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Chemistry Notes
Day 1
Chemistry – the study of the composition, structure, and properties of matter and the
changes it undergoes
Matter – anything that has mass and takes up space
Four Phases of Matter
 Solid – has definite shape and volume
 Liquid- has definite volume but no definite shape
 Gas – has no definite shape or volume
 Plasma – the material that makes up stars very dense and high energy
Atom – fundamental building block of all matter
Element – a pure substance made of only one kind of atom
92 naturally occurring elements exist
Periodic Table Square
 Element Name
 Atomic Symbol – abbreviation for the element (first letter always capital second
letter if there is one always lower case)
 Atomic Number – tells the number of protons in the atom
 Atomic Mass – the total mass of the element
Subatomic Particles
 Proton - positive charge – 1 amu
 Neutron - neutral charge – 1 amu
 Electron - negative charge – 0 amu
amu – atomic mass unit
Proton and neutron located in the nucleus of the atom
Electron located in the electron shells or electron cloud surrounding the nucleus
Day 2
Any unbonded atom of any element has an overall neutral charge
Numbers of subatomic particles in each atom
 Protons: determined by the atomic number
 Electrons: equals the number of protons
 Neutrons: Rounded Atomic Mass – Atomic Number = # of Neutrons
Maximum number of electrons in each electron shell:
Shell
1
2
3
4
5
6
7
Number of electrons
2
8
18
32
50
72
98
Solar system model
See your notes!!
Know element and symbols for the following:
hydrogen, helium, lithium, beryllium, boron, carbon, nitrogen, oxygen, fluorine, neon,
sodium, magnesium, aluminum, silicon, phosphorous, sulfur, chlorine, argon, potassium,
calcium, iron, copper, zinc, bromine, silver, iodine, gold, lead, mercury, radon.
Day 3
99% of the atoms mass in the nucleus
The energy of the atom in the electron shells
Most of an atom empty space
Isotopes – atoms of the same element that have the same number of protons and different
number of neutrons and different mass. (Hydrogen example)
Valence – outer most shell and electrons
All chemical bonding takes place in the valence shell between valence electrons of two or
more atoms.
Periodic Table - classification system for elements
Dimitri Mendeleeve – created the first periodic table, organized by atomic mass.
Current periodic table organized by atomic number
Properties of metals-75% of the table is made up of metals
 Shiny
 Good conductors of heat and electricity
 Malleable – can be bent or hammered in to thin sheets
 Ductile – can be stretched into thin wires
 Loose valence electrons when they bond
Properties of nonmetals
 Dull
 Brittle
 Poor conductors of heat and electricity
 Gain valence electrons when they bond
Properties of metalloids
 Elements that touch stair-step line between metals and nonmetals
 Have characteristics of metals and nonmetals
Family/Group – columns of elements
 Same physical and chemical properties
 Same number of valence electrons
Period – row of elements
 Same number of electron shells
 Left to right across the table: increase in atomic mass, decrease in atomic radius.
Family 18 called the Nobel Gasses they are all inert gasses
Inert – will not bond with any element
Transition Metals – section of metals on the middle of the table family 3-12