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AP Chem > VOCAB tk > Flashcards

VOCAB tk Flashcards

(87 cards)

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1
Q

Activation Energy

A

Minimum energy needs to be added to a system in order for the chemical reaction to occur

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2
Q

Alpha Particle

A

He+2. 2 protons, mass number=4, 2+charge Highly ionizing particle;Low energy

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3
Q

Anion

A

Negatively charge ion

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4
Q

Arrhenius Acid

A

Donates a H+ ion

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5
Q

Arrhenius Base

A

Donates a OH- ion

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6
Q

Atom

A

Smallest constituent unit of ordinary matter that has the properties of a chemical element

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7
Q

Atomic mass

A

Average of all naturally occurring isotopes

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8
Q

Atomic Number

A

Number of protons; defines the atom

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9
Q

Beta Particle

A

-1 proton, mass number=0; medium ionizing ability, medium energy

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10
Q

Boiling

A

Phase change from liquid to gas

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11
Q

Bronsted-Lowry Acid

A

Donates a proton, H+

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12
Q

Bronsted-Lowry Base

A

Accepts a proton, H+

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13
Q

Calorimetry

A

Means of measuring the heat gained/lost by a system during a chemical reaction

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14
Q

Catalyst

A

Lowers the activation energy. Not a reactant. Not a product

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15
Q

Cation

A

Positively charged ion

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16
Q

Chemical equilibrium

A

Rate of the forward reaction equals the rate of the reverse reaction

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17
Q

Condensation

A

Phase change from gas to a liquid

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18
Q

Covalent bond

A

Bond formed by the sharing of electrons between atoms

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19
Q

Deposition

A

Phase change from a gas to a solid

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20
Q

Dipole-Dipole

A

Permanent intermolecular forces present in polar molecules

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21
Q

Direct relationship

A

Relationship between two variables where when one changes, the other changes in the
same manner

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22
Q

Dissociate

A

To break into ions

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23
Q

Dissolve

A

To break into smaller pieces

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24
Q

Distillation

A

Process of separating liquids based on differences in boiling temperatures

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25
Double Bond
Two shared pairs of electrons
26
Electrolyte
Dissociates into charge particles which are capable of conducting electricity
27
Electrolytic Cell
Redox reaction that is nonspontaneous
28
Electronegativity
The ability of an atom to attract electrons from another atom. Quantity that can’t be measured. ****** Fluorine is most electronegative element.
29
Electron Affinity
Energy released when an atom gains an electron. Actual quantity that can be measured. *****Chlorine has highest electron affinity.
30
Electron
Negatively charged particle. Charge = -1, Mass ~ 0amu. Located in the orbitals surrounding the nucleus
31
Empirical formula
Lowest whole number ratio of atoms in a compound
32
Molecular Formula
The true formula representing the actual number of each atom present in the substance.
33
Endothermic
Energy is gained by the system
34
Exothermic
Energy is released by the system
35
Evaporation
Process of removing water from an aqueous solution. Solute is left behind
36
Filtrate
Liquid that passes through the filter paper
37
Filtration
Process of separating a precipitate from its aqueous solution
38
Formula Unit
Ionically bonded atoms
39
Freezing
Phase change from a liquid to a solid
40
Galvanic / Voltaic Cell
Redox reaction that is spontaneous
41
Gamma Ray
0 protons, mass number = 0, Low ionizing ability, high energy
42
Halogen
Elements in group 17. Form halides as ions
43
Hydrogen Bonding
Strong dipole-dipole that results when H is bonded to F, O, or N (Special dipole that exists in only selective polar molecules)
44
Indirect Relationship
Relationship between two variables where when one changes, the other changes in the opposite manner
45
Insoluble
Does not dissolve in water
46
Intermediate
Species produced in one step and consumed in another step
47
Intermolecular Forces, IMF
Attractive forces between molecules
48
Ion
Charge particle
49
Ionic Bond
Bond formed by the transfer of 1 or more electrons from the least electronegative atom to the more electronegative atom
50
Ionization Energy
Energy required to remove the outer electron
51
Kinetic Energy
Energy of motion, temperature is a measure of KE
52
Limiting reactant
Reactant that runs out first thus limiting the amount of product that can be formed
53
London Dispersion Forces
Temporary intermolecular forces caused by the movement of electrons. Present in all nonpolar and polar substances. Most prominent in Nonpolar molecules.
54
Lone pair
Unbonded electrons
55
Mass number
Mass of all protons and neutrons
56
Melting
Phase change from a solid to a liquid
57
Molar mass
grams per 1 mol
58
Molarity
moles of solute per liter of solution
59
Molecule
Covalently bonded atoms
60
Neutron
Neutral particle. No charge. Mass = 1amu, Located in the nucleus
61
Noble Gas
Group 18 on the PT. Each has 8 valence electrons. Nonreactive
62
Orbital
Regions of probability where electrons are located. Each orbital can contain up to 2 electrons
63
Oxidation Number
A charge assigned to an atom that represents that charge it would have if it contained an ionic bond. Oxidation numbers are written as charge value, +4, -6, +2
64
Oxidation
Process of losing electrons which increases the oxidation number
65
Percent Error
Absolute value (Theoretical – Experimental) / Theoretical) x 100%
66
Percent Yield
(Quantity produced / Theoretical Amount) x 100%
67
Precipitate
Solid matter that forms from the reaction of two aqueous solutions
68
Principle Energy Levels
n= 1 means first energy level. Energy levels contain sublevels
69
Proton
Positively charged particle. Charge = +1, Mass = 1amu, Located in the nucleus
70
Reduction
Process of gaining electrons which reduces the oxidation number
71
Single bond
One shared pair of electrons
72
Soluble
Dissolves in water
73
Solute
The species that gets dissolved to form a solution
74
Solution
Solute and solvent
75
Solvent
The species that does the dissolving to form a solution
76
Sources of Erorr
These are errors that you make in the lab which result in either increased or decreased yields. These do not include Human Error, Calculations, Massing…..
77
Specific Heat
Energy required to raise 1 gram of a substance 1C
78
Strong Acid
Dissociates 100%
79
Strong base
Dissociates 100%
80
Sublevel
s, p, d, and f. defines the shape
81
Sublimation
Phase change from a solid to a gas
82
Surroundings
This refers to everything outside of the system
83
System
This refers to the reaction
84
Triple bond
Three shared pairs of electrons
85
Valence electrons
Outer electrons which are available for bonding
86
Weak acid
Dissociate very little. Remains mostly in its molecular form
87
Weak base
Dissociate very little. Remains mostly in its molecular form

AP Chem (5 decks)

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