Atoms, Molecules, pH, and Reactions Flashcards
1
Q
Atoms are composed of three types of particles.
A
- Neutron
- Proton
- Electron
2
Q
Type of bonds
A
- Ionic
- Covalent
- Hydrogen bonds
- van der Waals interactions
3
Q
Each type of particle has a different charge
A
- A proton has an electrical charge of +1
- An electron has an electrical charge of -1
- A neutron has no electrical charge associated with it.
4
Q
Two of the three particles have significant mass.
A
- A proton has a mass of 1 Atomic mass unit (AMU)
- A neutron has a mass of 1 AMU
- An election has negligible mass (zero for our purposes)
5
Q
Cation
A
Positively charged ion
6
Q
Anion
A
Negatively charged ion
7
Q
Ionic bond
A
Attraction between an anion and a cation
8
Q
Ionic Compounds, AKA Salts
A
Formed by ionic bonds
9
Q
Ionic bond
A
- No sharing of electrons
- Only stealing.
- When ions stick together
10
Q
Hydrogen Bond
A
A hydrogen atom covalently bonded to one electronegativity atom is also attracted to another electronegativity-charged atom
11
Q
Van der waals interaction
A
Attractions that occur between molecules in close proximity to each other
12
Q
Valence
A
An atoms bonding capacity
13
Q
Covalent bond
A
Sharing of pairs of electrons between two atoms.
14
Q
Single covalent bond
A
One pass of shared electrons between two atoms (one from each atom)
15
Q
Double covalent bond
A
Two pairs of shared electrons between two atoms,
16
Q
Triple covalent bond:
A
Three pairs of shared elections between two atoms
17
Q
Structural Formula
A
Atoms connected with actual bands
* ex: H-O-H
18
Q
Empirical formula
A
The lowest ratio of atoms of each element indicated
* ex: H₂O, C₂ H₂O₂ → CH₂O
19
Q
Molecular formula
A
The actual number of atoms of each element indicated
* Ex. H2O2
20
Q
The Structure of Water
A
The atoms form polar covalent bonds giving the water a consistent shape and essential properties.
21
Q
Water has the following properties important to life.
A
- As a solid, it is less dense than a liquid.
- It has high surface tension.
- It is cohesive and adhesive.
- It is a solvent.
22
Q
The pH of a solution
A
Measures the concentration of hydrogen & hydroxide ions in the solution.
23
Q
pH
A
A measurement of how acidic/basic a solution is.
24
Q
acidic
A
A solution with high hydrogen ions is acidic and has a low pH value.
25
Basic/Alkaline
A solution with a high number of hydroxide ions is basic and has a high pH value.
26
Buffers
* Solutions that moderate pH changes when an acid or base is added to the buffer system.
* Buffers are essential in biological systems because of their ability to maintain constant pH conditions.
27
Law of Conservation of Matter
* Atoms (matter) are neither gained nor lost in a chemical reaction, merely rearranged.
* The number of atoms of each element must be equal (balanced) on either side of the equation.
28
Carbohydrates
* A group of macromolecules that are a vital energy source for the cell provides structural support to many organisms.
* They can be found on the cell's surface as receptors or for cell recognition.
29
Carbohydrates are classified (depending on the number of monomers in the molecule):
* Monosaccharides
* Disaccharides
* Polysaccharides
30
Monosaccharides
* Monosaccharides are simple sugars, the most common of which is glucose.
* Glucose, galactose, and fructose are isomeric monosaccharides.
* They have the same chemical formula but slightly different structures.
31
Disaccharides
Disaccharides form when two monosaccharides undergo a dehydration reaction.
32
Dehydration reaction
During this process, the hydroxyl group (OH) of one monosaccharide combines with a hydrogen atom of another monosaccharide, releasing a molecule of water and forming a covalent bond between atoms in the two sugar molecules.
33
Polysaccharides
Although their structures and functions differ, all polysaccharide carbohydrates are made up of monosaccharides and have the chemical formula (CH₂O).
34
Starch
The stored form of sugars in plants and is made up of amylase and amylopectin (both polymers of glucose).
35
Glycogen
It is used as stored energy in animals.
36
Cellulose
A polysaccharide that provides support in plant cells (found in cell walls).
37
Lipids
* A class of macromolecules that are nonpolar and hydrophobic.
* They do not form true polymers
38
Lipids
Major types include:
* fats and oils
* waxes
* phospholipids
* steroids.
39
Fats and oils
* A stored form of energy and can include triglycerides.
* Fats and oils are usually made up of fatty acids and glycerol.
40
triglyceride
A fat molecule consisting of two main components:
1. glycerol
2. fatty acids.
41
Glycerol
An organic compound with:
* three carbon atoms
* five hydrogen atoms
* three hydroxyl (OH) groups.
42
Fatty acids
A long chain of hydrocarbons to which an acidic carboxyl group is attached, hence the name "fatty acid."
43
Unsaturated fats
* They are liquid at room temperature and are called oils.
* Plant & Fish fats
44
Saturated
* In a fatty acid chain, if there are only single bonds between neighboring carbons in the hydrocarbon chain
* Are solid at room temperature
* Example: Animal fats
45
Saturated fatty acids
* Are saturated with hydrogen
* tend to get packed tightly
* solid at room temp.
46
Phospholipids
* The major constituent of the plasma membrane.
* Instead of three fatty acids attached, there are two fatty acids, and the glycerol backbone's third carbon is bound to a phosphate group.
47
Fatty acids are hydrophobic.
Phosphates are hydrophilic.
48
Steroids
* The building blocks of many hormones and vitamins.
* Unlike phospholipids and fats, steroids have a ring structure.
* They are grouped with other lipids because they are also hydrophobic.
49
Proteins
* One of the most abundant organic molecules in living systems and have the most diverse functions of all macromolecules.
* They are a class of macromolecules that can perform a diverse range of functions for the cell.
* They help metabolism by providing structural support and acting as enzymes, carriers, or hormones.
* They may be structural, regulatory, contractile, or protective; they & may serve in transport storage or membranes, or they may be toxins of enzymes.
50
Amino acids
* The building blocks of protein.
* A central carbon bonded to an amino group (NH2), a carboxyl group (-COOH), and a hydrogen atom.
* The central carbon's fourth bond varies among the different amino acids, as seen in these examples of alanine, valine, lysine, and aspartic acid.
* Amino acids are bonded via peptide bonds to form a polypeptide/protein.
51
Protein
* Polymers of amino acids are arranged in a linear sequence.
* Every protein has a unique shape due to the sequence of amino acids.
* Protein shape is critical to its function.
52
Denaturation
Changes in temperature, pH, and exposure to chemicals may permanently change the protein's shape, leading to a loss of function.
53
Polypeptide
* Peptide bonds link a long chain of amino acids.
* A polymer of amino acids
54
Proteins are organized at four levels.
1. Primary
2. secondary
3. tertiary
4. quaternary.
55
Enzymes
* Are catalysts in biochemical reactions and usually proteins.
* Each one is specific for the substrate (a reactant that binds to an enzyme) upon which it acts.
* They can function to break molecular bonds, rearrange bands, or form new bands.
56
Induced-fit model
An adjustment to the lock-and-key model. It explains how enzymes and substrates undergo dynamic modifications during the transition state to increase the affinity of the substrate for the active site.
57
Allosteric inhibition
Indirectly induces a conformational change to the active site such that the substrate no longer fits.
58
Allosteric activation
The activator molecule modifies the shape of the active site to allow a better fit of the substrate.
59
Nucleic acids
* DNA & RNA
* Molecules consist of repeating units of nucleotides that direct cellular activities such as cell division and protein synthesis.
60
Nucleotides
Monomers that contain:
1. a monosaccharide
2. a phosphate group
3. a nitrogenous base.
61
A nucleotide is made up of three components.
1. A nitrogenous base
2. A pentrose sugar
3. A phosphate group.
62
ATP- Adenosine triphosphate
Particular nucleotides that are vital to life.
63
Peptide bond
Link amino acids together.
64
Chitin
A structural polysaccharide found in arthropod skeletons.
65
Hydrolysis
Disassemble polymers into monomers, a reaction that is the reverse of dehydration.
66
Four types of macromolecules
1. Carbohydrates
2. Lipids
3. Protein
4. Nucleic acid
67
Polar covalent bond
* One atom is more electronegative; the atoms do not share the electron equally.
* Unequal sharing of electrons causes a partial positive or negative charge for each atom or molecule.
* One atom draws electrons nearer b/c of size differences.
68
Nonpolar covalent bonds
Atoms share the electron equally.
69
Chemical bonding
* Elements have electron shells
* 2 in the 1st, 8 in the 2nd & 3rd
* If the shells are not full, elements will form bonds with other elements.
70
Isotopes
* Different forms of elements because of a loss of neutrons.
* Form at predictable rates & can be used in dating.
71
Elements
* Unique to themselves
* It cannot be turned into something else.
72
Molecule
Two or more atoms are held together by covalent bonds.
73
Bonding
* Elements with partially full valence shells satisfy the octet rule.
* Atoms with incomplete valence shells share or transfer electrons.
