Tuesday 1/27 Intro to Bonding!

• Please take out your lab book

• Pencil

Warm Up on page 104:

Using the periodic table make a Lewis Dot Diagram for Ar & S….

BrainPop – Chemical Bonds

https://www.brainpop.com/science/matterandchemistry/chemicalbonds/

Chemical BondingMrs. Kaminer 2015

Where are you….Glue your learning scale on page 104 in your INB

1: I can identify the number of electrons in an element. I recognize a Lewis Dot diagram.

2: I can identify different types of bonds. I can recognize a Lewis Dot diagram.

3: I can draw a Lewis Dot diagram for any element or compound correctly.

4: I can draw a Lewis Dot diagram correctly and identify the types of bonding that form a chemical compound.

SW: Understand and demonstrate their knowledge of the composition of an atom,

and the role electrons play in bonding to make a chemical compound.

1/27 – Based on the above scale, I am a ______ because………

Types of Chemical Bonds

• Compound – substance made of the combined atoms of two or more elements

• Chemical Formula – tells what elements a compound contains and the exact number of the atoms of these elements

What do those numbers mean?

• Subscript – represents # of atoms in a molecule of a particular element.

•H₂O subscript SO₄• Supersupscript – represents the oxidation # or how many electrons

have been gained or lost

• SO₄ 2- supersubscript

Coefficient – represents the # of units of each substance

• 2 H₂O

Bonds

• Atoms form compounds to become chemically stable. An atom is chemically stable when the outer energy level is complete or full.

Chemical Bond – force that holds together the atoms in a substance

• Type of Bonds? Based on what you know about bonding, are the following covalent or ionic bonds (use your periodic table to determine the answer)• CaCl2

• NaO• H2

• H2O• SO2

• NaCl• KF• Mg I2

• CO2

• NH3

• How many atoms are in each of the above molecules?

Writing Formulas

Writing Formulas

Writing Formulas

• Hydrate – a compound that has water chemically attached to its ions and written into its chemical formula.

• Covalent compounds can form more than one compound with each other. Scientists use Greek prefixes to indicate # of atoms of each element in binary compounds.

Wednesday 1/28/15

• Please take out your lab book

• Pencil

• Glue stick

• 3 pieces of paper

• Warm Up on page 107• What type of bond are the following compounds and how many of each atom are in

each compound?• NH3

• CH4

• HCl• NaCl

Ratios and Chemical Formulas

Compound

Name

Atoms Atomic

Ratio

Chemical

Formula

Hydrogen

chloride

H Cl

Water H H O

Ammonia N H H H

Methane C H H H H

Propane C C C H H H H

H H H H

Foldable Tabs

Naming Compounds

Naming Compounds (front cover)

Rules for naming compounds (2nd tab)

Rule 1 – Rule for 2nd name (3rd tab)

Rule 2 for 2nd name (4th tab)

Formula Combinations

Nonmetal-Nonmetal compounds

Naming CompoundsCompounds are given names that come from the names of their

elements.

Rules for Naming Compounds

• All compounds have 2 names

• The first name of the compound comes from the first element in the formula

• A subscript after the first element doesn’t affect the name

Rules for the second name

• Rule 1• If the compound only has 2 elements and is a metal-nonmetal compound, the

second name is the name of the second element with the ending changed to “ide”

• Examples:• Cl Chlorine becomes Chloride

• S Sulfur becomes Sulfide

• I Iodine becomes Iodide

• O Oxygen becomes Oxide

Rules for the second name

• Rule 2

• If the compound has more than 2 elements, the second name will come from the combination of elements at the end of the formula

Formula combinations

• NO3 nitrate NaNO3 = Sodium Nitrate

• OH hydroxide

• PO4 phosphate NaPO4 = Sodium Phosphate

• CO3 carbonate CaCO3 = Calcium Carbonate

• SO4 sulfate

Nonmetal-Nonmetal Compounds• start with element to the left side on the periodic

table

• add -ide to the second element

• use Greek prefixes for number of atoms: mono (1), di (2), tri (3), tetra (4), penta (5), hexa (6), hepta(7), octa (8), nona (9), deca (10)

• Example: • CO carbon monoxide

• CO2 carbon dioxide

• N2O5 dinitrogen pentoxide