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Fundamentals of Chemistry
GFEs - Fundamentals of Chemistry - ILT '13
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Professional
07/05/2011

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Term

Define "states of matter"

Definition

 

The physical forms in which matter exists: solid, liquid, and gas.

 

Term
Define atomic weight
Definition

 

The weight of an element is defined as the weighted average of the masses of all of its natural occurring isotopes.

 

Term
Define molecular weight
Definition

 

The weight of a molecule is the total mass of the individual atoms.

 

Term
Define Mole
Definition

One mole represents a definite number of objects, substances, or particles. (For example, a mole of atoms, a mole of ions, a mole of molecules, and even,

theoretically, a mole of elephants.)

 

A mole is defined as the quantity of a pure substance that contains 6.02 x 1023

units (atoms, ions, molecules, or elephants) of that substance.

Term
Define gram atomic weight
Definition

The mass of a mole of atoms is called the gram atomic weight (GAW).

Term
Define gram molecular weight
Definition

The mass of a mole of molecules is called the molar mass or gram molecular weight (GMW).

Term

 

LIST the components of an atom, relative sizes, and charges.

 

Definition
[image]
Term

 

STATE the criterion used to classify an atom chemically

 

Definition

An atom is classified chemically by the number of protons in its nucleus (atomic number)

Term

 

DEFINE the following subdivisions of the periodic table:

 

– Periods

 

– Groups

 

– Classes

 

Definition
[image]
Term

 

Define Valence

 

Definition

The term valence (of an atom) is defined as the number of electrons an element gains or loses, or the number of pairs of electrons it shares when it interacts with other elements.

Term
Define ionic bonds
Definition
An ionic bond is formed when one or more electrons is wholly transferred from one element to another, and the elements are held together by the force of attraction due to the opposing charges.
Term
Define Van der Waals forces
Definition

The temporary dipole induces a similar temporary dipole on a nearby atom, ion, or molecule. Every instant, billions of these temporary dipoles form, break apart, and reform to act as a weak electrostatic force of attraction known as Van der Waals forces

.

 

 

These forces occur between the molecules of nonpolar covalent substances

 

These forces are generally believed to be caused by a temporary dipole, or unequal charge distribution, as electrons constantly move about in an atom, ion, or molecule.

 

Term
Define covalent bonding 
Definition

A covalent bond is formed when one or more electrons from an atom pair off with one or more electrons from another atom and form overlapping electron shells in which both atoms share the paired electrons.

Term
Define metallic bonding
Definition

In the metallic bond, an atom achieves a more stable configuration by sharing the electrons in its outer shell with many other atoms.

Term

 

DESCRIBE the physical arrangement and bonding of a polar molecule.

 

Definition

When the shared pair of electrons is

NOT

shared equally, one end of the bond is positive, and the other end is negative.

Term

 

DESCRIBE the three basic laws of chemical reactions.

 

Definition

The Law of Conservation of Mass - total mass of the products equals the total mass of the reactants

 

The Law of Definite Proportions -

no matter how a given chemical compound is prepared, it always contains the same elements in the same proportions by mass.

 

The Law of Multiple Proportions - 

if two elements combine to form more than one compound, the masses of one of the elements combining with a fixed mass of the other are in a simple ratio to one another

Term

 

STATE how elements combine to form chemical compounds.

 

Definition

The Laws of Definite Proportions and Multiple Proportions and the related portions of atomic theory form the bases for most quantitative calculations involving chemical reactions.

 

Regardless of the type of bond (ionic, covalent, or metallic), specific amounts of one element will react with specific amounts of the element(s) with which it

is combined.

Term
Define mixture
Definition

If two substances are placed together in a container, in any ratio, the result is a mixture.

Term
Define Solvent
Definition

The solvent is the material that dissolves the other substance(s).

Term
Define solubility
Definition

Solubility is defined as the maximum amount of a substance that can dissolve in a given amount of solvent at a specific temperature.

Term
Define Solute
Definition

The substances that dissolve in the solution are called solutes

.

Term
Define Solution
Definition

A homogeneous mixture of two or more substances is called a solution

Term
Define equilibrium
Definition

Equilibrium is the point at which the rates of the forward and reverse reactions are exactly equal for a chemical reaction if the conditions of reaction are constant.

Term

 

STATE Le Chateleir’s principle.

 

Definition

Le Chatelier's Principle states that if a stress (for example, heat, pressure, concentration of one reactant) is applied to an equilibrium, the system will

adjust, if possible, to minimize the effect of the stress.

Term
Define Parts per Million (ppm)
Definition

The term ppm is defined as the concentration of a solution in units of one part of solute to one million parts solvent.

Term
Define density
Definition

Density is the measure of the mass per unit volume of a material

 

(density = mass/volume).

Term
Define molarity
Definition

 

Molarity is defined as moles of solute per liter of solution.

 

Molarity (M) = moles of solute (n)/liters of solution (V)

 

Term
Define normality
Definition

Normality (N) is defined as the number of equivalents of solute dissolved in one liter of solution.

Term
Define acid
Definition

 

Acids are substances that dissociate in water to produce hydrogen (H+).

 

Term
Define salt
Definition

When an acid reacts with a base, forms two products: water and a salt.

 

A salt is an ionic compound composed of positive ions and negative ions

 

.

 

Term
Define pOH
Definition

 

The

 

pOH of a solution is defined as the negative logarithm of the hydroxyl concentration, represented as [OH-] in moles/liter.

 

Term
Define Alkalies
Definition

Certain soluble salts (principally sodium, potassium, magnesium, and calcium) that have the property of combining with acids to form neutral salts are called

alkalies.

Term
Define Base
Definition

Bases are substances that produce hydroxide ions (OH

-

) in water solutions.

Term
Define pH
Definition

ph is defined as the negative logarithm of the hydrogen concentration, represented as [H +] in moles/liter.

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