Types of Chemistry

Biochemistry

Organic

Inorganic

Analytical

Physical

Study of biological chemicals

Carbon based

All other elements

Method of analysis

Theory and Concept

1. Apply logical, organized reasoning to any observation(Observation) (Pattern Recognition)

2. Form a Hypothesis (Develop)

3. Reject or confirm that hypothesis by experiments (Experimentation)

Qualitative

Quantitative

Color

Oder

Taste

Feel

Density

Melting point

Boiling point

Compressibility

group of atoms

smallest part of a pure substance

(can be made by a single atom, several of the same atoms, or different atoms)

Diatomic

homotomic

heterotomic

2 atoms

one type of atom

2 or more types of atoms

Homogeneous

heterogeneous

Uniform

Non-uniform

Element

Data

defines quantities being measured

(all measurments must have units)

how close measurements are to the true value

(large random error)

how close to each other the measurement are

(large systematic error)

Systematic Errors

Random Errors

errors in one direction (high or low) can be corrected

Errors in any direction Can't be fixed

characteristic property of a substance

(mass/volume)

(g/cm^3) or (g/ml)

density of a substance/density of reference

unitless

reference material is normally water at 4 degrees celsius

measured by a hydrometer

Atomic mass

Atomic number

Charge

Number

Total protons and neutrons

#of protons or eletrons

+ or - values

# of atoms in a formula

lists elemements in compound

tells #of elements

may show how they are connected

small part of atom

dense

positive charge

protons and neutrons

surround nucleus

negative charge

different mass

different number of neutrons

Ex hydrogen and carbon

g/mol

(for mass of one unit or this don't change numbers just units)

lustrous, malleable, and ductile

conductors of heat and electricity

soild at room temp except mercury

will lose electron when reacting with non-metals

poor conductors of heat and electricity

many exist as diatomic molecules

wull gain electrons when reacting with metals but share with each other

varible chemical properties

act like non-metals when reacting with metals

act like metals when reacting with non-metals

semi-conductors

family or group

row or period

columns

rows across(a new layer is added to the atom for each row or period in the table)

Valence Electrons

Inner electrons

where most chemical reaction occur

Not much happens here under normal conditions

shells electrons

1

2

3

4

2

8

18

32

sublevel maxium# of electrons

N types

1 s

2 sp

3 spd

4 spdf

s=2

p=6

d=10

f=14

s=1

p=3

d=5

f=7

each orbital can hole 2 electrons

electrons fill inside out

 exceptions:

4s fills before 3d

5s fills before 4d

atoms are most stable when the outer shell is full or empty (normally 8 electrons except H and He)

atoms gain, lose or share to become stable based on what is easiest

positive ion

smaller than atom

Negative ions

Larger than atom

2 elements

overall formula must have no charge

positive element first

subscript given to elements

Don't exist as individual molecues

like to form crystals

name cation (1st +)

name anion ending in -ide(- charge)

name elements in order

use prefixes to indicate #of atoms(expect for the first atom)

use -ide for last element

linear

triagonal plane

tetrahedral

pyramidal

Bent

trigonal bipryamidal

trigonal pryamidal

octahedral

square pyramidal

square plane

temporary diople between molecules

weakest force

also called London Force

intermolecular attraction

Highly electronegative atom bonded directly to a hydrogen

surface tension

viscosity

vapor pressure

Ionic compound melting and boiling points?

Covalent compounds?

very high

lower normally

1.Dispersive forces

2.dipole forces

3.hydrogen bonds

4.inoic bonds

5.metallic bonds

6.covalent bonds