Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

chem final vocab > gen chem > Flashcards

gen chem Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Atomic number

A

number of protons in the neuclus of an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Atomic mass

A

Atomic mass is the average mass of the protons, neutrons, and electrons in an atom.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Elements

A

An element is a pure substance that is made from a single type of atom.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

compounds

A

a substance made up of two or more different chemical elements combined in a fixed ratio

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Isotopes

A

Atoms with the same number of protons but different numbers of neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Radioactivity

A

the release of energy from the decay of the nuclei of certain kinds of atoms and isotopes.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Avogadro’s number

A

the number of particles in 1 mole (or mol) of a substance.

6.022×10^23 mol−1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Building up principle

A

in the ground state of an atom or ion, electrons fill atomic orbitals of the lowest available energy level before occupying higher-energy levels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Quantum numbers

A

The set of numbers used to describe the position and energy of the electron in an atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Atomic orbitals

A

An orbital is a three dimensional description of the most likely location of an electron around an atom.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Pauli exclusion principle

A

in an atom or molecule, no two electrons can have the same four electronic quantum numbers.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Hund’s rule

A

every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Covalent bond

A

the force of attraction that holds together two atoms that share a pair of valence electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Bonding energies

A

the amount of energy required to break apart a mole of molecules into its component atoms.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Resonance

A

describes the delocalization of electrons within molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

delocalized bonding

A

a bond that appears in some resonance forms, but not others.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Polar covalent bond

A

a covalent bond in which the atoms have an unequal attraction for electrons, and so the sharing is unequal.

Slightly positive side, slightly negative charge ex H2O

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Dipole moment

A

a measure of the system’s overall polarity. a measurement of the separation of two opposite electrical charges.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Ionic bond

A

formed between two or more atoms by the transfer of one or more electrons between atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Intermolecular forces

A

he attractive and repulsive forces that arise between the molecules of a substance.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Hydrogen bonding

A

a weak bond between two molecules resulting from an electrostatic attraction between a proton in one molecule and an electronegative atom in the other.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Van der Waals forces

A

relatively weak electric forces that attract neutral molecules to one another in gases, in liquefied and solidified gases, and in almost all organic liquids and solids.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

dipole-dipole

A

attractive forces between the positive end of one polar molecule and the negative end of another polar molecule.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

London forces

A

a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Ideal gas law

A

ideal gas law, relation between the pressure P, volume V, and temperature T of a gas in the limit of low pressures and high temperatures, such that the molecules of the gas move almost independently of each other.

PV=nRT

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Sublimation

A

Sublimation is the transition of a substance directly from the solid to the gas state, without passing through the liquid state.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

lyophilization

A

a drying technique by which a product is solifidied by freezing and the solvent that contains it (usually water) is evaporated by sublimation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Microheterogeneous systems

A

A closed system containing at least two phases is called a heterogeneous system. Reactions (changes) between or among phases are driven by energy manifested in temperature of chemical potentials. ex ice, water and steam

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

colloidal state and size

A

a mixture that has particles ranging between 1 and 1000 nanometers in diameter, yet are still able to remain evenly distributed throughout the solution.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Tyndall effect

A

When light is passed through a colloidal solution, it is observed that the colloidal particles do not permit the light to pass through it completely

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Types of colloids

A

The types of colloids includes sol, emulsion, foam, and aerosol.

Sol is a colloidal suspension with solid particles in a liquid.

Emulsion is between two liquids.

Foam is formed when many gas particles are trapped in a liquid or solid.

Aerosol contains small particles of liquid or solid dispersed in a gas.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

hydrophobic

A

a property of molecules that do not mix with water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

hydrophilic

A

molecule is one that is able to interact with water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

dispersed

A

a system in which distributed particles of one material are dispersed in a continuous phase of another material.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

macromolecular

A

large polymer molecules made up of several smaller molecules bonded together by covalent bonds.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

association colloids

A

Associated colloids are those colloids which behave as normal strong electrolytes at low concentrations but exhibit colloidal properties at higher concentrations due to the formation of aggregated particles.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

Homogeneous systems

A

one whose properties are either the same throughout the system, or vary continuously from point to point with no discontinuities.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

Saturated solutions

A

A solution with solute that dissolves until it is unable to dissolve anymore, leaving the undissolved substances at the bottom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

unsaturated solutions

A

a solution that contains less than the maximum amount of solute that is capable of being dissolved.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

Solubility

A

is the ability of a substance, the solute, to form a solution with another substance, the solvent.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

Osmosis

A

the passage of water and small molecules across a semipermeable membrane with a net flow from a less concentrated solution to a more concentrated solution.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

Chemical equilibrium

A

a state of balance in a reaction where the forward and reverse reaction speed is equal and the concentrations of the products and reactants remain unchanged.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

equilibrium constant

A

expresses the relationship between products and reactants of a reaction at equilibrium with respect to a specific unit.

44
Q

law of mass action

A

the rate of a reaction is proportional to the product of the concentrations of each reactant.

45
Q

Le Chatelier’s principle

A

A change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.

46
Q

precipitation

A

is the formation of a solid in a solution during a chemical reaction.

47
Q

gas formation

A

a chemical reaction produces a gas as one of its products.

48
Q

neutralization

A

when an acid and a base react to form water and a salt and involves the combination of H+ ions and OH- ions to generate water.

49
Q

Solubility equilibrium

A

a type of dynamic equilibrium that exists when a chemical compound in the solid state is in chemical equilibrium with a solution of that compound.

Ksp=[A]^a[B]^b

50
Q

solubility product constant

A

Ksp​, is the equilibrium constant for a solid substance dissolving in an aqueous solution. It represents the level at which a solute dissolves in solution. The more soluble a substance is, the higher the Ksp value it has.

51
Q

Electrolytes

A

a substance that dissociates in water into charged particles called ions.

52
Q

degree of dissociation

A

the percentage of substance that has dissociated.

53
Q

Bronsted-Lowry

A

A Brønsted-Lowry acid is any species that can donate a proton, ‍ , and a base is any species that can accept a proton.

54
Q

Amphoteric species.

A

molecules or ions that can react as an acid as well as a base

55
Q

Lewis concept of acids and bases

A

a Lewis acid is an electron-pair acceptor. A Lewis base is any substance, such as the OH- ion, that can donate a pair of nonbonding electrons.

56
Q

Self-ionization of water

A

The reaction in which a water molecule donates one of its protons to a neighbouring water molecule

57
Q

Ion product of water

A

The ion product of water, Kw = [H3O+] [OH−], has the value 1.0 × 10^−14

58
Q

dissociation constants

A

(KD) is a specific type of equilibrium constant that measures the propensity of a larger object to separate (dissociate) reversibly into smaller components

59
Q

hydrolysis

A

a chemical reaction in which a molecule of water breaks one or more chemical bonds

60
Q

Acid-base titration

A

used to find the amount of a known acidic or basic substance through acid base reactions

61
Q

titration curves

A

a graphical representation of the pH of a solution during a titration. In a strong acid-strong base titration, the equivalence point is reached when the moles of acid and base are equal and the pH is 7

62
Q

Common-ion effect

A

an effect that suppresses the ionization of an electrolyte when another electrolyte (which contains an ion which is also present in the first electrolyte, i.e. a common ion) is added

63
Q

Buffers

A

a solution that can resist pH change upon the addition of an acidic or basic components

64
Q

Henderson-Hasselbalch equation

A

provides a relationship between the pH of acids (in aqueous solutions) and their pKa (acid dissociation constant).

pH= pKa+log [A-]/[HA]

65
Q

Types of buffers.

A

acidic buffer and basic buffer: A solution with weak acid and its salts containing strong bases is called an acidic buffer solution. E.g., A solution with CH3COOH, which is weak acid and CH3COONa, which is its salt is an acidic buffer solution

66
Q

Buffer capacity

A

the moles of an acid or base necessary to change the pH of a solution by 1, divided by the pH change and the volume of buffer in liters

67
Q

Thermodynamics

A

the study of the relations between heat, work, temperature, and energy.

68
Q

State functions

A

a property whose value does not depend on the path taken to reach that specific value

69
Q

Exothermic reactions

A

if heat is released by the system into the surroundings

70
Q

endothermic reactions

A

any chemical reaction that absorbs heat from its environment

71
Q

Internal energy

A

all the energy within a given system, including the kinetic energy of molecules and the energy stored in all of the chemical bonds between molecules.

72
Q

The first law of thermodynamics

A

energy cannot be created or destroyed; it can only be converted from one form to another

73
Q

The second laws of thermodynamics

A

the state of entropy of the entire universe, as an isolated system, will always increase over time

74
Q

The heat of reaction and enthalpy

A

the change in the enthalpy of a chemical reaction that occurs at a constant pressure. It is a thermodynamic unit of measurement useful for calculating the amount of energy per mole either released or produced in a reaction.

75
Q

Hess’s law

A

regardless of the multiple stages or steps of a reaction, the total enthalpy change for the reaction is the sum of all changes.

76
Q

Entropy

A

describes the randomness and disorder of molecules based on the number of different arrangements available to them in a given system or reaction.

order to disorder takes no energy but it is spontaneous

77
Q

third laws of thermodynamics

A

the entropy of a system approaches a constant value as the temperature approaches absolute zero

78
Q

Entropy changes for a reaction

A

the standard entropy change is the sum of the standard molar entropies of the products minus the sum of the standard molar entropies of the reactants.

79
Q

Spontaneous reactions

A

a reaction that favors the formation of products at the conditions under which the reaction is occurring there is a decrease in the energy of the system as energy is released to the surroundings as heat

80
Q

Gibbs Free energy

A

combines enthalpy and entropy into a single value. The change in free energy, ΔG, is equal to the sum of the enthalpy plus the product of the temperature and entropy of the system.

81
Q

Electrodes

A

a metal whose surface serves as the location where oxidation-reduction equilibrium is established between the metal and what is in the solution

82
Q

voltaic cells

A

use a thermodynamically favored redox reaction to generate an electric current

83
Q

standard potential

A

the ability of a species to gain or lose electrons, i.e., its reduction or oxidation potential.

84
Q

standard potential

A

a measure of the reducing power of any element or compound

85
Q

Electromotive force

A

the electric potential produced by either an electrochemical cell or by changing the magnetic field.

86
Q

Nernst equation

A

The Nernst Equation enables the determination of cell potential under non-standard conditions.

E=E˚-(RT/nF)*ln(Q)
E= reduction potential
E˚=standard potential
R=gas constant
T=temp
n= moles of electrons
F=faraday constant
Q=reaction quotient

87
Q

Redox reactions

A

are reactions that involve the transfer of electrons from one species to another

88
Q

Reaction kinetics

A

study of reaction rate

89
Q

Elementary reactions

A

chemical reaction in which one or more chemical species react directly to form products in a single reaction step and with a single transition state

90
Q

molecularity of a reaction

A

the number of molecules that come together to react in an elementary (single-step) reaction

91
Q

Reaction rate

A

the speed at which a chemical reaction proceeds

92
Q

Rate law

A

that provides a relationship between the rate of the reaction and the concentrations of the reactants participating in it.

93
Q

rate constant

A

the proportionality constant in the equation that expresses the relationship between the rate of a chemical reaction and the concentrations of the reacting substances

rate=K[A]^a[B]^b

94
Q

Reaction order

A

first order= concentration x2 rate x2
Second order= concentration x2 rate x4
zero order= concentration x2 rate x1

95
Q

Activation energy

A

the minimum energy required to cause a process (such as a chemical reaction) to occur.

96
Q

Activated complex

A

the state of a molecule when the reaction is at the point of activation energy.

97
Q

complex chemical reactions

A

takes place when the reactants are converted into products in multiple steps or more than one step

98
Q

Catalysts

A

a substance that speeds up a chemical reaction, or lowers the temperature or pressure needed to start one, without itself being consumed during the reaction.

99
Q

peroxides

A

any of a class of chemical compounds in which two oxygen atoms are linked together by a single covalent bond

99
Q

Enzymes

A

proteins that act upon substrate molecules and decrease the activation energy necessary for a chemical reaction to occur by stabilizing the transition state.

99
Q

oxides

A

a chemical compound containing at least one oxygen atom and one other element in its chemical formula. Oxide itself is the dianion (anion bearing a net charge of –2) of oxygen, an O2– ion with oxygen in the oxidation state of −2.

100
Q

superoxides

A

a compound that contains the superoxide ion, which has the chemical formula O−2

101
Q

Complex compounds

A

a class of substances with a chemical structure where the central atom is a metal and it is surrounded by non-metal atoms or a group of atoms

102
Q

Coordination number

A

the number of atoms, ions, or molecules that a central atom or ion carries in a complex or coordination compound or in a crystal as its closest neighbours.

103
Q

Chelate complexes

A

any of a class of coordination or complex compounds consisting of a central metal atom attached to a large molecule, called a ligand, in a cyclic or ring structure.

ex hemoglobin

chem final vocab (3 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions