Chapter Two: Chemistry Flashcards
1
Q
Matter
A
Anything that occupies space and has mass
2
Q
States of Matter
A
Solid, Liquid, or Gas
3
Q
Energy
A
The capacity to do work or put matter into motion
4
Q
Two types of energy
A
Kinetic and Potential
5
Q
What is an atomic symbol
A
One of two letter chemical shorthand for each element
6
Q
What is the atomic number?
A
- Element’s defining trait
- Tells the number of protons and electrons
Top number above the atomic symbol
7
Q
Where is the atomic mass found?
A
Bottom number
8
Q
What is the formula to find number of neutrons?
A
Atomic mass - atomic number = neutrons
9
Q
What charge are protons?
A
Positive
10
Q
What charge are electrons?
A
Negative
11
Q
What is the formula to find number of nucleons?
A
Protons + Neutons
12
Q
What is the backbone of biological macromolecules?
A
Carbon
13
Q
What are physical elements?
A
Detectable with our senses
14
Q
What are chemical elements?
A
How atoms interact and bond with one another
15
Q
What 4 elements make up 96.1% of the body’s mass?
A
Hydrogen
Oxygen
Carbon
Nitrogen
16
Q
Which 9 elements make up 3.9% of body mass
A
Calcium
Phosphorus
Potassium
Sulfur
Chlorine
Magnesium
Iodine
Iron
17
Q
What are trace elements?
A
Very minute mounts of 11 elements that make up less than 0.01% of the body’s mass
18
Q
Chemical energy
A
Stored in bonds of chemical substances
19
Q
Electrical energy
A
Results from movement of charged particles
20
Q
Mechanical energy
A
Directly involved in moving matter
21
Q
Atoms
A
- Smallest stable unit of matter
- Unique building blocks for each element
- Give each element its physical & chemical properties
- Smallest particles of an element with properties of that element
22
Q
Atoms are composed of __ particles
A
subatomic particles
Protons, neutrons, and electrons
23
Q
Protons, neutrons, and electrons are
A
Subatomic particles
24
Q
Where are protons located?
A
In the nucleus
25
Where are neutrons located?
In the nucleus
26
Where are electrons located?
In orbit in an electron cloud
27
What is the charge and mass of protons?
- positive charge
- Mass = 1 amu
28
What is the charge and weight of a neutron?
- no charge
- Mass = 1 atomic mass unit (amu)
29
What is the charge and weight of an electron?
- Negative charge
- o amu
30
Number of __tons and __trons are always equal
Number of protons and electrons are always equal
31
Atomic number
- Number of protons in nucleus of the atom
Written as subscript to left of atomic symbol
32
Mass number
- Total number of protons and neutrons in nucleus of the atom
- Total mass of atom
- Written as superscript to left of atomic symbol
33
What are Isotopes?
- Structural variations of atoms
- Differ in the number of neutrons they contain
34
Atomic weight
Average of mass numbers (relative weights) of all isotopes of an atom
35
Radioisotopes
- Heavy isotopes decompose to more stable forms
- Similar to tiny explosion
- Can transform into different element
36
__ are energy relationships between electrons of reacting atoms
Chemical bonds
37
Electrons can occupy up to __ electron shells (energy levels) around nucleus
7
38
Valence shell
- outermost electron shell
- Electrons here have most potential energy and are chemically reactive electrons
39
Octet rule
Except for the first shell (full with two electrons) atoms interact to have eight electrons in their valence shell
| Rule of 8's
40
Chemically Inert Elements
- Stable and unreactive
- Valence shell fully occupied or contains eight electrons
- Noble gases
41
Chemically reactive elements
- Valence shell is not full
- Tend to gain, lose, or share electrons to achieve stability
42
Three major types of chemical bonds
Ionic
Covalent
Hydrogen
43
Ions
Atom gains or loses electrons and becomes charged
| When the number of Protons ≠ Number of Electrons
44
Anion
Atom that gained one or more electrons
45
Atom that gained one or more electrons
Anion
46
Cation
Atom that lost one or more electrons
47
Atom that lost one or more electrons
Cation
48
Attraction of opposite charges results in an __ bond
ionic
49
Covalent bonds
- Formed by sharing of two or more valence shell electrons
- Allows each atom to fill its valence shell at least part of the time
50
Nonpolar covalent bonds
- Electrons shared equally
- Produces electrically balanced, nonpolar molecules such as CO2
51
Small atoms with six or seven valence shell electrons are __
electronegative
52
Most atoms with one or two valence shell electrons are __
electropositive
53
Ionic bond
Complete transfer of electrons
54
Polar covalent bond
Unequal sharing
of electrons
55
Nonpolar covalent bond
Equal sharing of
electrons
56
Molecule
- Two or more atoms bonded together
57
Compound
Two or more different kinds of atoms bonded together
(Can only be seperated by breaking bonds)
| All are homogeneous
58
Mixture
Two or more components physically intermixed
(No chemical bonding between components - Can be separated by physical means, such as straining or filtering)
| Heterogeneous and homogeneous
59
Three types of mixtures
- Solutions
- Colloids
- Suspensions
60
Homogeneous mixtures
Solutions
61
Heterogeneous mixtures
Colloids
Suspensions
62
Solvent
- Substance present in great amount in a mixture
- usually water
63
Solute
smaller amounts in a mixture, dissolved in a solvent
64
Colloids
Emulsions
- large solute particples do not settle out
| ex: jello
65
Suspensions
Large visible solutes settle out
| EX: blood
66
Chemical reactions occur when
chemical bonds are formed, rearranged, or broken
67
Patterns of chemical reactions
- synthesis
- decomposition
- exchange
68
reactants
The number and kinds of the interacting substances
69
products
The chemical composition of the result of the reaction
70
The number and kinds of the interacting substances
Reactants
71
The chemical composition of the result of the reaction
Products
72
When atoms or molecules combine to form a larger, more complex molecule
Synthesis
73
a molecule is broken down into smaller molecules or its constituent atoms
Decomposition
74
What type of reaction includes both synthesis and decomposition?
Exchange/displacement
75
Bonds formed by sharing of two or more valence shell electrons
Covalent bonds
76
Acidosis
A condition of acidity or low pH (below 7.35) of the blood
- high hydrogen ion concentration
77
Alkalosis
- A condition of basicity or high pH (above 7.45) of the blood
- low hydrogen ion concentration.
78
Most ionic compounds are __
salts
79
Attraction of opposite charges results in an ___ bond
ionic
80
Atoms with one or two valence shell electrons are
electropositive
81
What is the difference between nonpolar and polar covalent bonds?
Nonpolar covalent bonds : electrons are shared equally, and balanced nonpolar molecules are produced
Polar covalent bond: unequal sharing of electrons - can be electronegative or electropositive
82
How can compounds be separated?
Only by breaking bonds
83
Stored in bonds of chemical substances
Chemical energy
84
Results from movement of charged particles
Electrical energy
85
Directly involved in moving matter
Mechanical energy
86
Elements
– Matter is composed of elements
– Elements cannot be broken into simpler
substances by ordinary chemical methods
87
Which property is detectable with our senses/measurable?
Physical
88
Which property relates to how atoms bond with one another?
Chemical
89
___ are energy relationships between electrons of reacting atoms
Chemical bonds
90
Electrons in valenceshell
- Have most ___ energy
– Are chemically __electrons
Potential energy
Chemically reactive
91
In terms of reactivity and stability, noble gases are ___ and ____
stable and unreactive
92
Chemically Reactive Elements tend to ___ with other atoms to achieve stability
gain, lose, or share electrons
93
Anion is what charge
Negative
94
Cation is what charge
positive
95
Attraction of opposite charges results in a(n) ___ bond
Ionic
96
Attractive force between electropositive hydrogen of one molecule and an electronegative atom of another molecule results in which bond?
Hydrogen bond
97
# Which reaction is this?
Atoms or molecules combine to form larger, more complex molecule
– Always involve bond formation
– Anabolic
Synthesis
98
In a synthesis reaction, __ particles are bonded together to form larger, more complex molecules
smaller
99
# Which reaction is this?
– Molecule is broken down into smaller
molecules or its constituent atoms * Reverse of synthesis reactions
– Involve breaking of bonds
– Catabolic
Decomposition
100
# What type of reaction is shown here?
AB → A + B
Decomposition
101
# What type of reaction is shown here?
A + B → AB
Synthesis
102
# Which reaction is this?
– Also called displacement reactions
– Involve both synthesis and decomposition – Bonds are both made and broken
Exchange
103
# What type of reaction is shown here?
AB + C → AC + B
Exchange
104
# Exergonic Reactions
net __ of energy
Release
105
# Exergonic reactions
Products have __ potential energy than reactants
less
106
# Endergonic reactions
net __ of energy
Absoption
107
All chemical reactions are theoretically __
reversible
108
Chemical equilibrium occurs if neither a forward nor reverse reaction is __
dominant
109
Why are most biological reactions essentially irreversible?
energy requirements and removal of products
110
Catalysts: ↑ Rate without being chemically ___ or part of product
changed
111
___ are biological catalysts
Enzymes
112
What affects the rate of chemical reactions?
Temperature
Concentration of reactant
Particle size
113
Biochemistry is defined as
Study of chemical composition and reactions of living matter
114
Water, salts, and many acids and bases are examples of which class of compound?
Inorganic
115
Carbohydrates, fats, proteins, and nucleic
acids are examples of which class of compound?
organic compounds
116
Which classification of compound contains carbon?
organic
117
What is the most important inorganic compound?
Water
118
What is the most abundant inorganic compound? What percent of volume does it make up in living cells?
Water, and it makes up 60-80% of the volume of living cells
119
Water has a __ heat capacity
and a __ heat of vaporization
high heat capacity and high heat of vaporization
120
Salts
Ionic compounds that dissociate into ions in water
121
Ions (electrolytes) conduct __ currents in solution
electrical
122
Acids and Bases
- __ are electrolytes
- Ionize and __ in water
- Both
- dissociate
123
Acids and Bases
- Both are __
- __ and dissociate in water
- electrolytes
- ionize
124
Acids are __ donors
proton
125
Acids are proton __
donors
126
Bases are __ acceptors
proton
127
Bases are proton __
acceptors
128
Acids release __ in solution
H+
129
Take up H+ from solution
Bases
130
Bases take up __ from solution
H+
131
As free [H+] increases, __ increases
acidity
132
As free [H+] decreases __ increases
alkalinity
133
# What type of solution is being described?
[H+], ↓ pH
An acidic solution
134
# What type of solution is being described?
[H+], ↑ pH
A basic solution
- Alkaline
135
Acidic pH values:
0–6.99
136
Alkaline pH values:
7.01–14
137
All neutral solutions are pH __
7
138
Results from mixing acids and bases
Neutralization
139
pH is regulated by ___
kidney, lungs, and chemical buffers
140
Biological macromolecules
Carbohydrates, lipids, proteins, and nucleic acids
141
Polymers are __
chains of **monomers** that are similar units
142
Which biological macromolecule is not a polymer?
lipids
143
Biological macromolecules are synthesized by __
dehydration synthesis
144
Biological macromolecules are __ by dehydration synthesis
synthesized
145
Biological macromolecules are broken down by __ reactions
hydrolysis
146
Hydrolysis
Water molecule breaks down one or more chemical bonds
Monomers are released by the addition of a water molecule, adding OH to one monomer and H to the other
147
Dehydration synthesis
Monomers are joined by removal of OH from one monomer and removal of H from the other at the site of bond formation
148
What are the three classes of carbohydrates?
Monosaccarides
Disaccharides
Polysaccharides
149
What are the functions of carbohydrates?
- Major source of cellular fuel
- Structural molecules
150
Simple sugars containing three to seven C atoms
Monosaccharides
151
Double sugars that are too large to pass through cell membranes
Disaccharides
152
Sucrose, maltose, and lactose are what type of saccharides?
Disaccharides
153
Long chains of linked monosaccharides
Polysaccharides
154
Starch and glycogen are what type of saccharides?
Polysaccharides
155
Are polysaccharides soluble?
Polysaccharides are not very soluble
156
What are the main types of lipids?
- Neutral fats or triglycerides
- Phospholipids
- Steroids
157
# solubility
Lipids are __ in water
Insoluble
158
Neutral Fats or Triglycerides are called __ when solid and __ when liquid
fats when solid, oil when liquid
159
Triglycerides are comprised of __
Three fatty acids bonded to a glycerol molecule
160
What are the main functions of triglycerides?
- energy storage
- insulation
- protection
161
Solid animal fats are __ fatty acids
saturated
162
olive oil is an example of a(n) __ fatty acid
unsaturated
163
Single covalent bonds between C atoms make up
saturated fatty acids
164
One or more double bonds between C atoms make up
unsaturated fatty acids
165
Phosholipids are important for __
cell membrane structure
166
What is the most important steroid?
Cholesterol
167
Important in cell membranes, vitamin D synthesis, steroid hormones, and bile salts
Cholesterol
168
Lipoproteins transport __ in the blood
fats
169
__ are the monomers in proteins
amino acids
170
What are the 4 sequences of protein structure?
1. **Primary structure:**
The sequence of amino acids forms the polypeptide chain.
2. **Secondary structure:**
The primary chain forms spirals (α-helices) and sheets (β-sheets).
3. **Tertiary structure:**
Superimposed on secondary structure. α-Helices and/or β-sheets are folded up to form a compact globular molecule held together by intramolecular bonds.
4. **Quaternary structure:**
Two or more polypeptide chains, each with its own tertiary structure, combine to form a functional protein.
171
keratin, elastin, and collagen are examples of what proteins?
Fibrous
172
Fibrous (structural) proteins provide __ support and __ strength
mechanical support and tensile strength
173
antibodies, hormones, molecular chaperones, and enzymes are examples of what proteins?
Globular (functional)
174
Proteins that are compact, spherical, water-soluble and sensitive to environmental changes
Globular
175
Proteins that are standlike, water-insoluble, and stable
Fibrous proteins
176
What can cause protein denaturation?
Decreased pH or increased temperature
177
When denaturization occurs, Globular proteins __
unfold and lose shape
178
Globular proteins that act as biological catalysts
Enzymes
179
what is the function of Catalysts
regulate and increase speed of chemical reactions
