Chapter 2 Flashcards by Amanda Vestal

states that different samples of a given compound always contain the same elements in the same mass ratio

law of definite proportions

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states that if two elements can combine to form more than one compound with each other, the masses of the one element that combine with a fixed mass of the other element are in ratios of small whole numbers

law of multiple proportions

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-discovered the ratio of the electric charge to the mass of an individual electron using the cathode ray tube

J.J. Thomson

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determined the charge on an electron

milikan

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noticed that cathode rays caused glass and metal to emit another type of ray
he named the rays “X rays” because of their mysterious nature
caused fluoresence
were not defined by a magnet

wilhelm roentgen

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accidentally discovered that uranium darkened photographic film

antonine becquerel

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suggested name “radioactivity”
rays were highly energetic and not deflected by a magnet
however, rays arose spontaneously unlike the rays discovered by roentgen

marie curie

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describes a substance that spontaneously emits radiation

radioactive

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positively charged particles

alpha (a)

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electrons

beta (B)

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no charge and are unaffected by external electric or magnetic fields

gamma (y)

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number of protons in the nucleus of each atom of an element

atomic number (Z)

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total num,ber of neutrons and protons present in the nucleus

mass number (A)

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all atoms are not identical (as proposed by Dalton)

- same atomic number (Z) but different mass numbers (A)

isotopes

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horizontal rows

periods

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vertical columns

- elements in the same family have similar chemical and physical properties

families

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good conductors of heat and electricity (majority of elements on the table, located to the left of the stair step)

metals

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nonconductors (located in upper right-hand corner)

nonmetals

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in between metals and nonmetals (those that lie along the separation line)

metalloids

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is the mass of the atom in atomic mass units (amu)

atomic number

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is defined as a mass exactly equal to one-twelth the mass of one carbon- 12 atom

atomic mass unit

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combination of at least two atoms in a specific arrangement held together by chemical bonds

molecule

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2 of the same atoms

homonuclear- diatomic molecules

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2 different atoms

heteronuclear- diatomic molecules

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- contain more than 2 atoms - most molecules - may contain more than one element - ex: ozone, o3; white phosphorus, p4; water, h2o, and methane CH4

polyatomic molecules

shows exact number of atoms of each element in a molecule

molecules

one of the two or more distinct forms of an element | -ex: oxygen, ozone, diamond and graphite

allotrope

shows the general arrangement of atoms within the molecule | H-O-H

structural formula

mono

tri

tetra

penta

hexa

hepta

octa

nona

deca

a substance that produces hydrogen ions (H+) when dissolved in water

acid

contain carbon and hydrogen (sometimes with oxygen, nitrogen, sulfur and the halogens)

organic compounds

contain only carbon and hydrogen

hydrocarbons

simplest examples of hydrocarbons

alkanes

determines chemical properties

functional group

reveal the elements present and in what whole-number ratio they are combined

empirical formula

an atom or group of atoms that has a net positive or negative charge

ion

one atom with a positive or negative charge

monatomic ion

ion with a net positive charge due to the loss of one or more electrons

cation

ion with a net negative charge due to the gain of one or more electrons

anion

ions that are a combination of two or more atoms

polyatomic ions

- 5thh century B.C. - greek - "atomos" - which is to say "indivisible" - no substantial visual model - determine properties

Democritus

- english..1808 - billard ball model - solid sphere - determined composition - workable atomic theory - revived greek thoughts

Dalton

- early 1900's - discovered e's - plum-pudding model - but blueberry muffin model is better

JJ Thomson

- 1910 - gold foil experiment - nuclear model - what a surprise

Rutherford

- 1913 - planetary model - energy levels - defined orbits - not bad for the time

Bohr

- many contributors - schroedinger a key player - probability model with electron cloud - 1920's

Quantum-Mechanical

ammonium

NH4+

hydronium

H3O+

Mercury(I)

Hg2+2

azide

N3-

carbonate

CO3-2

Chlorate

ClO3-

chlorite

ClO2-

chromate

Cr2O7-2

cyanide

CN-

dichromate

Cr2O7-2

dihydrogen phosphate

H2PO4-

bicarbonate

HCO3-

hydrogen phosphate

HPO4-2

bisulfate

HSO4-

hydroxide

OH-

hypochlorite

ClO-

nitrate

NO3-

nitrite

NO2-

oxalate

C2O4-2

perchlorate

ClO4-

permanganate

MnO4-

peroxide

O2-2

phosphate

PO4-3

phosphite

PO3-3

sulfate

SO4-2

sulfite

SO3-2

thiocyanate

SCN-

compounds that have a specific number of water molecules within their solid structure

hydrates