine- has 3 carbons attached to it
197
If the nitrogen is not bonded to another atom it will bond to __________ to fulfill its octet.
For example the primary amine the N has bonded to one C and two H, but the secondary amine the N is attached to two carbons and one hydrogen.
Hydrogens
198
Both amines and amides are _______________. The N can gain another H. When the N has four covalent bonds to it, it will also have a positive charge.
Ionizable
199
Functional group:
The amide is a nitrogen containing functional group. The amide is an _________ but one of the carbons has a ___________ group. Just like the amines, amide has primary secondary and tertiary amides. They are named based on the number of ____________ carbons bonded to the nitrogen.
Amine
Carbonyl
Carbons
200
Functional group:
Sulfhdryl group is also known as the _______group. This group is a sulfur attached to a hydrogen.
Thiol
201
What are the 3 functional groups that we will see in cell biology.
Oxygen containing
Nitrogen containing
Sulfur containing
202
Amines and amides there are 3 types primary secondary and tertiary based on the number of _____________ bonded to the nitrogen. Again Nitrogen wants to make __________ covalent bonds and those bonds are carbons or hydrogens.
Carbon
3
203
What is the difference between the amine and the amide.
Amide is the one with the carbons bonded to the nitrogen makes a double bond to a oxygen
204
Sulfur containing functional groups include the sulfhdryl group which is an
S-H
205
Oxygen containing functional groups include
```
Alcohol / hydroxyl
Carbonyl
Ketone
Carboxyilic acid
Ether
Ester
Phosphoester
Phosphate
```
206
Nitrogen containing functional groups include (2)
Amine
| Amide
207
Sulfur containing functional groups
Sulfhydryl / thiol
208
Ketone has 3 _________ with carbonyl group
Carbons
209
Phosphate which has ______single bonded 1 double bonded oxygen
3
210
__________ is the making or breaking of a chemical bond.
Chemical reaction
211
Chemical reactions allow for _________ each other meaning it allows cells to convert food to energy and nutrients of the consumer.
Eating
212
There are two vocabulary words to describe the components of a chemical reaction _________ and ________.
Example: the reactants are the propane and oxygen gas whereas the products are carbon dioxide, water and energy.
Reactants
Products
213
________ the atoms, ions, or molecules that remain after the chemical reaction is complete
Products
214
________ the atoms, ions, or molecules that exists at the beginning of the chemical reaction.
Reactants
215
One common building reaction is called the _________ reaction also known as the dehydration reaction.
A dehydration reaction uses energy to take two smaller ________ and covalently bond them together during the process of water is produced.
Condensation
Molecules
216
During the condensation reaction a new functional group is produced. What was just produced.
Ether along with water
217
Condensation reaction aka dehydration reactions is a type of synthesis reaction in which 2 smaller molecules are joined together by a _________bond and a water molecule is released.
Loss of water
Covalently bonded monomers or small molecules to make large molecules
Requires energy
Covalent
218
The opposite of building reaction is a breakdown reaction aka hydrolysis decomposition reaction in which a covalent bond is __________ and the ionic components of water are added to the products.
Requires water
Produces monomers or smaller molecules
Makes energy
Broken
219
When water is added to the molecule, an OH from water is added to the first unit and the _______ is added to the ethers oxygen on the second subunit.
H
220
What are the two parts of a chemical reaction?
Reactant molecules present before the reaction
Product that are present after the chemical reaction
221
condensation reactions use energy to make covalent bonds and water. True or false
True
222
Do hydrolysis reactions use water to break up molecules and create energy. True or false
True
