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gen chem Flashcards

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1
Q

Atomic number

A

number of protons in the neuclus of an atom

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2
Q

Atomic mass

A

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

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3
Q

Elements

A

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

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4
Q

compounds

A

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

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5
Q

Isotopes

A

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

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6
Q

Radioactivity

A

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

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7
Q

Avogadro’s number

A

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

6.022×10^23 mol−1

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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

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9
Q

Quantum numbers

A

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

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10
Q

Atomic orbitals

A

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

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11
Q

Pauli exclusion principle

A

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

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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.

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13
Q

Covalent bond

A

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

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14
Q

Bonding energies

A

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

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15
Q

Resonance

A

describes the delocalization of electrons within molecules

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16
Q

delocalized bonding

A

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

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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

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18
Q

Dipole moment

A

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

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19
Q

Ionic bond

A

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

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20
Q

Intermolecular forces

A

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

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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.

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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.

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23
Q

dipole-dipole

A

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

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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.

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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

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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.

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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

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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

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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.

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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

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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.

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32
Q

hydrophobic

A

a property of molecules that do not mix with water

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33
Q

hydrophilic

A

molecule is one that is able to interact with water

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34
Q

dispersed

A

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

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35
Q

macromolecular

A

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

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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.

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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.

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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

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39
Q

unsaturated solutions

A

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

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40
Q

Solubility

A

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

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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.

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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.

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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)

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