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Exam 1
CHEM 121
106
Chemistry
Undergraduate 1
02/28/2010

Additional Chemistry Flashcards

 


 

Cards

Term
Made up of atoms
Definition
Matter
Term

columns 1A - 2A (2 groups)

columns 3A - 8A

Very predicable behavior

Definition
Main groups
Term

3B - 2B (8 groups, 10 columns)

Variable chemical properties

Definition
Transition Metals
Term
14 groups between 3B and 4B
Definition
Inner Transition Metals
Term

Left side of the zigzag line in the periodic table (except for hydrogen)

Hard, solide, malleable(except Hg, which is liquid)

Conducts electricity, not brittle

 

Definition
Metals
Term

Right side of the zigzag line in the periodic table

Gases

Not malleable or brittle

Insulators of electricity

Definition
Nonmetals
Term

Tend to lie along the zigzag line in the periodic table

Properties of metals and nonmetals

Definition
Metalloids
Term
React with water to produce acids (-1 anions)
Definition
Halogens
Term

column 1A

Form an alkali solution when combined with water (+1 cations when in water)

Definition
alkali metals
Term

column 2A

+2 cations with water

Most insoluable in water

Definition
alkaline earth metals
Term
Chemically inert
Definition
Nobel gases
Term

Independent of sample size

Temperature

Melting Point

Density

Definition
Intensive properties
Term

Dependent on sample size

Length

Volume

Definition
Extensive properties
Term

Amount of matter in an object

All matter has this

Definition
Mass
Term
Describes anything with a physical presence - anything you can touch, taste, or smell
Definition
Matter
Term

Measures the force with which gravity pulls on an object

 

Definition
Weight
Term

How close to the true value a given measurement is

Single measurement: percent error

Series of measurements: average

 

Definition
Accuracy
Term

How well a number of independent measurements agree with each other.

Characterized by the standard deviation.

Definition
Precision
Term

the number of meaningful digits in a measured or calculated quantity. They come from uncertainty in any measurement

Generally the last digit in a reported measurement is uncertain

Exact numbers and relationships (7 days in a week, 30 students in a class) effectively have an infinite number of this

Definition

Significant figures

 

Term

Mass is neither created nor destroyed in chemical reactions

Atoms do nto mutate in reactions

Definition
Law of Conservation of Mass
Term

Differenct samples of a pure chemical substance always contain the same proportion of elements by mass

A pure substane will always have the same type and mass of atoms

Definition
Law of Definite Proportions
Term
Elements are made up of tiny particles
Definition
Atoms
Term

Matter is made up of atoms, atoms combine in whole numbers, in reactions, atoms rearrange

Each element is characterized by the mass of its atoms. Atoms of the same element have the same mass, but atoms of different elements have different masses

Chemical combination of elements to make different substances occurs when atoms join together in small whole-number ratios

Chemical reactions only rearrange the way that atoms are combined, the atoms themselves don't change

Definition
Dalton's Atomic Theory and the Law of Multiple Proportions
Term
Elements can combine in different ways to form different substances, whose mass rations are small whole-number multiples of each other.
Definition
Law of Multiple Proportions
Term
J.J. Thomson proposed that cathode rays must consist of tiny negatively charged particles called
Definition
Electrons
Term

Rutherford bombarded gold foil with alpha particles.  Although most of the alpha particles passed through the foil undeflected, approximately 1 in every 20,000 particles were deflected.  A fraction of those particles were deflectedc back at an extreme angle.

He proposed that the atom must consist mainly of empty space with the mass concentrated in a tiny central core.

His experiment showed that the mass of the atom is found in the

Definition
Atomic Nucleus
Term
Alpha rays are scattered only when they hit nucleus. The nucleus must be very small relative to the atom volume
Definition
Interpretation of Rutherford's Results
Term

The mass of an atom is in the nucleus

The proton and neutrons have equal mass

The electron is negative

The proton is positive

Definition
Structure of Atoms
Term
Number of protons in an atom's nucleus.  Equivalent to the number of electrons around the atom's nucleus.
Definition
Atomic Number
Term
The sum of the number of protons and the number of neutrons in an atom's nucleus.
Definition
Mass Number
Term
Atoms with identical atomic numbers but different mass numbers
Definition
Isotope
Term
The weighted average of the isotopic masses of the element's naturally occurring isotopes
Definition
Atomic Mass
Term
Matter consists of ____, elements or compound
Definition
Pure substances
Term
Mixtures are
Definition
hetero or homogeneous
Term
Contain atoms connected by covalent bonds (collection of like molecules is a pure molecular compound)
Definition
Molecules
Term
Results when two atoms share several (usually two) electrons.  Typically a nonmetal bonded to a nonmetal.
Definition
Covalent Bond
Term
A transfer of one or more electrons from one atom to another.  An electrostatic attraction between charged particles.  Typically a metal bonded to a nonmetal.
Definition
Ionic Bond
Term

A class of compounds

Positive and negative atoms associate to form a neutral salt

Definition
Ionic compounds
Term
A charged particle
Definition
Ion
Term
A positively charged particle.  Metals tend to form these
Definition
Cation
Term
A negatively charged particle.  Nonmetals tend to form these
Definition
Anion
Term
____ are not individual molecules, rather a neutral aggregate of positive and negative ions
Definition
Salts
Term

Form when metals give up electrons to nonmetals

The metal cation is positive and the nonmetal anion is negative

Definition
Binary salts
Term

Class of compounds

____ release protons (H+) and ____ release hydroxide (OH-)

Definition
Acids and bases
Term

Compounds that are easiest to name

Identify the metal cation and its charge for the main group

1A to 3A the cation charge is the group number

Definition
Binary ionic compounds
Term

Identify the nonmetal anion

The charge for atoms from 5A to 7A is group number -8

Definition
Naming Ionic Compounds
Term
The name must indicate the charge since they vary for most for
Definition
transition metals
Term
Take the name of the element
Definition
cations
Term

Take the root of the nonmetal name and ide

The salt is the cation name plus the anion name

Definition
anions
Term

Fro molecular compounds, the number of each atom type must be given

Use prefixes mono, di, tri, tetra, penta, hexa, hepta, etc.

Definition
Naming binary molecular, covalent compounds
Term

The first element listed is more cation like and takes the name of the element

The second element listed is more anion like and takes the name of the element with an ide modification to the ending

Definition
Naming binary molecular, covalent compounds
Term

Named after the anion

ite to ous

ate to ic

Definition
Complex acids
Term

When hydrogen is listed first

Neutral

The correct number of hydrogens (+) have to be added to make it neutral

Definition
Acid
Term
A balanced chemical equation show that the _____ is adhered to
Definition
law of conservation of mass
Term
Sum of atomic masses of all atoms in a molecule
Definition
Molecular/Formula Mass
Term
Sum of atomic masses of all atoms in a formula unit of any compound, molecular or ionic
Definition
Formula/Molecular Mass
Term
One mole of any substance contains 6.022 * 10^23 formula units
Definition
Avogadro's Number
Term
One mole of any substance is equivalent to its
Definition
Molecular/Formula Mass
Term
The relative proportions in which elements form compounds or in which substances react
Definition
Stoichiometry
Term
The amount actually formed in a reaction
Definition
Actual Yield
Term
The amount predicted by calculations
Definition
Theorectical Yield
Term
(actual yield)/(theorectical yield) * 100
Definition
Percent Yield
Term
The reactant that is present in limiting amount.  The extent to which a chemical reaction takes place depends on this
Definition
Limiting Reactant
Term
Any of the other reactants still present after determination of the limiting reactant
Definition
Excess Reactant
Term

The number of moles of a substance dissolved in each liter of solution. 

(moles of solute)/(liters of solution)

Definition
Molarity
Term
A homogenous (well-mixed) mixture
Definition
Solution
Term
The dissolved substance in a solution
Definition
Solute
Term
The major component in a solution
Definition
Solvent
Term

Concentrated solution + solvent = _____

MiVi = MfVf

Definition
dilute solution
Term
A procedure for determing the concentration of a solution by allowing a carefully measured volume to react with a solution of another substance (the standard solution) whose concentration is known
Definition
Titration
Term

Expressed by identifying the elements present and giving the mass percent of each

(mass atom X)/(formula mass)*100

Definition
Percent Composition
Term
It tells only the rations of the atoms in a compound
Definition
Empirical Formula
Term
It tells the actual numbers of atoms in a compound.  It can be either the empirical formula or a multiple of it.
Definition
Molecular Formula
Term
Sulfide
Definition
S-2
Term
Sulfite
Definition
SO3^-2
Term
Sulfate
Definition
SO4^-2
Term
Nitride
Definition
N^-3
Term
Nitrite
Definition
NO2^-1
Term
Nitrate
Definition
NO3^-1
Term
Phosphide
Definition
P^-3
Term
Phosphite
Definition
PO3^-3
Term
Phosphate
Definition
PO4^-3
Term
Carbide
Definition
C^-4
Term
Carbonate
Definition
CO3^-2
Term
Chloride
Definition
Cl^-1
Term
Hypochlorite
Definition
ClO^-1
Term
Chlorite
Definition
ClO2^-1
Term
Chlorate
Definition
ClO3^-1
Term
Perchlorate
Definition
ClO4^-1
Term
Bromide
Definition
Br^-1
Term
Hypobromite
Definition
BrO^-1
Term
Bromite
Definition
BrO2^-1
Term
Bromate
Definition
BrO3^-1
Term
Perbromate
Definition
BrO4^-1
Term
Iodide
Definition
I^-1
Term
Hypoiodite
Definition
IO^-1
Term
Iodite
Definition
IO2^-1
Term
Iodate
Definition
IO3^-1
Term
Periodate
Definition
IO4^-1
Term
Hydroxide
Definition
OH^-1
Term
Cyanide
Definition
CN^-1
Term
Cyanate
Definition
CNO^-1
Term
Hydrogen phosphate
Definition
HPO4^-2
Term
Hydrogen sulfate
Definition
HSO4^-1
Term
Bicarbonate
Definition
HCO3^-1
Term
Ammonium
Definition
NH4^+1
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