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Biology > Chapter 2 - Chemistry - Orange Booklet > Flashcards

Chapter 2 - Chemistry - Orange Booklet Flashcards

LeCurse

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1
Q

Atom

A

The smallest particle of an element that has the traits of the element

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2
Q

Atomic Number

A
  • The number that identifies a particular element and is equal to the number of protons in each atom of the element
  • Never changes during chemical reactions
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3
Q

Chemical Bond

A

An interaction between atoms that holds the two atoms together based on events relating to electrons in the two atoms

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4
Q

Chemical Reaction

A

A rearrangement of atoms in substances that results in the production of new substances

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5
Q

Compound

A
  • A pure substance that is composed of particles made of two or more elements
  • will always have a charge of 0 or else will be unstable
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6
Q

Covalent Bond

A

A bond between atoms involving the sharing of a pair of electrons between the atoms involved to fill the atom’s valence level

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7
Q

Ionic Bond

A

A bond between atoms involving the formation of oppositely charged ions by the transfer of electron(s) from one atom to another

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8
Q

Electron

A
  • A subatomic particle with a negative charge, essentially no mass, and that is located in regions around the atom’s nucleus (cloud)
  • The farther from the nucleus, the higher the electron energy
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9
Q

Valence Electron

A
  • An electron that is located in the outermost occupied energy level of an atom
  • If levels are 1,2,3, you lose electrons to make the charge positive (metals)
  • if levels are 5,6,7, you gain electrons to make the charge negative (non-metals)
  • Electrons with 4 levels, you share
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10
Q

Neutron

A

A subatomic particle that is located in the nucleus of an atom and has a mass of 1 amu, and no charge (neutral)

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11
Q

Proton

A

A subatomic particle that is located in the nucleus of an atom, has a mass of 1 amu, and a positive charge

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11
Q

Element

A

A substance composed of only one type of atom

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12
Q

Energy Level

A

Relates to the position of electrons around an atom’s nucleus; higher energy levels have electrons with more energy and are located farther from the nucleus

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13
Q

Ion

A

A charged particle (anion = negatively charged particle; cation = positively charged particle) as a result of gaining/losing an electron

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14
Q

Mass

A

A measure of how much matter an object has (measured in grams (g))

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14
Q

Molecule

A

The smallest particle of a covalent compound

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14
Q

Matter

A

Anything with mass and volume

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15
Q

Nucleus

A

The area within an atom where protons and neutrons are located

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15
Q

Isotope

A

An atom that differs in its mass (and neutron #) from another atom of the same element

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16
Q

Energy

A
  • The ability to do work or cause change
  • Different types of energy too
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17
Q

Free Energy

A

Energy that’s available to do work

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18
Q

Electron Orbits

A
  • The path of an electron around the nucleus of an atom
  • Concept created by Niels Bohr
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19
Q

Electron Orbitals

A

Concept that describes the general regions where electrons travel as they circle the nucleus of the atom; each orbital is associated with a certain energy level

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20
Q

Charge-Cloud/Quantum Mechanic Model

A

Name of the modern model of the atom; involves a dense, positive nucleus surrounded by cloud-like areas (orbitals) where electrons travel

21
Q

Balanced Equation

A

Representation of the events of a chemical reaction that follows the law of conservation of matter (reactants → products)

22
Q

Law of conservation of matter

A

Concept that during any chemical reaction there is no creation and no destruction of matter

22
Q

Periodic Table

A
  • An ordered listing of the elements in such a way as to illustrate trends and similarities
  • Metals on the left
  • Non-Metals on the right
23
Q

Period (On Periodic Table)

A
  • A row on the periodic table
  • the number of the period indicates the number of occupied energy levels in neutral atoms of those elements, and the position in the period indicates the number of valence electrons in atoms of a particular element
  • Period goes horizontal (left to right)
24
Q

Activation Energy

A

The amount of energy that must be absorbed by reactants in order for a chemical reaction to proceed

25
Q

Catalyst

A
  • A substance or particle that reduces activation energy of a reaction, thereby increasing the rate of the reaction
  • Reactants DONT change with catalyst
26
Q

Endergonic Reaction

A
  • A reaction in which more energy is absorbed than is released
  • Pulls heat in
27
Q

Exergonic Reaction

A
  • Reaction in which more energy is released than is absorbed
  • Heat is a product
  • Doesn’t need as much energy to get started, starts on the line
28
Q

Endothermic Reaction

A

An endergonic reaction in which the type of energy involved is heat energy

29
Q

Exothermic Reaction

A

Exergonic reaction in which the form of energy involved is heat

30
Q

Reactant

A

The material that is present before a chemical reaction occurs

31
Q

Product

A

The material that is formed as a result of a chemical reaction

32
Q

State (of matter)

A

Arrangement of particles in a material; for our purposes, it may be solid, liquid or gas

33
Q

Acid

A
  • A substance that causes a mixture to have a higher hydronium ion concentration than hydroxide ion concentration
  • [H3O] > [OH]
  • pH < 7
  • Sour taste
  • Formula starts with H
34
Q

Base

A
  • A substance that causes a mixture to have a higher hydroxide ion concentration than hydronium ion concentration
  • [H3O] < [OH]
  • Bitter Taste
  • pH > 7
  • Formula starts with OH
  • Another name for Alkaline
35
Q

Alkaline

A

An adjective that is synonymous with “basic”, meaning the opposite of acidic

36
Q

Aqueous Solution

A

Any solution with water as the solvent

37
Q

Buffer

A

A mixture that neutralizes small amounts of added acid or base; such a mixture resists a change in pH

38
Q

Concentration

A

A measure of how much solute is present in a given amount of solvent
(e.g., molarity is a measure of concentration defined as moles of solute per 1 liter of solution)

39
Q

Dissociation (of water)

A

The natural breakdown of water molecules in any given sample of water

40
Q

Hydronium Ion

A
  • Positive ion formed by dissociation of water or by addition of acid; formula = H3O+
  • More acidic = Higher hydronium ion concentration → lower pH
41
Q

Hydroxide Ion

A
  • Negative ion formed by dissociation of water or by addition of base; formula = OH
  • Less acidic = More basic → Lower hydronium ion concentration → higher pH
42
Q

pH scale

A

Representation of the measure of hydronium ions in a solution, indicating level of acidity or basicity of a solution

43
Q

Saturated Solution

A

A solution that has the maximum amount of solute without the solute precipitating (falling to the bottom of container)

44
Q

Solute

A

For biology….the material in lesser amount

45
Q

Solution

A

A mixture in which particles are so small that they do not interfere with the passage of light nor do the particles precipitate (fall to bottom); solutions are clear

46
Q

Solvent

A

For biology… the material in greater amount in a solution

47
Q

Heterogenous Mixture

A

A mixture in which the materials are not evenly distributed (suspensions)

48
Q

Homogenous Mixture

A
  • A mixture in which the materials are uniformly distributed
  • True solution: clear
  • Colloidal solution: cloudy
49
Q

Suspension

A

A mixture that has particles large enough that they will precipitate (fall to the bottom of container) unless energy is consistently added

50
Q

Colloid

A

A mixture that has particles large enough to interfere with pass of light, but not large enough to precipitate (fall to bottom of container)

51
Q

John Dalton

A
  • First to propose a coherent theory of the atom
  • All matter is made of atoms which are indivisible and indestructible
  • All atoms of a given element are identical
  • Atoms of different elements combine in fixed ratios to make compounds
52
Q

J.J. Thomson

A
  • Created Crookes tube
  • Atoms have small particles that are negative
  • Because atoms are neutral, there must also be positive charge associated with the atom
53
Q

Ernest Rutherford

A
  • Used new knowledge of radioactive materials
  • Most of mass was in the center of an atom and the center was positively charged
  • Only a small volume of significant mass exists in an atom meaning the massive center must be positive because it repelled the positive alpha particles
54
Q

Niels Bohr

A
  • Electrons must absorb and release specific amounts of energy - climb up the ladder by raising leg-specific distances. Therefore electrons move in well-defined paths called “Orbits”

Biology (2 decks)

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