What is Chemistry?
Chapter 1
Introduction to Matter
Lesson 1: Describing Matter
Matter Crash Course Video
What is Matter (Advanced)
Chemical & Physical Changes Video
Many chemical reactions are NON-REVERSIBLE CHANGES .You cannot turn a baked cake back into its raw ingredients. Some chemical reactions can be reversed, and re-formed into the original substances. These are REVERSIBLE CHANGES.
Lesson 2: Classifying Matter
Below is the molecule for sugar
C6 - 6 carbon atoms H12 - 12 hydrogen atoms O6 - 6 oxygen atoms
Molecules to the Max
Chemical Changes
Mixtures
Lesson 3: Measuring Matter
When water freezes, water molecules form a crystalline structure maintained by hydrogen bonding. Solid water, or ice, is less dense than liquid water. Ice is less dense than water because the orientation of hydrogen bonds causes molecules to push farther apart, which lowers the density.
Lesson 4: Changes in Matter
Endothermic and Exothermic Reactions
Sodium metal reacts rapidly with water to form a colourless solution of sodiumhydroxide (NaOH) and hydrogen gas (H2). The resulting solution is basic because of the dissolved hydroxide. The reaction is exothermic.
Chapter 2: Solids, Liquids, and Gases
Lesson 1: States of Matter
Lesson 1 Vocab
Solid
Crystallin solid
amorphouse solid
liquid
fluid
surface tension
vicosity
gas
pressure
Lesson 2: Changes of State
Dry Ice Sublimation
Evaporation
States of Matter Melting Points
Difference Between Evaporation & Vaporization
Condensation
Water Cycle Video
Solids
Liquids
Gases
Lesson 3: Gas Behavior
The 3 Gas Laws
Plasma
Video Below
Labs
Chapter 3: Elements and the Periodic Table
Solving the puzzle of the periodic table - Eric Rosado
The genius of Mendeleev's periodic table - Lou Serico
Periodic Table Games & Apps
Lesson 1: Intro to Atoms
The Periodic Table Song
The Nucleus Crash Course
The Electron
Bohrs Model
Atoms Bombs
Tsar Bomba
See an Atom
Lesson 2: Organizing the Elements
Great Periodic Table Link: Ptable
Yes Another one!
Caesium in Water (slow motion) - Periodic Table of Videos
Lesson 3: Metals
What are the properties of metals?
metals: elements that are good conductors of electric current and heat
malleable: can be hammered or rolled into flat sheets or other shapes
ductile: material that can be made into long wires
thermal conductivity: objects ability to transfer heat
electrical conductivity: the ability to carry electric current
Ductility of Metals
A majority of elements in the periodic table are metals
Metals begin on the left side and continue across the table
Physical Properties of Metals
Properties of Metals
http://www.bbc.co.uk/schools/gcsebitesize/science/add_gateway_pre_2011/periodictable/metalsrev1.shtml
Metals Facts
Magnetic Metals: Co (Cobalt), Fe (Iron) Ni (Nickel)
Most metals are solid at room temp
Hg (Mercury) is liquid at room temp
Chemical Properties of Metals
reactivity: the ease and speed in which an element reacts or combines with other substances
Corrosion: deterioration of metal due to a chemical reaction in the environment, example rust.
Metals are mixed groups
Only some of the elements in groups 13-16 or metals
Lanthanides and Actinides
two bottom rows below the periodic table
Magnetic Metals: Co (Cobalt), Fe (Iron) Ni (Nickel)
Most metals are solid at room temp
Hg (Mercury) is liquid at room temp
Chemical Properties of Metals
reactivity: the ease and speed in which an element reacts or combines with other substances
Corrosion: deterioration of metal due to a chemical reaction in the environment, example rust.
Metals are mixed groups
Only some of the elements in groups 13-16 or metals
Lanthanides and Actinides
two bottom rows below the periodic table
- top row is Lanthanides, bottom row Actinides
Lanthanides contain Nd (neodymuim) used to make laser light. Used for surgery, cutting metals, military.
Actinides: most are made in labs and not found in nature.
Transuranium Elements: they follow uranium (U) in the periodic table. They are made. Pu (plutonium) is an example.
Metal Khan Academy Tutorial
Lesson 4: Nonmetals & Metalloids
Key Vocab (page 97)
nonmetal
noble gas
diatomic molecule
halogen
metalloid
semiconductor
Key Questions:
What are the properties of nonmetalsWhat are the families containing nonmetals?
What are the properties of nonmetals?
Some important nonmetals: C (carbon) N (nitrogen) P (Phosphorus)
H (hydrogen) O (oxygen)
some are poisonous and very reactive
they have a much wider variety of properties compared to metals
Physical Properties
nonmetal: an element that lacks most of the properties of a metal
all non metals are found on the right side of the periodic table except for H
tend to be dull and brittle
- if you hit most nonmetals with a hammer they would break
DNA is made up of non metals(N, P, H, O, C)
Chemical Properties
Gain or share electrons when they react with other atoms
If Na reacts with Cl to form table salt NaCl, the Na loses an electron to the Cl atom
NonMetals can combine with other nonmetals to form compounds.
- When two or more atoms do this they form a molecule.
What are the families containing nonmetals?
Nonmetals found in Group 1 and 14-18
Found in families: carbon (14), nitrogen(15), oxygen(16), halogen (17), noble gases (18) only one that contains all non metals, & Hydrogen (1)
Carbon Family
only 1 in group a nonmetal
Nitrogen Family
contains 2 nonmetals (N & P)
Nitrogen makes up 78% of Earth’s atmosphere
diatomic molecule: made up of two atoms
N2 is a diatomic molecule
TNT is made with nitrogen (trinitrotoluene)
Oxygen Family
Halogen Family
Metalloids
located between the metals and nonmentals
metalloids: have some properties of metals and nonmetals
they are semiconductors, used in computers, calculator, solar cells, lasers
semiconductors: conduct electricity under some conditions, but not all
Most common metalloid is Si (silicon) Silicon Valley??
Metals vs NonMetals
Chapter 4: Atoms & Bonding
Chapter 4 will cover 4 Lessons
- Atoms, Bonding, and the Periodic Table
- Ionic Bonds
- Covalent Bonds
- Bonding In Metals
Lesson 1: Atoms, Bonding and the Periodic Table
(pgs 124-129)
(pgs 124-129)
Key Vocab (pg 125)
valence electron
electron dot diagram
chemical bond
Key Questions:
- What determines an element's chemistry?
What Determines an Element’s Chemistry?
Valence Electrons
- valence electrons: electrons that have the highest energy
- The number of valence electrons in an atom helps determine the chemical properties of that element.
- electron dot diagrams: is the symbol for an element surrounded by dots, each dot stands for 1 valence electron
- Stable atoms: atoms with 8 valence electrons (Ne, Ar, Kr, Xe) Non reactive and stable (He is stable with 2)
- Atoms like to form bonds with other atoms so they can be more stable.
- H only needs 2 valence electrons to be stable
- When atoms bond they share electrons and they get bounced back and forth from each other or shared.
- chemical bond: force of attraction that holds atoms together as a result of the electrons being rearranged between them.
- Applying the Periodic Table
- The periodic table give you information about how many valence electrons in an atom.
- Rows = periods
- Columns = groups
- valence electron numbers increase from left to right
- elements within the same group have the same number of valence electrons, that is whey elements in a group have similar properties
- Noble Gases
- Elements in group 18 are Noble Gases and they have 8 valence electrons (except for He, has 2)
- They do not react easily with other elements
- unlikely to gain, lose, or share electrons
- Metals
- metal atoms react by losing electrons
- Nonmetals
- nonmetal atoms become stable when they gain or share enough electrons to have 8 valence electrons
- they usually combine with other nonmetals and metalloids by sharing electrons
- Halogens react easily with other elements
- Metalloids
- located in a zig zag line on the periodic table
- they can lose or share electrons
- Hydrogen
- it is placed in group 1 because it has 1 valence electron even though it is a considered a non metal
- its properties are very different from alkali metals
- hydrogen shares its electron when forming compounds with other non metals and becomes stable with 2 electrons
Lesson 2: Ionic Bonds
(pgs 130-137)
Key Vocab (pg 131)
ion
polyatomic ion
ionic bond
ionic compound
chemical formula
subscript
crystal
Key Questions:
How do ions form?
How are the formulas and names of ionic compounds written?
What are properties of ionic compounds?
How Do Ions Form?
ion: an atom or group of atoms that have an electrical charge
when a neutral atom loses a valence electron it loses a negative charge and becomes a positive ion
when a neutral atom gains an electron, it gains a negative charge and becomes a negative ion.
Metal atoms more likely to lose electron
Non metal atoms are more likely to gain electrons
Common Ions
Some ions are made up of several atoms.
Polyatomic ions: ions made up of more than 1 atom
example Ammonia is made up of 1 N and 4 H atoms
(A) The ammonium ion (NH4+) is a nitrogen atom (blue) bonded to four hydrogen atoms (white). (B) The hydroxide ion (OH-) is an oxygen atom (red) bonded to a hydrogen atom. (C) The carbonate ion (CO32-) is a carbon atom (black) bonded to three oxygen atoms.
Ionic Bonds
ionic bond: attraction between two oppositely charged ions (like Na and Cl) The resulting compound is called an ionic compound.
How Are The Formula Names of Ionic Compounds Written?
chemical formula: group of symbols that shows the ratio of elements in a compound. For example magnesium chloride is MgCl2
Subscripts: tell the ratio of elements in a compound.
To write the formula for an ionic compound write the symbol of the positive ion and then the symbol for the negative ion. Add the subscripts that are needed to balance the charges.
If there is not a subscript it is assumed to be 1
Naming Ionic Compounds
For an ionic compound, the name of the + (positive) ion comes first followed by the name of the - (negative) ion.
If the negative ion is a single element the end of its name changes to -ide. Example MgO magnesium oxide
If the negative ion is a polyatomic it usually ends in -ate, or -ite. Example Ammonium Nitrate (NH4NO3)
What are the names of the following compounds?
CuCl (composed of Cu+ and Cl-)
HgO (composed of Hg2+ and O2-)
Fe2O3 (composed of Fe3+ and O2-)
MnO2 (composed of Mn4+ and O2-)
Answers:
copper (I) chloride
mercury (II) oxide
iron (III) oxide
manganese (IV) oxide
What are Properties of Ionic Compounds?
HIgh Melting points
form hard crystals
Chapter 4
Lesson 3:Covalent Bonds
(pgs 138-145)
Lesson 3:Covalent Bonds
(pgs 138-145)
Key Vocab (pg 139)
covalent bond
molecule
double bond
triple bond
molecular compound
nonpolar bond
polar bond
Key Questions:
- How are atoms held together in a covalent bond?
- What are properties of molecular compounds?
- How do bonded atoms become fully charged?
How are atoms held together in a covalent bond?
Covalent Bond: When 2 atoms share an electron
COVALENT BONDS FORM MOLECULES..NOT IONS!!!
molecule: a group of atoms joined together by a covalent bond
Types of Bonds
What properties of molecular compounds?
molecular compound: compound made up of molecules
poor conductivity
lower melting points than ionic compounds
lower boiling points
How do bonded atoms become partially charges?
nonpolar bonds: where electrons are shared equally in a covalent bondpolar bonds: where electrons are not shared equally in a covalent bond. Also have stronger forces between them than non polar.
Here is a great picture to help you understand the differences between covalent
(polar and nonpolar) , and ionic!
Chapter 4
Lesson 4: Bonding in Metals
(pgs 146-151)
Lesson 4: Bonding in Metals
(pgs 146-151)
Key Vocab (pg 147)
metallic bond
alloy
Key Questions:
What is the structure of a Metal Crystal?What are the properties of Metals?
What is the structure of a metal crystal?
A metal crystal is a tightly packed group of positively charged metal ions. They are held together by a metallic bond.
What are the properties of metals?
shiny
luster
high levels of malleability
electrical conductivity
thermal conductivity
Differences in Bonds????
There is a couple different ways to determine if a bond is ionic or covalent.
By definition:
- an ionic bond is between a metal and a nonmetal
- covalent bond is between 2 nonmetals.
So you usually just look at the periodic table and determine whether your compound is made of a metal/nonmetal or is just 2 nonmetals. The exception is a compound made with ammonium (NH4+) Since ammonium is an ion, it forms ionic compounds. If the compound begins with H, it's an acid.
Ionic Bonds
NaBr = sodium bromide
|
Covalent Bonds
SO3 = sulfur trioxide
|
Practice
Balancing Equations Wks with Answers
Practice Wks #2
GAMES
Balancing Equations BattleShip
Balancing Chemical Equations
Name Ionic or Covalent Compounds
Chemical Compounds Rags to Riches
Balancing Equations
Balancing Equations
Chapter 4 Notes Click Here
Chapter 5: Chemical Reactions
Synthesis: This is the simplest type of chemical reaction. Two or more reactants are combined to create a more complex product.
A + B → AB
Decomposition: This is when a compound is broken down into its separate parts.
AB → A + B
Single replacement: This occurs when an element’s place in a compound is taken by another element.
A + BC → AC + B
Double replacement: In a double replacement, the ions in compounds are switched, creating a new compound.
AB + CD → AD + CB
Synthesis Reactions (Combination Reactions) - Examples and Practice
Double Replacement Reaction
Cool Chemical Reactions
Chapter 5: Chemical Reactions
Synthesis: This is the simplest type of chemical reaction. Two or more reactants are combined to create a more complex product.
A + B → AB
Decomposition: This is when a compound is broken down into its separate parts.
AB → A + B
Single replacement: This occurs when an element’s place in a compound is taken by another element.
A + BC → AC + B
Double replacement: In a double replacement, the ions in compounds are switched, creating a new compound.
AB + CD → AD + CB
Summary of Reactions.. Flinstones Style
Synthesis Reactions (Combination Reactions) - Examples and Practice
Decomposition Video
Single Replacement Video
Double Replacement Reaction
Precipitate Video
Cool Chemical Reactions
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