Length : Meter/Meter/Foot

Volume: Liter/Cubic meter/Quart

Mass: Gram/Kilogram/Pound

Time:Second/Second/Second

Temperature:Celsius/Kelvin/Fahrenheit

Pressure: (Metric=mmHG/atm/bar)(SI=Pascal)

Energy:Calorie/Joule

Times 10 to the...

9:giga:G

6:mega:M

3:kilo:k

-1:deci:d

-2:centi:c

-3:milli:m

-6:micro:weird u

-9:nano:n

-all the numbers you can read clearly plus one estimated digit

1)A zero at the end of a decimal number IS significant (25.0)

2)A zero between non-zero digits IS significant (205)

3) A zero at the beginning of a decimal number is NOT significant (0.00205 = 3sd)

4)Zeros as place holders are NOT significant (250,000,000 = 2 sd)

5)All digits of the coefficient in a number written in scientific notation are significant (5.600 x10^3 = 4sd)

multiplication/division : the final answer should retain the same number of significant figures as the measurement with the fewest significant figures

addition/subtraction: the final answer should retain the same number of decimal places as the measurement with the fewest decimal places

-a relationship written as a ratio

How many quarters in 25 dollars?

25$X4quarters/1 dollar = 25X4 = 100 quarters.

**the numerator should be in the same unit wanted for the final answer**

-try to cancel out other one...

K=C+273.15

F=1.8XC+32

0C=273.15K=32F

Came up with the first periodic table in 1800s

-contained 63 elements

-currently... 103 elements are typical & 118 known

-in 1911 proposed, based on famous gold-foil experiment, the spatial arrangement of the three subatomic particles within an atom.

(believe protons/neutrons to be in the middle, while electrons moved around like a cloud)

-1.67 X10^-24 grams

mass of a neutron is about the same

this number equals 1 AMU ***

Mass number is equal to the sum of protons and neutrons. (it is the number at top left of atom)

isotopes = atoms with different # of neutrons

isomers= same molecular formular with dif. bond formation

isotopes of an element coexist in certain proportions (abundance)  (i.e. C is 99% C-12 and 1% C-13)

-main levels numbered by these ..
"n"

can go up to and beyond 8.. but is never necessary

***"n" dictates how many sublevels a main level can have

-sublevels are given different names... s,p,d,f,g,h,..

s(one orbital),p(3orbital), d(5),etc

each orbital contains maximum of two electrons

n=4

total number orbitals = 1+3+5+7=16

each orbital = 2e... so max on 4th main level is 32 electrons

EC and the Periodic Table (patterns)

(first 18 elements)

1)The elements lined up in a column (group) all have the same number of electrons in the highest main level(i.e. valence e)

2)The column(group) number is the same as the number of electrons in the highest main level

3)elements with the same highest main level are lined up in a row (period)

4)The row number is the highest main level number

5)Elements in column 8 have fully-filled highest main level

the "d"block"

all other elements are called "main group elements" or "representative elements"

mission of every element is to have 8 electrons in the highest main level

Metals form _______

Non-metals form ______

cations (retain maiden name)

anions (add "ide")

ALL METALS ARE LOSERS>... EVEN TRANSITION (D-BLOCK) METALS!

how much energy is required to take away an electron

depends upon

1)distance from nucleus

2)core charge

euqal to the atomic number 'Z' minus the total number of electrons in the INNER SHELLS

ie. increases in 3rd period from 1(11-10) to 7(17-10)

core charge way higher in group 7!!

sizes of atoms

determined by the position of the valence shell

*increases as the valence shell becomes farther from the nucleus

*increases as core charge decreases

size increases: V<

a measure of electron affinity

increases: >^

has all atoms accounted for on both sides of the reaction arrow

-should have zero net charges on both side of  the equation***

IONIC 

-when cations and anions are glued together by a strong electrical force

-these are much stronger that covalent bonds

-the breaking of old bonds is always accompanied by the formation of stronger new bonds

i.e. Li2O

 ionic-electrons pretty much completely lost or gained

covalent bonds: electrons are shared

How do you find out charge of a transition metal?

Look at electron configuration.... what would make it stable?

quantum numbers

n=priciple quantum number

-level on periodic table(period)

-#of main levels

l=angular momentum (is n-1)

Ml=magnetic quantum number

s=spin

Pauli exclusion principle: every electron in an atom has a different set of quantum numbers

-electrons in same orbital have same n,l,ml but different spin

O-68%

C-18%

then..

H,N,Ca,P

Gasses and Liquids

11 gasses exist: He,Ne,Ar,Kr,Xe,Rn,N,O,Fl,Cl,H

2 Liquids exist: Br, Hg

EVERYTHING ELSE IS SOLID!!

scanning tunneling microscope

-allows us to see individual atoms

Dalton

(1766-1844)

-atoms are indivisible and indestructible

-chem reaction is a rearrangement of atoms

-compounds are 2+kinds of atom

atomic mass

-magnetic quantum number

-and electron occupying any given orbital can be found within this boundary  90% of the time

Ml is which orbital the electron is in.

i.e.

in s orbital, it will be 0

in P orbital, it will be -1,0,1

in D, it will be -2,-1,0,1,2

Cu = green

St= reddish

Na= yellow/red

K = purple

-electrons in aterials capable of giving off certain amount of energy that corresponds  to certain wavelength of visible light

(jumping to different orbitals)

 not the same as core charge

Zeff=Z-S

-can be used to explain important periodic trends

depends on how many electrons are shielding a valence electron from the inside

i.e. lose first electron... Zeff will be lower than when you lose the second electron, because there is one less that is shielding

-this means that there will be more ionization energy required, and more nuclear attraction

-how hungry an electron is

-smaller atom = higher affinity (lower r)

EA= 0 for nobles

increases ^>

-also affected by the number of electrons already in shells (will it be repelled?)

Systematic

Gold(1)/Gold (III)

Iron(II)/Iron(III)

traditional

(aurous/auric)

(ferrous/ferric)

two elements combine!!

-lone elements have 0 oxidation #

Physical

-change of state

-change of temperature

Chemical

-precipitate formation

-gas formation (bubbles) - not due to heat

-heat released or absorbed

-change colour

Inorganic/organic

-combination/addition

-decomposition/elimination

-replacement(single or double)/substitution

-combustion/combustion

-X/rearrangements(for isomers)

oxidation/reduction in organic vs inorganic chem

organic

-oxidation is adding O or losing H

-reduction is adding H or losing O

inorg

-oxidation is losing electrons

-reduction is gaining electrons

-for redox reactions, equations can be halfed to make it easier

for acid base... add H20 and H

what are names for ..

 Mg,Si,Sc,Ti,V,Cr,Mn,Co,Ni,Ga,Ge,As,Se

magnesium

silicon

scandium

titanium

vanadium

chromium

manganese

cobalt

nickel

gallium

germanium

arsenic

selenium