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Biology > Atoms, Molecules, pH, and Reactions > Flashcards

Atoms, Molecules, pH, and Reactions Flashcards

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AP® Biology flashcards Biology 101 flashcards
1
Q

Atoms are composed of three types of particles.

A
  1. Neutron
  2. Proton
  3. Electron
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2
Q

Type of bonds

A
  1. Ionic
  2. Covalent
  3. Hydrogen bonds
  4. van der Waals interactions
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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.
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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)
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5
Q

Cation

A

Positively charged ion

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6
Q

Anion

A

Negatively charged ion

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7
Q

Ionic bond

A

Attraction between an anion and a cation

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8
Q

Ionic Compounds, AKA Salts

A

Formed by ionic bonds

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9
Q

Ionic bond

A
  • No sharing of electrons
  • Only stealing.
  • When ions stick together
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10
Q

Hydrogen Bond

A

A hydrogen atom covalently bonded to one electronegativity atom is also attracted to another electronegativity-charged atom

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11
Q

Van der waals interaction

A

Attractions that occur between molecules in close proximity to each other

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12
Q

Valence

A

An atoms bonding capacity

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13
Q

Covalent bond

A

Sharing of pairs of electrons between two atoms.

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14
Q

Single covalent bond

A

One pass of shared electrons between two atoms (one from each atom)

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15
Q

Double covalent bond

A

Two pairs of shared electrons between two atoms,

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16
Q

Triple covalent bond:

A

Three pairs of shared elections between two atoms

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17
Q

Structural Formula

A

Atoms connected with actual bands
* ex: H-O-H

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18
Q

Empirical formula

A

The lowest ratio of atoms of each element indicated
* ex: H₂O, C₂ H₂O₂ → CH₂O

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19
Q

Molecular formula

A

The actual number of atoms of each element indicated
* Ex. H2O2

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20
Q

The Structure of Water

A

The atoms form polar covalent bonds giving the water a consistent shape and essential properties.

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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.
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22
Q

The pH of a solution

A

Measures the concentration of hydrogen & hydroxide ions in the solution.

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23
Q

pH

A

A measurement of how acidic/basic a solution is.

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24
Q

acidic

A

A solution with high hydrogen ions is acidic and has a low pH value.

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25
Q

Basic/Alkaline

A

A solution with a high number of hydroxide ions is basic and has a high pH value.

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26
Q

Buffers

A
  • 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.
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27
Q

Law of Conservation of Matter

A
  • 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.
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28
Q

Carbohydrates

A
  • 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.
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29
Q

Carbohydrates are classified (depending on the number of monomers in the molecule):

A
  • Monosaccharides
  • Disaccharides
  • Polysaccharides
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30
Q

Monosaccharides

A
  • 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
Q

Disaccharides

A

Disaccharides form when two monosaccharides undergo a dehydration reaction.

32
Q

Dehydration reaction

A

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
Q

Polysaccharides

A

Although their structures and functions differ, all polysaccharide carbohydrates are made up of monosaccharides and have the chemical formula (CH₂O).

34
Q

Starch

A

The stored form of sugars in plants and is made up of amylase and amylopectin (both polymers of glucose).

35
Q

Glycogen

A

It is used as stored energy in animals.

36
Q

Cellulose

A

A polysaccharide that provides support in plant cells (found in cell walls).

37
Q

Lipids

A
  • A class of macromolecules that are nonpolar and hydrophobic.
  • They do not form true polymers
38
Q

Lipids

A

Major types include:
* fats and oils
* waxes
* phospholipids
* steroids.

39
Q

Fats and oils

A
  • A stored form of energy and can include triglycerides.
  • Fats and oils are usually made up of fatty acids and glycerol.
40
Q

triglyceride

A

A fat molecule consisting of two main components:
1. glycerol
2. fatty acids.

41
Q

Glycerol

A

An organic compound with:
* three carbon atoms
* five hydrogen atoms
* three hydroxyl (OH) groups.

42
Q

Fatty acids

A

A long chain of hydrocarbons to which an acidic carboxyl group is attached, hence the name “fatty acid.”

43
Q

Unsaturated fats

A
  • They are liquid at room temperature and are called oils.
  • Plant & Fish fats
44
Q

Saturated

A
  • 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
Q

Saturated fatty acids

A
  • Are saturated with hydrogen
  • tend to get packed tightly
  • solid at room temp.
46
Q

Phospholipids

A
  • 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
Q

Fatty acids are hydrophobic.

A

Phosphates are hydrophilic.

48
Q

Steroids

A
  • 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
Q

Proteins

A
  • 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
Q

Amino acids

A
  • 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
Q

Protein

A
  • 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
Q

Denaturation

A

Changes in temperature, pH, and exposure to chemicals may permanently change the protein’s shape, leading to a loss of function.

53
Q

Polypeptide

A
  • Peptide bonds link a long chain of amino acids.
  • A polymer of amino acids
54
Q

Proteins are organized at four levels.

A
  1. Primary
  2. secondary
  3. tertiary
  4. quaternary.
55
Q

Enzymes

A
  • 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
Q

Induced-fit model

A

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
Q

Allosteric inhibition

A

Indirectly induces a conformational change to the active site such that the substrate no longer fits.

58
Q

Allosteric activation

A

The activator molecule modifies the shape of the active site to allow a better fit of the substrate.

59
Q

Nucleic acids

A
  • DNA & RNA
  • Molecules consist of repeating units of nucleotides that direct cellular activities such as cell division and protein synthesis.
60
Q

Nucleotides

A

Monomers that contain:
1. a monosaccharide
2. a phosphate group
3. a nitrogenous base.

61
Q

A nucleotide is made up of three components.

A
  1. A nitrogenous base
  2. A pentrose sugar
  3. A phosphate group.
62
Q

ATP- Adenosine triphosphate

A

Particular nucleotides that are vital to life.

63
Q

Peptide bond

A

Link amino acids together.

64
Q

Chitin

A

A structural polysaccharide found in arthropod skeletons.

65
Q

Hydrolysis

A

Disassemble polymers into monomers, a reaction that is the reverse of dehydration.

66
Q

Four types of macromolecules

A
  1. Carbohydrates
  2. Lipids
  3. Protein
  4. Nucleic acid
67
Q

Polar covalent bond

A
  • 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
Q

Nonpolar covalent bonds

A

Atoms share the electron equally.

69
Q

Chemical bonding

A
  • 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
Q

Isotopes

A
  • Different forms of elements because of a loss of neutrons.
  • Form at predictable rates & can be used in dating.
71
Q

Elements

A
  • Unique to themselves
  • It cannot be turned into something else.
72
Q

Molecule

A

Two or more atoms are held together by covalent bonds.

73
Q

Bonding

A
  • Elements with partially full valence shells satisfy the octet rule.
  • Atoms with incomplete valence shells share or transfer electrons.

Biology (2 decks)

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