Owens stolen chem quizlet

Density

mass/volume; in intensive (does not depend on the amount of material present)

What is an intensive property?

does not depend on the amount of material present

what is an extensive property?

does depend on the amount of material present

The Particulate Nature of Matter

all nature is made up of matter. More specifically, everything we see is comprised of the ~ 100 elements on the Periodic Table, which are made up of atoms

What can matter be divided into?

pure substances and mixtures

Elements

appear on the periodic table, and are made up of only one type of atom, with characteristics specific to that particular type of element

Compounds

made up of two or more atoms joined together in specific ratios by chemical bonds. Because they are joined by chemical bonds, they are considered to be pure substances even though they may have more than 2 types of elements

Mr. BrINCHlHOF

Br;I;N;Cl:H;O;F (put in calculator before test)

What is a solid (state of matter)

fixed volume and fixed shape

What two categories can solids be put into

Amorphous (no long-range structural pattern) or crystalline (meaning that they have long-range order)

Liquid (state of matter)

fixed volume but no fixed shape

Gas (state of matter)

no fixed volume or shape

What is an allotrope?

one of two or more different form in which an element can exist. For example diamond and graphite are 2 allotropes of the pure element carbon

physical properties

Can be observed or measured without changing the chemical composition of the material being described. Mass, color, boiling point, and density are examples of physical property

chemical properties

properties that relate to the ability to form new substances. these properties can routinely be observed without changing the composition of the material. Combustibility, acidity reactivity, and toxicity are examples

Physical Changes

changes in state, such as boiling, melting, sublimating, condensing, or freezing. Breaking an object, mixing two or more substances together. All the chemical composition of the material is not affected.

Chemical Changes

involve a change to the chemical composition of the material in question. Combustion and rusting are examples of chemical changes. (color changing is a chemical change)

homogeneous mixtures

even distribution; carbonated beverage or cup of coffee

heterogeneous mixture

not evenly distributed; soil or soup are examples

alloy

a mixture of elements that has metallic properties

substutional alloy

comprised of two or more metals, wherein minority component atoms replace some atoms of the major component

interstitial alloy

comprised of a metal and non-metal, in which the non-metal atom fits within the intersects (holes) between metal atoms

Antonie Lavoisier

law of conservation of mass

Joseph Proust

law of definite proportions

John Dalton

law of multiple proportions; early atom model

J.J. Tompson

discovered the electron; plum pudding model

Robert Millikan

discovered charge and mass of electron

Earnest Rutherford

discovery of nucleus and protons

James Chadwick

discovered neutrons

Dmitri Mandeleev

organized the periodic table

Niels Bohr

planetary model of the atom

Louis de Broglie

the wave model of the atom

Erwin Schrodinger

the quantum model of the atom

atomic structure

positive protons and un-charged neutrons in the nucleus, negatively charged electrons orbiting, mass of neutron and protons nearly identical.

isotopes

Atoms of the same element that have different numbers of neutrons

alkali metal

any metal in Group 1A of the periodic table

anion

A negatively charged ion

binary molecule

A molecule composed of exactly two different elements.

electron

negatively charged particle

ionic compounds

compounds composed of cations and anions

metals

Elements that are good conductors of electric current and heat.

neutrons

the particles of the nucleus that have no charge

polyatomic ion

A charged group of covalently bonded atoms

alkaline earth metal

An element in Group 2A of the periodic table; a very reactive metal having an oxidation number of +2.

atomic number (z)

the number of protons in the nucleus of an atom

cation

A positively charged ion

halogen

a nonmetal in Group 7A of the periodic table - 1

isotope

Atoms of the same element that have different numbers of neutrons

metaloids

(semiconductors) are the elements that have the properties of both metals and nonmetals

noble gases

the elements in Group 8A of the periodic table no charge

proton

positively charged particle

allotropes

Different forms of the same element

binary acid

an acid that contains only two different elements: hydrogen and one of the more electronegative elements

Electrolyte

A substance that dissolves in water to give a solution that conducts electric current

ion

A charged atom

mass number (A)

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

molecular compounds

A compound consisting of molecules of covalently bonded atoms

non-metals

an element or substance that is not a metal.

Transitional Metals

elements in groups 3-12

know how to do isotope and ion table

(z and p are the same number) (A is the periodic table number) (N = A - P) \#e- is n with the inverted charge for example (charge is -3 and N is 20 \#e- is 23)

Know the atomic mass problem

%/100 x The element number

the symbol of frequecy

v

symbol of wavelength

λ

symbol of

c

Planck's constant

6.626 x 10^-34 (h)

principle quantam number

(n \>= 1)

angular momentup quantam number

(l = 0 to (n-1))

magnetic quantum number

m sub l = -l to l

spin quantam number

denotes which electron in the orbital you're talking about; only 2 per orbital; one spins up and one spins down

use program for electron config on calculator

.

l = 0 - s - 1 - 2

.

l = 1 - p - 3 - 6

.

l = 2 - d - 5 -10

.

l = 3 - 4 - 7 - 14

.

bond length

the average distance between the nuclei of two bonded atoms

bond strength

energy required to break a bond

covalent bonding radius

a measure of the size of an atom that forms part of one covalent bond

effective nuclear charge (Zeff)

amount of charge felt by the most recently added electron

electorn affinity

how much an atom wants to gain an electron

Electronegativity

A measure of the ability of an atom in a chemical compound to attract electrons

electron shielding

the reduction of the attractive force between a positively charged nucleus and its outermost electrons due to the cancellation of some of the positive charge by the negative charges of the inner electrons

ionic bonds

Formed when one or more electrons are transferred from one atom to another

ionization energy

The amount of energy required to remove an electron from an atom

Isoelectronic

having the same number of electrons

lewis dot structures

diagrams that show valence electrons as dots

metallic characters

metals, metalloids, nonmetals

Non-bonding pairs

two paired valence electrons that tend not to participate in a chemical bond

octet rule

States that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons

valence shell electrons

electrons in the outermost shell

van der Waals forces

a slight attraction that develops between the oppositely charged regions of nearby molecules

be able to explain the periodic trends

see review

be able to show lewis dot structure with elements

(no compounds)

the three kinds of chemical bonds

ionic, covalent, metallic

formula unit

the smallest electrically neutral collection of ions

acids have what as the first element

hydrogen (exceptions are H2O and H2O2

what does mono, di, tri, and tetra mean

1, 2, 3, 4

ammonium

NH4+

Cabonate

CO3 2-

Hydride

OH-1

Nitrate

NO3 -1