Chem 107 Chapter 2

Front 1

dalton's atomic theory (of matter)

Back 1

ultimate, indivisible particles although experiments at the beginning of the present century showed that atoms themselves consist of particles
each element is composed of tiny, indestructible particles called atoms
all atoms of a given element have the same mass and other properties that distinguish them from atoms of other elements
atoms combine in simple, whole number ratios to form molecules of compounds
in a chemical reaction, atoms of one element cannot change into atoms of another element. they simply rearrange the way they are attached

Front 2

law of multiple proportions

Back 2

actual composition never changes, just the arrangement to form new substances/compounds
"ratio"

Front 3

JJ Thomson

Back 3

beam from cathode ray tube deflected toward positively charged plate
atoms contain negatively charged particles with a constant mass-to-charge ratio
also plum pudding model - electrons distributed throughout diffusely, positively charged sphere

Front 4

robert millikan

Back 4

determined the mass and charge of an electron with his oil droplet experiment
e=-1.6*10^--19 C
me=9.11*10^-28 C

Front 5

henri becquerel

Back 5

some materials produce invisible radiation, consisting of charged particles

Front 6

radioactivity

Back 6

spontaneous emission of high-energy radiation
beta particles (B, high energy electrons)
alpha particles (a, +2 charge, mass = He nucleus)

Front 7

rutherford

Back 7

bombarded a thin gold foil with alpha particles to test Thomson's model of the atom
theory predicted that the alpha particles would travel through the foil with little or no deflection
results indicated presence of dense particle within the atom
atom's positive charge is concentrated in the nucleus
proton has the opposite charge of the electron
mass of proton is 1840x mass of electron

Front 8

nucleus

Back 8

contains all positive charge and nearly all mass in an atom
1/10,000 the size of an atom
2 types of particles: proton (+), neutron (neutral)

Front 9

atomic mass units

Back 9

amu
relative scale to express masses of atoms and subatomic particles
based on 1 atom of Carbon
1amu=1Dalton

Front 10

aston's experiment

Back 10

positive ray analyzer results: 2 different kinds of neon gas atoms exist: 90%=20 amu, 10%=22 amu

Front 11

isotopes

Back 11

atoms of the same element (same number of protons), but different numbers of neutrons (different mass)

Front 12

A
X
z

Back 12

A=atomic mass
X= elemental symbol
Z= atomic number

Front 13

Ne-20
Ne-21
Ne-22

Back 13

Isotopes
Means 10 protons and 10 neutrons, 11 neutrons, 12 neutrons
atomic mass number - - - >

Front 14

natural abundance

Back 14

relative proportion of a given isotope compared to all the isotopes for the element found in a natural sample (%)

Front 15

average atomic mass

Back 15

weighted average mass of natural sample of an element
calculated by multiplying the natural abundance of each isotope by its exact mass in amu and then summing these products

Front 16

Mendeleev

Back 16

Period table - ordered elements by atomic mass, arranged elements in columns based on similar chemical and physical properties, left open spaces for elements not yet discovered

Front 17

periods

Back 17

horizontal rows (1->7)

Front 18

family/group

Back 18

column (1->18)

Front 19

alkali

Back 19

soft metals that react easily with water
ex. sodium metal
group 1

Front 20

alkaline earth

Back 20

reactive metallic elements with two electrons in the outermost energy level
ex. magnesium
harder, denser, stronger and have higher melting points, lower reactivity than alkali

Front 21

halogens

Back 21

group 17. VIIA elements. reactive elements

Front 22

noble gases

Back 22

group 18. inert gases but don't use it anymore because they have been able to react with other gases

Front 23

metals

Back 23

shiny solids, conduct heat and electricity, are malleable and ductile

Front 24

nonmetals

Back 24

solids, liquids, and gases, non-conductors, solids are brittle

Front 25

metalloids

Back 25

shiny solids (like metals), brittle (like nonmetals), semiconductors

Front 26

Law of Multiple Proportions

Back 26

if 2 elements can combine to form more than one compound, the mass of Y that will react with a given mass of X to form the compounds can be expressed as a ratio of small whole numbers.
ex. NO, NO2, N2O, N2O5, etc.

Front 27

molecular compounds

Back 27

composed of atoms held together by covalent bonds

Front 28

covalent bonds

Back 28

shared pairs of electrons that chemically bond atoms together

Front 29

molecular formulas

Back 29

the exact number and type of atoms present in one molecule of a compound
ex. C6H12O6

Front 30

empirical formula

Back 30

simplest whole-number ratio of elements in a compound
ex.CH2O

Front 31

ionic compound

Back 31

made of metal and a nonmetal
charged particles (ions) formed by a transfer of electrons between atoms
charges on ions depend on location in the periodic table
held together by electrostatic forces

Front 32

cations

Back 32

ions with positive charge
ex. Na+

Front 33

anions

Back 33

ions with negative charge
ex. Cl-

Front 34

binary molecular compounds

Back 34

compounds consisting of two nonmetals
-ide + prefixes

Front 35

one

Back 35

mono

Front 36

two

Back 36

di

Front 37

three

Back 37

tri

Front 38

four

Back 38

tetra

Front 39

five

Back 39

penta

Front 40

six

Back 40

hexa

Front 41

seven

Back 41

hepta

Front 42

eight

Back 42

octa

Front 43

nine

Back 43

nona

Front 44

ten

Back 44

deca

Front 45

binary ionic compounds

Back 45

cations (metals) and anions (nonmetals)
ex. MgCl2
must always be neutral
metals that form cations with different charges

Front 46

acetate

Back 46

(C2H3O2)-

Front 47

carbonate

Back 47

(CO3)2-

Front 48

perchlorate

Back 48

(ClO4)-

Front 49

nitrate

Back 49

(NO3)-

Front 50

sulfate

Back 50

(SO4)2-

Front 51

chromate

Back 51

(CrO4)2-

Front 52

hydroxide

Back 52

(OH)-

Front 53

ammonium

Back 53

(NH4)+

Front 54

hypochlorite
chlorite
chlorate
perchlorate

Back 54

(ClO)-
(ClO2)-
(ClO3)-
(ClO4)-

Front 55

binary acids

Back 55

hydrogen and a monoatomic anion
ex. Cl^-, S^2-
binary acids ex is halogen - HCl, HBr
hydro + halogen base name and ic
ex. HBr = hydrobromic acid

Front 56

oxy anions + related acids

Back 56

oxoanion ends in ate
ite
corresponding acid ends in
ic
ous

Front 57

hypochlorite

Back 57

(ClO)^-

Front 58

chlorite

Back 58

(ClO2)^-

Front 59

chlorate

Back 59

(ClO3)^-

Front 60

perchlorate

Back 60

(ClO4)^-

Front 61

hypochlorous acid

Back 61

HClO

Front 62

chlorous acid

Back 62

HClO2

Front 63

chloric acid

Back 63

HClO3

Front 64

perchloric acid

Back 64

HClO4