Chemistry Honors
, TABLE OF CONTENTS
Atomic Structure - 3
Average Atomic Mass - 4
Electron Configuration - 4
Periodic Table - 8
Covalent Bonding - 13
Metallic Bonding - 14
Types of Substances - 15
Intermolecular Forces of Attraction - 16
Matter - 16
Separation Methods - 18
Density - 18
Properties Of Matter - 19
Changes in Matter - 19
Measurements - 20
Stoichiometry - 20
Solutions - 22
Dissolving Rate and Solubility - 23
Concentration - 25
Molarity - 25
Colligative Properties - 25
Phases Of Matter - 26
Phase Changes - 27
Thermochemistry - 27
Measurement Of Heat Energy - 29
Vapor Pressure & Boiling Point - 30
Calorimetry - 31
Behavior Of Gases - 32
Combined Gas Law - 33
, ATOMIC STRUCTURE
Chemistry - the study of the composition and behavior of matter
Matter - anything that has mass and volume
Elements - substance that can’t be broken down by a chemical change, the simplest form of
a pure substance
Atoms - the smallest particle of an element that retains its identity (same properties)
Parts of the Subatomic
Particle
Atom: Location Charge Mass Symbol Particles
Protons nucleus + 1 amu - Protons
Neutrons nucleus 0 1 amu - Neutrons
Electrons orbital - 〜0 amu - Electrons
Atomic Number - number of protons in the nucleus.
Specific to the element
Mass Number - sum of protons and neutrons
mass number - atomic number equals number of neutrons
Isotopes:
Similarities: Differences:
- same number of protons - different number of neutrons
- same number of electrons DIFFERENT MASS
Examples of isotopes: BOTH ARE CARBON
Carbon–12 Carbon–14
6 Protons 6 Protons
6 Neutrons 8 Neutrons Reminder : Isotopes are atoms of
the same element that have
6 Electrons 6 Electrons
different number of neutrons, and
therefore have different masses.
, Hydrogen Isotope # of Protons # of Neutrons Mass # Symbol
Protium 1 0 1
Deuterium 1 1 2
Tritium 1 2 3
Calculating Electrons:
Neutral: An atom with no charge Ion :An atom with a positive (cation) or
# electrons = # of protons negative (anion) charge
Example: C, Mg, O # electrons = # of protons - charge
Example of a cation: Mg^+2
Example of an anion: F^-1
AVERAGE ATOMIC MASS
Atomic Mass - the average of all the isotopes in a sample of that element
Ex.: Look on the periodic table … what is the atomic mass of chlorine? 35.453 amu
Chlorine has 2 isotopes that contribute to this atomic mass: Cl-35 and Cl-37
Why is the average atomic mass not 36amu? … NOT EQUALLY ABUNDANT 35 37
General Formula:
Atomic mass = (percent/100) x (mass) + (percent/100) x (mass)
ELECTRON CONFIGURATION
Electron Configuration - how the electrons are distributed throughout an atom’s energy
levels.
Valence Electrons - electrons in the outermost energy level Electrons
Kernel - everything except the valence electrons determine an
Group - vertical column on the periodic table. The group
atom’s chemical
number can be used to determine the number of valence
electrons
properties.
Group 1 = 1 valence electron Group 15 = 5 valence electrons
, TABLE OF CONTENTS
Atomic Structure - 3
Average Atomic Mass - 4
Electron Configuration - 4
Periodic Table - 8
Covalent Bonding - 13
Metallic Bonding - 14
Types of Substances - 15
Intermolecular Forces of Attraction - 16
Matter - 16
Separation Methods - 18
Density - 18
Properties Of Matter - 19
Changes in Matter - 19
Measurements - 20
Stoichiometry - 20
Solutions - 22
Dissolving Rate and Solubility - 23
Concentration - 25
Molarity - 25
Colligative Properties - 25
Phases Of Matter - 26
Phase Changes - 27
Thermochemistry - 27
Measurement Of Heat Energy - 29
Vapor Pressure & Boiling Point - 30
Calorimetry - 31
Behavior Of Gases - 32
Combined Gas Law - 33
, ATOMIC STRUCTURE
Chemistry - the study of the composition and behavior of matter
Matter - anything that has mass and volume
Elements - substance that can’t be broken down by a chemical change, the simplest form of
a pure substance
Atoms - the smallest particle of an element that retains its identity (same properties)
Parts of the Subatomic
Particle
Atom: Location Charge Mass Symbol Particles
Protons nucleus + 1 amu - Protons
Neutrons nucleus 0 1 amu - Neutrons
Electrons orbital - 〜0 amu - Electrons
Atomic Number - number of protons in the nucleus.
Specific to the element
Mass Number - sum of protons and neutrons
mass number - atomic number equals number of neutrons
Isotopes:
Similarities: Differences:
- same number of protons - different number of neutrons
- same number of electrons DIFFERENT MASS
Examples of isotopes: BOTH ARE CARBON
Carbon–12 Carbon–14
6 Protons 6 Protons
6 Neutrons 8 Neutrons Reminder : Isotopes are atoms of
the same element that have
6 Electrons 6 Electrons
different number of neutrons, and
therefore have different masses.
, Hydrogen Isotope # of Protons # of Neutrons Mass # Symbol
Protium 1 0 1
Deuterium 1 1 2
Tritium 1 2 3
Calculating Electrons:
Neutral: An atom with no charge Ion :An atom with a positive (cation) or
# electrons = # of protons negative (anion) charge
Example: C, Mg, O # electrons = # of protons - charge
Example of a cation: Mg^+2
Example of an anion: F^-1
AVERAGE ATOMIC MASS
Atomic Mass - the average of all the isotopes in a sample of that element
Ex.: Look on the periodic table … what is the atomic mass of chlorine? 35.453 amu
Chlorine has 2 isotopes that contribute to this atomic mass: Cl-35 and Cl-37
Why is the average atomic mass not 36amu? … NOT EQUALLY ABUNDANT 35 37
General Formula:
Atomic mass = (percent/100) x (mass) + (percent/100) x (mass)
ELECTRON CONFIGURATION
Electron Configuration - how the electrons are distributed throughout an atom’s energy
levels.
Valence Electrons - electrons in the outermost energy level Electrons
Kernel - everything except the valence electrons determine an
Group - vertical column on the periodic table. The group
atom’s chemical
number can be used to determine the number of valence
electrons
properties.
Group 1 = 1 valence electron Group 15 = 5 valence electrons
