Chapter 2 The Chemical Foundation Of Life Flashcards
(134 cards)
1
Q
What is life composed of
A
Matter
2
Q
What are unique forms of matter with specific chemical and physical properties
A
Elements
3
Q
Elements cannot be
A
Broken down into small substances, they require energy
4
Q
What is sulfur
A
Protein
5
Q
What is phosphorus
A
DNA structure
6
Q
What is the smallest unit of matter that retains all chemical properties of an element
A
Atom
7
Q
Atoms contain how many regions
A
Two
8
Q
What is the center of the atom and what does it contain
A
Nucleus, contains protons and neutrons
9
Q
What is the outmost region that orbits around the nucleus
A
Electrons
10
Q
What are protons neutrons and electrons referred to as and why
A
Subatomic particles because they are smaller than the atom
11
Q
Where is a proton and what is its mass and charge
A
Nucleus, +1 charge, 1 amu
12
Q
Where is a neutron and what is its mass and charge
A
Nucleus, 1 amu, 0 charge
13
Q
Where is a electron and what is its mass and charge
A
Orbitals outside the nucleus, 0 amu, -1 charge
14
Q
Professional baseball stadium is an example of
Baseball is an example of
A fly in the stadium is an example of
A
Atom
Nucleus
Electron
15
Q
What is the number of protons in an element
A
Atomic number
16
Q
What is the mass of the atom, equal to the number of protons + neutrons
A
Mass number
17
Q
What are elements with different number of neutrons
A
Isotopes
18
Q
What is also related to energy levels, symbol “n”
A
Distance
19
Q
The closer to the nucleus the _ energy
A
Less
20
Q
The further from the nucleus the __ energy
A
More
21
Q
What is the outer shell known as in electrons
A
Valence shell
22
Q
How do u know when the electron configuration is most stable
A
When the valence shell is full
23
Q
What rule does electrons have to follow
A
Octet rule
24
Q
Substances used at the beginning of a reaction (will undergo a chemical change)
A
Reactants
25
Substances formed at the end of a reaction
Products
26
The arrows will always be pointed toward
Products
27
Proceeds in one direction until all the reactants are used up
Irreversible reaction
28
Reactants are converted to products but some product can be converted back to reactant
Reversible reaction
29
How do atoms bond to form molecules
Chemical bonds
30
What is a chemical bond
The attractive force that links atoms together to form molecules
31
What are the 3 types of chemical bonds
Ionic
Covalent
Hydrogen
32
How many types of ionic bonds are there
One type of
33
How many types f covalent bonds are there
Single
Double
Or triple bonds
34
Do covalent bonds or ionic bonds categorize as polar and non-polar
Covalent
35
Some atoms lose electrons and others gain electrons to achieve an octet in what formation
Ionic compound
36
What type is a positively charged ion and what is an example
Sodium, cation
37
38
What type is a negatively charged ion and what is an example
Chloride, anion
39
When two hydrogens and an oxygen share pairs of electrons via ____ _____, a water molecule is formed
Covalent bond
40
The oxygen atoms in O2 molecule are joined by a ___ ____
Double bond
41
When its specified by number of bonds what is it always
Always covalent
42
Oxygen has higher ____ than oxygen
Electronegativity
43
In ___ ____ bonds, electrons are unequally shared by the atoms and attracted more to one nucleus than the other
Polar covalent
44
There are now ___ charges on the atoms in this bond due to unequal sharing of electrons
Partial charges (pole)
45
In ___ ____ bonds, electrons are equally shared by the atoms
Non- polar covalent bonds
46
In what type of polar bonds are there no charge
Non-polar
47
Carbon and hydrogen have similar ___ because they share electrons equally
Electronegativity because they have neutral charges
48
interaction BETWEEN the partial positive charged ion of hydrogen and the partial negative charge of a more electronegative atom on another molecule- often between water molecules
Hydrogen bonds
49
Between means
Hydrogen
50
Inside means
Covalent
51
WEAK attractions or interactions between two or more molecules in close proximity due to changes in electron density
Vander waals interactions (dipole-dipole)
52
Why is water essential to life
It is a polar molecule
Forms hydrogen bonds
53
The chemical bonds between hydrogen and oxygen in water are __ ___ bonds
Polar covalent
54
Why is oxygen more electronegative than hydrogen
Because it is getting pulled toward oxygen
55
Oxygen has a slightly ___ charge
Negative
56
Hydrogen has a slightly ___ change
Positive
57
Hydrogen of one water molecule forms a weak ___ ___ with the oxygen of an adjacent water molecule
Hydrogen bonds
58
Characteristics of hydrogen bonds
Hashed lines
Attractions due to polarity
H2O
59
Characteristics of covalent bonds
Straight line
60
Why do oil and water not mix
Oil is non-polar and water is a polar charge (negative on oxygen positive on hydrogen)
61
Is oil hydrophobic or hydrophilic
Hydrophobic aka water fearing
62
Is water hydrophobic or hydrophilic
Hydrophilic aka water loving
63
Hydrogen bonds are constantly made, broken and remade
Liquid
64
A crystalline structure is maintained by hydrogen bonds
Solid
65
Water is the solvent or solute
Solvent
66
Increased kinetic energy causes hydrogen bonds to break and molecules escape into air
Gas
66
Increased kinetic energy causes hydrogen bonds to break and molecules escape into air
Gas
67
Compounds dissolved or mixed in with water are solvents or solutes
Solutes
68
When table salt (NaCl) is mixed in water, __ ___ are formed around the ions
Hydrogen shells
68
What is a key component of macromolecules (proteins, carbohydrate, lipids, and nucleic acids)
Carbon (C)
69
Carbon-containing molecules are known as
Organic molecules
70
What does the covalent bonds serve as for macromolecules
Backbones, “skeleton”
71
Carbon + hydrogen = what
Hydrocarbons
72
Carbon forms single bonds with other atoms-shape is
Tetrahedral
73
When table salt (NaCl) is mixed in water, __ ___ are formed around the ions
Hydrogen shells
74
Two carbon atoms form a double bond- shape is ____, or flat
Planar
75
___ bonds, like those found in ethane, are able to rotate
Single
76
___ bonds, like those found in ethane cannot rotate, so the atoms on either side are locked in place
Double
77
____ is particularly important hydrocarbon ring- used in some amino acids, cholesterol and its derivatives
Benzene
78
What does beta-carotene do
Gives carrots their orange color
79
Molecules that have the same chemical formulae but differ in placement or arrangement of atoms or types of bonds between atoms
Isomers
80
Have a different covalent arrangements of atoms
Structural isomers
81
Have a different arrangement of atoms around a double bond
Geometric isomers
82
Molecules that share chemical formulae and bonds but differ in 3D placement of atoms
Mirror image
83
Carbondale are on opposite sides of double bonds
Trans
84
Carbons on the same side of double bond
Cis
85
Groups of atoms within a molecule that confer consistent specific properties to these molecules
Functional groups
86
Functional groups often interact with other functional groups via
Hydrogen bonds
87
Why is it important for biologists to understand the chemistry of life?
It is important for biologists to understand the chemistry of life because it helps you understand how diseases are created.
88
How do matter, elements, and atoms differ from one another?
Matter is anything that has mass and takes up space. Elements are unique forms of matter with specific chemical and physical properties (cannot be broken into smaller substances). Atoms are the smallest units of an element that retain its chemical properties.
89
What are the most common elements that make up living cells?
The most common elements in living cells are carbon (C), hydrogen (H), oxygen (O), nitrogen (N), phosphorus (P), and sulfur (S).
90
How are protons, neutrons, and electrons interrelated, and what are their properties and arrangement in atoms?
Protons (positively charged) and neutrons (neutral) are found in the nucleus of an atom. Electrons (negatively charged) orbit the nucleus. The number of protons defines the element, neutrons contribute to atomic mass, and electrons determine chemical reactivity.
91
What is the relationship between electron energy levels and their position in electron shells?
Electrons are arranged in energy levels or shells around the nucleus.
92
How do the chemical properties of an atom relate to valence electrons and electron distribution in orbitals?
The chemical properties of an atom are determined by its valence electrons (outermost electrons).
93
How do the distribution of electrons in orbitals affect atoms?
The way these electrons are distributed in orbitals affects how atoms interact and bond with other atoms.
94
What are reactants in a chemical reaction?
Reactants are substances used at the beginning of reactions that will undergo a chemical change.
95
What are products in a chemical reaction?
Products are substances formed at the end of the reaction. The arrow always points toward products, meaning yields (-> to make).
96
How can electrons be donated or shared between atoms?
Electrons can be transferred from one atom to another, forming ionic bonds, or shared between atoms, forming covalent bonds.
97
What are cations and anions?
Cations are positively charged ions, while anions are negatively charged ions.
98
What types of covalent bonds exist?
Covalent bonds can be polar (unequal sharing) or non-polar (equal sharing).
99
What is an ion?
An ion is an atom or molecule that has gained or lost one or more electrons, resulting in a positive (cation) or negative (anion) charge.
100
What are weak chemical interactions?
Weak chemical interactions include hydrogen bonds and van der Waals forces.
101
What are hydrogen bonds?
Hydrogen bonds are interactions between the partial positive charge of hydrogen and a partial negative charge of a more electronegative atom or molecule (often water).
102
What are van der Waals forces?
Van der Waals forces are weak attractions or interactions between two or more molecules in close proximity due to changes in electron density.
103
How does a molecule's polarity relate to electronegativity?
Polarity depends on the difference in electronegativity between atoms in a molecule, creating a polar molecule with partial positive and negative charges.
104
How does water form hydrogen bonds?
Water forms hydrogen bonds through the interaction between its partial positive hydrogen atoms and the partial negative charge of oxygen.
105
Why do water molecules form hydrogen bonds?
Water molecules form hydrogen bonds because oxygen is highly electronegative and attracts electrons more than hydrogen. This creates partial negative and positive charges, allowing water molecules to form weak bonds with each other.
106
Why is water an excellent solvent?
Water is an excellent solvent because it is polar, meaning it can dissolve many substances by surrounding charged or polar molecules and breaking them apart.
107
How can the solvent and solute in a solution be identified?
The solvent is the substance that dissolves another substance, while the solute is the substance being dissolved or mixed in the water.
108
How can an organic molecule be distinguished from a non-organic molecule?
Organic molecules contain carbon and are typically associated with proteins, carbohydrates, lipids, and nucleic acids. Non-organic molecules do not necessarily contain carbon and are found in non-living systems.
109
Why is carbon's chemistry unique?
Carbon is unique because it can form covalent bonds with up to four different atoms, each carbon has four electrons in the outer shell, it forms four covalent bonds to 'fill' the outer shell to achieve the octet rule.
110
What shapes can carbon-containing molecules have?
Carbon-containing molecules can have linear, branched, ring, tetrahedral, and planar structures.
111
How do different types of isomers differ from one another?
Isomers are molecules with the same chemical formula but different structures or placements. Structural isomers have different shapes, geometric isomers differ in spatial arrangement (cis, trans: pencil + pen example), and enantiomers are mirror images of each other.
112
What role do functional groups play in biological molecules?
Functional groups are groups of atoms within a molecule that confer consistent specific properties to these molecules.
113
How can functional groups be distinguished?
Functional groups differ in their atomic composition and properties.
114
What is the structure of a Hydroxyl group?
R-OH
115
What are the properties of a Hydroxyl group?
Polar
116
What is the structure of a Methyl group?
R-CH3
117
What are the properties of a Methyl group?
Nonpolar, more hydrophobic
118
What is the structure of a Carbonyl group?
R-C(=O)-R'
119
What is the structure of a Carboxyl group?
R-COOH
## Footnote
Carboxyl groups can release H+ ions into solution, making them acidic.
120
What is the structure of an Amino group?
R-NH2
## Footnote
Amino groups can remove H+ from solution, making them basic.
121
What is the structure of a Phosphate group?
R-PO4^2-
## Footnote
Phosphate groups can release H+ ions into solution, making them acidic.
122
What is the structure of a Sulfhydryl group?
R-SH
123
What is the charge of a Carboxyl group?
Charged, ionizes to release H+.
124
What is the charge of an Amino group?
Charged, accepts H+ to form NH3+.
125
What is the charge of a Phosphate group?
Charged, ionizes to release H+.
126
What is an atom?
The smallest thing in the world.
127
What are subatomic particles?
Protons, neutrons, and electrons.
128
What is an isotope?
A variant of a chemical element that has the same number of protons but a different number of neutrons.
129
What are chemical reactions?
The making or breaking of chemical bonds.
130
What is an anion?
A negatively charged ion, often ending in -IDE.
131
How to find electronegativity?
Refer to the periodic table for values.
132
What are isomers?
Different compounds with the same molecular formula.
