Unit 2 Slides AY242

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76 Terms

1

Chemistry

The study of the chemical and physical interactions of matter, involving about 100 different atoms that create the macroscopic world.

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2

Atom

The basic unit of an element that can enter into chemical combinations; most originated with the birth of the universe.

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3

Atomic Nucleus

The dense center of an atom containing protons and neutrons, accounting for almost all of the atomic mass.

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4

Electron

A negatively charged subatomic particle that resides outside the nucleus and is involved in chemical bonding. Also determine chemical behavior.

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5

Atomic Number (Z)

The number of protons in an atom, which determines the chemical identity of the element.

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6

Mass Number (A)

The total number of protons and neutrons in an atom's nucleus.

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7

Isotope

Atoms of the same element with the same atomic number but different mass numbers due to varying numbers of neutrons.

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8

Valence Electrons

Electrons in the outermost shell of an atom that can participate in bond formation.

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9

Compound

A substance formed when two or more elements combine in definite proportions, often with different properties from the individual elements.

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10

Molecule

A molecular compound consisting of two or more atoms held together by chemical forces.

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11

Ionic Compound

A compound formed from ions in a 3D network, held together by ionic bonds due to the attraction between oppositely charged ions.

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12

van der Waals Forces

Weak attractions between molecules that arise from temporary charge separations due to electron movement.

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13

Polar Molecule

A molecule with a charge separation, leading to slightly positive and negative regions, such as water.

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14

Hydrogen Bond

active interaction between the hydrogen atom in a polar bond with oxygen, nitrogen, or fluorine and another oxygen nitrogen or fluorine atom

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15

Cohesion

The attraction between molecules of the same substance, responsible for surface tension in liquids like water.

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16

Adhesion

The attraction between molecules of different substances, which can be stronger than cohesion in some cases.

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17

pH Scale

A scale that indicates the concentration of hydrogen ions (H+) in a solution, with each step representing a tenfold change.

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18

Organic Chemistry

The study of compounds that contain carbon-to-carbon bonds, focusing on the six most abundant elements in living organisms.

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19

Macromolecules

Large organic compounds found in living cells, formed from smaller molecules through polymerization; includes carbohydrates, lipids, nucleic acids, and proteins.

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20

Amino Acid

The monomer of proteins, consisting of a central carbon atom, an amino group, a carboxyl group, and a variable side chain (R).

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21

Peptide Bond

A covalent bond formed between two amino acids during protein synthesis.

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22

Catalyst

A substance that speeds up a chemical reaction by lowering the activation energy required for the reaction to proceed.

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23

Enzyme

A specific type of protein that acts as a catalyst in biological reactions, facilitating the conversion of substrates into products.

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24

Endergonic Reaction

A reaction that requires energy input to proceed, resulting in a positive change in free energy (ΔG > 0).

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25

lipids

Also known as fats, oils, & waxes. Mostly made from carbon & hydrogen. Cannot form (enough) hydrogen bonds therefore, insoluble in water

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26

Active Site

The area on an enzyme where the substrates react. The environment is more favorable for a reaction.

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27

Substrates

reactants in an enzyme

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Protons

part of the nucleus determines atomic number has a positive charge

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neutrons

part of the atomic nucleus, neutral charge, provide mass and stability

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Core Electrons

Only 2 electrons in core

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Covalent Bonds

When molecules share two or more electrons (double bond shares 4) (tripe bond shares 6)

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ionic bonds

atoms donate or accept electrons to form ions

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33

solubility of hydrogen bonding atoms

atoms that hydrogen bond mix and dissolve well in water

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34

Heat Capacity

Water can absorb or release a large amount of energy with only a small change in temperature because it can form so many hydrogen bonds

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Mixture

combination of two or more substances in which the substances retain their distinct identities

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solution

type of mixture where all components are evenly distributed. The solute is dissolved in the solvent.

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37

Suspension

movement of water molecules keep small particles suspended but not fully dissolved

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38

Ionization of water

Water can ionize to form hydroxide ions (OH-) and hydrogen ions (H+). In pure water the concentration of hydroxide ions and hydrogen ions is equal.

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39

acids

forms H+ in solution

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40

base

forms OH- in solution

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buffers

Weak acids or bases that help keep the pH stable. This is critical for homeostasis. 

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42

six most abundant elements in living things

carbon, hydrogen, oxygen, nitrogen, phosphorus, and sulfur.

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43

How many valence electrons and covalent bonds can hydrogen make

1 valence 1 covalent bond

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44

How many valence electrons and covalent bonds can carbon make

4 valence, 4 covalent bonds

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How many valence electrons and covalent bonds can nitrogen make

5 valence, 3 covalent bonds

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How many valence electrons and covalent bonds can oxygen make

6 valence, 2 covalent

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47

polymerization

when monomers join together to form polymers

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48

monomer

one molecule in a polymer

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polymer

many monomers connected to each other

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dehydration synthesis

a water molecule is lost to combine two monomers

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51

hydrolysis

a water molecule is added to split a polymer

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52

carbohydrate

Also known as sugars & starches. Made from carbon, hydrogen, & oxygen, usually in a 1:2:1 ratio. (H - C - OH) It can form hydrogen bonds and, therefore, be soluble in water. Used for storing energy and providing structure

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monosaccharide

monomer of a carbohydrate

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polysaccharide

polymer of carbohydrates

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Cellulose

main structural component of plants

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Starch

main energy reserve in plants

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Glycogen

functions as an energy reserve for animals

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saturated lipids

have all carbon to carbon single bonds (solid at room temp)

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59

unsaturated lipids

at least one carbon-to-carbon double bond (liquid at room temp)

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60

what are nucleic acids made of

carbon, hydrogen, oxygen, nitrogen & phosphorus

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61

nucleic acids

Used for energy (ATP) & storing hereditary information

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nucleotide

monomer of nucleic acid

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nucleotide chemical structure

5-carbon sugar, Nitrogenous base, 1 to 3 phosphate groups (PO43-)

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what are proteins made of

carbon, hydrogen, oxygen, nitrogen, & sulfur

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polypeptide

string of amino acids

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protein

polypeptide with a function

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what are amino acids made of

amino group, side chain, carboxyl group

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68

protein folding primary structure (1o)

amino acid sequence.

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protein folding secondary (2o)

folds & coils due to the backbone forming hydrogen bonds.

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70

protein folding tertiary (3o)

three-dimensional shape

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protein folding quarternary (4o)

when a functional protein is made up of more than one polypeptide. Not all proteins have 4o structure

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chemical reaction

one or more substances are rearranged into one or more new substances. Chemical bonds are broken and new bonds form. Atoms are not created or destroyed, simply reorganized

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exergonic reaction

reaction that releases anergy

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74

activation energy

energy input required for a reaction to proceed

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75

what are the four types of macromolecules

carbohydrates, lipids, nucleic acids, proteins

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