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General Chemistry Flashcards

(51 cards)

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1
Q

Anode

A

The electrode at which oxidation occurs during a cell’s redox reaction. Electrons always flow from the anode in an electrochemical cell

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2
Q

Alkali Metals

A

The highly reactive elements found in Group IA of the periodic table (except for hydrogen)

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3
Q

Solute

A

A compound, commonly a solid, dissolved in a solvent to create a solution

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4
Q

Exothermic Reaction

A

A reaction that proceeds with the net release of energy (heat) into the surroundings

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5
Q

Decomposition Reaction

A

A chemical reaction in which one substance breaks down into multiple substances (e.g., C –> A + B)

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6
Q

Chemical Kinetics

A

The study of reaction rates and the factors that affect them

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7
Q

Aqueous Solution

A

A solution with water as its solvent

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8
Q

Effective Nuclear Charge

A

The attractive force a valence electron feels from the nucleus, after accounting for the shielding effect of inner core electrons.

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9
Q

Reduction

A

Part of a reaction in which a species gains electrons

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10
Q

Non-polar Covalent Bond

A

A type of covalent bond between atoms with the same electronegativities resulting in the equal sharing of electrons

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11
Q

Molecule

A

Two or more atoms joined by covalent bonds. A molecule is the smallest unit of a compound that still retains all the chemical properties of that compound

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12
Q

Effusion

A

the movement of gas through a small opening into an area of lower pressure

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13
Q

Bond Energy

A

the energy required to break one mole of a chemical bond; bond enthalpy

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14
Q

Law of Conservation of Energy

A

Law stating that energy cannot be created nor destroyed but only transferred and transformed

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15
Q

Adiabatic Process

A

A process in which no heat is transferred to or from the system by its surroundings

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16
Q

Titration

A

An analytical procedure in which a solution of known concentration is slowly added to a solution of unknown concentration to the point of molar equivalency, thereby providing the concentration of the unknown solution

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17
Q

Ideal Gas

A

A hypothetical gas whose particles would occupy zero volume and have no attractive intermolecular forces

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18
Q

Formula Weight

A

The sum of all the masses (in amu) present in one molecule of a molecular compound. Also called molecular weight

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19
Q

Conjugate Acids and Bases

A

A systematic pairing of a deprotonated species (base) with its protonated form of (conjugated acid). Conjugates appear on opposite sides of a chemical equation

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20
Q

Atomic Weight

A

The average mass, measured in amu, of all the isotopes of a given element as they occur naturally

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21
Q

Endothermic Reaction

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A

A reaction that proceeds with the net absorption of energy (heat) from the surroundings

22
Q

Molecular Formula

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A

A chemical formula showing the actual number of atoms present in a certain compound

23
Q

Free Radical

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A

At atom, usually a monoatomic halogen, that has an unpaired electron in its valence shell. Molecules whose substituents have unpaired electrons are also called free radicals

24
Q

Reversible Reaction

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A

A process that can proceed bidirectionally to form both product and reactant

25
State Function
A function that depends only on the initial and final states of a system, not on the path in between
26
Atom
The basic building block of all matter in the universe. An atom is made up of three main components: protons, neutrons, and electrons
27
Electronegativity
A measure of an atom's ability to pull electron diversity toward itself when involved in a chemical bond. Increases from left to right and from bottom to top on the periodic table
28
Metalloids
B, Si, Ge, As, Sb, Te, and Po are called metalloids and have properties that are in between those of metals and nonmetals
29
Common Ion Effect
The effect by which the molar solubility of one salt is reduced when another salt, having a common ion, is brought into the same solution
30
Cathode
The electrode at which reduction occurs during a cell's redox reaction. Electrons always flow towards the cathode in an electrochemical cell
31
Neutron
A subatomic particle with zero electric charge that is slightly heavier than a proton
32
Azeotrope
A liquid mixture of two or more substances that has its own constant boiling point, different from the
33
Indicator
A chemical species that changes color when undergoing dissociation. Indicators are used to signal the equivalence point of a titration
34
Polar Covalent Bond
A type of covalent bond between atoms of different electronegativities resulting in unequal sharing of electron density. Therefore, polar bonds have partial positive and partial negative poles
35
Empirical Formula
Chemical formula showing the smallest whole-number ration of atoms in a compound
36
Electron
A subatomic particle that orbits the nucleus and has a negative charge. The electron has a negligible mass and is often denoted by the symbol e-
37
Galvanic Cell
An electrochemical cell powered by a spontaneous redox reaction that produces an electric current flow; also called a voltaic cell
38
Vapor Pressure
The partial pressure of a vapor when it is in equilibrium with its solid or liquid phase
39
Common Ion Effect
The effect by which the molar solubility of one salt is reduced when another salt, having a common ion, is brought into the same solution
40
Colligative Properties
Certain properties of solutions - such as vapor pressure lowering, freezing point depression, boiling point elevation, and osmotic pressure-that are affected by the number of solute particles dissolved
41
Ionic Bond
A type of chemical bond in which there is a complete transfer of valence electrons to form positive and negative ions that are subsequently bound by electrostatic forces
42
Triple Point
The point on a phase diagram at which a substance exists in equilibrium between all three phases
43
Atomic Number
The number of protons in a single atom of an element, often denoted by the letter Z
44
Neutralization Reaction
A reaction in which an acid and a base are combined to form water and a salt
45
VSEPR
The acronym for Valence Shell Electron Pair Repulsion theory, which states that the three-dimensional molecular geometry about a central atom is determined by the electronic repulsions between its bonding and nonbonding electron pairs
46
Equilibrium
A dynamic point reached by a reversible reaction in which the rate of the forward reaction is equal to the rate of the reverse reaction. At chemical equilibrium, there is no net change in the concentrations of the products and reactants
47
Phase Diagram
A pressure versus temperature plot showing the conditions under which a substance exists in each phase--solid, liquid, or gas--and at which points those phases are in equilibrium with one another
48
Diffusion
Passive transport of a gas or solute throughout a medium by means of random motion
49
Reaction Quotient
A ratio of the concentrations of the products to the concentrations of the reactants at a given point during a reaction, commonly denoted by the letter by Q. In the expression, each reactant and product is raised to the power of its stoichiometric coefficient
50
Solution Equilibrium
The point at which a solution is fully saturated. At this point, the rate of dissociation of the solute equals the rate of its precipitation, and no further solute will dissolve
51
Normality
The gram equivalent weight of solute per liter of solution, often denoted by the letter N

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