Chemistry First Test (found on Quizlet)

Dalton's Atomic Theory

1) elements are composed of atoms. 2) atoms of same element are identical, but differ from other elements. 3) elements can mix together in integer or simple fraction ratios 4) a chemical reaction involves only the separation, combination, or rearrangement of atoms, not their creation or destruction

uncuttable or indivisible

atomos

law of definite proportions

different samples of the same compound always contain its constituent elements in the same proportion by mass

Law of Multiple Proportions

If two elements combine to form different compounds, the masses of one element that combine with a fixed mass of the other element are in ratios of small whole numbers

Law of Conservation of Mass

Matter is not created nor destroyed in any chemical or physical change

atom

the basic unit of an element that can enter into chemical combination

subatonic particles

protons, neutrons, electrons

Radiation

the emission and transmission of energy through space in the form of waves

JJ Thomson

used the cathode ray tube to discover electrons

coulumb

SI unit of electric charge

Robert Millikan

1909 oil drop experiment, calculated the charge and mass of electrons

William Roentgen

discovered x-rays in 1895

Radioactivity

The spontaneous emission of radiation by an unstable atomic nucleus

alpha, beta, gamma

3 types of radiation

alpha rays

consist of positively charged particles and are deflected by a positively charged plate

beta rays

consist of negatively charged particles and are deflected by a negatively charged plate

gamma rays

have no charge and are unaffected by external electric or magnetic fields

Plum Pudding Model

J.J Thomsons model of an atom, in which he thought electrons were randomly distributed within a positively charged cloud

James Chadwick

Discovered the neutron

neutron

the particles of the nucleus that have no charge, and a mass slightly larger than that of a proton

mass number

the sum of the number of neutrons and protons in an atomic nucleus

isotope

Atoms of the same element that have different numbers of neutrons

protons and electrons

chemical properties are determined primarily by these two subatomic particles

physical and chemical properties

elements in the periodic table are grouped by their similar...

periods

Horizontal rows on the periodic table

groups or families

Vertical columns on the periodic table

metals, nonmetals, metalloids

three classes of elements

metal

good conductor of heat and electricity

Nonmetal

an element that is a poor conductor of heat and electricity

Metalloid

An element that has some characteristics of both metals and nonmetals

alkali metals

Group 1

alkaline earth metals

Group 2

Halogens

Group 7A

noble gases

Group 8A

Molecule

aggregate of at least two atoms in a definite arrangement held together by chemical forces

diatomic molecule

A molecule consisting of only two atoms

polyatomic molecule

a molecule that consists of more than two atoms

ion

An atom or group of atoms that has a positive or negative charge.

Cation

A positively charged ion

Anion

A negatively charged ion

ionic compound

A compound that consists of positive and negative ions

monatomic ion

an ion formed from only one atom

polyatomic ion

an ion made of two or more atoms

molecular formula

shows the exact number of atoms of each element in the smallest unit of a substance

Allotrope

one of two or more distinct forms of an element

structural formula

shows how atoms are bonded to one another in a molecule

empirical formula

tells us which elements are present and the simplest whole-number ratio of their atoms

organic compounds

Compounds that contain carbon, usually in combination with elements such as hydrogen, oxygen, nitrogen, and sulfur

binary compound

a compound composed of two elements

ternary compound

a compound composed of three elements

transition metals

groups 1B, 3B-8B

acid

A substance that increases the hydrogen ion concentration of a solution.

Oxoacids

acids that contain hydrogen, oxygen, and another element

Base

A substance that decreases the hydrogen ion concentration in a solution.

hydrate

A compound that has a specific number of water molecules bound to its atoms

ionic compounds, molecular compounds, acids and bases, and hydrates

What are the four major categories of inorganic compounds?

oxoanion

an anion derived from an oxoacid

bromic acid, hypobromous acid

HBrO3 -> HBrO (name before and after)

nitric acid, nitrous acid

HNO3-> HNO2 (name before and after)

chloric acid, perchloric acid

HClO3-> HClO4 (name before and after)

Stock system

A method for naming ions of elements that can form more than one possible positive charge by using a Roman numeral after the ion name to denote the ion's charge.

C=(F-32)x5/9

Celsius to Fahrenheit conversion

carbonic acid, carbonate

H2CO3-> CO3- (name before and after)

chlorous acid, chlorite

HClO2-> ClO2-

"per-ic" acid

addition of one O atom to the "-ic" acid changes the acid's name to

"-ous" acid

Removal of one O atom from the "-ic" acid changes the acid's name to

"hypo...-ous" acid

Removal of two O atoms from the "-ic" acid changes the acid's name to

"-ate"

When all the H ions are removed from the "-ic" acid, the anion's name ends with

"-ite"

When all the H ions are removed from the "-ous" acid, the anion's name ends with

atomic mass

The average mass of all the isotopes of an element

atomic mass unit

a mass exactly equal to one twelfth the mass of a carbon-12 atom

mole

the amount of a substance that contains as many elementary entities (atoms, molecules, or other particles) as there are atoms in exactly 12 g of carbon-12 isotope

molar mass

the mass in grams of one mole of a substance

molecular mass

the sum of the atomic masses in the molecule

percent composition by mass

the percent by mass of each element in a compound

chemical reaction

the process by which one or more substances change to produce one or more different substances

Stoichiometry

the quantitative study of reactants and products in a chemical reaction

mole method

the stoichiometric coefficients in a chemical equation can be interpreted as the number of moles of each substance

stoichiometric amounts

in the proportions indicated by the balanced equation

limiting reagent

the reactant that will be exhausted first in a chemical reaction

excess reagent

a reagent present in a quantity that is more than sufficient to react with a limiting reagent; any reactant that remains after the limiting reagent is used up in a chemical reaction

theoretical yield

the amount of product that would result if all the limiting reagent reacted

actual yield

the amount of product actually obtained from a reaction

percent yield

the proportion of the actual yield to the theoretical yield

6.022*10^23

Avogadro's number

6.022*10^23amu

One gram is equal to how many amu?

1.661*10^-24g

how many grams are in one amu

Avogadro's number

number of representative particles in a mole, 6.02 X 10^23

Solute

the substance present in a smaller amount

Solution

A homogeneous mixture of two or more substances

Solvent

the substance present in the larger amount

Electrolyte

a substance that, when dissolved in water, results in a solution that can conduct electricity

nonelectrolyte

does not conduct electricity when dissolved in water

Hydration

the process in which an ion is surrounded by water molecules arranged in a specific manner

reversible reaction

a reaction that can occur in both directions

precipitation reaction

a reaction which results in the formation of an insoluble product or precipitate

precipitate

an insoluble solid that separates from the solution

metathesis reaction

a reaction that involves the exchange of parts between two compounds

Solubility

the maximum amount of solute that can dissolve in a given amount of solvent at a given temperature

molecular equation

the formulas of the compounds are written as though all species existed as molecules or whole units